Published by National Book Foundation, Islamabad
CHEMISTRY
For Class-XI
1. STOICHIOMETRY
Introduction
1.1 Mole and Avogadro’s Number
1.2 Mole Calculations
1.3 Percentage Composition
1.4 Excess and Limiting Reagents
1.5 Theoretical Yield and Actual Yield as percentage
2. ATOMIC STRUCTURE
Introduction
2.1 Discharge Tube Experiments
2.2 Application of Bohr’s Model
2.2.1 Derivation of Radius, Energy, Frequency, Wave Length, Wave Number
2.2.2 Spectrum of Hydrogen Atom
2.2.3 Defects of Bohr’s Theory
2.3 Planck’s Quantum Theory_
2.3.1 Postulates With Derivation of E =hcν
2.4 X-Rays
2.4.1 Production, Properties and Uses
2.4.2 Types
2.4.3 X-rays and Atomic Number
2.4.4 Moseley’s Experiment
2.4.5 Moseley’s Law
2.5 Quantum Numbers and Orbitals
2.5.1 Principle Quantum Number
2.5.2 Azimuthal Quantum Number
2.5.3 Magnetic Quantum Number
2.5.4 Spin Quantum Number
2.5.5 Shapes of s, p and d Orbitals
2.6 Electronic Configuration
2.6.1 Aufbau Principle
2.6.2 Pauli’s Exclusion Principle
2.6.3 Hund’s Rule
2.6.4 Electronic Configurations
3. THEORIES OF COVALENT BONDING AND SHAPES OF MOLECULES
Introduction
3.1 Shapes of molecules
3.1.1 VSEPR
3.1.2 Resonance
3.2 Theories of covalent bonding
3.2.1 VBT and hybridization
3.2.2 MOT
3.3 Bond Characteristics
3.3.1 Bond Energy
3.3.2 Bond Length
3.3.3 Ionic Character
3.3.4 Dipole Moment
3.4 Effect of Bonding on Physical and Chemical Properties
3.4.1 Solubility of Ionic and Covalent Compounds
3.4.2 Reactions of Ionic and Covalent Compounds
3.4.3 Directional and Non Directional Nature of Ionic and Covalent Bonds
4. STATES OF MATTER I: GASES
Introduction
4.1 Kinetic Molecular Theory of Gases
4.1.1 Postulates of Kinetic Molecular Theory
4.1.2 Pressure and Its Units
4.2 Absolute Temperature Scale on the Basis of Charles Law
4.2.1 Brief recall of Boyle’s and Charles’ Law
4.2.2 Graphical Explanation of Absolute Zero
4.3 Avogadro’s Law
4.4 Ideal Gas Equation
4.4.1 Derivation
4.4.2 Gas Constant and its Units
4.5 Deviation From Ideal Gas Behavior
4.5.1 Graphical Explanation
4.5.2 Causes for Deviation
4.6 Van der Waals Equation
4.6.1 Volume Correction
4.6.2 Pressure Correction
4.7 Dalton’s Law of Partial Pressure
4.8 Graham’s Law of Diffusion and Effusion
4.9 Liquefaction of Gases
4.9.1 Joule-Thomson Effect
4.9.2 Linde’s Method of Liquefaction of Gases
4.10 Fourth State of Matter: Plasma
5. STATES OF MATTER II: LIQUIDS
Introduction
5.1 Kinetic Molecular Interpretation of Liquids
5.1.1 Simple properties of Liquids Describing Diffusion, Compression, Expansion, Motion of Molecules, Kinetic Energy
5.2 Intermolecular Forces (Vander Waals Forces)
5.2.1 Dipole-Dipole interaction
5.2.2 Hydrogen Bonding
5.2.3 London Forces
5.3 Energetics of Phase Changes
5.3.1 Molar Heat of Fusion, Molar Heat of Vaporization, Molar Heat of Sublimation
5.3.2 Energy Changes and Intermolecular Attractions
5.3.3 Change of State and Dynamic Equilibrium
5.4 Liquid Crystals
5.4.1 Brief Description
5.4.2 Uses from Daily Life
6. STATES OF MATTER III: SOLIDS
Introduction
6.1 Kinetic Molecular Interpretation of Solids
6.1.1 Simple Properties of Solids Describing Vibration of Molecules, Intermolecular Forces, Kinetic Energy
6.2 Types of Solids
6.2.1 Amorphous
6.2.2 Crystalline
6.3 Properties of Crystalline Solids
6.3.1 Symmetry
6.3.2 Geometrical Shape
6.3.3 Melting Point
6.3.4 Cleavage Plane
6.3.5 Habit of Crystal
6.3.6 Crystal Growth
6.3.7 Anisotropy
6.3.8 Isomorphism
6.3.9 Polymorphism
6.3.10 Allotropy
6.3.11 Transition Temperature
6.4 Crystal Lattice
6.4.1 Unit Cell
6.4.2 NaCl Crystal
6.4.3 Lattice Energy
6.5 Types of Crystalline Solids
6.5.1 Ionic Solids
6.5.2 Covalent Solids
6.5.3 Metallic Solids
6.5.4 Molecular Solids
7. CHEMICAL EQUILIBRIUM
Introduction
7.1 Reversible Reactions and Dynamic Equilibrium
7.1.1 Concept and Explanation
7.1.2 Law of Mass Action and Expression for Equilibrium Constant
7.1.3 Relationship between Kc, Kp, Kx, Kn
7.1.4 Importance of K and Reaction Quotient
7.2 Factors Affecting Equilibrium ( Le-Chatelier’s Principle )
7.2.1 Effect of Change in Concentration
7.2.2 Effect of Change in Pressure or Volume
7.2.3 Effect of Change in Temperature
7.3 Industrial Application of Le-Chatelier’s Principle (Haber’s Process)
7.4 Solubility Product and Precipitation Reactions
7.5 Common Ion Effect
8. ACIDS, BASES AND SALTS
Introduction
8.1 Acidic, Basic and Amphoteric Substances
8.2 Bronsted-Lowery Definitions of Acids and Bases
8.2.1 Proton Donors and Acceptors
8.2.2 Relative Strength of Acids and Bases
8.3 Conjugate Acid-Base Pairs
8.4 Expressing the Strength of Acids and Bases
8.4.1 Ionization Equation of Water
8.4.2 pH, pOH and pKw
8.4.3 Acid Ionization Constant, Ka and pKa
8.4.4 Leveling Effect
8.4.5 Base Ionization Constant, Kb and pKb
8.4.6 Relationship of Ka and Kb
8.5 Lewis Definitions of Acids and Bases
8.6 Buffer Solutions and their Applications
8.7 Salt Hydrolysis
9. CHEMICAL KINETICS
Introduction
9.1 Chemical Kinetics
9.2 Rates of Reactions
9.2.1 Rate law or Rate Expression
9.2.2 Elementary and overall Rate Constant and Units
9.2.3 Order of Reaction and its Determination
9.2.4 Factors Affecting Rate of Reaction
9.3 Collision Theory, Transition State and Activation Energy
9.4 Catalysis
9.4.1 Characteristics of Catalysts
9.4.2 Homogeneous Catalysis
9.4.3 Heterogeneous Catalysis
9.4.4 Enzyme Catalysis
10. SOLUTIONS AND COLLOIDS
Introduction
10.1 General Properties of Solutions
10.1.1 Solution, Suspension and Colloids
10.1.2 Hydrophilic and Hydrophobic Molecules
10.1.3 The Nature of Solutions in Liquid Phase
10.1.4 The Effect of Temperature and Pressure on Solubility
10.2 Concentration Units
10.2.1 Percent
10.2.2 Molarity
10.2.3 Molality
10.2.4 Mole fraction
10.2.5 Parts per million, billion, and trillion
10.3 Raoult’s Law
10.3.1 Non-Volatile Non- -Electrolyte Solutes in Volatile solvents
10.3.2 When both Components are Volatile
10.4 Colligative Properties of dilute Solutions
10.4.1 Vapour Pressure Lowering
10.4.2 Boiling Point Elevation and Freezing Point Depression
10.4.3 Molar Mass Determination by Vapor Pressure Lowering, Boiling Point Elevation and Freezing Point Depression
10.4.4 Osmotic Pressure and Reverse Osmosis
10.5 Colloids
10.5.1 Properties of Colloids
10.5.2 Types of Colloids
11. THERMOCHEMISTRY
Introduction
11.1 Energy in Chemical Reactions
11.2 Thermodynamics
11.3 Internal Energy
11.4 First Law of Thermodynamics
11.5 Standard State and Standard Enthalpy Changes
11.6 Heat Capacity
11.7 Calorimeter
11.8 Hess’s Law: Enthalpy Change Calculations
11.9 Born Haber Cycle
12. ELECTROCHEMISTRY
Introduction
12.1 Oxidation-Reduction Concepts
12.1.1 Oxidation and Reduction
12.1.2 Oxidation Numbers
12.1.3 Recognizing Oxidation Reduction Reactions
12.1.4 Balancing Oxidation Reduction Equations by Oxidation Number Method
12.1.5 Balancing Oxidation Reduction Equations by the Half Reaction Method
12.1.6 Chemistry of Some Important Oxidizing and Reducing Agents
12.2 Electrode, Electrode Potential and Electrochemical Series
12.3 Types of Electrochemical Cells
12.3.1 Electrolytic Cells
12.3.2 Electrolysis of Aqueous NaCl
12.3.3 Voltaic Cells
12.3.3.1 Standard State Cell Potential for Voltaic Cell
12.3.3.2 Standard State Reduction Half Cell Potential
12.3.3.3 Standard State Cell Potentials and Spontaneous Reaction
12.3.4 Batteries
12.3.4.1 Primary Batteries
12.3.4.2 Secondary Batteries
12.3.4.3 Fuel Cells
12.3.5 Corrosion and its Prevention
Prescribed textbook
A textbook of Chemistry for Class-XI
Published by National Book Foundation, Islamabad
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