Vocab From Chemistry 12

Front 1

electrochemistry

Back 1

branch of chemistry which is concerned with the conversion of chemical energy to electrical energy, and vice versa

Hint 1

electrochemical cells, electrolytic cells, redox

Front 2

oxidation reaction

Back 2

half-reaction in which a species loses electrons

Hint 2

LEO the lion says GER

Front 3

reduction reaction

Back 3

half-reaction in which a species ganes electrons

Hint 3

LEO the lion says GER

Front 4

oxidizing agent

Back 4

substance which is reduced during an electrochemical reaction

Hint 4

Pb2+ + 2e- -> Pb(s)

Front 5

reducing agent

Back 5

substance which is oxidized during an electrochemical reaction

Hint 5

Pb(s) -> Pb2+ + 2e-

Front 6

half-cell reaction

Back 6

isolated reduction reaction or oxidation reaction

Hint 6

Mg2+ + 2e- -> Mg(s)

Front 7

redox reaction

Back 7

reaction involving the loss and gain of electrons

Hint 7

F2(g) + 2Li(s) -> 2F- + 2Li2+

Front 8

oxidation number

Back 8

charge that an atom would possess if the species containing the atom were made up of ions

Hint 8

O.N. of O = -2
O.N. of H = +1
O.N. halogens = -1
O.N. alkali = +1
O.N. alkaline earth = +2

Front 9

spontaneous redox reaction

Back 9

reaction which occurs by itself, without outside assistance

Hint 9

O.A > R.A

Front 10

Major Hydroxide

Back 10

when balancing half-reactions, balance Major species, then O atoms (with water), then H atoms (with protons), then charge (with electrons)

Hint 10

Major OH-

Front 11

disproportionation reaction

Back 11

redox reaction in which the same species is both reduced and oxidized

Hint 11

SO4-

Front 12

ΔON

Back 12

difference between ON of two species (ON of product - ON of reactant)

Hint 12

ΔON of Pb2+ -> Pb(s) = -2

Front 13

redox titration

Back 13

titration using redox reaction

Hint 13

if you know [AuCl4-], you can determine the [Cr2+] by performing a redox reaction

Front 14

potassium permanganate

Back 14

used as an oxidizing agent in titrations, purple in solution, strong oxidizing agent

Hint 14

KMnO4-

Front 15

electrode

Back 15

conductor at which half-reaction occurs

Hint 15

Pt inert electrode

Front 16

molecular compound

Back 16

compound which is bonded covalently and tends to produce non-ionic solutions

Hint 16

C6H12O6(s) -> C6H12O6(aq)

Front 17

ionic compound

Back 17

compound which is bonded ionically and tends to produce ionic solutions

Hint 17

Na2SO4(s) -> 2Na+(aq) + SO42-(aq)

Front 18

electrolyte

Back 18

substance which dissolves to give an electrically conducting solution containing ions

Hint 18

HCl(g) -> H+(aq) + Cl-(aq)

Front 19

non-electrolyte

Back 19

substance which dissolves to give a non-conducting solution containing only neutral molecules

Hint 19

C2H2(g) -> C2H2(aq)

Front 20

solubility

Back 20

maximum amount of a substance which can dissolve in a given amount of solvent at a given temperature; equilibrium [] of a substance in a solution at a given temperature

Hint 20

g/L, mol/L

Front 21

molar solubility

Back 21

molar [] of a saturated soltuion (mol/L)

Hint 21

molar solubility of lead (II) iodided is 0.00137 M

Front 22

saturated solution

Back 22

solution in which a dissolved substance is in EQ with some of the undissolved substance

Hint 22

CaSO4 <-> Ca2+ + SO42-

Front 23

dissociation reaction/dissolving reaction

Back 23

process of dissolving; opposite of a crystallization reaction; when an ionic compound dissolves into its ions

Hint 23

FeCl3(s) -> Fe3+ + 3Cl-

Front 24

ionization reaction

Back 24

reaction in which a polar covalent solid dissolves to form ions

Hint 24

(NH4)3PO4(s) -> 3NH4+(aq) + PO43-(aq)

Front 25

crystallization reaction

Back 25

porcess in which a substance in solution forms crystals of a solid; opposite of a dissolving reaction

Hint 25

Ag+(aq) + BrO3-(aq) -> AgBrO3(s)

Front 26

low solubility

Back 26

solubility possessed by a substance which produces a saturated solution having a [] of less than 0.1 M

Hint 26

AgCl, CuI, PbBr2, etc.

Front 27

precipitate

Back 27

solid which forms in a reaction involving aqueous reactants

Hint 27

supernatant is above the precipitate

Front 28

spectator ion

Back 28

ions which do not take part in a reaction; if a solubility EQ, the ions do not form a precipitate

Hint 28

Na+, NO3-, etc.

Front 29

supernatant

Back 29

clear liquid that remains above a sediment/precipitate

Hint 29

supernatant is above the precipitate

Front 30

aliquot

Back 30

smaller sample from a larger sample; usually a liquid

Hint 30

vile of sea water

Front 31

formula equation

Back 31

balanced chemical equation in which all the reactants and products are given by their chemical formulae

Hint 31

2AgNO3 + Na2CO3 -> Ag2CO3(s) + 2NaNO3

Front 32

complete ionic equation

Back 32

balanced chemical equation in which all soluble ionic species are shown broken into their respective ions

Hint 32

2Ag+ + 2NO3- + 2Na+ + CO32- -> Ag2CO3(s) + 2Na+ + 2NO3-

Front 33

qualitative analysis

Back 33

use of experimental procedures to determine which elements or ions are present in a substance

Hint 33

solution contains Ag+, Pb2+, or Cu+ if it forms a precipitate with Cl-

Front 34

solubility product expression

Back 34

EQ expressions for a salt in EQ with its dissolved ions, having the form Ksp = [A+][B-]

Hint 34

Ksp BaCO3 = [Ba2+][CO32-]

Front 35

solubility product constant

Back 35

numerical value of Ksp in the solubility product expression Ksp = [A+][B-]

Hint 35

Ksp BaCO3 = 2.6 x 10-9

Front 36

trial ion product

Back 36

product of the ion []s which actually exist in solution, having the form Q = [A+][B-]and used for comparisons with the value of Ksp to decide if a solution is saturated

Hint 36

Q<Ksp, no ppt; Q=Ksp, ppt just forms, Q>Ksp, ppt forms

Front 37

titration

Back 37

process in which a measured amount of a solution is reacted with a known volume of another solution until a desired equivalence/stoichiometric point is reached (one of the solutions has an unkown [])

Hint 37

determining [Cl-] by adding a known [Ag+] and using CrO4 to signal when the titration is complete

Front 38

equivalence/stoichiometric point

Back 38

point in a titration where the stoichiometry of the reaction is exactly satisfied

Hint 38

in reaction Ag+(aq) + Cl-(aq) <-> AgCl(s), when the ratio is 1:1:1

Front 39

permanently hard water

Back 39

water which contains Ca2+ and/or Mg2+ and does not contain HCO3-

Hint 39

can't soften by boiling

Front 40

temporarily hard water

Back 40

water which contains Ca2+ and/or Mg2+ and HCO3-

Hint 40

can soften by boiling

Front 41

stearate ion

Back 41

C17H35COO-, commonly found in soaps

Hint 41

reacts with Mg2+/Ca2+ to form a precipitate

Front 42

common ion effect

Back 42

lowering of the solubility of a salt by adding a second salt which has one ion in common with the first salt

Hint 42

to decrease the solubility of AgCl, add AgNO3

Front 43

Arrhenius acid

Back 43

substance which releases H+(aq) in water; any ionic species whose formula starts with "H"

Hint 43

HCl, HClO4, etc.

Front 44

Arrhenius base

Back 44

substance which releases OH-(aq) in water; any ionic species whose formula ends with "OH"

Hint 44

NaOH, Cr(H2O)5(OH)2+, etc.

Front 45

Bronsted-Lowry acid

Back 45

substance which donates a proton to another substance

Hint 45

NH4+ + H2O <-> H3O+ + NH3

Front 46

Bronsted-Lowry base

Back 46

substance which accepts a proton from another substance

Hint 46

SO4- + H2O <-> HSO4- + OH-

Front 47

strong acid

Back 47

acid which is 100% dissociated in solution

Hint 47

HI -> H+ + I- (no EQ)

Front 48

strong base

Back 48

base which is 100% dissociated in solution

Hint 48

NH2 + H+ -> NH3 (no EQ)

Front 49

weak acid

Back 49

acid which is less than 100% ionized in solution

Hint 49

HCOOH <-> H+ + HCOO- (EQ)

Front 50

weak base

Back 50

base which is less than 100% ionized in solution

Hint 50

CO32- + H+ <-> HCO3- (EQ)

Front 51

conjugate acid

Back 51

member of a conjugate pair which has the extra proton

Hint 51

HC2O4- vs. C2O42-

Front 52

conjugate base

Back 52

member of a conjugate pair which lacks the extra proton

Hint 52

HPO42- vs. H2PO4-

Front 53

conjugate pair

Back 53

pair of chemical species which differ by only one proton

Hint 53

HC2O4- and C2O42-

Front 54

proton

Back 54

basic particle in an atomic nucleus that has a positive charge

Hint 54

H+ has no electrons

Front 55

hydronium ion

Back 55

H3O+; this is what is produced when acids react with water

Hint 55

HCl + H2O -> Cl- + ?

Front 56

monoprotic

Back 56

acid which can supply one proton

Hint 56

HPO42-

Front 57

diprotic

Back 57

acid which can supply up to two protons

Hint 57

H2PO4-

Front 58

polyprotic

Back 58

acid which can supply more than one proton

Hint 58

H3PO4

Front 59

amphiprotic

Back 59

subtance which can act as either an acid or a base; apart from water, they start with "H" and have a - charge

Hint 59

H3PO4 -> H2PO4- -> HPO42- -> PO43-

Front 60

amphoteric

Back 60

amphiprotic

Front 61

pH

Back 61

-log[H3O+]; measure of the acidity of a substance (the [H3O+] of a substance)

Hint 61

pH of 4 is acidic, pH of 7 is neutral, pH of 10 is basic

Front 62

pOH

Back 62

-log[OH-]; measure of the alkalinity of a substance (the [OH-] of a substance)

Hint 62

pOH of 4 is basic, pOH of 7 is neutral, pOH of 10 is acidic

Front 63

Kw

Back 63

[OH-][H3O+] = 1.00 x 10-14; Ka x Kb

Hint 63

Kw of water = 1.00 x 10-14

Front 64

Ka

Back 64

acid ionization constant; [H3O+][A-]/[HA]

Hint 64

Ka = Kw/Kb

Front 65

Kb

Back 65

base ionization constant; [HA][OH-]/[A-]

Hint 65

Kb = Kw/Ka

Front 66

pKw

Back 66

pH + pOH = 14.000 = -log(Kw)

Hint 66

-log(1.0x10-14)

Front 67

pKa

Back 67

-log(Ka)

Hint 67

pKa of hydrogen peroxide = -log(2.4x10-12) = 11.62

Front 68

pKb

Back 68

-log(Kb)

Hint 68

pKb of fluorine ion = -log(1.0x10-14/3.5x10-4) = 10.54

Front 69

titration

Back 69

a process in which a measured amount of a solution is reacted with a known volume of another solution (one of solutions has unkown []) until a desired EQ point is reached

Hint 69

25 mL of H2SO4 titrated with 0.2 M NaOH; [H2SO4] = ?

Front 70

transition/end point

Back 70

point in a titration at which an indicator is half-way through its colour change

Hint 70

transition point when [HIn]=[In-]

Front 71

titration curve

Back 71

graph showing the change in pH which occurs when an acid is titrated with a base, or vice versa

Hint 71

when titrating strong acid with strong base, graph is steady, then does a sharp increase, then levels off

Front 72

neutralization

Back 72

pH=pOH (7); [H3O+]=[OH-]; when an acid and a base react to form water and a neutral salt

Hint 72

NaOH + HCl -> NaCl + H2O

Front 73

salt

Back 73

neutralization product which results when an acid and a base react; any ionic compound which is neither acid nor base

Hint 73

KCl

Front 74

hydrolysis

Back 74

reaction between water and the cation/anion (or both) contained in the salt so as to produce an acidic/basic solution

Hint 74

NaNO2 -> Na+ + NO2-; NO2- is a base, so the solution is basic

Front 75

acidic salt

Back 75

salt which when put in water dissociates to produce an acidic solution

Hint 75

NaHC2O4 -> Na+ + HC2O4-

Front 76

basic salt

Back 76

salt which when put in water dissociates to produce a basic solution

Hint 76

NaHS -> Na+ + HS-

Front 77

primary standard

Back 77

substance which can be obtained in a pure and stable form, which doesn't absorb water or CO2 from the air, and which has a known molar mass such that it can be used to prepare a solution of know []

Hint 77

KHC8H4O4 (potassium hydrogen phthalate)

Front 78

standard solution

Back 78

a solution with an accurately known []

Hint 78

a primary standard titrated with a solution creates a standard solution

Front 79

indicator

Back 79

weak organic acid/base with different colours for its conjugate acid and base forms

Hint 79

phenolphtalein, bromythol blue, etc.

Front 80

phenolphtalein

Back 80

indicator which turns from colourless to pink at pH of 8.2-10.0

Hint 80

mixing phenolphthalein with seawater makes it turn pink

Front 81

suitable indicator

Back 81

an indicator used in a titration that has an end/transition point pH about equal to the titration's equivalence/stoichiometric point pH

Hint 81

EQP of titration of NaOH and HCl = pH 7, suitable indicator = bromythol blue, with end pt. pH of 6.8

Front 82

acid rain

Back 82

any precipitation with a pH less than 5.6

Hint 82

naturally occuring rain water can be pH 5.6

Front 83

buffer

Back 83

solution containing appreciable amounts of a weak acid and its conjugate weak base

Hint 83

CH3COOH + NaCH3COO

Front 84

acidic buffer solution

Back 84

solution which buffers the pH in the acidic region

Hint 84

CH3COOH + H2O <-> CH3COO- + H3O+ keeps pH @ 4.74

Front 85

basic buffer solution

Back 85

solution which buffers the pH in the basic region

Hint 85

NH4+ + H2O <-> NH3 + H3O+ keeps pH @ 9.25

Front 86

caustic soda or lye

Back 86

very corrosive; very exothermic reaction with water; deliquesces rapidly; absorbs CO2(g) from air rapidly; found in cleaning products (oven cleaner and drain cleaner); used to make sodium salts, glass, pulp and paper, plastics, aluminum, soap

Hint 86

sodium hydroxide (NaOH)

Front 87

oil of vitriol or battery acid

Back 87

dehydrating agent; very exothermic reactino with water; []ed form chars some types of organic material (sugars); reacts with some metals; good electrolyte; used to make sulphates, fertilizers, explosices, dyes, insecticides, detergents, plastics; used in car batteries as an electrolyte; used to absorb water

Hint 87

sulphuric acid (H2SO4)

Front 88

muriatic acid

Back 88

good electrolyte; []ed solution has choking odour; reacts with some metals; used to make chlorides; used as metal cleaning product (removing "boiler scale"); catalyst in some reactions; "stomach acid"

Hint 88

hydrochloric acid (HCl)

Front 89

vinegar (5% aqueous solution)

Back 89

non-electrolyte when []ed; weak electrolyte when diluted; only affects highly reactive metals; used to make acetates, textiles, plastics; used to preserve food

Hint 89

acetic acid (CH3COOH)

Front 90

nitric acid

Back 90

colours protein yellow; very reactive, quickly attacks almost all metals; used to make nitrates, fertilizers, explosives, dyes

Hint 90

nitric acid (HNO3)

Front 91

ammonia ("ammonium hydroxide")

Back 91

colourless; highly toxic; corrosice gas; pungent odour; highly soluble in water; exothermic reaction with water; used to make nitric acid, explosives, ferilizers, synthetic fibres; used as refrigeration gas

Hint 91

ammonia (NH3)

Front 92

caustic potash

Back 92

much the same as NaOH but melts at lower temperature; used to make liquid soap, potassium salts; electrolyte in alkaline batteries; used to absorb CO2

Hint 92

potassium hydroxide (KOH)

Front 93

anode

Back 93

electrode at which oxidation occurs; electrode receiving the elctrons from a substance being oxidized; electrode toward which anions travel; electrode from which electrons leave to flow to the cathode

Hint 93

"An Ox CaRed"

Front 94

cathode

Back 94

electrode at which reduction occurs; electrode supplying electrons to a substance being reduced; electrode toward which cations travel; electrons flow here from anode

Hint 94

"An Ox CaRed"

Front 95

electrical potential

Back 95

potential energy per unit charge associated with a static electric field, also called the electrostatic potential, typically measured in volts; electric potential may be conceived of as "electric pressure" that can push electric charges to different locations

Hint 95

tendency for electrons to migrate in an electrochemical cell

Front 96

standard reduction potential (Eº)

Back 96

voltage of a reduction reaction occuring in an electrochemical cell where all reactants and products are at 1.0M [] or 1 atm pressure

Hint 96

s.r.p. for Ag+ + e- <-> Ag(s) = +0.80 V

Front 97

cell potential

Back 97

amount of volts an electrochemical cell can produce

Hint 97

Eºcell = Eºred - Eºox

Front 98

preferred reaction

Back 98

when given a group of species, the reaction that involves the species with the highest strenght as an O.A. and the highest strength as an R.A.

Hint 98

Fe3+ will reduce before Cu2+

Front 99

lead-acid storage battery

Back 99

storage battery using lead (Pb) and lead peroxide (PbO2 ) as the electrodes and an electrolyte solution of water and sulfuric acid (H2SO4)

Hint 99

car battery

Front 100

fuel cell

Back 100

electrochemical device into which fuel is continuously fed and from which electricity is continuously ontained

Hint 100

hydrogen fuel cell

Front 101

cathodic protection

Back 101

term applied to the process of protecting a substance from unwanted oxidation by connecting it to a substance having a higher tendency to oxidize

Hint 101

putting a chunk of zinc on an iron boat hull

Front 102

electrolysis

Back 102

process of supplying electrical energy to a molten ionic compound or to a solution containing ions so as to produce a chemical change

Hint 102

using an electrolytic cell

Front 103

inert electrode

Back 103

electrodes which do not undergo any change during electrolysis

Hint 103

platinum, carbon, etc.

Front 104

overpotential effect

Back 104

fact that some species react before water, even though they may have a weaker electrical potential

Hint 104

Br- and Cl- react before H2O as reducing agents

Front 105

electroplating

Back 105

electrolytic process in which a metal is reduced or "plated out" at a cathode, and having the purpose of covering the underlying material

Hint 105

plating iron with a layer of gold

Front 106

electrorefining

Back 106

process of purifying a metal by electrolysis

Hint 106

purifing pig iron into pure iron

Front 107

bauxite

Back 107

only commercial ore of aluminum, corresponding to the formula Al2O3xH2O

Hint 107

where to get aluminum

Front 108

activated complex

Back 108

intermediate molecule which occurs when reactants are in the process of rearranging to form products

Hint 108

OH- + H3O+ = H4O2

Front 109

activation energy

Back 109

minimum P.E. required to change reactants into an activated complex

Hint 109

Ea = 159 kJ

Front 110

bond energy

Back 110

amount of energy required to break a bond between two atoms

Hint 110

energy to break SO4 into S and O4

Front 111

catalyst

Back 111

chemical which can be added to a reaction to increase the rate of reaction; substance which provides an overall reaction with an alternative mechanism having a lower activation energy

Hint 111

platinum in car exhausts

Front 112

closed system

Back 112

system which nothing can enter or leave

Hint 112

stopped flask of a substance

Front 113

collision/kinetic molecular theory

Back 113

theory stating that molecules act as small, hard spheres which bounce off each other and transfer energy among themselves during their collisions

Hint 113

analogy of kids bling folded bumbing around in a square room

Front 114

dynamic equilibrium

Back 114

equilibrium situation in which microscopic changes occur, but macroscopic changes don't

Hint 114

<->

Front 115

elementary process

Back 115

individual step in a reaction mechanism

Hint 115

HBr + O2 -> HOOBr

Front 116

endothermic reaction

Back 116

reactino which absorbs heat, so that products have more energy than reactants

Hint 116

ax + by + heat -> bx + ay; ax + by -> bx + ay, ∆H:+

Front 117

enthalphy

Back 117

total kinetic and potential energy which exists in a system when it is at constant pressure

Hint 117

∆H

Front 118

entropy

Back 118

amount of randomness in a system

Hint 118

gases>aqueous ions>liquids>solids

Front 119

equilibrium

Back 119

situation which exists when the rate of the forward reaction is equal to the rate of the reverse reaction in a reversable reaction

Hint 119

[reactants] and [products] remain constant

Front 120

equilibrium constant

Back 120

numerical value of Keq in the equilibrium expression: [products]/[reactants]

Hint 120

14, products favoured

Front 121

equilbrium expression

Back 121

ratio of the [products] divided by the [reactants]

Hint 121

A2 + B3 <-> C3 + D2; Keq = [A]2[B]3/[C]3[D]2

Front 122

exothermic reaction

Back 122

reaction which gives off heat, so that products have less energy than reactants

Hint 122

ax + by -> bx + ay + heat; ax + by -> bx + ay, ∆H:-

Front 123

heterogenous reaction

Back 123

reaction in which all the reactnats are present in different phases

Hint 123

solid + solid, solid + liquid, 2 immiscible liquids, etc.

Front 124

homogenous reaction

Back 124

reaction in which all the reactnats are in the same phase

Hint 124

gas + gas, 2 miscible liquids, 2 aqueous solutions, etc.

Front 125

inhibitor

Back 125

chemical which reduces a reaction rate by combining with a catalyst or one of the reactants in such a way as to prevent the reaction form occuring

Hint 125

paint

Front 126

kinetic energy

Back 126

energy which a system possesses because of movement within the system

Hint 126

running person

Front 127

le Chatelier's principle

Back 127

states that is a closed system at equilibrium is subjected to change, processes will occur that tend to counteract that change

Hint 127

increasing the concentration of reactants, reaction moves to product side

Front 128

macroscopic changes

Back 128

visible, or large scale changes

Hint 128

opposite of microscopic changes

Front 129

nature of the reactant

Back 129

term used to describe the chemical properties of a substance

Hint 129

H2O is a polar molecule with the O end negative and the H end positive

Front 130

open system

Back 130

system which substances can either enter or leave

Hint 130

an open flask

Front 131

overall reaction

Back 131

sum of all the steps in a reaction mechanism

Hint 131

4HBr + O2 -> 2H2O + 2Br2

Front 132

potential energy

Back 132

energy existing as a result of an object's position in space, as well as the sum of all the attractive and repulsive forces existing among the particles which make up the object

Hint 132

stretched elastic band

Front 133

rate-determining step

Back 133

slowest step in a reaction mechanism

Hint 133

bottle-neck

Front 134

reaction intermediate

Back 134

molecules which are produced in one step of a reactino mechanism and subsequently consumed in another step

Hint 134

HOOBr, HOBr

Front 135

reacton kinetics

Back 135

study of the rates of reactions and the factors which affect the rates

Hint 135

study

Front 136

reaction mechanism

Back 136

actual sequence of steps which make up an overall reaction

Hint 136

HBr + O2 -> HOOBr
HBr + HOOBr -> 2HOBr
2HBr + 2HOBr -> 2H2O + 2Br2

Front 137

reaction quotient

Back 137

"trial value" for equilibrium expression, used for comparison with the value for Keq to decide if a system is at equilibrium

Hint 137

Q > Keq, reaction will shift to reactants to establish EQ; Q = Keq, reaction at EQ; Q < Keq, reaction will shift to products to establish EQ

Front 138

reaction rate

Back 138

amount of a reactant or product involved in a reaction in a specific time

Hint 138

1.3g/s

Front 139

spontaneous reaction

Back 139

reaction which occurs by itself, without outside assistance

Hint 139

max. entropy, min. enthalpy