not use ai please Question Two1.Compare and contrast the d-orbitals of the transition metals to the 4f orbitals that occur in the lanthanideseries.(6)

SIMILARITIES1)Inner shell orbitals -Both d and 4f orbitals are inner shell orbitals. They are not…

Answered: Question Two 1. Compare and contrast…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter22: The Chemistry Of The Transistion Elements

Section: Chapter Questions

Problem 14PS

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Similar questions

Would you expect salts of the gold(I) ion, Au+, to be colored? Explain.
The ferrate ion, FeO42, is such a powerful oxidizing agent that in acidic solution, aqueous ammonia is reduced to elemental nitrogen along with the formation of the iron(III) ion. a. What is the oxidation state of iron in FeO42, and what is the electron configuration of iron in this polyatornic ion? b. lf 25.0 mL of a 0.243 M FeO42 solution is allowed to react with 55.0 mL of 1.45 M aqueous ammonia, what volume of nitrogen gas can form at 25C and 1.50 atm?
(a) What is the lanthanide contraction? (b) How does it affectatomic size down a group of transition elements? (c) How doesit influence the densities of the Period 6 transition elements?
Lanthanide contraction caused the similarities of the radius of the 4d and 5d metals and is responsible for the low reactivity of the 2nd and 3rd transition series.* True or false
(i) Name the element of 3d transition series which shows maximum number of oxidation states. Why does it show so? (ii) Which transition metal of 3d series has positive E°(M2+/M) value and why? (iii) Out of Cr3+ and Mn3+, which is a stronger oxidizing agent and why? (iv) Name a member of the lanthanoid series which is well known to exhibit + 2 oxidation state. (v) Complete the following equation: MnO4– + 8H+ + 5e- ———->
(a) Explain the major difference between the number of oxi-dation states of most transition elements and that of most main-group elements. (b) Why is the +2 oxidation state so commonamong transition elements?
Explain the following observations :(i) Copper atom has completely filled d orbitals (3d10) in its ground state, yet it is regarded as a transition element.(ii) Cr2+ is a stronger reducing agent than Fe2+ in aqueous solutions.
(a) Draw the electronic configuration of [NiCl6]3. (b) Determine whether its paramagnetic or diamagnetic. (c) What is expected to happen to the color if the ligand is replaced by carbonyl?
(a) Explain the major difference between the number of oxidation states of most transition elements and that of most main-group elements. (b) Why is the +2 oxidation state so common among transition elements?
Give reasons :(i) Zn is not regarded as a transition element.(ii) Cr2+ is a strong reducing agent.
Explain giving reasons :(i) Transition metals and their compounds generally exhibit a paramagnetic behaviour.(ii) The chemistry of actinoids is not so smooth as that of lanthanoids.
What are the oxidation states of manganese in the following series of oxides? MnO, MnO2, Mn2O3, Mn2O7, Mn3O4, and [MnO4]-? Recall that you must include the total charge on the ion for ionic species.

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Question Two 1. Compare and contrast the d-orbitals of the transition metals to the 4f orbitals that occur in the lanthanide series. (6)