Nitrogen forms nitride ion by accepting 3 electrons
N + 3 electrons N3-
2 Cu[s] + O2 [g] 2CuO[S]
Reddish brown black powder
The remaining part of air is mainly nitrogen.
It contains rare gases (inert gases) and water vapour as the major impurities
The apparatus is set up as shown in the diagram above. On heating, sodium nitrate reacts ammonium nitrate which decomposes to give nitrogen gas?
Na NO2 [aq] + NH4CL [aq] NH4NO2 [aq] + NaCL[aq]
NH4NO2aq N2 + 2H2O [L]
The gas is collected over water.
A VIDEO ABOUT ION FORMATION
Other methods for the preparation of nitrogen
The action of chlorine on excess ammonia
3CL2[g] + 8NH3 [g] N2 [g] + 6NH4CL[s]
Passing ammonia gas over heated copper (II) oxide
3NH3 [g] + 3CuONH [s] 3Cu [s] + N2 [g] 3H2O[g]
Reduction of oxides of nitrogen by heated copper
2Cu[s] + 2NO[s] 2CuO[s] + 2N2 [g]
Industrial preparation of nitrogen
Tests for nitrogen
Nitrogen is chemically inert. It doesn’t support burning, has no smell. It has no effects on litmus and no effect on the lime water.
It’s slightly less dense than air and is only slightly soluble in water.
Chemical reactions of nitrogen
Under ordinary conditions, nitrogen is chemically inert. Inert nature of nitrogen is due to strong bonding n the nitrogen molecules.
The energy required to break the triple bond is high
In the presence of iron catalyst the moderate temperature (450 – 5000C) at high pressure. Nitrogen reacts with hydrogen gas to form ammonia.
N2 [g] + 3N2 [g] 2NH3 [g]
Nitrogen reacts with magnesium calcium and lithium metals to form the corresponding metal which appears as white solids.
3Mg[s] + N2 [g] Mg3N2
2Ca[s] + N2 [g] Ca3N2
3Li + N2 [g] Li3N2
Uses of nitrogen
- 3It is a plant nutrient – required in protein synthesis
- Use in the manufacture of ammonia by Haber process
- Used as a coolant (refrigerant)