CHE 110 Lecture Notes - Lecture 10: Valence Bond Theory, Vsepr Theory, Trigonal Planar Molecular Geometry

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blackspider363

7 May 2018

School

Quinnipiac University

Department

Chemistry

Course

CHE 110

Professor

James Kirby

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Chapter 10 Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals

I. Molecular Geometry

a. How do we determine the shapes of simple covalent molecules?

i. The electrons on the central atom determine the shape – number of

atoms bonded to the central atom AND lone pairs of electrons.

ii. Form: AXnEm

1. A = central atom

2. X = atoms bonded to central atoms

3. E = lone pairs on central atom

b. Valence Shell Electron Pair Repulsion Theory (VSEPR) will be applied.

i. Electrons repel each other.

ii. They will be as FAR away as is possible.

iii. 2 directions  linear (180°)

iv. 3 directions  trigonal planar (120°)

v. 4 directions  tetrahedral (109.5°)

vi. 5 directions  trigonal bipyramidal (120° and 180° combined)

vii. 6 directions  octahedral (90°)

c. Observed Shapes for Each VSEPR Class

Class

Shape

Angle

AX2

Linear

180°

AX3

Trigonal Planar

120°

AX2E

Angular (Bent)

<120°

AX4

Tetrahedral

109.5°

AX3E

Pyramidal

<109.5°

AX2E2

Angular (Bent)

<109.5°

AX5

Trigonal Bipyramidal

120°/180°

AX4E

See-Saw

<90°/<120°

AX3E2

T-Shaped

<90°

AX2E3

Linear

180°

AX6

Octahedral

90°

AX5E

Square Pyramidal

<90°

AX4E2

Square Planar

90°

II. Polar Molecules

a. Review from Chapter 9

i. In Chapter 9 we discussed how to determine if a covalent bond is polar.

ii. In this chapter, we will use that information and look at the shape of the

molecule to determine if the molecule is polar covalent.

b. Dipole Moment: an unequal charge distribution caused by differences in

electronegativity values of atoms in covalent bonds

c. Considering Polarity of Molecules

i. Covalent or Ionic?

1. If covalent, continue:

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Related Questions

Draw the Lewis structure for , then answer the following questions:

a. How many valence electrons does this compound have?

b. How many bonded electrons does this compound have?

c. How many lone pairs of electrons does this compound have?

d. How many single bonds does this compound have?

e. How many double bonds does this compound have?

f. What is the electron group arrangement (aka electron pair geometry) (enter one of the following: linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral)?

g. What is the molecular arrangement (aka shape) (enter one of the following: linear, trigonal planar, tetrahedral, trigonal pyramidal, bent, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal, square planar)?

h. Predict the approximate bond angle (enter e.g. 90, 109.5, 120, 180, <109.5, >109.5).

tanjellyfish484

1. The molecular geometry (shape) of the PF4+ ion is __________.

Tetrahedral
Trigonal planar
Trigonal bipyramidal
Octahedral
Trigonal pyramidal

2. Using VSEPR Theory, the predicted Cl-B-Cl bond angle for BCl3 is __________.

180°
107°
120°
109.5°
90°

3. Using VSEPR Theory the molecular geometry (shape) for SF4 is __________.

Square planar
Trigonal bipyramidal
T-shaped
Octahedral
See-saw

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CHE 110 Lecture Notes - Lecture 10: Valence Bond Theory, Vsepr Theory, Trigonal Planar Molecular Geometry

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