Write the electron configuration for each ion. c. K⁺

Verified step by step guidance

1. Identify the electron configuration of the neutral potassium (K) atom. Potassium has an atomic number of 19, so its electron configuration is \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^1\).
2. Recognize that \(K^+\) is a potassium ion that has lost one electron.
3. Remove one electron from the outermost shell of the neutral potassium atom to account for the positive charge.
4. The electron removed will be from the 4s orbital, as it is the highest energy level in the neutral potassium atom.
5. Write the electron configuration for \(K^+\) as \(1s^2 2s^2 2p^6 3s^2 3p^6\), which is the same as the electron configuration of argon (Ar), a noble gas.

Key Concepts

Electron Configuration

Electron configuration describes the distribution of electrons in an atom or ion's orbitals. It is represented using a notation that indicates the energy levels and sublevels occupied by electrons, following the Aufbau principle, Pauli exclusion principle, and Hund's rule. Understanding electron configuration is essential for predicting chemical behavior and bonding properties.

Ionic Charge

Ionic charge refers to the electrical charge that an atom or ion carries due to the loss or gain of electrons. For example, a potassium ion (K⁺) has a +1 charge, indicating it has lost one electron compared to its neutral state. This change in electron count directly affects the electron configuration, as the configuration must reflect the new number of electrons.

Potassium Ion (K⁺)

Potassium (K) is an alkali metal with an atomic number of 19, meaning it has 19 electrons in its neutral state. When it forms a K⁺ ion, it loses one electron, resulting in a total of 18 electrons. The electron configuration for K⁺ is thus 1s² 2s² 2p⁶ 3s², which can be simplified to [Ar] to denote the configuration of the nearest noble gas, argon.