Problem 1
Give the electronic configurations of the following atoms and ions: \((\mathrm{a}) \mathrm{V}^{3+} ;(\mathrm{b}) \mathrm{Fe} ;(\mathrm{c}) \mathrm{Cr},(\mathrm{d}) \mathrm{Ag}^{+} ;(\mathrm{e}) \mathrm{Fe}(0)\left(\mathrm{in}\left[\mathrm{Fe}(\mathrm{CO})_{5}\right]\right]\) \((f) C u^{2+} ;(g) R u^{2+} ;(h) W^{4+},(\text { Section } 28.1)\)
Problem 2
Explain why the +3 oxidation state becomes increasingly less stable with respect to the +2 oxidation state on moving from left to right across the first row of the d-block elements. (Section \(28.2)\)
Problem 4
Name the following coordination compounds (Section 28.3 ): (a) \(\left[\mathrm{NiI}\left(\mathrm{NH}_{3}\right)_{5}\right] \mathrm{NO}_{3} ;(\mathrm{b}) \mathrm{K}\left[\mathrm{Co}(\mathrm{ox})_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right] ;(\mathrm{c})\left[\mathrm{Fe}(\text { dien })_{2}\right] \mathrm{SO}_{4}\) (d) \(\mathrm{Na}\left[\mathrm{AuBr}_{2} \mathrm{Cl}_{2}\right]\)
Problem 5
Determine the formulae for the following coordination compounds (Section 28.3): (a) chloro(diethylsulfide)gold(I); (b) tetraethylammonium tetrabromoferrate(ll); (c) bis(2,2'-bipyridine)dicarbonylmolybdenum(0): (d) potassium hexanitrito-xO-cobaltate(ll).
Problem 6
Compounds \(X\) and \(Y\) have the same molecular formula and contain \(18.25 \%\) titanium, \(40.54 \%\) chlorine, \(36.59 \%\) oxygen, and \(4.61 \%\) hydrogen by mass. When \(0.5000 \mathrm{g}\) of \(\mathrm{X}\) was dissolved in water and treated with silver nitrate solution, \(0.2731 \mathrm{g}\) of silver chloride were precipitated. \(0.5000 \mathrm{g}\) of \(\mathrm{Y}\) were dissolved in water and titrated against \(0.2000 \mathrm{moldm}^{-3}\) silver nitrate solution, of which \(28.2 \mathrm{cm}^{3}\) were required. Identify \(X\) and \(Y\), and determine any possible isomers. (Section 28.3 )
Problem 7
Which of the following pairs of compounds are isomers? Name the type of any isomerism present. (Section 28.3 ) (a) \(\quad \mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{8}\right]\) and \(\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (b) \(\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{3}\right] \mathrm{Se} \mathrm{O}_{4}\) and \(\left[\mathrm{Co}\left(\mathrm{SeO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{3}\right] \mathrm{C}\) (c) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right]\left[\mathrm{Pt} \mathrm{Br}_{4}\right]\) and \(\left[\mathrm{PtBr}\left(\mathrm{NH}_{3}\right)\right]\left[\mathrm{PtBr}_{3}\left(\mathrm{NH}_{3}\right)\right]\) (d) \(\left[\mathrm{Co}\left(\mathrm{NO}_{2}\right)\left(\mathrm{NH}_{3}\right)_{3}\right] \mathrm{Cl}_{2}\) and \(\left[\mathrm{Co}(\mathrm{ONO})\left(\mathrm{NH}_{3}\right)\right] \mathrm{Cl}_{2}\)
Problem 8
Sketch the possible isomers for the following compounds and identify the type of isomerism involved: (a) \(\left[\mathrm{Co}(\mathrm{ox})_{3}\right]^{3-}\) (b) \(\left[\mathrm{NiCl}_{2}(\mathrm{en})_{2}\right]\) ; (c) \(\left[\mathrm{NiCl}_{2}(\mathrm{py})_{2}\right]\) I; \((d)\left[F e F_{3}\left(H_{2} O\right)_{3}\right]\) (Section 28.3 )
Problem 9
Dimethyl sulfoxide (DMSO, Me_SO) is an ambidentate ligand as it can act as an S-donor or an 0 -donor. (Sections 28.3,5.2 ) (a) Use VSEPR theory to show there is a lone pair on the sulfur atom. (b) Use the hard and soft acids and bases theory to predict Which atom will coordinate to (i) \(\mathrm{Pt}^{2 *}\) and (ii) \(\mathrm{Fe}^{3+}\).
Problem 16
\(\mathrm{Na}_{2}\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]\) is diamagnetic, not paramagnetic. Use this information to determine the geometry of the anion. (Section \(28.7)\)
