General topics:
Concept of atoms and molecules;
Dalton’s atomic theory;
Mole concept; Chemical formulae; Balanced chemical equations; Calculations (based on mole concept) involving common oxidation-reduction, neutralisation, and displacement reactions;
Concentration in terms of mole fraction, molarity, molality and normality.
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Showing posts with label Physical Chemistry. Show all posts
Showing posts with label Physical Chemistry. Show all posts
Monday, October 29, 2007
IIT JEE Chemistry Questions Ch.2. GASEOUS, LIQUID AND SOLID STATES
Gaseous and liquid states: Absolute scale of temperature, ideal gas equation; Deviation from ideality, van der Waals equation; Kinetic theory of gases, average, root mean square and most probable velocities and their relation with temperature; Law of partial pressures; Vapour pressure; Diffusion of gases.
Solid state: Classification of solids, crystalline state, seven crystal systems (cell parameters a, b, c, alpha, beta, gamma), close packed structure of solids (cubic), packing in fcc, bcc and hcp lattices; Nearest neighbours, ionic radii, simple ionic compounds, point defects.
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Solid state: Classification of solids, crystalline state, seven crystal systems (cell parameters a, b, c, alpha, beta, gamma), close packed structure of solids (cubic), packing in fcc, bcc and hcp lattices; Nearest neighbours, ionic radii, simple ionic compounds, point defects.
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IIT JEE Chemistry Questions Ch.3. ATOMIC STRUCTURE
Atomic structure :
Bohr model,
spectrum of hydrogen atom,
quantum numbers;
Wave-particle duality,
de Broglie hypothesis;
Uncertainty principle;
Qualitative quantum mechanical picture of hydrogen atom,
shapes of s, p and d orbitals;
Electronic configurations of elements (up to atomic number 36);
Aufbau principle;
Pauli’s exclusion principle and
Hund’s rule;
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Direct theory questions
1. Explain the following terms
a. Energy level
b. Sublevel
c. orbital
d.aufbau order
e. Hund's rule
f. principal quantum number
g. secondary quantum number
h. magentic quantum number
i. spin quantum number
j. Pauli exclusion principle
2. What is Bohr theory of atomic struncture?
3. Wuat is the quantum mechanical theory or model of atomic structure?
Aplication questions
1. How does Hund's rule explain the fact that oxygen has two unpaired electrons?
2. Explain why the maximum number of electrons in the fifth energy level is 50 (2*2^2).
3. Tell what is wrong in the following set of quantum numbers
2,2,0, +1/2
Bohr model,
spectrum of hydrogen atom,
quantum numbers;
Wave-particle duality,
de Broglie hypothesis;
Uncertainty principle;
Qualitative quantum mechanical picture of hydrogen atom,
shapes of s, p and d orbitals;
Electronic configurations of elements (up to atomic number 36);
Aufbau principle;
Pauli’s exclusion principle and
Hund’s rule;
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Direct theory questions
1. Explain the following terms
a. Energy level
b. Sublevel
c. orbital
d.aufbau order
e. Hund's rule
f. principal quantum number
g. secondary quantum number
h. magentic quantum number
i. spin quantum number
j. Pauli exclusion principle
2. What is Bohr theory of atomic struncture?
3. Wuat is the quantum mechanical theory or model of atomic structure?
Aplication questions
1. How does Hund's rule explain the fact that oxygen has two unpaired electrons?
2. Explain why the maximum number of electrons in the fifth energy level is 50 (2*2^2).
3. Tell what is wrong in the following set of quantum numbers
2,2,0, +1/2
IIT JEE Chemistry Questions Ch.5. BONDING AND MOLECULAR STRUCTURE
Orbital overlap and covalent bond;
Hybridisation involving s, p and d orbitals only;
Orbital energy diagrams for homonuclear diatomic species;
Hydrogen bond;
Polarity in molecules, dipole moment (qualitative aspects only);
VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, trigonal bipyramidal, tetrahedral and octahedral).
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Theory Questions
Orbital overlap and covalent bond;
1. State the octet rule?
2. What are the instances where octet rule was found inadequate?
3. What is covalent bond?
4. What is coordinate covalent bond?
5. Name some molecules of having same atoms that have double bond.
6. Name some molecules of having same atoms that have triple double bond.
7. Name some compounds where N atom does not complete it octet.
8. do covalent bonds have directional character.
9. what is a coordinate bond?
10. give some examples of molecules having coordinate bonds.
Hybridisation involving s, p and d orbitals only;
1. Explain the need for the concept of hybridization?
2. Exlain the concept of hybridization.
3.
Orbital energy diagrams for homonuclear diatomic species;
VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, trigonal bipyramidal, tetrahedral and octahedral).
1. What is VSEPR formulated? What does it try to explain?
2. What are the postulates of VSEPR theory?
3. What is the strength of repulsive forces over various possible pairs of electrons?
4.Why there are distortions in certain molecules from standard geometrical shapes indicated by the number of electron pairs?
5. Give examples of molecules that have linear arrangement of atoms.
6. Give examples of molecules that have trigonal planar arrangement of atoms.
7. Give examples of molecules that have tetrahedral arrangement of atoms.
8.Give examples of molecules that have trigonal bipyramidal arrangement of atoms.
9. Give examples of molecules that have octahedral arrangement of atoms.
10. Give examples of molecules that have pentagonal bipyramidal arrangement of atoms.
11. Give the geometrical shapes for molecules havng 2 to 7 electronic pairs around the central atom in a molecule.
Polarity in molecules, dipole moment (qualitative aspects only);
Hydrogen bond;
Concepts
1. State the octet rule?
2. What are the instances where octet rule was found inadequate?
3. Give important features of valence bond theory.
4. give different overlaps between 's' and 'p' orbitals and also give one example of each.
5. Explain the need for the concept of hybridization?
6. Exlain the concept of hybridization.
7. Explain the formation of sigma bond.
8.Explain the formation of pi bond.
9. Define bond energy?
10. What is ionic bond?
11. What is covalent bond?
12. What is coordinate covalent bond?
Applications and Examples
1. Why is H-F bond polar?
2. Give the geometry of hyubridised orbital in the following compounds.
a. Methane
b. water
c. ethyne
d. Boron trifluoride
e. Ammonia
f. BeF-2
g. ethene
3. Why bond angle in ammonia molecule is less than the expected tetrahedral bond angle?
4. There is only one pi-bond in ethylene molecule but here are two pi-bonds in the acytylene moecule. Explain.
5. Why a sigma bond is stronger than pi-bond?
6. The bond energy of PCl-3 is larger than the bond energy ni PCl-5. Why?
7. Bond energy in HF is larger than HI. Why?
8. Why H-O-H bond angle in water molecule is reduced to 104° 35'?
Hybridisation involving s, p and d orbitals only;
Orbital energy diagrams for homonuclear diatomic species;
Hydrogen bond;
Polarity in molecules, dipole moment (qualitative aspects only);
VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, trigonal bipyramidal, tetrahedral and octahedral).
------------------
Theory Questions
Orbital overlap and covalent bond;
1. State the octet rule?
2. What are the instances where octet rule was found inadequate?
3. What is covalent bond?
4. What is coordinate covalent bond?
5. Name some molecules of having same atoms that have double bond.
6. Name some molecules of having same atoms that have triple double bond.
7. Name some compounds where N atom does not complete it octet.
8. do covalent bonds have directional character.
9. what is a coordinate bond?
10. give some examples of molecules having coordinate bonds.
Hybridisation involving s, p and d orbitals only;
1. Explain the need for the concept of hybridization?
2. Exlain the concept of hybridization.
3.
Orbital energy diagrams for homonuclear diatomic species;
VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, trigonal bipyramidal, tetrahedral and octahedral).
1. What is VSEPR formulated? What does it try to explain?
2. What are the postulates of VSEPR theory?
3. What is the strength of repulsive forces over various possible pairs of electrons?
4.Why there are distortions in certain molecules from standard geometrical shapes indicated by the number of electron pairs?
5. Give examples of molecules that have linear arrangement of atoms.
6. Give examples of molecules that have trigonal planar arrangement of atoms.
7. Give examples of molecules that have tetrahedral arrangement of atoms.
8.Give examples of molecules that have trigonal bipyramidal arrangement of atoms.
9. Give examples of molecules that have octahedral arrangement of atoms.
10. Give examples of molecules that have pentagonal bipyramidal arrangement of atoms.
11. Give the geometrical shapes for molecules havng 2 to 7 electronic pairs around the central atom in a molecule.
Polarity in molecules, dipole moment (qualitative aspects only);
Hydrogen bond;
Concepts
1. State the octet rule?
2. What are the instances where octet rule was found inadequate?
3. Give important features of valence bond theory.
4. give different overlaps between 's' and 'p' orbitals and also give one example of each.
5. Explain the need for the concept of hybridization?
6. Exlain the concept of hybridization.
7. Explain the formation of sigma bond.
8.Explain the formation of pi bond.
9. Define bond energy?
10. What is ionic bond?
11. What is covalent bond?
12. What is coordinate covalent bond?
Applications and Examples
1. Why is H-F bond polar?
2. Give the geometry of hyubridised orbital in the following compounds.
a. Methane
b. water
c. ethyne
d. Boron trifluoride
e. Ammonia
f. BeF-2
g. ethene
3. Why bond angle in ammonia molecule is less than the expected tetrahedral bond angle?
4. There is only one pi-bond in ethylene molecule but here are two pi-bonds in the acytylene moecule. Explain.
5. Why a sigma bond is stronger than pi-bond?
6. The bond energy of PCl-3 is larger than the bond energy ni PCl-5. Why?
7. Bond energy in HF is larger than HI. Why?
8. Why H-O-H bond angle in water molecule is reduced to 104° 35'?
IIT JEE Chemistry Questions Ch. 6 ENERGETICS
Energetics:
First law of thermodynamics;
Internal energy, work and heat, pressure-volume work;
Enthalpy, Hess’s law;
Heat of reaction, fusion and vapourization;
Second law of thermodynamics;
Entropy;
Free energy;
Criterion of spontaneity.
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1. Define the following terms;
a. Thermodynamics.
b. Open system
c. Heat capacity
d. Heat of formation
e. Enthalpy
f. Heat of combustion
g. Heatof neutralization
h. Isothermal process
i. Isothermal process
j. Intramole energy
k. Intermole energy
l. Molar heat energy
m. Heat of reaction
n. Heat of combustion
o. Adiabatic process
p. Exothermic reaction
q. Endothermic reaction
2. State the first law of thermodynamics in its two forms.
3. Give two statements of law conservation of energy.
4. What is Kirchoff's equation?
5. How do you express a thermochemical equation?
First law of thermodynamics;
Internal energy, work and heat, pressure-volume work;
Enthalpy, Hess’s law;
Heat of reaction, fusion and vapourization;
Second law of thermodynamics;
Entropy;
Free energy;
Criterion of spontaneity.
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1. Define the following terms;
a. Thermodynamics.
b. Open system
c. Heat capacity
d. Heat of formation
e. Enthalpy
f. Heat of combustion
g. Heatof neutralization
h. Isothermal process
i. Isothermal process
j. Intramole energy
k. Intermole energy
l. Molar heat energy
m. Heat of reaction
n. Heat of combustion
o. Adiabatic process
p. Exothermic reaction
q. Endothermic reaction
2. State the first law of thermodynamics in its two forms.
3. Give two statements of law conservation of energy.
4. What is Kirchoff's equation?
5. How do you express a thermochemical equation?
IIT JEE Chemistry Questions Ch. 7. CHEMICAL EQUILIBRIA
Chemical equilibrium:
Law of mass action;
Equilibrium constant,
Le Chatelier's principle (effect of concentration, temperature and pressure); Significance of DG and DGo in chemical equilibrium;
Solubility product,
common ion effect,
pH and buffer solutions;
Acids and bases (Bronsted and Lewis concepts);
Hydrolysis of salts.
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Law of mass action;
Equilibrium constant,
Le Chatelier's principle (effect of concentration, temperature and pressure); Significance of DG and DGo in chemical equilibrium;
Solubility product,
common ion effect,
pH and buffer solutions;
Acids and bases (Bronsted and Lewis concepts);
Hydrolysis of salts.
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IIT JEE Chemistry Questions Ch.8 ELECTROCHEMISTRY
Electrochemistry:
Electrochemical cells and cell reactions;
Standard electrode potentials;
Nernst equation and its relation to DG;
Electrochemical series, emf of galvanic cells;
Faraday's laws of electrolysis;
Electrolytic conductance, specific, equivalent and molar conductivity, Kohlrausch's law;
Concentration cells.
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1. What electrolysis?
2. State Faraday's first law of electrolysis
3. State Faraday's second law of electrolysis.
4. What is electrochemical cell?
5.How is galvanic cell represented?
6. what is a reference electrode?
7. what is a Standard Hydrogen Electrode?
8. what is the purpose of a salt bridge?
9. Distinguish between electrolytic and electrochemical cell.
10. What is standard oxidation potential?
11. What is an electrochemical series?
12. Give the Nernst equation.
Electrochemical cells and cell reactions;
Standard electrode potentials;
Nernst equation and its relation to DG;
Electrochemical series, emf of galvanic cells;
Faraday's laws of electrolysis;
Electrolytic conductance, specific, equivalent and molar conductivity, Kohlrausch's law;
Concentration cells.
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1. What electrolysis?
2. State Faraday's first law of electrolysis
3. State Faraday's second law of electrolysis.
4. What is electrochemical cell?
5.How is galvanic cell represented?
6. what is a reference electrode?
7. what is a Standard Hydrogen Electrode?
8. what is the purpose of a salt bridge?
9. Distinguish between electrolytic and electrochemical cell.
10. What is standard oxidation potential?
11. What is an electrochemical series?
12. Give the Nernst equation.
IIT JEE Chemistry Questions Ch 9. SOLUTIONS
Solutions:
Raoult's law;
Molecular weight determination from lowering of vapour pressure, elevation of boiling point and depression of freezing point.
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Raoult's law;
Molecular weight determination from lowering of vapour pressure, elevation of boiling point and depression of freezing point.
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Sunday, October 28, 2007
IIT JEE Chemistry Questions Ch.10. CHEMICAL KINETICS
Chemical kinetics:
Rates of chemical reactions;
Order of reactions;
Rate constant;
First order reactions;
Temperature dependence of rate constant (Arrhenius equation).
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Theory
1. Define or explain each of the following concepts
a) Chemical kinetics
b) reaction rate
c) rate law
d) reaction constant
e) reaction mechanism
f) rate determining step
g) Law of Mass Action
h) Order of reaction of a reactant
i) Overall order of reaction
j) Collision theory
k) activation energy
l) catalyst
k) negative catalyst
l) inhibitor
2. What changes rate constant of a reaction for a given set of reactants?
3. What changes rate of reaction for a given set of reactants?
4. How can you predict change in rate of reaction if you know the rate law?
5. What are units of rate of reaction?
6. What is the order of a reaction? How is it determined?
7. When are the units of rate constant and rate of reaction identical?
8. Describe the behaviour of rate constant with respect to temperature?
9. what are the units of activation energy?
10. How do you measure activation energy?
Rates of chemical reactions;
Order of reactions;
Rate constant;
First order reactions;
Temperature dependence of rate constant (Arrhenius equation).
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Theory
1. Define or explain each of the following concepts
a) Chemical kinetics
b) reaction rate
c) rate law
d) reaction constant
e) reaction mechanism
f) rate determining step
g) Law of Mass Action
h) Order of reaction of a reactant
i) Overall order of reaction
j) Collision theory
k) activation energy
l) catalyst
k) negative catalyst
l) inhibitor
2. What changes rate constant of a reaction for a given set of reactants?
3. What changes rate of reaction for a given set of reactants?
4. How can you predict change in rate of reaction if you know the rate law?
5. What are units of rate of reaction?
6. What is the order of a reaction? How is it determined?
7. When are the units of rate constant and rate of reaction identical?
8. Describe the behaviour of rate constant with respect to temperature?
9. what are the units of activation energy?
10. How do you measure activation energy?
IIT JEE Chemistry Questions Ch. 11. SURFACE CHEMISTRY
Surface chemistry:
Elementary concepts of adsorption (excluding adsorption isotherms);
Colloids: types, methods of preparation and general properties;
Elementary ideas of emulsions, surfactants and micelles (only definitions and examples).
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1. What is adsorption?
2. distinguish between adsoprtion and absoprtion.
3. Distinguish between physical adsoprtion and chemical adsoprtion.
4. What is adsorbent?
5. what is adsorbate?
6. Explain the role of adsorption in catalysis.
7. Distinguish between emulsion and gel.
8. Distinguish between colloid solution and true solution.
9. Distinguish between lyophilic colloids and lyophobic colloids.
Elementary concepts of adsorption (excluding adsorption isotherms);
Colloids: types, methods of preparation and general properties;
Elementary ideas of emulsions, surfactants and micelles (only definitions and examples).
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1. What is adsorption?
2. distinguish between adsoprtion and absoprtion.
3. Distinguish between physical adsoprtion and chemical adsoprtion.
4. What is adsorbent?
5. what is adsorbate?
6. Explain the role of adsorption in catalysis.
7. Distinguish between emulsion and gel.
8. Distinguish between colloid solution and true solution.
9. Distinguish between lyophilic colloids and lyophobic colloids.
IIT JEE Chemistry Question Bank Ch.12. NUCLEAR CHEMISTRY
Nuclear chemistry:
Radioactivity:
isotopes and isobars;
Properties of alpha, beta and gamma rays;
Kinetics of radioactive decay (decay series excluded), carbon dating;
Stability of nuclei with respect to proton-neutron ratio;
Brief discussion on fission and fusion reactions.
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1. Isotopes have same atomic number. State True or false.
2. What is atomic number(Z)?
3. what is Mass Number (A)?
4. What is neutron number (N)?
5. What are isobars?
6. What is mass defect?
7. What is binding energy?
8. what is radioactivity?
9. What is radioactive constant?
10. What is half life period?
11. What is artificial transmutation?
Radioactivity:
isotopes and isobars;
Properties of alpha, beta and gamma rays;
Kinetics of radioactive decay (decay series excluded), carbon dating;
Stability of nuclei with respect to proton-neutron ratio;
Brief discussion on fission and fusion reactions.
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1. Isotopes have same atomic number. State True or false.
2. What is atomic number(Z)?
3. what is Mass Number (A)?
4. What is neutron number (N)?
5. What are isobars?
6. What is mass defect?
7. What is binding energy?
8. what is radioactivity?
9. What is radioactive constant?
10. What is half life period?
11. What is artificial transmutation?
IIT JEE Chemistry Questions 20. Inductive and Resonance Effects
Resonance and hyperconjugation;
Keto-enol tautomerism;
Determination of empirical and molecular formulae of simple compounds (only combustion method);
Hydrogen bonds: definition and their effects on physical properties of alcohols and carboxylic acids;
Inductive and resonance effects on acidity and basicity of organic acids and bases; Polarity and inductive effects in alkyl halides;
Reactive intermediates produced during homolytic and heterolytic bond cleavage; Formation, structure and stability of carbocations, carbanions and free radicals.
Keto-enol tautomerism;
Determination of empirical and molecular formulae of simple compounds (only combustion method);
Hydrogen bonds: definition and their effects on physical properties of alcohols and carboxylic acids;
Inductive and resonance effects on acidity and basicity of organic acids and bases; Polarity and inductive effects in alkyl halides;
Reactive intermediates produced during homolytic and heterolytic bond cleavage; Formation, structure and stability of carbocations, carbanions and free radicals.
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