2. For each of the following compounds, 1) write the formal oxidation state of the transition metal and 2) the corresponding number of d electrons. 3) State whether or not each one is likely to be stable enough to be characterized. (a) [Re(CO)5] (b) [Cr(η6 -C6H6)2] (c) [Mo(CO)3(PPh3)3] (d) [Fe(η2 -C2H4)(CO)4] (e) [Zr(η5 -C5H5)Cl(OH)] (f) [Co(η5 -C5H5)2]
3. Identify the first-row transition metal (M) that follows the 18-electron rule for each of the following compounds (show how you arrived at your answer): (a) [M(CO)2(PPh3)2] − (b) [M(η 4 -C4H4)(CO)3] (c) [M(η 5 -C5H5)(CO)3]2 (assume single M−M bond)
4. Assuming that each of the following obeys the 18-electron rule, determine the number of metal-metal bonds in each complex. Show how you arrived at your answer and sketch a possible structure in each case. (a) [Mn(η5 -C5H5)(CO)2]2 (b) μ-CO-[Fe(η4 -C4H4)(CO)2]2 (c) (μ-Br)2-[Mn(CO)4]2
5. When [Mo(η 5 -C5H5)(CO)3]2 is heated, it loses two CO ligands to become [Mo(η5 -C5H5)(CO)2]2, and the energies of the CO stretches change from 1960 cm−1 and 1915 cm−1 to 1859 cm−1 and 1819 cm−1 . The Mo-Mo bond length also shortens by 80 pm. Suggest plausible chemical structures for each of the compounds, and explain the change in energy of the CO stretches.
6. First, briefly explain the following trend for the CO stretching energy. Next, predict the trend in the M-C and C-O bond lengths. M(CO)6 ν(CO), cm−1 [W(CO)6] 1977 [Re(CO)6] + 2085 [Os(CO)6] 2+ 2190 [Ir(CO)6] 3+ 2254
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
2. For each of the following compounds, 1) write the formal oxidation state of the transition...
2. For each of the following compounds, 1) write the formal oxidation state of the transition metal and 2) the corresponding number of d electrons. 3) State whether or not each one is likely to be stable enough to be characterized. (a) [Re(CO)5] (b) [Cr(η6 -C6H6)2] (c) [Mo(CO)3(PPh3)3] (d) [Fe(η2 -C2H4)(CO)4] (e) [Zr(η5 -C5H5)Cl(OH)] (f) [Co(η5 -C5H5)2] 3. Identify the first-row transition metal (M) that follows the 18-electron rule for each of the following compounds (show how you arrived at...
Q1) For each of the following compounds, determine the formal oxidation state of the transition metal and the corresponding number of d electrons. State whether each one is likely to be stable enough to be characterized. (1) [Re(CO)5] (2) [HFe(CO)4]- (3) ((ŋ6-C5H5)2Fe) (4) ((ŋ6-C6H6)2Cr) (5) ((ŋ5-C5H5)ZrCl(OCH3) (6) (IrCl(PPh3)3) (7) (Mo(CO)3(PPh3)3) (8) (Fe(CO)4(C2H4)) (9) (W(CO)5Cl)- (10) Ni(CO)4)Q2) Use the 18-electron rule to predict the number of carbonyl ligands, n, in each of the following complexes: (1) [Cr(CO)n] (2) [Fe(CO)n(PPh3)2)] (3) [Mo(CO)n(PMe3)3] ...
5. (a) When [Mo(?5 -C5H5)(CO)3]2 is heated, it loses two CO ligands to become [Mo(?5 -C5H5)(CO)2]2, and the energies of the CO stretches change from 1960 cm?1 and 1915 cm?1 to 1859 cm?1 and 1819 cm?1 . The Mo-Mo bond length also shortens by 80 pm. Suggest plausible chemical structures for each of the compounds, and explain the change in energy of the CO stretches. (b) Explain the following trend in the energy of the CO stretch. Predict the trend...
Identify the first-row transition metal (M) that follows the 18-electron rule for each of the following compounds (show how you arrived at your answer): (a) [M(CO)2(PPh3)2] (c) [M(n5-CsHs)(CO)3]2 (assume single M-M bond) (b) [M(nt-C4H4)(CO)3] Identify the first-row transition metal (M) that follows the 18-electron rule for each of the following compounds (show how you arrived at your answer): (a) [M(CO)2(PPh3)2] (c) [M(n5-CsHs)(CO)3]2 (assume single M-M bond) (b) [M(nt-C4H4)(CO)3]
For each of the following transition metal complexes, determine the oxidation state of the metal, its coordination number, and the number of d electrons on that metal. (a) RuO4 (b) (CO(NH3).]3+ (c) [Cr(H2O).]8+ (d) Cr(H2O)3Cl2 (e) [Fe(H2O).]3+ (1) (Co(NH3).]2+ (9) MOCI (h) (Pt(CN)4]2- () [Mn(H2O).]2+ (1) Re(CO).Br (k) (Ag(CN 2] (1) [ReH9]?
In which of the following compounds does the transition-metal have the highest oxidation number? In which of the following compounds does the transition-metal have the highest oxidation number? K4[Mn(CN)6] Na[Ag(CN)2] K2[PtCl6] [Co(NH3)4Cl2] Rb3[MoO3F3]
choose the correct answer C-O in [Fe(CO)6]2+ have stretching bands higher in energy than those in free CO? Due to positively transition metal decreases the electrons toward oxygen. As result of that, bond between oxygen and carbon become stronger and the stretching of bond requires lower frequency. Due to positively transition metal decreases the electrons toward oxygen. As result of that, bond between oxygen and carbon become weaker and the stretching of bond requires higher energy. Due to positively transition...
Section B The following organometallic compounds are stable and have a second-row transition metal at their centre. Find out the metal and its formal oxidation state. Ph Ph. OC CO -M -M OC со [Nb, +1] [Nb, +2] [Zr, +2] O [Zr, +1] CI CF3 [Cd, + 4] O [Cd, + 2] O (Cd, +6] O [Cd, + 5] Ph HoM Ph OC со O [Tc, +2] O [Mo, +1] O [TC, +1] O [Mo, +2] Ph-pin..M.IPCy3 Ph + H...
2.) Give the point group assignment of the following transition metal compounds: a.) trans- [PtCl2Br2]the ion has a square planar shape with Pt as the central atom b.) [CO(NH3)sBr]? the ion has an octahedral shape with Co as the central atom. Treat the NH3 groups as a large, spherical atom attached to the Co. c.) [Fe(CO)s) the compound is a square pyramidal shape, with Fe as the central atom. Assume that the Fe-C-O bond angle for each attached CO is...
For each of the transition metal ions : (a) [Fe(H2O)4 ]3+ (b) [Mn(H2O)4 Cl2 ]+ (c) [Re(H2O)4 Cl2 ]+ (d) [Co(NH3)2 (en)2]2+ (i) Draw the structure of each transition metal complex. (ii) Determine the number of d electrons (iii) Draw the arrangement of d electrons in the ground state (iv) Calculate the LFSE (in units of deltao or deltaT ) for each complex