Chm-115 Final Exam

Front 1

Boyle's Law

Back 1

The volume of a fixed quantity of a gas at constant temperature is inversely proportional to the pressure

PV=k

Front 2

Charles's Law

Back 2

The volume of a fixed quantity of gas at constant pressure is directly proportional to its absolute temperature

V/T=k

Front 3

Combined Gas Law

Back 3

P1V1/T1=P2V2/T2

Front 4

Ideal Gas Law

Back 4

PV=nRT

Front 5

Graham's Law

Back 5

m1/m2 = v2^2/v1^2

Front 6

Van der Waals Equation

a

Back 6

a is the stickiness of the molecules-

Adjusting for pressure measured too low

Front 7

Van der Waals Equation

b

Back 7

b is the open space-

Adjusting for the volume measured too high

Front 8

Daltons Law

Back 8

PT = P1+P2+P3........

Front 9

High boiling point

Back 9

Higher IMF (ie hydrogen bonding)

Front 10

Higher Melting Point

Back 10

Higher IMF (ie hydrogen bonding)

Front 11

Higher Enthalpy of vaporization

Back 11

Higher IMF (ie hydrogen bonding)

Front 12

Greater Likelyhood of Being miscible in water

Back 12

Higher IMF (ie hydrogen bonding)

Front 13

Higher Enthalpy of Fusion

Back 13

Lower IMF

Front 14

Higher Vapor Pressure at STP

Back 14

Lower IMF

Front 15

Higher Volatility

Back 15

Lower IMF

Front 16

Strength of IMF

Ionic and Dispersion (KCl)

Back 16

1

Front 17

Strength of IMF

Hydrogen Bonding and Dispersion (CH3OH)

Back 17

2

Front 18

Strength of IMF

Dipole-Dipole and Dispersion (CH2O)

Back 18

3

Front 19

Strength of IMF

Dispersion only (O2)

Back 19

4

Front 20

1 atm = ? mmhg

Back 20

760 mmhg

Front 21

1 atm = ? kPa

Back 21

101.325 kPa

Front 22

Sublimation

Back 22

Solid to gas

Front 23

Deposition

Back 23

Gas to Solid

Front 24

7 Diatomic Elements

Back 24

H2 O2 F2 N2 Cl2 Br2 I2

Front 25

Alkali Metals

Back 25

Group 1

Front 26

Alkaline Metals

Back 26

Group 2

Front 27

Chalogens

Back 27

Group 16

Front 28

Halogens

Back 28

Group 17

Front 29

Noble Gases

Back 29

Group 18

Front 30

Mass Number

Back 30

Protons + Neutrons

Front 31

Atomic Mass

Back 31

Protons

Front 32

Law of Conservation of Mass

Back 32

Antoine Lavoisier 1789

Front 33

Discovery of Electrons

Back 33

J.J. Thomson 1897

Front 34

Basic Atomic Theory

Back 34

John Dalton 1803

Front 35

The Nuclear Atom

Back 35

Ernest Rutherford 1911

Front 36

Avagadros Number

Back 36

6.022 x 10^23

Front 37

Combustion

Back 37

_______ + O2 ---> CO2 + H2O

Front 38

Decomposition

Back 38

AB ----> A + B (HEAT)

Front 39

Molarity * Volume =

Back 39

Moles

Front 40

1 Cal = ? Joules

Back 40

4.184 Joules

Front 41

Work = ?

Back 41

-(Change in)Pressure X Volume

Front 42

Electron Affinity

Back 42

The energy required or released for one mole of a gaseous atom to gain an electron

Front 43

First Ionizarion energy

Back 43

The energy required for a gaserous atom to lose it most loosely fitted electron

Front 44

Electronegativity

Back 44

The relative attraction that an atom exhibits for the electrons in a bond

Front 45

Ionic Bond

Back 45

Metal & Non-Metal

High electronegativity difference

High Energy to break

Front 46

Covalent Bond

Back 46

Low non metals

Electrons shared

Lower energy to break