Chem Final

Front 1

Liquids are_____________ because its molecular motion is_____________ but the molecularspacing is ____________

Back 1

Incompressible; free relative to one another;close together

Front 2

Data that have random error but otherwise fall in a narrow range are

Back 2

precise but not accurate

Front 3

The polymer backbone and the monomer are the constituent parts of an alkane

Back 3

false

Front 4

The polymer backbone and the monomer are the constituent parts of a polymer

Back 4

true

Front 5

____________________ explained the law of conservation of mass, as well as other laws and observations, by proposing that all matter was composed of small, indestructible particles called atoms

Back 5

Dalton

Front 6

what is a lattice

Back 6

In an ionic bond, ions are assemble into an extended array called a lattice that are heldtogether by the attraction between oppositely charged ions

Front 7

what is an alkane

Back 7

a hydrocarbon connected with only single bonds

Front 8

what is an isomer

Back 8

A molecule with the same chemical formula butdifferent structure

Front 9

The molar fraction of a gas is " " to its partial pressure: directly/inverse proportional

Back 9

directly

Front 10

no more than 2 electrons can occupy any orbital

Back 10

Pauli exclusion principle

Front 11

electrons occupying orbitals must start with the lowest energy level andproceed to the higher

Back 11

Aufbau principle

Front 12

if two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs

Back 12

Hund's rule

Front 13

Van der Waals equation

Back 13

has a correction factor for the volume, b, and a correction factor that accounts for the attractions between particles in the gas, a

Front 14

Calorimetry technique measures the heat evolved or absorbed by the system by measuring the_______________ change in the surroundings

Back 14

temperature

Front 15

1. When a chemical bond breaks, energy is released/absorbed/either/neither

Back 15

absorbed

Front 16

specific heat

Back 16

c

physical property of a substance that describes the amount of heat required to raise the temperature of one gram of substance by one °C

q=mc(change in)T

Front 17

(molar) heat capacity

Back 17

Cp

physical property of a substance that describes the amount of heat required to raise the temperature of one mole of substance by one °C.

q = nCp(change in)T

Front 18

Dispersion forces are also called

Back 18

London forces

Front 19

a small separation of charge (positive or negative) that happens because of a fluctuation in the position of the electrons of an atom or molecule

Back 19

instantaneous dipole

Front 20

What are the two specific intermolecular forces for liquids

Back 20

Surface tension and Viscosity

Front 21

exists in all polar molecules as they have permanent dipoles that interact withpermanent dipoles of other molecules

Back 21

dipole-dipole force

Front 22

occurs in mixtures where ionic compounds and polar compounds are present

Back 22

Ion-dipole force

Front 23

occurs in polar molecules with hydrogen atoms bonded to fluorine, oxygen, or nitrogen

Back 23

Hydrogen bonding

Front 24

the amount of energy required to remove an electron

Back 24

ionization energy

Front 25

the amount of energy required to add an electron

Back 25

electron affinity

Front 26

what determines strength of an ion's lattice energy

Back 26

smaller ions = greater lattice energy

bigger charge = greater lattice energy

Front 27

What are the units of k for a zero orderreaction

Back 27

(mol)(L^-1)(s^-1)

Front 28

What are the units of k for a first order reaction

Back 28

s^-1

Front 29

What are the units of k for a second order reaction

Back 29

(L)(mol^-1)(s^-1)

Front 30

uses a combination of adiabatic (no heat is exchanged) and isothermal processes(temperature is constant)

Back 30

the Carnot cycle

Front 31

In the following equilibrium reaction in a closed system, indicate how theequilibrium is shifted by the addition of HF(g) to the system:

HF(g) + H2O(l) > H3O+(aq)+ F-(aq)

Back 31

equilibrium will shift toward the products

Front 32

an energy threshold that reactants must overcome to become products

Back 32

Activation energy

Front 33

Determine the formula of the conjugate base for this acid HSO4(-), andthe conjugate acid for this base HPO429(2-)

Back 33

SO4(2-) and H2PO4(-), respectively

Front 34

The rate of reaction decreases as the temperature of the reaction is decreases: t/f

Back 34

true

Front 35

randomness/disorder of a system

Back 35

entropy

Front 36

Bronsted-Lowry acid

Back 36

proton doner

Front 37

Bronsted-Lowry base

Back 37

proton receiver

Front 38

conjugate base

Back 38

The conjugate base of an acid is the base formed when the acid donated a proton

Front 39

conjugate acid

Back 39

The conjugate acid of a base is the acid formed when the base accepted a proton

Front 40

Spontaneous processes take place without continuous intervention, according tothermodynamics: T/F

Back 40

true

Front 41

Sig figs in multiplication & division

Back 41

result should have same number of SIG FIGS as the number with the least number of sig figs

Front 42

sig figs in addition and subtraction

Back 42

result should have the same number of DECIMAL PLACES as the number with the least number of decimal places

Front 43

What is Charles' law and how is T and V related

Back 43

V1/T1 = V2/T2

Front 44

What is Boyle's law and how are P and V related

Back 44

P1xT1 = P2xT2

Front 45

What is Avagodro's law and how are n and V related

Back 45

V1/n1 = V2/n2

Front 46

what is the value of R, the universal gas constant

Back 46

R = .08206 (L*atm)/(mol*K)

Front 47

What is the law of partial pressures

Back 47

Total pressure is equivalent to the sum of the partial pressures of each proponent gas

Front 48

what is the law of partial pressures expressed in terms of the mole fraction

Back 48

the mole fraction(Xi) for a gas is the moles of the gas(ni) divided by the total moles of the different gases present(n): (Xi= ni/n)

the partial pressure of each gas is related to its molar: (Pi = P*Xi)

Front 49

Van der Waals equation

Back 49

(P + an^2/V^2)(V - nb) = nRT

a corrects for attractive forces

b corrects for volume occupied by gas molcs.

Front 50

what is the speed of light and Planck's constant

Back 50

c = 2.99 x 10^8 m/s

h = 6.626 x 10^-34

Front 51

what is the energy equation

Back 51

E = hc/(wavelength)

Front 52

Binding energy

Back 52

energy holding an electron to a metal

Front 53

threshold frequency

Back 53

minimum frequency of light needed to emit an electron

Front 54

what is electronegativity

Back 54

the attraction of an atom for the shared electrons in a covalent bond

Front 55

Exceptions to the Octet rule

Back 55

odd number of electrons

small elements

expanded octet

Front 56

zero order integrated rate law

Back 56

[A]t = [A]o - kt

Front 57

first order integrated rate law

Back 57

[A]t = [A]oe^(-kt)

Front 58

second order integrated rate law

Back 58

1/[A]t - 1/[A]o = -kt

Front 59

the degradation of metals by chemical reactions with the environment

Back 59

corrosion

Front 60

uniform corrosion

Back 60

even corrosion over a large portion of a surface

Front 61

galvanic corrosion

Back 61

occurs when two different metals contact each other in the presence of an appropriate electrolyte

Front 62

crevice corrosion

Back 62

occurs when two pieces of metal touch each other leaving a small gap or crevice between metals

Front 63

What is oxidation

Back 63

loss of electrons from some chemical species

Front 64

What is reduction

Back 64

the gain of electrons from some chemical species

Front 65

Reducing agent

Back 65

species undergoing oxidation

Front 66

Oxidizing agent

Back 66

species undergoing reduction

Front 67

an electrochemical cell in which a spontaneous chemical reaction can be used to generate an electric current

Back 67

GALVANIC CELL

Front 68

electrode

Back 68

electrically conducting sites at which either oxidation or reduction occurs

Front 69

anode

Back 69

electrode where oxidation occurs

Front 70

cathode

Back 70

electrode where reduction occurs

Front 71

what is proper cell notation

Back 71

anode | anode electrolyte || cathode electrolyte | cathode