Chemistry: Chapter 17 & 18.1 - Solutions

Front 1

allows for 4 hydrogen bonds

Back 1

tetrahedral

Front 2

with 2 lone e-pairs allows for polarity

Back 2

bent

Front 3

gives the solid phase less density than the liquid phase

Back 3

hexagonal

Front 4

Effects of hydrogen bonding: ___ surface tension, ___ boiling and melting point, ___ specific heat capacity, ___ heat of vaporation

Back 4

high; high; high; high

Front 5

the amount of heat needed to raise the temperature of 1g of water to 1C

Back 5

Specific Heat Capacity

Front 6

The specific heat capacity of water:

Back 6

4.18 Joules

Front 7

the amount of energy needed to convert 1g of a substance from a liquid to a gas at the boiling point

Back 7

heat of vaporization

Front 8

Something is considered soluble when ___g can dissolve in ___ml of solvent.

Back 8

.1 ; 100

Front 9

Intermolecular bonding is described as:

Back 9

"like dissolves like"

Front 10

H2O, Sugar, Salt, NaNO3, and alcohol are examples molecules of ___ and ___ intermolecular forces.

Back 10

polar; ionic

Front 11

Oils, grease, gasoline, benzene, and CCl4 are all:

Back 11

nonpolar

Front 12

C6H12 is:

Back 12

Hexane

Front 13

when a solute particle is surrounded by the solvent

Back 13

solvation

Front 14

C6H12O6:

Back 14

glucose

Front 15

C12H22O11

Back 15

sucrose

Front 16

A solid in a liquid is an _________ force.

Back 16

induced dipople-induced dipole

Front 17

incapable of being mixed

Back 17

immiscible

Front 18

What is the chemical formula for methanol?

Back 18

CH3OH

Front 19

What is the chemical formula for ethanol?

Back 19

C2H5OH

Front 20

What is the chemical formula for propanol?

Back 20

C3H7OH

Front 21

What determines solubility?

Back 21

The length of the hydrocarbon chain.

Front 22

Why is Ammonia extremely soluble in water?

Back 22

because of hydrogen bonding

Front 23

Solubility is ___ dependent.

Back 23

Pressure

Front 24

S1/P1= ?

Back 24

S2/P2

Front 25

___ will always float on water.

Back 25

Hydrocarbon

Front 26

The hydrocarbon layer is the ___.

Back 26

organic layer

Front 27

For a separate solute, the heat is ___.

Back 27

+

Front 28

For a separate solvent, the heat is ___.

Back 28

+

Front 29

For the solute and solvent combined, the heat is ___.

Back 29

-

Front 30

What is enthalphy?

Back 30

heat

Front 31

The heat of a solution may be + or - depending on _____ energy.

Back 31

bonding

Front 32

The heat of a solution =

Back 32

[/\H1+ /\H2] - [/\H3]

Front 33

What causes 95% of all ionic compounds to be soluble in water even though their enthalpy is +?

Back 33

entropy

Front 34

What does stirring do?

Back 34

increase collisions

Front 35

What does unsaturated mean?

Back 35

The maximum amount has been dissolved.

Front 36

+/\Hsoln =

Back 36

heat + ionic solute + h2O --><-- soln

Front 37

-/\Hsoln=

Back 37

gas solute + H2O --><-- solv + heat

Front 38

How is something supersaturated?

Back 38

By heating; You can increase the solute so theres more room for the solvent

Front 39

What is the rate of dissolving?

Back 39

change in concentration
-----------------------------------
change in temperature

Front 40

Ions conduct ____.

Back 40

electricity

Front 41

What indicates the degree of ionization?

Back 41

the amount of current

Front 42

Strong electrolytes are ___% ions.

Back 42

100

Front 43

Ionic salts in H2O and strong acids in H2O and strong bases in H2O are ____ electrolytes.

Back 43

strong

Front 44

Weak electrolytes are <__% ions.

Back 44

100

Front 45

What are the strong bases in H2O?

Back 45

Elements in group IA and IIA (hydroxides)

Front 46

Weak acids and weak bases are ____ electrolytes.

Back 46

weak

Front 47

Hc2, H3O2, H2CO3, and HF are:

Back 47

weak acids

Front 48

H C2 H3 O2:

Back 48

Acetic Acid

Front 49

NH3 (gas) is a _____.

Back 49

nonelectrolyte

Front 50

Cl, Br, I, NO3, CLO4, SO4 are strong ___ in H2O.

Back 50

acids

Front 51

What are some molecular substances that are nonelectrolytes?

Back 51

sugars, gasoline, sulfur, benzene, naphthalene, glucose, sucrose

Front 52

Why aren't colloids and suspensions true solutions?

Back 52

They are 2 phases, particles are larger and they show the Tyndall effect

Front 53

0.1-1 nm is a:

Back 53

solution

Front 54

1-100 nm is a:

Back 54

colloid

Front 55

100-1000 nm is a:

Back 55

suspension

Front 56

For a solution: tyndall? settles? stays n filter? Uniformity:

Back 56

no ; no; no; homogenous

Front 57

For a colloid: tyndall? settles? stays n filter? Uniformity:

Back 57

yes; no; no; borderline

Front 58

For a suspension: tyndall? settles? stays n filter? Uniformity:

Back 58

yes; yes; yes; heterogeneous

Front 59

What is emulsion?

Back 59

when a liquid is dispersed in a liquid

Front 60

__ is a solid disp. in liquid

Back 60

gel

Front 61

___ is a gas disp in liquid

Back 61

foam

Front 62

___ is a liquid disp in gas (fog)

Back 62

aerosol

Front 63

Water is most dense at ___C.

Back 63

4

Front 64

Salt water is/is not a colloid

Back 64

is not

Front 65

A substance that will lose its water of hydration due to its high vapor pressure is said to be:

Back 65

efflorescent

Front 66

solvent:

Back 66

what the solute is dissolved in

Front 67

solute:

Back 67

what is dissolved

Front 68

Sugar is/is not an electrolyte.

Back 68

is not

Front 69

What is the heat of vaporization of water?

Back 69

2.26 kJ/g

Front 70

An inward force that tends to minimize the surface area of a liquid is its

Back 70

surface tension

Front 71

The particles of a colloid are kept in suspension by numerous collisions known as:

Back 71

brownian motion

Front 72

A type of colloid where both dispersed phase and dispersion medium are liquids is known as __

Back 72

emulsion

Front 73

The fact that polar solvents dissolve polar solutes and nonpolar solutes dissolve in nonpolar solvents is summarized as _____.

Back 73

like dissolves like