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General Chemistry Principles And Modern Applications 11th Edition Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette - Solutions

Explain why 1.0 M Fe(NO3)3(aq) is acidic.
Write the formula and name of (a) a complex ion having Cr3+ as the central ion and two NH3 molecules and four Cl– ions as ligands (b) a complex ion of iron(III) having a coordination number of 6 and CN– as ligands (c) a coordination compound comprising two types of complex ions: one a
Absorbance is a measure of the proportion of monochromatic (single-color) light that is absorbed as the light passes through a solution. An absorption spectrum is a graph of absorbance as a function of wavelength. High absorbances correspond to large proportions of the light entering a solution
(A) What are the coordination number and oxidation state of nickel in the ion [Ni(CN)4I]3–?(B) Write the formula of a complex with cyanide ion ligands, an iron ion with an oxidation state of +3, and a coordination number of 6.
What are the coordination number and oxidation state of Co in the complex ion [CoCl(NO2)(NH3)4]+? Co34
A complex of Al(III) can be formulated as AlCl3 · 3 H2O. The coordination number is not known but is expected to be 4 or 6. Describe how Werner’s methods, that is, reaction with AgNO3(aq) or conductivity measurements, could help elucidate the actual coordination number.
What are the coordination number and the oxidation state of the central metal ion in each of the following complexes? Name each complex.(a) [Co(NH3)6]2+(b) [AlF6]3–(c) [Cu(CN)4]2–(d) [CrBr2(NH3)4]+(e) [Co(ox)3]4–(f) [Ag(S2O3)2]3–.
(A) What is the formula of the compound potassium hexachloridoplatinate(IV)?(B) What is the name of the compound [Co(NH3)5(SCN)]?
The ligand diethylenetriamine (abbreviated det), H2NCH2CH2NHCH2CH2NH2, can form complexes. Classify this ligand as mono-, bi-, tri-, or quadridentate.
(a) What is the name of the complex [CoCl3(NH3)3]?(b) What is the formula of the compound pentaaquachloridochromium(III) chloride? (c) What is the name of the compound K3[Fe(CN)6]?
Supply acceptable names for the following:(a) [Ag(NH3)2]Cl (b) [Cu(H2O)2(NH3)4]SO4 (c) PtCl2(en)(d) [CrBr(H2O)5]2+(e) Rb[AgF4](f) Na2[Fe(CN)5NO].
(A) Sketch the geometric isomers of [CoCl2(NH3)2(ox)]–.(B) Sketch the geometric isomers of [Mo(C5H5N)2(CO)2Cl2]+.
A student named a coordination complex tripotassium dichloridodibromidodihy-droxidoiron. The student’s instructor pointed out that although the correct formula for the compound could be deduced, this name violates the IUPAC convention. How does this name violate IUPAC rules, and what is the
Sketch structures of all the possible isomers of [CoCl(NH3)3(ox)].
Write appropriate formulas for the following.(a) Potassium hexacyanidoferrate(III)(b) Bis(ethylenediamine)copper(II) ion (c) Pentaaquahydroxidoaluminum(III) chloride (d) Amminechloridobis(ethylenediamine) chromium(III) sulfate (e) Tris(ethylenediamine)iron(III) hexacyanidoferrate(II).
(A) How many unpaired electrons would you expect to find in the octahedral complex [MnF6]2–?(B) How many unpaired electrons would you expect to find in the tetrahedral complex Would you expect more, fewer, or the same number of unpaired electrons as in the octahedral complex [Co(H2O)6]2+?
How many unpaired electrons would you expect to find in the octahedral complex [Fe(CN)6]3–? ENERGY Strong field YN N Low-spin complex [Fe(CN)61³- 4>P d₂2, d 2-y2 4₂ dxy dxz dyz
Explain why the substitution of a fourth Cl– for an NH3 in mer-[CoCl3(NH3)3] may produce some of the same product as the substitution of a fourth Cl– for an NH3 in fac-[CoCl3(NH3)3], or it may also produce a different product.
Draw Lewis structures for the following ligands:(a) H2O(b) CH3NH2(c) ONO–(d) SCN–.
Of the following complex cations, which are identical, which are geometrical isomers, which are enantiomers? (a) (d) (b) (e) (c) = Cr³+ = CI- = H₂NCH₂CH₂NH₂
(A) The complex ion [Co(CN)4]2– is paramagnetic with three unpaired electrons. Use ideas from the crystal field theory to speculate on its probable structure.(B) Would you expect [Cu(NH3)4]2+ to be diamagnetic or paramagnetic? Can you use this information about the magnetic properties
The complex ion [Ni(CN)4]2– is diamagnetic. Use ideas from the crystal field theory to speculate on its probable structure.
Draw Lewis structures for the following ligands:(a) Hydroxido (b) Sulfato (c) Oxalato (d) Thiocyanato-N-.
Table 24.5 lists the color of [Cr(H2O)6]Cl3 as violet, whereas that of [Cr(NH3)6]Cl3 is yellow. Explain this difference in color.Table 24.5 TABLE 24.5 Some Coordination Compounds Isomer of Cr³+ and Their
(A) The color of [Co(H2O)6]2+ is pink, whereas that of tetrahedral [CoCl4]2– is blue. Explain this difference in color.(B) One of the following solids is yellow, and the other is green: Fe(NO3)2 · 6 H2O; K4[Fe(CN)6] · 3 H2O. Indicate which is which, and explain your reasoning.
From the following crystal field splitting diagrams identify: (i) A tetrahedral Mn2+ complex; (ii) A strong-field octahedral complex of Co3+; (iii) A weak-field octahedral complex of Fe2+; (iv) A tetrahedral Ni2+ complex; (v) A high-spin octahedral complex of Fe3+.
Draw a plausible structure to represent:(a) [FeBr(ox)2]2–(b) [CoBr4(NH3)2]–(c) [Cu(EDTA)]2–(d) [CrBr2(H2O)4]+(e) [PtBr6]2–.
(A) The compound [CoCl(en)2(NO2)2] has been prepared in a number of isomeric forms. One form undergoes no reaction with either AgNO3 or en and is optically inactive. A second form reacts with AgNO3 to form a white precipitate, does not react readily with en, and is optically inactive. A third form
The Cr(III) cation in aqueous solution can form 6-coordinate complexes with ethylenediamine and EDTA4–. Which complex do you expect to be the most stable if all water molecules in the six-coordinate Cr3+(aq) ion are replaced?
The electrode potential diagram for manganese in acidic solutions in Figure 23-14 does not include a value of E° for the reduction of MnO4– to Mn2+. Use other data in the figure to establish this E°, and compare your result with the value found in Table 19.1.Figure 23-14Table 19.1 Acidic
Use data from the text to construct a standard electrode potential diagram relating the following chromium species in acidic solution. Cr₂0₂²- Cr³+ Cr2+ - Cr
Use data from the text to construct a standard electrode potential diagram relating the following vanadium species in acidic solution. ta vo VO2+ V3+ V2+ V
When a soluble lead compound is added to a solution containing primarily orange dichromate ion, yellow lead chromate precipitates. Describe the equilibria involved.
When yellow BaCrO4 is dissolved in HCl(aq), a green solution is obtained. Write a chemical equation to account for the color change.
When Zn(s) is added to K2Cr2O7 dissolved in HCl(aq), the color of the solution changes from orange to green, then to blue, and, over a period of time, back to green. Write equations for this series of reactions.
If CO2(g) under pressure is passed into Na2CrO4(aq), Na2Cr2O7(aq) is formed. What is the function of the CO2(g)? Write a plausible equation for the net reaction.
Use equation (23.19) to determine [Cr2O72–] in a solution that has [CrO2–] = 0.20 M and pH of (a) 7.12(b) 9.15.Eq. 23.19 Kc = [Cr₂0₂²] [CrO4²-]²[H+]² = 3.2 x 1014 (23.19)
If a solution is prepared by dissolving 1.505 g Na2CrO4 in 345 mL of a buffer solution with pH = 7.55, what will be [CrO42–] and [Cr2O72–]?
How many grams of chromium would be deposited on an object in a chrome-plating bath after 1.00 h at a current of 3.4 A?
Which of these octahedral complexes would you expect to exhibit geometric isomerism? Explain.(a) [Cr(NH3)5OH]2+(b) [CrCl2(H2O)(NH3)3]+(c) [CrCl2(en)2]+(d) [CrCl4(en)]–(e) [Cr(en)3]3+.
The structures of four complex ions are given. Each has Co3+ as the central ion. The ligands are H2O, NH3, and oxalate ion, C2O42–. Determine which, if any, of these complex ions are isomers (geometric or optical); which, if any, are identical (that is, have identical structures); and which, if
Describe how the crystal field theory explains the fact that so many transition metal compounds are colored.
Cyanido complexes of transition metal ions (such as Fe2+ and Cu2+) are often yellow, whereas aqua complexes are often green or blue. Explain the basis for this difference in color.
If the ion Co2+ is linked with strong-field ligands to produce an octahedral complex, the complex has one unpaired electron. If Co2+ is linked with weak-field ligands, the complex has three unpaired electrons. How do you account for this difference?
In contrast to the case of Co2+ considered in Exercise 19, no matter what ligand is linked to Ni2+ to form an octahedral complex, the complex always has two unpaired electrons. Explain this fact.Exercise 19If the ion Co2+ is linked with strong-field ligands to produce an octahedral complex, the
Predict:(a) Which of the complex ions, [MoCl6]3– and [Co(en)3]3+, is diamagnetic and which is paramagnetic;(b) The number of unpaired electrons expected for the tetrahedral complex ion [CoCl4]2–.
Predict:(a) Whether the square-planar complex ion [Cu(py)4]2+ is diamagnetic or paramagnetic (b) Whether octahedral [Mn(CN)6]3– or tetrahedral [FeCl4]– has the greater number of unpaired electrons.
In Example 24-5, we chose between a tetrahedral and a square-planar structure for [Ni(CN)4]2– based on magnetic properties. Could we similarly use magnetic properties to establish whether the ammine complex of Ni(II) is octahedral [Ni(NH3)6]2+ or tetrahedral [Ni(NH3)4]2+? Explain.Example 24-5The
In both [Fe(H2O)6]2+ and [Fe(CN)6]4– ions, the iron is present as Fe(II); however, [Fe(H2O)6]2+ is paramagnetic, whereas [Fe(CN)6]4– is diamagnetic. Explain this difference.
Write equations to represent the following observations.(a) A mixture of Mg(OH)2(s) and Zn(OH)2(s) is treated with NH3(aq). The Zn(OH)2 dissolves, but the Mg(OH)2(s) is left behind.(b) When NaOH(aq) is added to CuSO4(aq), a pale blue precipitate forms. If NH3(aq) is added, the precipitate
Which of the following complex ions would you expect to have the largest overall Kf, and why? [Cu(H₂O) 12+; [Cu(H₂O)²(NH3)]²+; [Cu(en)]²+; [Cu(en)₂(H₂O)₂]2+; [Cu(en)(NH3)4]²+.
Write equations to represent the following observations.(a) A quantity of CuCl2(s) is dissolved in concentrated HCl(aq) and produces a yellow solution. The solution is diluted to twice its volume with water and assumes a green color. On dilution to ten times its original volume, the solution
Use data from Table 24.6 to determine values of (a) β4 for the formation of [Zn(NH3)4]2+;(b) β4 for the formation of [Ni(H2O)2(NH3)4]2+.
Write a series of equations to show the stepwise displacement of H2O ligands in [Fe(H2O)6]3+ by ethylenediamine, for which log10 K1 = 4.34, log10 K2 = 3.31, and log10 K3 = 2.05. What is the overall formation constant, β3 = Kf, for [Fe(en)3]3+?
For the overall reaction [Cu(H2O)6]2+ + 4NH3 ⇌ [Cu(H2O)2(NH3)4]2+ + 4H2O, a tabulation of formation constants lists the following log10 K values: log10 K1 = 4.25, log10 K2 = 3.61, log10 K3 = 2.98, and log10 K4 = 2.24. What is the overall formation constant β4 = Kf for [Cu(H2O)2(NH3)4]2+?
Which of the following would you expect to react as a Brønsted–Lowry acid: [Cu(NH3)4]2+, [FeCl4]–, [Al(H2O)6]3+, or [Zn(OH)4]2–?Why?
From data, (a) Derive an equilibrium constant for reaction (24.13), and explain why this reaction (the fixing of photographic film) is expected to go essentially to completion.(b) Explain why NH3(aq) cannot be used in the fixing of photographic film.Reaction (24.13) AgBr(s) + 2S,O3(aq) »
Write simple chemical equations to show how the complex ion [Cr(H2O)5(OH)]2+ acts as (a) An acid;(b) A base.
Show that the oxidation of [Co(NH3)6]2+ to [Co(NH3)6]3+ should occur spontaneously in alkaline solution with H2O2 as an oxidizing agent.
Explain why K2[PtCl4] is first converted to K2[PtI4] in the synthesis of the anticancer drug cisplatin, cis-PtCl2(NH3)2.
Draw dashed and solid wedge diagrams of transplatin, trans-PtCl2(NH3)2, and cisplatin, cis-PtCl2(NH3)2. Then, explain how transplatin can be more reactive yet less effective at killing cancer cells than is cisplatin.
From each of the following names, you should be able to deduce the formula of the complex ion or coordination compound intended. Yet, these are not the best systematic names that can be written. Replace each name with one that is more acceptable: (a) Cupric tetraammine ion; (b)
Magnus’s green salt has the empirical formula PtCl2 · 2 NH3. It is a coordination compound consisting of both complex cations and complex anions. Write the probable formula of this coordination compound according to Werner’s theory, and assign it a systematic name.
How many isomers are there of the complex ion [CoCl2(en)(NH3)2]+? Sketch their structures.
For polyprotic acids, ionization constants for successive ionization steps decrease rapidly. That is,Ka1 ≫ Ka2 ≫ Ka3. The ionization constants for the first two steps in the ionization of [Fe(H2O)6]3+ (reactions 24.10 and 24.11) are more nearly equal in magnitude. Why does this multistep
The cis and trans isomers of [CoCl2(en)2]+ can be distinguished via a displacement reaction with oxalate ion. What difference in reactivity toward oxalate ion would you expect between the cis and trans isomers? Explain.
Write half-equations and an overall equation to represent the oxidation of tetraammineplatinum(II) ion to trans-tetraamminedichloridoplatinum(IV) ion by Cl2. Then make sketches of the two complex ions.
For a solution that is 0.100 M in [Fe(H2O)6]3+, (a) Assuming that ionization of the aqua complex ion proceeds only through the first step, equation (24.10), calculate the pH of the solution.(b) Calculate [[Fe(H2O)5(OH)]2+] if the solution is also 0.100 M HClO4. (ClO4– does not complex with
Following are the names of five coordination compounds containing complexes with platinum(II) as the central metal ion and ammonia molecules and or chloride ions as ligands: (a) Potassium amminetrichloridoplatinate(II); (b) Diamminedichloridoplatinum(II); (c) Triamminechloridoplatinum(II)
A solution that is 0.010 M in Pb2+ is also made to be 0.20 M in a salt of EDTA (that is, having a concentration of the EDTA4– ion of 0.20 M). If this solution is now made 0.10 M in H2S and 0.10 M in H3O+, will PbS(s) precipitate?
Without performing detailed calculations, show why you would expect the concentrations of the various ammine–aqua complex ions to be negligible compared with that of [Cu(NH3)4]2+ in a solution having a total Cu(II) concentration of 0.10 M and a total concentration of NH3 of 1.0 M. Under what
Estimate the total [Cl–] required in a solution that is initially 0.10 M CuSO4 to produce a visible yellow color.Assume that 99% conversion of [Cu(H2O)4]2+ to [CuCl4]2– is sufficient for this to happen, and ignore the presence of any mixed aqua–chlorido complex ions. [Cu(H₂O)4]²+ + 4Cl
Verify that neither Ca2+ nor Mg2+ found in natural waters is likely to precipitate from the water on the addition of other reagents if the ions are complexed with EDTA. Assume reasonable values for the total metal ion concentration and that of free EDTA, such as 0.10 M each.
Refer to the stability of [Co(NH3)6]3+(aq)(a) Verify that E°cell reaction (24.12) is +0.59 V.(b) Calculate [Co3+] in a solution at equilibrium that has a total concentration of cobalt of 0.1 M and [NH3] = 0.1 M.(c) Show that for the value of [Co3+] calculated in part (b), reaction (24.12) will not
The following concentration cell is constructed.If Kf for [Ag(CN)2]– is 5.6 x 1018, what value would you expect for Ecell? Ag Ag (0.10 M[Ag(CN)2], 0.10 M CN¯) ||Ag+ (0.10 M)| Ag
A Cu electrode is immersed in a solution that is 1.00 M NH3 and 1.00 M in [Cu(NH3)4]2+. If a standard hydrogen electrode is the cathode, Ecell is +0.08 V. What is the value obtained by this method for the formation constant, Kf, of [Cu(NH3)4]2+?
The compound CoCl2 · 2 H2O · 4 NH3 may be one of the hydrate isomers [CoCl(H2O)(NH3)4]Cl · H2O or [Co(H2O)2(NH3)4]Cl2. A 0.10 M aqueous solution of the compound is found to have a freezing point of –0.56 °C. Determine the correct formula of the compound. The freezing-point depression constant
Explain why aqueous solutions of [Sc(H2O)6]Cl3 and [Zn(H2O)4]Cl2 are colorless, but an aqueous solution of [Fe(H2O)6]Cl3 is not.
Provide a valence bond description of the bonding in the Cr(NH3)63+ ion. According to the valence bond description, how many unpaired electrons are there in the Cr(NH3)63+ complex? How does this prediction compare with that of crystal field theory?
Acetyl acetone undergoes an isomerization to form a type of alcohol called an enol.The enol, abbreviated acacH, can act as a bidentate ligand as the anion acac–. Which of the following compounds are optically active: Co(acac)3; trans-[Co(acac)2(H2O)2]Cl2; cis-[Co(acac)2(H2O)2]Cl2?
A tabulation of formation constants lists the following log10 K values for the formation of [Cu(NH3)4]2+: log10 K1 = 4.28, log10 K2 = 3.59, log10 K3 = 3.00, and log10 K4 = 2.18. Calculate the mole fractions of Cu2+, [Cu(NH3)]2+, [Cu(NH3)2]2+, [Cu(NH3)3]2+, and [Cu(NH3)4]2+ in solution when [NH3]eq
We have seen that complex formation can stabilize oxidation states. An important illustration of this fact is the oxidation of water in acidic solutions by Co3+(aq) but not by [Co(en)3]3+. Use the following data.Show that [Co(en)3]3+ is stable in water but Co3+(aq) is not. [Co(H₂0)6]³+ + e [Co
The amino acid glycine (NH2CH2CO2H, denoted Hgly) binds as an anion and is a bidentate ligand. Draw and name all possible isomers of [Co(gly)3]. How many isomers are possible for the compound [CoCl(gly)2(NH3)]? NH2CH2CO2– is the glycinate anion.
The graph that follows represents the molar conductivity of some Pt(IV) complexes. The ligands in these complexes are NH3 molecules or Cl– ions, the coordination number of Pt(IV) is 6, and the counter ions (for balancing charge) are K+ or Cl–.Write formulas for the coordination compounds
The structure of K2[PtCl6] in the solid state is shown in the next column. Identify the type of cubic unit cell, and describe the structure in terms of the holes occupied by the various ions.
A structure that Werner examined as a possible alternative to the octahedron is the trigonal prism.(a) Does this structure predict the correct number of isomers for the complex ion [CoCl2(NH3)4]+? If not, why not?(b) Does this structure account for optical isomerism in [Co(en)3]3+? Explain.
Werner demonstrated that octahedral complexes can exhibit optical isomerism, and to Werner’s satisfaction, this confirmed the octahedral arrangement of ligands. However, skeptics of his theory said that because the ligands contained carbon atoms, he could not rule out carbon as the source of the
In your own words, describe the following terms or symbols: (a) Coordination number; (b) Δo;(c) Ammine complex; (d) Enantiomer.
Briefly describe each of the following ideas, phenomena, or methods: (a) Spectrochemical series; (b) Crystal field theory; (c) Optical isomer; (d) Structural isomerism.
Explain the important distinction between each of the following pairs: (a) Coordination number and oxidation number; (b) Monodentate and polydentate ligands; (c) Cis and trans isomers; (d) Dextrorotatory and levorotatory compounds; (e) Low-spin and highspin complexes.
The oxidation state of Ni in the complex ion [Ni(CN)4I]3– is (a) –3; (b) –2;(c) 0; (d) +2;(e) 3+;
The coordination number of Pt in the complex ion [PtCl2(en)2]2+ is (a) 2; (b) 3; (c) 4; (d) 5; (e) 6.
Of the following complex ions, the one that exhibits isomerism is (a) [Ag(NH3)2]+;(b) [CoNO2(NH3)5]2+;(c) [Pt(en)(NH3)2]2+;(d) [CoCl(NH3)5]2+;(e) [PtCl6]2–.
Of the following complex ions, the one that is optically active is (a) cis-[CoCl2(en)2]+;(b) [CoCl2(NH3)4]+;(c) [CoCl4(NH3)2]–;(d) [CuCl4]–.
The number of unpaired electrons in the complex ion [Cr(NH3)6]2+ is (a) 5; (b) 4; (c) 3; (d) 2; (e) 1.
Of the following, the one that is a Brønsted–Lowry acid is (a) [Cu(NH3)4]2+;(b) [FeCl4]–;(c) [Fe(H2O)6]3+;(d) [Zn(OH)4]–.
The most soluble of the following solids in NH3(aq)is (a) Ca(OH)2;(b) Cu(OH)2;(c) BaSO4;(d) MgCO3;(e) Fe2O3.
Name the following coordination compounds. Which one(s) exhibit(s) stereoisomerism? Explain.(a) [CoBr(NH3)5]SO4(b) [Cr(NH3)6][Co(CN)6](c) Na3[Co(NO2)6](d) [Co(en)3]Cl3.
Write appropriate formulas for the following species.(a) Dicyanidoargentate(I) ion (b) Triamminenitrito-N-platinum(II) ion (c) Aquachloridobis(ethylenediamine)cobalt(III) ion (d) Potassium hexacyanidochromate(II).
Draw structures to represent these four complex ions:(a) [PtCl4]2–;(b) [FeCl4(en)]–;(c) cis-[FeCl2(en)(ox)]–;(d) trans-[CrCl(NH3)4(OH)]+.

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