nitrogen and oxygen
The oxides of nitrogen III , nitrogen IV , and nitrogen V react with water and form nitrogen-containing oxyacids. Nitrogen III oxide, N2O3, is the anhydride of nitrous acid; HNO2 forms when N2O3 reacts with water. There are no stable oxyacids containing nitrogen with an oxidation state of 4+; therefore, nitrogen IV oxide, NO2, disproportionates in one of two ways when it reacts with water. In cold water, a mixture of HNO2 and HNO3 forms. At higher temperatures, HNO3 and NO will form. Nitrogen V oxide, N2O5, is the anhydride of nitric acid; HNO3 is produced when N2O5 reacts with water: N 2 O 5 s + H 2 O l 2HNO 3 aq The nitrogen oxides exhibit extensive oxidation-reduction behavior. Nitrous oxide resembles oxygen in its behavior when heated with combustible substances. N2O is a strong oxidizing agent that decomposes when heated to form nitrogen and oxygen. Because one-third of the gas liberated is oxygen, nitrous oxide supports combustion better than air one-fifth oxygen . A glowing splinter bursts into flame when thrust into a bottle of this gas. Nitric oxide acts both as an oxidizing agent and as a reducing agent. For example: oxidizing agent: P 4 s + 6NO g P 4 O 6 s + 3N 2 g .