Lesson Notes By Weeks and Term v4 - SHS 3
PERIODICITY
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PERIODICITY
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Subject: Chemistry
Class: SHS 3
Term: 2nd Term
Week: 20
Grade code: 3.2.1.LI.2
Strand code: 2
Sub-strand code: 1
Content standard code: 3.2.1.CS.1
Indicator code: 3.2.1.LI.2
Theme: SYSTEMATIC CHEMISTRY OF THE ELEMENTS
Subtheme: PERIODICITY
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Welcome, students! Today, we will explore a fascinating part of the Periodic Table. Look around you. The iron rods in our classroom building, the aluminum roofing sheets on houses, the copper wires that bring electricity to our school, and the gold jewelry worn by our mothers and chiefs – these are all metals. However, they don't all behave in the same way. Iron rusts, but gold does not. Sodium, a metal, is soft enough to cut with a knife, while iron is very hard. This lesson focuses on understanding the key differences and similarities between two major families of metals: the Main Group Metals (like sodium and aluminum) and the Transition Metals (like iron, copper, and gold).
2.1. Defining the Metal Groups
First, let's identify our two groups on the Periodic Table. Main Group Metals (or Representative Metals): These are the metals found in the s-block (Groups 1 and 2) and the p-block (Groups 13 to 16). They have their valence (outermost) electrons in s or p orbitals. Examples: Sodium (Na), Magnesium (Mg), Aluminium (Al), Potassium (K). Transition Metals: These are the metals found in the d-block of the Periodic Table, typically Groups 3 to 12. They are called "transition" because they form a bridge between the highly reactive metals of the s-block and the non-metals of the p-block. Their defining feature is having partially filled d-orbitals. Examples: Iron (Fe), Copper (Cu), Gold (Au), Zinc (Zn), Manganese (Mn).
*(Image showing the s-block, p-block, and d-block on the periodic table)* 2.2. Detailed Comparison of Properties
Let's compare these two groups based on the properties listed in our curriculum.