Question

The electronic configuration of chlorine is

• A. \([Ne]\,3s^2\,3p^2\)
• B. \([Ne]\,3s^2\,3p^3\)
• C. \([Ne]\,3s^2\,3p^4\)
• D. \([Ne]\,3s^2\,3p^5\)

Hint:

Chlorine has atomic number 17, so its valence shell configuration becomes: \[ 3s^2\,3p^5 \]

Answer 1

The Correct Option is D

Concept:
Chlorine has atomic number: \[ 17 \] This means chlorine contains 17 electrons. Electronic configuration is written according to the Aufbau principle, where electrons fill lower energy orbitals first.

Step 1: Filling electrons into orbitals systematically.
The orbital filling order is: \[ 1s,\ 2s,\ 2p,\ 3s,\ 3p \] Now filling 17 electrons: \[ 1s^2 \] \[ 2s^2 \] \[ 2p^6 \] \[ 3s^2 \] Total electrons filled so far: \[ 2+2+6+2 = 12 \] Remaining electrons: \[ 17-12 = 5 \] Thus, \[ 3p^5 \]

Step 2: Writing the final electronic configuration.
Therefore, \[ 1s^2\,2s^2\,2p^6\,3s^2\,3p^5 \] Using noble gas notation: \[ \boxed{[Ne]\,3s^2\,3p^5} \] Hence, the correct option is: \[ \boxed{(4)\ [Ne]\,3s^2\,3p^5} \]