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- The four TT molecular orbitals of [Cr(C6H6)2] based on MO 2 to MO 5 are below and form four doubly degenerate pairs, labelled A to D what are their IRREPS? Cr A Bwhat is the reasonance structure of this?Average Bond Dissociation Energies at 298 K Bond Energy, kJ mol1 H-H 432 O=0 495 H-O 467 The tables above contain information for determining thermodynamic properties of the reaction below. 2H,(g) + 02(8) - 2H,O(g) (a) Calculate the AH° for the reaction above, using the table of average bond dissociation energy. (b) Use the table below to calculate the entropy for the formation of water. 2H, + 02 - 2H,O Substance S°(J/mol· K) H2 131.0 H20 69.91 O2 205.0 (c) Calculate the value of AG°298K for the synthesis of water.
- 5. Structure I below is imipramine - an antidepressant drug. Structures II and III are analogs of imipramine. Arrange the compounds in order of increasing logP values (lowest logP first). a) II, III, I b) III, I, II c) III, II, I d) I, III, II 11 -CI III -OHIn the reaction of CN- + H + → HCN; Which boundary orbitals are used? Explain the orbital overlaps of the product according to VBT.4. Amphotericin B is a polyene antifungal agent. In the molecule, 6 C-C single bonds and 7 C=C double bonds alternate along a chain of 14 C atoms; see a schematic of the structure of the molecule below. OH OH HO O OH OH OH OH O,,.. OH HO" ОН OH NH₂ Each C atom contributes 1 p electron to the 77 orbitals in the conjugated system giving 14 electrons that move along the molecule. Assuming an average inter-nuclear distance of 140 pm, and that, in the ground state of amphotericin B, each quantum state is occupied by two electrons, use the particle-in-a-box model to calculate (a) the energy separation between the highest occupied state and the lowest unoccupied state, and (b) the frequency of the radiation required to produce a transition between the two states.
- 13. Which of the following resonance structures could contribute favorably to the bonding of the fulminate anion [CNO]° 1. [:C=N=O:]- 2. [:C-N=O:]- 3. [:C=N-O:] - 4. [:C=N-0:]- 5. [:C-N=O:]- 1, 4 b. 3, 5 1, 2, 4 d. 3, 4, 5 All structures contribute equally а. с. е.28W.) The number of protons is necessary to illustrate covalent bondingX.) A bond contains two electronsY.) Head-to-head overlap of p orbitals result in pi bondZ.) In Madelung's rule, 3s is followed by 4sA.) If all 4 statements are trueB.) If 3 of the 4 statements are trueC.) If 2 of the 4 statements are trueD.) If only 1 of the 4 statements is trueE.) If none of the 4 statements is trueBro 1) The orbital potential energies for the 4s and 4p of Br are -18.65 ev and -12.49ev, respectively. Recall that the H 1s is -13.61ev. The MO diagram for HBr is not exactly the same as HF. Draw the MO diagram for HBr, including energy levels, each orbitals shape, each orbitals character (meaning what atomic orbitals contribute to each M.O. and how much), symmetry labels (e.g. o and t, o* and a*), indicate the HOMO and LUMO, the bond order (show your work), whether the molecule is paramagnetic or diamagnetic. Now
- 23. Given AH+ [(NF3(g)] = -132 kJ mol-¹ and the bond enthalpy (D) data, D(N₂) = 946 kJ mol-¹ and D(F2) = 159 kJ mol-, which of the following statements is/are FALSE? The average N-F bond enthalpy in NF3 is 281 kJ mol-¹. AH+ [(NF3(g)] > AH+ [(NF3(1)] AH+ [(F(8)] = 159 kJ mol-¹ CEECan anyone hand draw the complete MO diagram for [CoCl6]4- Please this is very urgent...Which of the structures below is not expected to contribute to the CO2 resonance hybrid?