4. Introducing n-interactions from our M-Lo-only description. a. Using group theory, derive the full MO diagram for the hypothetical ion ReCla in square planar geometry, showing all the metal valence orbitals and all relevant ligand orbitals. For simplicity, you should disregard the n-donor ability (which is pretty weak) of the chlorines in all questions (here and below), and view each Cl atom as presenting a single a-symmetry orbital toward the metal. Also, Re 6s and 5d orbitals are at -8.76 and -9.70 ev, respectively, consider the CI SALCS at -13.67 ev. Populate your diagram with electrons. Your d-splitting diagram should reflect the relative spacing that you expect from the Angular Overlap Method.

4. Introducing n-interactions from our M-Lo-only description. a. Using group theory, derive the full MO diagram for the hypothetical ion ReCla in square planar geometry, showing all the metal valence orbitals and all relevant ligand orbitals. For simplicity, you should disregard the n-donor ability (which is pretty weak) of the chlorines in all questions (here and below), and view each Cl atom as presenting a single a-symmetry orbital toward the metal. Also, Re 6s and 5d orbitals are at -8.76 and -9.70 ev, respectively, consider the CI SALCS at -13.67 ev. Populate your diagram with electrons. Your d-splitting diagram should reflect the relative spacing that you expect from the Angular Overlap Method.

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...

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3c) Determine the valence electron count of the complex shown below. Use both counting models and compare your results. Assume that the Re-N-O bonding angle is 180°. ON!...Re ORPPh3 Ph 3d) The nitrosyl cation is notorious for its ability to function as a non-innocent ligand. This means that coordinated NO* can affect the oxidation state of the metal to which it is bound. If the central atom M (1) can adopt more than one stable oxidation state and (2) if the metal is not too electronegative, the NO* can withdraw two electrons from M. Does this redox process alter the geometry of the originally linear M-N-O bond and the electron count of the nitrosyl ligand? If yes, describe the changes and the modifications that have to be made when determining the valence electron count.
The ligand-field-stabilization-energies (LFSE) of three pairs of [ML6]** and [ML6]?" complexes are given in the following table. Calculate the difference in LFSE for each pair of reduced and oxidized complexes, that is, the differences in LFSE between [MLs]*" and [MLs]", assuming [ML6]* complexes are low-spin complexes and [ML6J** complexes are high-spin complexes. Arrange the differences in cm' in order of increase in magnitude. A. (cm') [Co(H2O)s]" 16,750 [Co(H;O).J?" [Mn(H20).] 8,400 15,800 [Mn(H2O)s]** 7,850 [Fe(H2O),J** 14,000 [Fe(H2O)«]?* 9,350 A. 5,500 (Fe"/Fe) <9,580 (Mn"/Mn³")< 25,080 (Co"/Co³") B. 5,560 (Fe²"/Fe")<25,080 (Co²"/Co³")< 25,280 (Mn²"/Mn³") C. -20 (Co²"/Co³") <-3,740 (Fe²"/Fe³") < 25,280 (Mn²"/Mn²") D. 24,260 (Fe"/Fe³") < 25,280 (Mn²"/Mn*")< 33,480 (Co"/Co") E. 9,480 (Mn² /Mn³") < 24,260 (Fe²"/Fe³") < 33,480 (Co²"/Co³")
Sketch the orientation of the orbitals relative to the ligandsin an octahedral complex to explain the splitting and the relativeenergies of the dxyand dx2-y2 the orbitals.
Give a clear handwritten answer..
Many transition metal complexes are said to follow the “18-electron rule,” meaning they form particularly stable complexes when the metal + ligand electrons contributing to the MOs add up to a total of 18 electrons. a. Use the full MO diagram for an octahedral metal complex with pi-acidic ligands we derived in class to justify why 18-electrons might be particularly stable. b. Use the 18-electron rule to predict which 1st row transition metal would be most likely to form an octahedral M(CO)6 (Note: there is no charge; the metal retains all its electrons.) c. Qualitatively, how would you expect the CO bond to change when it forms this complex? Would it be stronger, weaker, or the same compared to free CO? (Hint: think about what a ? −???? means and what the orbital does from the perspective of the M–CO interaction as well as the C– O interaction).
i. Identify the oxidation sate of both metal ions. ii. Explain the role of complex charge toward their bio-distribution properties. iii. Contrast their ligand coordination environments with respect to complex stability in vivo. iv. Using the structure of Ceretec only, predict the possible pharmacokinetic effects of substituting the peripheral methyl group (shown in red) with the following R groups; acetic (-CH₂COOH), isopropyl (-CH(CH3)2), and benzyl (-CH2C6H5). 7+ •N:C...... oti ZEO •N:C Tc EN ya •GEN Cardiolite H H3C''' H3C H3C CH3 N Ceretec CH3 CH3
The molecule (CUFJK, has a unique structure (due to jahn-teller distortion) where it has an elongated z-axis in the octahedral structure which changes its point group from O, to Dah. Answer the following questions related to elongated structure of (CuFeJK. a. The oxidation state of Cu: and F: b. Calculate the total number of electrons for [CuFd]: C. Draw the MO diagram for sigma bonding only of (CuFa]Ka including the following i. Correct energy positions for each orbital ii. Symmetry labels including the type of bonding (i.e. the (non-bonding) for an octahedral structure) iii. Fill orbitals with the correct number of electrons
1) What role do the protons play in the transformation of [(SALEN)VO] to [(SALEN)Cl2]? --- Consider the number of anionic charges for all the ligands as well as the charge of the overall complex. Has the oxidation of vanadium changed in this reaction?
1. The molecule listed to the left was originally MX6 where the symmetry was On. After reduction of the metal center the coordination environment changed and the ligands along the Z-axis elongated(hint: this means that the extent of overlap of orbitals that interact with the z-axis point charges would be lesser than the On molecule). Draw the crystal field splitting of both the On symmetry molecule as well as elongated z-axis molecule with symmetry labels.
Draw the full molecular orbital diagram for [Fe(H2O)6] + 2. Each MO must have a drawing of the interaction and the appropriate Mulliken symbol. Approximate ligands down to their lone pairs, and derive the point group from only the geometry created by those donating atoms.
Chemistry can somone answer this 3 part question cleary and in full. thanks Question 4. (i.) Draw a simple molecular orbital diagram for the carbon monoxide (CO) molecule and explain, using an accurate bonding description, how this molecule can act as a ligand within metal carbonyl compounds. (ii.) Explain why CO possesses one infrared (IR) active vibrational mode u(CO), whereas, the di-nitrogen molecule, N2, does not? (iii.) Using your bonding description from part (i.), together with the knowledge that CO ligands contain an IR active vibrational mode, explain the variations in u(CO) cm' values which arise for the following isoelectronic complexes: Compound [V(CO)] Cr(CO)6 [Mn(CO)] CO (uncoordinated) UCO) cm 1860 2000 2095 2143
(d) On problem set 1 we considered the alkene complex [Mn(CO)s(PhzC=CPH2)]. This complex and two related complexes are depicted below. Order these complexes from having the MOST metallocyclopropane character to having the LEAST metallocyclopropoane character. Explain your ranking. *Note: Complexes are drawn as an olefin complex for clarity. This does not imply anything in regards to the electronic structure of the coordinated alkene* 7- Ph Ph CS Ph Ph CNME E Ph Ph CO SCMn sc cs Ph Ph MeNCM MENC čo Ph Ph ČNMe Ph Ph