In which of the following compounds, the nitrogen atom exhibits negative oxidation state?

Question

In which of the following compounds, the nitrogen atom exhibits negative oxidation state? (A) Sodium nitrate (B) NO (C) Sodium azide (D) Sodium nitrite

Tardigrade Admin · Accepted Answer

Sodium azide is NaN3 . In azide (.N3-.) ion the average oxidation number of N is -1/3. In NO the oxidation number of Nitrogen is +2. In sodium nitrate (.NaNO3.) the oxidation number of nitrogen is +5. In sodium nitrite (.NaNO2.) the oxidation number of nitrogen is +3.

Q. In which of the following compounds, the nitrogen atom exhibits negative oxidation state?

Sodium nitrate

NO

Sodium azide

Sodium nitrite

Sodium azide is $N a N_{3}$ . In azide $(N_{3}^{-})$ ion the average oxidation number of N is -1/3.

In NO the oxidation number of Nitrogen is +2.

In sodium nitrate $(N a N O_{3})$ the oxidation number of nitrogen is +5.

In sodium nitrite $(N a N O_{2})$ the oxidation number of nitrogen is +3.

Q. In which of the following compounds, the nitrogen atom exhibits negative oxidation state?

Sodium nitrate

NO

Sodium azide

Sodium nitrite

Sodium azide is NaN3​ . In azide (N3−​) ion the average oxidation number of N is -1/3. In NO the oxidation number of Nitrogen is +2. In sodium nitrate (NaNO3​) the oxidation number of nitrogen is +5. In sodium nitrite (NaNO2​) the oxidation number of nitrogen is +3.

Sodium azide is $N a N_{3}$ . In azide $(N_{3}^{-})$ ion the average oxidation number of N is -1/3.

In NO the oxidation number of Nitrogen is +2.

In sodium nitrate $(N a N O_{3})$ the oxidation number of nitrogen is +5.

In sodium nitrite $(N a N O_{2})$ the oxidation number of nitrogen is +3.