Topic 1.1 Introduction to the particulate nature of matter

• Describe the three states of matter
• Understand the changes involved when there is a change in state
• Understand that compounds have different properties to the elements they are made from
• Understand how to balance chemical equations
• Understand how to use state symbols in chemical equations
• Describe the differences between elements, compounds and mixtures
• Understand the differences between homogenous and heterogenous mixtures

Topic 1.2 The mole concept

• 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).
• Molar mass (M) has the units g mol-1. 
• The empirical formula and molecular formula of a compound give the simplest ratio and the actual number of atoms present in a molecule respectively. 
• The mole is a fixed number of particles and refers to the amount, n, of substance. 

Topic 1.3 Reacting Masses and Volumes

• Reactants can be either limiting or excess.
• The experimental yield can be different from the theoretical yield.
• Avogadro’s law enables the mole ratio of reacting gases to be determined from volumes of the gases.
• The molar volume of an ideal gas is a constant at specified temperature and pressure.
• The molar concentration of a solution is determined by the amount of solute and the volume of solution.
• A standard solution is one of known concentration. 

Study guides for unit exam

Application and Skills checklist (IB specific): Stoichiometric Relationships Study Guide
Stoichiometric Relationship Practice Problems: Stoichiometric Relationships Practice Problems
Stoichiometry Review Problems
Stoichiometry Practice Test