Triad – I `[N^(3–), O^–2, Na^+]` Triad – II `[N^+, C^+, O^+]` Choose the species with lowest IP from triad – I and the species of highest IP from triad – II respectively

Options

A. `N^(3–) , O^+`
B. `Na^+, C^+`
C. `N^(3–) , N^+`
D. `O^–, C^+`

Answer

To solve the problem, we need to determine the species with the lowest ionization potential (IP) from Triad I and the species with the highest ionization potential from Triad II.

### Step-by-Step Solution:

**Step 1: Analyze Triad I `[N^(3–), O^(–2), Na^(+)]`**
- We need to find the ionization potential of each species.
- **N^(3–)**: The electronic configuration is 1s² 2s² 2p⁶ (10 electrons). It has 7 protons (N) and a -3 charge, meaning it is less tightly bound.
- **O^(–2)**: The electronic configuration is also 1s² 2s² 2p⁶ (10 electrons). It has 8 protons (O) and a -2 charge, which means it holds its electrons more tightly than N^(3–).
- **Na^(+)**: The electronic configuration is 1s² 2s² 2p⁶ (10 electrons). It has 11 protons (Na) and a +1 charge, which means it holds its electrons even more tightly than both N^(3–) and O^(–2).

**Conclusion for Triad I**: The species with the lowest ionization potential is **N^(3–)** because it has the least positive charge and thus holds its electrons the least tightly.

**Step 2: Analyze Triad II `[N^(+), C^(+), O^(+)]`**
- We need to find the ionization potential of each species.
- **N^(+)**: The electronic configuration is 1s² 2s² 2p² (4 valence electrons). It has 7 protons and a +1 charge.
- **C^(+)**: The electronic configuration is 1s² 2s² 2p¹ (3 valence electrons). It has 6 protons and a +1 charge.
- **O^(+)**: The electronic configuration is 1s² 2s² 2p³ (5 valence electrons). It has 8 protons and a +1 charge.

**Conclusion for Triad II**: The species with the highest ionization potential is **O^(+)** because it has a half-filled p subshell (2p³), which is more stable and requires more energy to remove an electron.

### Final Answer:
- The species with the lowest ionization potential from Triad I is **N^(3–)**.
- The species with the highest ionization potential from Triad II is **O^(+)**.