Use the letters only written in the periodic table given below to answer the questions that follow

(i) State the number of valence electrons in atom $\mathrm{J}$.

(ii) Which element forms ions with a single negative charge?

(iii) Out of $\mathrm{I}$ and $\mathrm{R}$ which one is more reactive?

(iv) Which element has its electrons arranged in four shells?

The metals of the group $2$ from top to bottom are $\mathrm{B}\mathrm{e}, \mathrm{M}\mathrm{g}, \mathrm{C}\mathrm{a}, \mathrm{S}\mathrm{r}$ and $\mathrm{B}\mathrm{a.}$

(i) Which one of these elements will form ions most readily and why?

(ii) State the common feature in the electronic configuration of all these elements.

Arrange the following as per the instructions given in the bracket.

$\mathrm{M}\mathrm{g}, \mathrm{C}\mathrm{l}, \mathrm{N}\mathrm{a}, \mathrm{S}, \mathrm{S}\mathrm{i}$ (Decreasing order of atomic size).

Arrange the following as per the instructions given in the bracket.

$\mathrm{N}\mathrm{a}, \mathrm{K}, \mathrm{C}\mathrm{l}, \mathrm{S}, \mathrm{S}\mathrm{i}$ (Increasing order of ionisation energy).

Element $\mathrm{X}$ is a metal with a valency $2,\mathrm{Y}$ is a non-metal with a valency $3$.

(i) Write an equation to show how $\mathrm{Y}$ forms an ion?

(ii) If $\mathrm{Y}$ is a diatomic gas, write an equation for the direct combination of $\mathrm{X}$ and $\mathrm{Y}$ to form a compound.