Question

Which of the following is the electronic configuration of Lanthanide elements?

• A. (n - 2)f$^{14}$(n - 1) 5s$^2$ 4d$^0$ 4n$^2$
• B. (n - 2)f$^{14}$(n - 1) 4s$^2$ 4d$^{10}$ns$^2$
• C. (n - 2)f$^{14}$(n - 1) 4d$^0$ 1n$^0$ns$^2$
• D. (n - 2)d$^0$ 1n$^2$

Hint:

Lanthanides have electrons filling the 4f orbitals, and their configuration generally follows the pattern (n - 2)f$^{14}$.

Answer 1

The Correct Option is A

Step 1: Lanthanides electronic configuration.
Lanthanides are elements with atomic numbers from 58 to 71. These elements are characterized by filling the 4f orbitals. The general configuration for Lanthanide elements involves the (n - 2)f orbitals being filled after the (n - 1) 4s orbital.
Step 2: Apply the options.
- Option (A) gives the correct configuration where the 4f orbital is filled and the 4s orbital remains as the second shell of electrons.
Final Answer: \[ \boxed{\text{(n - 2)f}^{14}\text{(n - 1) 5s}^2\text{4d}^0\text{4n}^2} \]