Correct order of `IE_(1)` are:
(P) `Li lt B lt Be lt C` (Q) `O lt N lt F`
(R) `Be lt N lt Ne`

Options

A. P,Q
B. Q only
C. P,R
D. P,Q,R

Explanation

To determine the correct order of first ionization energies (IE₁) for the given elements, we will analyze the trends in ionization energy based on their electronic configurations and periodic trends.

### Step-by-Step Solution:

1. **Identify the Elements and Their Electronic Configurations**:
- The elements in question are from the second period:
- Lithium (Li): 1s² 2s¹
- Beryllium (Be): 1s² 2s²
- Boron (B): 1s² 2s² 2p¹
- Carbon (C): 1s² 2s² 2p²
- Nitrogen (N): 1s² 2s² 2p³
- Oxygen (O): 1s² 2s² 2p⁴
- Fluorine (F): 1s² 2s² 2p⁵
- Neon (Ne): 1s² 2s² 2p⁶

2. **Understand the Trend of Ionization Energy**:
- Ionization energy generally increases across a period from left to right due to increasing nuclear charge, which holds the electrons more tightly.
- However, there are exceptions due to half-filled and fully filled subshells which provide extra stability.

3. **Analyze Each Given Order**:
- **(P) `Li < B < Be < C`**:
- Lithium has the lowest IE₁ because it has one electron in the outer shell and is easily ionized.
- Boron has a higher IE₁ than lithium but lower than beryllium because it has a higher nuclear charge but is less stable than beryllium.
- Beryllium has a higher IE₁ than boron because it has a fully filled 2s subshell, making it more stable and harder to ionize.
- Carbon has a higher IE₁ than beryllium due to its increased nuclear charge and stability.
- Therefore, this order is correct.

- **(Q) `O < N < F`**:
- Oxygen has a lower IE₁ than nitrogen because removing an electron from oxygen results in a half-filled p subshell (2p³), which is more stable.
- Nitrogen has a higher IE₁ than oxygen but lower than fluorine, as fluorine has a very high nuclear charge and is very electronegative.
- Thus, this order is also correct.

- **(R) `Be < N < Ne`**:
- Beryllium has a lower IE₁ than nitrogen because it is stable with a filled 2s subshell.
- Nitrogen has a lower IE₁ than neon because neon has a completely filled outer shell, making it very stable.
- Therefore, this order is also correct.

4. **Conclusion**:
- All three orders (P, Q, R) are correct regarding the first ionization energies of the elements.

### Final Answer:
The correct order of first ionization energies is **P, Q, R**.