Element X has atomic number 12 and Y has atomic number 16. The period to which these elements belong and the type of bond, they form are respectively

Options

A. Second period and ionic bond
B. Third period and covalent bond
C. Third period and ionic bond
D. Second period and covalent bond

Explanation

To solve the question regarding elements X and Y, we need to determine the period they belong to and the type of bond they form based on their atomic numbers.

### Step-by-Step Solution:

1. **Identify the Elements:**
- Element X has an atomic number of 12.
- Element Y has an atomic number of 16.

2. **Determine the Electronic Configuration:**
- For Element X (Atomic number 12):
- The electronic configuration is:
- 1st shell: 2 electrons
- 2nd shell: 8 electrons
- 3rd shell: 2 electrons
- Therefore, the configuration is 2, 8, 2.

- For Element Y (Atomic number 16):
- The electronic configuration is:
- 1st shell: 2 electrons
- 2nd shell: 8 electrons
- 3rd shell: 6 electrons
- Therefore, the configuration is 2, 8, 6.

3. **Determine the Period:**
- Both elements have their outermost electrons in the third shell.
- Thus, both Element X and Element Y belong to **Period 3**.

4. **Determine the Type of Bond Formed:**
- Element X (with 2 electrons in the outer shell) tends to lose these 2 electrons to achieve a stable configuration (like Neon).
- Element Y (with 6 electrons in the outer shell) tends to gain 2 electrons to achieve a stable configuration (also like Neon).
- When Element X loses 2 electrons, it becomes X²⁺.
- When Element Y gains 2 electrons, it becomes Y²⁻.
- The transfer of electrons from X to Y indicates that they form an **ionic bond**.

### Final Answer:
- The period to which these elements belong is **Period 3**.
- The type of bond they form is an **ionic bond**.