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1. ionization of Cl2 (Cl2 —> Cl2+ + e-) leads to a shortening of the Cl-Cl distance (199 pm in Cl2, 189 pm in Cl2+), why?
2. why the C-O bond distance is nearly identical in CO (113 pm) and CO+ (112 pm)?
3. Derive the MO diagram of a linear C-H (i.e. one carbon atom bonded to one hydrogen atom). Draw out the MOs for orbitals containing electrons Would you expect C-H to behave as a carbocation, carbanion, or radical? Would removal of one electron from C-H to generate C-H+ increase or decrease the bond length between carbon and hydrogen?
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- ST 9C.2- Calculate the energy (in eV) of an antibonding molecular orbital for the molecule XY (with X being more electronegative) given the information below. Note how much closer (a little bit higher) it is to the energy of Y's atomic orbital than X's atomic orbital. a (X) = -11.2 eV a (Y) = -8.8 eV B = -1.0 eV Type your answer...Draw Lewis structures and assign formal charges for the following compounds and ions. Note any resonance forms and explain which resonance form is the most important. Make a note of any other unusual features (such as "this one doesn't work" and why-what are the shortcomings of the model.) 2- CO3²- B₂H6 CO O₂ (paramagnetic) H₂O* LiF IF, NO₂ CNO (include isomers) Al₂Cl61. lewis structure of Cesium 2-hydroxyacetate, HOCH2CO2Cs 2. assign the VSEPR model of the central atom3. Value of the corresponding theoretical angle4. classify 3 of the different bonds around the central atom as ionic or covalent5. draw the complete 3-D structure with respect to the central atom (s)6. draw the lewis structure for another mnolecule or species with a different atomic arrangement
- Draw a Lewis structure for the C3Hg molecule using the connectivity shown in the spacefilling model in the window. • Gray C; white = H; red = 0; blue = N; dark green= Cl; brown = Br; light green = F; purple I; yellow = S; orange = P. Use your drawing to answer the following questions. The total number of electrons in C-H bonds = The number of C-C single bonds = Previous Use your drawing to answer the following questions. The total number of electrons in C-H bonds = The number of C-C single bonds = The number of C=C double bonds = The total number of unshared pairs = NextBecause the structure of a tetrahedrom molecule uses 3 dimensions, a tetrahedron has a bond angle of 109.5 instead of the expected 90 degrees. True or False?2- Which of the TeCl4 and SnCl4 compounds has a dipole moment? Why is that? (Te: VIA, Sn: IVA, Cl: VIIA)
- 32W.) A pi bond is formed by the parallel overlap of s orbitalsX.) Since bromine is from Group VIIA, it needs 7 electrons to complete its octetY.) The bond angle between methane's bond pairs is 109.5⁰Z.) The orbital of f with a shape of y(3x²-y²) contains 14 electronsA.) 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 trueThe molecular orbital diagram for the carbide anion (C₂2-) would have which of the following molecular orbital configurations? (01)²(0*13)²(02)²(0*23)²(π2p)²¹(02p)²(π*2p)² s 4 0)4(020)² ○ (015)²(0*15)²(02)²(0*25) ² (2p)4 0 (015) ² (0*15)²(02)²(0*2s)²(₂p)*(0₂)²(π* 2p) 4 115. Calculate the AH for the decomposition of one mole af nitroglycerin using the standard bond enthalpies of the following reaction (N=O 607 kl/mol): CH N,Og)> + H,Ole) + N2 + Ozte) H O- H HH H 16. Determine the molecular shape and hybridization of the N in the above molecule. 17. How many sigma and pi bonds are present in the molecule of nitroglycerin?
- 3. – For the following chemical structures (1) CIF† (ii) SİF4 (iii) SeBr4 (iv) BrF - For each species, answer the following questions - Predict the bond angles. Explain any deviation from the expected bond angle. - Determine the molecular polarity of these molecules. For a polar one, include the net dipole moment on the 3-D drawings (sketches). - Do (ii) and (iii) have the same molecular shape? Explain why or why not.According to the below Lewis structurerepresentation there are 2 π-electrons between C1and C2 and 2 π-electrons between C3 and C4.This is wrong according to the MO theory.Discuss and illustrate where the 4 π-electronsare actually most likely to be found. CH2 = CH - CH = CH21 2 3 4Would you expect the nonbonding electron-pair domain in NH3 to be greater or less in size than for the corresponding one in PH3>?