Chapter 5: Gases, Liquids, And Solids

Front 1

Heat of fusion is

Back 1

the energy used to change matter from a solid to a liquid. *additional heat raises the temperature of the liquid until it reaches its boiling point

Front 2

Heat of vaporization is

Back 2

the energy used to change a substance from a liquid to a gas. *additional heat raises the temperature of the gas

Front 3

Sublimation is

Back 3

the conversion of a solid directly into a gas. The substance never goes through a liquid phase. Examples: dry ice, CO2 undergoes sublimation

Front 4

Deposition is

Back 4

the reverse of sublimation, a becomes becomes a solid without ever becoming a liquid

Front 5

Heat rule of sublimation & deposition:

Back 5

Specific heat of a substance is the amount of heat required to raise the temperature of 1g of the substance by 1celcius

Front 6

Spontaneous reactions are

Back 6

reactions that occur as writtin

Front 7

Nonspontaneous reactions

Back 7

cannot occur as written. Generally energy must be added for these reactions to occur.

Front 8

Enthalpy is

Back 8

heat, designated by letter H.

Front 9

Exothermic reactions

Back 9

release heat. Triangle (change) in heat is negative.

Front 10

Endothermic reactions

Back 10

gain heat. Triangle (change) in heat is positive.

Front 11

Entropy is

Back 11

a measure of disorder, designated by S. Triangle (change in) S.

Front 12

Free energy is

Back 12

designated by G and used to determine whether a reaction is spontaneous. ΔG = ΔH − TΔS (temp change in entropy)

Front 13

Is ΔG is negative then

Back 13

the reaction is spontaneous

Front 14

Pressure is

Back 14

the force of collisions that take place between gas particles and the walls of the container they are held in

Front 15

Barometers are used

Back 15

to measure atmospheric pressure

Front 16

Pressure is measured in

Back 16

torr, mmHg or atm. 760 torr = 760 mmHg = 1 atm

Front 17

Standard temperature and pressure (STP) is

Back 17

0 degrees Celcius and 1atm

Front 18

Combined Gas Law

Back 18

P1V1/T1 = P2V2/T2

Front 19

Dalton's Law of Partial Pressure

Back 19

Ptotal = p1 + p2 + p3

you are either adding or subtracting all pressures for total

Front 20

Liquids: Viscosity describes

Back 20

the thickness of a liquid or it's resistance to flow

Front 21

Liquids: Density is used

Back 21

for liquids and solids. It is a measure of the amount of mass contained in a given volume/ D = m/v

Front 22

Liquids: Specific gravity

Back 22

relates the density of a substance to that of water. Specific gravity = density of a substance/ density of water. *There are no units for the specific gravity calculation!

Front 23

Liquids: Vapor pressure is the

Back 23

maximum pressure exerted by a gas formed by the evaporation of a liquid

Front 24

Liquids: Boiling point is

Back 24

the temp at which the vapor pressure of the liquid equals atmospheric pressure

Front 25

Solids: Crystalline solids

Back 25

have a highly ordered arrangement of particles (sugar)

Front 26

Solids: Amorphous solids are

Back 26

solids with a disorganized internal structure (glass)

Front 27

Solids: Ionic solids

Back 27

consist of oppositely charged ions held together by ionic bonds. These are highly organized!

Front 28

Covalent solids are

Back 28

held together by covalent bonds

Front 29

Molecular solids

Back 29

consist of an ordered arrangement of molecules attracted to one another by noncovalent interactions

Front 30

Metallic solids structure

Back 30

is an array of metal cations immersed in a cloud of electrons that spans the structure