Answer :
The oxidation state of oxygen (O) in is, (+2)
The oxidation state of carbon (C) in is, (+2)
The oxidation state of nitrogen (N) in is, (-3)
Explanation :
Oxidation number : It represent the number of electrons lost or gained by the atoms of an element in a compound.
Oxidation numbers are generally written with the sign (+) and (-) first and then the magnitude.
When the atoms are present in their elemental state then the oxidation number will be zero.
Rules for Oxidation Numbers :
The oxidation number of a free element is always zero.
The oxidation number of a monatomic ion equals the charge of the ion.
The oxidation number of Hydrogen (H) is +1, but it is -1 in when combined with less electronegative elements.
The oxidation number of oxygen (O) in compounds is usually -2, but it is -1 in peroxides.
The oxidation number of a Group 1 element in a compound is +1.
The oxidation number of a Group 2 element in a compound is +2.
The oxidation number of a Group 17 element in a binary compound is -1.
The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.
The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.
(a) The given compound is,
Let the oxidation state of 'O' be, 'x'
The oxidation state of oxygen (O) in is, (+2)
(b) The given compound is,
Let the oxidation state of 'C' be, 'x'
The oxidation state of carbon (C) in is, (+2)
(c) The given compound is,
Let the oxidation state of 'N' be, 'x'
The oxidation state of nitrogen (N) in is, (-3)