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Chapter 21: Problem 20

Write electron configurations for each of the following. a. \(\mathrm{Cr}, \mathrm{Cr}^{2+}, \mathrm{Cr}^{3+}\) b. \(\mathrm{Cu}, \mathrm{Cu}^{+}, \mathrm{Cu}^{2+}\) c. \(\mathrm{V}, \mathrm{V}^{2+}, \mathrm{V}^{3+}\)

Short Answer

Expert verified
a. Cr: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}3d^{5}\), Cr²⁺: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{4}\), Cr³⁺: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{3}\) b. Cu: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}3d^{10}\), Cu⁺: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}\), Cu²⁺: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{9}\) c. V: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{3}\), V²⁺: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{2}\), V³⁺: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{1}\)

Step by step solution

01

Determine the atomic number of the element

The atomic number of Chromium (Cr) is 24.
02

Write the electron configuration for Cr

Using the periodic table and applying the rules, we find the electron configuration of Chromium to be: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}3d^{5}\]
03

Write the electron configuration for Cr²⁺

For the Cr²⁺ ion, we need to remove two electrons. The electron configuration becomes: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{4}\]
04

Write the electron configuration for Cr³⁺

For the Cr³⁺ ion, we need to remove three electrons. The electron configuration becomes: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{3}\] b. Cu, Cu⁺, Cu²⁺
05

Determine the atomic number of the element

The atomic number of Copper (Cu) is 29.
06

Write the electron configuration for Cu

Using the periodic table and applying the rules, we find the electron configuration of Copper to be: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}3d^{10}\]
07

Write the electron configuration for Cu⁺

For the Cu⁺ ion, we need to remove one electron. The electron configuration becomes: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}\]
08

Write the electron configuration for Cu²⁺

For the Cu²⁺ ion, we need to remove two electrons. The electron configuration becomes: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{9}\] c. V, V²⁺, V³⁺
09

Determine the atomic number of the element

The atomic number of Vanadium (V) is 23.
10

Write the electron configuration for V

Using the periodic table and applying the rules, we find the electron configuration of Vanadium to be: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{3}\]
11

Write the electron configuration for V²⁺

For the V²⁺ ion, we need to remove two electrons. The electron configuration becomes: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{2}\]
12

Write the electron configuration for V³⁺

For the V³⁺ ion, we need to remove three electrons. The electron configuration becomes: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{1}\]

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Most popular questions from this chapter

Almost all metals in nature are found as ionic compounds in ores instead of being in the pure state. Why? What must be done to a sample of ore to obtain a metal substance that has desirable properties?

What is the lanthanide contraction? How does the lanthanide contraction affect the properties of the \(4 d\) and \(5 d\) transition metals?

The following statements discuss some coordination compounds. For each coordination compound, give the complex ion and the counterions, the electron configuration of the transition metal, and the geometry of the complex ion. a. \(\mathrm{CoCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) is a compound used in novelty devices that predict rain. b. During the developing process of black-and-white film, silver bromide is removed from photographic film by the fixer. The major component of the fixer is sodium thiosulfate. The equation for the reaction is: \(\operatorname{AgBr}(s)+2 \mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}(a q) \longrightarrow \mathrm{Na}_{3}\left[\mathrm{Ag}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}\right](a q)+\mathrm{NaBr}(a q)\) c. In the production of printed circuit boards for the electronics industry, a thin layer of copper is laminated onto an insulating plastic board. Next, a circuit pattern made of a chemically resistant polymer is printed on the board. The unwanted copper is removed by chemical etching, and the protective polymer is finally removed by solvents. One etching reaction is: \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}(a q)+4 \mathrm{NH}_{3}(a q)+\mathrm{Cu}(s) \longrightarrow 2 \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}(a q)\) Assume these copper complex ions have tetrahedral geometry.

Write electron configurations for the following metals. a. \(\mathrm{Ni}\) b. \(\mathrm{Cd}\) c. \(\mathrm{Zr}\) d. \(\mathrm{Os}\)

Draw geometrical isomers of each of the following complex ions. a. \(\left[\mathrm{Co}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]^{-}\) c. \(\left[\operatorname{Ir}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3}\right]\) b. \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{2}\right]^{2+}\) d. \(\left[\mathrm{Cr}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2} \mathrm{I}_{2}\right]^{+}\)
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