Consider the molecular orbital diagram for the H₂* molecule. Select the correct diagram from the options below. (a) E18 (c) E18 E_= a - B V_ V+ E+ = a +3 E = a - B V V E+ = a +3 Els E18 (b) Els (d) E18 E_ V_ V+ E+ E V_ V+ E + = = = = a - B 1 + S a + B 1+ S α- B 1- S a + ß 1 + S E18 E18
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- -10. Which diagram depicts the atomic orbital diagram for the valence electrons of a ground state O-atom before hybridization? (A) 145 444 AL (B) 12 (C) 1000 (0) 4Draw an example for each case, showing the geometry of AXmYn(where X=bonded atomsand Y=lone pair electrons) with the combinations of(a) m=5, n=1 (b) m=4, n=2, (c) m=5, n=0, (d) m=2, n=2 (e) m=3, n=2indicate the approximate values for the indicated bond angles in the following molecules. 1 (a) H 0-N=ö 2. Н 4 H. (b) H C-c=0 H H H (c) H-N-O–H . H. (d) H-C-C=N: H.
- Complete the following table : Lewis atoms: bonds between orbitals/hybrids making e total bond order structure hybridization atoms: type each valence bond: between two atoms C and H make o = sp?(C) + 1s(H) = sp?(C) + sp°(CI) = sp?(C) + sp?(0) = p(C) + p(0) H 1s C and H = 1 :0: C sp? C and Cl make o C and Cl = 1 CI sp3 C and O make o C and O = 2 O sp? C and O make n Cl and H make (CI) + (H) Cl andH = H-CI-H N. N and N make _(N) + (N) N and N = N=N N N and N make (N) + _(N) N and H = H N and H make (N) + (H) N N and C make (N) + (C) N and C = N and C make (N) + (C) : NEC-0: N and C make _(N) + (C) C and O = C and O make _(C) + (0) II II II I.Acetylsalicylic acid, better known as aspirin, has the Lewisstructure (a) What are the approximate values of the bond angles labeled1, 2, and 3? (b) What hybrid orbitals are used about thecentral atom of each of these angles? (c) How many s bondsare in the molecule?H- H a. What orbitals are overlapping to form each of the following bonds? b. Classify whether the bond formed is sigma or pi? H 3 (a) c=c H H C H H cH 10 H 1 A W N 3 4 5 6 7 8 9 10 (b)
- Indicate whether each statement is true or false. (a) s orbitalscan only make σ or σ* molecular orbitals. (b) The probabilityis 100% for finding an electron at the nucleus in a π* orbital.(c) Antibonding orbitals are higher in energy than bondingorbitals (if all orbitals are created from the same atomic orbitals).(d) Electrons cannot occupy an antibonding orbital.The strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy.(A) N-N(B) N≡N ...... (A,B) ____(C) C=N(D) C≡N ...... (C,D) _____(a) What orbitals are overlapping to form each of the following bonds? b) Classify whether the bond formed is sigma or pi? (a) (b) H. : 3 1 2 H 4 5 6 7 10 H 8 9 10
- esonance X MKbWpeF2TQ5uxk ✓ Norton - My Sub X Please solve all the questions presented Value: 1 Which of the structures (if any) is least probable? a) b) # 6/8 o Mail-Miche O a. a O b. b О с. с O d. all are equally probable S 5: Š: ✓ Norton - My SubWhich compound in each of the following pairs would you expect to have the greaterdipole moment μ? Why?(a) HF or HCl (d) CHCl3 or CCl3F(b) HF or BF3 (e) CH3NH2 or CH3OH(c) (CH3)3CH or (CH3)3CCl (f) CH3NH2 or CH3NO2Acetyl salicylic acid (aspirin), the most widely used medi-cine in the world, has the Lewisstructure at right. (a) What is the hybridization of each C and each O atom? (b) How many localized π bonds are present? (c) How many C atoms have a trigonal planar shape around them? A tetra hedral shape?