The mixture covalence of oxygen is

Options

A. two
B. four
C. Three
D. six

Answer

2

Explanation

In practice ,`O` is never more than divalent because when it has formed two covalent bonds it has attained a noble gas configuration ,and there are no low energy empty orbitals (such as d-orbitals )which can be used to form further bonds.Using its two lone pairs it can extend its covalence to four. However, the rest of the Group `16` element have empty d orbitals in their valence shell which can be used for bonding and hence they can form four or six bonds by unpiring ns and np electrons.
The `+4` show sboth oxidizing and reducting properties.Fluorine and oxygen bring out the maximum oxidation state of `+6`.Compounds in the `+6`state show oxidizing properties.The higher oxidation state becomes less stable on descending the group.These compounds are typically volatile because they are covalents.