Chem – Full Book Quiz — Chemistry (SSC-I (9th), Afaq Sun) | 22 MCQs

Sample Questions

See what you’ll practice in this quiz.

Which branch of chemistry deals with the study of compounds of carbon?
Which state of matter has a definite shape and a definite volume?
The process in which a solid changes directly into a gas without passing through the liquid state is called:

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What You’ll Practice

Chapter 1: States of Matter and Phase Changes What is Chemistry?: Branches of Chemistry: Physical; Inorganic; Organic; Environmental; Analytical; Biochemistry; Nuclear; Polymer; Geochemistry (and others) | States of Matter: Solids; Liquids; Gases; Plasma and exotic states; Changes of state; Density, compressibility and fluidity | Element, Compound and Mixture: Definition of element; Definition of compound; Definition of mixture; Homogeneous and heterogeneous mixtures; Separation of mixtures | Allotropic Forms of Substances: Meaning of allotropy; Diamond; Graphite; Fullerenes; Allotropes of oxygen, phosphorus and sulphur | Differences between Elements, Compounds and Mixtures: Composition; Chemical combination; Fixed ratio; Separation by physical or chemical means; Properties and energy change | Solution, Colloidal Solutions and Suspension: Solutions; Colloids; Suspensions; Particle size; Tyndall effect; Examples | Formation of Unsaturated and Saturated Solutions: Unsaturated solution; Saturated solution; Supersaturated solution; Solubility | Effect of Temperature on the Solubility of Solutes: Solubility of solids and gases with temperature; Solubility curves; Interpreting saturated, unsaturated and supersaturated regions
Chapter 10: Environmental Chemistry Composition of Atmosphere: Nitrogen; Oxygen; Argon; Carbon dioxide; Water vapour and trace gases; Layers of atmosphere | Air Pollutants: Carbon monoxide; Carbon dioxide; Sulphur dioxide; Nitrogen oxides; Particulates; CFCs; Sources and effects | Acid Rain: Sources (SO2 and NOx); Reactions forming acids; Effects; Prevention | Global Warming (Greenhouse Effect): Natural greenhouse effect; Greenhouse gases; Human causes; Effects of global warming | Strategies to Reduce Environmental Issues: Renewable energy; Afforestation; Cleaner fuels and catalytic converters; Waste management; International agreements
Chapter 11: Hydrocarbons Hydrocarbons: Alkanes; Alkenes; Alkynes; Aromatic hydrocarbons; Sources and uses | Alkanes: General formula CnH2n+2; Homologous series; IUPAC naming; Isomerism; Physical properties | Preparation of Alkanes: 1 | Important Reactions: Combustion of alkanes; Substitution (halogenation) reactions; Cracking
Chapter 12: Empirical Data Collection and Analysis SI Units in Chemistry: 1 | Tools and Techniques to Manage Accuracy and Precision: Choice of apparatus; Calibration; Repeating and averaging; Reducing parallax and errors; Significant figures | Accuracy and Precision: Definition of accuracy; Definition of precision; Systematic and random errors; Percentage error
Chapter 13: Laboratory and Practical Skills Chemical Hazards in the Laboratory: 13.1.1 Flammable and Explosive Chemical Hazards; 13.1.2 Corrosive Hazards; 13.1.3 Toxic Chemical Hazards; 13.1.4 Reactive Chemical Hazards; 13.1.5 Radiation Hazards; 13.1.6 Asphyxiation Hazards | Hazard Signs: Flammable; Oxidising; Explosive; Corrosive; Toxic; Irritant; Health hazard; Environmental hazard | Personal Protective Equipment (PPE): Lab coat; Safety goggles; Gloves; Closed shoes; Correct use and disposal | Location of Fire Extinguisher: Position of extinguishers; Types of extinguishers; Fire blanket and sand; PASS method | Emergency Situation in the Lab: Spills; Chemical splashes in eyes and skin; Burns; Fire; Inhalation of fumes; Reporting accidents
Chapter 2: Atomic Structure Structure of Atom: Discovery of Electrons; Discovery of Proton; Discovery of Neutron; Discovery of Nucleus | Atomic Number and Mass Number: Atomic number (Z); Mass number (A); Protons, neutrons and electrons count; Atomic notation | Isotopes and their Masses: Meaning of isotopes; Isotopes of hydrogen, carbon and chlorine; Properties; Applications; Mass spectrometer | Relative Atomic Mass: Atomic mass unit; Carbon-12 standard; Weighted average of isotopes; Calculation of relative atomic mass
Chapter 3: Chemical Bonding Why do Atoms Form Chemical Bonds?: Stability and energy; Noble gas configuration; Octet and duplet rules; Valence electrons | Chemical Bond: 3.2.1 Ionic Bond; 3.2.2 Covalent Bond; 3.2.3 Coordinate Covalent Bond | Metallic Bond: Sea of delocalised electrons; Metal ions; Properties of metals (conductivity, malleability, ductility); Strength of metallic bond | Electropositive Character of Metals: Tendency to lose electrons; Formation of cations; Trends in groups and periods; Reactivity of metals | Electronegative Character of Non-metals: Tendency to gain electrons; Formation of anions; Electronegativity trend; Bond polarity | Compare the Properties of Ionic and Covalent Compounds: Structure; Melting and boiling points; Solubility; Electrical conductivity; Hardness and brittleness; Exceptions | Intermolecular Forces of Attraction: London dispersion forces; Dipole-dipole forces; Hydrogen bonding; Effect on boiling point and solubility | Nature of Bonding and Properties: Ionic lattices; Simple molecular substances; Giant covalent structures; Metals; Link between bonding and properties
Chapter 4: Stoichiometry Chemical Formula: Molecular formula; Structural formula; Formula unit; Use in calculations | Empirical Formula: Definition; Steps to determine; Relation to molecular formula; Combustion analysis | Chemical Formulas of Binary Ionic Compounds: Writing symbols and charges; Criss-cross method; Naming with -ide; Examples such as Al2O3 and MgCl2 | Chemical Formulas of Compounds: Polyatomic ions (radicals); Use of brackets; Covalent compound naming with prefixes; Valency | Deduce the Molecular Formula from the Structural Formula: Reading a structural formula; Counting atoms; Examples such as ethane and ethanol; Isomers | Avogadro's Number (Nₐ): Value 6.022 x 10^23; Particles in one mole; Number of particles calculations | The Mole and Molar Mass: Definition of mole; Molar mass; Moles, mass and particles relationships; Molar volume of gases (22.4 dm3) | Chemical Equations and Chemical Reactions: Reactants and products; Balancing equations; Law of conservation of mass; State symbols; Types of reactions | Calculations Based on Chemical Equation: Mole ratios; Mass-mass calculations; Mass-volume calculations; Limiting reactant; Percentage yield
Chapter 5: Energetics System and Surroundings: System; Surroundings; Open, closed and isolated systems; Heat exchange | Enthalpy: Heat content; Enthalpy change (delta H); Standard enthalpy changes; Measurement by calorimeter | Exothermic and Endothermic Reactions: Exothermic reactions; Endothermic reactions; Sign of delta H; Energy level diagrams; Bond breaking and bond making | How does a Reaction Take Place?: Collision theory; Activation energy; Transition state; Effect of a catalyst; Factors affecting rate | Aerobic and Anaerobic Respiration: Aerobic respiration equation; Anaerobic respiration in yeast and muscles; Energy released; Glycolysis
Chapter 6: Equilibria Reversible and Irreversible Reactions: Irreversible reactions; Reversible reactions; Use of double arrow; Closed systems | Dynamic Equilibrium: Equal forward and backward rates; Constant concentrations; Equilibrium constant; Physical equilibrium | Changing the Physical Conditions of a Chemical Equilibrium: Le Chatelier's principle; Effect of concentration; Effect of temperature; Effect of pressure; Role of a catalyst
Chapter 7: Acid Base Chemistry Acids and Bases: Properties of acids; Properties of bases and alkalis; Strong and weak acids and bases; pH scale; Indicators | Different Concepts of Acids and Bases: Arrhenius concept; Bronsted-Lowry concept; Lewis concept; Limitations of each concept | Brønsted–Lowry Concepts of Acids and Bases: Proton donors and acceptors; Conjugate acid-base pairs; Amphoteric nature of water; Ammonia as a base | Properties of Acids and Bases: Taste and feel; Action on indicators; Reaction with metals and carbonates; Neutralisation; Safety | Acid Rain and its Effects: Formation from SO2 and NOx; pH below 5.6; Effects on buildings, water and forests; Control measures
Chapter 8: Periodic Table and Periodicity Modern Periodic Table: Mendeleev's table; Moseley and atomic number; Periods and groups; Blocks (s, p, d, f) | Salient Features of Modern Periodic Table: Seven periods; Eighteen groups; Metals, non-metals and metalloids; Alkali metals, halogens and noble gases | Similarities in the Chemical Properties of Elements: Same valence electrons in a group; Similar reactions of alkali metals; Similar reactions of halogens; Predicting properties | Variation of Periodic Properties in Periods and Groups: Atomic size; Ionisation energy; Electronegativity; Electron affinity; Metallic character trends | Metallic Character and Reactivity: Metallic character trend; Reactivity of metals; Reactivity of non-metals; Reactivity series
Chapter 9: Group Properties and Elements Properties of Group 1 Elements: Physical properties; Reaction with water; Reaction with oxygen and halogens; Flame tests; Trend in reactivity | Properties of Group 17 Elements: Diatomic molecules; Physical state and colour trend; Reactivity trend; Displacement reactions; Uses | Group Properties of Transition Elements: Physical properties; Variable oxidation states; Coloured compounds; Catalytic activity; Uses | Properties of Noble Gases: Stable electronic structure; Physical properties; Monatomic nature; Uses of helium, neon, argon and others | Physical Properties of Metals and Non-metals: Lustre, hardness and density; Conductivity; Malleability and ductility; Properties of non-metals; Metalloids

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SSC-I (9th) Chemistry Afaq Sun Series Chapter 1: States of Matter and Phase Changes

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Chem – Full Book

Chapter 1: Nature of Chemistry in Science

Chapter 2: Matter

Chapter 3: Atomic Structure

Chapter 4: Periodic Table and Periodicity of Properties

Chapter 5: Chemical Bonding

Chapter 6: Stoichiometery

Chapter 7: Electrochemistry

Chapter 8: Energetics

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