For each of the following ions, draw diagrams (on a pieceof paper), like the one to the right below, to show orbitaloccupancies for both weak and strong octahedral fields.Indicate (on the table below) the total number ofunpaired electrons in each case. Ion # Unpaired Weakfield # Unpaired Strong field (a) Pd4+ (b) Cr3+ (c) Cd2(d) Ni2 + (e) Co2 +

Here I draw the orbital occupancies for both strong and weak octahedral field

Answered: For each of the following ions, draw…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter20: Chemistry Of Selected Transition Elements And Coordination Compounds

Section: Chapter Questions

Problem 105QRT

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Similar questions

Four different octahedral chromium coordination compounds exist that all have the same oxidation state for chromium and have H2O and Cl as the ligands and counterions. When 1 mole of each of the four compounds is dissolved in water, how many moles of silver chloride will precipitate upon addition of excess AgNO3?
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+
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+
Determine deltao of the following. (a) [Fe(CN)6]3- (b) [CoF6]3-
Consider the octahedral complex [FeBr6] 4−. In water solution it has an absorption peak at 864 nm with a molar absorptivity (ε) of 3.6 L mol-1 cm-1 . (a) What is the energy (in wavenumbers, cm-1 ) of the absorption peak? Show all work. (b) How many valence d electrons does the metal center have? Justify your answer. (c) How many unpaired electrons per molecule would a magnetic susceptibility experiment predict? What would the S number be for this transition metal center? Justify your answers. (d) What electronic transition results from absorption of 864-nm light? (e) Calculate the ligand stabilization energy (in units of ∆o) and units of coulombic (Πc) energy. (f) How would the ligand field strengths (∆o) of [Fe(NH3)6] 2+ and [Fe(bipy)3] 2+ differ from that of [FeBr6] 4−? Why?
Give the electron configuration and the number of unpaired electrons for: (a) Cr3+; (b) Ti4+; (c) Co3+; (d) Ta2+.
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+
(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
Draw appropriate energy diagrams and determine all possible numbers of unpaired electrons in compounds of the following ions within an octahedral crystal field: (a) Mn2 +, (b) Co3 +, (c) Ni2 +, (d) Fe3 +
Draw the crystal field diagram of [W(CO)6]. Determine the (a) Electronic configuration in terms t2geg (b) Number of unpaired electrons (c) Ligand field stabilization energy in terms of ΔO or ΔT
Assign reason for each of the following :(i) Transition elements exhibit paramagnetic behaviour.(ii) Co2+. is easily oxidised in the presence of a strong ligand.
How many electrons are in the valence d orbitals in these transition-metal ions? (a) Os3+

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