Chem 111 Chapter 3 And 4

Front 1

mole

Back 1

# of particles = to # of atoms in 12 g of C-12

Front 2

Avogadro's #

Back 2

6.022x10^23

Front 3

molar mass

Back 3

mass of one mole of atoms

Front 4

mass percent of an element equation

Back 4

mas %= mass of element in compound of element/mass of compound times 100

Front 5

empirical formula

Back 5

indicates relative # of atoms of each element in the compound. Simplest type of formula

Front 6

molecular formula

Back 6

shows actual # of atoms of each element in a molecule of the compound

Front 7

stoichiometric coefficients

Back 7

#'s in front of chemical formulas; give ratio of reactants and products

Front 8

stoichiometric ratios

Back 8

balanced chemical equations give # of moles of reactant required to produce a certain # of moles of product

Front 9

theoretical yield

Back 9

amount of product predicted from stoichiometry taking into account limiting reagents

Front 10

percent yield

Back 10

relates actual yield to theoretical yield.
% yield= actual yield/theoretical yield x 100

Front 11

solution

Back 11

solute dissolved in solvent (homogeneous mixture)

Front 12

solute

Back 12

present in smaller amounts

Front 13

solvent

Back 13

present in greater amount

Front 14

aqueous solution

Back 14

water as solvent

Front 15

molarity

Back 15

moles of solute per liter of solution
Moles/liter

Front 16

the # of moles is the same in dilute and concentrated solutions due to...

Back 16

conservation of mass.

M1 x V1= M2 x V2

Front 17

pure water

Back 17

doesn't conduct electricity, but an aqueous solution can

Front 18

what does there need to be for something to conduct electrcity?

Back 18

there need to be ions

Front 19

strong electrolytes

Back 19

completely soluble
usually ionic compounds
conduct strongly

Front 20

weak electrolytes

Back 20

partially soluble
conduct weakly

Front 21

nonelectrolytes

Back 21

insoluble
frequently molecular compounds
do not conduct electricity at all

Front 22

Perchloric acid

Back 22

HClO4

Front 23

strong acids

Back 23

perchloric acid
nitric acid
sulfuric acid
hydrochloric acid

Front 24

nitric acid

Back 24

HNO3

Front 25

sulfuric acid

Back 25

H2SO4

Front 26

Hydrochloric acid

Back 26

HCl

Front 27

strong bases

Back 27

sodium hydroxide
potassium hydroxide
calcium hydroxide

Front 28

sodium hydroxide

Back 28

NaOH

Front 29

potassium hydroxide

Back 29

KOH

Front 30

Calcium hydroxide

Back 30

Ca(OH)2

Front 31

which ions are ALWAYS soluble no matter what it is paired with?

Back 31

Li+, Na+, K+, NH4+, NO3-, C2H3O2-,

Front 32

Cl-, Br-, I- pair with what elements to be insoluble?

Back 32

Ag+, Hg2^2+, Pb^2+

Front 33

SO4^2- pairs with what elements to be insoluble

Back 33

Ag+, Ca2+, Sr2+, Ba2+, Pb2+

Front 34

OH- pairs with what elements to be insoluble?

Back 34

Li+, Na+, K+, NH4+, Ca2+, Sr2+, Ba2+

Front 35

S2- pairs with what elements to become insoluble?

Back 35

Li+, Na+, K+, NH4+, Ca2+, Sr2+, Ba2+

Front 36

CO3^2-, PH4^3-, CrO4^2- pairs with what elements to be insoluble?

Back 36

Li+, Na+, K+, NH4+

Front 37

double displacement reactions

Back 37

involve swapping ions in solution

Front 38

double displacement reactions will lead to a change in solution if one of 3 things occurs:....

Back 38

-an insoluble solid is formed
-weak or nonelectolytes are formed
-an insoluble gas is formed

Front 39

precipitate

Back 39

when 2 solutions are mixed and a solid is formed

Front 40

spectator ions

Back 40

ions that remain in solution

Front 41

molecular equation

Back 41

shows all reactants and products as intact, undissociated compounds

Front 42

total ionic equations

Back 42

shows all of soluble ionic substances dissociated into ions

Front 43

net ionic equation

Back 43

eliminates spectator ions and shows the actual chemical change taking place.

Front 44

acids

Back 44

substances that produces H+ in water

Front 45

bases

Back 45

substances that produces OH- in water

Front 46

titrant

Back 46

solution of known concentration used in titration

Front 47

analyte

Back 47

sustance being analyzed

Front 48

equivalence point

Back 48

enough titrant added to react exactly with the analyte

Front 49

end point

Back 49

the indicator changes color so you can tell the equivalence point has been reached

Front 50

neutralization reactions

Back 50

occurs when a solution of and acid and base are mixed

Front 51

salt

Back 51

ionic compound whose cation comes from a base and anion from an acid

Front 52

neutralization btwn acid and metal hydroxide produces...

Back 52

water and a salt

Front 53

weak acids dissociate and form...

Back 53

H2O and a gas.

Front 54

oxidized

Back 54

atom, molecule or ion becomes more positively charged.

Front 55

oxidation

Back 55

loss of electrons

occurs when an atom's oxidation state increases during a reaction

Front 56

reduced

Back 56

atom, molecule, or ion becomes less positively charged

Front 57

reduction

Back 57

gain of electrons

occurs when an atom's oxidation state decreases during a reaction

Front 58

key points about redox reactions

Back 58

oxidation always follows reduction

oxidizing agent is reduced, the reducing agent is oxidized

the # of electrons gained by oxidizing agent always equals # lost by reducing agent

Front 59

reducing agent

Back 59

the reactant that reduces an element in another reactant.

contains the element that is oxidized

Front 60

oxidizing element

Back 60

reactant that oxidizes an element in another reactant

contains the element that is reduced

Front 61

types of double displacement reactions

Back 61

precipitation: form a solid
acid-based: form water and salt

Front 62

oxidation-reduction type reactions (transfer of electrons)

Back 62

single displacement (consult activity series)
combination: more reactants than products
decomposition: more products than reactants
combustion: has O2 as a reactant