Chapter 7

Question 1

VSPER

Answer 1

says electrons want to get as far away from each other in a 3D space

Question 2

Axn

Answer 2

A is central atom, x is # of electron pairs, n positive whole numbers

Question 3

highly symmetric molecule

Answer 3

every angle is the same

Question 4

electron domain geometry

Answer 4

describes only the positions of bonding pairs.

Question 5

molecular geometry

Answer 5

describes positions of all electron pairs.

Question 6

5 electron domain geometries

Answer 6

linear, 2 terminal atoms
trigonal planar, three terminal atoms
tetrahedral: 4 terminal atoms
trigonal bipyramidal: 5 terminal atoms
octahedral: 6 terminal atoms

Question 7

which electron-domain geometry does not exhibit high symmetry

Answer 7

trigonal bipyramidal

Question 8

angle in linear electron domain

Answer 8

180

Question 9

angle in trigonal planar geometry

Answer 9

120

Question 10

angle in tetrahedral geometry

Answer 10

109.5

Question 11

angles in trigonal bipyramidal geometry

Answer 11

90 (b/w top and middle) and 120 (b/w 2 middle atoms)

Question 12

angle in octahedral geometry

Answer 12

octahedral

Question 13

2 bonded pairs molecular geometry

Answer 13

linear

Question 14

2 BP 1 LP mol. geometry

Answer 14

bent

Question 15

2 BP 1 LP mol. geo.

Answer 15

bent

Question 16

2 BP 3 LP molecular geo.

Answer 16

linear

Question 17

3 BP molecular geometry

Answer 17

trigonal planar

Question 18

3 BP 1 LP mol. geometry

Answer 18

trigonal pyramidal

Question 19

3 BP 2 LP mol. geometry

Answer 19

t-shaped

Question 20

4 BP mol. geometry

Answer 20

tetrahedral

Question 21

4 BP 1 LP mol. geometry

Answer 21

seesaw

Question 22

4 BP 2 LP mol. geometry

Answer 22

square planar

Question 23

5 BP mol. geometry

Answer 23

trigonal bipyramidal

Question 24

5 BP 1 LP mol. geometry

Answer 24

square pyramidal

Question 25

6 BP mol. geometry

Answer 25

octahedral

Question 26

why are multiple bonds counted as single pairs?

Answer 26

there is only 1 sigma bond in a 2 or 3 pair.

Question 27

sigma bond

Answer 27

formed by head-on-head overlap. represent single bonds. Only one in double and triple bonds.

Question 28

pi bonds

Answer 28

formed by side-to-side overlap. 1 in double bonds and 2 in triple bonds

Question 29

polarity criteria

Answer 29

1. must have polar bonds | 2. the overall dipole is the vector sum of individual dipoles (so if they cancel, they are not polar)

Question 30

molecules that are usually polar

Answer 30

non-symmetric molecules and when there is the presence of at least one lone pair.

Question 31

types of intermolecular forces

Answer 31

dispersion, dipole-dipole, hydrogen bonding, ion-dipole interaction

Question 32

ion-dipole interaction

Answer 32

happens when there is an ion and a polar substance

Question 33

dispersion forces

Answer 33

happen in everything

Question 34

hydrogen bonding

Answer 34

occur when H is paired with a highly electronegative element (N, O, F) that has at least one lone pair.

Question 35

dipole-dipole

Answer 35

occurs when a polar molecule interacts with another polar molecule

Question 36

what causes nitrogen (a non-polar gas) to become liquid when temp. drops

Answer 36

dispersion forces, heavier things are harder to turn into a gas

Question 37

low boiling point corresponds with what kind of dipole moments?

Answer 37

low dipole moments, and weak attractions

Question 38

valence bond theory

Answer 38

atoms share electrons when an atomic orbital on one atom overlaps with an atomic orbital on another. It balances electron attraction with repulsion from protons.

Question 39

according to valence bond theory, how many bonds would you expect an oxygen atom to form

Answer 39

2

Question 40

problems with valence bond theory

Answer 40

simple diatomic molecules are the only things that can be explained by VB theory. (# of orbitals and degrees do not match p)

Question 41

hybridization

Answer 41

using atomic orbitals in a combination to form hybrid orbitals that have correct geometry to explain bonding in larger molecules.

Question 42

tetrahedral (4 bonds) electron domain hybridization

Answer 42

sp3

Question 43

trigonal planar (3 bonds) electron domain hybridization

Answer 43

sp2

Question 44

linear (2 bonds) electron domain hybridization

Answer 44

sp

Question 45

trigonal bipyramidal (5 bonds) electron domain hybridization

Answer 45

sp3d

Question 46

octahedral (6 bonds) electron domain hybridization

Answer 46

sp3d2

Question 47

is it possible to hybridize just part of the atomic orbitals

Answer 47

yes