Question

The electonic configuration of four different elements is given below. Identify the group 14 element among these

• A. $\left[He\right]2s^1$
• B. $\left[He\right]3s^2$
• C. $\left[Ne\right]3s^{2}3p^2$
• D. $\left[Ne\right]3s^{2}3p^5$

Answer 1

The correct option is C $\left[Ne\right]3s^{2}3p^2$

The general elctronic configuration of group 14 elements is [noble gas] $n{s}^{2}n{p}^2$.
$\left[Ne\right]3s^{2}3p^2$ is electronic configuration of Silicon which belongs to group 14.
Hence correct option is c.

THEORY
Group 14 element:
1. Electronic configuration- $\left[\text{noble gas}\right]n{s}^{2}n{p}^2$
$\text{Atomic number}\text{Element}$
$6\text{Carbon(C)}$
$14\text{Silicon(Si)}$
$32\text{Germanium(Ge)}$
$50\text{Tin(Sn)}$
$82\text{Lead(Pb)}$
2. Naturally occurring carbon contains three isotopes
${}^{12}C$ ,${}^{1}3C$ ,${}^{14}C$
${}^{12}C$ ,${}^{13}C$ are stable isotopes.
${}^{14C}$ is a Radioactive isotope with half-life 5770 years.
3. Silicon is a very important component of ceramics, glass and cement. Germanium exists only in traces.
4. Tin occurs mainly as cassiterite, $Sn{O}_2$ and lead as galena, PbS.
5. Covalent radii:
Down the group, for each successive member one extra shell of electrons is added. This decreases the attraction between nucleus and outermost electrons. Since the nuclear charge decreases down the group the atomic radius of the element increases.
Considerable increase in covalent radius from C to Si, followed by a small increase from Si to Pb.This is due to the presence of completely filled d and f orbitals in heavier members.