Chemistry

Atomic Structure and Chemical bonding

De Broglie equation λ = h / mv or λ = h / p

Heisenberg`s Uncertainty Principle

Number of waves in nth orbit

h

Schrodinger wave equation

Energy of hydrogen atom E_n =

Angular momentum of the electron =

Spin angular momentum of electron =

Bond order = ------- N_b --- is no of electrons in bonding molecular orbital

N_a --- is no of electrons in antibonding molecular orbitals

Radius of n^th orbit of Hydrogen atom is = 5.29 nm

No. of orbitals in n^th shell = n²

No of electrons in n^th shell =2n²

The no of spectral lines when an electron jumps from n^th level to ground level (n=1)

=

No of spherical nodes in an orbital =

Type of Hybridization	Orbitals participating	Examples
		CH4 ,SiF4 ,OF2 ,H2O ,NH3, ,
sp3d		PCl5 ,,

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The Solid State

Bragg’s equation -----

Density formula gcm^-3

Radius ratio and Coordination number

Radius ratio	Structure	Coordination no	Example
0.155-0.225	Planar triangular	3	B2O3
0.225-0.414	Tetrahedral	4	ZnS, CuCl, CuBr, CuI, BaS, HgS
0.414-0.732	Octahedral	6	NaCl, MgO, NaBr, CaS , CaO
0.732-1.000	Cubic	8	CsCl, CsBr, TlBr, NH4Br

Relationship between the nearest neighbor distance and radius of atom and edge length (a)

Unit Cell	Distance bt Nearest neighbor (d)	Radius (r)
Simple Cubic
Face centered cubic
Body centered cubic

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Solution

Mass % of component A is =

Volume % of component A is =

Parts per million (ppm) =

(W_A is the mass solute & W_solution is the mass of total solution)

Molarity of a solution =

Molality of a solution =

Mole fraction of solute A is ( x_A) = Mole fraction of solvent B is (x_B) = ; ( x_A + x_B = 1)

Normality = =

(E_equivalent is the no. of gram equivalent of solute)

Molarity equation M₁V₁ = M₂ V₂ ;

Henary `s law m = K.p

Raoult`s law for binary solution of Volatile liquids

Raoults law for binary solution of Non Volatile liquids

Determination of molar masses of solute by using colligative properties

1. Relative lowering of vapour pressure

2. Elevation in boiling point

3.Depression in freezing point

4. Osmotic pressure

Abnormal molar masses and Van`t Hoff factor

Degree of dissociation (ά) = =

Degree of association (ά) = =

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Thermodynamics

First law of thermodynamic

Enthalpy change or ( for gaseous Rx )

Entropy and entropy change

Free energy change

- (for electric work)

Efficiency of fuel cell =

Standard free energy change

; K =

Third law of thermodynamics S =

Spontaneity and Temperature

Sign of Enthalpy	Sign of Entropy	Value of T	Spontaneity
+ve	+ve	high	Spontaneous
+ve	+ve	Low	Non Spontaneous
+ve	-ve	Low/high	Non Spontaneous
-ve	-ve	low	Spontaneous
-ve	-ve	high	Non Spontaneous
-ve	+ve	Low/high	Spontaneous

for isothermal process

for isobaric process

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Electrochemistry

Faraday`s first law of electrolysis W = ZQ or W = Zit

Faraday`s second law of electrolysis

=

Conductance = ; Conductivity =

Equivalent conductance = Λ_eq

Molar conductance = Λ_m =

Units of Molar conductance Ω^-1cm²mol^{-1 ;} Scm²mol^-1 ; Sm²mol^-1 (SI units)

Units of Equivalent conductance Ω^-1cm²gequ^-1 ; Scm²gequ^-1 ; Sm²gequ^-1

Kohlrausch`s law

for a hypothetical reaction Kohlrausch`s law becomes

Degree of dissociation

Dissociation constant of a weak electrolyte =

Solubility of a sparingly soluble salt =

Nernest equation =

Chemical Kinetics

Rate of reaction = (for a reaction A → P)

For a Rx. the unique reaction rate is

Law of mass action for is rate =

and rate law is rate = Where ά and β are the experimental

found exponent and there sum is known as order of reaction

Units of rate constant for different order reactions are

For zero order Rx -- Mol L^-1 S^-1

For 1^st order Rx. -- S^-1

For 2^nd order Rx. -- L Mol^-1 S^-1

Integrated rate equation for different order reactions

Zero order where [A_o] is the initial concentration and [A] is final concentration

1^st order or where is initial conc. and x is the amount consumed

Half life equation for different order reactions for zero order

For 1^st order Rx.

Amount left after n half lives where n is no. of half lives i.e.

Calculation of order of a reaction by half life method

n is the order of reaction

Arrhenius equation or

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Surface Chemistry

Freundlich adsorption isotherm

Langmuir adsorption isotherm

Type of colloidal system

S.No.	Dispersed Phase	Dispersion Medium	Name	Example
1	Solid	Solid	Solid Sol	Some coloured glasses, gemstone
2	Solid	Liquid	Sol	Some paints , cell fluids
3	Solid	Gas	Aerosol	Smoke , dust
4	Liquid	Solid	Gel	Cheese , butter , jellies
5	Liquid	Liquid	Emulsion	Milk , hair cream
6	Liquid	Gas	Aerosol	Fog , mist, cloud
7	Gas	Solid	Solid foam	Pumice stone , foam rubber
8	Gas	Liquid	Foam	Froth, whipped cream soap lather

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