1St Test

Front 1

when oxides of sulfur, nitrogen, or other nonmetals dissolve in water, they produce __________________.

Back 1

hydrogen ions

Front 2

what forms instead of H+ to combine with a water molecule?

Back 2

H3O+

Front 3

T/F: H+, proton, and H3O+ all refer to the same species

Back 3

true

Front 4

the acid (donates/accepts) a proton

Back 4

donates

Front 5

the base (donates/accepts) the proton

Back 5

base

Front 6

water can be a base : T or F

Back 6

T

Front 7

a reaction where an acid and a base are eliminated is called a __________________ reaction

Back 7

neutralization

Front 8

if a compound is completely soluble in water it is a (Strong/weak) electrolyte

Back 8

strong

Front 9

T or F: the spectator ions removed are the species in an equation

Back 9

False

Front 10

how do you know what the species taking part in a reaction are?

Back 10

the ones that still remain in the net ionic after getting rid of the spectator ions

Front 11

Nonmetal oxides other than carbon dioxide form solutions that are much more (acidic/basic) than carbonic acid

Back 11

acidic

Front 12

what are the six strong acids?

Back 12

HCl, HBr, HI, HNO3, H2SO4, HClO4

-hydrochloric acid, hydrobromic acid, hydroiodic acid, nitric acid, sulfuric acid, perchloric acid

Front 13

what is a monoprotic acid? give an example

Back 13

an acid that donates one proton; HCl, HNO3

Front 14

what is a diprotic acid? give an example

Back 14

an acid that can donate up to two protons; H2SO4

Front 15

in chemical reactions "---->" means

Back 15

complete ionization

Front 16

in chemical reactions

"----->

<------" means

Back 16

incomplete ionization

Front 17

for any diprotic acid, the HX- formed when the first proton dissociates is a (weaker/stronger) acid than the original acid H2X

Back 17

weaker

Front 18

what is the order for the proton donors in a triprotic acid?

Back 18

H3X> H2X- > HX2-

Front 19

strong bases include _____, Group____, and Group ______.

Back 19

hydroxides, 1, 2

Front 20

when ammonia dissolves in water is produces

Back 20

NH4+

Front 21

what is an amphiprotic substance? give an example

Back 21

can act as an acid or base; H2O

Front 22

what is Molarity?

Back 22

amount of solute/liter of solution

Front 23

if a compound has and OH in it is it a strong base or weak base?

Back 23

strong

Front 24

oxidation refers to a chemical reaction in which a substance ___________ electrons

Back 24

loses

Front 25

Reduction refers to a chemical reaction in which a substance ___________ electrons

Back 25

gains

Front 26

what is the oxidation number in monoatomic ions? (F-, O2-, Na+)

Back 26

the charge on the ion

Front 27

each atom in a pure element (F2, Na,Fe, O2) has the oxidation # of _____

Back 27

0

Front 28

the in compounds that have fluorine and one or more other elements, the oxidation of fluorine is always ____.

Back 28

-1

Front 29

T/F the oxidation number of Oxygen in H2O2 is -2

Back 29

False

Front 30

the oxidation number of chlorine and bromine is -1 unless combined with __________ or ___________

Back 30

fluorine or oxygen

Front 31

the __________ agent is reduced and the _________ is oxidated

Back 31

oxidation; reducing

Front 32

if K>1, the concentrations of products in a reaction mixture at equilibrium are much (larger/smaller) than the concentrations of reactants

Back 32

larger

Front 33

if K<1, the concentrations of products at equilibrium are much (larger/smaller) than the concentrations of reactants

Back 33

smaller

Front 34

T/F: K value can be negative

Back 34

False

Front 35

what is delta n in kp=kc(RT)^delta n

Back 35

# of moles on products side-# of moles on reactants side

Front 36

for decomposition or reverse process, K2=

Back 36

1/K1

Front 37

if the balanced equation is multiplied by some factor, n, then the value of of K2=(k1)^n

Back 37

raised to the nth power

Front 38

if the chemical reaction is the sum of two or more other reactions, the value of K is _______

Back 38

the product of the k values of the other reactions

Front 39

when Q

Back 39

right

Front 40

when Q>K the reaction shifts to the _______

Back 40

left

Front 41

when Q=K the reaction _________

Back 41

is at equilibrium

Front 42

which phases are emitted from the K equation?

Back 42

solids and liquids

Front 43

if partial pressure or concentration of a product/reactant is increased what will happen to reach equilibrium?

Back 43

it will shift to so that more of what increased is consumed

Front 44

if partial pressure or concentration of a product/reactant is decreased what will happen to the equilibrium?

Back 44

it will shift so there will be more production if what was decreased

Front 45

under what conditions will changing the overall volume occupied by the reactants and products shift the equilibrium mixture?

Back 45

a reaction of gases where moles of gas change as the reaction proceeds at a constant temp and pressure

Front 46

decreasing volume shifts equilibrium towards side the (left/right)

Back 46

right

Front 47

increasing volume shifts the equilibrium toward the side (left/right)

Back 47

left

Front 48

how can pressure be changed in a reaction?

Back 48

adding a gas not involved in the reaction

Front 49

(increasing/decreasing) temperature forms more reactants

Back 49

increasing

Front 50

Adding heat to an endothermic reaction will shift equilibrium to the

Back 50

Right

Front 51

k decreases with (exothermic/endothermic)

Back 51

exothermic

Front 52

k increases with (exothermic/endothermic)

Back 52

endothermic

Front 53

in an exothermic reaction, increasing temperature will shift equilibrium to the

Back 53

Left

Front 54

a small equilibrium constant means (a lot/very little) products will form

Back 54

very little

Front 55

Ka values for weak acids are (less/greater) than 1

Back 55

less

Front 56

an acid forms a conjugate base when it donates a _________

Back 56

H+ ion

Front 57

(acid/base) +H2O(l)-->conj.(base/acid) + H3O+

Back 57

acid; base

Front 58

(acid/base) +H2O(l)-->conj.(base/acid) + OH-

Back 58

base; acid

Front 59

what are the most common strong bases?

Back 59

hydroxides of group 1 and 2

Front 60

T/F reverse reactions do not happen for reactions with strong acids

Back 60

true

Front 61

what autoionization of water?

Back 61

production of very small concentrations of H3O+ and OH-

Front 62

ph>7 the solution is __________

Back 62

basic

Front 63

large pH correspond with values of (small/large) [H+]

Back 63

small

Front 64

pKa=

Back 64

-log(Ka)

Front 65

Ka=

Back 65

[A][H+]/[HA]

Front 66

% ionization =

Back 66

([H+] @equil/[HA] @initial) *100%

Front 67

for weak acids, the degree to which they ionize (increases/decreases) as their concentration decreases

Back 67

increases

Front 68

increasing numbers of oxygen atoms bonded to the central atom (increases/decreases) acid strength

Back 68

increases

Front 69

what does [HA] equil =

Back 69

acid initial- acid ionized