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2c. The ionic bonding of the compound sodium chloride
Doc Brown's Chemistry: Chemical Bonding and structure GCSE level, IGCSE, O, IB, AS, A level US grade 9-12 level Revision Notes
Example 2c. A Group 1 Alkali Metal combining with a Group 7 Halogen non–metal
* metals \ non-metals (zig-zag line)
e.g. sodium + chlorine ==> sodium chloride NaCl or its ionic formula Na+Cl–
In terms of electron arrangement in the formation of the ionic compound sodium chloride, the sodium donates its outer electron to a chlorine atom forming a single positive sodium ion and a single negative chloride ion.
Na (2.8.1) + Cl (2.8.7) ==> Na+ (2.8) Cl– (2.8.8)
add diagrams of original atoms from 4_71atom ? group pages?
can be summarised electronically to give the stable 'noble gas' structures as [2,8,1] + [2,8,7] ==> [2,8]+ [2,8,8]–
so both the sodium and chloride ions have a full outer shell like a noble gas
ONE atom combines withONE atom to form
Note in this electron diagram, only the original outer electrons are shown above.
The outer electron of the sodium atom (2.8.1) is transferred to the outer shell of the chlorine atom (2.8.7) giving it a complete octet shell of outer electrons, just like a noble gas (2.8.8). At the same time, the sodium ion also attains a stable noble gas electron structure (2.8).
Li is 2.1, K is 126.96.36.199, F is 2.7, rest of dot and cross diagram is up to you.
All the formula highlighted in yellow can be described in the same way as sodium chloride
The Group 1 Alkali Metal atom loses one electron to form a singly charged positive ion
The Group 7 Halogen atom gains one electron to form a singly charged negative ion
empirical formula - mention on each page and explain
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