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Essential ideas:
 Physical and chemical properties depend on the ways in which different atoms combine.
 The mole makes it possible to correlate the number of particles with the mass that can be measured.
 Mole ratios in chemical equations can be used to calculate reacting ratios by mass and gas volume.
1.1 States of matter, changes of state and state symbols

This video covers states of matter, changes of state and state symbols.
Applications and skills: Application of the state symbols (s), (l), (g) and (aq) in equations. 
1.1 Elements, compounds, mixtures

Understandings:
Atoms of different elements combine in fixed ratios to form compounds, which have different properties from their component elements. Mixtures contain more than one element and/or compound that are not chemically bonded together and so retain their individual properties. Mixtures are either homogeneous or heterogeneous. Applications and skills: Explanation of observable changes in physical properties and temperature during changes of state. 
1.1 Physical and chemical changes

This video covers the differences between physical and chemical changes.

1.1 Balancing chemical equations

Applications and skills:
Deduction of chemical equations when reactants and products are specified. Application of the state symbols (s), (l), (g) and (aq) in equations. Guidance: Balancing of equations should include a variety of types of reactions. 
1.2 Relative atomic mass and molecular mass

Understandings:
Masses of atoms are compared on a scale relative to 12C and are expressed as relative atomic mass (Ar) and relative formula/molecular mass (Mr). 
1.1 Atom economy

Utilization:
Atom economy  the atom economy of chemical reaction is a measure of the amount of starting materials that become useful products. 
1.2 The mole concept

Understandings:
The mole is a fixed number of particles and refers to the amount, n, of substance. Applications and skills: Calculation of the molar masses of atoms, ions, molecules and formula units. 
1.2 Molar ratio

This video explains how to use the coefficients in a balanced equation to calculate amounts of products.

1.2 Molar mass

Understandings:
Molar mass (M) has the units g mol1. Applications and skills: Calculation of the molar masses of atoms, ions, molecules and formula units. 
1.2 Mole calculations

Applications and skills:
Solution of problems involving the relationships between the number of particles, the amount of substance in moles and the mass in grams. 
1.2 Empirical and molecular fomula

Understandings:
The empirical formula and molecular formula of a compound give the simplest ratio and the actual number of atoms present in a molecule respectively. Applications and skills: Determination of the molecular formula of a compound from its empirical formula and molar mass. 
1.2 Calculating percentage composition by mass

This video covers how to calculate the percentage composition by mass of an element in a compound.

1.2 Calculating empirical formula from % composition by mass

Applications and skills:
Interconversion of the percentage composition by mass and the empirical formula. 
1.2 Calculating empirical formula from combustion analysis

This video covers how to calculate the empirical formula organic compound from combustion data.

1.2 Water of crystallisation

This video covers how to calculate the water of crystallisation from experimental data.

1.2 Calculate empirical formula from experimental data

Applications and skills:
Obtaining and using experimental data for deriving empirical formulas from reactions involving mass changes. 
1.3 Limiting and excess reactants

Understandings:
Reactants can be either limiting or excess. Applications and skills: Solve problems relating to reacting quantities and limiting and excess reactants. 
1.3 Percent yield

Understandings:
Reactants can be either limiting or excess. The experimental yield can be different from the theoretical yield. Applications and skills: Solve problems relating to reacting quantities, limiting and excess reactants, theoretical, experimental and percentage yields. 
1.3 Percentage purity

This video covers how to calculate percentage purity.

1.3 Molar volume of a gas

Understandings:
The molar volume of an ideal gas is a constant at specified temperature and pressure. 
1.3 Avogadro's law

Understandings:
Avogadro’s law enables the mole ratio of reacting gases to be determined from volumes of the gases. Applications and skills: Calculation of reacting volumes of gases using Avogadro’s law. 
1.3 Solve problems involving temperature and volume for an ideal gas.

Applications and skills:
Solution of problems and analysis of graphs involving the relationship between temperature, pressure and volume for a fixed mass of an ideal gas. 
1.3 Ideal gas equation

Applications and skills:
Solution of problems relating to the ideal gas equation. 
1.3 Calculating molar mass of a gas using PV=nRT

Applications and skills:
Solve problems relating to the ideal gas equation. Obtaining and using experimental values to calculate the molar mass of a gas from the ideal gas equation. 
1.3 Determine molar mass of a gas experimentally

Applications and skills:
Obtaining and using experimental values to calculate the molar mass of a gas from the ideal gas equation. 
1.3 Ideal gases

Applications and skills:
Explanation of the deviation of real gases from ideal behaviour at low temperature and high pressure. 
1.3 Concentration of solutions

Understandings:
The molar concentration of a solution is determined by the amount of solute and the volume of solution. Applications and skills: Solve problems involving molar concentration, amount of solute and volume of solution. Units of concentration to include: g dm3, mol dm3 and parts per million (ppm). 
1.3 Thermometric titration

This video covers how to calculate the concentration of a solution using a thermometric titration.

1.3 Back titration

This video covers how to determine the percentage calcium carbonate in an egg shell using a back titration.

Review of past exam questions (old syllabus) but still relevant for new syllabus.

A review of some past quantitative chemistry exam questions for the old syllabus.
