The general formula of the compound formed when a metal $(M)$ of group $1$ reacts with a non-metal $(X)$ of group $16$ is:

What would be the formula of the compound formed between the following elements?
$(i)$ Aluminium and Bromine
$(ii)$ Sodium and Oxygen
$(iii)$ Silicon and Oxygen
$(iv)$ Phosphorus and Chlorine

Number of elements from the following that $CANNOT$ form compounds with valencies which match with their respective group valencies is
$B, C, N, S, O, F, P, Al, Si$

Consider the following information about elements $P$ and $Q$:

Element	Information
$P$	Period number: $2$,Group number: $15$
$Q$	Period number: $3$,Group number: $2$

Then,the formula of the compound formed by elements $P$ and $Q$ is:

The oxidation states of phosphorus vary from

In view of the signs of $\Delta_{r} G^{\circ}$ for the following reactions:
$PbO_2 + Pb \longrightarrow 2 PbO, \Delta_{r} G^{\circ} < 0$
$SnO_2 + Sn \longrightarrow 2 SnO, \Delta_{r} G^{\circ} > 0$
Which oxidation states are more characteristic for lead and tin?