An element has atomic no. 16 It will belong to which period of the periodic table ?

Options

A. 2
B. 3
C. 4
D. 5

Explanation

To determine the period of an element with atomic number 16, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Atomic Number**: The atomic number of the element is given as 16. This number represents the total number of electrons in a neutral atom of the element.

2. **Determine the Electronic Configuration**: The electronic configuration describes how the electrons are distributed in the various energy levels (shells) around the nucleus. For atomic number 16, we can fill the electrons in the shells as follows:
- The first shell (K shell) can hold a maximum of 2 electrons.
- The second shell (L shell) can hold a maximum of 8 electrons.
- The third shell (M shell) can hold more electrons, but we will fill it according to the number of remaining electrons.

3. **Fill the Electrons in the Shells**:
- Fill the K shell: 2 electrons (total = 2)
- Fill the L shell: 8 electrons (total = 10)
- Remaining electrons to fill in the M shell: 16 - 10 = 6 electrons (total = 16)

Therefore, the electronic configuration of the element is:
- K: 2
- L: 8
- M: 6

4. **Count the Filled Shells**: The filled shells are K, L, and M. Since we have electrons in three different shells, we can conclude that the element belongs to the third period of the periodic table.

5. **Conclusion**: The element with atomic number 16 belongs to Period 3 of the periodic table.

### Final Answer:
The element with atomic number 16 belongs to Period 3 of the periodic table.

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