(a) Write out the ground-state electron configuration (1 s^2, 2 s^2, …) for the carbon atom. (b)

step 1 So we have the carbon has the atomic number is 6. Then atomic number carbon is 6. Then we have 6

(a) Write out the ground-state electron configuration (1...

(a) Write out the ground-state electron configuration $\left(1 s^{2}, 2 s^{2}, \ldots\right)$ for the carbon atom. (b) What element of next-larger $Z$ has chemical properties similar to those of carbon? Give the groundstate electron configuration for this element.

Key Concepts

Ground-State Electron Configuration

This concept refers to the arrangement of electrons in the orbitals of an atom when it is in its lowest energy state. It follows the rules such as the Aufbau principle, which dictates the order in which orbitals are filled, as well as the Pauli exclusion principle and Hund's rule. Understanding the ground-state electron configuration is crucial for predicting how atoms behave chemically and how they interact with other atoms.

Aufbau Principle

The Aufbau principle is the guideline that electrons fill atomic orbitals in order of increasing energy. This means that lower-energy orbitals are populated before electrons move into higher-energy ones. This principle is central to constructing the electron configuration of atoms systematically and understanding periodic trends.

Periodic Trends and Group Similarity

Elements that are positioned in the same column (group) of the periodic table share similar valence electron configurations, which leads them to exhibit similar chemical properties. Being able to identify which element is in the same group as another, based on its electron configuration, is key in predicting chemical behavior across different elements.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom and are responsible for its chemical reactivity and bonding characteristics. By analyzing the configuration of valence electrons, one can determine an element's position in the periodic table and its potential chemical similarities with other elements in the same group.

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