Lesson Note on Chemistry SS2 Second Term
SCHEME OF WORK
Week One: Rate of reactions
Week Two: Types of Chemical Reactions
Week Three: Chemical Equilibrium
Week Four: Non-metals
Week Five: Oxygen
Week Six: Halogen
Week Seven: Nitrogen
Week Eight: Compounds of Nitrogen
Week Nine: Sulphur
Week Ten: Compounds of Sulphur
Week Eleven: Revision
Week Twelve: Examination
Chemistry Lesson Note For SS2 (Second Term)
Below are the 2022 complete Chemistry lesson notes for SS2 Second Term
Week One: Rate of reactions
INTRODUCTION:
A chemical reaction is a process that transforms one set of chemical substances to another. The substances that take part in chemical reactions are known as reactants and the substances produced by the reaction are known as products.
The reaction rate is a measure of the change in the concentration of reactants or products over time in a chemical reaction. In other words, the rate of chemical change is the number of moles of the reacting substances which disappear or the number of moles of products which appear per unit time for a given quantity of the reacting species. As products are formed reactants are used up.To learn more, click here.
Week Two: Types of Chemical Reactions
INTRODUCTION:
Chemical reactions are changes in which some new chemical substances are formed. The substances which undergo the chemical change are known as reactants while the new substances formed are called products. Here’s a list of the different types of reactions, with examples of each type included. To learn more, click here.
Week Three: Chemical Equilibrium
INTRODUCTION:
Chemical equilibrium has been reached in a reaction when the rate of the forward reaction is equal to the rate of the reverse reaction. When a chemical reaction has reached equilibrium, collisions are still occurring: the reaction is now happening in each direction at the same rate.
This means that reactants are being formed at the same rate as products are being formed, and this is indicated by double arrows. At equilibrium, the reaction can lie far to the right, meaning that there are more products in existence at equilibrium, or far to the left, meaning that at equilibrium there are more reactants. The concentration of the reactants and products in a reaction at equilibrium can be expressed by the equilibrium constant, symbolized K or Keq. To learn more, click here.
Week Four: Non-metals
INTRODUCTION:
Hydrogen was first isolated and shown to be a discrete element by Henry Cavendish in 1766. Before that, Robert Boyle and Paracelsus both used reactions of iron and acids to produce hydrogen gas. Antoine Lavoisier gave hydrogen its name because it produced water when ignited in air. Hydrogen comes from the Greek meaning “water producer” (“hydro” =water and “gennao”=to make). To learn more, click here.
Week Five: Oxygen
INTRODUCTION:
Oxygen is a colourless, odourless, tasteless gas. It is denser than air and only slightly soluble in water. A poor conductor of heat and electricity, oxygen supports combustion but does not burn. Normal atmospheric oxygen is a diatomic gas (O2). Ozone is a highly reactive triatomic (O3) allotrope of oxygen.To learn more, click here.
Week Six: Halogen
INTRODUCTION:
Halogens are the collective name given to the elements in group VII of the Periodic Table. There are five halogens; fluorine, chlorine, bromine, iodine and astatine. Astatine is very radioactive and cannot exist for more than a few microseconds before decaying. We will thus be concerned with the chemistry of fluorine, chlorine, bromine and iodine. To learn more, click here.
Week Seven: Nitrogen
INTRODUCTION:
The nitrogen family includes the following compounds: nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi).
All Group 5 elements have the electron configuration ns2np3 in their outer shell, where n is equal to the principal quantum number. The nitrogen family is located in the p-block in Group 5, having 5 electrons in their outer energy level. As you move down the nitrogen family: atomic radius increases, ionic radius increases, ionization energy decreases, and electronegativity decreases. Nitrogen family elements often form covalent compounds, usually with the oxidation numbers +3 or +5. Nitrogen and phosphorus are non-metals, Arsenic and Antimony are metalloids, while Bismuth is a metal. To learn more, click here.
Week Eight: Compounds of Nitrogen
INTRODUCTION:
Ammonia was earlier known by the name “alkaline air.” It was identified in 1716 by J. Kunckel. It was prepared in a lab for the first time by Joseph Priestly in 1774. Although Claude Berthelot studied the chemical composition of the gas in 1785, it was Davy who proved in 1800 that it was composed of the elements nitrogen and hydrogen. In nature, ammonia occurs in both free as well as in the combined state. To learn more, click here.
Week Nine: Sulphur
INTRODUCTION:
Sulphur is a yellow, brittle non-conducting solid with a fairly low melting point (115oC). It is insoluble in water but soluble in other solvents such as carbon disulphide or methylbenzene. In the lab, sulphur can be found as two forms: roll sulphur and flowers of sulphur. (Note: these are not allotropes but just different forms – polymorphs. Sulphur is extracted from the earth’s crust via Frasch process. To learn more, click here.
Week Ten: Compounds of Sulphur
INTRODUCTION:
Hydrogen Sulphide occurs naturally in petroleum deposits and is also an air pollutant. It is easily identified by its characteristic smell.
Laboratory Preparation
Hydrogen Sulphide is prepared by the action of dilute hydrochloric acid on iron (II) sulphide. The liberated gas is collected above warm water (since it readily dissolves in cold water) or by downward delivery. To learn more, click here.
Week Eleven: Revision
This week, we would be doing a revision of all that we learned during the term.
Week Twelve: Examination
Afterwards, we would write an examination, which would test our knowledge of what has been taught so far.
