DEFINING & CALCULATING the RELATIVE ATOMIC MASS A_r of an element

Doc Brown's Chemistry - GCSE/IGCSE/GCE (basic A level) O Level Online Chemical Calculations

1. Defining, explaining and calculating relative atomic mass RAM or A_r, also mention of relative isotopic mass

Sub-index for page

(a) Introduction - defining relative atomic mass - carbon-12 scale - isotopes

(b) How to calculate relative atomic mass - examples explained

(c) How to calculate relative atomic mass with accurate relative isotopic masses

(c) is for advanced level chemistry students only and includes how to work out isotopic composition given the relative atomic mass.

(d) Table of relative atomic masses for elements 1 to 92 (2 decimal places)

Spotted any careless error on my part? EMAIL query ? comment

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Self-assessment Quizzes on relative atomic mass:

type in answer QUIZ  or  multiple choice QUIZ

(a) Introduction - defining relative atomic mass - carbon-12 scale

• Every atom has its own unique relative atomic mass (RAM) based on a standard comparison or relative scale e.g. it has been based on hydrogen H = 1 amu and oxygen O = 16 amu in the past (amu = relative atomic mass unit).
  • The relative atomic mass of an element takes into account the different masses of the isotopes of that element and the abundance of the isotopes in the naturally occurring element (meaning the percentage of each isotope present).
  • Relative atomic mass is defined and explained below, and examples of how to calculate it from data.
• The relative atomic mass scale is now based on an isotope of carbon, namely, carbon-12, nuclide symbol , which is given the arbitrary value of 12.0000 amu by international agreement.
  • The unit 'amu' is now being replaced by a lower case u, where u is the symbol for the unified atomic mass unit.
    • Therefore one atom of carbon, isotopic mass 12, equals 12 u, or,
    • 1 u = ¹/₁₂th the mass of one atom of the carbon-12 isotope.
  • Note that for the standard nuclide notation, , the top left number is the mass number (12) and the bottom left number is the atomic/proton number (6).
• Since the relative atomic mass of an element is now based on the carbon-12 isotope it can now be defined as ...
  • ... relative atomic mass equals the average mass of all the atoms in an element compared to ¹/₁₂th the mass of a carbon-12 atom (carbon-12 isotope).
  • Examples are shown in the Periodic Table diagram above.
  • Note
    • (i) Because of the presence of neutrons in the nucleus, the relative atomic mass is usually at least double the atomic/proton number because there are usually more neutrons than protons in the nucleus (mass proton = 1, neutron = 1). Just scan the periodic table above and examine the pairs of numbers.
      • You should also notice that generally speaking the numerical difference between the atomic/proton number and the relative atomic mass tends to increase with increasing atomic number.
      • This has consequences for nuclear stability.
    • (ii) For many calculation purposes, relative atomic masses are usually quoted and used at this academic level (GCSE/IGCSE/O level) to zero or one decimal place eg.
      • hydrogen H = 1.008 or ~1; calcium Ca = 40.08 or ~40.0; chlorine Cl = 35.45 ~35.5, copper Cu = 63.55 or ~63.5/64, silver Ag = 107.9 or ~108 etc.
    • At Advanced level, values of relative atomic masses may be quoted to one or two decimal places.
      • Many atomic masses are known to an accuracy of four decimal places, but for some elements, isotopic composition varies depending on the mineralogical source, so four decimal places isn't necessarily more accurate!
    • Note that in the case of carbon, there are three isotopes carbon-12 ¹²C the most abundant and small amounts of carbon-13 ¹³C and carbon-14 ¹⁴C. The average calculated mass of the atoms compared to carbon 12 is 12.01, but for most purposes at pre-university level, 12.0 is sufficient accuracy.
• In using the symbol A_r for RAM, you should bear in mind that the letter A on its own usually means the mass number of a particular isotope and amu is the acronym shorthand for atomic mass units.
• However there are complications due to isotopes and so very accurate atomic masses are never whole integer numbers.
• Isotopes are atoms of the same element with different masses due to different numbers of neutrons.
  • The very accurate relative atomic mass scale is based on a specific isotope of carbon, carbon-12, ¹²C = 12.0000 units exactly, for most purposes C = 12 is used for simplicity.
  • For example hydrogen-1, hydrogen-2, and hydrogen-3, are the nuclide notation for the three isotopes of hydrogen, though the vast majority of hydrogen atoms have a mass of 1.
  • When their accurate isotopic masses, and their % abundance are taken into account the average accurate relative mass for hydrogen = 1.008, but for most purposes H = 1 is good enough!
  • See also GCSE/IGCSE/AS Atomic Structure Notes
• Therefore, a stricter definition of relative atomic mass (A_r) is that it equals the average mass of all the isotopic atoms present in the element compared to ¹/₁₂th the mass of a carbon-12 atom.
  • AND, the relative isotopic mass of carbon-12 is assigned a numerical value of 12.0000.
  • So, in calculating relative atomic mass you must take into account the different isotopic masses of the same elements, but also their % abundance in the element.
  • Therefore you need to know the percentage (%) of each isotope of an element in order to accurately calculate the element's relative atomic mass.
  • For approximate calculations of relative atomic mass you can just use the mass numbers of the isotopes, which are obviously all integers ('whole numbers'!) e.g. in the two calculations below.
  • To the nearest whole number, isotopic mass = mass number for a specific isotope.
  • If an element only has one isotope, relative atomic mass = relative mass of this isotope.

    • A good example is fluorine.
    • All fluorine atoms have a mass of 19 (¹⁹F), therefore its relative atomic mass is 19 and no calculation is needed.

Above is typical periodic table used in GCSE science-chemistry specifications

and I've 'usually' used these values in my exemplar calculations to cover most syllabuses

(b) Examples of relative atomic mass calculations for GCSE 9-1/IGCSE/AS/A level chemistry students

How do I calculate relative atomic mass?

You can calculate relative atomic mass from isotopic abundances

• For accurate chemical calculations relative atomic mass must be used and not an individual mass number.
  • Therefore relative atomic mass takes into account all the different 'stable' isotopes of an element which are naturally present.
  • The relative atomic mass is the average mass and is quite easily calculated from the percentage composition (% abundance).
  • The presence of isotopes accounts for why some relative atomic masses are not even close to a whole number.
  • Some relative atomic masses are nearly whole numbers due to coincidence of % isotopes, others because one isotope might dominate the composition with only tiny amounts of lighter or heavier isotopes.
• Example 1.1 Calculating the relative atomic mass of bromine and
  • bromine consists of two isotopes, 50% ⁷⁹Br and 50% ⁸¹Br, calculate the A_r of bromine from the mass numbers (top left numbers).
  • Think of the calculation in terms of '100 atoms'
  • A_r = [ (50 x 79) + (50 x 81) ] /100 = 80
  • So the relative atomic mass of bromine is 80 or RAM or A_r(Br) = 80
  • Note the full working shown. Yes, ok, you can do it in your head BUT many students ignore the %'s and just average all the isotopic masses (mass numbers) given, in this case bromine-79 and bromine-81.
  • The element bromine is the only case I know where averaging the isotopic masses actually works! so beware!
  • -

• Example 1.2 Calculating the relative atomic mass of chlorine based on the and isotopes
  • Chlorine consists of two isotopes, 75% chlorine-35 and 25% chlorine-37, so using these two mass numbers ...
  • ... again think of the data based on 100 atoms, so 75 have a mass of 35 and 25 atoms have a mass of 37.
  • The average mass = [ (75 x 35) + (25 x 37) ] / 100 = 35.5
  • So the relative atomic mass of chlorine is 35.5 or RAM or A_r(Cl) = 35.5
  • Note: ³⁵Cl and ³⁷Cl are the most common isotopes of chlorine, but, there are tiny percentages of other chlorine isotopes which are usually ignored at GCSE/IGCSE and Advanced GCE AS/A2 A level.
  • -

• Example 1.3: Calculating the relative atomic mass of copper from its isotopic composition (isotope abundance)
  • Naturally occurring copper consists of 69.2% copper-63 (⁶³Cu) and 30.8% copper-65 (⁶⁵Cu)
  • Still think in terms of 100 atoms and don't be put off by decimal fractions, it still works out correctly because 69.2 + 30.8 = 100!
  • average mass = relative atomic mass of copper = {(63 x 69.2) + (65 x 30.8)} / 100 = 63.6
  • -
• Example 1.4: Silver atoms consist of 51.4% of the isotope ¹⁰⁷Ag and 48.6% of the isotope ¹⁰⁹Ag
  • Calculate the relative atomic mass of silver.

  • 		(51.4 x 107) + (48.6 x 109)	5499.8 + 5297.4
    Ar(Ag)	=	--------------------------------------	=    ---------------------------	= 108.0
    		100	100

  • The relative atomic mass of silver is 108.0 (to 1 decimal place)
  • -
• Example 1.5: Europium atoms consist of 47.8% Eu-151 and 52.2% of Eu-153
  • Calculate the relative atomic mass of europium.

  • 		(47.8 x 151) + (52.2 x 153)	7217.8 + 7986.6
    Ar(Eu)	=	--------------------------------------	=    ---------------------------	= 152.0
    		100	100

  • The relative atomic mass of europium is 152.0 (to 1 decimal place)
  • -
• Example 1.6: Atoms of the element silicon consist of 92.2% silicon-28, 4.7% silicon-29 and 3.1% of silicon-30.
  • Calculate the relative atomic mass of silicon.

  • 		(92.2 x 28) + (4.7 x 29) + (3.1 x 30)	2581.6 + 136.3 + 93.0
    Ar(Si)	=	--------------------------------------------------	=  --------------------------------	= 28.1
    		100	100

  • The relative atomic mass of silicon is 28.1 (to 1 decimal place or 3 significant figures)
  • -
• See below and mass Spectrometer and isotope analysis on the GCSE-Advanced A Level (basic) Atomic Structure Notes, with further relative atomic mass calculations.

(1) Very accurate calculation of relative atomic mass (need to know and define what relative isotopic mass is)

Relative isotopic mass is defined as the accurate mass of a single isotope of an element compared to ¹/₁₂th the mass of a carbon-12 atom e.g. the accurate relative isotopic mass of the cobalt-5 is 58.9332

This definition of relative isotopic mass is a completely different from the definition of relative atomic mass, except both are based on the same international standard of atomic mass i.e. 1 unit (1 u) = 1/12th the mass of a carbon-12 isotope (¹²C).

If we were to redo the calculation of the relative atomic mass of chlorine (example 1.1 above), which is quite adequate for GCSE purposes (and maybe A level too), but more accurately at A level, we might do ....

chlorine is 75.77% ³⁵Cl of isotopic mass 34.9689 and 24.23% ³⁷Cl of isotopic mass 36.9658

so A_r(Cl) = [(75.77 x 34.9689) + (24.23 x 36.9658)] / 100

= 35.4527 (but 35.5 is usually ok in calculations pre-university!)

See also Mass Spectrometer and isotope analysis on the GCSE/A level Atomic Structure Notes, with further RAM calculations.

(2) Calculations of % composition of isotopes

It is possible to do the reverse of a relative atomic mass calculation if you know the A_r and which isotopes are present.

It involves a little bit of arithmetical algebra.

The A_r of boron is 10.81 and consists of only two isotopes, boron-10 and boron-11

The relative atomic mass of boron was obtained accurately in the past from chemical analysis of reacting masses but now mass spectrometers can sort out all of the isotopes present and their relative abundance.

If you let X = % of boron 10, then 100-X is equal to % of boron-11

Therefore A_r(B) = (X x 10) + [(100-X) x 11)] / 100 = 10.81

so, 10X -11X +1100 =100 x 10.81

-X + 1100 = 1081, 1100 - 1081 = X (change sides change sign!)

therefore X = 19

so naturally occurring boron consists of 19% ¹⁰B and 81% ¹¹B

(the data books actually quote 18.7 and 81.3, but we didn't use the very accurate relative isotopic masses mentioned above!)

TOP OF PAGE and sub-index

On other pages on Atomic structure and Relative Formula Mass

Self-assessment Quizzes on relative atomic mass

type in answer  QUIZ  or  multiple choice QUIZ

APPENDIX 1. A typical periodic table used in pre-university examinations

Above is typical periodic table used in GCSE science-chemistry specifications in doing chemical calculations, and I've 'usually' used these values in my exemplar calculations to cover most syllabuses

TOP OF PAGE and sub-index

(d) APPENDIX 2. Table of relative atomic masses for elements 1 to 92

Notes on the relative atomic mass data:

(i) The list of relative atomic mass are in alphabetical order by element name, together with chemical symbol and proton/atomic number from 1 to 92.

(ii) The relative atomic masses are quoted to two decimal places, though it is essential to be aware that values in pre-university examinations might be rounded to the nearest integer or one decimal place.

(iii) Trans-uranium elements have been eliminated because their isotopic composition varies depending on the source e.g. cyclotron, nuclear reactor etc. AND all their isotopes are highly radioactive and most are very unstable (so your relative atomic mass changes all the time!)

(iv) * radioactive, mass number of most stable isotope quoted

OTHER CALCULATION PAGES

1. What is relative atomic mass?, relative isotopic mass & calculating relative atomic mass (this page)

2. Calculating relative formula/molecular mass of a compound or element molecule

3. Law of Conservation of Mass and simple reacting mass calculations

4. Composition by percentage mass of elements in a compound

5. Empirical formula and formula mass of a compound from reacting masses (easy start, not using moles)

6. Reacting mass ratio calculations of reactants and products from equations (NOT using moles) and brief mention of actual percent % yield and theoretical yield, atom economy and formula mass determination

   • Reacting masses, concentration of solution and volumetric titration calculations (NOT using moles)

7. Introducing moles: The connection between moles, mass and formula mass - the basis of reacting mole ratio calculations (relating reacting masses and formula mass)

8. Using moles to calculate empirical formula and deduce molecular formula of a compound/molecule (starting with reacting masses or % composition)

9. Moles and the molar volume of a gas, Avogadro's Law

10. Reacting gas volume ratios, Avogadro's Law and Gay-Lussac's Law (ratio of gaseous reactants-products)

11. Molarity, volumes and solution concentrations (and diagrams of apparatus)

12. How to do acid-alkali titration calculations, diagrams of apparatus, details of procedures

13. Electrolysis products calculations (negative cathode and positive anode products)

14. Other calculations e.g. % purity, % percentage & theoretical yield, dilution of solutions (and diagrams of apparatus), water of crystallisation, quantity of reactants required, atom economy

    • 14.1 % purity of a product 14.2a % reaction yield 14.2b atom economy 14.3 dilution of solutions

    • 14.4 water of crystallisation calculation  14.5 how much of a reactant is needed?

15. Energy transfers in physical/chemical changes, exothermic/endothermic reactions

16. Gas calculations involving PVT relationships, Boyle's and Charles Laws

17. Radioactivity & half-life calculations including dating materials

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Alphabetical order of the elements of the periodic table symbol name atomic number: relative atomic mass of Ac Actinium 89, relative atomic mass of Al Aluminium 13, relative atomic mass of Sb Antimony 51, relative atomic mass of Ar Argon 18, relative atomic mass of As Arsenic 33, relative atomic mass of At Astatine 85, relative atomic mass of Ba Barium 56, relative atomic mass of Be Beryllium 4, relative atomic mass of Bi Bismuth 83, relative atomic mass of B Boron 5, relative atomic mass of Br Bromine 35, relative atomic mass of Cd Cadmium 48, relative atomic mass of Cs Caesium 55, relative atomic mass of Ca Calcium 20, relative atomic mass of C Carbon 6, relative atomic mass of Ce Cerium

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