Rank the compounds below in order of increasing oxidation level (1 = lowest oxidation level, 4 = highest oxidation level). If two compounds are at the same oxidation level, give them the same rank. (For example, an answer might be of the form 1,1,3,4 or 1,2,2,4.)

1. In a C-H bond, the H is treated as if it has an oxidation state of +1. This means that every C-H bond will decrease the oxidation state of carbon by 1.

2. Any two bonds between the same atom do not affect the oxidation state (recall that the oxidation state of Cl in Cl-Cl (and that of H in H-H) is zero. So a carbon attached to 4 carbons has an oxidation state of zero.

When calculating the oxidation state in an organic compound, your attention to be directed towards the carbon bearing the functional group. form there, apply the oxidation rules.

Oxidation Rules:

Every Bond between C and an electronegative element (C, N, O) would increase its oxidation by 1.

Every Bond between C and H would decrease its oxidation state by 1.

Every Bond between C and C does not alter its oxidation state so it is ignored in the solvings.

A)

The functional group is the Amine group hence emphasis is on the last Carbon. It is attached to 2 Hydrogen (-1) and a Nitrogen (+1).

2H+N =C

2(-1)+ 1 = C

-2 +1 = C

-1 = C

C= -1

B)

The functional group is the bromine hence emphasis is on the last Carbon. It is attached to 2 Hydrogen (-1) and a Bromine (+1).

2H+ Br =C

2(-1) +1 = C

-2 +1 = C

-1 = C

C = - 1

C)

The functional group is the Carbonyl group hence emphasis is on the middle Carbon.

Since there are two oxygen atoms it would increase it by 2 * 1 = + 2

D)

The functional group is the Chlorine group hence emphasis is on the last Carbon. It is attached to 2 Hydrogen (-1) and a Chlorine (+1).

2H +Cl = C

2(-1) +1 = C

-2 + 1 = C

C = −1