(a)
Interpretation: The
Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.
Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.
To determine: The correct arrangement for
(b)
Interpretation: The
Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.
Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.
To determine: The Lewis structure of
(c)
Interpretation: The
Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.
Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.
To determine: The description of multiple bonding in
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Chapter 9 Solutions
Chemistry
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- Consider the molecules PF3 and PF5. A. Draw the Lewis electron-dot structures for PF3 and PF5 and predict the molecular geometry. B. Is the PF3 polar or non-polar and why? C. On the basis of bonding principles, predict whether each of the following compounds exists. In each case, explain your prediction. (i) NF5 (ii) AsF5arrow_forward27. Which of the following statements is/are true? Correct the false statements. a. It is impossible to satisfy the octet rule for all atoms in XeF2. b. Because SF, exists, OF, should also exist, because oxy- gen is in the same family as sulfur. c. The bond in NO* should be stronger than the bond in NO. d. As predicted from the two Lewis structures for ozone, one oxygen-oxygen bond is stronger than the other oxygen- oxygen bond.arrow_forward5.a. Explain how the lattice energy of an ionic compound such as KCI can be determined using the Born-Haber cycle. On what law is this procedure based? How do the ionization energy and the electron affinity determine whether atoms of elements will combine to form ionic compounds? b. 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 H2²*. Explain why the bond order of N2 is greater than that of N2*, but the bond order of 02 is less than that of O2*.arrow_forward
- This question is related to valence bond theory. a. Explain the assumptions made in bonding models under valence bond theory. What best describes bonding under these models? b. Draw the Lewis structure of SO2. Identify bonds in the moldule as either sigma or pi bonds. Draw orbital diagrams for ground state S and O atoms. Use these orbital diagrams determine the geometry of SO2 using valence bond theory (hint: SO2 must be descried using hybrid atomic orbitals. In other words, which orbitals on which atoms overlap to give rise to which bonds? C. d. Explain why valence bond theory does not adequately describe the bonding in SO2, even though it accurately predicts the geometry/bond angle.arrow_forward28. For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (in- cluding bond angles), and give the expected hybrid orbitals for sulfur. a. SO, b. SO, c. S,0,2- s- d. S,0,2-0-$-O–0–$–0 e. SO,²- f. SO,²- g. SF, h. SF, i. SF, j. F,S–SF k. SF,*arrow_forwardThe ion PCI4 has a structure that would be described as? a. octahedral d. T-shaped b. Square planar c. trigonal pyramidal e. see-saw (This question is asking molecular shape)arrow_forward
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