Exam 2

Question 1

Greek for “measure elements”, involves calculations based on chemical formulas & chemical equations

Answer 1

Stoichiometry

Question 2

Avagadro’s number

Answer 2

6.022*10^23

Question 3

SI base unit for the amount of a substance

Answer 3

Mole

Question 4

The molar mass in grams of a substance is numerically equal to atomic mass measured in

Answer 4

amu

Question 5

Sum of the atomic mass of all atoms in the chemical formula

Answer 5

Formula mass

Question 6

Sum of the atomic masses of all atoms of the molecular substance

Answer 6

Molecular mass

Question 7

The percent composition of elements by mass is

Answer 7

The percent by mass of each element in a compound

Question 8

How to determine limiting reagant

Answer 8

Calculate the amount of product that each reactant would produce if it reacted completely

Question 9

Max amount of product that can be obtained from a given amount of reactants, based on the limiting reactant

Answer 9

Theoretical yield

Question 10

How to find percent yield

Answer 10

Actual yield/theoretical yield * 100

Question 11

Solvent vs solute

Answer 11

Solvent: substance solutes are dissolved in

Question 12

Concentrated vs dilute solution

Answer 12

C: large amount of solute, D: small amount of solute

Question 13

An exact measurement of the amount of solute in a given quantity of solvent or solution

Answer 13

Quantitative description

Question 14

Molarity is what

Answer 14

Moles of solute/ solution volume (L)

Question 15

Formula for dilution of solutions

Answer 15

Mi(Vi)=Mf(Vf)

Question 16

T or F, pure water is a good conductor of electricity

Answer 16

F

Question 17

Are most ionic compounds electrolytes or nonelectrolytes

Answer 17

Electrolyte

Question 18

Are molecular compounds generally electrolytes or nonelectrolytes

Answer 18

Nonelectrolyte

Question 19

Who discovered that electroyltic solutions are composed of dissolved ions

Answer 19

Svante Arrhenius

Question 20

Dissolve in the solvent exclusively as dissociated ions

Answer 20

Strong electrolytes

Question 21

Partially dissociate to ions for the dissolved species

Answer 21

Weak elctrolytes

Question 22

Molecular compounds that are acids or bases are

Answer 22

Electrolytes

Question 23

Arrhenius definition for an acid

Answer 23

A substance that produces H+ ions (H30+) when dissolved in water

Question 24

Bronsted definition for an acid

Answer 24

Hydrogen ion (proton) donor

Question 25

Arrhenius definition for bases

Answer 25

A substance that produces OH- ions when dissolved in water

Question 26

Bronsted definition for bases

Answer 26

Hydrogen ion (proton) acceptor

Question 27

Name the strong acids

Answer 27

HCl, HBr, HI, HClO3, HClO4, H2SO4, HNO3

Question 28

Name the strong bases

Answer 28

Group 1A metal hydroxides, Group 2A heavy metal hydroxides

Question 29

Define a salt, which is a special type of ionic compound

Answer 29

Cation from a base, anion from an acid

Question 30

The max amount of solute that can dissolve in a given quantity of solvent at a specific temperature

Answer 30

Solubility

Question 31

Row one solubility table

Answer 31

Alkali metal ions, NH4; no exceptions

Question 32

Row two solubility table

Answer 32

NO3, C2H3O2, HCO3, ClO3, ClO4; no exceptions

Question 33

Row three solubility table

Answer 33

Cl, Br, I; exceptions are salts of Ag, Hg, and Pb

Question 34

Row four solubility table

Answer 34

SO4; exceptions are salts of Ca, Sr, Ba, Hg, Pb, Ag

Question 35

Row one insoluble table

Answer 35

CO3, PO4, SO3, S, CrO4; exceptions are salts of NH4, alkali metal ions

Question 36

Row two insoluble table

Answer 36

OH; exceptions are NH4, alkali metal ions, Ca, Sr, Ba

Question 37

Row three insoluble table

Answer 37

O; exceptions are all alkali metal ions, Ca, Sr, Ba

Question 38

Used to determine concentration of an unknown solution by using a solution of known concentration

Answer 38

Titrations

Question 39

Conversion of the elemental form of a metal to a metal compound by reaction with a substance in its environment

Answer 39

Corrosion

Question 40

Metals at the top of the activity series are

Answer 40

More easily oxidized by metals towards the bottom

Question 41

Names for metals at top & bottom of activity series

Answer 41

Top: Active, Bottom: Noble

Question 42

Any neutral metal in the table can be oxidized by cations of

Answer 42

Elements below it

Question 43

Charge an atom would have if there was a complete electron transfer

Answer 43

Oxidation number

Question 44

Oxidation number of any free element

Answer 44

O

Question 45

Oxidation number of any monatomic ion

Answer 45

Charge of ion

Question 46

Oxidation numbers of F, H, O

Answer 46

F: -1, H: +1, O: -2

Question 47

When an ion/atom in a compound is replaced by an ion/atom of another element

Answer 47

Displacement reaction

Question 48

Types of displacement reactions

Answer 48

Hydrogen, metal, halogen

Question 49

One element is both oxidized and reduced in the reaction

Answer 49

Disproportionation reaction