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Chapter 24: Problem 4

Write appropriate formulas for the following. (a) potassium hexacyanoferrate(III) (b) bis(ethylenediamine)copper(II) ion (c) pentaaquahydroxoaluminum(III) chloride (d) amminechlorobis(ethylenediamine) chromium(III) sulfate (e) tris(ethylenediamine)iron(III) hexacyanoferrate(II)

Short Answer

Expert verified
The chemical formulas for these compounds are (a) \( K_3[Fe(CN)_6] \) (b) \( [Cu(C_2H_8N_2)_2]^{2+} \) (c) \( [Al(H_2O)_5OH]Cl_2 \) (d) \( [Cr(NH_3)(C_2H_8N_2)_2]SO_4 \) (e) \( [Fe(C_2H_8N_2)_3]_2[Fe(CN)_6] \).

Step by step solution

01

Potassium hexacyanoferrate(III)

In potassium hexacyanoferrate(III), 'potassium' indicates the K+. 'Hexacyanoferrate(III)' is ion containing Fe with an oxidation state of +3 and six cyanide ions. Thus, the formula is \( K_3[Fe(CN)_6] \).
02

bis(ethylenediamine)copper(II) ion

In bis(ethylenediamine)copper(II) ion, 'bis' indicates we have 2 ethylenediamine molecules. Copper(II) means we have a Cu2+. So, the formula is \( [Cu(C_2H_8N_2)_2]^{2+} \).
03

Pentaaquahydroxoaluminum(III) chloride

In pentaaquahydroxoaluminum(III) chloride, 'pentaaqua' indicates five water molecules. 'Hydroxo' refers to one hydroxide group. 'Aluminum(III)' suggests we have Al in +3 oxidation state. 'chloride' is just Cl-. Hence, the formula is \( [Al(H_2O)_5OH]Cl_2 \).
04

Amminechlorobis(ethylenediamine)chromium(III) sulfate

In amminechlorobis(ethylenediamine)chromium(III) sulfate, 'ammine' refers to one group of ammonia, while 'chlorobis' refers to two groups of ethylenediamine. 'Chromium(III)' indicates Cr with +3 charge. 'Sulfate' is SO4^2-. So, the resulting formula is \( [Cr(NH_3)(C_2H_8N_2)_2]SO_4 \).
05

Tris(ethylenediamine)iron(III) hexacyanoferrate(II)

In tris(ethylenediamine)iron(III) hexacyanoferrate(II), 'tris' indicates three molecules of ethylenediamine. 'Iron(III)' means we have Fe3+. 'Hexacyanoferrate(II)' shows an ion with Fe in +2 oxidation state with six cyanide ions. Therefore, the chemical formula for this compound is \( [Fe(C_2H_8N_2)_3]_2[Fe(CN)_6] \).

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Most popular questions from this chapter

The coordination number of \(\mathrm{Pt}\) in the complex ion \(\left[\mathrm{PtCl}_{2}(\mathrm{en})_{2}\right]^{2+}\) is \((\mathrm{a}) 2 ;(\mathrm{b}) 3 ;(\mathrm{c}) 4 ;(\mathrm{d}) 5 ;(\mathrm{e}) 6\).

Provide a valence bond description of the bonding in the \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}^{3+}\) ion. According to the valence bond description, how many unpaired electrons are there in the \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}^{3+}\) complex? How does this prediction compare with that of crystal field theory?

The following concentration cell is constructed. \(\mathrm{Ag} | \mathrm{Ag}^{+}\left(0.10 \mathrm{M}\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}, 0.10 \mathrm{M} \mathrm{CN}^{-}\right)\) $$\| \mathrm{Ag}^{+}(0.10 \mathrm{M}) | \mathrm{Ag}$$ If \(K_{f}\) for \(\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}\) is \(5.6 \times 10^{18},\) what value would you expect for \(E_{\text {cell }}\) ? [Hint: Recall that the anode is on the left.]

Indicate what type of isomerism may be found in each of the following cases. If no isomerism is possible, so indicate. (a) \(\left[\mathrm{Cr}(\mathrm{en})_{2} \mathrm{Br}_{2}\right]^{+}\) (b) \(\left[\operatorname{Co}(\text { ox })_{2} \operatorname{Br}(\text { SCN })\right]^{3-}\) (c) \(\left[\mathrm{NiCl}_{4}(\mathrm{en})\right]^{2-}\) (d) \([\mathrm{PtBrCl}(\text { ox })]^{-}\) (e) \(\left[\operatorname{Cr}(\text { Cl })_{3}(\text { det })\right],\) det is \(\mathrm{H}_{2} \mathrm{N}\left(\mathrm{CH}_{2}\right)_{2} \mathrm{NH}\left(\mathrm{CH}_{2}\right)_{2} \mathrm{NH}_{2}\)

Write appropriate formulas for the following species. (a) dicyanoargentate(I) ion (b) triamminenitrito-N-platinum(II) ion (c) aquachlorobis(ethylenediamine)cobalt(III) ion (d) potassium hexacyanochromate(II)
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