The electron configuration of a carbon atom is 1s² 2s² 2p².
Understanding Carbon's Electron Configuration
Carbon, with an atomic number of 6, possesses 6 protons, 6 neutrons, and 6 electrons in its neutral state. The electron configuration describes the arrangement of these 6 electrons within the atom's electron shells and subshells.
Shells and Subshells
- Shells: Electrons occupy different energy levels or shells around the nucleus, labeled as n=1, 2, 3, etc. The first shell (n=1) is closest to the nucleus and has the lowest energy.
- Subshells: Each shell consists of one or more subshells, denoted as s, p, d, and f. Each subshell has a characteristic shape and energy level.
- The s subshell is spherical and can hold up to 2 electrons.
- The p subshell is dumbbell-shaped and can hold up to 6 electrons.
Aufbau Principle
The Aufbau principle dictates the order in which electrons fill the orbitals: electrons first occupy the lowest energy levels available to them. The order is generally: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, and so on.
Carbon's Electron Configuration Explained
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1s²: The first two electrons fill the 1s subshell, which is the lowest energy level.
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2s²: The next two electrons fill the 2s subshell.
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2p²: The final two electrons enter the 2p subshell. Since the p subshell can hold up to 6 electrons, these two electrons each occupy a separate p orbital (according to Hund's rule, which states that electrons will individually occupy each orbital within a subshell before doubling up in any one orbital).
Therefore, the complete electron configuration for carbon is 1s² 2s² 2p².
