In which period of the periodic table, an element with atomic number 14 is placed ?

Options

A. 4
B. 3
C. 2
D. 1

Explanation

To determine the period of the periodic table in which an element with atomic number 14 is placed, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Atomic Number**: The atomic number given is 14. This means the element has 14 protons and, in a neutral atom, also 14 electrons.

2. **Write the Electronic Configuration**: We need to fill the electron orbitals according to the Aufbau principle. The order of filling is:
- 1s
- 2s
- 2p
- 3s
- 3p

3. **Fill the Orbitals**:
- **1s**: Can hold a maximum of 2 electrons. So, we fill 1s with 2 electrons.
- **2s**: Can also hold a maximum of 2 electrons. Fill 2s with 2 electrons.
- **2p**: Can hold a maximum of 6 electrons. Fill 2p with 6 electrons.
- **3s**: Can hold a maximum of 2 electrons. Fill 3s with 2 electrons.
- **3p**: Can hold a maximum of 6 electrons. Since we have already filled 12 electrons (2 from 1s, 2 from 2s, 6 from 2p, and 2 from 3s), we need to fill 2 more electrons in 3p.

Thus, the electronic configuration for the element with atomic number 14 is:
\[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^2 \]

4. **Determine the Valence Shell**: The outermost shell (valence shell) for the element is the third shell (n=3), which contains the electrons in the 3s and 3p orbitals.

5. **Identify the Period**: The period number corresponds to the highest principal quantum number (n) of the valence shell. In this case, since the valence shell is the third shell (n=3), the element with atomic number 14 is placed in the **third period** of the periodic table.

### Final Answer:
The element with atomic number 14 is placed in the **third period** of the periodic table.

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