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Chemistry: Principles and Practice

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.59QE

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Question

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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Write the valence-bond wavefunction for the resonance hybrid N2 ↔ N+N− ↔ N2−N2+ ↔ structures of similar energy.
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.
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).
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.
Calculate the formal charges of all of the atoms in each of the following molecules. Part A CO Enter the charge in the order in which the atoms are numbered. Seperate each charge with a comma. Make sure to include the appropriate "+" or "-" if the charge is not "O. :C=0: Πν ΑΣφ
Consider a molecule AB6, where element A has 6 valence electrons and B has 7 valence electrons. If the ΔEn for each bond = 1.2, predict the shape, bond hybridization and polarity (polar or non-polar) of the molecule. Your answer should follow the format: a) number of total electrons for bonding; b) Steric Number and Lone Pairs; c) name of shape based on the VSEPR chart, d) bond hybridization and e) molecular polarity.
There are three unique molecules (excluding ring structures) that have the molecular formula C₂H3N. Draw a Lewis structure for each molecule. Hint: In each structure, each atom has a formal charge of zero. Arrange the following in order of decreasing bond strength. NO NO₂ NO3
alculate the formal charge (example +1) of chlorine in the most stable form of the perchlorate anion (Hint: draw its Lewis structure first):
Complete the following Lewis structures for the CICN molecule by adding dots for unshared valence electrons and indicating formal charges. Evaluate the importance of each structure as a contributor to a resonance hybrid. Cl – C = N, Cl = C – N, Cl = C = N
According to Huckel theory, what is the difference in total energy between the anion (C6H6) and the dication (C6H6)2+ of Benzene? In your work, explicitly state which orbitals are occupied in case of the anion and the dictation and what the total energy of each of the two ions is. The total energy difference is defined as AE = Eanion Ea dication· O 2a – 23 O 3a + B O a + B O 2a + 28 3a - B

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