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SS1: CHEMISTRY - 1ST TERM

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  1. Introduction to Chemistry and Laboratory Apparatus | Week 1
    5 Topics
    |
    1 Quiz
  2. Nature of Matter | Week 2
    3 Topics
    |
    1 Quiz
  3. Separation Techniques I | Week 3
    1 Topic
  4. Separation Techniques II | Week 4
    5 Topics
    |
    1 Quiz
  5. Particulate Nature of Matter I | Week 5
    5 Topics
    |
    1 Quiz
  6. Particulate Nature of Matter II | Week 6
    9 Topics
    |
    1 Quiz
  7. Symbols, Formulae & Oxidation Number | Week 7
    7 Topics
    |
    1 Quiz
  8. Laws of Chemical Combination | Week 8
    4 Topics
    |
    1 Quiz
  9. Chemical Equation & Chemical Combination (Chemical Bonding) I | Week 9
    4 Topics
    |
    1 Quiz
  10. Chemical Combination (Chemical Bonding) II | Week 10
    4 Topics
    |
    1 Quiz
  11. Chemical Combination (Chemical Bonding) III & Shapes of Covalent Molecules | Week 11
    3 Topics
    |
    1 Quiz



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Topic Content:

  • Meaning of Relative Atomic Mass

The relative Atomic mass of an element is the number of times the average mass of one atom of that element is heavier than one-twelfth the mass of one atom of carbon-12.

\(\scriptsize Relative \: Atomic\: Mass = \normalsize \frac{mass \: of \: 1 \: atom \: of \: the\: element }{\frac{1}{12} \: \times \: mass \: of \:1\: atom \: of \: Carbon-12 } \)

From the definition,

1 carbon atom has a mass of 12

1 oxygen atom has a mass of 16

1 hydrogen atom has a mass of 1

The relative atomic mass of an element which exhibits Isotopy is the average mass of its various isotopes.

Relative atomic mass is not a whole number because of the existence of an isotope.

Example 6.4.1:

A natural occurring Chlorine contains 75% of \( \scriptsize _{17} ^{35} \textrm {Cl} \) and 25% of \( \scriptsize _{17} ^{37} \textrm {Cl} \)

Calculate the relative atomic mass of Chlorine.

 

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