APCHEM Intermolecular

Question 0

Which phase are IMFs strongest?

Answer 0

Solid, they are strongest enough to hold led the molecule in place.

Question 1

Which phase are IMFs weakest?

Answer 1

Gas, because the particles are so far apart.

Question 2

What 2 things does a state of a substance depend on?

Answer 2

Kinetic energy (temp.)- keeps particles moving and apart 
Attraction between particles- draws particles close together

Question 3

What does heating and cooling do to particles?

Answer 3

Heating makes the particles speed up and have more kinetic energy making it harder for attraction exist. Cooling slows them down, losing kinetic energy but making it easier for attraction to exist.

Question 4

What 2 things can be done to change the phase of a substance?

Answer 4

Increase or decrease pressure, cool or heat

Question 5

What does increasing and decreasing pressure do?

Answer 5

Increasing the pressure causes particles to be forced closer together, increasing attraction. Decreasing makes them move away, decreasing attraction.

Question 6

LDFS have ____ boiling points than the other 2 forces

Answer 6

Lower

Question 7

The bigger the molecule, and the greater the polarization, the ____ the LDF

Answer 7

Stronger

Question 8

Polarizability

Answer 8

The degree which the electron cloud can be distorted to bring about temporary dipoles

Question 9

DDP strength increases with increased ____

Answer 9

Polarity using electronegativity values

Question 10

HBFS have binds between…

Answer 10

H-F H-O or H-N

Question 11

All molecules have ___

Answer 11

LDFS

Question 12

Nonpolar molecules only have ____

Answer 12

LDFS

Question 13

Vaporization

Answer 13

When molecules leave the liquid surface and enter the gaseous state

Question 14

What allows molecules at liquid surface to overcome attractive forces and become a gas?

Answer 14

A great deal of kinetic energy

Question 15

What liquid molecules evaporate quicker?

Answer 15

Ones with Weaker IMFS

Question 16

Dynamic equilibrium

Answer 16

The rate of evaporation and the rate of condensation are equal

Question 17

Equilibrium vapor pressure

Answer 17

Measure of a molecule’s tendency to escape from the liquid phase to the gas phase

Question 18

What two things make higher vapor pressure occur?

Answer 18

Weaker IMFS and lower temps

Question 19

When does boiling occur?

Answer 19

when vapor pressure and atmospheric pressure are equal.

Question 20

Boyle’s Law

Answer 20

If temperature and amount are constant, pressure and volume are indirectly proportional P1V1=P2V2

Question 21

Charles law

Answer 21

When pressure and amount are constant, volume and temperature are directly proportional V1/T1=V2/T2

Question 22

Ideal Gas Law

Answer 22

PV=nRT

Question 23

Combined gas law

Answer 23

P1v1/T1=P2v2/T2

Question 24

Density and molar mass formula

Answer 24

D=P(mm)/RT (in g/L)

Question 25

Conversion values

Answer 25

1atm=760mmHg=760torr=101.325kpa=101325pa=14.7lb/in^2

Question 26

What does volatile mean?

Answer 26

It evaporates quickly

Question 27

Effusion

Answer 27

The escape of gas molecules into an area of lower concentration

Question 28

Diffusion

Answer 28

The spreading of a gaseous substance throughout space or through a second substance

Question 29

What are ideal gases?

Answer 29

Gases that occupy no space and have no attraction between mc

Question 30

What are real gases?

Answer 30

Gases that do not have volume and have attraction between mc

Question 31

When pressure is increased, will there be more or less chance for there to be attraction between mc?

Answer 31

More

Question 32

When temperature is low, what happens to molecules that make contact with each other?

Answer 32

They are less likely to have enough energy to overcome the attractive forces between them

Question 33

Triple point

Answer 33

Represents the conditions in which all three phases can coexist in equilibrium

Question 34

Critical temperature and pressure

Answer 34

The temp and pressure at which the gas can no longer be liquified

Question 35

Surface tension

Answer 35

The energy required to break through the surface of a liquid

Question 36

Viscosity

Answer 36

The resistance of a liquid to flow

Question 37

Name something that has a high viscosity and a low viscosity

Answer 37

Maple syrup has high and water has low

Question 38

Dalton's Law of Partial Pressures

Answer 38

Since gases all behave independently of each other within a mixture, the pressure of a mixture of gases is the sum of the partial pressures of the different gases pt=p1+p2+p3

Question 39

Molecules with ___ IMFS evaporate quicker

Answer 39

Weaker

Question 40

If temperature is doubled, what else is doubled?

Answer 40

Pressure, because the two are directly proportional

Question 41

The lighter the molecule, the ___ it moves

Answer 41

Faster

Question 42

Mole fraction (definition)

Answer 42

The number of moles of a substance in a mixture divided by the number of miles of all substance

Question 43

Mole fraction equation

Answer 43

``` Pa=(Na/Nt)Pt Pa-pressure of ideal gas Na-individual moles of gas Nt-total moles Pt-total pressure ```

Question 44

"Normal" means what pressure?

Answer 44

1atm

Question 45

Least dense to most dense of the phases

Answer 45

Gas, solid, liquid

Question 46

Kinetic molecular theory

Answer 46

Energy isn't gained or lost when mc collide Molecules are in constant rapid motion Gas mc take up a negligible amount of space in relation to the container

Question 47

Ideal behavior for gas mc according to kmt

Answer 47

Real molecules exhibit finite volumes, thus excluding some volume from compression. Real molecules exhibit attractive forces, thus leading to fewer collisions with the walls and a lower pressure. Real molecules do have some extent of attraction for each other.

Question 48

Ideal gases have what kind of pressure and temp?

Answer 48

Low pressure high temp High temperature result in high kinetic energies. This energy overcomes the attractive forces. Low pressure increases the distance between molecules. (So molecules comprise a small part of the volume or attractive forces are small.)

Question 49

Decreasing temperature does what to the number of collisions of mc?

Answer 49

Reduces them bc it reduce the ake