The document defines key chemistry concepts related to moles, including: - A mole refers to Avogadro's number (6.02x10^23) of particles like atoms, molecules, ions or formula units. - 1 mole of an element contains 6.02x10^23 atoms, 1 mole of a molecular compound contains 6.02x10^23 molecules, and 1 mole of an ionic compound contains 6.02x10^23 formula units. - Gram atomic mass refers to the mass of one mole of an element in grams, and gram formula mass refers to the sum of atomic weights that make up one mole of a compound. - Chemical formulas represent the

2.  It is a measure of the amount of
particles in matter.

3. Mole =
𝒎𝒂𝒔𝒔
𝒎𝒐𝒍𝒆𝒄𝒖𝒍𝒂𝒓 𝒎𝒂𝒔𝒔
;
𝑵𝒐.𝒐𝒇 𝒑𝒂𝒓𝒕𝒊𝒄𝒍𝒆𝒔
𝑨𝒗𝒐𝒈𝒂𝒅𝒓𝒐′ 𝒔 𝑵𝒖𝒎𝒃𝒆𝒓
 Refers to Avogadro’s number of any substance in honor ofAmadeo
Avogado di Quarenga and is equal to 6.02 x 𝟏𝟎 𝟐𝟑
number of
particles
 Number of particles:
particles, atoms, ions, molecules, or formula units
grams MOLE Number of particles

4.  1 mole of an element = 6.02 x 𝟏𝟎 𝟐𝟑 atom
 1 mole of Al = 6.02 x 𝟏𝟎 𝟐𝟑
atom
 1 mole of molecular compound = 6.02 x 𝟏𝟎 𝟐𝟑 molecules
 1 mole of N2 = 6.02 x 𝟏𝟎 𝟐𝟑
molecules
 1 mole of any ionic compound= 6.02 x
𝟏𝟎 𝟐𝟑
formula units
 1 mole of NaCl and a mole of MgO each contains 6.02 x
𝟏𝟎 𝟐𝟑
formula units

5. Mole =
𝑵𝒐.𝒐𝒇 𝒂𝒕𝒐𝒎𝒔
𝑨𝒗𝒐𝒈𝒂𝒅𝒓𝒐′ 𝒔 𝑵𝒖𝒎𝒃𝒆𝒓
Ex:
1. How many moles are 2.80 x 1023
atoms of Si?
2. How many atoms are 0.360 moles of
Al?

6. 1. How many molecules are 5.0 moles of table
sugar?
2. How many moles are there in 4.65 x 1024
molecules of CO2?

7.  It is atomic mass of an element expressed in
grams.
 The gram atomic mass of any element contains one
mole of atoms (6.02 x 𝟏𝟎 𝟐𝟑 atom) of that element.
 Ex: 12.0 g of Carbon = 12. 0 g is 1 mol of C or
6.02 x 𝟏𝟎 𝟐𝟑 atoms of C
27.0 g of Aluminum = 27. 0 g is 1 mol of Al or 6.02 x
𝟏𝟎 𝟐𝟑
atoms of Al.

8.  What is the mass of 1 mol of Ca, Na,
and S?
 What is the gram formula mass of
MgCl2?

9.  The sum of atomic weight of gram
compound or molecules.
 Ex:
▪ 𝐻2O =
▪ C𝐻3 =

10.  How many grams are 2.5 moles of
CaS?
 Find the number of moles in 5.44 g
of H2O2.

11.  It gives the lowest whole number atomic ratio
of elements in a compound.
 A formula that is written using the simplest
whole number ratio.
 Ex:
▪ 𝐶2 𝐻6 =
▪ 𝐶6 𝐻12 𝑂6 =

12.  The mass of each element in a compound
compared to the entire mass of the compound
multiplied by 100%.
% mass of element =
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑖𝑛 𝑡ℎ𝑒 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑡ℎ𝑒 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑
x 100 %

13.  𝐻2O
 𝐻2S 𝑂4
 Mg(OH )4

14. Prepared by:
Jimnaira U.Abanto