Nitrogen can have several different oxidation numbers ranging in value from -3 to +5. (b) Based on oxidation numbers, which nitrogen oxide from part (a) cannot react with molecular oxygen?

검증된 단계별 안내

insert step 1: Identify the oxidation numbers of nitrogen in the different nitrogen oxides.

insert step 2: Determine the possible oxidation states of nitrogen, which range from -3 to +5.

insert step 3: Recognize that a nitrogen oxide with nitrogen in its highest oxidation state (+5) cannot be further oxidized by molecular oxygen.

insert step 4: Compare the oxidation numbers of nitrogen in each oxide to identify which one has nitrogen in the +5 oxidation state.

insert step 5: Conclude that the nitrogen oxide with nitrogen in the +5 oxidation state cannot react with molecular oxygen, as it is already fully oxidized.

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Oxidation Numbers

Oxidation numbers are a way to keep track of electrons in chemical reactions, indicating the degree of oxidation of an atom in a compound. They can be positive, negative, or zero, and help determine how atoms will interact during reactions. For nitrogen, common oxidation states include -3 (in ammonia) and +5 (in nitric acid), reflecting its ability to gain or lose electrons.

Nitrogen Oxides

Nitrogen oxides are a group of gases that include various compounds formed by nitrogen and oxygen, such as NO, NO2, and N2O. Each oxide has distinct properties and reactivity based on the oxidation state of nitrogen. Understanding the specific nitrogen oxide in question is crucial for predicting its behavior, particularly its ability to react with molecular oxygen.

Reactivity with Molecular Oxygen

The reactivity of a compound with molecular oxygen (O2) depends on its oxidation state and the stability of its bonds. Compounds with lower oxidation states, like -3, are generally less reactive with O2, while those with higher oxidation states, such as +5, are more likely to react. Identifying which nitrogen oxide cannot react with O2 involves analyzing its oxidation state and stability.