chapter 7

Question 1

acid

Answer 1

substance produces H+ ions when dissolved in water

Question 2

base

Answer 2

substance produces OH- ions when dissolved in water

Question 3

molecular equation

Answer 3

balanced (in lowest ratio)
compounds stay in tact
includes phases

Question 4

complete ionic equation

Answer 4

compounds written as ions (with charges)
includes phases

Question 5

net ionic equation

Answer 5

remove spectator ions
include charges
include phases

Question 6

oxidation

Answer 6

looses an electron

Question 7

reduction

Answer 7

gains an electron

Question 8

oxidizing agent

Answer 8

the substance that becomes reduced,
causing the oxidation

Question 9

reducing agent

Answer 9

the substance that becomes oxidized,
causing the reduction

Question 10

types of reactions

Answer 10

1. acid - base
2. combustion
3. neutralization
4. oxidation-reduction
5. precipitation
6. single displacement
7. redox

Question 11

Acid - base reaction

Question 12

Combustion reaction

Answer 12

a redox reaction that the reductant and the oxidant react vigorously and produces heat “(g)”.

Question 13

Neutralization reaction

Answer 13

a specific type of acid-base reaction
reactants are an acid and base
products are often salt and water

Question 14

Oxidation-reduction reaction

Answer 14

one or more elements involved undergo a change in oxidation number.

Question 15

Precipitation reaction

Question 16

Single displacement reaction

Answer 16

redox reactions in which an ion in the solution is displaced or replaced.

Question 17

Redox reaction

Answer 17

two or more element undergo a change in oxidation number

Question 18

precipitate

Answer 18

the solid formed during a reaction
NOT soluble

(use the solubility chart for products!!!)

Question 20

percent yield

Answer 20

(actual yield / theoretical yield ) x 100

Question 21

oxidation state / number

Answer 21

the charge of each atom of an element would have if it were ionic.

                      rules: 1. when in elemental form is always zero.

2. in monatomic ions, O.N = ions charge.
3. common non metals:
   hydrogen: +1 when w/ nonmetals
   hydrogen: -1 when w/ metals

oxygen: -2 in most compounds
oxygen:-1 when peroxides
oxygen:-1/2 when superoxides

halogens: -1 always for F
halogens: -1 mostly for other halogens
EXCEPT when combined with oxygen or other halogens

4. the sum of oxidation numbers for all atoms in molecule equals zero.

Question 22

limiting reactant

Answer 22

the reactant that is entirely consumed;
limiting the amount of product that can be generated

Question 23

excess reactant

Answer 23

the reactant that is left over/ extra

Question 24

Emperical formula

Question 25

formula

Question 26

Equivalence point of titration

Question 27

end point of titration

Question 28

ppm

Question 29

molarity

Question 30

molality