Lesson Notes By Weeks and Term - Senior Secondary 2

TERM׃ 3^RD TERM

WEEK ONE

Class: Senior Secondary School 2

Age: 16 years

Duration: 40 minutes of 5 periods each

Date:

Subject: Chemistry

Topic: Sulphur 1

SPECIFIC OBJECTIVES: At the end of the lesson, pupils should be able to

1. identify the general properties of group VI elements.
2. explain the electronic configuration of sulphur,
3. identify the allotropes of suphur.
4. Identify the uses of sulphur.

INSTRUCTIONAL TECHNIQUES: Identification, explanation, questions and answers,

demonstration, videos from source

INSTRUCTIONAL MATERIALS: Videos, loud speaker, textbook, pictures

INSTRUCTIONAL PROCEDURES

PERIOD 1-2

NOTE

SULPHUR 1

Sulfur is a chemical element with the symbol "S" and atomic number 16. It is a non-metal and can be found in various forms, including elemental sulfur, sulfide minerals, and sulfate minerals.

General properties of group VI elements

Group VI elements, also known as the oxygen group, include oxygen (O), sulfur (S), selenium (Se), tellurium (Te), and polonium (Po). Some properties of Group VI elements include;

1. Valence Electrons: Group VI elements have six valence electrons, making them tend to gain two electrons to achieve a stable electron configuration.
2. Oxidation States: Members of this group can exhibit various oxidation states, but the -2 oxidation state is the most common. They often form compounds by gaining two electrons.
3. Oxides: Group VI elements form oxides, such as water (H₂O) and carbon dioxide (CO₂), where oxygen typically exhibits a -2 oxidation state.
4. Acid-Base Properties: These elements can act as both acids and bases. For example, oxides of sulfur can react with water to form acidic solutions.

Electronic Configuration of Sulfur

The electronic configuration of sulfur (S) is [Ne] 3s² 3p⁴. This indicates that sulfur has 16 electrons arranged in two energy levels, with 2 electrons in the 3s subshell and 4 electrons in the 3p subshell.

Allotropes of Sulfur

Sulfur exhibits several allotropes, which are different structural forms of the same element. The most common allotropes of sulfur are:

1. Rhombic Sulfur (α-Sulfur): This is the stable form at lower temperatures, consisting of S₈ rings. It appears as yellow crystals.

2. Monoclinic Sulfur (β-Sulfur): This allotrope is stable at higher temperatures and consists of S₈ rings in a different crystalline arrangement. It transforms into rhombic sulfur upon cooling.
3. Amorphous Sulfur: This is a non-crystalline form of sulfur without a definite structure. It is formed when sulfur is melted and cooled rapidly.

Uses of Sulfur

1. Sulfuric Acid Production: Sulfuric acid (H₂SO₄) is a widely used industrial chemical, and sulfur is a key raw material in its production.
2. Fertilizers: Sulfur is an essential component in the production of fertilizers, providing plants with the necessary nutrients.
3. Pharmaceuticals: Sulfur compounds are used in the pharmaceutical industry for the synthesis of various drugs.
4. Vulcanization of Rubber: Sulfur is crucial in the vulcanization of rubber, a process that improves its elasticity and durability.
5. Pesticides and Insecticides: Sulfur is used in the production of certain pesticides and insecticides for agricultural purposes.
6. Chemical Synthesis: Sulfur compounds are involved in the synthesis of a wide range of chemicals, including dyes, detergents, and solvents.

EVALUATION:   1. Identify 4 properties of group VI elements

2. Write down the electronic configuration of sulphur
3. Mention at least two allotropes of sulphur
4. Enumerate 4 uses of sulphur

CLASSWORK: As in evaluation

CONCLUSION: The teacher commends the students positively