In ammonia (NH₃), the oxidation number of nitrogen (N) can be determined by considering the oxidation states of the constituent atoms and the overall charge of the molecule. Here’s a step-by-step breakdown:
Understand Oxidation Numbers:
- Oxidation numbers represent the hypothetical charge of an atom if all bonds were completely ionic.
- Hydrogen typically has an oxidation number of +1 in compounds.
- The sum of the oxidation numbers in a neutral molecule must equal zero.
- Oxidation numbers represent the hypothetical charge of an atom if all bonds were completely ionic.
Set Up the Equation:
Let ( x ) be the oxidation number of nitrogen in NH₃.
Since there are three hydrogen atoms, each with an oxidation number of +1, the equation becomes:
[ x + 3(+1) = 0 ]Solve for ( x ):
[ x + 3 = 0 \implies x = -3 ]Conclusion:
The oxidation number of nitrogen (N) in ammonia (NH₃) is (-3).
Why This Matters
Understanding oxidation numbers is crucial for predicting chemical behavior, such as reactivity in redox reactions. In NH₃, nitrogen’s (-3) oxidation state indicates it is reduced and can potentially be oxidized in reactions, such as in the Ostwald process for nitric acid production.
FAQ Section
How does the oxidation number of nitrogen in NH₃ compare to NO₂?
+In NO₂, nitrogen has an oxidation number of +4. This contrasts with NH₃ (-3), highlighting nitrogen’s versatility in oxidation states depending on the compound.
Can nitrogen in NH₃ be further reduced?
+No, nitrogen in NH₃ is already in its lowest oxidation state (-3). Further reduction would require breaking N-H bonds, which is energetically unfavorable.
Why is hydrogen’s oxidation number +1 in NH₃?
+Hydrogen typically has a +1 oxidation number in compounds with non-metals, as it donates its electron to form a bond.
This analysis underscores the importance of oxidation numbers in chemical analysis and their role in understanding molecular properties and reactivity.
