Ch. 3.5-5.6

Question 1

solute

Answer 1

the substance dissolved in the solvent (ex: NaCl)

Question 2

solvent

Answer 2

the substance that dissolves the solute (ex: H2O)

Question 3

molarity

Answer 3

moles of solute/L of solution

Question 4

all common compounds of group 1A(1) ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+)

Answer 4

soluble ionic compounds

Question 5

all common nitrates (NO3-), acetates (CH3COO- or C2H3O2-), and most perchlorates (ClO4-)

Answer 5

soluble ionic compounds

Question 6

all common chlorides (Cl-), bromides (Br-), and iodides (I-), except those of Ag+, Pb2+, Cu+, and Hg22+

Answer 6

soluble ionic compounds

Question 7

all common fluorides (F-), except those of Pb2+ and group 2A(2)

Answer 7

soluble ionic compounds

Question 8

all common sulfates (SO42-), except those of Ca2+, Sr2+, Ba2+, Ag+, and Pb2+

Answer 8

soluble ionic compounds

Question 9

all common metal hydroxides, except those of group 1A(1) and the larger members of group 2A(2) (beginning with Ca2+)

Answer 9

insoluble ionic compounds

Question 10

all common carbonates (CO32-) and phosphates (PO43-), except those of group 1A(1), group 2A(2), and NH4+

Answer 10

insoluble ionic compounds

Question 11

strong acids

Answer 11

acid that dissociates 100% in solution ex: HCl, HBr, HI, HNO3, H2SO4, HClO4

Question 12

weak acids

Answer 12

acid that only dissociates some in solution. ex: HF, H3PO4, CH3COOH

Question 13

strong bases

Answer 13

base that dissociates 100% in solution. ex: NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

Question 14

weak bases

Answer 14

base that only dissociates some in solution. ex: NH3

Question 15

oxidation

Answer 15

lose electrons - can identify when you see an increase in oxidation number

Question 16

reduction

Answer 16

gain electrons - can identify when you see a decrease in oxidation number

Question 17

oxidizing agent

Answer 17

oxidizes something else and is reduced in the process (oxidation number decreases)

Question 18

reducing agent

Answer 18

reduces something else and is oxidized in the process (oxidation number increases)

Question 19

oxidation number

Answer 19

the charge an atom would have if it “owned” all the electrons it shares with other atoms

Question 20

general oxidation number rules

Answer 20

1. O.N. = 0 for an atom in its elemental form
2. O.N. = ion charge for a monatomic ion
3. O.N. = 0 for the sum of O.N. values for the atoms in a molecule or formula unit of a compound
4. O.N. = ions charge for the sum of O.N. values for the atoms in a polyatomic ion

Question 21

specific O.N. rule for group 1A(1)

Answer 21

O.N. = +1 in all compounds

Question 22

specific O.N. rule for group 2A(2)

Answer 22

O.N. = +2 in all compounds

Question 23

specific O.N. rule for hydrogen

Answer 23

O.N. = +1 in combination with nonmetals
O.N. = -1 in combination with metals and boron

Question 24

specific O.N. rule for fluorine

Answer 24

O.N. = -1 in all compounds

Question 25

specific O.N. rule for oxygen

Answer 25

O.N. = -1 in peroxides
O.N. = -2 in all other compounds (except with F)

Question 26

specific O.N. rule for group 7A(17)

Answer 26

O.N. = -1 in combination with metals, nonmetals (except O), and other halogens lower in the group

Question 27

ideal gas law

Answer 27

PV=nRT

Question 28

STP

Answer 28

standard temperature & pressure - 273.15K & 1 atm

Question 29

standard molar volume

Answer 29

at STP 1 mol of ideal gas = 22.4L