Edexcel GCSE 9-1 CHEMISTRY/Combined Science QUIZ on TOPIC 1 "KEY CONCEPTS in CHEMISTRY" (HT)

Which four quantities a, b, c and d are required to balance the equation ...
aCH_4(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-1]
1. 1 2 1 2
2. 1 1 1 2
3. 1 2 2 1
4. 1 1 1 1
Which four quantities a, b, c and d are required to balance the equation ...
aC₂H_6(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-2]
1. 1 2 1 3
2. 2 7 4 6
3. 2 4 4 6
4. 1 7 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aC₃H_8(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-3]
1. 1 3 3 4
2. 2 10 4 6
3. 1 5 3 4
4. 2 5 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aC₄H_10(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-4]
1. 1 13 8 4
2. 2 7 4 10
3. 1 5 3 4
4. 2 13 8 10
Which four quantities a, b, c and d are required to balance the equation ...
aC₅H_12(l) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-5]
1. 1 8 5 6
2. 1 4 4 6
3. 2 4 5 12
4. 2 8 10 12
Which four quantities a, b, c and d are required to balance the equation ...
aC₆H_14(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-6]
1. 2 9 6 14
2. 2 19 12 14
3. 1 9 6 7
4. 1 10 12 7
Which four quantities a, b, c and d are required to balance the equation ...
aC₇H_16(l) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-7]
1. 1 5 7 8
2. 2 12 14 16
3. 1 11 7 8
4. 2 11 14 16
Which four quantities a, b, c and d are required to balance the equation ...
aC₈H_18(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-8]
1. 1 13 8 18
2. 1 13 8 9
3. 2 13 16 18
4. 2 25 16 18
Which four quantities a, b, c and d are required to balance the equation ...
aC₂H_4(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-9]
1. 1 3 2 2
2. 1 2 2 2
3. 2 3 4 4
4. 2 6 4 4
Which four quantities a, b, c and d are required to balance the equation ...
aC₃H_6(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-10]
1. 2 5 6 6
2. 2 9 6 6
3. 1 5 3 3
4. 1 9 3 3
Which four quantities a, b, c and d are required to balance the equation ...
aC₄H_8(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-11]
1. 2 12 8 8
2. 2 6 8 8
3. 1 6 4 4
4. 1 3 4 4
Which four quantities a, b, c and d are required to balance the equation ...
aC₇H_8(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-12]
1. 2 9 4 8
2. 2 10 14 8
3. 1 5 7 4
4. 1 9 7 4
Which three quantities a, b and c are required to balance the equation ...
aFe_(s) + bO_2(g) ==> cFe₃O_4(s) ? [eq-13]
1. 3 2 1
2. 3 4 1
3. 6 4 2
4. 6 2 2
Which three quantities a, b and c are required to balance the equation ...
aLi_(s) + bO_2(g) ==> cLi₂O_(s) ? [eq-14]
1. 2 1 2
2. 4 1 2
3. 4 2 1
4. 2 2 1
Which three quantities a, b and c are required to balance the equation ...
aAl_(s) + bO_2(g) ==> cAl₂O_3(s) ? [eq-15]
1. 1 3 2
2. 4 6 4
3. 4 3 2
4. 2 3 2
Which three quantities a, b and c are required to balance the equation ...
aMg_(s) + bO_2(g) ==> cMgO_(s) ? [eq-16]
1. 1 1 2
2. 4 2 2
3. 2 1 1
4. 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aZn_(s) + bHCl_(aq) ==> cZnCl_2(aq) + dH_2(g) ? [eq-17]
1. 1 2 1 1
2. 2 2 2 1
3. 2 1 1 2
4. 1 1 2 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe_(s) + bH₂SO_4(aq) ==> cFeSO_4(aq) + dH_2(g) ? [eq-18]
1. 1 1 1 2
2. 1 1 1 1
3. 2 2 2 1
4. 2 1 2 2
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bHCl_(aq) ==> cAlCl_3(aq) + dH_2(g) ? [eq-19]
1. 1 6 3 2
2. 2 3 2 3
3. 2 6 2 3
4. 1 3 3 2
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bH₂SO_4(aq) ==> cAl₂(SO₄)_3(aq) + dH_2(g) ? [eq-20]
1. 1 3 1 3
2. 2 3 2 3
3. 1 2 2 2
4. 2 3 1 3
Which four quantities a, b, c and d are required to balance the equation ...
aNa_(s) + bH₂O_(l) ==> cNaOH_(aq) + dH_2(g) ? [eq-21]
1. 2 2 2 1
2. 2 1 2 1
3. 1 2 1 2
4. 1 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aCa_(s) + bH₂O_(l) ==> cCa(OH)_2(aq) + dH_2(g) ? [eq-22]
1. 2 2 2 1
2. 1 2 1 1
3. 1 2 1 2
4. 2 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe_(s) + bH₂O_(g) ==> cFe₃O_4(s) + dH_2(g) ? [eq-23]
1. 3 4 1 2
2. 2 3 1 4
3. 3 4 1 4
4. 2 3 2 2
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bH₂O_(g) ==> cAl₂O_3(s) + dH_2(g) ? [eq-24]
1. 3 4 1 6
2. 1 3 1 3
3. 2 4 2 6
4. 2 3 1 3
Which four quantities a, b, c and d are required to balance the equation ...
aMg_(s) + bCuSO_4(aq) ==> cMgSO_4(aq) + dCu_(s) ? [eq-25]
1. 1 1 1 1
2. 2 1 2 2
3. 1 2 1 2
4. 2 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aCu_(s) + bAgNO_3(aq) ==> cCu(NO₃)_2(aq) + dAg_(s) ? [eq-26]
1. 1 1 2 1
2. 1 2 1 2
3. 2 2 1 2
4. 2 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aZn_(s) + bFe₂(SO₄)_3(aq) ==> cZnSO_4(aq) + dFe_(s) ? [eq-27]
1. 3 2 6 2
2. 3 1 3 3
3. 3 1 3 2
4. 2 2 6 3
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bFe₂O_3(s)) ==> cAl₂O_3(s) + dFe_(s) ? [eq-28]
1. 1 2 2 1
2. 3 1 1 3
3. 2 3 2 3
4. 2 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aCl_2(aq) + bKBr_(aq) ==> cKCl_(aq) + dBr_2(aq) ? [eq-29]
1. 1 2 2 1
2. 2 1 1 1
3. 1 1 2 2
4. 2 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aBr_2(aq) + bNaI_(aq) ==> cNaBr_(aq) + dI_2(aq) ? [eq-30]
1. 1 2 1 2
2. 1 2 2 1
3. 1 1 2 2
4. 2 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aCl_2(aq) + bCaI_2(aq) ==> cCaCl_2(aq) + dI_2(s) ? [eq-31]
1. 2 1 2 1
2. 1 2 2 2
3. 1 1 1 1
4. 2 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aAlBr_3(aq) + bCl_2(aq) ==> cAlCl_3(aq) + dBr_2(s) ? [eq-32]
1. 1 3 2 2
2. 1 3 1 3
3. 3 2 2 2
4. 2 3 2 3
Which five quantities a, b, c, d and e are required to balance the equation ...
aCaCO_3(s) + bHCl_(aq) ==> cCaCl_2(aq) + dH₂O_(l) + eCO_2(g) ? [eq-33]
1. 1 2 1 1 1
2. 2 2 1 2 1
3. 1 1 1 1 1
4. 2 1 2 2 2
Which five quantities a, b, c, d and e are required to balance the equation ...
aNa₂CO_3(s) + bHCl_(aq) ==> cNaCl_(aq) + dH₂O_(l) + eCO_2(g) ? [eq-34]
1. 1 4 4 2 2
2. 1 2 2 1 1
3. 2 2 4 2 2
4. 2 2 2 1 1
Which five quantities a, b, c, d and e are required to balance the equation ...
aTl₂(CO₃)_3(s) + bHCl_(aq) ==> cTlCl_3(aq) + dH₂O_(l) + eCO_2(g) ? [eq-35]
1. 2 6 4 3 6
2. 1 3 2 6 2
3. 1 6 2 3 3
4. 2 3 4 3 6
Which five quantities a, b, c, d and e are required to balance the equation ...
aTl₂(CO₃)_3(s) + bH₂SO_4(aq) ==> cTl₂(SO₄)_3(aq) + dH₂O_(l) + eCO_2(g) ? [eq-36]
1. 2 6 4 3 6
2. 1 3 2 6 6
3. 1 6 2 6 3
4. 1 3 1 3 3
Which three quantities a, b and c are required to balance the equation ...
aNa_(s) + bCl_2(g) ==> cNaCl_(s) ? [eq-37]
1. 2 1 2
2. 1 1 1
3. 1 2 1
4. 2 1 1
Which three quantities a, b and c are required to balance the equation ...
aAl_(s) + bCl_2(g) ==> cAlCl_3(s) ? [eq-38]
1. 1 3 1
2. 2 3 2
3. 2 2 3
4. 1 3 2
Which three quantities a, b and c are required to balance the equation ...
aCa_(s) + bCl_2(g) ==> cCaCl_2(s) ? [eq-39]
1. 1 2 1
2. 1 1 2
3. 1 1 1
4. 2 2 1
Which three quantities a, b and c are required to balance the equation ...
aP_(s) + bCl_2(g) ==> cPCl_5(s) ? [eq-40]
1. 1 5 1
2. 1 5 2
3. 2 5 4
4. 2 5 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe₂O_3(s) + bCO_(g) ==> cFe_(l) + dCO_2(g) ? eq-41]
1. 1 3 2 3
2. 1 6 2 6
3. 2 6 4 3
4. 2 3 4 6
Which four quantities a, b, c and d are required to balance the equation ...
aCuO_(s) + bH_2(g) ==> cCu_(l) + dH₂O_(g) ? [eq-42]
1. 2 1 1 1
2. 1 1 1 1
3. 1 2 2 1
4. 2 1 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aCuO_(s) + bC_(s) ==> cCu_(s) + dCO_2(g) ? [eq-43]
1. 1 2 1 2
2. 2 2 2 1
3. 2 1 2 1
4. 1 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe₃O_4(s) + bC_(s) ==> cFe_(l) + dCO_2(g) ? [eq-44]
1. 2 1 3 2
2. 1 3 2 1
3. 2 1 2 1
4. 1 2 3 2
Which four quantities a, b, c and d are required to balance the equation ...
aNaOH_(aq) + bHCl_(aq) ==> cNaCl_(aq) + dH₂O_(l) ? [eq-45]
1. 1 1 1 1
2. 1 2 2 1
3. 2 1 1 2
4. 1 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aCa(OH)_2(aq) + bHCl_(aq) ==> cCaCl_2(aq) + dH₂O_(l) ? [eq-46]
1. 1 2 1 1
2. 1 2 1 2
3. 2 1 1 2
4. 2 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aAl(OH)_3(s) + bHCl_(aq) ==> cAlCl_3(aq) + dH₂O_(l) ? [eq-47]
1. 2 6 2 3
2. 1 6 2 6
3. 1 3 1 3
4. 2 3 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aFe₂O_3(s) + bHCl_(aq) ==> cFeCl_3(aq) + dH₂O_(l) ? [eq-48]
1. 2 6 2 3
2. 1 6 2 6
3. 1 3 1 3
4. 1 6 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aMgO_(s) + bHCl_(aq) ==> cMgCl_2(aq) + dH₂O_(l) ? [eq-49]
1. 1 2 1 1
2. 1 1 1 1
3. 2 2 1 2
4. 1 4 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aMg(OH)_2(s) + bH₂SO_4(aq) ==> cMgSO_4(aq) + dH₂O_(l) ? [eq-50]
1. 1 2 1 1
2. 1 1 1 2
3. 2 2 1 2
4. 1 4 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aLi₂O_(s) + bHCl_(aq) ==> cLiCl_(aq) + dH₂O_(l) ? [eq-51]
1. 1 2 1 1
2. 1 1 1 1
3. 1 2 2 1
4. 1 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aKOH_(aq) + bH₂SO_4(aq) ==> cK₂SO_4(aq) + dH₂O_(l) ? [eq-52]
1. 1 2 1 1
2. 1 1 1 1
3. 2 2 1 2
4. 2 1 1 2
Which electron arrangement is a Halogen? [as-5]
1. electron arrangement W
2. electron arrangement X
3. electron arrangement Y
4. electron arrangement Z
Which electron arrangement corresponds to the most reactive metal? [as-6]
1. electron arrangement W
2. electron arrangement X
3. electron arrangement Y
4. electron arrangement Z
Which electron arrangement corresponds to the first element on period 2 of the Periodic Table? [as-8]
1. electron arrangement W
2. electron arrangement X
3. electron arrangement Y
4. electron arrangement Z
Which electron arrangement corresponds to the most reactive non-metallic element of the Periodic Table? [as-9]
1. electron arrangement W
2. electron arrangement X
3. electron arrangement Y
4. electron arrangement Z
Which electron arrangement corresponds to a metal in Group 3 of the Periodic Table? [as-10]
1. electron arrangement W
2. electron arrangement X
3. electron arrangement Y
4. electron arrangement Z
Which electron arrangements correspond to two elements in the same Group of the Periodic Table? [as-11]
1. electron arrangement W and X
2. electron arrangements X and Z
3. electron arrangement Y and Z
4. electron arrangement W and Z
Which electron arrangements correspond to two elements on the same period of the Periodic Table? [as-13]
1. electron arrangement W and X
2. electron arrangements X and Z
3. electron arrangement Y and Z
4. electron arrangement W and Z
Which of the elements listed has 1 outer electron? [as-19]
1. element Q
2. element R
3. element Z
4. element G
Which of the elements listed is a Halogen? [as-20]
1. element Q
2. element R
3. element Z
4. element G
Which of the elements listed is an Alkali Metal? [as-21]
1. element Q
2. element R
3. element Z
4. element G
Which of the elements listed would be chemically the most similar? [as-22]
1. elements Q and R
2. elements R and A
3. elements M and X
4. elements G and M
Which of the elements listed are in the same period? [as-23]
1. elements Q and R
2. elements R and A
3. elements M and X
4. elements G and M
Which of the elements listed are both Halogen non-metals with 7 outer electrons? [as-25]
1. elements Z and Y
2. elements Q and R
3. elements G and E
4. elements T and W
Which of the elements listed are both in Group 3? [as-26]
1. elements Z and Y
2. elements Q and E
3. elements G and E
4. elements D and Y
Which of the elements listed are both Noble Gases? [as-27]
1. elements Z and T
2. elements Q and R
3. elements G and E
4. elements T and W
The nucleus of an atom consists of? [as-28]
1. protons and neutrons
2. neutrons and electrons
3. protons and electrons
4. protons only
The Atomic Number of an element is? [as-29]
1. the number of neutrons in the nucleus
2. the sum of the protons and neutrons in the nucleus
3. the number of protons in the nucleus
4. the number of electrons in the outer shell
The Mass Number of an element is? [as-30]
1. the number of neutrons in the nucleus
2. the sum of the protons and neutrons in the nucleus
3. the number of protons in the nucleus
4. the number of electrons in the outer shell
Which description corresponds to a neutron? [as-31]
1. mass = ¹/₁₈₅₀, electric charge = -1
2. mass = 1, electric charge = 0
3. mass = 1, electric charge = +1
4. mass = 4, electric charge = +2
Which description corresponds to a proton? [as-32]
1. mass = ¹/₁₈₅₀, electric charge = -1
2. mass = 1, electric charge = 0
3. mass = 1, electric charge = +1
4. mass = 4, electric charge = +2
Which description corresponds to a electron? [as-36]
1. mass = ¹/₁₈₅₀, electric charge = -1
2. mass = 1, electric charge = 0
3. mass = 1, electric charge = +1
4. mass = 4, electric charge = +2
Which is an electron arrangement of an element in Group 5 of the Periodic Table? [as-37]
1. 2.5
2. 2.7
3. 2.8.8
4. 2.8.8.1
Which is an electron arrangement of a Halogen? [as-38]
1. 2.5
2. 2.7
3. 2.8.8
4. 2.8.8.1
Which is the electron arrangement of a Noble Gas? [as-39]
1. 2.5
2. 2.7
3. 2.8.8
4. 2.8.8.1
Which is the electron arrangement of an Alkali Metal? [as-40]
1. 2.5
2. 2.7
3. 2.8.8
4. 2.8.8.1
Which is an electron arrangement of a Noble Gas? [as-41]
1. 2
2. 2.3
3. 2.8.5
4. 2.8.8.2
Which is an electron arrangement of a Period 1 element? [as-42]
1. 2
2. 2.3
3. 2.8.7
4. 2.8.8.1
Which is an electron arrangement of a Period 2 element? [as-43]
1. 2
2. 2.3
3. 2.8.6
4. 2.8.8.2
Which is an electron arrangement of a Group 3 element? [as-44]
1. 2
2. 2.3
3. 2.8.5
4. 2.8.8.2
Which is an electron arrangement of a Group 5 element? [as-45]
1. 2
2. 2.3
3. 2.8.5
4. 2.8.8.2
Which is an electron arrangement of a Period 3 element? [as-46]
1. 2.1
2. 2.3
3. 2.8.5
4. 2.8.8.2
Which is an electron arrangement of a Group 2 element? [as-47]
1. 2
2. 2.3
3. 2.8.6
4. 2.8.8.2
Which is an electron arrangement of a Period 4 element? [as-48]
1. 2
2. 2.4
3. 2.2
4. 2.8.8.2
How many protons does this sodium atom have? [as-1]
1. 11
2. 12
3. 23
4. 44
How many neutrons does this sodium atom have? [as-2]
1. 11
2. 12
3. 23
4. 44
How many neutrons plus protons does this atom have in total? [as-3]
1. 11
2. 12
3. 23
4. 44
How many electrons does this atom have in total? [as-4]
1. 11
2. 12
3. 23
4. 44
Which electron arrangement most likely corresponds to a non-metallic element? [as-7]
1. electron arrangement W
2. electron arrangement X
3. electron arrangement Y
4. electron arrangement Z
Which electron arrangements corresponds to two very reactive metallic elements of the Periodic Table? [as-12]
1. electron arrangements W and X
2. electron arrangements X and Z
3. electron arrangements Y and Z
4. electron arrangements W and Z
Which of the following have/has no neutrons? [as-14]
1. V only
2. V and Y
3. W and Y
4. Y and Z
Which of the following have/has one neutron? [as-15]
1. V only
2. W and Y
3. X and Y
4. Y and Z
Which of the following have/has two neutrons? [as-16]
1. V only
2. W and Y
3. X and Z
4. W and X
Which of the following have/has one proton? [as-17]
1. V only
2. W and Y
3. Y and Z
4. V, W and X
Which of the following have/has two protons? [as-18]
1. V only
2. X and Z
3. Y and Z
4. V, W and X
Which elements are both likely to be metals? [as-24]
1. elements Z and Y
2. elements Q and R
3. elements G and E
4. elements T and W
Which of the two particles W, X, Y and Z represent different isotopes of the same element? [as-33]
... Particle W: 12 protons, 14 neutrons, 12 electrons
... Particle X: 13 protons, 14 neutrons, 14 electrons
... Particle Y: 14 protons, 13 neutrons, 14 electrons
... Particle Z: 14 protons, 14 neutrons, 12 electrons
1. W and X
2. X and Y
3. X and Z
4. Y and Z
The symbol for an isotope of sodium is .
Which gives the correct numbers of protons, neutrons and electrons in this atom? [as-34]
1. 11 protons, 13 neutrons, 11 electrons
2. 13 protons, 11 neutrons, 11 electrons
3. 24 protons, 12 neutrons, 13 electrons
4. 24 protons, 13 neutrons, 24 electrons
Which of the following could be the symbol for a proton particle? [as-35]
1. symbol Q
2. symbol W
3. symbol Y
4. symbol Z
The symbol of an isotope of cobalt is .
Which gives the correct numbers of protons, neutrons and electrons in this atom? [as-49]
1. 27 protons, 33 neutrons, 27 electrons
2. 33 protons, 27 neutrons, 27 electrons
3. 60 protons, 33 neutrons, 60 electrons
4. 27 protons, 33 neutrons, 33 electrons
The symbol of an isotope of iron is .
Which gives the correct numbers of protons, neutrons and electrons in this atom? [as-50]
1. 31 protons, 26 neutrons, 31 electrons
2. 26 protons, 31 neutrons, 26 electrons
3. 26 protons, 26 neutrons, 31 electrons
4. 31 protons, 31 neutrons, 26 electrons
The symbol for an atom of strontium is .
What is the atomic number of the atom? [as-51]
1. 52
2. 128
3. 38
4. 90
The symbol for an atom of strontium is .
What is the mass number of the atom? [as-52]
1. 52
2. 128
3. 38
4. 90
The symbol for an atom of strontium is .
What is the proton number of the atom? [as-53]
1. 38
2. 90
3. 52
4. 128
The symbol for an atom of strontium is .
What is the neutron number of the atom? [as-54]
1. 38
2. 52
3. 90
4. 128
Chlorine consists of 75% chlorine-35 and 25% chlorine-37. Calculate the A_r of chlorine to 3sf/1dp. [ram-1]
1. 35.5
2. 35.0
3. 36.0
4. 35.6
Bromine consists of the isotopes: 50.5% Br-79 and 49.5% Br-81. Calculate the relative atomic mass, A_r, of bromine to 3sf/1dp. [ram-2]
1. 80.1
2. 80.0
3. 79.9
4. 79.8
Lithium consists of 7.4% lithium-6 and 92.6% lithium-7. Calculate the relative atomic mass, A_r, of lithium to 2sf/1dp. [ram-3]
1. 6.5
2. 6.7
3. 6.9
4. 6.6
Boron is 19.7% B-10 and 80.3% B-11. Calculate the relative atomic mass, A_r, of boron to 3sf/1dp. [ram-4]
1. 10.5
2. 10.9
3. 10.3
4. 10.8
Antimony (Sb) is 57.2% Sb-121 and 42.8% Sb-123. Calculate the A_r of Sb to 4sf/1dp. [ram-5]
1. 121.9
2. 122.0
3. 122.1
4. 121.2
Chromium has four stable isotopes. 4.31% Cr-50, 83.76% Cr-52, 9.55% Cr-53 and 2.38% Cr-54. Calculate the relative atomic mass, A_r, of chromium to 3sf/1dp. [ram-6]
1. 52.3
2. 52.1
3. 52.2
4. 52.5
Copper consists of 69.1% Cu-63 and 30.9% Cu-65. Calculate the relative atomic mass, A_r, of copper to 3sf/1dp. [ram-7]
1. 64.0
2. 63.3
3. 63.6
4. 64.5
Europium consists of 47.8% Eu-151 and 52.2% Eu-153. Calculate A_r(Eu) to 4sf/1dp. [ram-8]
1. 151.9
2. 152.2
3. 151.5
4. 152.0
Gallium is made up of 60.2% gallium-69 and 39.8% of gallium-71. Calculate the A_r of gallium to 3sf/1dp. [ram-9]
1. 69.8
2. 70.0
3. 69.9
4. 69.5
Iron has four stable isotopes.
5.8% Fe-54, 91.7% Fe-56, 2.2% Fe-57 and 0.3% Fe-58. Calculate the A_r of iron to 3sf/1dp. [ram-10]
1. 56.2
2. 55.9
3. 56.3
4. 56.1
Magnesium consists of 78.6% ²⁴Mg, 10.1% ²⁵Mg and 11.3% of ²⁶Mg. Calculate the relative atomic mass, A_r, of magnesium to 3sf/1dp. [ram-11]
1. 25.0
2. 24.7
3. 24.3
4. 24.1
Neon consists of 90.9% ²⁰Ne, 0.3% ²¹Ne and 8.8% ²²Ne. Calculate the relative atomic mass, A_r, of neon to 3sf/1dp. [ram-12]
1. 20.5
2. 20.1
3. 20.3
4. 20.2
Rhenium (Re) consists of 37.1% ¹⁸⁵Re and 62.9% ¹⁸⁷Re. Calculate the relative atomic mass, A_r, of rhenium to 4sf/1dp. [ram-13]
1. 186.3
2. 186.0
3. 185.6
4. 185.5
Rubidium consists of the stable isotopes: ⁸⁵Rb (72.2%) and ⁸⁷Rb (27.8%). Calculate A_r(Rb) to 3sf/1dp. [ram-14]
1. 86.0
2. 85.6
3. 85.9
4. 85.5
Thallium consists of 29.5% thallium-203 and 70.5% thallium-205. Calculate the relative atomic mass, A_r, of to 4sf/1dp. [ram-15]
1. 204.0
2. 204.2
3. 204.4
4. 204.1
Given the following relative atomic masses: Cu = 64, S = 32 and O = 16; calculate the relative formula mass of copper sulfate, CuSO₄ [rfm-1]
1. 160
2. 112
3. 96
4. 336
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of ethane, C₂H₆ [rfm-2]
1. 13
2. 30
3. 18
4. 25
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of octane, C₈H₁₈ [rfm-3]
1. 13
2. 96
3. 114
4. 112
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of nitric acid, HNO₃ [rfm-4]
1. 31
2. 93
3. 62
4. 63
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of ammonium nitrate, NH₄NO₃ [rfm-5]
1. 80
2. 31
3. 90
4. 180
Given the following relative atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the relative formula mass of ammonium sulfate, (NH₄)₂SO₄ [rfm-6]
1. 63
2. 132
3. 216
4. 100
Given the following relative atomic masses: H = 1, O = 16 and S = 32; calculate the relative formula mass of sulfuric acid, H₂SO₄ [rfm-7]
1. 49
2. 194
3. 98
4. 66
Given the following relative atomic masses: O = 16, Al = 27 and S = 32; calculate the relative formula mass of aluminium sulfate, Al₂(SO₄)₃ [rfm-8]
1. 75
2. 315
3. 171
4. 342
Given the following relative atomic masses: H = 1 and Cl = 35.5, calculate the relative formula mass of hydrochloric acid, HCl [rfm-9]
1. 36.5
2. 18
3. 35.5
4. 37.5
Given the following relative atomic masses: Na = 23 and Cl = 35.5, calculate the relative formula mass of sodium chloride, NaCl [rfm-10]
1. 40
2. 58.5
3. 49.5
4. 35
Given the following relative atomic masses: Ca = 40 and Cl = 35.5, calculate the relative formula mass of calcium chloride, CaCl₂ [rfm-11]
1. 75.5
2. 151
3. 111
4. 146.5
Given the following relative atomic masses: H = 1, O = 16 and Mg = 24, calculate the relative formula mass of magnesium hydroxide, Mg(OH)₂ [rfm-12]
1. 41
2. 82
3. 42
4. 58
Given the following relative atomic masses: Al = 27 and Cl = 35.5, calculate the relative formula mass of aluminium chloride, AlCl₃ [rfm-13]
1. 133.5
2. 62.5
3. 187.5
4. 98
Given the following relative atomic masses: H = 1, O = 16 and Al = 27, calculate the relative formula mass of aluminium hydroxide, Al(OH)₃ [rfm-14]
1. 44
2. 78
3. 132
4. 46
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of glucose, C₆H₁₂O₆ [rfm-5]
1. 29
2. 40
3. 180
4. 90
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of ethanol ('alcohol'), C₂H₅OH [rfm-16]
1. 29
2. 23
3. 41
4. 46
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of ethanoic acid ('acetic acid'), CH₃COOH [rfm-17]
1. 60
2. 29
3. 84
4. 58
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(II) oxide, FeO [rfm-18]
1. 40
2. 72
3. 56
4. 16
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(III) oxide, Fe₂O₃ [rfm-19]
1. 72
2. 200
3. 160
4. 216
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of the iron oxide, Fe₃O₄ [rfm-20]
1. 72
2. 272
3. 174
4. 232
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of methane, CH₄ [rfm-21]
1. 16
2. 13
3. 52
4. 10
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of propane, C₃H₈ [rfm-22]
1. 13
2. 44
3. 99
4. 40
Given the following relative atomic masses: C = 12 and O = 16; calculate the relative molecular mass of carbon dioxide, CO₂ [rfm-23]
1. 28
2. 56
3. 44
4. 14
Given the following relative atomic masses: C = 12, O = 16 and Cu = 64; calculate the relative formula mass of copper carbonate, CuCO₃ [rfm-24]
1. 92
2. 276
3. 148
4. 124
Given the following relative atomic masses: C = 12, O = 16 and Ca = 40; calculate the relative formula mass of calcium carbonate, CaCO₃ [rfm-25]
1. 100
2. 68
3. 204
4. 124
If 54g of aluminium combines with oxygen to form 102g of aluminium oxide, work out the formula of aluminium oxide. (Relative atomic masses: Al = 27 and O = 16) [emp-1]
1. Al₂O₃
2. Al₂O
3. AlO₂
4. AlO₃
In an experiment, 56g of iron combined with exactly 64g of sulfur. Work out the formula of the iron sulfide formed. (Relative atomic masses: Fe = 56 and S = 32) [emp-2]
1. FeS
2. FeS₂
3. Fe₂S
4. FeS₃
In an experiment, 21g of lithium combined with exactly 14g of nitrogen. Work out the formula of lithium nitride. (Relative atomic masses: Li = 7 and N = 14) [emp-3]
1. LiN₂
2. Li₂N
3. Li₃N
4. LiN₃
If 168g of iron combined with oxygen to form 232g of an iron oxide, work out the formula of the iron oxide. (Relative atomic masses: Fe = 56 and O = 16) [emp-4]
1. FeO
2. FeO₂
3. Fe₂O₃
4. Fe₃O₄
If 28g of silicon combined with oxygen to form 60g of silicon oxide, work out the formula of silicon oxide. (Relative atomic masses: Si = 28 and O = 16) [emp-5]
1. SiO₂
2. SiO
3. Si₂O
4. SiO₃
In an experiment, heating 128g of copper combined with exactly 32g of sulfur. Work out the formula of the copper sulfide formed. (Relative atomic masses: Cu = 64 and S = 32) [emp-6]
1. CuS
2. Cu₂S
3. CuS₂
4. CuS₄
In an experiment, excess chlorine was passed over 24g of heated magnesium metal until all the metal had reacted. If 95g of white magnesium chloride solid was formed, work out the formula of magnesium chloride. (Relative atomic masses: Mg = 24 and Cl = 35.5) [emp-7]
1. MgCl
2. Mg₂Cl
3. MgCl₂
4. MgCl₃
In an experiment, excess chlorine was passed over 27g of heated aluminium metal until all the metal had reacted. If 133.5g of white aluminium chloride was formed work out the formula of aluminium chloride. (Relative atomic masses: Al = 27 and Cl = 35.5) [emp-8]
1. Al₃Cl
2. AlCl₂
3. AlCl₄
4. AlCl₃
In an experiment, excess chlorine was passed over 28g of heated silicon until all of it had reacted. If 170g of liquid silicon chloride was formed work out the formula of silicon chloride. (Relative atomic masses: Si = 28 and Cl = 35.5) [emp-9]
1. SiCl₄
2. SiCl₂
3. Si₂Cl
4. Si₄Cl
In an experiment, excess chlorine was passed over 31g of hot phosphorus until all of it had reacted. If 208.5g of white phosphorus chloride was formed work out the formula of phosphorus chloride. (Relative atomic masses: P = 31 and Cl = 35.5) [emp-10]
1. PCl₃
2. PCl₅
3. PCl₆
4. PCl₇
If 8g of sulfur combines with 12g of oxygen, what is the formula of the sulfur oxide formed? (Relative atomic masses: S = 32 and O = 16) [emp-11]
1. SO
2. SO₂
3. SO₃
4. SO₄
If 16g of sulfur combines with 103.5g of lead, what is the formula of the lead sulfide formed? (Relative atomic masses: S = 32 and Pb = 207) [emp-12]
1. Pb₂S
2. PbS₂
3. PbS₆
4. PbS
If 40g of calcium combines with 160g of bromine, what is the formula of calcium bromide? (Relative atomic masses: Ca = 40 and Br = 80) [emp-13]
1. CaBr₂
2. CaBr
3. CaBr₃
4. Ca₂Br
78g of potassium combines with 160g of bromine. What is the simplest formula of potassium bromide? (Relative atomic masses: K = 39 and Br = 80) [emp-14]
1. KBr₂
2. KBr
3. K₂Br
4. KBr₄
48g of magnesium combines with 320g of bromine, what is the formula of magnesium bromide? (Relative atomic masses: Mg = 24 and Br = 80) [emp-15]
1. MgBr
2. Mg₂Br
3. MgBr₂
4. MgBr₃
160g of calcium combines with 64g of oxygen, what is the formula of calcium oxide? (Relative atomic masses: Ca = 40 and O = 16) [emp-16]
1. CaO₂
2. Ca₂O
3. Ca₄O₄
4. CaO
What is the formula of the phosphorus oxide formed when 62g of phosphorus combines with 80g of oxygen? (Relative atomic masses: P = 31 and O = 16) [emp-17]
1. P₂O₅
2. PO
3. P₂O
4. PO₅
72g of magnesium combines with 48g of oxygen, what is the formula of magnesium oxide? (Relative atomic masses: Mg = 24 and O = 16) [emp-18]
1. MgO₂
2. MgO
3. Mg₃O₃
4. Mg₂O
46g of sodium combined with 16g of oxygen. What is the formula of the sodium oxide formed? (Relative atomic masses: Na = 23 and O = 16) [emp-19]
1. NaO
2. NaO₂
3. Na₂O
4. Na₂O₂
78g of potassium combined with 32g of sulfur. What is the formula of potassium sulfide formed? (Relative atomic masses: K = 39 and S = 32) [emp-20]
1. KS
2. KS₂
3. K₂S₂
4. K₂S
56g of iron combined with 240g of bromine. What is the formula of the iron bromide formed? (Relative atomic masses: Fe = 56 and Br = 80) [emp-21]
1. FeBr₃
2. FeBr₂
3. Fe₃Br
4. FeBr
If 20.9g of bismuth combines with 24.0g of bromine, what is the formula of the bismuth bromide formed? (Relative atomic masses: Bi = 209 and Br = 80) [emp-22]
1. BiBr
2. BiBr₃
3. Bi₃Br
4. BiBr₂
If 54g of aluminium combines with 96g of sulfur, what is the formula of aluminium sulfide? (Relative atomic masses: Al = 27 and S = 32) [emp-23]
1. AlS
2. AlS₃
3. Al₂S₃
4. Al₂S
When 117g of potassium combines with 31g of phosphorus, what is the formula of the potassium phosphide formed? (Relative atomic masses: K = 39 and P = 31) [emp-24]
1. KP
2. KP₃
3. KP₂
4. K₃P
Given the following symbol equation:
2Mg + O₂ ==> 2MgO
Calculate how many g of magnesium oxide is formed by burning 24g of magnesium in air.
(Relative atomic masses, A_r: Mg = 24 and O = 16) [com-1]
1. 40
2. 16
3. 20
4. 80
Given the following symbol equation:
2Mg + O₂ ==> 2MgO
Calculate how many tonne of magnesium is needed to make 80 tonne of magnesium oxide.
(Relative atomic masses, A_r: Mg = 24 and O = 16) [com-2]
1. 96
2. 48
3. 24
4. 16
Given the following symbol equation:
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Calculate how many kg of calcium carbonate is needed to make 56 kg of calcium oxide.
(Relative atomic masses, A_r: Ca = 40, C = 12 and O = 16) [com-3]
1. 50
2. 44
3. 100
4. 40
Given the following symbol equation:
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Calculate how many g of carbon dioxide is formed if 25g of calcium carbonate is decomposed on heating to form 14g of calcium oxide.
(Relative atomic masses, A_r: Ca = 40, C = 12 and O = 16) [com-4]
1. 22
2. 44
3. 10
4. 11
Given the symbol equation to show the formation of iron sulfide:
Fe + S ==> FeS
Calculate the mass in g of iron sulfide formed when 5.6g of iron combines with 3.2g of sulfur.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-5]
1. 8.8
2. 2.4
3. 5.6
4. 3.2
Given the symbol equation to show the formation of iron sulfide:
Fe + S ==> FeS
Calculate the mass in g of iron sulfide formed when 28g of iron combines with 16g of sulfur.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-6]
1. 12
2. 44
3. 28
4. 16
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of calcium chloride formed when 20g of calcium combines with 35.5g of chlorine.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-7]
1. 15.5
2. 70.0
3. 55.5
4. 17.5
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of chlorine needed when 40g of calcium forms 111g of calcium chloride.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-8]
1. 80
2. 100
3. 151
4. 71
Given the symbol equation to show the formation of aluminium sulfide by heating a mixture of aluminium and sulfur:
2Al + 3S ==> Al₂S₃
How many g of sulfur is needed if 54g of aluminium is reacted to form 150g of aluminium sulfide?
(Relative atomic masses, A_r: Al = 27 and S = 32) [com-9]
1. 96
2. 204
3. 64
4. 27
Given the symbol equation to show the formation of aluminium sulfide by heating a mixture of aluminium and sulfur:
2Al + 3S ==> Al₂S₃
How many kg of sulfur is needed if 108kg of aluminium is reacted to form 300kg of aluminium sulfide?
(Relative atomic masses, A_r: Al = 27 and S = 32) [com-10]
1. 408
2. 192
3. 96
4. 32
Given the symbol equation to show the formation of iron sulfide by heating a mixture of iron and sulfur:
Fe + S ==> FeS
Calculate the mass in g of iron unreacted when 60g of iron reacts with 32g of sulfur to form 88g of iron sulfide.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-11]
1. 8
2. 32
3. 4
4. 56
Given the symbol equation to show the formation of iron sulfide by heating a mixture of iron and sulfur:
Fe + S ==> FeS
Calculate the mass in g of sulfur unreacted when 28g of iron reacts with 22g of sulfur to form 44g of iron sulfide.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-12]
1. 22
2. 16
3. 12
4. 6
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of calcium left unreacted when 25g of calcium reacts with 35.5g of chlorine.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-13]
1. 10.5
2. 5.0
3. 7.1
4. 12.5
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of chlorine left unreacted when 80g of calcium reacts with 150g of chlorine to form 222g of calcium chloride.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-14]
1. 70
2. 8
3. 16
4. 72
Given the equation: 2Mg_(s) + O_2(g) ==> 2MgO_(s)
and the atomic masses: Mg = 24, O = 16, how many g of magnesium is needed to make 10g of magnesium oxide? [rmc-1]
1. 6.0
2. 3.0
3. 1.2
4. 2.4
Given the equation: 2Mg_(s) + O_2(g) ==> 2MgO_(s)
and the atomic masses: Mg = 24, O = 16, how many tonne of magnesium oxide can be made from 3 tonne of magnesium? [rmc-2]
1. 2.4
2. 5.0
3. 8.0
4. 4.8
Given the equation: 2Mg_(s) + O_2(g) ==> 2MgO_(s)
and the atomic masses: Mg = 24, O = 16, what mass of oxygen in g, combines with 240g of magnesium? [rmc-3]
1. 64
2. 80
3. 160
4. 32
Iron sulfide can be made by heating an iron and sulfur mixture.
Fe_(s) + S_(s) ==> FeS_(s)
Given the atomic masses: Fe = 56, S = 32, how many g of iron sulfide can be made from 14g of iron? [rmc-4]
1. 44
2. 28
3. 16
4. 22
Iron sulfide can be made by heating an iron and sulfur mixture.
Fe_(s) + S_(s) ==> FeS_(s)
Given the atomic masses: Fe = 56, S = 32, how many g of sulfur reacts with 224g of iron? [rmc-5]
1. 128
2. 32
3. 64
4. 112
Iron sulfide can be made by heating an iron and sulfur mixture.
Fe_(s) + S_(s) ==> FeS_(s)
Given the atomic masses: Fe = 56, S = 32, how many g of iron is needed to make 440g of iron sulfide? [rmc-6]
1. 56
2. 280
3. 220
4. 168
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how many tonne of iron can be made from 40 tonnes of haematite ore? [rmc-7]
1. 56
2. 14
3. 28
4. 7
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how many tonne of haematite ore are needed to make 224 tonne of iron? [rmc-8]
1. 160
2. 480
3. 640
4. 320
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how g of carbon monoxide are needed to reduce 32g of iron oxide to iron? [rmc-9]
1. 16.8
2. 33.6
3. 8.4
4. 28.0
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how many g of carbon dioxide are formed when 80 g of haematite is reduced to iron? [rmc-10]
1. 44
2. 66
3. 33
4. 40
Lime (calcium oxide) is made by heating limestone (calcium carbonate).
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Given the atomic masses: Ca = 40, C = 12, O = 16, how many tonne of limestone is needed to make 112 tonne of lime? [rmc-11]
1. 224
2. 400
3. 200
4. 300
Lime (calcium oxide) is made by heating limestone (calcium carbonate).
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Given the atomic masses: Ca = 40, C = 12, O = 16, what mass in g of lime is made from 20g of limestone? [rmc-12]
1. 8.8
2. 5.6
3. 4.4
4. 11.2
Lime (calcium oxide) is made by heating limestone (calcium carbonate).
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Given the atomic masses: Ca = 40, C = 12, O = 16, how many tonne of carbon dioxide is formed by decomposing 400 tonne of calcium carbonate? [rmc-13]
1. 176
2. 44
3. 88
4. 132
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of zinc carbonate are needed to make 68g of zinc chloride?? [rmc-14]
1. 125.0
2. 62.5
3. 68.0
4. 136.0
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of HCl are needed to make 408g of zinc chloride? [rmc-15]
1. 109.5
2. 36.5
3. 219.0
4. 71.0
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, what mass of zinc chloride in g can be made from 25g of zinc carbonate? [rmc-16]
1. 54.4
2. 12.5
3. 13.6
4. 27.2
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of water are formed when 250g of zinc carbonate reacts? [rmc-17]
1. 36
2. 18
3. 9
4. 27
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of carbon dioxide are formed when 3.65g of hydrochloric acid reacts? [rmc-18]
1. 4.4
2. 2.2
3. 1.1
4. 8.8
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of sodium hydroxide is needed to make 213g of sodium sulfate? [rmc-19]
1. 40
2. 80
3. 120
4. 160
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, what mass in g of sulfuric acid is needed to make 7.1g of sodium sulfate? [rmc-20]
1. 9.8
2. 14.7
3. 19.6
4. 4.9
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of sodium sulfate is formed when 8g of sodium hydroxide reacts? [rmc-21]
1. 14.2
2. 28.4
3. 7.1
4. 21.3
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of water are formed when 49g of sulfuric acid reacts? [rmc-22]
1. 9
2. 18
3. 36
4. 23
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many g of copper can be made from 320g of the copper ore?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-23]
1. 128
2. 64
3. 256
4. 192
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many tonnes of oxygen are needed to convert 40 tonnes of ore to copper?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-24]
1. 16
2. 32
3. 12
4. 8
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many tonnes of sulfur dioxide are produced for every 1280 tonnes of ore processed?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-25]
1. 512
2. 128
3. 256
4. 64
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many tonnes of ore are needed to make 25.6 tonnes of copper?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-26]
1. 64
2. 32
3. 48
4. 56
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the hydrogen chloride reaction is:
2Al_(s) + 6HCl_(g) ==> 2AlCl_3(s) + 3H_2(g)
How many kg of aluminium chloride can be made from 27 kg of aluminium?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1.0) [rmc-27]
1. 267.0
2. 400.5
3. 133.5
4. 66.75
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the hydrogen chloride reaction is:
2Al_(s) + 6HCl_(g) ==> 2AlCl_3(s) + 3H_2(g)
How many tonnes of hydrogen would be produced by reacting 108 tonnes of aluminium?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1.0) [rmc-28]
1. 2
2. 3
3. 6
4. 12
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the chlorine reaction is:
2Al_(s) + 3Cl_2(g) ==> 2AlCl_3(s)
How much aluminium is needed to make 89 g of aluminium chloride?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H =1) [rmc-29]
1. 18
2. 27
3. 54
4. 9
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the chlorine reaction is:
2Al_(s) + 3Cl_2(g) ==> 2AlCl_3(s)
How many tonne of chlorine is needed to make 1068 tonne of aluminium chloride?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1) [rmc-30]
1. 71
2. 852
3. 426
4. 213
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many tonne of lead can be made from 223 tonne of ore?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-31]
1. 414.0
2. 103.5
3. 207.0
4. 310.5
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many tonne of ore is needed to make 828 tonne of lead?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-32]
1. 223
2. 446
3. 1784
4. 892
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many kg of carbon is needed to make 828 kg of lead?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-33]
1. 24
2. 12
3. 6
4. 48
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many g of carbon dioxide are formed when 207 g of lead are produced?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-34]
1. 44
2. 22
3. 11
4. 33
How many moles of iron are there in 2.8g? (atomic mass Fe = 56) [mam-1]
1. 0.05
2. 156.8
3. 20.0
4. 2.0
How many moles of sulfur are there in 64g? (atomic mass S = 32) [mam-2]
1. 2048
2. 2.0
3. 0.5
4. 0.05
How many moles of sodium are there in 115g? (atomic mass Na = 23) [mam-3]
1. 2645
2. 0.2
3. 5
4. 4
How many moles of carbon are there in 3g? (atomic mass C = 12 ) [mam-4]
1. 36
2. 4
3. 0.5
4. 0.25
How many moles of zinc are there in 1.625g? (atomic mass Zn = 65) [mam-5]
1. 0.025
2. 105.6
3. 40.0
4. 100.0
How many moles of iodine are there in 12.7g of I₂? (atomic mass I = 127) [mam-6]
1. 10.0
2. 0.05
3. 0.10
4. 5.0
How many moles of chlorine are there in 213g of Cl₂? (atomic mass Cl = 35.5) [mam-7]
1. 0.17
2. 0.33
3. 3.0
4. 6.0
How many moles of bromine are there in 6.4g of Br₂? (atomic mass Br = 80) [mam-8]
1. 512
2. 1024
3. 0.08
4. 0.04
How many moles of phosphorus are there in 24.8g of P₄? (atomic mass P = 31) [mam-9]
1. 0.2
2. 0.8
3. 7688
4. 1922
How many moles of oxygen are there in 128g of O₂? (atomic mass O = 16) [mam-10]
1. 8
2. 4
3. 2048
4. 1032
How many moles of water are there in 4.5g of H₂O? (atomic masses: H = 1, O = 16) [mam-11]
1. 81
2. 0.26
3. 0.25
4. 72
How many moles of methane are there in 112g of CH₄? (atomic masses: C = 12, H = 1) [mam-12]
1. 8.6
2. 1792
3. 0.14
4. 7.0
How many moles of sodium sulfate are there in 7.1g of Na₂SO₄? (atomic masses: Na = 23, S = 32, O = 16) [mam-13]
1. 0.05
2. 10082
3. 20
4. 5
How many moles of sulfuric acid are there in 2.45g of H₂SO₄? (atomic masses: H = 1, S = 32, O = 16) [mam-14]
1. 240.1
2. 0.025
3. 40.0
4. 3.0
How many moles of calcium hydroxide are there in 25.9g of Ca(OH)₂? (atomic masses: Ca = 40, O = 16, H = 1) [mam-15]
1. 2.86
2. 1916
3. 0.35
4. 45.0
How many g are there in 1.5 moles of aluminium? (atomic mass Al = 27) [mam-16]
1. 0.056
2. 18.0
3. 9.0
4. 40.5
How many g are there in 0.02 moles of uranium? (atomic mass U = 238) [mam-17]
1. 4.76
2. 11900
3. 0.00008
4. 2.58
How many g are there in 0.65 moles of magnesium? (atomic mass Mg = 24) [mam-18]
1. 0.027
2. 15.6
3. 36.9
4. 7.8
How many g are there in 0.23 moles of silicon? (atomic mass Si = 28) [mam-19]
1. 0.0082
2. 121.7
3. 6.44
4. 0.82
How many g are there in 7.3 moles of boron? (atomic mass B = 10.8) [mam-20]
1. 0.68
2. 1.48
3. 70.0
4. 78.84
How many g are there in 0.05 moles of nitrogen, N ₂? (atomic mass N = 14) [mam-21]
1. 1.4
2. 2.4
3. 0.0035
4. 280
How many g are there in 0.75 moles of ozone, O₃? (atomic mass O = 16) [mam-22]
1. 0.047
2. 36.0
3. 12.0
4. 0.016
How many g are there in 2.5 moles of oxygen, O₂? (atomic mass O = 16) [mam-23]
1. 4.0
2. 6.4
3. 80.0
4. 40.0
How many g are there in 0.16 moles of chlorine, Cl₂? (atomic mass Cl = 35.5) [mam-24]
1. 5.68
2. 221.8
3. 443.8
4. 11.36
How many g are there in 1.65 moles of iodine, I₂? (atomic mass I = 127) [mam-25]
1. 419.1
2. 77.0
3. 154.0
4. 209.6
How many g are there in 3.6 moles of sodium hydroxide, NaOH? (atomic masses: Na = 23, O = 16, H = 1) [mam-26]
1. 0.09
2. 144
3. 11.1
4. 7.2
How many g are there in 1.5 moles of nitric acid, HNO₃? (atomic masses: H = 1, N = 14, O = 16) [mam-27]
1. 42.0
2. 0.024
3. 94.5
4. 46.5
How many g are there in 0.15 moles of ammonium sulfate, (NH₄)₂SO₄? (atomic masses: N = 14, H = 1, S = 32, O = 16) [mam-28]
1. 0.0011
2. 880.0
3. 17.1
4. 19.8
How many g are there in 0.8 moles of aluminium hydroxide, Al(OH)₃? (atomic masses: Al = 27, O = 16, H = 1) [mam-29]
1. 62.4
2. 97.5
3. 0.01
4. 10.0
How many g are there in 0.005 moles of sodium thiosulfate, Na₂S₂O₃? (atomic masses: Na = 23, S = 32, O =16) [mam-30]
1. 0.71
2. 0.79
3. 0.63
4. 0.55
It was found that 0.2 moles of atoms of an element had a mass of 3.2g. What is the relative atomic mass of the element? [mam-31]
1. 6.4
2. 8.0
3. 16.0
4. 15.0
It was found that 0.005 moles of atoms of an element had a mass of 0.295g. What is the relative atomic mass of the element? [mam-32]
1. 15
2. 60
3. 16
4. 59
It was found that 0.15 moles of atoms of an element had a mass of 10.95g. What is the relative atomic mass of the element? [mam-33]
1. 73
2. 164
3. 82
4. 146
It was found that 0.4 moles of atoms of an element had a mass of 56.2g. What is the relative atomic mass of the element? [mam-34]
1. 22.5
2. 140.5
3. 224.0
4. 25.0
It was found that 0.015 moles of atoms of an element had a mass of 2.88g. What is the relative atomic mass of the element? [mam-35]
1. 432
2. 450
3. 192
4. 200
It was found that 0.25 moles of atoms of an element had a mass of 40.65g. What is the relative atomic mass of the element? [mam-36]
1. 10.2
2. 102.0
3. 16.0
4. 162.6
It was found that 0.002 moles of a compound had a mass of 0.24g. What is the relative formula mass of the compound? [mam-37]
1. 120
2. 12
3. 48
4. 480
It was found that 0.005 moles of a compound had a mass of 0.2025g. What is the relative formula mass of the compound? [mam-38]
1. 101.3
2. 40.5
3. 24.7
4. 247
It was found that 0.25 moles of a compound had a mass of 14.05g. What is the relative formula mass of the compound? [mam-39]
1. 177.8
2. 35.1
3. 56.2
4. 28.1
It was found that 0.025 moles of a compound had a mass of 0.70g. What is the relative formula mass of the compound? [mam-40]
1. 175
2. 280
3. 140
4. 28
0.55g of boron combined with 1.2g of oxygen. Deduce the empirical formula of boron oxide.
(relative atomic masses, A_r: B = 11, O = 16) [efm-1]
1. B₂O₃
2. BO
3. B₂O
4. BO₂
1.35g of aluminium was burned in excess fluorine to form 4.2g of aluminium fluoride. Deduce the empirical formula of aluminium fluoride.
(relative atomic masses, A_r: Al = 27, F = 19) [efm-2]
1. AlF
2. AlF₃
3. Al₃F
4. AlF₂
3.4g of an unusual carbon oxide contained 1.8g of carbon. Deduce the empirical formula of the carbon oxide.
(relative atomic masses, A_r: C=12, O=16) [efm-3]
1. CO
2. CO₂
3. C₃O₂
4. C₂O₃
In an experiment 3.175g of copper combined with 0.400g of oxygen. What is the empirical formula of the copper oxide?
(relative atomic masses, A_r: Cu = 63.5, O = 16) [efm-4]
1. CuO
2. CuO₂
3. Cu₂O₂
4. Cu₂O
8.875g of chlorine combined with 14.25g of fluorine. What is the formula of the chlorine fluoride?
(relative atomic masses, A_r: Cl = 35.5, F = 19) [efm-5]
1. ClF₃
2. Cl₃F
3. ClF
4. ClF₂
A gas formed by the combination of hydrogen and sulfur consisted of 5.88% hydrogen and 94.12% sulfur. What is its empirical formula?
(relative atomic masses, A_r: H = 1, S = 32) [efm-6]
1. HS
2. H₂S
3. HS₂
4. H₂S₂
5.08g of iodine combined with 1.6g of oxygen. What is the formula of the iodine oxide?
(relative atomic masses, A_r: I = 127, O = 16) [efm-7]
1. IO₅
2. I₂O
3. I₂O₅
4. I₂O₃
2.8g of lithium was heated in a stream of air forming 6.0g of lithium oxide. What is its formula?
(relative atomic masses, A_r: Li = 7, O =16) [efm-8]
1. LiO
2. LiO₂
3. LiO₃
4. Li₂O
A iron-copper sulfide ore consisted of 30.5% iron, 34.6% copper, and 34.9% sulfur. What is the empirical formula of the ore?
(relative atomic masses, A_r: Fe = 56, Cu = 63.5, S = 32) [efm-9]
1. FeCuS₂
2. FeCuS
3. FeCu₂S
4. Fe₂CuS₂
0.48g of magnesium combined with 3.20g of bromine. What is the formula of magnesium bromide?
(relative atomic masses, A_r: Mg = 24, Br = 80) [efm-10]
1. Mg₂Br
2. MgBr₂
3. MgBr
4. MgBr₃
0.7g of nitrogen combined with 5.325g of chlorine. Deduce the formula of nitrogen chloride.
(relative atomic masses, A_r: N = 14, Cl = 35.5) [efm-11]
1. NCl
2. NCl₂
3. NCl₃
4. N₃Cl
Fluorine oxide consists of 70.4% fluorine and 29.6% oxygen by mass. Deduce the formula of fluorine oxide.
(relative atomic masses, A_r: F = 19, O = 16) [efm-12]
1. FO
2. FO₂
3. FO₃
4. F₂O
47.6g of uranium combined with 22.8g of fluorine. What is the empirical formula of this uranium fluoride?
(relative atomic masses, A_r: U = 238, F = 19) [efm-13]
1. UF₆
2. UF₃
3. UF₂
4. UF₄
10.35g of lead was heated in excess oxygen. If 11.95g of a lead oxide was formed, deduce its empirical formula.
(relative atomic masses, A_r: Pb = 207, O = 16) [efm-14]
1. PbO
2. PbO₂
3. Pb₂O
4. PbO₃
10.8g of aluminium combined with 19.2g of sulfur. What is the empirical formula of aluminium sulfide?
(relative atomic masses, A_r: Al = 27, S = 32) [efm-15]
1. Al₃S₂
2. AlS₃
3. Al₂S₃
4. AlS₂
A hydrocarbon of molecular mass 30 consisted of 80% carbon and 20% hydrogen by mass. Deduce the molecular formula of the hydrocarbon.
(relative atomic masses, A_r: C = 12, H = 1) [efm-16]
1. CH₃
2. C₂H₃
3. CH₁₈
4. C₂H₆
6g of carbon combines with 71g of chlorine. What is the formula of the carbon chloride?
(relative atomic masses, A_r: C = 12, Cl = 35.5) [efm-17]
1. CCl₄
2. C₄Cl
3. CCl₂
4. C₂Cl
An organic compound consisted of 52.18% carbon, 13.04% hydrogen and 34.78% oxygen by mass. Deduce its empirical formula.
(relative atomic masses, A_r: C = 12, H = 1, O = 16) [efm-18]
1. CH₆O
2. C₂H₆O
3. C₂H₆O₂
4. CH₃O
An chlorinated hydrocarbon molecule consisted of 37.21% carbon, 7.75% hydrogen and 55.04% chlorine by mass. Deduce its empirical formula.
(relative atomic masses, A_r: C = 12, H = 1, Cl = 35.5) [efm-19]
1. C₂H₆Cl
2. CH₃Cl
3. C₂H₅Cl
4. C₂H₄Cl₂
A calcium mineral consisted of 29.4% calcium, 23.5% sulfur and 47.1% oxygen by mass. Calculate the empirical formula of the mineral.
(relative atomic masses, A_r: Ca = 40, S = 32, O = 16) [efm-20]
1. CaSO₂
2. CaSO₃
3. Ca₂SO₄
4. CaSO₄
A salt consisted of 27.06% sodium, 16.47% nitrogen and 56.47% oxygen by mass. Deduce the formula of the salt.
(relative atomic masses, A_r: Na = 23, N = 14, O = 16) [efm-21]
1. NaNO₃
2. NaNO₂
3. Na₂NO₃
4. NaNO
A brominated hydrocarbon consisted of 12.77% carbon, 2.13% hydrogen and 85.10% bromine by mass. If its molecular mass is 188, deduce the molecular formula of the molecule.
(relative atomic masses, A_r: C = 12, H = 1, Br =80) [efm-22]
1. CH₂Br
2. C₂H₄Br₂
3. CH₁₆Br₂
4. C₂H₆Br₂
It was found that 24g of carbon was combined with 5g of hydrogen in a hydrocarbon. If its molecular mass was 58, what is its molecular formula?
(relative atomic masses, A_r: C = 12, H = 1) [efm-23]
1. C₂H₅
2. C₃H₈
3. C₄H₁₀
4. C₃H₂₂
A hydrocarbon consisted of 92.3% carbon and 7.7% hydrogen. If its molecular mass is 78, work out its molecular formula.
(relative atomic masses, A_r: C = 12, H = 1) [efm-24]
1. C₅H₁₈
2. CH
3. CH₆
4. C₆H₆
A carbohydrate on analysis consisted of 40.00% carbon, 6.67% hydrogen and 53.33% oxygen. If its molecular mass is 180, deduce the molecular formula of the carbohydrate.
(relative atomic masses, A_r: C = 12, H = 1, O = 16) [efm-25]
1. C₆H₁₂O₆
2. CH₂O
3. C₅H₈O₇
4. C₃H₆O₃
7.75g of an alcohol consisted of 3.00g carbon, 0.75g hydrogen and 4.00g oxygen. If its molecular mass is 62, work out the molecular formula.
(relative atomic masses, A_r: C = 12, H = 1, O = 16) [efm-26]
1. C₃H₁₀O
2. C₂H₆O₂
3. CH₃O
4. C₂H₆O
An alcohol consisted of 39.13% carbon, 8.70% hydrogen and 52.17% oxygen. If its molecular mass is 92, deduce its molecular formula.
(relative atomic masses, A_r: C = 12, H = 1, O = 16) [efm-27]
1. CH₂O
2. C₃H₆O₃
3. C₃H₈O₃
4. C₂H₄O₄
In an experiment 6g of carbon combined with 19g of fluorine. Calculate the molecular formula of the compound formed if the molecular mass of it is 100.
(relative atomic masses, A_r: C = 12, F = 19) [efm-28]
1. CF₂
2. C₄F₂
3. CF₄
4. C₂F₄
A compound of hydrogen and oxygen was made up of 0.5g hydrogen and 8g of oxygen. What is its empirical formula?
(relative atomic masses, A_r: H = 1, O = 16) [efm-29]
1. HO
2. H₂O₂
3. H₂O
4. HO₂
A lithium compound consisted of 7g of lithium combined with 16g of sulfur and 32g of oxygen. What is the empirical formula of the compound?
(relative atomic masses, A_r: Li = 7, S = 32, O = 16) [efm-30]
1. LiSO₂
2. Li₂SO₄
3. LiSO₄
4. Li₂SO₃
58g of a sodium phosphate salt consisted of 34.5g of sodium, 15.5g of phosphorus and 32.0g of oxygen. What is the simplest formula of the compound?
(relative atomic masses, A_r: Na = 23, P = 31, O = 16) [efm-31]
1. Na₄PO₃
2. Na₂PO₄
3. Na₃PO₄
4. Na₂PO₃
A sodium compound consisted of 46g of sodium combined with 254g of iodine and 128g of oxygen. What is the compounds empirical formula?
(relative atomic masses, A_r: Na = 23, I = 127, O = 16) [efm-32]
1. NaIO₃
2. NaIO₂
3. Na₂IO₄
4. NaIO₄
16g of copper, after heating in oxygen, formed 20g of a copper oxide. What is the formula of the oxide?
(relative atomic masses, A_r: Cu = 64, O = 16) [efm-33]
1. CuO
2. CuO₂
3. Cu₂O
4. CuO₃
An oxide of carbon consisted of 3g of carbon combined with 4g of oxygen. What is the formula of the oxide?
(relative atomic masses, A_r: C = 12, O = 16) [efm-34]
1. CO₂
2. CO
3. C₂O4
4. C₂O
1.95g of potassium combined with 4.00g of bromine. What is the empirical formula of the compound?
(relative atomic masses, A_r: K = 39, Br = 80) [efm-35]
1. K₂Br
2. KBr₂
3. KBr
4. KBr₃
5g of calcium on heating in oxygen formed 7g of calcium oxide. What is the simplest formula of calcium oxide?
(relative atomic masses, A_r: Ca = 40, O = 16) [efm-36]
1. CaO₂
2. Ca₂O
3. CaO₃
4. CaO
13g of zinc combined with 6.4g of sulfur. What is the empirical formula of zinc sulfide?
(relative atomic masses, A_r: Zn = 65, S = 32) [efm-37]
1. ZnS
2. ZnS₂
3. Zn₂S
4. ZnS₃
An oxide of copper contained 80% copper and 20% oxygen by mass. What is the formula of the copper oxide?
(relative atomic masses, A_r: Cu = 64, O = 16) [efm-38]
1. Cu₂O
2. CuO
3. CuO₂
4. CuO₃
If magnesium oxide consists of 60% magnesium and 40% oxygen, what is its simplest formula?
(relative atomic masses, A_r: Mg = 24, O = 16) [efm-39]
1. Mg₂O
2. MgO₂
3. MgO
4. MgO₃
2.3g of sodium combined with 1.6g of sulfur. What is the formula of sodium sulfide?
(relative atomic masses, A_r: Na = 23, S = 32) [efm-40]
1. NaS
2. NaS₂
3. NaS₃
4. Na₂S
In an experiment 1.28g of copper combined with 0.16g of oxygen. What is the formula of the copper oxide?
(relative atomic masses, A_r: Cu = 64, O = 16) [efm-41]
1. Cu₂O
2. CuO
3. CuO₂
4. CuO₃
13.8g of sodium combined with 6.2g of phosphorus. What is the formula of sodium phosphide?
(relative atomic masses, A_r: Na = 23, P = 31) [efm-42]
1. NaP
2. Na₃P
3. NaP₂
4. Na₂P
10g of calcium combined with 40g of bromine. What is the formula of calcium bromide?
(relative atomic masses, A_r: Ca = 40, Br = 80) [efm-43]
1. CaBr
2. Ca₂Br
3. CaBr₂
4. CaBr₃
22g of boron combined with 114g of fluorine. What is the empirical formula of boron fluoride?
(relative atomic masses, A_r: B = 11, F = 19) [efm-44]
1. BF
2. BF₂
3. B₃F
4. BF₃
1.2g of titanium, after heating in oxygen, formed 2.0g of a titanium oxide. What is the empirical formula for the titanium oxide?
(relative atomic masses, A_r: Ti = 48, O = 16) [efm-45]
1. TiO₂
2. TiO
3. Ti₂O
4. TiO₃
0.800g of magnesium reacted with 8.47g of iodine. Calculate the empirical formula for magnesium iodide.
(relative atomic masses, A_r: Mg = 24, I = 127) [efm-46]
1. MgI
2. MgI₂
3. Mg₂I
4. MgI₃
Which substance is likely to have a simple molecular structure? [cb-1]
1. melts at 17^oC, insoluble in water, non-conductor of electricity either when solid or molten
2. melts at 670^oC, dissolves in water, non-conductor of electricity when molten, undergoes electrolysis in aqueous solution
3. melts at 2600^oC, dissolves in water, non-conductor of electricity when solid, undergoes electrolysis in aqueous solution
4. melts at 1400^oC, insoluble in water, good conductor of electricity either when solid or molten
Which substance is likely to have a giant ionic structure? [cb-2]
1. melts at 17^oC, insoluble in water, non-conductor of electricity either when solid or molten
2. melts at 2800^oC, insoluble in water, non-conductor of electricity when molten or solid
3. melts at 2600^oC, dissolves in water, non-conductor of electricity when solid, undergoes electrolysis in aqueous solution
4. melts at 1400^oC, insoluble in water, good conductor of electricity either when solid or molten
Which substance is likely to have a metallic structure? [cb-3]
1. melts at 17^oC, insoluble in water, non-conductor of electricity either when solid or molten
2. melts at 2800^oC, insoluble in water, non-conductor of electricity when molten or solid
3. melts at 2600^oC, dissolves in water, non-conductor of electricity when solid, undergoes electrolysis in aqueous solution
4. melts at 1400^oC, insoluble in water, good conductor of electricity either when solid or molten
Which substance is likely to have a giant covalent structure? [cb-4]
1. melts at 17^oC, insoluble in water, non-conductor of electricity either when solid or molten
2. melts at 2800^oC, insoluble in water, non-conductor of electricity when molten or solid
3. melts at 2600^oC, dissolves in water, non-conductor of electricity when solid, undergoes electrolysis in aqueous solution
4. melts at 1400^oC, insoluble in water, good conductor of electricity either when solid or molten
Which substance is likely to have a simple molecular structure but form ions in aqueous solution? [cb-5]
1. melts at 17^oC, reacts with water, non-conductor of electricity either when solid, molten or in water
2. melts at 370^oC, dissolves in water, non-conductor of electricity when molten or solid, solution conducts electricity
3. melts at 2600^oC, dissolves in water, non-conductor of electricity when solid, undergoes electrolysis in aqueous solution
4. melts at 1400^oC, insoluble in water, good conductor of electricity either when solid or molten
A solution of sodium chloride conducts electricity because the? [cb-6]
1. current breaks down sodium chloride into sodium ions and chloride ions
2. ions formed from the water carry the current
3. sodium ions and chloride ions are free to move and carry the current
4. the free moving water molecules are good conductors
An atom can turn into an ion if it? [cb-7]
1. gains an electron
2. loses a proton
3. gains a neutron
4. loses a neutron
An atom can turn into an ion if it? [cb-8]
1. gains a proton
2. loses a proton
3. gains a neutron
4. loses an electron
When a covalent bond is formed between atoms of different elements ? [cb-9]
1. electrons are shared
2. electrons are transferred
3. protons are shared
4. protons are transferred
When an ionic bond is formed between atoms of different elements? [cb-10]
1. electrons are shared
2. electrons are transferred
3. protons are shared
4. protons are transferred
Metal atoms form ions with a positive charge by? [cb-11]
1. gaining protons
2. gaining electrons
3. losing electrons
4. losing protons
Non-metal atoms form ions with a negative charge by? [cb-12]
1. gaining protons
2. gaining electrons
3. losing electrons
4. losing protons
Atoms of Group 7 of the Periodic Table are most likely to form ions with? [cb-13]
1. a single negative charge by gaining one electron
2. a single positive charge by losing one electron
3. a double negative charge by gaining two electrons
4. a double positive charge by losing two electrons
Atoms of Group 1 of the Periodic Table are most likely to form ions with? [cb-14]
1. a single negative charge by gaining one electron
2. a single positive charge by losing one electron
3. a double negative charge by gaining two electrons
4. a double positive charge by losing two electrons
Atoms of Group 6 of the Periodic Table are most likely to form ions with [cb-15]
1. a single negative charge by gaining one electron
2. a single positive charge by losing one electron
3. a double negative charge by gaining two electrons
4. a double positive charge by losing two electrons
Atoms of Group 2 of the Periodic Table are most likely to form ions with? [cb-16]
1. a single negative charge by gaining one electron
2. a single positive charge by losing one electron
3. a double negative charge by gaining two electrons
4. a double positive charge by losing two electrons
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 1, with a non-metal X from Group 7 of the Periodic Table? [cb-17]
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 1, with a non-metal X from Group 6 of the Periodic Table? [cb-18]
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 2, with a non-metal X from Group 6 of the Periodic Table? [cb-19]
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 2, with a non-metal X from Group 7 of the Periodic Table? [cb-20]
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 3, with a non-metal X from Group 6 of the Periodic Table? [cb-21]
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 3, with a non-metal X from Group 7 of the Periodic Table? [cb-22]
Which of the following substances consists of an ionic lattice? [cb-23]
1. high melting point, solid doesn't conduct electricity, aqueous solution conducts electricity
2. high melting point, solid conducts electricity, insoluble in water
3. low melting point, solid conducts electricity, insoluble in water
4. low melting point, solid doesn't conduct electricity, aqueous solution doesn't conduct electricity
What is an ion? [cb-24]
1. an atom which has lost or gained electrons
2. a negatively charged particle in the shells of an atom
3. an uncharged particle in the nucleus of an atom
4. a positively charged particle in the nucleus of an atom
Which of the following substances consists of a metal lattice? [cb-25]
1. high melting point, solid doesn't conduct electricity, aqueous solution conducts electricity
2. high melting point, solid conducts electricity, insoluble in water
3. low melting point, solid doesn't conduct electricity, insoluble in water
4. low melting point, solid doesn't conduct electricity, aqueous solution doesn't conduct electricity
A substance has an ionic structure. It conducts electricity when molten but not when solid. The substance could be? [cb-26]
1. copper
2. petrol
3. ice
4. sodium chloride
Which of the following substances consists of small molecules? [cb-27]
1. high melting point, solid doesn't conduct electricity, aqueous solution conducts electricity
2. high melting point, solid conducts electricity, insoluble in water
3. low melting point, solid conducts electricity, insoluble in water
4. low melting point, solid doesn't conduct electricity, aqueous solution doesn't conduct electricity
Molten or dissolved sodium chloride conducts electricity. The current is carried in the melt by? [cb-28]
1. ions
2. metal atoms
3. molecules
4. electrons
Sodium chloride has a high melting point because it has? [cb-29]
1. a giant covalent 3-dimentional structure
2. many ions strongly attracted together
3. molecules packed tightly together
4. strong covalent double bonds
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-30]
1. conduct electricity when molten
2. conduct electricity when solid
3. have a low melting point
4. consist of small NaCl molecules
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-31]
1. not conduct electricity when molten
2. conduct electricity when dissolved in water
3. have a low melting point
4. consist of small NaCl molecules
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-32]
1. not conduct electricity when molten
2. not conduct electricity when dissolved in water
3. have a high melting point
4. consist of small NaCl molecules
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-33]
1. conduct electricity when solid
2. not conduct electricity when dissolved in water
3. have a low melting point
4. consist of charged particles
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-34]
1. not conduct electricity when solid
2. not conduct electricity when dissolved in water
3. have a low melting point
4. consist of NaCl molecules
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-35]
1. conduct electricity when solid
2. will dissolved in water
3. have a low melting point
4. consist of NaCl molecules
A substance has a giant covalent structure and has a high melting point. The substance could be [cb-36]
1. aluminium
2. copper
3. poly(ethene)
4. carbon (diamond)
Solid iodine consists of I₂ molecules symmetrically arranged in a crystal lattice. Relatively high temperatures are needed to change iodine molecules into iodine atoms because the? [cb-37]
1. forces holding the atoms together in an iodine molecule are strong
2. forces holding the molecules together in iodine are weak
3. iodine is an element and a non-metal
4. iodine is ionically bonded and the forces between ions are very strong
Solid iodine consists of I₂ molecules symmetrically arranged in a crystal lattice. Only relatively low temperatures (e.g. gentle warming) are needed to change solid iodine into iodine vapour because the? [cb-38]
1. forces holding the atoms together in an iodine molecule are strong
2. forces holding the molecules together in iodine are weak
3. iodine is an element and a non-metal
4. iodine is ionically bonded and the forces between ions are very strong
Potassium has an atomic number of 19. Which represents the electron configuration of the stable potassium ion K⁺? [cb-39]
Calcium has an atomic number of 20. Which represents the electron configuration of the stable calcium ion Ca²⁺? [cb-40]
Sulphur is a solid non-metallic element at room temperature, so it is? [cb-41]
1. a brittle substance
2. a good conductor of electricity
3. a good conductor of heat
4. a substance with a high melting point
Sulphur is a solid non-metallic element at room temperature, so it is? [cb-42]
1. easily bent into shape
2. a poor conductor of electricity
3. a good conductor of heat
4. a substance with a high melting point
Sulphur is a solid non-metallic element at room temperature, so it is? [cb-43]
1. easily bent into shape
2. a good conductor of electricity
3. a poor conductor of heat
4. a substance with a high melting point
Sulphur is a solid non-metallic element at room temperature, so it is? [cb-44]
1. easily bent into shape
2. a good conductor of electricity
3. a good conductor of heat
4. a substance with a low melting point
Copper is a metallic element so it is likely to be a? [cb-45]
1. substance with a high melting point
2. poor conductor of electricity
3. substance with a low boiling point
4. poor conductor of heat
Copper is a metallic element so it is likely to be a? [cb-46]
1. substance with a low melting point
2. good conductor of electricity
3. substance with a low boiling point
4. poor conductor of heat
Copper is a metallic element so it is likely to be a? [cb-47]
1. substance with a low melting point
2. poor conductor of electricity
3. substance with a high boiling point
4. poor conductor of heat
Copper is a metallic element so it is likely to be a? [cb-48]
1. substance with a low melting point
2. poor conductor of electricity
3. substance with a low boiling point
4. good conductor of heat
Copper is a metallic element so it is likely to be a? [cb-49]
1. substance with a low melting point
2. poor conductor of electricity
3. substance with a shiny surface
4. poor conductor of heat
Copper is a metallic element so it is likely to be a? [cb-50]
1. substance with a low melting point
2. poor conductor of electricity
3. substance easily hammered into shape
4. poor conductor of heat
To form an ion with a single positive charge, a metal atom must? [cb-51]
1. gain an electron
2. gain a proton
3. lose an electron
4. share an electron
To form an ion with a single negative charge, a non-metal atom must? [cb-52]
1. gain an electron
2. gain a proton
3. lose an electron
4. share an electron
Aluminium fluoride is an ionic compound. When this compound is formed from aluminium and fluorine? [cb-53]
1. electrons are shared
2. electrons are transferred
3. protons are shared
4. protons are transferred
Water is a covalent compound. When this compound is formed from hydrogen and oxygen? [cb-54]
1. electrons are shared
2. electrons are transferred
3. protons are shared
4. protons are transferred
From four substances described below, which is most likely to be an ionic compound? [cb-55]
1. melting point 20^oC, molten substance doesn't conduct electricity
2. melting point 150^oC, molten substance doesn't conduct electricity
3. melting point 800^oC, molten substance readily conducts electricity
4. melting point 1500^oC, molten substance is a poor electrical conductor
From four substances described below, which is most likely to consist of small molecules? [cb-56]
1. melting point 20^oC, molten substance doesn't conduct electricity
2. melting point 1150^oC, molten substance conducts electricity
3. melting point 480^oC, molten substance readily conducts electricity
4. melting point 1500^oC, molten substance is a poor electrical conductor
From four substances described below, which is most likely to consist of a giant covalent structure? [cb-57]
1. melting point 20^oC, molten substance doesn't conduct electricity
2. melting point 1150^oC, molten substance readily conducts electricity
3. melting point 480^oC, molten substance readily conducts electricity
4. melting point 1500^oC, molten substance is poor electrical conductor
Fluorine (F) has an atomic number of 9. Which represents the electron arrangement of the fluoride ion (F^-)? [cb-58]
Magnesium (Mg) has an atomic number of 12. Which represents the electron arrangement of the magnesium ion (Mg²⁺)? [cb-59]
Which electronic dot and cross diagram represents the compound formed when hydrogen (Q), at. no. 1 , combines with chlorine (X), Gp 7, at. no. 17? (only the outer shell o/x electrons are shown) [cb-60]
1. diagram (6)
2. diagram (2)
3. diagram (4)
4. diagram (1)
Which electronic dot and cross diagram represents the compound formed when hydrogen (Q), at. no. 1 , combines with oxygen (X), Gp 6, at. no. 8? (only the outer shell o/x electrons are shown) [cb-61]
1. diagram (3)
2. diagram (4)
3. diagram (7)
4. diagram (1)
Which electronic dot and cross diagram represents the compound formed when hydrogen (Q), at. no. 1 , combines with nitrogen (X), Gp 5, at. no. 7? (only the outer shell o/x electrons are shown) [cb-62]
1. diagram (6)
2. diagram (5)
3. diagram (7)
4. diagram (1)
Which electronic dot and cross diagram represents the compound formed when hydrogen (Q), at. no. 1 , combines with carbon (X), Gp 4, at. no. 6? (only the outer shell o/x electrons are shown) [cb-63]
1. diagram (3)
2. diagram (5)
3. diagram (7)
4. diagram (8)
Which electronic dot and cross diagram represents the compound formed when chlorine (Q), at. no. 17 , combines with carbon (X), Gp 4, at. no. 6? (only the outer shell o/x electrons are shown) [cb-64]
1. diagram (3)
2. diagram (5)
3. diagram (7)
4. diagram (8)
Which substance is likely to have a simple molecular structure? [cb-1]
1. melts at 17^oC, insoluble in water, non-conductor of electricity either when solid or molten
2. melts at 670^oC, dissolves in water, non-conductor of electricity when molten, undergoes electrolysis in aqueous solution
3. melts at 2600^oC, dissolves in water, non-conductor of electricity when solid, undergoes electrolysis in aqueous solution
4. melts at 1400^oC, insoluble in water, good conductor of electricity either when solid or molten
Which substance is likely to have a giant ionic structure? [cb-2]
1. melts at 17^oC, insoluble in water, non-conductor of electricity either when solid or molten
2. melts at 2800^oC, insoluble in water, non-conductor of electricity when molten or solid
3. melts at 2600^oC, dissolves in water, non-conductor of electricity when solid, undergoes electrolysis in aqueous solution
4. melts at 1400^oC, insoluble in water, good conductor of electricity either when solid or molten
Which substance is likely to have a metallic structure? [cb-3]
1. melts at 17^oC, insoluble in water, non-conductor of electricity either when solid or molten
2. melts at 2800^oC, insoluble in water, non-conductor of electricity when molten or solid
3. melts at 2600^oC, dissolves in water, non-conductor of electricity when solid, undergoes electrolysis in aqueous solution
4. melts at 1400^oC, insoluble in water, good conductor of electricity either when solid or molten
Which substance is likely to have a giant covalent structure? [cb-4]
1. melts at 17^oC, insoluble in water, non-conductor of electricity either when solid or molten
2. melts at 2800^oC, insoluble in water, non-conductor of electricity when molten or solid
3. melts at 2600^oC, dissolves in water, non-conductor of electricity when solid, undergoes electrolysis in aqueous solution
4. melts at 1400^oC, insoluble in water, good conductor of electricity either when solid or molten
Which substance is likely to have a simple molecular structure but form ions in aqueous solution? [cb-5]
1. melts at 17^oC, reacts with water, non-conductor of electricity either when solid, molten or in water
2. melts at 370^oC, dissolves in water, non-conductor of electricity when molten or solid, solution conducts electricity
3. melts at 2600^oC, dissolves in water, non-conductor of electricity when solid, undergoes electrolysis in aqueous solution
4. melts at 1400^oC, insoluble in water, good conductor of electricity either when solid or molten
A solution of sodium chloride conducts electricity because the? [cb-6]
1. current breaks down sodium chloride into sodium ions and chloride ions
2. ions formed from the water carry the current
3. sodium ions and chloride ions are free to move and carry the current
4. the free moving water molecules are good conductors
An atom can turn into an ion if it? [cb-7]
1. gains an electron
2. loses a proton
3. gains a neutron
4. loses a neutron
An atom can turn into an ion if it? [cb-8]
1. gains a proton
2. loses a proton
3. gains a neutron
4. loses an electron
When a covalent bond is formed between atoms of different elements ? [cb-9]
1. electrons are shared
2. electrons are transferred
3. protons are shared
4. protons are transferred
When an ionic bond is formed between atoms of different elements? [cb-10]
1. electrons are shared
2. electrons are transferred
3. protons are shared
4. protons are transferred
Metal atoms form ions with a positive charge by? [cb-11]
1. gaining protons
2. gaining electrons
3. losing electrons
4. losing protons
Non-metal atoms form ions with a negative charge by? [cb-12]
1. gaining protons
2. gaining electrons
3. losing electrons
4. losing protons
Atoms of Group 7 of the Periodic Table are most likely to form ions with? [cb-13]
1. a single negative charge by gaining one electron
2. a single positive charge by losing one electron
3. a double negative charge by gaining two electrons
4. a double positive charge by losing two electrons
Atoms of Group 1 of the Periodic Table are most likely to form ions with? [cb-14]
1. a single negative charge by gaining one electron
2. a single positive charge by losing one electron
3. a double negative charge by gaining two electrons
4. a double positive charge by losing two electrons
Atoms of Group 6 of the Periodic Table are most likely to form ions with [cb-15]
1. a single negative charge by gaining one electron
2. a single positive charge by losing one electron
3. a double negative charge by gaining two electrons
4. a double positive charge by losing two electrons
Atoms of Group 2 of the Periodic Table are most likely to form ions with? [cb-16]
1. a single negative charge by gaining one electron
2. a single positive charge by losing one electron
3. a double negative charge by gaining two electrons
4. a double positive charge by losing two electrons
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 1, with a non-metal X from Group 7 of the Periodic Table? [cb-17]
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 1, with a non-metal X from Group 6 of the Periodic Table? [cb-18]
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 2, with a non-metal X from Group 6 of the Periodic Table? [cb-19]
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 2, with a non-metal X from Group 7 of the Periodic Table? [cb-20]
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 3, with a non-metal X from Group 6 of the Periodic Table? [cb-21]
Which electronic diagram is correct for the compound formed by combining a metal M, from Group 3, with a non-metal X from Group 7 of the Periodic Table? [cb-22]
Which of the following substances consists of an ionic lattice? [cb-23]
1. high melting point, solid doesn't conduct electricity, aqueous solution conducts electricity
2. high melting point, solid conducts electricity, insoluble in water
3. low melting point, solid conducts electricity, insoluble in water
4. low melting point, solid doesn't conduct electricity, aqueous solution doesn't conduct electricity
What is an ion? [cb-24]
1. an atom which has lost or gained electrons
2. a negatively charged particle in the shells of an atom
3. an uncharged particle in the nucleus of an atom
4. a positively charged particle in the nucleus of an atom
Which of the following substances consists of a metal lattice? [cb-25]
1. high melting point, solid doesn't conduct electricity, aqueous solution conducts electricity
2. high melting point, solid conducts electricity, insoluble in water
3. low melting point, solid doesn't conduct electricity, insoluble in water
4. low melting point, solid doesn't conduct electricity, aqueous solution doesn't conduct electricity
A substance has an ionic structure. It conducts electricity when molten but not when solid. The substance could be? [cb-26]
1. copper
2. petrol
3. ice
4. sodium chloride
Which of the following substances consists of small molecules? [cb-27]
1. high melting point, solid doesn't conduct electricity, aqueous solution conducts electricity
2. high melting point, solid conducts electricity, insoluble in water
3. low melting point, solid conducts electricity, insoluble in water
4. low melting point, solid doesn't conduct electricity, aqueous solution doesn't conduct electricity
Molten or dissolved sodium chloride conducts electricity. The current is carried in the melt by? [cb-28]
1. ions
2. metal atoms
3. molecules
4. electrons
Sodium chloride has a high melting point because it has? [cb-29]
1. a giant covalent 3-dimentional structure
2. many ions strongly attracted together
3. molecules packed tightly together
4. strong covalent double bonds
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-30]
1. conduct electricity when molten
2. conduct electricity when solid
3. have a low melting point
4. consist of small NaCl molecules
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-31]
1. not conduct electricity when molten
2. conduct electricity when dissolved in water
3. have a low melting point
4. consist of small NaCl molecules
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-32]
1. not conduct electricity when molten
2. not conduct electricity when dissolved in water
3. have a high melting point
4. consist of small NaCl molecules
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-33]
1. conduct electricity when solid
2. not conduct electricity when dissolved in water
3. have a low melting point
4. consist of charged particles
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-34]
1. not conduct electricity when solid
2. not conduct electricity when dissolved in water
3. have a low melting point
4. consist of NaCl molecules
Sodium chloride is a typical ionic compound formed by combining a metal with a non-metal. Sodium chloride will? [cb-35]
1. conduct electricity when solid
2. will dissolved in water
3. have a low melting point
4. consist of NaCl molecules
A substance has a giant covalent structure and has a high melting point. The substance could be [cb-36]
1. aluminium
2. copper
3. poly(ethene)
4. carbon (diamond)
Solid iodine consists of I₂ molecules symmetrically arranged in a crystal lattice. Relatively high temperatures are needed to change iodine molecules into iodine atoms because the? [cb-37]
1. forces holding the atoms together in an iodine molecule are strong
2. forces holding the molecules together in iodine are weak
3. iodine is an element and a non-metal
4. iodine is ionically bonded and the forces between ions are very strong
Solid iodine consists of I₂ molecules symmetrically arranged in a crystal lattice. Only relatively low temperatures (e.g. gentle warming) are needed to change solid iodine into iodine vapour because the? [cb-38]
1. forces holding the atoms together in an iodine molecule are strong
2. forces holding the molecules together in iodine are weak
3. iodine is an element and a non-metal
4. iodine is ionically bonded and the forces between ions are very strong
Potassium has an atomic number of 19. Which represents the electron configuration of the stable potassium ion K⁺? [cb-39]
Calcium has an atomic number of 20. Which represents the electron configuration of the stable calcium ion Ca²⁺? [cb-40]
Sulphur is a solid non-metallic element at room temperature, so it is? [cb-41]
1. a brittle substance
2. a good conductor of electricity
3. a good conductor of heat
4. a substance with a high melting point
Sulphur is a solid non-metallic element at room temperature, so it is? [cb-42]
1. easily bent into shape
2. a poor conductor of electricity
3. a good conductor of heat
4. a substance with a high melting point
Sulphur is a solid non-metallic element at room temperature, so it is? [cb-43]
1. easily bent into shape
2. a good conductor of electricity
3. a poor conductor of heat
4. a substance with a high melting point
Sulphur is a solid non-metallic element at room temperature, so it is? [cb-44]
1. easily bent into shape
2. a good conductor of electricity
3. a good conductor of heat
4. a substance with a low melting point
Copper is a metallic element so it is likely to be a? [cb-45]
1. substance with a high melting point
2. poor conductor of electricity
3. substance with a low boiling point
4. poor conductor of heat
Copper is a metallic element so it is likely to be a? [cb-46]
1. substance with a low melting point
2. good conductor of electricity
3. substance with a low boiling point
4. poor conductor of heat
Copper is a metallic element so it is likely to be a? [cb-47]
1. substance with a low melting point
2. poor conductor of electricity
3. substance with a high boiling point
4. poor conductor of heat
Copper is a metallic element so it is likely to be a? [cb-48]
1. substance with a low melting point
2. poor conductor of electricity
3. substance with a low boiling point
4. good conductor of heat
Copper is a metallic element so it is likely to be a? [cb-49]
1. substance with a low melting point
2. poor conductor of electricity
3. substance with a shiny surface
4. poor conductor of heat
Copper is a metallic element so it is likely to be a? [cb-50]
1. substance with a low melting point
2. poor conductor of electricity
3. substance easily hammered into shape
4. poor conductor of heat
To form an ion with a single positive charge, a metal atom must? [cb-51]
1. gain an electron
2. gain a proton
3. lose an electron
4. share an electron
To form an ion with a single negative charge, a non-metal atom must? [cb-52]
1. gain an electron
2. gain a proton
3. lose an electron
4. share an electron
Aluminium fluoride is an ionic compound. When this compound is formed from aluminium and fluorine? [cb-53]
1. electrons are shared
2. electrons are transferred
3. protons are shared
4. protons are transferred
Water is a covalent compound. When this compound is formed from hydrogen and oxygen? [cb-54]
1. electrons are shared
2. electrons are transferred
3. protons are shared
4. protons are transferred
From four substances described below, which is most likely to be an ionic compound? [cb-55]
1. melting point 20^oC, molten substance doesn't conduct electricity
2. melting point 150^oC, molten substance doesn't conduct electricity
3. melting point 800^oC, molten substance readily conducts electricity
4. melting point 1500^oC, molten substance is a poor electrical conductor
From four substances described below, which is most likely to consist of small molecules? [cb-56]
1. melting point 20^oC, molten substance doesn't conduct electricity
2. melting point 1150^oC, molten substance conducts electricity
3. melting point 480^oC, molten substance readily conducts electricity
4. melting point 1500^oC, molten substance is a poor electrical conductor
From four substances described below, which is most likely to consist of a giant covalent structure? [cb-57]
1. melting point 20^oC, molten substance doesn't conduct electricity
2. melting point 1150^oC, molten substance readily conducts electricity
3. melting point 480^oC, molten substance readily conducts electricity
4. melting point 1500^oC, molten substance is poor electrical conductor
Fluorine (F) has an atomic number of 9. Which represents the electron arrangement of the fluoride ion (F^-)? [cb-58]
Magnesium (Mg) has an atomic number of 12. Which represents the electron arrangement of the magnesium ion (Mg²⁺)? [cb-59]
Which electronic dot and cross diagram represents the compound formed when hydrogen (Q), at. no. 1 , combines with chlorine (X), Gp 7, at. no. 17? (only the outer shell o/x electrons are shown) [cb-60]
1. diagram (6)
2. diagram (2)
3. diagram (4)
4. diagram (1)
Which electronic dot and cross diagram represents the compound formed when hydrogen (Q), at. no. 1 , combines with oxygen (X), Gp 6, at. no. 8? (only the outer shell o/x electrons are shown) [cb-61]
1. diagram (3)
2. diagram (4)
3. diagram (7)
4. diagram (1)
Which electronic dot and cross diagram represents the compound formed when hydrogen (Q), at. no. 1 , combines with nitrogen (X), Gp 5, at. no. 7? (only the outer shell o/x electrons are shown) [cb-62]
1. diagram (6)
2. diagram (5)
3. diagram (7)
4. diagram (1)
Which electronic dot and cross diagram represents the compound formed when hydrogen (Q), at. no. 1 , combines with carbon (X), Gp 4, at. no. 6? (only the outer shell o/x electrons are shown) [cb-63]
1. diagram (3)
2. diagram (5)
3. diagram (7)
4. diagram (8)
Which electronic dot and cross diagram represents the compound formed when chlorine (Q), at. no. 17 , combines with carbon (X), Gp 4, at. no. 6? (only the outer shell o/x electrons are shown) [cb-64]
1. diagram (3)
2. diagram (5)
3. diagram (7)
4. diagram (8)

Edexcel GCSE 9-1 CHEMISTRY/Combined Science QUIZ on TOPIC 1 "KEY CONCEPTS in CHEMISTRY" (HT)

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