no. of mol = Mass of Mole
n= given mass (gm)/ 1 mol related Law of During chemical reaction , Initial mass of
W/GAM molecular atom = to Conservation mass of reactant is equal to reactant = Mass of
mass(gm) Its GAM GAM of Mass mass of product , when product + Mass of
Mass of 1 mol Mole Mole is that (Lavoisier) reaction is 100% complete. unreacted reactant
n= W/GMM molecule = Its related to quantity of
Law of In Compound, ratio of
GMM GMM substance
Constant different element with respect eg. CO2 =>
which contain Mole Proportion to their masses is always fixed, Mass => 3:8
n= Given no 1 mol = 6.022 Mol
of particles/ x 10²³ related to
as many Concept Laws of (Proust) no matter how it's prepared
particles as
N⁰[6.022 x particles of no. of there are in 12
Chemical Law of When different masses of one element which
10²³] substance particles g of Carbon Combination multiple combines with fixed mass of another element to
P₁V₁/T₁ = 1 mol gas at NTP Mole proportions form a no. of compound, then the different masses
n= V (Dalton) of the element bear a simple whole no. ratio.
P₂V₂/T₂ occupy 22.4 L Vol. related to
given (L)
NTP known as Molar Vol. of gas Gay- States that, gases react with each other in the simple ratio
/ 22.4(L)
Given Vol. at NTP Lussac's of their volume & if the product is also in gaseous state,
Law of the volume of product also bears a simple ratio with volume
VD of Substance VD = Density of Substance(in gas)/ Relationship of Vapour gaseous of gaseous reactants provided all the volume are measured
volume under similar condition of temp. and pressure.
x 2 = GMM Density of H₂ in gas Density(Unitless) & GMM
When mass of atoms or molecules is 1 amu = [Mass of 1 atom of ¹²₆C
Smallest particle of element or comp'd which Relative
expressed in relation to some other (1.9924 x 10⁻²³)] / 12
has independent existence & stable System of mass elements like Carbon. Unit => amu / u 1 amu =0.166 x 10⁻²³ = 1.66 x 10⁻²⁴ g
(complete octet). (Shows all properties of
comp'd) Some Basic
No. of times 1 atom of an AM = [Mass of 1 atom of element (in
eg. NH₃ =>
No. of atoms Concepts of Atomic
element is heavier than 12th gm)]/
present in 1 Mass
Tetra-
molecule of
Atomicity Molecule Chemistry part of mass of 1 atom of ¹²₆C. [(Mass of 1 atom of ¹²₆C (in gm)) /12]
atomic
substance Atomic Gram Atomic mass of elements is expressed in gm
mass & Atomic Mass rather than amu with same numeral value
Homoatomic eg. H₂, O₂, O₃
Types No. of times 1 molecule of a
Heteroatomic eg.CH₄, NH₃ molecul Molecular MM = [Mass of 1 molecule (in gm)]/
substance is heavier than 12th
ar mass Mass
part of mass of 1 atom of ¹²₆C
[(Mass of 1 atom of ¹²₆C (in gm)) /12]
Smallest particle of element that can take part in Chemical reac'n &
can't exist freely due to incomplete octet. (Exception - Noble gases) Atom
Gram Molecular mass of substance is expressed in
Molecular Mass gm rather than amu with same numeral value
Under similar conditions of temp. & pressure, equal
volumes of all gases contain equal no. of molecules. Avogadro Law
Average Used for elements which exist in AAM = [Mass of 1 isotope x %age +
FM of NaCl = Mass calculated according to formula of ionic comp'd Formula Atomic Mass nature in a no. of stable isotopic forms. Mass of another isotope x %age] / 100
23+35.5 = 58.5 u (Ionic comp'd don't exist in discrete molecules) Mass
n= given mass (gm)/ 1 mol related Law of During chemical reaction , Initial mass of
W/GAM molecular atom = to Conservation mass of reactant is equal to reactant = Mass of
mass(gm) Its GAM GAM of Mass mass of product , when product + Mass of
Mass of 1 mol Mole Mole is that (Lavoisier) reaction is 100% complete. unreacted reactant
n= W/GMM molecule = Its related to quantity of
Law of In Compound, ratio of
GMM GMM substance
Constant different element with respect eg. CO2 =>
which contain Mole Proportion to their masses is always fixed, Mass => 3:8
n= Given no 1 mol = 6.022 Mol
of particles/ x 10²³ related to
as many Concept Laws of (Proust) no matter how it's prepared
particles as
N⁰[6.022 x particles of no. of there are in 12
Chemical Law of When different masses of one element which
10²³] substance particles g of Carbon Combination multiple combines with fixed mass of another element to
P₁V₁/T₁ = 1 mol gas at NTP Mole proportions form a no. of compound, then the different masses
n= V (Dalton) of the element bear a simple whole no. ratio.
P₂V₂/T₂ occupy 22.4 L Vol. related to
given (L)
NTP known as Molar Vol. of gas Gay- States that, gases react with each other in the simple ratio
/ 22.4(L)
Given Vol. at NTP Lussac's of their volume & if the product is also in gaseous state,
Law of the volume of product also bears a simple ratio with volume
VD of Substance VD = Density of Substance(in gas)/ Relationship of Vapour gaseous of gaseous reactants provided all the volume are measured
volume under similar condition of temp. and pressure.
x 2 = GMM Density of H₂ in gas Density(Unitless) & GMM
When mass of atoms or molecules is 1 amu = [Mass of 1 atom of ¹²₆C
Smallest particle of element or comp'd which Relative
expressed in relation to some other (1.9924 x 10⁻²³)] / 12
has independent existence & stable System of mass elements like Carbon. Unit => amu / u 1 amu =0.166 x 10⁻²³ = 1.66 x 10⁻²⁴ g
(complete octet). (Shows all properties of
comp'd) Some Basic
No. of times 1 atom of an AM = [Mass of 1 atom of element (in
eg. NH₃ =>
No. of atoms Concepts of Atomic
element is heavier than 12th gm)]/
present in 1 Mass
Tetra-
molecule of
Atomicity Molecule Chemistry part of mass of 1 atom of ¹²₆C. [(Mass of 1 atom of ¹²₆C (in gm)) /12]
atomic
substance Atomic Gram Atomic mass of elements is expressed in gm
mass & Atomic Mass rather than amu with same numeral value
Homoatomic eg. H₂, O₂, O₃
Types No. of times 1 molecule of a
Heteroatomic eg.CH₄, NH₃ molecul Molecular MM = [Mass of 1 molecule (in gm)]/
substance is heavier than 12th
ar mass Mass
part of mass of 1 atom of ¹²₆C
[(Mass of 1 atom of ¹²₆C (in gm)) /12]
Smallest particle of element that can take part in Chemical reac'n &
can't exist freely due to incomplete octet. (Exception - Noble gases) Atom
Gram Molecular mass of substance is expressed in
Molecular Mass gm rather than amu with same numeral value
Under similar conditions of temp. & pressure, equal
volumes of all gases contain equal no. of molecules. Avogadro Law
Average Used for elements which exist in AAM = [Mass of 1 isotope x %age +
FM of NaCl = Mass calculated according to formula of ionic comp'd Formula Atomic Mass nature in a no. of stable isotopic forms. Mass of another isotope x %age] / 100
23+35.5 = 58.5 u (Ionic comp'd don't exist in discrete molecules) Mass
