Lecture 7 - States of Matter: Gases, Liquids, Solids

Question 1

solid has ______ shape/volume

Answer 1

definite

Question 2

liquid has _______ shape/volume

Answer 2

indefinite

Question 3

gas has ________ shape/volume

Answer 3

indefinite

Question 4

solid has _____ density

Answer 4

high

Question 5

liquid has _____ density

Answer 5

high

Question 6

gas has _____ density

Answer 6

very low

Question 7

solid has ______ compressibility

Answer 7

very low

Question 8

liquid has _____ compressibility

Answer 8

very low

Question 9

gas has _____ compressibility

Answer 9

very high

Question 10

solid has _____ thermal expansion

Answer 10

very small

Question 11

liquid has _____ thermal expansion

Answer 11

small

Question 12

gas has _____ thermal expansion

Answer 12

moderate

Question 13

particles are in constant random motion describes

Answer 13

kinetic energy

Question 14

particles attract/repel each other describes

Answer 14

potential energy

Question 15

particles motion ______ with temperature

Answer 15

increases

Question 16

particles transfer energy through _____

Answer 16

collisions

Question 17

kinetic energy = ________ = particles ______

Answer 17

disruptive force, far apart

Question 18

potential energy = _____ = particles _____

Answer 18

cohesive, close together

Question 19

formula to figure our how much pressure is exerted on a surface

Answer 19

P = (F/A)

p: pressure
f: force
a: area

Question 20

Boyles Equation

Answer 20

P1V1 = P2V2

Question 21

Boyles Law:

as pressure increases, volume _______

Answer 21

decreases

Question 22

Charles Equation

Answer 22

V1/T1 = V2/T2

Question 23

Charles Law:

as temperature increases, volume ______

Answer 23

increases

Question 24

Gay-Lussac’s Equation

Answer 24

P1/T1 = P2/T2

Question 25

Gay Lussac's Law: | as temperature increases, pressure _____

Answer 25

increases

Question 26

Combined Gas Equation

Answer 26

(P1V1)/T1 = (P2V2)/T2

Question 27

empirical gas law

Answer 27

1 mole gas = 22.4 L

Question 28

What is STP

Answer 28

Standard Temperature = 273 K | Standard Pressure = 1 atm

Question 29

Ideal Gas Equation

Answer 29

PV = nRT

Question 30

solid -> liquid

Answer 30

melting

Question 31

liquid -> gas

Answer 31

evaporation

Question 32

gas -> liquid

Answer 32

condensation

Question 33

liquid -> solid

Answer 33

freezing

Question 34

solid -> gas

Answer 34

sublimation

Question 35

gas -> solid

Answer 35

deposition

Question 36

heat is absorbed and the energy of the system increases

Answer 36

endothermic change of state

Question 37

heat energy is given off and the energy of the system decreases

Answer 37

exothermic change of state

Question 38

forces that exist between molecules

Answer 38

intermolecular forces

Question 39

forces within molecules

Answer 39

intramolecular

Question 40

which is stronger, intermolecular or intramolecular

Answer 40

intramolecular (made of covalent bonds)

Question 41

exist between polar molecules

Answer 41

dipole-dipole

Question 42

special type of extra strong dipole-dipole interaction between a hydrogen atom covalently bonded to a small, very electronegative atoms (F, O, or N) and an unshared pair of electrons on another small, very electronegative atom (F, O, N)

Answer 42

hydrogen bonding

Question 43

how to identify hydrogen bonding

Answer 43

H is bonded to N, O, or F

Question 44

the amount of heat energy required to convert the solid to liquid

Answer 44

heat of fusion

Question 45

the amount of heat energy required to convert the liquid to a gas

Answer 45

heat of vaporization

Question 46

molecules in nonpolar molecular liquids and solids are held together by weak electrostatic forces (larger molecule = stronger force)

Answer 46

London Forces

Question 47

a weak temporary intermolecular force that occurs between an atom or molecule (polar or nonpolar) and another atom or molecule (polar or nonpolar)

Answer 47

London Force

Question 48

They results from the temporary uneven e- distribution in molecules at any one moment, thus crating an instantaneous temporary dipole

Answer 48

London Force

Question 49

They are the weakest type of intermolecular force

Answer 49

London Force

Question 50

They are important because they occur between all molecules

Answer 50

London Force

Question 51

Comparing Intermolecular Forces: - add the the effect of London Forces and are found in polar molecules

Answer 51

Dipole-Dipole

Question 52

Comparing Intermolecular Forces: - the strongest intermolecular force and occurs in molecules which have H atoms bonded to F, O, or N atoms

Answer 52

Hydrogen Bonds

Question 53

Comparing Intermolecular Forces: - are found in all substances and are the weakest intermolecular force

Answer 53

London Force

Question 54

List the Intermolecular Forces from strongest to weakest

Answer 54

Hydrogen Bonding > Dipole-Dipole > London

Question 55

increasing the temperature of a liquid ________ its evaporation rate

Answer 55

increases

Question 56

molecules that escape (evaporate) from liquid water at room temperature

Answer 56

water vapor

Question 57

the pressure exerted by a vapor above a liquid when the liquid and vapor are in equilibrium

Answer 57

vapor pressure

Question 58

the temperature at which the vapor pressure equals the atmospheric pressure

Answer 58

boiling point