Question

1. draw the lewis structures of 2 elements from each of the 4 families.

Explanation:

Lewis structures represent the bonding between atoms of a molecule and the lone - pair electrons present. First, identify the valence electrons of the elements from the given families. Then, arrange the atoms and distribute the electrons to satisfy the octet rule (except for hydrogen which follows the duet rule).

Answer:

Let's assume four common families: alkali metals (Group 1), halogens (Group 17), noble gases (Group 18), and carbon - group elements (Group 14).

• Alkali metals (e.g., Li and Na):
• Lithium (Li): It has 1 valence electron. The Lewis structure is Li•.
• Sodium (Na): It has 1 valence electron. The Lewis structure is Na•.
• Halogens (e.g., F and Cl):
• Fluorine (F): It has 7 valence electrons. The Lewis structure is :F• with 3 lone - pairs and 1 unpaired electron.
• Chlorine (Cl): It has 7 valence electrons. The Lewis structure is :Cl• with 3 lone - pairs and 1 unpaired electron.
• Noble gases (e.g., Ne and Ar):
• Neon (Ne): It has 8 valence electrons. The Lewis structure is :Ne: with 4 lone - pairs.
• Argon (Ar): It has 8 valence electrons. The Lewis structure is :Ar: with 4 lone - pairs.
• Carbon - group elements (e.g., C and Si):
• Carbon (C): It has 4 valence electrons. The Lewis structure is •C• with 4 unpaired electrons.
• Silicon (Si): It has 4 valence electrons. The Lewis structure is •Si• with 4 unpaired electrons.