Select the correct statement `(s)`

Options

A. Alkali metals have lowest `IE` in respective period.
B. Noble gas have highest `IE` is respective period.
C. `EA_(1)` of `N lt EA_(1)` of `O`.
D. `F^(ɵ)` is the strongest reducing agent among halide ions.

Answer

To solve the question, we need to evaluate the given statements about alkali metals, noble gases, electron affinity, and halide ions. Here’s a step-by-step breakdown of the analysis:

### Step 1: Evaluate the first statement
**Statement:** Alkali metals have the lowest ionization energy in their respective periods.

**Analysis:**
- Alkali metals are located in Group 1 of the periodic table.
- As you move from left to right across a period, ionization energy increases due to increasing nuclear charge.
- Since alkali metals are on the far left, they indeed have the lowest ionization energy in their respective periods.

**Conclusion:** This statement is correct.

### Step 2: Evaluate the second statement
**Statement:** Noble gases have the highest ionization energy in their respective periods.

**Analysis:**
- Noble gases are located in Group 18 of the periodic table.
- They have a complete valence shell, making them very stable and requiring a significant amount of energy to remove an electron.
- Therefore, noble gases do have the highest ionization energy in their respective periods.

**Conclusion:** This statement is correct.

### Step 3: Evaluate the third statement
**Statement:** The electron affinity for nitrogen is less than the electron affinity for oxygen.

**Analysis:**
- Nitrogen (N) has a half-filled p subshell (2p3), which is relatively stable.
- Oxygen (O) has a p subshell that is not half-filled (2p4), making it less stable than nitrogen.
- Due to nitrogen's stability, it has a lower tendency to gain an electron compared to oxygen, which has a higher electron affinity.

**Conclusion:** This statement is correct.

### Step 4: Evaluate the fourth statement
**Statement:** F- is the strongest reducing agent among halide ions.

**Analysis:**
- Halide ions include F-, Cl-, Br-, and I-.
- The strength of a reducing agent is determined by its ability to lose electrons.
- Iodine (I-) is the least electronegative and thus the most willing to lose an electron, making it a stronger reducing agent than F-.
- Therefore, F- is not the strongest reducing agent among halide ions.

**Conclusion:** This statement is incorrect.

### Final Conclusion
The correct statements are:
- Statement 1: Correct
- Statement 2: Correct
- Statement 3: Correct
- Statement 4: Incorrect

Thus, the correct options are A, B, and C.

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