Concept explainers
a.
Interpretation: The molecular orbitals for linear and cyclic
Concept introduction: The formation of molecular orbital takes place by mathematical combination of wave functions of atomic orbitals possessing nearly same energies of the atoms involved in bond formation. The number of molecular orbitals formed are always equal to the number of atomic orbitals involved. Thus, the orbitals which have lower energies compared to atomic orbitals are bonding orbital and those which have higher energies compared to atomic orbitals are antibonding orbitals.
b.
Interpretation: The species that is more likely to exist should be determined.
Concept introduction: The formation of molecular orbital takes place by mathematical combination of wave functions of atomic orbitals possessing nearly same energies of the atoms involved in bond formation. The number of molecular orbitals formed are always equal to the number of atomic orbitals involved. Thus, the orbitals which have lower energies compared to atomic orbitals are bonding orbital and those which have higher energies compared to atomic orbitals are antibonding orbitals.
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Inorganic Chemistry
- Which of the following molecules or ions are para-magnetic? What is the highest occupied molecular orbital (HOMO) in each one? Assume the molecular orbital diagram in Figure 9.16 applies to all of them. (a) NO (b) OF (c) O22 (d) Ne2+arrow_forwardThe molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) CN (b) CO (c) BeB (d) BC+ Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.arrow_forwardWhy is L46. Sketch the molecular orbital and label its type (o or T; bond- r antibonding) that would be formed when the following atomic orbitals overlap. Explain your labels. a. +. b. C. d. the ie bond.To Whioh +. 1.arrow_forward
- — Use molecular orbital energy diagrams to determine which of the following is most stable (has highest bond order). (A) C22+ (B). N22+ (C). B2 (D). C22– (E). B22+ —Consider the molecule CH2CF2. A. Draw the best Lewis structure for this molecule. B. Label each bond angle. C. Redraw the shape of the molecule (according to the exacting specifications of your instructor). Draw all dipoles. D. Is the overall molecule polar?arrow_forward3. (1) Show the all shapes of bonding and antibonding molecular orbitals (MOs) by combinations of two p orbitals. (2) Describe the sigma (o) and pi (1) bond for ethylene (C2H4). - H. Harrow_forwarda. Using the molecular orbital diagram, calculate the bond order of F2+. Show show your work or give a brief explanation of the process. b. Do you expect this to have a shorter or longer bond length than F2? Explain your answer. c. Do you expect F2+ to be paramagnetic or diamagnetic? Explain your answer. Please label your answers a-c and place them on separate lines. Be as specific in your explanation as you can.arrow_forward
- XeF + ions can react with Xe gas and other molecules SbF5 to produce + Xe2 ion.a. Write the reaction equation for this reaction!b. Describe the hybridization process for compound SbF5!c. Draw the MO (molecular orbital) schematic for Xe2+. State the bond order magnitude and magnetic properties of the particle!Atomic Number Sb = 51, F = 9arrow_forward6. The energy required (or released) when one electron is captured by a neutral atom or ion is the atomic properties named...? A. lonization Energy B. Electronegativity C. Electron Affinity D. Polarizability E. None of these are correct 7. The orbital hybridization at the central carbon of the linear hydrocarbon allene (CH2=C=CH2) is best described as...? А. 2sp В. 2sp? С. 2sp3 D. 2s?p? E. None of the abovearrow_forward1. 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?arrow_forward
- A. Which of the following statements is TRUE about the neutral nitrogen molecule, N2? Select one: . It is paramagnetic. . Its N–N bond length is shorter than that in the cationic nitrogen molecule ion. . Its calculated bond order is 2. . Its molecular orbital diagram shows that each nitrogen atom has two lone pairs. B. What is the correct complete molecular orbital notation for the N2 molecule? Select one: . σ1s² σ*1s² π2p⁴ σ*2p² . σ2s² σ*2s² π2p⁴ σ*2p² . σ1s² σ*1s² σ2s² σ*2s² π2p⁴ σ2p² . σ1s² σ*1s² σ2s² σ*2s² σ*2p² π2p⁴arrow_forwardBromine trifluoride, BrF3, has a nonzero dipole moment. Indicate which of the following geometries are consistent with this information: a. trigonal planar; b. trigonal pyramidal; c. Tshaped.arrow_forwardb. Explain in molecular orbital terms the changes in H-H inter-nuclear distance that occurs as the molecular H2 is ionized first to H2* and then to H,²*. Explain why the bond order of N2 is greater than that of N2*, but the bond order of O2 is less than that of O2*.arrow_forward
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