Inorganic Chemistry (B.A./B.Sc) 1st Sem Previous Year Solved Question Paper 2022

Group 14 of the periodic table includes carbon , silicon (Si), germanium (Ge), tin (Sn), and lead (Pb). The elements in this group show a wide range of oxidation states due to the increasing number of available electrons and the ability to participate in various types of chemical bonding. Here’s a brief discussion of the variation of oxidation states in Group 14:

1. Carbon :
 - Carbon primarily exhibits oxidation states of -4 (in compounds like CH4, methane), +2 (in compounds like CO2, carbon dioxide), and +4 (in compounds like CH4O, formaldehyde).
 - Carbon forms strong covalent bonds and often shares electrons, leading to a diverse range of organic compounds.

2. Silicon (Si):
 - Silicon commonly displays oxidation states of -4 (in compounds like SiH4, silane) and +4 (in compounds like SiO2, silicon dioxide).
 - Silicon is essential in the semiconductor industry and forms a variety of inorganic compounds.

3. Germanium (Ge):
 - Germanium primarily exhibits oxidation states of -4 (in compounds like GeH4, germane) and +4 (in compounds like GeO2, germanium dioxide).
 - Germanium is used in semiconductors and shares similarities with both silicon and tin.

4. Tin (Sn):
 - Tin displays oxidation states ranging from -4 to +4, but the most common oxidation states are +2 (in compounds like SnCl2, tin dichloride) and +4 (in compounds like SnO2, tin dioxide).
 - Tin also forms compounds with lower oxidation states, such as Sn2+ and Sn4+.

5. Lead (Pb):
 - Lead exhibits oxidation states of +2 (in compounds like PbCl2, lead dichloride) and +4 (in compounds like PbO2, lead dioxide).
 - Lower oxidation states, such as +2 and +4, are more common in lead compounds.

The variation in oxidation states within Group 14 elements is mainly influenced by the number of valence electrons and the tendency to form covalent bonds. As you move down the group, the number of available valence electrons increases, allowing for a wider range of oxidation states. Elements in this group can form a variety of compounds with different elements, resulting in diverse oxidation states.