Chemistry 122 Exam 1

Front 1

Ionic bonding uses what types of elements?

Back 1

Metal to nonmetal

Front 2

Covalent bonding uses what type of elements?

Back 2

nonmetal to nonmetal

Front 3

Metallic bonding uses what type of elements?

Back 3

metal to metal

Front 4

Metals __ valence e- making them a ___

Back 4

lose.
cation.

Front 5

nonmetals___ valence e- making them an ___

Back 5

gain.
anion.

Front 6

Electronnegativity is

Back 6

the abiltiy of an element to attract e- to itself within a covalent bond

Front 7

Pure covalent bonds (nonpolar bonds) have no ____ moment.

Back 7

dipole

Front 8

Mass % =

Back 8

Mass Solute
______________ x 100
Mass Solution

Front 9

Mole fraction =

Back 9

Mole solute/ mole soulte + mole slovent

Front 10

Molality =

Back 10

Moles of solute/ kg of slovent

Front 11

Molarity =

Back 11

Moles of soute/ L of solution

Front 12

Mass solution =

Back 12

mass solute + mass solvent

Front 13

Molarity containing density =

Back 13

mass solution= d solution x v solution

Front 14

metals lose ______ e- and become ______.

Back 14

valence, cations

Front 15

nonmetals gain ______ e- and become _______.

Back 15

valence, anions

Front 16

Ionic bonding

Back 16

metal to nonmetal

Front 17

covalent bonding

Back 17

metal to metal

Front 18

Nonpolar covalent bonds

Back 18

Bonds between two nonmetal atoms with equal EN.

Front 19

The _______ the EN, the closer bonding e- pair to itself

Back 19

greater

Front 20

polar molecules dissolve ________ molecules.

Back 20

polar

Front 21

nonpolar molecules dissolve __________ molecules.

Back 21

nonpolar

Front 22

intramolecular forces

Back 22

forces between atoms/ ions (within molecules)

Front 23

ion-dipole forces

Back 23

forces between ions and charge centers from polar molecules.

Front 24

dipole-dipole forces

Back 24

attraction of opposite charge poles of two molecules

Front 25

The more _____ the molecule the more attraction between molecules, the _____ the forces.

Back 25

Polar, stronger

Front 26

The more electrons, the more ________.

Back 26

polarizability

Front 27

The greater the ______ the more polarizability.

Back 27

size

Front 28

Down a group, polarizability

Back 28

increases

Front 29

Cross a period (L to R)
polarizability

Back 29

decreases

Front 30

less polarizable

Back 30

cations

Front 31

more polarizable

Back 31

anion

Front 32

The greater ________, the more space and easier for charge to
build up, the greater ________ _______ moment

Back 32

polarizability, instaneous, dipole

Front 33

The more ________ in a
molecule, the ______ size
of a molecule, the _______
polarizability, the greater
_________

Back 33

electrons, bigger, greater, induced dipole

Front 34

London forces (Dispersion forces)

Back 34

Instantaneous dipole – induced dipole forces

Front 35

Exist in ALL covalent molecules

Back 35

London forces (Dispersion forces)
Instantaneous dipole – induced dipole forces

Front 36

The more electrons within a molecule, the stronger _______.

Back 36

london forces

Front 37

The larger the molecule, the stronger ________

Back 37

london (dispersion) forces

Front 38

Occur in all polar molecules

Back 38

dipole-dipole forces

Front 39

The more polarity, the stronger the

Back 39

dipole forces

Front 40

London < dipole if molecules are less

Back 40

polarizable

Front 41

London > dipole if molecules are more

Back 41

polarizable

Front 42

The greater the intermolecular forces, the higher

Back 42

boiling point

Front 43

The greater intermolecular forces, the
more ________ molecules to move around

Back 43

difficult

Front 44

The higher the IM forces, the _______ ΔHvap, the _____ Pvap

Back 44

higher, lower

Front 45

The _______ the T, the ______ Pvap

Back 45

higher, higher

Front 46

A liquid “boils” when its vapor pressure is _______ to an
externally applied pressure

Back 46

equal

Front 47

Line where liquid and solid
phases exist in equilibrium

Back 47

fusion curve

Front 48

Line where liquid and gas
phases exist in equilibrium

Back 48

Vaporization curve

Front 49

Line where solid and gas
phases exist in equilibrium

Back 49

sublimation curve

Front 50

________ occurs when
substance has a triple point higher than 1 atm

Back 50

Sublimation

Front 51

A combination of lowest T, P
where liquid and gas phases
are no longer distinct

Back 51

critical point

Front 52

The temperature on the
vaporization curve where
Pressure is 1 atm

Back 52

normal boiling point

Front 53

The temperature on the fusion curve where Pressure is 1 atm

Back 53

normal melting point

Front 54

the slope of a positive fusion curve m.p. increases as P _______, solid occupies _______ space and has a ______ density.

Back 54

increases, less, greater

Front 55

P increases⇒ V ________, when the slope of fusion curve is positive.

Back 55

decreases

Front 56

m.p. ______ as P increase when the slope of the fusion curve is negative

Back 56

decreases

Front 57

When the slope of the fusion curve is negative, solid occupies _____ space and has _____ density.

Back 57

more, less

Front 58

different molecular forms of the same element

Back 58

allotropes

Front 59

2 C.C
0 lone pairs

Back 59

Linear

Front 60

3 C.C
0 lone pairs

Back 60

Trigonal planar

Front 61

3 C.C
1 lone pair

Back 61

Bent shape

Front 62

4 C.C
0 lone pairs

Back 62

Tetrahedral

Front 63

4 C.C.
1 lone pair

Back 63

Trigonal pyramidal

Front 64

4 C.C.
2 lone pairs

Back 64

Bent

Front 65

5 C.C.
0 lone pairs

Back 65

trigonal bipyramidal

Front 66

5 C.C.
1 lone pair

Back 66

seesaw

Front 67

5 C.C
2 lone pairs

Back 67

T-shape

Front 68

5 C.C
3 lone pairs

Back 68

linear

Front 69

6 C.C
0 lone pairs

Back 69

octahedral

Front 70

6 C.C
1 lone pair

Back 70

Square pyramidal

Front 71

6 C.C
2 lone pairs

Back 71

Square planar