(b) [Zn(II)(H2O)6]?* can undergo successive reactions with phen ligands: [Zn(II)(H2O)«(phen)]²* + 2H2O [Zn(1I)(H2O)2(phen)2]?* + 2H2O log K2 = 6.09 [Zn(II)(phen)3]* + 2H2O [Zn(II)(H2O)6]?* + phen log Kn = 6.31 [Zn(1I)(H2O)«(phen)]?* + phen [Zn(II)(H2O)2(phen)2}²* + phen log Ks = 4.77 Explain the decrease in successive log Km values as the number of phen ligands increases and calculate log Ba for the overall reaction: [Zn(II)(H2O)6]?* + 3 phen - (Zn(II)(phen)s]²* + 6H2O (c) Explain why each of the complexes above are colourless and diamagnetic. Which would be more stable: [Ni(II)(phen)3]²* or [Zn(1I)(phen);]²* based on electronic configuration?

(b) [Zn(II)(H2O)6]?* can undergo successive reactions with phen ligands: [Zn(II)(H2O)«(phen)]²* + 2H2O [Zn(1I)(H2O)2(phen)2]?* + 2H2O log K2 = 6.09 [Zn(II)(phen)3]* + 2H2O [Zn(II)(H2O)6]?* + phen log Kn = 6.31 [Zn(1I)(H2O)«(phen)]?* + phen [Zn(II)(H2O)2(phen)2}²* + phen log Ks = 4.77 Explain the decrease in successive log Km values as the number of phen ligands increases and calculate log Ba for the overall reaction: [Zn(II)(H2O)6]?* + 3 phen - (Zn(II)(phen)s]²* + 6H2O (c) Explain why each of the complexes above are colourless and diamagnetic. Which would be more stable: [Ni(II)(phen)3]²* or [Zn(1I)(phen);]²* based on electronic configuration?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

How would the addition of AgNO3 affect equilibrium system (D)? 2+ 2- [Co(H20)6] (ag) + 4 Cl (ag) A.The solution would become bluer since the silver would precipitate with the chloride ions shifting the = [Co(H2O)2CI4] (ag) + 4 H2O() equilibrium to the left. B. The solution would become pinker since the silver would precipitate with the chloride ions shifting the equilibrium to the left. C. The solution would become pinker since the silver would precipitate with the chloride ions shifting the equilibrium to the right. D. The solution would become bluer since the silver would precipitate with the chloride ions shifting the equilibrium to the right. I D Focus W
Consider bis(ethylenediamine) copper(ii) complex ion, Cu(en)22+ : A ) Explain the bond formation in this ion in terms of lewis acid- base theory. B) Sketch the ion with some drgree of three- dimensional clarity. Indicate the structure of the ion.
Structural, Geometric and Optical Isomers For visual clarity, brackets [] and charges on the complex ions have been omitted. OH, OH, Br OH2 Br Mn Mn Br 'CI Br 'CI OH, What is the relationship between the two structures shown above? Not Isomers Optical Isomers Same Substance Structural Isomers Geometric Isomers is page
Which of the following statements about 10Dq is false? A. In the [CoX(NH3)5]n+ complex, the color changes from dark violet to yellow when X is replaced by I-, Br-, Cl-, H2O, and NH3, respectively.B. [VCl6]2- has a greater 10Dq than [VCl4] complex.C. [MnF6]2- has a higher 10Dq value than [TcF6]2-.D. [V(H2O)6]3+ has a higher 10Dq value than [V(H2O)6]2+.
In the following chemical reaction what is the concentrations of [H3O+] in a solution that is 0.00045 M [Al(H2O)6]3+. Assume that the [Al(H2O)6]3+ dissociates 100% completely and assume 1 Liter of solution. [Al(H2O)6]3+ + 3H2O ↔ [Al(H2O)3(OH)3]2+ + 3H3O+
Write the name for [MNCI(H2O)4(NH3)]NO3. C amminetetraaquachloronitratomanganese (II) amminetetraaquachloronitratomanganate (II) amminetetraaquachloromanganese (III) nitrate C amminetetraaquachloromanganese (II) nitrate amminetetraaquachloromanganate (II) nitrate Camminetetraaquachloromanganate (II) nitrate amminetetraaquachloronitratomanganese (II) C amminetetraaquachloronitratomanganate (III)
Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH", the Al³+ (aq) ion forms a hydroxide complex ion, Al(OH)4. Calculate the concentration of free Al³+ ion when 1.20x10-2 mol AI(CH3COO) 3(S) is added to 1.00 L of solution in which [OH ] is held constant (buffered at pH 12.90). For Al(OH)4, Kf = 1.1x1033. [A1³+] = Check & Submit Answer Show Approach M
This is the lab with my data sheet and please answer all of them. Thank you My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour question: What can you infer about the system from the colour change of the solution?  How can this be possible if no additional Fe3+(aq) has been introduced? What does the addition of the solution do to the [Fe3+(aq)]?
Ni2* forms a complex with ammonia (NH3) which has the formula [Ni(NH:)6]?*. Calculate the [Ni2*], [NH3], and [Ni(NH:)6"]´at equilibrium, when 0.300 M of [Ni²*] and 1.200 M of [NH3] are present in the solution initially. [Kr for [Ni(NH3)6]?* is 5.5x10$] Ni forms a complex with ammonia (NH) which has the formula [Ni(NH) J+ Calculate the [Ni). [NH), and [Ni(NH.)"] at equilibrium, when 0.300 M of [Ni ] and 1.200 M of [NH] are present in the solution initially. [Kr for [Ni(NH.)F is 5.5x10 ]
Name the following: [Pt(H2O)4l2]Br O tetraaquadiiodo platinum(II) bromide O tetraaquadiiodo platinum(III) bromide platinum(II) diiodotetraquabromide O diiodotetrahydroplatinum bromide diiodotetrahydroplatinum(I) bromide
Please use the values in the resources listed below instead of the textbook values. Sometimes equilibria for complex ions are described in terms of dissociation constants, Ka. For the complex ion Cu(CN)4 3- the dissociation reaction is as follows. [Cu*]• [CN 14 Kd [Cu(CN)43-] Cu(CN)4 3- = Cu+ + 4 CN- = 5.0X10° n-31 = Calculate the value of the formation constant, Kf, for Cu(CN)4°¯. 4.0
COBALT COMPLEX: [CoCl4]2-(aq) + 6H2O(l) « [Co(H2O)6]2+(aq) + 4Cl-(aq) + Heat Blue Pink STEPS #- Solutions Observations 1-DISSOLVE COBALT COMPLEX PINK SOLUTION 2-SOLUTION PLUS HCl BLUE SOLUTION 3-ADD WATER PINK SOLUTION 4-HEAT SOLUTION BLUE SOLUTION According to the equilibrium equation, which ion(s) do you have when the solution dissolved? Explain how you know the identity of the ion(s) present. 2. Explain what happened when the HCl was added to the solution. 3. Explain what happened when the H2O was added to the solution. 4. Explain what happened when the solution was heated. Was the reaction exothermic or endothermic?