Final answer:
The electron configuration of an element is the arrangement of its electrons in shells and subshells. It can be determined based on the element's position on the periodic table. The principles and rules governing electron configuration include the Aufbau principle, Hund's rule, and the Pauli exclusion principle. Electron configuration varies across different elements based on their positions and the number of electrons they have. The electron configuration of an atom is significant in determining its chemical properties, reactivity, bonding behavior, and stability.
Step-by-step explanation:
The electron configuration of an element refers to the arrangement of the electrons in its shells and subshells. It can be determined by the element's position on the periodic table. For example, the electron configuration of Ge (Germanium) is 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p², and the electron configuration of C (Carbon) is 1s²2s²2p².
The principles and rules that govern electron configuration include the Aufbau principle, Hund's rule, and the Pauli exclusion principle. The Aufbau principle states that electrons occupy the lowest energy levels first, while Hund's rule states that electrons prefer to occupy separate orbitals before pairing up. The Pauli exclusion principle states that no two electrons in an atom can have the same set of quantum numbers.
Variations in electron configuration across different elements can be observed based on their positions and the number of electrons they have. Elements in the same group or period tend to have similar electron configurations, with variations due to the number of valence electrons and the filling of subshells.
The electron configuration of an atom plays a significant role in determining its chemical properties. It affects the atom's reactivity, bonding behavior, and ability to gain or lose electrons. For example, noble gases have full outer electron shells, making them stable and nonreactive, while elements with partially filled or empty outer electron shells tend to form bonds to achieve a more stable configuration.