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Chapter 23: Problem 13

For each of the following compounds, determine the electron configuration of the transition-metal ion. (a) CuO, (b) \(\mathrm{Cu}_{2} \mathrm{O}\) (c) \(\mathrm{V}_{2} \mathrm{O}_{5}\) (d) \(\mathrm{MnO}\).

Short Answer

Expert verified
The electron configurations of the transition-metal ions in the given compounds are as follows: a) CuO: Cu\(^{2+}\) has an electron configuration of \([Ar] 3d^9\). b) \(\mathrm{Cu}_{2}\mathrm{O}\): Cu\(^{+}\) has an electron configuration of \([Ar] 3d^{10}\). c) \(\mathrm{V}_{2}\mathrm{O}_{5}\): V\(^{5+}\) has an electron configuration of \([Ar] 3d^0\). d) \(\mathrm{MnO}\): Mn\(^{2+}\) has an electron configuration of \([Ar] 3d^5\).

Step by step solution

01

Identify the transition-metal ion and its oxidation state

In this compound, the transition-metal ion is copper (Cu). Oxygen usually has an oxidation state of -2. Since there's only one Cu atom, its oxidation state must be +2 to balance the overall charge of the compound.
02

Determine the electron configuration of Cu\(^{2+}\)

The electron configuration of a neutral Cu atom is \([Ar] 3d^{10} 4s^1\). Removing two electrons from the outer shell (4s) and one from the inner shell (3d) gives the electron configuration of Cu\(^{2+}\): \([Ar] 3d^9\). #b) \(\mathrm{Cu}_{2}\mathrm{O}\)#
03

Identify the transition-metal ion and its oxidation state

In this compound, the transition-metal ion is still copper (Cu). Since there are two Cu atoms and one O atom, the overall oxidation state of the two Cu atoms must be +2 to balance the overall charge of the compound (since O has an oxidation state of -2). Therefore, each Cu atom will have an oxidation state of +1.
04

Determine the electron configuration of Cu\(^{+}\)

The electron configuration of a neutral Cu atom is \([Ar] 3d^{10} 4s^1\). Removing one electron from the outer shell (4s) gives the electron configuration of Cu\(^{+}\): \([Ar] 3d^{10}\). #c) \(\mathrm{V}_{2}\mathrm{O}_{5}\)#
05

Identify the transition-metal ion and its oxidation state

In this compound, the transition-metal ion is vanadium (V). Oxygen usually has an oxidation state of -2. Since there are five O atoms (each with an oxidation state of -2), the overall oxidation state of the two V atoms must be +10 (to balance the overall charge). Therefore, each V atom will have an oxidation state of +5.
06

Determine the electron configuration of V\(^{5+}\)

The electron configuration of a neutral V atom is \([Ar] 3d^3 4s^2\). Removing both electrons from the outer shell (4s) and three from the inner shell (3d) gives the electron configuration of V\(^{5+}\): \([Ar] 3d^0\). #d) \(\mathrm{MnO}\)#
07

Identify the transition-metal ion and its oxidation state

In this compound, the transition-metal ion is manganese (Mn). Oxygen usually has an oxidation state of -2. Since there's only one Mn atom, its oxidation state must be +2 to balance the overall charge of the compound.
08

Determine the electron configuration of Mn\(^{2+}\)

The electron configuration of a neutral Mn atom is \([Ar] 3d^5 4s^2\). Removing both electrons from the outer shell (4s) gives the electron configuration of Mn\(^{2+}\): \([Ar] 3d^5\).

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Most popular questions from this chapter

Solutions of $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+},\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ (both octahedral), and \(\left[\mathrm{CoCl}_{4}\right]^{2-}(\) tetrahedral) are colored. One is pink, one is blue, and one is yellow. Based on the spectrochemical series and remembering that the energy splitting in tetrahedral complexes is normally much less than that in octahedral ones, assign a color to each complex.

Consider an octahedral complex, \(\mathrm{MA}_{2} \mathrm{~B}_{4}\). How many geometric isomers are expected for this compound? Will any of the isomers be optically active? If so, which ones?

The complex \(\left[\mathrm{Mn}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\) contains five unpaired electrons. Sketch the energy-level diagram for the \(d\) orbitals, and indicate the placement of electrons for this complex ion. Is the ion a high-spin or a low-spin complex?

(a) Using Werner's definition of valence, which property is the same as oxidation number, primary valence or secondary valence? (b) What term do we normally use for the other type of valence? (c) Why can \(\mathrm{NH}_{3}\) serve as a ligand but \(\mathrm{BH}_{3}\) cannot?

Consider the following three complexes: \(\left(\right.\) Complex 1) $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{SCN}\right]^{2+}$ \(\left(\right.\) Complex 2) $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3}\right]^{2+}$ \(\left(\right.\) Complex 3) \(\mathrm{CoClBr} \cdot 5 \mathrm{NH}_{3}\) Which of the three complexes can have (a) geometric isomers, (b) linkage isomers, (c) optical isomers, (d) coordination-sphere isomers?
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