Which of the following factor generally favours electrovalence

Options

A. Cation with pseudo inert gas configuration
B. High charge on ions
C. Large cation and small anion
D. Small cation and large anion

Answer

To determine which factor generally favors electrovalence (or ionic character) in chemical bonding, we can analyze the options provided based on the principles of ionic and covalent character in bonds.

### Step-by-Step Solution:

1. **Understanding Electrovalence**: Electrovalence refers to the ionic character of a bond. A bond with high ionic character is more electrovalent, while a bond with significant covalent character is less electrovalent.

2. **Factors Affecting Ionic and Covalent Character**:
- **Cation Size**: Smaller cations tend to have higher charge density, which increases their ability to polarize anions, leading to more covalent character.
- **Anion Size**: Larger anions can be more easily polarized by cations, which also tends to increase covalent character.
- **Charge on Ions**: Higher charges on ions increase the polarization of the bond, leading to more covalent character.

3. **Analyzing the Options**:
- **Option 1: Cation with pseudo-inert gas configuration**: This typically leads to covalent character due to the stability of the configuration, hence it does not favor electrovalence.
- **Option 2: High charge on the anions**: High charge on anions increases covalent character, thus does not favor electrovalence.
- **Option 3: Large size cation and small size anion**: This configuration favors electrovalence because the large cation has a lower charge density and the small anion can be polarized less, leading to increased ionic character.
- **Option 4: Small size cation and large size anion**: This configuration favors covalent character due to the high charge density of the small cation and the polarizability of the large anion.

4. **Conclusion**: The option that favors electrovalence is **Option 3: Large size cation and small size anion**.

### Final Answer:
**Large size cation and small size anion favors electrovalence.**

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