Which of these statements is true?

Options

A. The lowest ionization energy in group 14 is possessed by Tin
B. The lowest electron affinity in group 16 is that of oxygen
C. In group 17 the highest value of electron gain enthalpy (Modulus) is possessed by Chlorine.
D. All of these are correct statements.

Answer

To determine which of the given statements is true, we will analyze each statement one by one based on periodic trends and properties.

### Step-by-Step Solution:

1. **Analyze Statement 1: "The lowest ionization energy in group 14 is possessed by tin."**
- Group 14 elements include carbon (C), silicon (Si), germanium (Ge), tin (Sn), and lead (Pb).
- As we move down the group, the atomic size increases, leading to a decrease in ionization energy due to the increased distance of the outermost electrons from the nucleus.
- However, due to lanthanide contraction, the atomic size of lead (Pb) is smaller than expected, making its ionization energy slightly higher than that of tin (Sn).
- Therefore, this statement is **true**.

2. **Analyze Statement 2: "The lowest electron affinity in group 16 is that of oxygen."**
- Group 16 elements include oxygen (O), sulfur (S), selenium (Se), tellurium (Te), and polonium (Po).
- Electron affinity generally decreases down the group due to increasing atomic size and decreased effective nuclear charge.
- Oxygen has a small atomic size, which leads to significant electron-electron repulsion when an electron is added, resulting in a lower (less negative) electron affinity compared to sulfur.
- Thus, this statement is also **true**.

3. **Analyze Statement 3: "In group 17, the highest value of electron gain enthalpy is possessed by chlorine."**
- Group 17 elements (halogens) include fluorine (F), chlorine (Cl), bromine (Br), and iodine (I).
- Electron gain enthalpy is the energy released when an electron is added to a neutral atom.
- Fluorine, despite being highly electronegative, has a less negative electron gain enthalpy compared to chlorine due to its small size causing significant electron-electron repulsion.
- Chlorine, being larger, can accommodate an additional electron more easily, resulting in a more negative electron gain enthalpy.
- Therefore, this statement is **true**.

4. **Conclusion:**
- All three statements are true. Therefore, the correct answer is that all of these statements are correct.

### Final Answer:
All of the statements provided are true.

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