The electronic configuration of four elements `L, P, Q` and `R` are given in brackets
`L (1s^(2), 2s^(2), 2p^(4)) , P (1s^(2), 2p^(6), 3s^(1))`
`Q (1s^(2), 2s^(2)2p^(6), 3s^(2)3p^(5)), R (1s^(2), 2s^(2)2p^(6), 3s^(2))`
The formula of ionic compounds that can be formed between elements are

Options

A. `L_(2)P, RL, PQ and R_(2)Q`
B. `LP, RL, PQ and RQ`
C. `P_(2)L, RL, PQ and RQ_(2)`
D. `LP, R_(2)L, P_(2)Q and RQ`

Explanation

To determine the formulas of ionic compounds that can be formed between the elements L, P, Q, and R based on their electronic configurations, we will follow these steps:

### Step 1: Identify the Valence Electrons
1. **Element L**: Electronic configuration is \(1s^2, 2s^2, 2p^4\).
- Valence electrons = 6 (needs 2 more electrons to complete its octet).
- Valence = 2.

2. **Element P**: Electronic configuration is \(1s^2, 2p^6, 3s^1\).
- Valence electrons = 1 (can lose 1 electron).
- Valence = 1.

3. **Element Q**: Electronic configuration is \(1s^2, 2s^2, 2p^6, 3s^2, 3p^5\).
- Valence electrons = 7 (needs 1 more electron to complete its octet).
- Valence = 1.

4. **Element R**: Electronic configuration is \(1s^2, 2s^2, 2p^6, 3s^2\).
- Valence electrons = 2 (can lose 2 electrons).
- Valence = 2.

### Step 2: Determine Possible Ionic Compounds
1. **Combination of P and Q**:
- P (valence = 1) can combine with Q (valence = 1).
- The formula for the ionic compound is \(PQ\).

2. **Combination of P and L**:
- P (valence = 1) can combine with L (valence = 2).
- The formula for the ionic compound is \(P_2L\) (2 P ions for every L ion).

3. **Combination of R and Q**:
- R (valence = 2) can combine with Q (valence = 1).
- The formula for the ionic compound is \(RQ_2\) (1 R ion for every 2 Q ions).

4. **Combination of R and L**:
- R (valence = 2) can combine with L (valence = 2).
- The formula for the ionic compound is \(RL\) (1 R ion for every 1 L ion).

### Step 3: Summary of Ionic Compounds
The ionic compounds that can be formed are:
- \(PQ\)
- \(P_2L\)
- \(RQ_2\)
- \(RL\)