Arrange the given compounds in order of decreasing oxidation state of nitrogen

(A)    \(N_2\)

(B)    \(NO\)

(C)    \(HNO_3\)

(D)   \(NH_4Cl\)

Choose the correct answer from the options given below:

\(HNO_3 > NO > N_2 > NH_4Cl\)

The correct answer is: (2) \(HNO_3 > NO > N_2 > NH_4Cl\)

The oxidation state is the number of electrons an atom has lost or gained relative to its neutral state. Nitrogen can have a wide range of oxidation states, from -3 to +5.

In \(HNO_3\), nitrogen has the highest oxidation state of +5. In \(NO\), nitrogen has an oxidation state of +2. In \(N_2\), nitrogen has an oxidation state of 0. And in \(NH_4Cl\), nitrogen has an oxidation state of -3.

Therefore, the compounds in order of decreasing oxidation state of nitrogen are: \(HNO_3 > NO > N_2 > NH_4Cl\)

The other options are incorrect:
(1) \(HNO_3 > NO > NH_4Cl > N_2\): \(NH_4Cl\) has a lower oxidation state of nitrogen than \(NO\).
(3) \(HNO_3 > NH_4Cl > NO > N_2\): \(NH_4Cl\) has a higher oxidation state of nitrogen than \(NO\).
(4) \(NO > HNO_3 > NH_4Cl > N_2\): \(HNO_3\) has a higher oxidation state of nitrogen than \(NO\).