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Chapter 23: Problem 36

Write the formula for each of the following compounds, being sure to use brackets to indicate the coordination sphere: (a) hexaammineiron(II) nitrate (b) tetraaquadibromochromium(III) perchlorate (c) ammonium hexachloropalladate(IV) (d) diammineoxolatonickel(II) (e) Hexaamminemolybdenum(III) tetrachlorocuprate(II)

Short Answer

Expert verified
(a) \([Fe(NH3)_6] (NO3)_2\) (b) \([Cr(H2O)_4Br_2] (ClO4)_3\) (c) \((NH4)_2 [PdCl_6]\) (d) \([Ni(NH3)_2(C2O4)]\) (e) \([Mo(NH3)_6] [CuCl_4]_2\)

Step by step solution

01

Identify the components

In this compound, we have a central metal ion of iron (Fe) with an oxidation state of +2, the ligand is ammine (NH3) which has a coordination number of 6, and the counterion is nitrate (NO3^-).
02

Write the formula

Now we can write the formula as: \([Fe(NH3)_6] (NO3)_2\) (b) tetraaquadibromochromium(III) perchlorate
03

Identify the components

Here, we have a central metal ion of Chromium (Cr) with an oxidation state of +3, the ligands are aqua (H2O) with a coordination number of 4, and bromo (Br^-) with a coordination number of 2. The counterion is perchlorate (ClO4^-).
04

Write the formula

The formula for this compound is: \([Cr(H2O)_4Br_2] (ClO4)_3\) (c) ammonium hexachloropalladate(IV)
05

Identify the components

In this compound, the central metal ion is palladium (Pd) with an oxidation state of +4, the ligand is chloro (Cl^-) with a coordination number of 6, and the counterion is ammonium (NH4^+).
06

Write the formula

The formula for this compound is: \((NH4)_2 [PdCl_6]\) (d) diammineoxolatonickel(II)
07

Identify the components

Here, we have a central metal ion of nickel (Ni) with an oxidation state of +2, and the ligands are ammine (NH3) with a coordination number of 2, and oxolato (C2O4^2-) with a coordination number of 1.
08

Write the formula

The formula for this compound is: \([Ni(NH3)_2(C2O4)]\) (e) Hexaamminemolybdenum(III) tetrachlorocuprate(II)
09

Identify the components

In this compound, we have a central metal ion of molybdenum (Mo) with an oxidation state of +3, the ligand is ammine (NH3) with a coordination number of 6. The counterion is tetrachlorocuprate(II) \([CuCl_4]^{2-}\).
10

Write the formula

The formula for this compound is: \([Mo(NH3)_6] [CuCl_4]_2\)

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Most popular questions from this chapter

Indicate the coordination number and the oxidation number of the metal for each of the following complexes: (a) \(\mathrm{K}_{2} \mathrm{PtCl}_{4}\) (b) \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right] \mathrm{Br}_{2}\) (c) \(\mathrm{OsO}_{4}\) (d) \(\left[\mathrm{Mn}(\mathrm{en})_{3}\right]\left(\mathrm{NO}_{3}\right)_{2}\) (e) $\left[\mathrm{Cr}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{3}$ (f) \(\left[\mathrm{Zn}(\mathrm{bipy})_{2}\right]\left(\mathrm{ClO}_{4}\right)_{2}\)

Give the number of (valence) \(d\) electrons associated with the central metal ion in each of the following complexes: (a) $\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right] \mathrm{Cl}_{2},$, (b) $\mathrm{K}_{2}\left[\mathrm{Cu}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}\right]$, (c) \(\left[\mathrm{Os}(\mathrm{en})_{3}\right] \mathrm{Cl}_{3}\), (d) $[\mathrm{Cr}(\mathrm{EDTA})] \mathrm{SO}_{4},(\mathbf{e})\left[\mathrm{Cd}\left(\mathrm{H}_{2} ,\mathrm{O}\right)_{6}\right] \mathrm{Cl}_{2}$.

Draw the crystal-field energy-level diagrams and show the placement of \(d\) electrons for each of the following: (b) \(\left[\mathrm{Mn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\), (a) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (four unpaired electrons), (a high-spin complex), (c) $\left[\mathrm{Ru}\left(\mathrm{NH}_{3}\right)_{5}\left(\mathrm{H}_{2} \mathrm{O}\right)\right]^{2+}$ (a low-spin complex), (d) \(\left[\mathrm{IrCl}_{6}\right]^{2-}\) (a low-spin complex), (e) \(\left[\mathrm{Cr}(\mathrm{en})_{3}\right]^{3+}\), (f) \(\left[\mathrm{NiF}_{6}\right]^{4-}\).

The total concentration of \(\mathrm{Ca}^{2+}\) and \(\mathrm{Mg}^{2+}\) in a sample of hard water was determined by titrating a 0.100-L sample of the water with a solution of EDTA^{4-} \text { . The EDTA } ^ { 4 - } \text { chelates } the two cations: $$ \begin{aligned} \mathrm{Mg}^{2+}+[\mathrm{EDTA}]^{4-} & \longrightarrow[\mathrm{Mg}(\mathrm{EDTA})]^{2-} \\ \mathrm{Ca}^{2+}+[\mathrm{EDTA}]^{4-} & \longrightarrow[\mathrm{Ca}(\mathrm{EDTA})]^{2-} \end{aligned} $$ It requires \(31.5 \mathrm{~mL}\) of \(0.0104 \mathrm{M}\) [EDTA \(]^{4-}\) solution to reach the end point in the titration. A second 0.100 -L sample was then treated with sulfate ion to precipitate \(\mathrm{Ca}^{2+}\) as calcium sulfate. The \(\mathrm{Mg}^{2+}\) was then titrated with \(18.7 \mathrm{~mL}\) of 0.0104 \(M[\mathrm{EDTA}]^{4-}\). Calculate the concentrations of \(\mathrm{Mg}^{2+}\) and \(\mathrm{Ca}^{2+}\) in the hard water in \(\mathrm{mg} / \mathrm{L}\).

For each of the following molecules or polyatomic ions, draw the Lewis structure and indicate if it can act as a monodentate ligand, a bidentate ligand, or is unlikely to act as a ligand at all: (a) ethylamine, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{2}\), (b) trimethylphosphine, \(\mathrm{P}\left(\mathrm{CH}_{3}\right)_{3}\), (c) carbonate, \(\mathrm{CO}_{3}^{2-}\) (d) ethane, \(\mathrm{C}_{2} \mathrm{H}_{6}\).
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