(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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EBK CHEMISTRY: AN ATOMS FIRST APPROACH
- Lets look more closely at the process of hybridization. (a) What is the relationship between the number of hybrid orbitals produced and the number of atomic orbitals used to create them? (b) Do hybrid atomic orbitals form between different p orbitals without involving 5 orbitals? (c) What is the relationship between the energy of hybrid atomic orbitals and the atomic orbitals from which they are formed?arrow_forwardGive the expected hybridization of the central atom for the molecules in Exercises 21 and 22.arrow_forwardA paper published in the research Journal Science in 2007 (S. Vallina and R. Simo, Science, Vol. 315, p. 506, January 26, 2007) reported studies of dimethylsulfide (DMS), an important green-house gas that is released by marine phytoplankton. This gas represents the largest natural source of atmospheric sulfur and a major precursor of hygroscopic (i.e., cloud-forming) particles in clean air over the remote oceans, thereby acting to reduce the amount of solar radiation that crosses the atmosphere and is absorbed by the ocean. (a) Sketch the Lewis structure of dimethylsulfide, CH3SCH3, and list the bond angles in the molecule. (b) Use electronegativities to decide where the positive and negative charges lie in the molecule. Is the molecule polar? (c) The mean seawater concentration of DMS in the ocean in the region between 15 north latitude and 15 south latitude is 2.7 nM (nanomolar). How many molecules of DMS are present in 1.0 m3 of seawater?arrow_forward
- 5.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_forwardConsider 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_forwardWhich of the following statements true about the bonds in the figure above? a. Only sigma bonds use hybridized orbitals to overlap in forming the bonds b. Sigma bonds form from the end-to-end overlap of two hybridized s and p orbitals c. Pi bonds for from the side-to-side overlap of hybridized sp, sp2, sp3 orbitals d. The maximum number of sigma and pi bonds between two atom are different, but the energy level of the two bondsarrow_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
- 2. Explain the following: a. Ethylene, C₂H4, is a planar molecule, but hydrazine, N₂H₂, is not. b. ICl, is linear, but NH₂ is bent. c. Of the compounds mercury (II) cyanate, Hg(OCN)2, and mercury(II) fulminate, Hg(CNO)2, one is highly explosive, and the other is not.arrow_forwardWhich one of the following species is paramagnetic? (Consider the necessary molecular orbitals) Li Be "Lanthanide series57" ** Actinide series Select one: O a. H2 O b. N Oc O2 O d. F2 品 に8Y ”山 あ非arrow_forwardIn reference to the following figure, which of the following statements is not true? a. The bond in the hydrogen molecule is formed by the overlap of 1s atomic orbitals. b. The overlap of electron waves represented by the atomic orbitals may result in constructive (in-phase) or destructive (out-of-phase) interference. c. In-phase overlap between two 1s orbitals results in a new orbital having higher energy than either of the s orbitals. This new orbital concentrates the electron probability between the two nuclei. d. Out-of-phase overlap between two 1s orbitals results in a new orbital having higher energy than either of the s orbitals. This new orbital places most of the electron probability to the left and right of the two nuclei. e. All of the above statements are true.arrow_forward
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