For each ion, identify the neutral atom that is isoelectronic with it.
a. Cl−
b. Sc3+
c. Fe2+
d. Zn2+
e.Sn4+

Verified step by step guidance

1. Identify the number of electrons in each ion.
2. Determine the number of electrons in the neutral atom by adding or subtracting electrons based on the ion's charge.
3. For Cl^−, add one electron to the atomic number of Cl to find the isoelectronic neutral atom.
4. For Sc^3+, subtract three electrons from the atomic number of Sc to find the isoelectronic neutral atom.
5. Repeat the process for Fe^2+, Zn^2+, and Sn^4+ by adjusting the number of electrons according to their charges to find the isoelectronic neutral atoms.

Key Concepts

Isoelectronic Species

Isoelectronic species are atoms or ions that have the same number of electrons, resulting in identical electron configurations. This concept is crucial for identifying which neutral atom corresponds to a given ion, as it allows for the comparison of electron counts rather than atomic numbers.

Electron Configuration

Electron configuration describes the distribution of electrons among the various orbitals of an atom or ion. Understanding how to write and interpret electron configurations is essential for determining the number of electrons in an ion and finding the neutral atom that shares the same configuration.

Charge of Ions

The charge of an ion indicates the number of electrons lost or gained compared to its neutral atom. For example, a cation like Sc3+ has lost three electrons, while an anion like Cl− has gained one. Recognizing the charge helps in calculating the number of electrons in the ion, which is necessary for identifying the corresponding isoelectronic neutral atom.