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Chapter 20: Problem 5

Write the electron configurations of these ions: \(\mathrm{V}^{5+}\) \(\mathrm{Cr}^{3+}, \mathrm{Mn}^{2+}, \mathrm{Fe}^{3+}, \mathrm{Cu}^{2+}, \mathrm{Sc}^{3+}, \mathrm{T}_{1}^{4+}\)

Short Answer

Expert verified
The electron configurations are \( \mathrm{V}^{5+} = [Ar] \), \( \mathrm{Cr}^{3+} = [Ar]3d^3 \), \( \mathrm{Mn}^{2+} = [Ar]3d^5 \), \( \mathrm{Fe}^{3+} = [Ar]3d^5 \), \( \mathrm{Cu}^{2+} = [Ar]3d^9 \), \( \mathrm{Sc}^{3+} = [Ar] \), \( \mathrm{T}_{1}^{4+} = [Xe]4f^{14}5d^{10}6s^2 \).

Step by step solution

01

Electron Configuration of \( \mathrm{V}^{5+} \)

Vanadium (V) has an atomic number of 23, so its electron configuration is \( [Ar]4s^23d^3 \). As this ion is +5, it means 5 electrons have been removed. Electrons are removed from highest energy level down, hence configuration of \( \mathrm{V}^{5+} \) is \( [Ar] \) as both 4s and 3d electrons have been removed.
02

Electron Configuration of \( \mathrm{Cr}^{3+} \)

Chromium (Cr) has an atomic number of 24, its unique electron configuration is \( [Ar]4s^13d^5 \). For \( \mathrm{Cr}^{3+} \), it means 3 electron has been removed. Hence, the configuration of \( \mathrm{Cr}^{3+} \) is \( [Ar]3d^3 \).
03

Electron Configuration of \( \mathrm{Mn}^{2+} \)

Manganese (Mn) has an atomic number of 25, so its electron configuration is \( [Ar]4s^23d^5 \). As \( \mathrm{Mn}^{2+} \), it means 2 electrons have been removed. Hence, the configuration of \( \mathrm{Mn}^{2+} \) is \( [Ar]3d^5 \).
04

Electron Configuration of \( \mathrm{Fe}^{3+} \)

Iron (Fe) has an atomic number 26, so its electron configuration is \( [Ar]4s^23d^6 \). As this ion is +3, it means 3 electrons have been removed. Hence, the configuration of \( \mathrm{Fe}^{3+} \) is \( [Ar]3d^5 \).
05

Electron Configuration of \( \mathrm{Cu}^{2+} \)

Copper (Cu) has an atomic number 29, its unique electron configuration is \( [Ar]4s^13d^{10} \). As \( \mathrm{Cu}^{2+} \), it means 2 electrons have been removed. Hence, the configuration of \( \mathrm{Cu}^{2+} \) is \( [Ar]3d^9 \).
06

Electron Configuration of \( \mathrm{Sc}^{3+} \)

Scandium (Sc) has an atomic number 21, so its electron configuration is \( [Ar]4s^23d^1 \). As \( \mathrm{Sc}^{3+} \), it means 3 electrons have been removed. Hence, all the electrons outside the Argon kernel have been removed and the configuration of \( \mathrm{Sc}^{3+} \) is \( [Ar] \).
07

Electron Configuration of \( \mathrm{T}_{1}^{4+} \)

Thallium (Tl) has an atomic number of 81, and its unique electron configuration is \( [Xe] 4f^{14} 5d^{10} 6s^2 6p^1 \). For \( \mathrm{T}_{1}^{4+} \), it means 4 electrons have been removed. Hence, the configuration of \( \mathrm{T}_{1}^{4+} \) is \( [Xe]4f^{14}5d^{10}6s^2 \).

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Most popular questions from this chapter

Predict the number of unpaired electrons in these complex ions: (a) \(\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]^{4-}(\mathrm{b})\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\)

Aqueous copper(II) sulfate solution is blue in color. When aqueous potassium fluoride is added, a green precipitate is formed. When aqueous potassium chloride is added instead, a bright-green solution is formed. Explain what is happening in these two cases.

A concentrated aqueous copper(II) chloride solution is bright green in color. When diluted with water, the solution becomes light blue. Explain.

Which of these hydrated cations are colorless: \(\mathrm{Fe}^{2+}(a q), \mathrm{Zn}^{2+}(a q), \mathrm{Cu}^{+}(a q), \mathrm{Cu}^{2+}(a q), \mathrm{V}^{5+}(a q)\) \(\mathrm{Ca}^{2+}(a q), \mathrm{Co}^{2+}(a q), \mathrm{Sc}^{3+}(a q), \mathrm{Pb}^{2+}(a q) ?\) Explain your choice.

Write the formulas for each of these ions and compounds: (a) tetrahydroxozincate(II), (b) pentaaquochlorochromium(III) chloride, (c) tetrabromocuprate(II), (d) ethylenediaminetetraacetatoferrate(II).
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