Metal & Nonmetal : Chemical Properties Of metal || Reactivity of metal towards Acid & dilute HNO3

Описание: Metal & Nonmetal : Chemical Properties Of metal || Reactivity of metal towards Acid & dilute HNO3



Nitric acid (HNO3) is a very strong oxidising agent. It is a strong acid and thus, it dissociates completely. Nitric acid can be concentrated or dilute depending on its concentration.
Concentrated nitric acid on reaction with metals generally gives metal nitrates. Along with metal nitrates it produces nitrogen dioxide and water.
Dilute nitric acid on reaction with metals generally gives metal nitrates. Along with metal nitrates it produces highly flammable hydrogen gas.
We know that magnesium belongs to group 2 of the periodic table. Magnesium is highly reactive in nature.
When magnesium metal reacts with very dilute nitric acid it gives magnesium nitrate (Mg(NO3)2). Along with magnesium nitrate highly flammable hydrogen gas (H2) is also produced.
The balanced chemical reaction of magnesium metal (Mg) with very dilute nitric acid (HNO3) is as follows:
Mg+2HNO3→Mg(NO3)2+H2
Thus, magnesium on reaction with very dilute HNO3 gives H2.

Concentrated nitric acid on reaction with metals generally gives metal nitrates. Along with metal nitrates it produces nitrogen dioxide and water. Magnesium metal on reaction with concentrated nitric acid gives magnesium nitrate. Along with magnesium nitrate it produces nitrogen dioxide and water. The reaction of magnesium metal with concentrated nitric acid is as follows:
Mg+2HNO3→Mg(NO3)2+NO2+H2O


NO2 Gas is a brown coloured gas whereas
H2 is colourless gas.


Curly strips of zinc and magnesium are dropped into 2M hydrochloric acid, and bubbles of hydrogen gas are observed as a result of the reactions.
In this Chemistry video in Hindi for Class 10 we explained one of the chemical properties of metals. We discussed on how metals react with acids.

Metal + Dilute acid → Salt + Hydrogen

But, hydrogen gas is not evolved when a metal reacts with nitric acid. It is because HNO₃ is a strong oxidising agent. It oxidises the H₂ produced to water.

But magnesium (Mg) and manganese (Mn) react with very dilute HNO₃ to evolve H₂ gas. Because, these are strong reducing agents and reduces H₂O into H₂


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An experiment demonstrating the reaction of sodium, potassium, zinc, aluminium and iron (nail, steel wool and filings) with oxygen. Some methods of increasing reaction rate are shown.

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