Write the condensed electron configuration for the nickel (III) ion and state if it is paramagnetic or diamagnetic.

• A. $\left\lbrack Ar\right\rbrack3d^7$; Diamagnetic
• B. $\left\lbrack Ar\right\rbrack3d^7$; Paramagnetic
• C. $\left\lbrack Ar\right\rbrack3d^8$; Paramagnetic
• D. $\left\lbrack Ar\right\rbrack3d^74s^1$; Paramagnetic

Answer: (B)

Verified step by step guidance

1. Identify the electron configuration of a neutral nickel atom. Nickel (Ni) has an atomic number of 28, so its electron configuration is [Ar]3d^8 4s^2.
2. Determine the electron configuration for the nickel (III) ion (Ni^3+). To form a Ni^3+ ion, three electrons are removed from the neutral atom. Electrons are typically removed from the outermost shell first, which means removing the 4s electrons before the 3d electrons.
3. Remove the two 4s electrons from the neutral nickel configuration: [Ar]3d^8 4s^2 becomes [Ar]3d^8.
4. Remove one more electron from the 3d subshell to account for the third electron removed: [Ar]3d^8 becomes [Ar]3d^7.
5. Determine if the Ni^3+ ion is paramagnetic or diamagnetic. Paramagnetic substances have unpaired electrons, while diamagnetic substances have all electrons paired. Since [Ar]3d^7 has unpaired electrons, the Ni^3+ ion is paramagnetic.