The oxidation state shown by silicon when it combines with strongly electropositive metals is

Options

A. `-2`
B. `-4`
C. `+4`
D. `-2`

Explanation

To determine the oxidation state of silicon when it combines with strongly electropositive metals, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Atomic Structure of Silicon**:
- Silicon (Si) has an atomic number of 14, which means it has 14 electrons. Its electron configuration is 1s² 2s² 2p⁶ 3s² 3p².

2. **Determine the Valence Electrons**:
- The valence electrons of silicon are in the 3s and 3p orbitals. Specifically, silicon has 2 electrons in the 3s orbital and 2 electrons in the 3p orbital, giving it a total of 4 valence electrons.

3. **Understand the Behavior with Electropositive Metals**:
- Electropositive metals (like sodium and potassium) tend to lose electrons easily and can donate electrons to nonmetals or metalloids like silicon. When silicon combines with these metals, it can accept electrons.

4. **Calculate the Maximum Electrons Silicon Can Accept**:
- Silicon can accept up to 4 electrons (2 from the 3s and 2 from the 3p orbitals).

5. **Determine the Charge on Silicon**:
- When silicon accepts 4 electrons, it gains a charge of -4 (since gaining electrons results in a negative charge).

6. **Conclude the Oxidation State**:
- The oxidation state of silicon when it combines with strongly electropositive metals is -4.

### Final Answer:
The oxidation state shown by silicon when it combines with strongly electropositive metals is -4.

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