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Chapter 21: Problem 84

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. \(\left[\mathrm{Co}(\mathrm{en})_{2}(\mathrm{SCN}) \mathrm{Cl}\right] \mathrm{Cl}\)

Short Answer

Expert verified
a. Tetrakis(oxalato)nickelate(II) sodium b. Potassium tetrachlorocobaltate(II) c. Tetraamminecopper(II) sulfate d. Pentaamminethiocyanato-κN-chlorocobalt(III) chloride

Step by step solution

01

Identify the central metal ion

Find the metal atom in each coordination complex as it will be the central metal ion. a. Ni (Nickel) b. Co (Cobalt) c. Cu (Copper) d. Co (Cobalt)
02

Identify the ligands

Determine the ligands surrounding the central metal ion in each coordination complex. a. \(C_{2}O_{4}\) (Oxalate) b. Cl (Chloride) c. \(NH_{3}\) (Ammine) d. en (Ethylenediamine), SCN (Thiocyanate), Cl (Chloride)
03

Determine the charge on the coordination complex

Calculate the overall charge on each coordination complex. a. Charge on \(Na_{4}\) = +4, therefore charge on the complex = -4 b. Charge on \(K_{2}\) = +2, therefore charge on the complex = -2 c. Charge on \(SO_{4}\) = -2, therefore charge on the complex = +2 d. Charge on \(Cl\) = -1, therefore charge on the complex = +1
04

Name the coordination complex using the standard nomenclature rules

Name each coordination complex following IUPAC nomenclature rules. a. Tetrakis(oxalato)nickelate(II) sodium b. Potassium tetrachlorocobaltate(II) c. Tetraamminecopper(II) sulfate d. Pentaamminethiocyanato-κN-chlorocobalt(III) chloride So, the names of the coordination complexes are: a. Tetrakis(oxalato)nickelate(II) sodium b. Potassium tetrachlorocobaltate(II) c. Tetraamminecopper(II) sulfate d. Pentaamminethiocyanato-κN-chlorocobalt(III) chloride

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Most popular questions from this chapter

The ferrate ion, \(\mathrm{FeO}_{4}{ }^{2-}\), is such a powerful oxidizing agent that in acidic solution, aqueous ammonia is reduced to elemental nitrogen along with the formation of the iron(III) ion. a. What is the oxidation state of iron in \(\mathrm{FeO}_{4}{ }^{2-}\), and what is the electron configuration of iron in this polyatomic ion? b. If \(25.0 \mathrm{~mL}\) of a \(0.243 \mathrm{M} \mathrm{FeO}_{4}^{2-}\) solution is allowed to react with \(55.0 \mathrm{~mL}\) of \(1.45 M\) aqueous ammonia, what volume of nitrogen gas can form at \(25^{\circ} \mathrm{C}\) and \(1.50 \mathrm{~atm}\) ?

A coordination compound of cobalt(III) contains four ammonia molecules, one sulfate ion, and one chloride ion. Addition of aqueous \(\mathrm{BaCl}_{2}\) solution to an aqueous solution of the compound gives no precipitate. Addition of aqueous \(\mathrm{AgNO}_{3}\) to an aqueous solution of the compound produces a white precipitate. Propose a structure for this coordination compound.

Compounds of copper(II) are generally colored, but compounds of copper(I) are not. Explain. Would you expect \(\mathrm{Cd}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\) to be colored? Explain.

Sketch a \(d\) -orbital energy diagram for the following. a. a linear complex with ligands on the \(x\) axis b. a linear complex with ligands on the \(y\) axis

A metal ion in a high-spin octahedral complex has two more unpaired electrons than the same ion does in a low-spin octahedral complex. Name some possible metal ions for which this would be true.
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