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Notes
Avagadro constant is 6.02 x 10^23. Particles present in 22.4 L
There also another no. that is quite usable in every cases. It is Loschmidt number-
2.68 X 10^19. That is particels present in 1ml or 1 cubic capacity.
Mass of the single atom of an element is known as atomic mass.
It is a number which tells how much is a atom heavier than 1/12 of a C-12 atom.
amu- Atomic Mass Unit
It is equal to 1/12th of mass of a C-12 atom.
The mass of one whole C-12 atom was found by using a technique known as
"Mass of Spectroscopy", and it was found that it's mass was around 1.99 X 10^-23 g.
amu, u(unified mass), D(Dalton) all are the same.
1 amu is equal is to 1.66 X 10^-24 g.
Atomic Mass (AMU)
Oxygen-16 am
Nitrogen- 14 amu
Sodium- 23 amu
Carbon- 12 amu
Magnesium- 24 amu
Hydrogen- 1 amu
Aluminium- 27 amu
Chlorine- 35.5 amu
Iodine- 127 amu
Sulphur- 32 amu
Notes 1
, Potassium- 39 amu
Manganese- 55 amu
Calcium- 40 amu
Phosporous -31 amu
Copper=63.5
Mass of one molecule is known as molecular mass.
It is the sum of atomic masses in a compoud.
CH4= 12+1(4) amu
=16 amu
Particles in CH4 =16 X 6.022 X 10^23 g
NA- It is known as avagadro's number.
It's value is 6.022 X 10^23
1/NA = 1.66 X 10^-24
amu=1/NA
Molar Mass
Also known as gram molecular mass
It is defined as the mass of one mole of a substance.
1 mole is 6.022 X 10^23 particles.
Mole is a unit.
Molar mass is expressed in grams.
Molar mass of O= Mass of one O atom X NA
Notes 2
, =16 amu X NA
=16 X 1/NA X NA
=16g is the molar mass of oxygen
Both atomic mass and molar mass of elements will be same in
magnitude but differ in units. Represented as amu in atomic
mass and as grams in molar mass.
Molar Mass
There is also another term that is known as mass number which
is just the addition of the number of protons and neutrons.
It is also the same as atomic mass but the only difference is it
doesn't have any units.
Notes 3
Notes
Avagadro constant is 6.02 x 10^23. Particles present in 22.4 L
There also another no. that is quite usable in every cases. It is Loschmidt number-
2.68 X 10^19. That is particels present in 1ml or 1 cubic capacity.
Mass of the single atom of an element is known as atomic mass.
It is a number which tells how much is a atom heavier than 1/12 of a C-12 atom.
amu- Atomic Mass Unit
It is equal to 1/12th of mass of a C-12 atom.
The mass of one whole C-12 atom was found by using a technique known as
"Mass of Spectroscopy", and it was found that it's mass was around 1.99 X 10^-23 g.
amu, u(unified mass), D(Dalton) all are the same.
1 amu is equal is to 1.66 X 10^-24 g.
Atomic Mass (AMU)
Oxygen-16 am
Nitrogen- 14 amu
Sodium- 23 amu
Carbon- 12 amu
Magnesium- 24 amu
Hydrogen- 1 amu
Aluminium- 27 amu
Chlorine- 35.5 amu
Iodine- 127 amu
Sulphur- 32 amu
Notes 1
, Potassium- 39 amu
Manganese- 55 amu
Calcium- 40 amu
Phosporous -31 amu
Copper=63.5
Mass of one molecule is known as molecular mass.
It is the sum of atomic masses in a compoud.
CH4= 12+1(4) amu
=16 amu
Particles in CH4 =16 X 6.022 X 10^23 g
NA- It is known as avagadro's number.
It's value is 6.022 X 10^23
1/NA = 1.66 X 10^-24
amu=1/NA
Molar Mass
Also known as gram molecular mass
It is defined as the mass of one mole of a substance.
1 mole is 6.022 X 10^23 particles.
Mole is a unit.
Molar mass is expressed in grams.
Molar mass of O= Mass of one O atom X NA
Notes 2
, =16 amu X NA
=16 X 1/NA X NA
=16g is the molar mass of oxygen
Both atomic mass and molar mass of elements will be same in
magnitude but differ in units. Represented as amu in atomic
mass and as grams in molar mass.
Molar Mass
There is also another term that is known as mass number which
is just the addition of the number of protons and neutrons.
It is also the same as atomic mass but the only difference is it
doesn't have any units.
Notes 3
