Answer question 2,3,4,5 and 6 -- - -- -pair of unshared electrons and three bond groups surrounding it.: Br:(Note: single, double, and triple bonds all count as single bond groups)Number of Bond GroupsMolecular ShapeNumber of Unshared ElectronPairs Around the CentralAround Central AtomAtomLinearBentTrigonal PlanarTrigonal PyramidalTetrahedral2. What is the electrostatic charge of all ele ctron groups. either shared (Le. bonds) or unshared?3. Since all electron groups have this same charge, do they attract or repel each other?4. How many unshared electron pairs are present in the carbon atom in CO,?5. Considering your answers to the previous three questions, explain why co, is not bent?6. Explain why H.O is not linear.If you wish to read more about the thegry that explains molecular shapes, here's a link to Che

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Answered: Molecular Shape Number of Unshared…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Covalent Bonding: Orbitals

Section: Chapter Questions

Problem 57E: Use Figs. 4-54 and 4-55 to answer the following questions. a. Would the bonding molecular orbital in...

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For each of the following molecules or molecular ions, give the steric number, sketch and name the approximate molecular geometry, and describe the direction of any distortions from the approximate geometry due to lone pairs. In each case, the central atom is listed first and the other atoms are all bonded directly to it. (a) TeH2 (b) AsF3 (c) PCl4+ (d) XeF5+
Use VSEPR to explain why the HBH bond angle of BH3 is 120°. (Hint: What is one-third of360°?)
Use Figs. 4-54 and 4-55 to answer the following questions. a. Would the bonding molecular orbital in HF place greater electron density near the H or the F atom? Why? b. Would the bonding molecular orbital have greater fluorine 2p character, greater hydrogen 1s character, or an equal contribution from both? Why? c. Answer the previous two questions for the antibonding molecular orbital in HF.
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.
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?
Given the following molecules and/or ions, characterize them according to the formatshown in the table below. The central atom of the molecule/ion is shown in boldface.The central atom or molecules marked with an asterisk (*) do not obey the octet rule. SF6* XeF2* SnCl4 A=Bonding electronsB= Sigma-bondsC =Nonbonding electron pairsD= Hybrid orbitals havingnonbonding electron pairsE =Hybrid orbitals usedF= 3-D structure (NAME)G =Polar (P) or nonpolar (NP) MOLECULE OR ION LEWIS STRUCTURE A B C D E F G
Given the following molecules and/or ions, characterize them according to the formatshown in the table below. The central atom of the molecule/ion is shown in boldface.The central atom or molecules marked with an asterisk (*) do not obey the octet rule. H3O+ A =Bonding electronsB =Sigma-bondsC= Nonbonding electron pairsD =Hybrid orbitals havingnonbonding electron pairsE =Hybrid orbitals usedF= 3-D structure(NAME)G =Polar (P) or nonpolar (NP) MOLECULE OR IONS LEWIS STRUCTURE A B C D E F G
(a) If these three balloons are all the same size, what angleis formed between the red one and the green one? (b) If additionalair is added to the blue balloon so that it gets larger,will the angle between the red and green balloons increase,decrease, or stay the same? (c) Which of the following aspectsof the VSEPR model is illustrated by part (b): (i) Theelectron-domain geometry for four electron domains is tetrahedral.(ii) The electron domains for nonbonding pairs arelarger than those for bonding pairs. (iii) The hybridizationthat corresponds to a trigonal planar electron-domain geometryis sp2. [Section 9.2]
As article in a journal, Inorganic Chemistry, cites both BF3 and PF3 as examples of flat or planar molecules with bond angles of 120 degrees. Another article reports the F-P-F bond angle as 98 degrees. Which report is consistent with the VSEPR model?? Explain
A benzene molecule can be modeled as six carbon atoms arrangedin a regular hexagon in a plane. At each carbon atom, one of threeradicals NH2, COOH, or OH can be attached. How many suchcompounds are possible? (Make no distinction between single anddouble bonds between the atoms.)
what bond angle is predictedfor a trigonal planner molecule? which molecules were trigonal planar? list consists of- CH4, CO2, H2CO, HCN, NH3, H2O, C2H2, C2H4
Which hybirdization(s) can form sigma bonds?

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