Question

Explain anomalous behaviour of oxygen in group 16 with respect to: i. Atomicity ii. Magnetic property iii. Oxidation state

Hint:

Oxygen’s unique magnetic properties (paramagnetic behavior) and its ability to exhibit various oxidation states make it different from other elements in group 16.

Answer 1

i. Atomicity:
In group 16, oxygen exists as a diatomic molecule (\(O_2\)), unlike other elements in the group, such as sulfur, which exist in polyatomic forms. Oxygen’s small size, high electronegativity, and the ability to form strong bonds lead it to exist as a diatomic molecule. ii. Magnetic Properties:
Oxygen (\(O_2\)) is paramagnetic, meaning it has unpaired electrons. This is due to the presence of two unpaired electrons in its molecular orbital configuration, which makes it attract a magnetic field. iii. Oxidation State:
Oxygen shows an oxidation state of -2 in most of its compounds, but it can also exhibit positive oxidation states, such as +1 in peroxide (\(O_2^{2-}\)) and +2 in oxygen difluoride (\(OF_2\)). The tendency of oxygen to exhibit positive oxidation states is an anomaly compared to other elements in group 16.