Question

electron configuration practice chemistry h. determine which of the following electron configurations are rule has been violated. 16) 1s²2s²2p⁶3s²3p⁶4s²4d¹⁰4p⁵ 17) 1s²2s²2p⁶3s³3d⁵ 18) ra 7s²5f⁸ 19) kr 5s²4d¹⁰5p⁵ 20) xe

Explanation:

Step1: Recall electron - filling rules

Electrons fill orbitals in the order of increasing energy (Aufbau principle), with a maximum of 2 electrons per orbital (Pauli - exclusion principle) and parallel spins in degenerate orbitals (Hund's rule). Also, s - subshells can hold a maximum of 2 electrons, p - subshells 6, d - subshells 10, and f - subshells 14.

Step2: Analyze 16) $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}4d^{10}4p^{5}$

The 4d orbitals should not fill before the 3d orbitals. Violation of the Aufbau principle.

Step3: Analyze 17) $1s^{2}2s^{2}2p^{6}3s^{3}3d^{5}$

The 3s subshell can hold a maximum of 2 electrons. Violation of the Pauli - exclusion principle.

Step4: Analyze 18) $[Ra]7s^{2}5f^{8}$

This is a valid electron configuration following all rules. No violation.

Step5: Analyze 19) $[Kr]5s^{2}4d^{10}5p^{5}$

This is a valid electron configuration following all rules. No violation.

Step6: Analyze 20) $[Xe]$

This is just a noble - gas core notation and not a complete electron configuration on its own. But assuming no further context, no rule violation in terms of filling rules for the given part.

Answer:

1. Aufbau principle
2. Pauli - exclusion principle
3. No violation
4. No violation
5. No violation (assuming no further context about incomplete configuration being a violation)