Silicon resembles `B` due to

Options

A. Similar values of atomic radii
B. Similar values of `EN`
C. Similar values of `IE`
D. All of the above

Answer

To answer the question "Silicon resembles B due to", we will break down the reasoning step by step.

### Step-by-Step Solution:

1. **Identify the Elements**:
- We are comparing Silicon (Si) and Boron (B).
- Boron is in Group 13 of the periodic table, while Silicon is in Group 14.

2. **Determine Their Periods**:
- Boron is located in the second period of the periodic table.
- Silicon is located in the third period.

3. **Consider the Diagonal Relationship**:
- Silicon and Boron exhibit a diagonal relationship in the periodic table. This relationship often leads to similarities in properties between elements that are not in the same group but are close to each other in the periodic table.

4. **Compare Atomic Size**:
- Both Silicon and Boron have similar atomic sizes. The atomic radius of Silicon is comparable to that of Boron, which is significant because similar atomic sizes often lead to similar chemical behavior.

5. **Analyze Ionization Energy**:
- Ionization energy is inversely proportional to atomic size. Since Silicon and Boron have similar atomic sizes, they also have comparable ionization energies.

6. **Evaluate Electronegativity**:
- Electronegativity is directly related to ionization energy. Because Silicon and Boron have similar ionization energies, they also exhibit similar electronegativity values.

7. **Conclusion**:
- Given that Silicon and Boron share similarities in atomic size, ionization energy, and electronegativity, we can conclude that Silicon resembles Boron due to these shared properties.

### Final Answer:
Silicon resembles Boron due to similar atomic size, ionization energy, and electronegativity.