Identify what is wrong with each electron configuration and...

Identify what is wrong with each electron configuration and write the correct ground state (or lowest energy) configuration based on the number of electrons. (a) $1 s^{3} 2 s^{3} 2 p^{9}$ (b) $1 s^{2} 2 s^{2} 2 p^{6} 2 d^{4}$ (c) $1 s^{2} 1 p^{5}$ (d) $1 s^{2} 2 s^{2} 2 p^{8} 3 s^{2} 3 p^{1}$

Identify what is wrong with each electron configuration and write the correct ground state (or lowest energy) configuration based on the number of electrons.
(a) $1 s^{3} 2 s^{3} 2 p^{9}$
(b) $1 s^{2} 2 s^{2} 2 p^{6} 2 d^{4}$
(c) $1 s^{2} 1 p^{5}$
(d) $1 s^{2} 2 s^{2} 2 p^{8} 3 s^{2} 3 p^{1}$

Key Concepts

Pauli Exclusion Principle

This principle states that no two electrons in an atom can have the same set of all four quantum numbers. As a consequence, each orbital can hold a maximum of two electrons, each with opposite spins. This rule is fundamental in determining the correct electron distribution among orbitals.

Aufbau Principle

This principle governs the order in which atomic orbitals are filled with electrons. Electrons are added to the lowest available energy orbitals first before proceeding to higher energy orbitals. This stepwise filling ensures that the atom is in its lowest energy, or ground state, and helps reveal mistakes when electrons are placed in orbitals inconsistent with increasing energy levels.

Electron Configuration

This concept describes the distribution of electrons among the atomic orbitals of an atom. It is based on quantum numbers that define the energy levels and shapes of orbitals and follows established rules for electron placement. Correct electron configurations ensure that electrons occupy available orbitals in a way that minimizes the energy of the atom, representing its ground state.

Orbital Capacities and Validity

Each atomic orbital has a maximum number of electrons it can contain: s orbitals can hold 2 electrons, p orbitals 6, d orbitals 10, and f orbitals 14. Additionally, not all orbitals exist at every principal energy level; for example, at n = 1 only s orbitals exist, and orbitals like '1p' or '2d' are not allowed. Recognizing these limits is crucial for identifying errors in electron configurations.

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