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Summary Grade 12 IEB Physical Science (Chemistry) Paper 2: All SAG Definitions & Polyatomic ions R70,00
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Summary Grade 12 IEB Physical Science (Chemistry) Paper 2: All SAG Definitions & Polyatomic ions

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This aesthetic, neatly typed document contains all the IEB Grade 12 Chemistry SAG Definitions from each section: Quantitative Chemistry, Chemical bonding, Energy Change & Rates of Reactions, Chemical Equilibrium, Acids & Bases, Electrochemistry, and Organic Chemistry

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  • January 21, 2023
  • 5
  • 2022/2023
  • Summary

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Grade 12 IEB Physical Science: Chemistry (Paper 2) SAG De nitions:


Section A: Quantitative Chemistry:

• Molar mass: The mass in grams of one mole of that substance



• Solution: A homologous mixture of solute and solvent

• Solute: The substance that is dissolved in the solution

• Solvent: The substance in which another substance is dissolved, forming a solution

• Concentration: The amount of solute per unit volume of solution



• Yield: A measure of the extent of a reaction, generally measured by comparing the amount of

product against the amount of product that is possible



Section B: Chemical Bonding:

• Covalent bond: A sharing of at least one pair of electrons by two non-metal atoms

• Non-polar covalent bond (Pure covalent): An equal sharing of electrons

• Polar covalent bond: An unequal sharing of electrons leading to a dipole forming (as a result of

electronegativity di erence)

• Electronegativity: A measure of the tendency of an atom to attract a bonding pair of electrons

• Ionic bond: A transfer of electrons and subsequent electrostatic attraction

• Metallic bonding: Between a positive kernel and a sea of delocalised electrons



• Intermolecular forces: A weak force of attraction between molecules, ions or atoms of noble

gases



Section C: Energy Change & Rates of Reactions:

• Heat of reaction: The net change of chemical potential energy of the system

• Exothermic reactions: Reactions which transform chemical potential energy into thermal energy




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, • Endothermic reactions: Reactions which transform thermal energy into chemical potential energy



• Activation energy: The minimum energy required to start a chemical reaction OR The energy

required to form the activated complex

• Activated complex: A high energy, unstable, temporary transition state between the reactants and

the products



• Reaction rate: The change in concentration per unit time of either a reactant or product

• Catalyst: A substance that increases the rate of reaction but remains unchanged at the end of the

reaction



Section D: Chemical Equilibrium:

• Closed system: one in which mass is conserved inside the system but energy can enter or leave

the system freely

• Open system: one in which both energy and matter can be exchanged between the system and

its surroundings

• Reversible reaction: Reaction in which products can be converted back into reactants



• Le Châtelier's principle: When an external stress (change in pressure, temperature or

concentration) is applied to a system in dynamic chemical equilibrium, the equilibrium point will

change in such a way as to counteract the stress



Section E: Acids & Bases:

• Acid: A proton donor

• Base: A proton acceptor

• ionisation: The reaction of a molecular substance with water to produce ions

• Strong acid: An acid that ionises completely in an aqueous solution

• Weak acid: Acid that only ionises partially in an aqueous solution

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