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Chapter 21: Problem 37

Give formulas for the following. a. potassium tetrachlorocobaltate(II) b. aquatricarbonylplatinum(II) bromide c. sodium dicyanobis(oxalato)ferrate(III) d. triamminechloroethylenediaminechromium(III) iodide

Short Answer

Expert verified
The chemical formulas for the given compounds are: a. \(K_2[CoCl_4]\) b. \([Pt(CO)_3(H_2O)]Br_2\) c. \(Na_3[Fe(CN)_2(C_2O_4)_2]\) d. \([Cr(NH_3)_3Cl(en)]I_3\)

Step by step solution

01

Identify the cation and anion

The cation in this compound is potassium (K^+), and the anion is tetrachlorocobaltate(II) (Co^2+ with four chloride ions, Cl^-).
02

Write the chemical formula

To balance the charges, we need two potassium ions for each tetrachlorocobaltate ion. The resulting chemical formula is \(K_2[CoCl_4]\). b. aquatricarbonylplatinum(II) bromide:
03

Identify the cation and anion

The cation in this compound is aquatricarbonylplatinum(II) (Pt^2+ with three CO ligands and one H2O ligand) and the anion is bromide (Br^-).
04

Write the chemical formula

To balance the charges, we need one bromide ion for each aquatricarbonylplatinum ion. The resulting chemical formula is \([Pt(CO)_3(H_2O)]Br_2\). c. sodium dicyanobis(oxalato)ferrate(III):
05

Identify the cation and anion

The cation in this compound is sodium (Na^+) and the anion is dicyanobis(oxalato)ferrate(III) (Fe^3+ with two CN ligands and two oxalate ligands C2O4^2-).
06

Write the chemical formula

To balance the charges, we need three sodium ions for each dicyanobis(oxalato)ferrate ion. The resulting chemical formula is \(Na_3[Fe(CN)_2(C_2O_4)_2]\). d. triamminechloroethylenediaminechromium(III) iodide:
07

Identify the cation and anion

The cation in this compound is triamminechloroethylenediaminechromium(III) (Cr^3+ with three NH3 ligands, one Cl^- ligand and one ethylenediamine ligand (en)) and the anion is iodide (I^-).
08

Write the chemical formula

To balance the charges, we need three iodide ions for each cationic complex ion. The resulting chemical formula is \([Cr(NH_3)_3Cl(en)]I_3\).

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Most popular questions from this chapter

Use standard reduction potentials to calculate \(\mathscr{E}^{\circ}, \Delta G^{\circ}\), and \(K\) (at \(298 \mathrm{~K}\) ) for the reaction that is used in production of gold: $$2 \mathrm{Au}(\mathrm{CN})_{2}^{-}(a q)+\mathrm{Zn}(s) \longrightarrow 2 \mathrm{Au}(s)+\mathrm{Zn}(\mathrm{CN})_{4}^{2-}(a q)$$ The relevant half-reactions are $$\begin{aligned}\mathrm{Au}(\mathrm{CN})_{2}^{-}+\mathrm{e}^{-} \longrightarrow \mathrm{Au}+2 \mathrm{CN}^{-} & \mathscr{C}^{\circ} &=-0.60 \mathrm{~V} \\ \mathrm{Zn}(\mathrm{CN})_{4}^{2-}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Zn}+4 \mathrm{CN}^{-} & \mathscr{E}^{\circ} &=-1.26 \mathrm{~V} \end{aligned}$$

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

Name the following coordination compounds. a. \(\mathrm{Na}_{4}\left[\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) b. \(\mathrm{K}_{2}\left[\mathrm{CoCl}_{4}\right]\) c. \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\) d. \(\left[\mathrm{Co}(\mathrm{en})_{2}(\mathrm{SCN}) \mathrm{Cl}\right] \mathrm{Cl}\)

Silver is sometimes found in nature as large nuggets; more often it is found mixed with other metals and their ores. Cyanide ion is often used to extract the silver by the following reaction that occurs in basic solution: $$\mathrm{Ag}(s)+\mathrm{CN}^{-}(a q)+\mathrm{O}_{2}(g) \stackrel{\text { Basis }}{\longrightarrow} \mathrm{Ag}(\mathrm{CN})_{2}^{-}(a q)$$ Balance this equation by using the half-reaction method.

. Which is more likely to be paramagnetic, \(\mathrm{Fe}(\mathrm{CN})_{6}^{4-}\) or \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{2+}\) ? Explain.
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