How many o bonds and bonds are in the molecule below? H H NH H. o bonds T bonds Identify the molecular geometry for selenium dibromide. O T-shaped O seesaw O octahedral O trigonal bipyramidal O square planar O square pyramidal O trigonal planar O trigonal pyramidal O tetrahedral O linear O bent Determine the chemical formula for the following molecules, then build them in molview.org . Fill in the table with the appropriate MolView bond angles. MolView bond angle Molecule Chemical formula (*) Methane Ammonia Water

How many o bonds and bonds are in the molecule below? H H NH H. o bonds T bonds Identify the molecular geometry for selenium dibromide. O T-shaped O seesaw O octahedral O trigonal bipyramidal O square planar O square pyramidal O trigonal planar O trigonal pyramidal O tetrahedral O linear O bent Determine the chemical formula for the following molecules, then build them in molview.org . Fill in the table with the appropriate MolView bond angles. MolView bond angle Molecule Chemical formula (*) Methane Ammonia Water

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter6: Quantum Mechanics And Molecular Structure

Section: Chapter Questions

Problem 61P: Discuss the nature of the bonding in the nitrite ion (NO2) . Draw the possible Lewis resonance...

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Sketch the molecular orbital and label its type ( or , bonding or antibonding) that would be formed when the following atomic orbitals overlap. Explain your labels. a. b. c. d.
Give the expected hybridization of the central atom for the molecules in Exercises 21 and 22.
The antibiotic thiarubin-A was discovered by studying the feeding habits of wild chimpanzees in Tanzania. The structure for thiarubin-A is a. Complete the Lewis structure, showing all lone pairs of electrons. b. Indicate the hybrid orbitals used by the carbon and sulfur atoms in thiarubin-A. c. How many and bonds are present in this molecule?
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?
What hybrid orbitals would be expected for the central atom in each of the following molecules or ions?
For each of the following molecules, complete the Lewis structure and use the VSEPR model to determine the bond angles around each central atom. Note that the drawings are only skeleton structures and may depict the angles incorrectly.
Give the expected hybridization of the central atom for the molecules or ions in Exercises 81 and 87 from Chapter 3.
Discuss the nature of the bonding in the nitrite ion (NO2) . Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central nitrogen atom, and the geometry of the ion. Show how the use of resonance structures can be avoided by introducing a de-localized MO. What bond order does the MO model predict for the NO bonds in the nitrite ion?
Carbon monoxide (CO) forms bonds to a variety of metals and metal ions. liS ability to bond to iron in hemoglobin is the reason that CO is so toxic. The bond carbon monoxide forms to metals is through the carbon atom: MCO a. On the basis of electronegativities, would you expect the carbon atom or the oxgen atom to form bonds to metals? b. Assign formal charges to the atoms in CO. Which atom would you expect to bond to a metal on this basis? c. In the MO model, bonding MOs place more electron density near the more electronegative atom. (See the HF molecule in Figs. 4-54 and 4-55.) Antibonding MOs place more electron density near the less electronegative atom in the diatomic molecule. Use the MO model to predict which atom of carbon monoxide should form bonds to metals.