Tag: p- block elements-ii

$N _{2}O _{5}$ in solid form exists as $NO _{3}^{-}$ and $NO _{2}^{-}$.

N forms such bonds as,
$N \equiv N;  -C \equiv N;  N\equiv O$

As vacant d-orbital are present in P and other elements of this group except N so they can expand their valency and forms stable pentavalence product but due to absence of d-orbitals nitrogen cannot form pentavalence products.

Nitrogen differs from other members of the group due to its smaller size, high electronegativity, high IE and non availability of d-orbitals. Nitrogen has unique ability to form $p\pi - p\pi $ multiple bonds with itself and with other elements having small size and high electronegativity.

Here, $X$ is nitrogen with atomic number 7 and electronic configuration $ { 1s }^{ 2 }{ 2s }^{ 2 }{ 2p }^{ 3 } $ 

In atoms of nitrogen molecule, nonpolar covalent bonds are present.
Nonpolar covalent bond is formed between two atoms having zero electronegativty difference.

Nitrates of divalent and trivalent metals (Mg, Ca, Ba, Pb, Cu, Zn, Hg, Al, Fe etc.) decompose on heating to give reddish brown fumes of nitrogen dioxide.

The nitrates, chlorates, and acetates of all metals are soluble in water.

Nitrates are not stable to heat they decompose to release nitrogen dioxide.

Nitrogen molecule ($\displaystyle N _2$) is relatively more stable. Each $N$ atom has completed its octet and there is a triple bond between two $N$ atoms. In other molecules, there is either a single bond or a double bond between two atoms. A triple bond is stronger than a single or double bond.

$NH _4Cl+NaNO _2 \rightarrow N _2+NaCl+2H _2O$

The weak catenation property of nitrogen is due to lone pair repulsion of lone pair of electrons on nitrogen molecule.