Metals that react with nitric acid:
* Active metals: These metals are highly reactive and readily react with nitric acid to produce nitrates, hydrogen gas, and water. Examples include:
* Group 1 metals (alkali metals): Lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr).
* Group 2 metals (alkaline earth metals): Beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).
* Less active metals: These metals react with nitric acid, but the reaction is more complex and may produce nitrogen oxides instead of hydrogen gas. Examples include:
* Transition metals: Iron (Fe), zinc (Zn), nickel (Ni), copper (Cu), silver (Ag), and mercury (Hg).
* Other metals: Aluminum (Al), tin (Sn), and lead (Pb).
Metals that do not react with nitric acid:
* Noble metals: These metals are very unreactive and do not react with nitric acid. Examples include:
* Group 11 metals: Gold (Au) and platinum (Pt).
Important notes:
* Concentration of nitric acid: The concentration of nitric acid influences the reaction products. Dilute nitric acid will typically produce nitrates, hydrogen gas, and water, while concentrated nitric acid will produce nitrogen oxides and nitrates.
* Passivation: Some metals, such as aluminum and chromium, can form a protective oxide layer on their surface when exposed to nitric acid. This oxide layer prevents further reaction with the acid, a phenomenon known as passivation.
Examples of reactions:
* Reaction of zinc with dilute nitric acid:
Zn(s) + 2 HNO₃(aq) → Zn(NO₃)₂(aq) + H₂(g)
* Reaction of copper with concentrated nitric acid:
Cu(s) + 4 HNO₃(conc.) → Cu(NO₃)₂(aq) + 2 NO₂(g) + 2 H₂O(l)
It's important to remember that these are just general guidelines, and the actual reaction products can vary depending on specific conditions. Always consult a reliable chemistry reference for detailed information about the reactions of specific metals with nitric acid.
