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Chapter 21: Problem 34

Name the following complex ions. a. \(\mathrm{Ru}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}^{2+}\) b. \(\mathrm{Fe}(\mathrm{CN})_{6}{ }^{4-}\) c. \(\mathrm{Mn}\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)_{3}{ }^{2+}\) d. \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{NO}_{2}{ }^{2+}\) e. \(\mathrm{Ni}(\mathrm{CN})_{4}{ }^{2-}\) f. \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}^{+}\) g. \(\mathrm{Fe}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}{ }^{3-}\) h. \(\mathrm{Co}(\mathrm{SCN})_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}^{+}\)

Short Answer

Expert verified
a. pentaamminechloridoruthenium(II) b. hexacyanoferrate(II) c. tris(ethylenediamine)manganese(II) d. pentaamminenitrito-N-cobalt(III) e. tetracyanonickelate(II) f. tetraamminedichlorochromium(III) g. trioxalatoferrate(III) h. diamminetetrakis(thiocyanato-N)cobalt(II)

Step by step solution

01

a. Ru(NH3)5 Cl^2+

This complex ion has a central ruthenium (Ru) atom, five ammonia (NH3) ligands, and one chloride (Cl) ligand with a 2+ charge overall. Therefore, the name is pentaamminechloridoruthenium(II).
02

b. Fe(CN)6^4-

This complex ion has a central iron (Fe) atom, six cyanide (CN) ligands, and an overall charge of 4-. Therefore, the name is hexacyanoferrate(II).
03

c. Mn(NH2CH2CH2NH2)3^2+

This complex ion has a central manganese (Mn) atom and three ethylenediamine (NH2CH2CH2NH2) ligands with a 2+ charge overall. Therefore, the name is tris(ethylenediamine)manganese(II).
04

d. Co(NH3)5 NO2^2+

This complex ion has a central cobalt (Co) atom, five ammonia (NH3) ligands, and one nitrito-N (NO2) ligand with a +2 charge. Therefore, the name is pentaamminenitrito-N-cobalt(III).
05

e. Ni(CN)4^2-

This complex ion has a central nickel (Ni) atom and four cyanide (CN) ligands with an overall charge of 2-. Therefore, the name is tetracyanonickelate(II).
06

f. Cr(NH3)4 Cl2^+

This complex ion has a central chromium (Cr) atom, four ammonia (NH3) ligands, and two chloride (Cl) ligands with a +1 charge. Therefore, the name is tetraamminedichlorochromium(III).
07

g. Fe(C2O4)3^3-

This complex ion has a central iron (Fe) atom and three oxalate (C2O4) ligands with an overall charge of 3-. Therefore, the name is trioxalatoferrate(III).
08

h. Co(SCN)2(H2O)4^+

This complex ion has a central cobalt (Co) atom, two thiocyanato-N (SCN) ligands, and four aqua (H2O) ligands with a +1 charge. Therefore, the name is diamminetetrakis(thiocyanato-N)cobalt(II).

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Most popular questions from this chapter

How many bonds could each of the following chelating ligands form with a metal ion? a. acetylacetone (acacH), a common ligand in organometallic catalysts: b. diethylenetriamine, used in a variety of industrial processes: $$ \mathrm{NH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{NH}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{NH}_{2} $$ c. salen, a common ligand for chiral organometallic catalysts: d. porphine, often used in supermolecular chemistry as well as catalysis; biologically, porphine is the basis for many different types of porphyrin- containing proteins, including heme proteins:

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: $$ \mathrm{Ag}(s)+\mathrm{CN}^{-}(a q)+\mathrm{O}_{2}(g) \stackrel{\text { Basic }}{\longrightarrow} \mathrm{Ag}(\mathrm{CN})_{2}^{-}(a q) $$ Balance this equation by using the half-reaction method.

Which of the following molecules exhibit(s) optical isomerism? a. \(c i s-\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\) b. trans \(-\mathrm{Ni}(\mathrm{en})_{2} \mathrm{Br}_{2}\) (en is ethylenediamine) c. cis-Ni(en) \(_{2} \mathrm{Br}_{2}\) (en is ethylenediamine) d.

There are three salts that contain complex ions of chromium and have the molecular formula \(\mathrm{CrCl}_{3} \cdot 6 \mathrm{H}_{2} \mathrm{O}\). Treating \(0.27 \mathrm{~g}\) of the first salt with a strong dehydrating agent resulted in a mass loss of \(0.036 \mathrm{~g}\). Treating \(270 \mathrm{mg}\) of the second salt with the same dehydrating agent resulted in a mass loss of \(18 \mathrm{mg}\). The third salt did not lose any mass when treated with the same dehydrating agent. Addition of excess aqueous silver nitrate to \(100.0\) -mL portions of \(0.100 M\) solutions of each salt resulted in the formation of different masses of silver chloride; one solution yielded \(1430 \mathrm{mg} \mathrm{AgCl}\); another, \(2870 \mathrm{mg} \mathrm{AgCl}\); the third, \(4300 \mathrm{mg} \mathrm{AgCl}\). Two of the salts are green and one is violet. Suggest probable structural formulas for these salts, defending your answer on the basis of the preceding observations. State which salt is most likely to be violet. Would a study of the magnetic properties of the salts be helpful in determining the structural formulas? Explain.

The complex ion \(\mathrm{Fe}(\mathrm{CN})_{6}{ }^{3-}\) is paramagnetic with one unpaired electron. The complex ion \(\mathrm{Fe}(\mathrm{SCN})_{6}{ }^{3-}\) has five unpaired electrons. Where does \(\mathrm{SCN}^{-}\) lie in the spectrochemical series relative to \(\mathrm{CN}^{-}\) ?
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