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A r  and M r
Let’s try counting the number of rice particles in a bucket of rice. Is it easy?
Relative atomic mass, A r   Atoms are  very tiny particles .  Atoms have  very small masses . For example, mass of hydrogen atom = 1.4 X 10 -24  g mass of lead atom = 2.9 x 10 -22 g Mass of carbon – 12 atom = 1.7 X 10 -23 g It is not practical to use actual masses of atoms in calculations.     Chemists often  compare  masses of different atoms with each other.
In 1961… ,[object Object],[object Object],[object Object]
Why carbon – 12? ,[object Object],[object Object],[object Object]
Relative Atomic Mass The  relative atomic mass   of any atom is the  number of times  the mass of one atom of an element is greater than  1/12 of the mass of one carbon-12 atom .  Relative atomic mass = Mass of 1/12 of an atom of carbon-12 Mass of one atom of the element
Relative Atomic Mass The symbol for relative atomic mass is  A r . Relative atomic mass is a  ratio  and has no  unit . The  relative atomic mass  of each element is given in the Periodic Table.
 
What is the relative atomic mass, A r , of oxygen in the periodic table? ,[object Object],   One atom of oxygen is 16 times heavier than 1/12 of an atom of carbon-12.
Relative Atomic Mass of Some Elements Some A r   values are not whole numbers. 35.5 Chlorine 64 Copper 23 Sodium 1 Hydrogen Relative atomic mass, A r Element
 
Why are some A r  values not whole numbers?  This is because such elements occur as mixtures of  isotopes . For example, chlorine exists in two isotopic forms: chlorine-35 and chlorine-37.
How do we derive the A r  of chlorine? Hence, relative atomic mass of chlorine  = (0.75 × 35) + (0.25 × 37)  = 26.25 + 9.25  =  35.5  A sample of chlorine is made up of  75%  of chlorine-35 atoms and  25%  of chlorine-37 atoms.
Relative Molecular Mass, M r ,[object Object],Hence, we use  relative molecular mass  instead of relative atomic mass. C l C l
[object Object],[object Object],Relative Molecular Mass, M r M r Mass of 1 molecule Mass of 1/12 of a carbon-12 atom =
[object Object],Relative Molecular Mass, M r
How do we calculate the relative molecular mass of chlorine gas (Cl 2 )? A r  of Cl = 35.5 M r  of Cl 2  = 35.5 X 2 = 71
How do we calculate the relative molecular mass of ammonia (NH 3 )? A r  of N = 14 A r  of H = 1 M r  of NH 3  = 14 + 1    3 = 17
Relative Formula Mass, M r   Many substances such as water are covalent and exist as molecules. However, substances like sodium chloride, NaCl, are ionic and do not exist as molecules. The ‘relative molecular mass’ of an ionic compound is more accurately known as  relative formula mass, M r .
Relative Formula Mass, M r   ,[object Object],[object Object],For example, the relative formula mass of sodium chloride (NaC l ) is 23 + 35.5 = 58.5.
Relative Formula Mass  Many substances such as water are covalent and exist as molecules. However, substances like sodium chloride are ionic and  do not exist as molecules. The ‘relative molecular mass’ of an ionic compound  is more accurately known as  relative formula mass .
Relative Formula Mass  ,[object Object],For example, the relative formula mass of sodium chloride (NaC l ) is 23 + 35.5 = 58.5.
Calculating M r  of MgSO 4 A r  of Mg = 24 A r  of S = 32 M r  of MgSO 4  = 24 + 32 + (16    4) = 120 A r  of O = 16
(1 X 64) + (1 X 32) + (9 x 16) + (10 x 1) =  250 CuSO 4.  5H 2 O Copper (II) sulphate crystals (1 X 40) + (2 X 14) + (6 X 16) =  164 Ca(NO 3 ) 2  Calcium nitrate  (1 X 26) + (1 X 32) + (4 X 16) =  120 MgSO 4 Magnesium sulphate  Relative formula mass, M r Chemical Formula Compound

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The Mole Ar And Mr

  • 1. A r and M r
  • 2. Let’s try counting the number of rice particles in a bucket of rice. Is it easy?
  • 3. Relative atomic mass, A r Atoms are very tiny particles . Atoms have very small masses . For example, mass of hydrogen atom = 1.4 X 10 -24 g mass of lead atom = 2.9 x 10 -22 g Mass of carbon – 12 atom = 1.7 X 10 -23 g It is not practical to use actual masses of atoms in calculations.  Chemists often compare masses of different atoms with each other.
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  • 6. Relative Atomic Mass The relative atomic mass of any atom is the number of times the mass of one atom of an element is greater than 1/12 of the mass of one carbon-12 atom . Relative atomic mass = Mass of 1/12 of an atom of carbon-12 Mass of one atom of the element
  • 7. Relative Atomic Mass The symbol for relative atomic mass is A r . Relative atomic mass is a ratio and has no unit . The relative atomic mass of each element is given in the Periodic Table.
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  • 10. Relative Atomic Mass of Some Elements Some A r values are not whole numbers. 35.5 Chlorine 64 Copper 23 Sodium 1 Hydrogen Relative atomic mass, A r Element
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  • 12. Why are some A r values not whole numbers? This is because such elements occur as mixtures of isotopes . For example, chlorine exists in two isotopic forms: chlorine-35 and chlorine-37.
  • 13. How do we derive the A r of chlorine? Hence, relative atomic mass of chlorine = (0.75 × 35) + (0.25 × 37) = 26.25 + 9.25 = 35.5 A sample of chlorine is made up of 75% of chlorine-35 atoms and 25% of chlorine-37 atoms.
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  • 17. How do we calculate the relative molecular mass of chlorine gas (Cl 2 )? A r of Cl = 35.5 M r of Cl 2 = 35.5 X 2 = 71
  • 18. How do we calculate the relative molecular mass of ammonia (NH 3 )? A r of N = 14 A r of H = 1 M r of NH 3 = 14 + 1  3 = 17
  • 19. Relative Formula Mass, M r Many substances such as water are covalent and exist as molecules. However, substances like sodium chloride, NaCl, are ionic and do not exist as molecules. The ‘relative molecular mass’ of an ionic compound is more accurately known as relative formula mass, M r .
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  • 21. Relative Formula Mass Many substances such as water are covalent and exist as molecules. However, substances like sodium chloride are ionic and do not exist as molecules. The ‘relative molecular mass’ of an ionic compound is more accurately known as relative formula mass .
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  • 23. Calculating M r of MgSO 4 A r of Mg = 24 A r of S = 32 M r of MgSO 4 = 24 + 32 + (16  4) = 120 A r of O = 16
  • 24. (1 X 64) + (1 X 32) + (9 x 16) + (10 x 1) = 250 CuSO 4. 5H 2 O Copper (II) sulphate crystals (1 X 40) + (2 X 14) + (6 X 16) = 164 Ca(NO 3 ) 2 Calcium nitrate (1 X 26) + (1 X 32) + (4 X 16) = 120 MgSO 4 Magnesium sulphate Relative formula mass, M r Chemical Formula Compound