The correct order of basicity of the following compounds is:
- IV > III > II > I
Basicity is the tendency of an atom or molecule to accept an electron pair. The more basic an atom or molecule is, the stronger its attraction for electrons.
In the given compounds, the central atom is nitrogen. Nitrogen has a valence of 5, which means it can form 5 bonds. In compound I, nitrogen is bonded to 3 hydrogen atoms and 1 oxygen atom. In compound II, nitrogen is bonded to 2 hydrogen atoms and 2 oxygen atoms. In compound III, nitrogen is bonded to 1 hydrogen atom and 3 oxygen atoms. In compound IV, nitrogen is bonded to 0 hydrogen atoms and 4 oxygen atoms.
Oxygen is more electronegative than hydrogen. This means that oxygen has a stronger attraction for electrons than hydrogen. In compound I, nitrogen is bonded to 3 hydrogen atoms and 1 oxygen atom. The oxygen atom will pull electrons away from the nitrogen atom, making it less basic. In compound II, nitrogen is bonded to 2 hydrogen atoms and 2 oxygen atoms. The oxygen atoms will pull electrons away from the nitrogen atom, but not as strongly as in compound I. In compound III, nitrogen is bonded to 1 hydrogen atom and 3 oxygen atoms. The oxygen atoms will pull electrons away from the nitrogen atom, but not as strongly as in compound I or II. In compound IV, nitrogen is bonded to 0 hydrogen atoms and 4 oxygen atoms. The oxygen atoms will pull electrons away from the nitrogen atom very strongly, making it the least basic of the four compounds.
Therefore, the correct order of basicity of the given compounds is:
- IV > III > II > I