Consider each of the following molecules and/or ions. Give the hybridization for the central atom in each case, and alsogive the molecular geometry. Ignore any distortions in the geometry due to non-equivalent terminal atoms.moleculecentral atomor ionhybridizationfor central atommoleculargeometry(a)PO43-P(b)CH3C(c)NOBrN(d)CO2C(e)CO32-C

Steric number helps predict the hybridization, molecular geometry, and electron geometry of a…

Answered: Consider each of the following…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter20: The Representative Elements

Section: Chapter Questions

Problem 68E: Give the Lewis structure, molecular structure, and hybridization of the oxygen atom for OF2. Would...

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Give the Lewis structure, molecular structure, and hybridization of the oxygen atom for OF2. Would you expect OF2 to be a strong oxidizing agent like O2F2 discussed in Exercise 61?
What is the hybridization of the central atom in each of the following? (a) BeH2 (b) SF6 (c) PO43 (d) PCl5
For each of the following, indicate the hybridization of the nitrogen atom (for N3-. the central nitrogen). (a) N2F4 (b) NH2- (C) NF3 (d) N3-
Acrylonitrile, C3H3N is the building mer Orlon. Its Lewis structure is What is the hybridization of nitrogen and of the three numbered carbon atoms?
Sketch the resonance structures for the N2O molecule. Is the hybridization of the N atoms the same or different in each structure? Describe the orbitals involved in bond formation by the central N atom.
Bromine forms a number of oxides of varying stability. (a) One oxide has 90.90% Br and 9.10% O. Assuming its empirical and molecular formulas are the same, draw a Lewis structure of the molecule and specify the hybridization of the central atom (O). (b) Another oxide is unstable BrO. Assuming the molecular orbital diagram in Figure 9. 16 applies to BrO, write its electron configuration (where Br uses 45 and 4p orbitals). What is the highest occupied molecular orbital (HOMO) for the molecule?
Draw a Lewis electron dot diagram for each of the following molecules and ions. Formulate the hybridization forthe central atom in each case and give the moleculargeometry.(a) CCl4(b) CO2(c) OF2(d) CH3-(e) BeH2
(a) What are the C— C— C bond angles in diamond?(b) What are they in graphite (in one sheet)? (c) Whatatomic orbitals are involved in the stacking of graphitesheets with each other? The solid wedges in the figure indicate bonds from carbonthat come out of the plane of the page; the dashed wedgesindicate bonds that lie behind the plane of the page.(a) What is the hybridization of orbitals at each carbonatom? What angles do you expect between the bonds?(b) Now imagine that the polymer is polypropylenerather than polyethylene. Draw structures for polypropylenein which (i) the CH3 groups all lie on thesame side of the plane of the paper (this form is calledisotactic polypropylene), (ii) the CH3 groups lie on alternatingsides of the plane (syndiotactic polypropylene),or (iii) the CH3 groups are randomly distributedon either side (atactic polypropylene). Which of theseforms would you expect to have the highest crystallinityand melting point, and which the lowest? Explainin terms of…
For each of the following molecules, indicate the hybridization: (a) carbon dioxide (CO2) central O hybridization (b) formaldehyde (COH2) central C hybridization (c) phosphorous dioxide (PO2) central P hybridization (d) phosphate ion (PO43-) central P hybridization
For which of the following molecules or ions does the followingdescription apply? “The bonding can be explained usinga set of sp2 hybrid orbitals on the central atom, with one ofthe hybrid orbitals holding a nonbonding pair of electrons.”(a) CO2(b) H2S(c) O3(d) CO32 -(e) More than one of the above
The Electron pair geometry, molecular geometry and Hybridization for NCl3 is (a) Tetrahedral, Trigonal pyramidal, sp^3 (b) Trigonal planar, Bent, sp^2 (c) Bent, Trigonal planar, sp^2 (d) None
(a) Sketch the molecular orbitals of the H2- ion and draw itsenergy-level diagram. (b) Write the electron configuration ofthe ion in terms of its MOs. (c) Calculate the bond order inH2-. (d) Suppose that the ion is excited by light, so that anelectron moves from a lower-energy to a higher-energy molecularorbital. Would you expect the excited-state H2- ion to bestable? (e) Which of the following statements about part (d) is correct: (i) The light excites an electron from a bonding orbitalto an antibonding orbital, (ii) The light excites an electronfrom an antibonding orbital to a bonding orbital, or (iii)In the excited state there are more bonding electrons thanantibonding electrons?

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