6. How orbitals overlap to make a bond (σ bond: head-on overlap, л bond: sideways overlap)7. The shapes of sp, sp², and sp³ hybrid orbitals8. How to assign the hybridization to each atom (including heteroatoms) and how to estimate abond anale (See many examples in tovthook and ham...

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Answered: 6. How orbitals overlap to make a bond…

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 10.110QE

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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?
7.59 What type of hybrid orbital is generated by combining the valence s orbital and all three valence p orbitals of an atom? How many hybrid orbitals result?
• explain how hybridization reconciles observed molecular shapes with the orbital overlap model.
Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?
Compare and contrast the molecular orbital and ionic bonding descriptions of LiF.
Predict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. (a) Na,2+ (b) Mg,2 (c) AI,2 (d) Si,2 (e) p2+ (f) s,2 (g) F,2 (h) Ar,2 40. Predict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. (a) Na22+ (b) Mg22+ (c) Al22+ (d) Si22+ (e) P22+ (f) S22+ (g) F22+ (h) Ar22+
Do lone pairs about a central atom affect the hybridization of the central atom? If so, how?
7.57 What observation about molecules compels us to consider the hybridization of atomic orbitals?
Methylcyanoacrylate is the active ingredient in super glues. Its Lewis structure is (a) How many sigma bonds are in the molecule? (b) How many pi bonds are in the molecule? (c) What is the hybridization of the carbon atom bonded to nitrogen? (d) What is the hybridization of the carbon atom bonded to oxygen? (e) What is the hybridization of the double-bonded oxygen?
Which atomic orbitals overlap to form the bonds in ClF?
Why is the concept of hybridization required in valence bond theory?
3. What hybridization and molecular geometry would you expect for the underlined atom in each of the following (Hint: Drawing Lewis structures is a very good place to start.)? Are these polar or non-polar molecules? If a molecule is polar, indicate the direction of the polarity using the crossed arrow notation. a. CH₂O b. BH4 C. SO3 d. CBr3H e. SCI5I f. AsF5

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6. How orbitals overlap to make a bond (σ bond: head-on overlap, л bond: sideways overlap) 7. The shapes of sp, sp², and sp³ hybrid orbitals 8. How to assign the hybridization to each atom (including heteroatoms) and how to estimate a bond anale (See many examples in tovthook and ham...