O-Level-Chemistry-Notes-2

Chemistry Q Level Notes Study Guide

Page 1: Student Information

  • Name:

  • Syllabus Code: 5070

  • Aim for O Level:

  • Class:

  • Author: abi 5dec94

  • Publisher: O ASN Publishing Co. Ltd.

Note: No content of this booklet should be published without author's consent.

Page 2: Table of Contents

CHAPTER 1: Experimental Chemistry

  • 1.1 Experimental Design

  • 1.2 Methods of Purification and Analysis

  • 1.3 Identification of Ions

  • 4.1 Introductory Electrolysis

  • 4.2 Electrolysis of Molten and Gases

  • 4.3 Electrolysis of Aqueous Solutions

  • 4.4 Electrolysis Using Different Types of Electrodes

  • 4.5 Electroplating

  • 4.6 Electric Cells

CHAPTER 2: The Particulate Nature of Matter

  • 2.1 Kinetic Particle Theory

  • 2.2 Atomic Structure

  • 2.3 Structures and Properties of Materials

CHAPTER 3: Formulae, Stoichiometry and The Mole Concept

  • 3.1 Relative Atomic Mass

  • 3.2 Relative Molecular Mass and Relative Formula Mass

  • 3.3 Percentage Composition

  • 3.4 Counting Particles

  • 3.5 Moles of Particles

  • 3.6 Molar Mass

  • 3.7 Different Kinds of Chemical Formulae

  • 3.8 Molar Volume of Gases

  • 3.9 Concentration of Solutions

  • 3.10 Constructing Chemical Equations

  • 3.11 Calculations from Equations

  • 3.12 Introductory Chemical Analysis

  • 3.13 Use of Physical Tests to Identify Substances

CHAPTER 4: Chemical Reactions

  • 4.1 Speed of Reaction

  • 4.2 Redox Reactions

  • 4.3 Reversible Reactions

CHAPTER 5: Energy from Chemicals

  • 5.1 Exothermic Reaction

  • 5.2 Endothermic Reaction

  • 5.3 Heat of Reaction

  • 5.4 Heat Change and Enthalpy

  • 5.5 Activation Energy

  • 5.6 Fuels

CHAPTER 6: The Chemistry and Uses of Acids, Bases and Salts
CHAPTER 7: The Periodic Table
CHAPTER 8: Organic Chemistry

  • 11.1 Alkanes

  • 11.2 Alkenes

  • 11.3 Alcohols

  • 11.4 Carboxylic Acids

  • 11.5 Synthetic Macromolecules

  • 11.6 Natural Macromolecules

Page 3: Continuation of Table of Contents

CHAPTER 9: Metals

  • 9.1 Properties of Metals

  • 9.2 Reactivity Series

  • 9.3 Extraction of Metals

  • 9.4 Iron

CHAPTER 10: Atmosphere and Environment

  • 10.1 Air

  • 10.2 Water

INSERTS

  • INSERT 1: Identification of Ions and Gases

  • INSERT 2: The Periodic Table

Chapter 1: Experimental Chemistry

1.1 Experimental Design
Volume of Liquids

  • SI Unit: cubic meter (m³)

  • Measurement Units:

    • Large volume: decimeter (dm³)

    • 1 dm³ = 1,000 cm³

    • Everyday measurements: milliliters (mL) or liters (L), where 1 L = 1,000 mL

Apparatus for Measuring Liquids

  1. Beaker: Holds approximate volumes of 100 cm³ and 250 cm³.

  2. Conical Flask: Holds approximate volumes of 100 cm³ and 250 cm³.

  3. Measuring Cylinder: Accuracy to 1 cm³; readings taken nearer to the meniscus.

  4. Burette: Long scale of 0 – 50 cm³, accurate to 0.1 cm³.

  5. Bulb Pipette: Measures exact volumes such as 20.0, 25.0, or 50.0 cm³.

Volume of Gases

  • MEASURED WITH: Gas syringe, up to 100 cm³.

Temperature Measurement

  • Measured With: Thermometer (types include mercury-in-glass, alcohol-in-glass).

  • SI Unit: Kelvin (K), daily life measurement: degree Celsius (°C).

  • Relation: K=°C+273K = °C + 273

Time Measurement

  • SI Unit: seconds (s); other units include minutes (min), hours (h).

  • Measured With: Clock or digital stopwatch.

Mass

  • Mass: Measure of the amount of matter in a substance.

  • SI Unit: kilogram (kg); other units: grams (g), milligrams (mg), tonnes (t).

  • Measured With: Electric “top-pan” balance or triple beam balance.

1.2 Methods of Purification and Analysis
Pure Substance

  • Defined as a single substance not mixed with anything else (examples include white sugar, copper sulfate crystals, distilled water).

Mixture

  • Contains two or more substances; more common in nature (e.g., seawater, milk).

Purification

  • The separation of mixtures into pure substances using physical methods (no chemical reactions).

Techniques include:

  1. Filtration: Separates insoluble solids from liquids through filter paper, trapping large particles as residue.

  2. Crystallization: Separation of dissolved solids as pure crystals as the solution cools.

  3. Evaporation to Dryness: Evaporates all liquid in a solution leaving the solid (like salt crystals).

  4. Sublimation: Separates a mixture where one component sublimes (e.g., iodine with sand).

  5. Simple Distillation: Separates pure liquid from solution; cooled steam forms pure liquid (distillate).

  6. Fractional Distillation: Separate mixtures of miscible liquids with differing boiling points using a fractionating column.

  7. Reverse Osmosis: Separates seawater by applying pressure against a membrane.

  8. Separating Funnel: Used to separate immiscible liquids.

  9. Chromatography: Separates colored substances (e.g., in dyes) and can identify mixtures.

1.3 Identification of Ions and Gases

  • Refer to Insert 1 for details.

Chapter 2: The Particulate Nature of Matter

2.1 Kinetic Particle Theory

  • Matter: Anything that has mass and takes up space. Exists in three forms: solids, liquids, gases.

    • Solids: Fixed volume and shape; incompressible.

    • Liquids: Fixed volume but not fixed shape; incompressible; flow easily.

    • Gases: No fixed volume or shape; compressible; flow in all directions.

The Kinetic Particle Theory

  • Particles are too small to be seen directly; there are spaces between them, varying with state.

  • Particles are in constant motion, with speed differing among phases.

Diffusion

  • Definition: Spreading and mixing of particles in gases or liquids.

  1. Diffusion of Gases: E.g., bromine gas filling jars.

  2. Diffusion of Liquids: E.g., CuSO4 crystals dissolving in water.

Factors Affecting Rate of Diffusion

  1. Temperature: Higher temperature increases the kinetic energy and speed of the particles, increasing the rate of diffusion. Lower temperature decreases the rate.

  2. Mass of Particles: Heavier particles diffuse slower compared to lighter ones.

Particulate Models of Matter

  • Properties of Matter in Different States:

    • Solid Particles: Packed closely in an orderly arrangement, vibrating in fixed positions.

    • Liquid Particles: Close-packed but not orderly, moving freely throughout the liquid.

    • Gas Particles: Far apart and randomly arranged, moving freely throughout a container.

Changes of State

  • Melting: Transition from solid to liquid.

  • Freezing: Transition from liquid to solid.

  • Boiling: Transition from liquid to gas.

  • Evaporation: Transition from liquid to gas at temperatures below boiling.

  • Condensation: Transition from gas to liquid.

  • Sublimation: Transition from solid to gas without liquid formation.

2.2 Atomic Structure

  1. Components of Atoms: Protons, neutrons (found in the nucleus), and electrons (move around nucleus).

    • Protons: Positive charge, mass = 1.

    • Neutrons: No charge, mass = 1.

    • Electrons: Negative charge, negligible mass.

  2. Proton Number: Number of protons in an atom.

  3. Nucleon Number: Total number of protons and neutrons in nucleus.

    • Formula: $$ ext