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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- 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?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?
- Write the valence-bond wavefunction for the resonance hybrid N2 ↔ N+N− ↔ N2−N2+ ↔ structures of similar energy.(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?The molecular structure of the molecule sulfur cyanide trifluoride, CF3NS, is characterized by the following bond lengths: C-N/ 116 picometers, S-C/ 174 picometers, and S-F/ 160 picometers. Using the observed bond lengths as a guide, draw a realistic lewis structure for sulfur cyanide tirfluoride and assign formal charges to each atom. Are there any resonance structures? Predict the hybridization of the C , N, and S atoms.
- 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.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.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?
- 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.Draw the Lewis structure of HClO₃ (with minimized formal charges) and then choose the appropriate pair of molecular geometries of the two central atoms. Your answer choice is independent of the orientation of your drawn structure.Two of the top 50 chemicals produced in the United States, ammonium nitrate and ammonium sulfate, both used as fertilizers, contain the ammonium ion. Predict the electron-pair geometry and molecular structure of the NH4+ cation.