Use molecular orbital diagrams to rank the bond energies of the following diatomic species from weakest to strongest: He₂, He₂+, He₂2+ Note: enter He₂2+ as He2(2+) in the answer field.
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- Construct the molecular orbital diagram for SrCl. Would yo u expect the bond length of SrCl+ to be longer or shorter than that of SrCl? Explain and elaborate.Describe the structure of a P2 molecule in valence-bond terms. Why is P4 a more stable form of molecular phosphorus than P2?Based on average bond enthalpies, would you expect a photon capable ofdissociating a C¬Cl bond to have sufficient energy to dissociate a C¬Br bond?
- (a) How does a polar molecule differ from a nonpolar one? (b) Atoms X and Y have different electronegativities. Will the diatomic molecule X—Y necessarily be polar? Explain. (c) What factors affect the size of the dipole moment of a diatomic molecule?Write the valence-bond wavefunction for the resonance hybrid N2 ↔ N+N− ↔ N2−N2+ ↔ structures of similar energy.1)Using molecular orbital theory, determine the electronic structure of the first excited electronic state of N2. What differences are expected in the properties of the excited state of N2 compared with the same properties of the ground state? 2)Describe the bonding (including σ and п bonds) on an N atom in dinitrogen difluoride, N2F2, using valence bond theory. 3)Magic numbers are associated with protons and neutrons in a nucleus. State the magic numbers for protons and neutrons, and give two evidences to support the existence of these magic numbers
- Describe the location of the maximum electron density of σ- and π-bonds. How is the difference in the spatial arrangement of the electron density of these bonds reflected on their strength?9. Resonance and hybridization questions. (a) Write valence bond wavefunction for the resonance hybrid HF + H'F (allow for different contributions for each structure). (b) Write valence bond wavefunction for the resonance hybrid CO + Co* + C*o' (allow for different contributions for each structure).Identify the likely structure dipole moment of the theoretical molecule C(OH)3Cl. Provide a hand-drawn illustration showing the molecule's 3D structure and dipole moment if applicable.
- There are two main types of covalent bond breakage. In ho-molytic breakage , each atom in the bond gets one of the shared electrons. In some cases, the electronega-tivity of adjacent atoms affects the bond energy. In heterolytic breakage, one atom gets both electrons and the other gets none;thus, a cation and an anion form. (a) Why is the C−C bond in H₃C−CF₃(423 kJ/mol) strongerthan that in H₃C−CH₃(376 kJ/mol)?(b) Use bond energy and any other data to calculate the heat ofreaction for the heterolytic cleavage of O₂.Calculate the (molar) energy of electrostatic repulsion between two hydrogen nuclei at the separation in H2 (74.1 pm). The result is the energy that must be overcome by the attraction from the electrons that form the bond. Does the gravitational attraction between the nuclei play any significant role? Hint: The gravitational potential energy of two masses is equal to −Gm1m2/r; the gravitational constant G is listed inside the front cover.Which of the following bonds are polar? (a) B¬F,(b) Cl¬Cl, (c) Se¬O, (d) H¬I. Which is the moreelectronegative atom in each polar bond?