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CHAPTER NO. 1 || STOICHIOMETRY |
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Define: (i) Mole (ii) Limiting reactant
(iii) Molar Volume (v) Avogadro's number |
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Differentiate between: (i) Theoretical
Yield and Practical yield |
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Numerical: 1,2,3,5 |
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CHAPTER NO. 2 || ATOMIC STRUCTURE |
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Define : (i) All series of Hydrogen atom |
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1. Define quantum
numbers? Give use and significance of each quantum number 2. Give the postulate
of Bohr atomic theory derive Rydberg equation 3. What is
Radioactivity? Write properties of alpha, beta and gamma rays. 4. Write the electronic
configuration of the following and also give the number of protons and
electrons in each. (i) Cu(Z=29) (ii) Mg+2 (Z=12) (iii) Cl-1(
Z=17) (iv) Mo (Z =42) (v) Ag ( Z = 47) |
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Differentiate the
following: (i) Line
and Continuous Spectrum |
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Numerical: 1,2 |
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CHAPTER NO. 3 || THEORIES OF COVALENT BONDING & SHAPES OF
MOLECULES |
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Differentiate between the following: (i) Sigma and pi bond (ii) Valence
Bond Theory and molecular orbital theory |
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Define (i) Bond Energy (ii) Bond Length |
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1. Explain shapes of following molecules on the basis of hybrid orbital model and electron pair repulsion model. (i) NH3 (ii) H2O (iii) CH(iv) BeCl2: (v) CHCI3 (vi) BCI3 (vii) C2H4 2. Explain atomic orbital hybridization with respect to
sp3,sp2 and sp modes of hybridization for CH4, C2H4,
and C2H2. |
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Give reasons: (i) Sigma Bond is stronger than Pi Bond (ii) HF has
greater ionic character than HCL |
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CHAPTER NO. 4 || STATES OF MATTER I :
GAS |
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State and explain: (i) Boyles law (ii) Charles Law
(iii)Dalton’s Law (iv) Graham’s law of Diffusion |
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1. Derive General Gas
Equation. 2. Explain the causes
of deviation of real gases from ideal behavior. |
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Define: (i) Plasma and its properties(ii) Absolute
zero |
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Numerical: 2,4,6,7,8 |
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CHAPTER NO. 5 || STATES OF MATTER II : LIQUIDS |
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Define (i) Molar heat of fusion and
vaporization (ii) Liquid crystals with uses (iii) Dipole Dipole Moment (iv)
London Dispersion forces |
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1. Define Hydrogen
Bonding and its applications 2. Describe Surface
tension and capillary action. |
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Give reasons: (i) Evaporation is cooling
process. (ii) Liquid rises in capillary tube. (iii) A falling drop of liquid
is spherical (iv) Honey is more viscous than water (iv) Mercury has its
meniscus upwad. |
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CHAPTER NO. 6 || STATES OF MATTER III : SOLIDS |
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Define (i) Allotropy (ii) Sublimation (iii) Unit Cell |
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Differentiate between (i)Isomorphism and Polymorphism (ii) Crystalline
solids and amorphous solids |
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Explain different types
of crystalline solids |
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Give reasons: (i) Why diamond is non conductor
and graphite is conductor (ii) Some solids are sublime in nature (iii)
Compressibility of solids is nearly zero |
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CHAPPTER NO. 7|| CHEMICAL EQUILIBRIUM |
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1. Define and explain
common on effect with examples. 2. Give relationship
between Kc and Kp 3. State and explain
Law of Mass action. State Le-chatelier's principle and discuss its industrial
applications using Haber’s process. |
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Numerical: 1,2,3,4 |
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CHAPTER NO. 8|| ACID, BASES AND SALTS |
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Define following terms: (i) pH and pOH
(ii) Salt (iii) Buffer solution |
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1. Explain
Bronsted-Lowry theory of acids and bases. What is meant by conjugate acid
base pair give examples. 2. Write equations and
indicate acid base pairs of following: (i) acetic acid and
ammonia (ii) Hydrochloric acid and water. 3. Define Hydrolysis.
Explain behavior of following in aqueous solution (i) K2CO3
(ii) (NH4)2SO4 (iii) NaNO3 |
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Numerical: 1,2 |
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CHAPTER NO. 9|| CHEMICAL KINETICS |
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Define following terms: (i) Rate
expression (ii) Rate constant (iii) Threshold energy (iv) Energy of
Activation. (v) Order of reaction |
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Give reasons: (i) The energy of activation
decrease with increase in temperature. (ii) Milk sour more rapidly in summer
than in winter. (iii) Powdered CaCO3 reacts quickly with HCL acid than solid
lump of marble. (iv) Rate of reaction increase with rise in temperature. |
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What is rate of reaction? Discuss various
factors which affect the rate of reaction. |
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Differentiate
between: (1) Rate
of reaction and Rate constant (ii) Rate constant and Specific rate constant
(iii) Promoters and Inhibitors (iv) Threshold and Activation energy |
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CHAPTER NO. 10|| SOLUTION &
COLLOIDS |
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Define following terms: (i) Molarity (ii)
Molality |
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Give reasons: (i) Why n-hexane is immiscible in
water (ii) Boiling point of liquid get raised when non volatile solute is
added. |
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1. State Raoult’s Law and
derive mathematical equation. 2. Define Osmosis and
Osmotic pressure. Give examples from daily life. |
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Differentiate
between: (i)
Miscible and immiscible liquids (ii)
Ideal and non ideal solution (iii) True solution,
colloidal solution and suspension on the basis of (i) Particle size (ii)
Visibility |
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Numerical: 1,2 |
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CHAPTER NO. 11|| THERMOCHEMISTRY |
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Define (i) Intensive properties (ii)
Extensive properties (iii) System (iv) State of the system (v) Standard heat
of formation |
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1. State and explain
Hess's law of constant heat summation along with its application. 2. Drive
Pressure-Volume work expression on the basis of the First law of
Thermodynamics. 3. What is meant by
enthalpy? Why is |
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Numericals : 1,3,4,6 |
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CHAPTER NO. 12|| ELECTROCHEMISTRY |
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Differentiate between the following: (i) Oxidation and Reduction (ii) Primary
and secondary cells |
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1. Define oxidation
number and determine oxidation number 2. Balance following
chemical equations by ion electron method: 3. What is corrosion? Describe its
cause and prevention. 4. Define an electrochemical series?
Give its properties. |
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