Kinetic Particle Theory

• States of Matter
  1.1.1. Describe the solid liquid and gaseous states of matter.
• Kinetic Particle Theory
  1.2.1. State the kinetic particle theory
  1.2.2. Describe the states of matter using the kinetic particle theory
• Changes in States of Matter and the Kinetic Particles Theory
  1.3.1. Explain the inter conversion od states of matter in terms of the kinetic particle theory and energy changes.

Measurement and Experimental Techniques

• Measuring Physical Quantities
  2.1.1. Name the appropriate apparatus for measuring mass, time, temperature and volumes of liquid and gases.
• Selecting Suitable Apparatus for Experiments
  2.2.1. Select suitable apparatus for collecting a sample of gas

Separation and Purification

• Obtaining Pure Substances from Mixtures
  3.1.1. Understand the difference between pure substances and mixtures
• Separating a Solid from a Liquid
  3.2.1. Describe methods of separating and purifying mixtures of a solid and a liquid.
• Separating Solids
  3.3.1. Describe a method of separating and purifying mixtures of solids
• Separating a Liquid from a Solution
  3.4.1. Describe a method to separate and purify a solvent from a solution
• Separating Liquids
  3.5.1. Describe a method of separating and purifying mixtures of miscible liquids
• Chromatography
  3.6.1. Describe chromatography and interpret chromatogram
• Determining Purity
  3.7.1. Identify substances and their purity , given their melting and boiling points.

Elements, Compounds and Mixtures

• Elements
  4.1.1. Define an element
  4.1.2. State the chemical symbol for a number of elements
• Compounds

4.2.1. Define a compound
4.2.2. Describe the differences between elements and compounds
4.2.3. Deduce the formula of a compound from the ratio of elements present

• Mixtures
  4.3.1. Define a mixture
  4.3.2. Differentiate between compounds and mixtures

Atomic Structure

• Inside Atoms
  5.1.1. State the relative charges and relative masses of a proton, a neutron and an electron
  5.1.2. Describe the structure of an atom.
• The Proton Number and Nucleon Number
  5.2.1. Define proton (atomic ) number and nucleon (mass) number
  5.2.2. Deduce the numbers of proton, neutrons and electrons in an atom;
  5.2.3. Interpret and use symbols that represent an element’s nucleon and proton number
• Isotopes
  5.3.1. Define isotopes
• Arrangement of Electrons in Atoms
  5.4.1. Use the diagrams to describe atoms as containing Protons and neutrons in the nucleus Electrons arranged in the electron shells (energy levels).

Chemical Bonding

• The Stable Electronic Configuration of a Noble Gas
  6.1.1. Describe the stable electronic configuration of a noble gas.
• Forming Ions
  6.2.1. Describe the formation of positive ions (cations) and negative ions (anions) to achieve the electronic configuration of a noble gas
• Ionic Bond: Transferring Electrons
  6.3.1. Describe how ionic bonds are formed between metals and non-metals
  6.3.2. Deduce the formula of an ionic compound from the charges on the ions and vice versa.
• Structure and Physical Properties of Ionic Compounds
  6.4.1. State that ionic compounds form giant lattice structures
  6.4.2. Relate the physical properties of ionic compounds to their lattice structures.
• Covalent Bond: Sharing Electrons
  6.5.1. Describe the formation of a covalent bond by the sharing of electrons
  6.5.2. Describe the formation of covalent bonds between non-metallic elements using ‘dot and
  cross’ diagram
  6.5.3. Deduce the arrangement of electrons in covalent molecules.
• Structure and Properties of Covalent Substances
  6.6.1. Relate the physical properties of covalent substances to their structure and bonding

Writing Chemical Equations

• Chemical Equations
  7.1.1. Interpret chemical equations with state symbols
  7.1.2. Write balanced chemical equations with state symbols
• Ionic Equations
  7.2.1. Write ionic equation with state symbols

The Mole

• Relative Atomic Mass
  8.1.1. Define relative atomic mass Ar
• Relative Molecular Mass and Relative Formula Mass
  8.2.1. Define relative molecular mass Mr
  8.2.2. Calculate relative molecular mass or relative formula mass of a substance.
• The Mole and Molar Mass
  8.3.1. Convert number of particles into number of moles and vice versa
  8.3.2. Perform calculations involving the number of moles, mass and molar mass of a substance.
• Molar Volume of Gases
  8.4.1. Perform calculations involving molar gas volume and the number of moles of a gas
• The Concentration of Solution
  8.5.1. Perform calculations involving the concentration of a solution (g/dm3 or mol/dm3)

Oxidation and Reduction

• Oxidation and Reduction as Gain or Loss of Oxygen
  12.1.1. Define oxidation as the gain of oxygen
  12.1.2. Define reduction as the loss of oxygen
  12.1.3. Define redox reactions
• Oxidation and Reduction as Gain or Loss of Hydrogen
  12.2.1. Define oxidation as the loss of hydrogen
  12.2.2. Define reduction as the gain of hydrogen
• Oxidation and reduction as Gain or Loss of Electrons
  12.3.1. Define oxidation as the loss of electrons
  12.3.2. Define reduction as the gain of electrons
• Oxidation and Reduction in Terms of Changes in Oxidation States
  12.4.1. Define oxidation as an increase in oxidation state
  12.4.2. Define reduction as a decrease in oxidation state
• Oxidising and Reducing Agents
  12.5.1. Test for oxidisng agents and reducing agents using aqueous potassium iodide and acidified potassium manganate (VII).

Acids and Bases

• Acids
  10.1.1. Define acids as substances that produce hydrogen ions in aqueous solution
  10.1.2. Describe the properties of acids and their reaction with metals, bases and carbonates
• Bases and Alkalis
  10.2.1. Define alkalis as substances that produce hydroxide ions in aqueous solution
  10.2.2. Describe what is meant by neutralization and write the ionic equation for the neutralization reaction

10.2.3. Describe the properties of alkalis and their reactions with acids and ammonium salts

• The pH Scale
  10.3.1. Describe the effects of acids and alkalis on Universal Indicator
  10.3.2. Describe the use of Universal Indictor nd the pH scale to test hydrogen ion concentration and relative acidity
  10.3.3. Describe the reasons for controlling the pH of soil and the methods used to reduce excess acidity in soil.
• Types of Oxides
  10.4.1. Classify oxides as acidic , basic, amphoteric or neutral based on their metallic or non-metallic properties.

Salts

• Salts
  11.1.1. Define a salt
• Preparation of Salts
  11.2.1. Suggest a suitable method and the starting materials for preparing a salt
  11.2.2. Describe the methods of separation and purification used in preparing salts
• Qualitative Analysis
  11.3.1. Describe the tests to identify aqueous cations
  11.3.2. Describe the tests to identify anions
  11.3.3. Describe the tests to identify gases

Chemical Calculations

• Calculation from Chemical Reactions
  9.1.1. Calculate the masses of reactants and products by using the mole ratio in a chemical equation.
• The Volumes of Reacting Gases
  9.2.1. Calculate the volumes of gaseous reactants and products using the mole ratio in a chemical equation.
• Limiting Reactants
  9.3.1. Perform stoichiometric calculations involving the idea of limiting reactant
• Volumetric Analysis
  9.4.1. Process the results of volumetric experiments
  9.4.2. Perform stoichiometric calculations involving concentrations of solutions