Question

Electronic configuration of some elements are given below:
$L:1s^{2}2s^{2}2p^4$
$Q:1s^{2}2s^{2}2p^{6}3s^{2}3p^5$
$P:1s^{2}2s^{2}2p^6,3s^1$
$R:1s^{2}2s^{2}2p^{6}3s^2$
The ionic compound that can be formed by these elements are:

• A. $L_{2}P,RL,PQ$ and $R_{2}Q$
• B. $LP,RL,PQ$ and $RQ$
• C. $P_{2}L,RL,PQ$ and $R{Q}_2$
• D. $LP,R_{2}L,P_{2}Q$ and $RQ$

Answer 1

The correct option is C $P_{2}L,RL,PQ$ and $R{Q}_2$

Based on the given electronic configurations, it can be inferred that,
L represents O atom,
Q represents Cl atom,
P represents Na atom and
R represents Mg atom.

So,
The compound formed between L and P will $P_{2}L$.
The compound formed between L and R will be $RL$.
The compound formed between P and Q will be $PQ$.
The compound formed between R and Q will be $R{Q}_2$.