Identify two ions that have the following ground-state electron configurations: (c) [Kr]5s²4d¹⁰

Verified step by step guidance

1. Identify the given electron configuration: [Kr]5s^2 4d^10.
2. Recognize that this configuration corresponds to a filled 4d subshell and a filled 5s subshell, which is characteristic of a transition metal ion.
3. Determine the element with this electron configuration in its neutral state. The configuration [Kr]5s^2 4d^10 corresponds to Cadmium (Cd) in its neutral state.
4. Consider the possible ions that can be formed by removing electrons from the outermost shell. For Cadmium, the common ion is Cd^2+.
5. Identify another ion with the same electron configuration. Silver (Ag) can lose one electron to form Ag^+ with the same electron configuration as Cd^2+.

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, the notation [Kr]5s²4d¹⁰ indicates that the atom has a core configuration similar to krypton, with additional electrons in the 5s and 4d orbitals.

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 identifying ions based on their electron configurations.

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. They typically have partially filled d orbitals, which play a crucial role in their chemical behavior. The electron configuration [Kr]5s²4d¹⁰ suggests that the ions in question may be derived from transition metals, which often exhibit complex electron arrangements.