iGCSE Chemistry (Triple) OxfordAQA

This subject is broken down into 42 topics in 10 modules:

  1. Atomic Structure and the Periodic Table 3 topics
  2. Structure, Bonding and the Properties of Matter 6 topics
  3. Chemical Changes 4 topics
  4. Chemical Analysis 4 topics
  5. Acids, Bases and Salts 2 topics
  6. Quantitative Chemistry 4 topics
  7. Trends within the Periodic Table 3 topics
  8. Rates of Reactions and Chemical Change 4 topics
  9. Energy Changes 4 topics
  10. Organic Chemistry 8 topics
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This page was last modified on 28 September 2024.

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Chemistry (Triple)

Atomic Structure and the Periodic Table

Solids, Liquids and Gases

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Solids, Liquids and Gases

Matter and Its States

  • Matter is anything that occupies space and has mass, comprised of tiny particles called atoms.
  • Atoms can exist freely, or they can combine to form molecules.
  • Matter can mainly be in three states: solid, liquid, or gas.
  • The state of matter depends on how the atoms or molecules are arranged and the energy they possess.

Solids

  • In solids, the particles are tightly packed together in a fixed, regular arrangement.
  • The particles in a solid vibrate in place but don't move from their fixed positions — this makes solids maintain a fixed shape and volume.
  • Solids have the strongest intermolecular forces.
  • Solids do not flow and are not generally compressible.

Liquids

  • In liquids, particles are in a random arrangement but are still close together.
  • The particles in a liquid can move around each other but are still in close contact; this allows a liquid to flow and take the shape of its container.
  • Liquids have medium strength intermolecular forces.
  • Although liquids can be slightly compressed, they are mostly incompressible.

Gases

  • In gases, the particles are well separated and in a completely random arrangement.
  • The particles in a gas move quickly in all directions and have complete freedom of movement; this allows a gas to fill any given space.
  • Gases have the weakest intermolecular forces.
  • Gases are highly compressible and always expand to fill their containers.

Changing States

  • Melting, freezing, evaporation, and condensation are the processes of state changes.
  • When a solid is heated, it will melt into a liquid at its melting point.
  • When a liquid is cooled, it will freeze into a solid at its freezing point.
  • When a liquid is heated, it will evaporate into a gas at its boiling point.
  • When a gas is cooled, it will condense into a liquid at its condensation point.

The Kinetic Theory of Matter

  • The Kinetic Theory of matter states that all particles of matter are in constant motion and this motion has consequences that can be studied on a macroscopic level (what we can see) and microscopic (what we cannot see but can imagine or model).
  • Increasing the temperature of a substance increases the kinetic energy of its particles, making them move more rapidly and irregularly.
  • The kinetic energy of particles and the attractive forces between particles are what determine the state of the substance - solid, liquid, or gas.

Course material for Chemistry (Triple), module Atomic Structure and the Periodic Table, topic Solids, Liquids and Gases

Chemistry (Triple)

Quantitative Chemistry

Quantitative Chemistry: The Mole Concept

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Quantitative Chemistry: The Mole Concept

Understanding the Mole Concept in Quantitative Chemistry

  • Familiarise yourself with the mole concept. It is a fundamental concept in chemistry which is used to quantify the amount of chemical substance.
  • Know that one mole of any substance contains 6.02 x 10^23 entities. These entities could be atoms, molecules, ions etc.
  • Understand that this number - 6.02 x 10^23 - is known as Avogadro's number, named after the Italian scientist Amedeo Avogadro.
  • Recognise that a mole is a bridge between the atomic world and the macroscopic world. It helps us count very small particles by weighing them.

Chemical Calculations Involving Moles

  • Be aware that the molar mass is the mass of one mole of a substance. Its unit is 'g/mol'.
  • Get a solid understanding of how to calculate the number of moles using the formula: Number of moles = mass (g) / molar mass (g/mol).
  • Be able to use the avogadro constant, by counting moles via the function: Moles = Number of particles / 6.02 x 10^23
  • Get comfortable calculating the mass of a substance using the formula: Mass (g) = number of moles x molar mass (g/mol).

The Mole Concept in Balancing Chemical Reactions

  • Understand that balanced chemical equations involve the mole concept. The coefficients in front of each formula represent the number of moles of that substance.
  • Be able to apply the mole concept in stoichiometric calculations. For instance, use the mole ratios (from a balanced chemical equation) to predict the amount of products formed or reactants used in a reaction.

Applications of Mole Concept in Quantitative Chemistry

  • Understand that molar calculations have important implications in scientific and industrial settings. For instance, determining the amount of reactant needed or product formed in a reaction.
  • Realise that molar calculations ensure efficiency and cost-effectiveness in chemical processes, as they prevent wastage or surplus of reactants.

Special Aspects and Other Considerations

  • Familiarise yourself with how the mole concept applies to gases using Avogadro's law - at the same temperature and pressure, equal volumes of gases contain an equal number of moles.
  • Understand that in reactions that involve gases, one must consider partial pressure when making molar calculations.
  • Remember the principle of conservation of mass - the total mass of the reactants equals the total mass of the product(s). This applies regardless of whether the substances are solid, liquid or gas.

Course material for Chemistry (Triple), module Quantitative Chemistry, topic Quantitative Chemistry: The Mole Concept

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