Physical Properties: Group 13,14 and 15 elements

Write the general outer electronic configuration of group $15$ elements.

The metallic character of group $14$ elements _____ on moving down the group.

 The atomic radius of gallium is more than that of aluminium.

What is the reason behind gallium having less atomic radius than aluminium?

The nitrogen family elements have more ionisation enthalpy than oxygen family. The valence shell electronic configuration of bismuth is $\mathrm{X}$. $\mathrm{X}$ can be _____:

$\mathrm{A}. \mathrm{X}=\left[\mathrm{Xe}\right] 4{\mathrm{f}}^{14}5{\mathrm{d}}^{10}6{\mathrm{s}}^{2}6{\mathrm{p}}^3, \mathrm{B}. \mathrm{X}=\left[\mathrm{Xe}\right] 4{\mathrm{f}}^{14}5{\mathrm{d}}^{10}6{\mathrm{s}}^{2}6{\mathrm{p}}^2, \mathrm{C}. \mathrm{X}=\left[\mathrm{Xe}\right] 4{\mathrm{f}}^{14}5{\mathrm{d}}^{10}6{\mathrm{s}}^{1}6{\mathrm{p}}^3$

" Enter your answer as $\mathrm{A}, \mathrm{B}$ or $\mathrm{C}$."

Why does nitrogen show high ionisation than oxygen?

Discuss how does ionisation vary in group$-15$. 

The ionization energy of nitrogen is higher than oxygen. Why?

An allotrope of carbon which exhibits only two types of $\mathrm{C}-\mathrm{C}$ bond distance of $143.5 \mathrm{pm}$ and $138.3 \mathrm{pm}$, is

Why Boron has high melting point?

The acidic nature of oxides of group $13$ increases down the group.

Which element from the following pairs has higher ionization enthalpy? $\mathrm{B}$ and $\mathrm{Tl}$, $\mathrm{N}$ and $\mathrm{Bi}$.

Correct order of melting points of ${13}^{\text{th }}$group elements?

The correct order:

Which one of these does not show catenation.

Which of the following elements has the lowest melting point?

The liquefied metal that expands on solidification is

Boron has an exceptionally high melting point in the group ${13}^{\mathrm{t}\mathrm{h}}$ elements, because -

Boron has an exceptionally high melting point in the group 13 elements, because -

Catenation is the ability of