Which of the following represent electron configuration that...

Which of the following represent electron configuration that violate the Pauli exclusion principle? I. $[\mathrm{Ne}] 3 \mathrm{~s}^{1} 3 \mathrm{p}^{5}$ II. $[\mathrm{Kr}] 4 \mathrm{~d}^{12} 5 \mathrm{~s}^{2} 5 \mathrm{p}^{3}$ III. $[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{2} 4 \mathrm{p}^{2}$ a. Only (II) b. Only (I) c. Both (I) and (III) d. Both (II) and (III)

Which of the following represent electron configuration that violate the Pauli exclusion principle?
I. $[\mathrm{Ne}] 3 \mathrm{~s}^{1} 3 \mathrm{p}^{5}$
II. $[\mathrm{Kr}] 4 \mathrm{~d}^{12} 5 \mathrm{~s}^{2} 5 \mathrm{p}^{3}$
III. $[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{2} 4 \mathrm{p}^{2}$
a. Only (II)
b. Only (I)
c. Both (I) and (III)
d. Both (II) and (III)

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Key Concepts

Orbital Capacity

Orbital capacity refers to the maximum number of electrons that can occupy a specific type of orbital. For example, the s orbital can hold 2 electrons, the p orbital can hold 6, the d orbital can hold 10, and the f orbital can hold 14 electrons. Knowing these capacities is important for understanding how electrons are distributed among orbitals in accordance with the Pauli exclusion principle.

Electron Configuration

Electron configuration represents the systematic arrangement of electrons in the orbitals of an atom based on energy levels and subshells. This concept is essential in predicting the chemical behavior of elements, as electrons fill orbitals in a specific order according to rules such as the Aufbau principle, which dictates the order in which orbitals are occupied.

Pauli Exclusion Principle

This principle states that no two electrons within an atom can have the same set of four quantum numbers. In practical terms, it means that each orbital can hold a maximum of two electrons, and these electrons must have opposite spins. This rule is critical when assigning electrons to various orbitals to ensure that electron configurations are valid.

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