Hydrocarbons
Structure of carbon and its valency
Hydrocarbon
Examples of hydrocarbons and their structure
Isomerism and examples.
Homologous series as it relates to the physical and chemical properties of hydrocarbons
Distinguishing between aliphatic and aromatic hydrocarbon
Hydrocarbons
Structure of carbon and its valency
Hydrocarbon
Examples of hydrocarbons and their structure
Isomerism and examples.
Homologous series as it relates to the physical and chemical properties of hydrocarbons
Distinguishing between aliphatic and aromatic hydrocarbon
Hydrocarbons
Structure of carbon and its valency
Hydrocarbon
Examples of hydrocarbons and their structure
Isomerism and examples.
Homologous series as it relates to the physical and chemical properties of hydrocarbons
Distinguishing between aliphatic and aromatic hydrocarbon
Hydrocarbons
Structure of carbon and its valency
Hydrocarbon
Examples of hydrocarbons and their structure
Isomerism and examples.
Homologous series as it relates to the physical and chemical properties of hydrocarbons
Distinguishing between aliphatic and aromatic hydrocarbon
Electrolysis (i)
Explaining the quantitative aspects of electrolysis
-Defining electrolytes (strong, weak, fused/molten, non-electrolytes), electrolytic and electrochemical cells
-Differentiating between strong and weak electrolytes
-Illustrating the electrolysis of acidified water, copper II sulphates and brines;
-Identifying factors affecting the discharge of ions during Electrolysis
-Construction of electrolytic and electrochemical cells
-Faraday’s laws of Electrolysis
-Calculating the amount of substances liberated or deposited at electrodes during electrolysis
-The uses of electrolysis in the extraction and purification of metals
Electrolysis (i)
Explaining the quantitative aspects of electrolysis
-Defining electrolytes (strong, weak, fused/molten, non-electrolytes), electrolytic and electrochemical cells
-Differentiating between strong and weak electrolytes
-Illustrating the electrolysis of acidified water, copper II sulphates and brines;
-Identifying factors affecting the discharge of ions during Electrolysis
-Construction of electrolytic and electrochemical cells
-Faraday’s laws of Electrolysis
-Calculating the amount of substances liberated or deposited at electrodes during electrolysis
-The uses of electrolysis in the extraction and purification of metals
Electrolysis (i)
Explaining the quantitative aspects of electrolysis
-Defining electrolytes (strong, weak, fused/molten, non-electrolytes), electrolytic and electrochemical cells
-Differentiating between strong and weak electrolytes
-Illustrating the electrolysis of acidified water, copper II sulphates and brines;
-Identifying factors affecting the discharge of ions during Electrolysis
-Construction of electrolytic and electrochemical cells
-Faraday’s laws of Electrolysis
-Calculating the amount of substances liberated or deposited at electrodes during electrolysis
-The uses of electrolysis in the extraction and purification of metals
Electrolysis (i)
Explaining the quantitative aspects of electrolysis
-Defining electrolytes (strong, weak, fused/molten, non-electrolytes), electrolytic and electrochemical cells
-Differentiating between strong and weak electrolytes
-Illustrating the electrolysis of acidified water, copper II sulphates and brines;
-Identifying factors affecting the discharge of ions during Electrolysis
-Construction of electrolytic and electrochemical cells
-Faraday’s laws of Electrolysis
-Calculating the amount of substances liberated or deposited at electrodes during electrolysis
-The uses of electrolysis in the extraction and purification of metals
Oxidation-Reduction (Redox) Reactions
Defining of oxidation as the addition of oxygen removal of hydrogen;
Process of electron loss
Process of increase of oxidation number of a substance
Define reduction as the reverse of any of the above processes.
Calculating oxidation numbers of elements using a set of arbitrary rules:
(a) oxidation number of free elements = 0
(b) oxidation number of oxygen in any compound is except in peroxides where it is – 1
(c) oxidation number of H is + 1, except in hydrides where it is – 1
(d) the oxidation number of a neutral molecule or compound is zero e.g. H2SO4 =0 etc.
Use oxidation numbers to name inorganic compounds, to include the number of oxygen atom and water
molecules (if hydrated) determine the oxidation states number of common elements in their compounds
Defining of oxidizing and reducing agents in terms of addition and removal of oxygen and hydrogen respectively loss and gain of electrons change in oxidation numbers/states
Writing and balancing redox equations.
Oxidation-Reduction (Redox) Reactions
Defining of oxidation as the addition of oxygen removal of hydrogen;
Process of electron loss
Process of increase of oxidation number of a substance
Define reduction as the reverse of any of the above processes.
Calculating oxidation numbers of elements using a set of arbitrary rules:
(a) oxidation number of free elements = 0
(b) oxidation number of oxygen in any compound is except in peroxides where it is – 1
(c) oxidation number of H is + 1, except in hydrides where it is – 1
(d) the oxidation number of a neutral molecule or compound is zero e.g. H2SO4 =0 etc.
Use oxidation numbers to name inorganic compounds, to include the number of oxygen atom and water
molecules (if hydrated) determine the oxidation states number of common elements in their compounds
Defining of oxidizing and reducing agents in terms of addition and removal of oxygen and hydrogen respectively loss and gain of electrons change in oxidation numbers/states
Writing and balancing redox equations.
Oxidation-Reduction (Redox) Reactions
Defining of oxidation as the addition of oxygen removal of hydrogen;
Process of electron loss
Process of increase of oxidation number of a substance
Define reduction as the reverse of any of the above processes.
Calculating oxidation numbers of elements using a set of arbitrary rules:
(a) oxidation number of free elements = 0
(b) oxidation number of oxygen in any compound is except in peroxides where it is – 1
(c) oxidation number of H is + 1, except in hydrides where it is – 1
(d) the oxidation number of a neutral molecule or compound is zero e.g. H2SO4 =0 etc.
Use oxidation numbers to name inorganic compounds, to include the number of oxygen atom and water
molecules (if hydrated) determine the oxidation states number of common elements in their compounds
Defining of oxidizing and reducing agents in terms of addition and removal of oxygen and hydrogen respectively loss and gain of electrons change in oxidation numbers/states
Writing and balancing redox equations.
Oxidation-Reduction (Redox) Reactions
Defining of oxidation as the addition of oxygen removal of hydrogen;
Process of electron loss
Process of increase of oxidation number of a substance
Define reduction as the reverse of any of the above processes.
Calculating oxidation numbers of elements using a set of arbitrary rules:
(a) oxidation number of free elements = 0
(b) oxidation number of oxygen in any compound is except in peroxides where it is – 1
(c) oxidation number of H is + 1, except in hydrides where it is – 1
(d) the oxidation number of a neutral molecule or compound is zero e.g. H2SO4 =0 etc.
Use oxidation numbers to name inorganic compounds, to include the number of oxygen atom and water
molecules (if hydrated) determine the oxidation states number of common elements in their compounds
Defining of oxidizing and reducing agents in terms of addition and removal of oxygen and hydrogen respectively loss and gain of electrons change in oxidation numbers/states
Writing and balancing redox equations.
Mass, Volume Relationships: Stoichiometry
– Explain the concept of the mole, molar, s.t.p.; Relative densities and relative molar mass (RMM)
-Solve problems involving reacting masses and volumes in chemical reactions.
-State the SI units of various basic quantities.
Mass, Volume Relationships: Stoichiometry
– Explain the concept of the mole, molar, s.t.p.; Relative densities and relative molar mass (RMM)
-Solve problems involving reacting masses and volumes in chemical reactions.
-State the SI units of various basic quantities.
Mass, Volume Relationships: Stoichiometry
– Explain the concept of the mole, molar, s.t.p.; Relative densities and relative molar mass (RMM)
-Solve problems involving reacting masses and volumes in chemical reactions.
-State the SI units of various basic quantities.
Chemical Reactions
Identifying reactants and products of any chemical reaction
Explaining the terms reaction time and reaction rate; and the relationship between the two.
Explaining collision theory with respect to reaction time and reaction rate
Describing the influence of the following on chemical reaction rates:
– nature of substances;
– concentration/pressure,
– temperature and catalysts
Endothermic and exothermic reactions
Equations for simple equilibrium reaction
Le Chateller’s principle
Influence of the following factors on the equilibrium of chemical reactions:
– Concentration
– Temperature
– Pressure
Periodic Table(i)
-The periodic law
-Arrangement of common elements into groups (families) and periods
-Distinguishing between the families of elements on the periodic table
-The changes in the properties of elements down the group and across periods
-The relationship between ionization energy and electron affinity and the properties of elements down the groups and across periods
-The diagonal relationship in the properties of elements
Periodic Table(i)
-The periodic law
-Arrangement of common elements into groups (families) and periods
-Distinguishing between the families of elements on the periodic table
-The changes in the properties of elements down the group and across periods
-The relationship between ionization energy and electron affinity and the properties of elements down the groups and across periods
-The diagonal relationship in the properties of elements
Periodic Table(i)
-The periodic law
-Arrangement of common elements into groups (families) and periods
-Distinguishing between the families of elements on the periodic table
-The changes in the properties of elements down the group and across periods
-The relationship between ionization energy and electron affinity and the properties of elements down the groups and across periods
-The diagonal relationship in the properties of elements
Periodic Table(i)
-The periodic law
-Arrangement of common elements into groups (families) and periods
-Distinguishing between the families of elements on the periodic table
-The changes in the properties of elements down the group and across periods
-The relationship between ionization energy and electron affinity and the properties of elements down the groups and across periods
-The diagonal relationship in the properties of elements