introduction to Mole

1. MOLES
INTRODUCTORY LESSON
BY
ABDUL MOIZ

3.  WHAT IS A MOLE???
The mole is the unit of measurement for amount of substance in the
International System of Units (SI)
The mole is widely used in chemistry as a convenient way to express amounts
of reactants and products of chemical reactions.

4. WHY MOLE!!!!
 From previous knowledge you know that atom are very small and have
very very small masses so it is not practical to measure them in KG or
grams.
 For atom we use what is called moles . This is the amount of a chemical
substance that contains atoms in 12 grams of carbon-12 (12C),
the isotope of carbon with standard atomic weight 12 by definition. This
number is expressed by the Avogadro constant, which has a value of
approximately 6.022×1023 mol−1. The mole is an SI base unit, with the unit
symbol mol.

5. What is Relative Atomic Mass
 For definition refer to book
 How much is the given element is greater than C-12
 Basically you divide the mass of the given element by 1/12 the mass of
carbon-12 which is 1

6. Continued
 Most of the elements R.A.M are not whole no.
why?????
give example?????

8.  Do you relative abundance ???
 how to calculate R.A.M

12. Short exercise
 Tell me the RAM of boron , beryllium &lithium
10 9 7
Tell me MAM acetic acid (CH3COOH) and nylon 6-6(C12H20N2O2 )
60 224

13. Relative Formula Units
 Substances that are bonded ironically are measured in formula units
according to the standard international scheme

15. Mini exercise
 Why ionic compounds are described by formula units ?
 Difference b/w RAM , MAM and RFM?

19.  How many particles are there in one mole ?
 Avogadro's no.?

20.  Avogadro’s number, number of atomic mass / molecular mass / formula
units in one mole of any substance equal to 6.022 × 10 23

32.  Difference b/w empirical and molecular formula ?
Molecular formulas tell you how many atoms of each element are in a
compound, and empirical formulas tell you the simplest or most reduced ratio
of elements in a compound. If a compound's molecular formula cannot be
reduced any more, then the empirical formula is the same as the molecular
formula.

38. Molar gas volume