A chemistry student drew the following incorrect electron configuration for carbon. (a) Correct the diagram.

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Understand the electron configuration of carbon: Carbon has an atomic number of 6, meaning it has 6 electrons. These electrons are distributed in orbitals according to the Aufbau principle, Hund's rule, and the Pauli exclusion principle.

Recall the order of orbital filling: Electrons fill orbitals in the order of increasing energy levels. For carbon, the order is 1s, 2s, and then 2p. The correct configuration should be written as:

1s^2 2s^2 2p^2

Apply Hund's rule for the 2p orbitals: When filling the 2p orbitals, electrons are placed in separate orbitals with parallel spins before pairing. This minimizes electron repulsion and stabilizes the atom.

Correct the diagram: Ensure that the 1s and 2s orbitals are fully filled with two electrons each, and the 2p orbitals have one electron in two separate orbitals with parallel spins.

Double-check the corrected diagram: Verify that the total number of electrons is 6, and that the configuration adheres to the principles of electron distribution (Aufbau principle, Hund's rule, and Pauli exclusion principle).

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주요 개념

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Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. For carbon, which has six electrons, the correct configuration is 1s² 2s² 2p². This notation indicates that two electrons occupy the 1s orbital, two occupy the 2s orbital, and two occupy the 2p orbitals, reflecting the principles of quantum mechanics.

Aufbau Principle

The Aufbau principle states that electrons fill atomic orbitals in order of increasing energy levels, starting from the lowest. This means that before electrons can occupy higher energy orbitals, such as 2p, the lower energy orbitals (1s and 2s) must be filled first. Understanding this principle is crucial for accurately determining the electron configuration of an element.

Pauli Exclusion Principle

The Pauli Exclusion Principle asserts that no two electrons in an atom can have the same set of four quantum numbers. This principle explains why each orbital can hold a maximum of two electrons with opposite spins. It is essential for understanding how electrons are arranged in orbitals and helps prevent incorrect configurations.