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VSEPR Model and Valence Bond Theory

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Chapter 11 Homework: VSEPR and Valence Bonding

1.Select all the polar molecules.

a. BrF5
b. BF3
c. PF6−
d. IF4−
e. NH4+
f. CH2F2

Select all the polar molecules.

a. I3−
b. IF3
c. TeF42−
d. SeF4
e. ClO3−
f. ClO4−

What is the molecular geometry for AsCl4+?

a. trigonal planar
b. tetrahedral
c. square planar
d. see-saw
e. trigonal pyramidal
f. trigonal bipyramidal

What is the molecular geometry for I3−?

a. trigonal bipyramidal
b. tetrahedral
c. bent
d. trigonal planar
e. trigonal pyramidal
f. linear

Select all the molecules that have tetrahedral molecular geometry.

a. BF4−
b. CHCl3
c. SF4
d. XeF4
e. TeF42−
f. PO43−

What hybrid orbitals are used by the central atom in IF3?

a. sp2
b. sp3
c. sp3d2
d. sp3d
e. sp

Select all the polar molecules.

a. ClO3−
b. BF3
c. PH3
d. ClF3
e. I3−
f. SO3

What is the molecular geometry for IF2+?

a. bent
b. T-shaped
c. tetrahedral
d. see-saw
e. linear
f. trigonal planar

What hybrid orbitals are used by the central atom in I3−?

a. sp3
b. sp2
c. sp3d2
d. sp3d
e. sp

What is the molecular geometry for ClO2−?

a. tetrahedral
b. bent
c. linear
d. trigonal bipyramidal
e. trigonal pyramidal
f. trigonal planar

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https://brainmass.com/chemistry/organic-chemistry-bonding/vsepr-model-and-valence-bond-theory-264339

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This solution explains how to find the VSEPR geometry for a variety of molecules.

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VSEPR model to predict the probable shapes

1. Use the VSEPR model to predict the probable shapes of (a) PCl4+, (b) PCl4-, (c) AsCl5.

2. Give balanced chemical equations for each of the following reactions.
(a) Oxidation of P4 with excess oxygen, (b) reaction of the product from part (a) with excess water, (c) reaction of the product from part (b) with a solution of CaCl2 and name the product.

3. State whether the following oxides are acidic, basic, neutral, or amphoteric: CO2, P2O5, SO3, MgO, K2O, Al2O3, CO.

4. Rank the following species from the strongest reducing agent to the strongest oxidizing agent: SO42-, SO32-, O3SO2SO32-.

5. SF4 reacts with BF3 to form [sF3] [BF4]. Use VSEPR theory to predict the shapes of the cation and anion.

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