The second ionization energies of Li, Be, B and C are in the order

Options

A. `Li gt C gt B gt Be`
B. `LigtBgtBegtC`
C. `BgtCgtBegtLi`
D. `BegtCgtBgtLi`

Answer

To determine the order of second ionization energies for Li, Be, B, and C, we need to understand the electronic configurations and the stability of the resulting ions after the second ionization.

### Step-by-Step Solution:

1. **Understand Ionization Energy**:
- Ionization energy is the energy required to remove an electron from an atom in the gaseous state. The second ionization energy refers to the energy needed to remove a second electron after the first has already been removed.

2. **Write the Electronic Configurations**:
- Lithium (Li): 1s² 2s¹
- Beryllium (Be): 1s² 2s²
- Boron (B): 1s² 2s² 2p¹
- Carbon (C): 1s² 2s² 2p²

3. **Identify the Ions After First Ionization**:
- After the first ionization:
- Li⁺: 1s² (stable noble gas configuration)
- Be⁺: 1s² 2s¹
- B⁺: 1s² 2s²
- C⁺: 1s² 2s² 2p¹

4. **Consider the Stability of the Resulting Ions**:
- Removing a second electron from Li⁺ (which has a stable configuration) requires significantly more energy.
- For Be⁺, removing the second electron (from 2s¹) is easier than from Li⁺ but still requires a fair amount of energy.
- For B⁺, removing the second electron (from 2s²) is less energy-intensive than Be⁺.
- For C⁺, removing the second electron (from 2p¹) is the least energy-intensive because it is removing an electron from a p-orbital.

5. **Order of Second Ionization Energies**:
- Based on the stability and the energy required to remove the second electron, the order of second ionization energies is:
- Li < Be < B < C

### Final Answer:
The second ionization energies of Li, Be, B, and C are in the order: **Li < Be < B < C**.