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Chapter 18: Problem 1

Write the electronic configurations for the following. (a) \(\mathrm{Fe}^{3+}\) (b) \(\mathrm{Co}^{+}\) (c) \(\mathrm{Mn}^{4+}\) (d) \(\mathrm{Ni}^{2+}\)

Short Answer

Expert verified
The electronic configurations for these ions are: (a) \( \mathrm{Fe}^{3+} : 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s² \), (b) \( \mathrm{Co}^{+} : 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁷ 4s² \), (c) \( \mathrm{Mn}^{4+} : 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ \), (d) \( \mathrm{Ni}^{2+} : 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁸ \).

Step by step solution

01

Identify the neutral atom's atomic number

Look up each ion on the periodic table to find its atomic number, which equals the number of electrons in a neutral atom. For example, Fe (Iron) has an atomic number of 26, meaning a neutral iron atom has 26 electrons.
02

Adjust for ion charge

An ion's charge tells you how many electrons have been lost or gained. A positive charge indicates lost electrons; a negative charge indicates gained electrons. So, Fe^3+ has lost 3 electrons, meaning that it has \(26 - 3 = 23\) electrons.
03

Write the electronic configuration

Starting with the energy level 1s, list the orbitals in the order they are filled: 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p. Stop when you have accounted for all the electrons. The electronic configuration for Fe^3+ is then 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s².
04

Repeat the process for the other ions

Repeat this three-step process for the other ions: Co^+, Mn^4+, and Ni^2+.

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Most popular questions from this chapter

How do transition elements differ from \(s\) and \(p\) -block elements.

Explain the following: (a) Transition elements form alloys. (b) Transition metals are usually hard solids but mercury exists as liquid at room temperature. (c) \(\mathrm{VCl}_{5}\) doesn't exist but \(\mathrm{VF}_{5}\) exists. (d) What are the characteristic properties of transition elements?

What are the characteristic properties of transition elements?

Account for the statement: Zinc, cadmium and mercury are not strictly transition elements.

Give reasons for the following (a) \(\mathrm{Mn}^{2+}\) shows the maximum magnetic character among the divalent ions of \(3 d\) -transition series. (b) \(\mathrm{Cu}^{+}\) is diamagnetic but \(\mathrm{Cu}^{2+}\) is paramagnetic. (c) Transition metals have high electrode potential but they are not good reducing agents. (d) Alkali metals are more reactive than transition metals
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