For each of the following ions, draw diagrams (on a piece of paper), like the one to the right below, to show orbital occupancies for both weak and strong octahedral fields. Indicate (on the table below) the total number of unpaired electrons in each case. (a) (b) (c) (d) (e) Ion Pd³+ Mn³+ V²+ Cu²+ Cr4+ # Unpaired # Unpaired Weak field Strong field eg t29 do

For each of the following ions, draw diagrams (on a piece of paper), like the one to the right below, to show orbital occupancies for both weak and strong octahedral fields. Indicate (on the table below) the total number of unpaired electrons in each case. (a) (b) (c) (d) (e) Ion Pd³+ Mn³+ V²+ Cu²+ Cr4+ # Unpaired # Unpaired Weak field Strong field eg t29 do

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter8: Bonding In Transition Metal Compounds And Coordination Complexes

Section: Chapter Questions

Problem 53AP

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(a) Calculate the number of unpaired electrons in the following gaseous state ions: Mn2+, Cr3+, V3+ and Fe2+ which one of these in the most stable in aqueous solutions? (At. nos. V = 23, Cr = 24, Mn = 25, Fe = 26) (b) Explain the following observations: (i) The transition metal ions are usually coloured in aqueous solutions. (ii) Cu(I) is not stable in an aqueous solution. (iii) The highest oxidation state of a transition metal is exhibited in its oxide or fluoride.
(a) The spectrochemical series of (a) Fe³+, (b) Co²+ and (c) Mn²+ ions follow the order: (b) Benzene is a field ligand relative to NH3 in the spectrochemical series. (c) For an octahedral Co³* complex with A. = 24,000 cm¹ and pairing energy per electron pair, P = 14,000 cm¹, the CFSE is m-¹. (enter final answer only). OR cm
For each of the following ions, draw diagrams (on a piece of paper), like the one to the right below, to show orbital occupancies for both weak and strong octahedral fields. Indicate (on the table below) the total number of unpaired electrons in each case. Ion # Unpaired Weak field # Unpaired Strong field (a) Pd4+ (b) Cr3+ (c) Cd2+ (d) Ni2+ (e) Co2+
For each of the following ions, draw diagrams like thosein Figure 8.18 to show orbital occupancies in both weakand strong octahedral fields. Indicate the total number ofunpaired electrons in each case.(a) Mn2+ (c) Cr3+ (e) Fe2+(b) Zn2+ (d) Mn2+
For each of the following ions, draw diagrams (on a piece of paper), like the one to the right below, to show orbital occupancies for both weak and strong octahedral fields. Indicate (on the table below) the total number of unpaired electrons in each case. Ion # UnpairedWeak field # UnpairedStrong field (a) Rh4+ (b) Ni2+ (c) Fe2+ (d) Nb2+ (e) Cr4+
How would you account for the following: (i) Metal-metal bonding is more extensive in the 4d and 5d series of transition elements than the 3d series. (ii) Mn(III) undergoes disproportionation reaction easily. (iii) Co (II) is easily oxidised in the presence of strong ligands
2. (a) Calculate the spin only magnetic moment of: 4+ SO₂ (b) The corrected molar susceptibility of K3[Fe(CN)6] is about 1.8 x 103 cgs at room temperature. (i) Calculate μ. (ii) Is this high or low spin complex? Defend your answer.
Give reasons :(i) Zn is not regarded as a transition element.(ii) Cr2+ is a strong reducing agent.
(b) Consider the oxalate (ox) ligand and answer the following questions:(i) Draw the structure of the ox ligand.(ii) Identify all the donor atoms of the ligand.(iii) What is the denticity of the ligand?(iv) What is the charge of the ligand?(v) Draw the structure of a homoleptic octahedral complex with ox as the ligand.Clearly show the geometry at the metal centre.(vi) Identify the stereoisomer in the structure drawn.
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.
For each of the following ions, draw diagrams (on a piece of paper), like the one to the right below, to show orbital occupancies for both weak and strong octahedral fields. Indicate (on the table below) the total number of unpaired electrons in each case. Ion # Unpaired Weak field # Unpaired Strong field (a) Pd4+ (b) Cr3+ (c) Cd 2(d) Ni2 + (e) Co2 +
How would you account for the following?(i) Many of the transition elements are known to form interstitial compounds.(ii) The metallic radii of the third (5d) series of transition metals are virtually the same as those of the corresponding group members of the second (4d) series.(iii) Lanthanoids form primarily +3 ions, while the actinoids usually have higher oxidation states in their compounds, +4 or even +6 being typical.