Identify two ions that have the following ground-state electron configurations: (b) [Ar]3d⁵

Verified step by step guidance

1. Identify the neutral atom with the given electron configuration.
2. Recognize that the configuration [Ar]3d^5 corresponds to the element Manganese (Mn) in its neutral state.
3. Determine the possible ions by adding or removing electrons from the neutral atom.
4. Consider the removal of electrons to form a cation: Mn^2+ is a common ion, which would have the configuration [Ar]3d^5 after losing two 4s electrons.
5. Consider the addition of electrons to form an anion: Technically, Mn does not commonly form anions, but if it did, adding electrons would fill the 3d orbitals further.

Key Concepts

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It is represented using a notation that indicates the energy levels and sublevels occupied by electrons. For example, [Ar]3d5 indicates that the electron configuration follows the argon core, with five electrons in the 3d subshell, which is crucial for identifying specific ions.

Ionic Charge

Ionic charge refers to the electrical charge that an atom or molecule acquires when it loses or gains electrons. Cations are positively charged ions formed by losing electrons, while anions are negatively charged ions formed by gaining electrons. Understanding the ionic charge is essential for determining which ions correspond to a given electron configuration.

Transition Metals

Transition metals are elements found in the d-block of the periodic table, characterized by their ability to form variable oxidation states and colored compounds. The electron configuration [Ar]3d5 corresponds to a half-filled d subshell, which is a stable configuration often seen in transition metal ions like Mn2+ and Cr3+. Recognizing these elements helps in identifying the ions with the specified electron configuration.