Chem Test 2

Front 1

STERIC NUMBER

Back 1

(# OF ATOMS BONDED TO CENTER ATOM ) + (# LONE PAIRS ON CENTRAL ATOMS)

Front 2

LAW OF MULTIPLE PROPORTIONS

Back 2

COMPARISON BETWEEN 2 DIFFERENT COMPOUNDS

Front 3

LAW OF DEFINITE PROPORTIONS

Back 3

APPLIES TO A SINGLE COMPOUND (RATIO OF MASS IS CONSTANT)

Front 4

IONIC BONDING (3)

Back 4

*ELECTRONS LOST AND GAINED
*TRY TO BE LIKE NOBLE GASES
*METAL + NON METAL ONLY (SALT)

Front 5

COVALENT BONDING (6)

Back 5

*ELECTRONS SHARED
*CHEMICAL BOND
*NOT IONIC B/C NOT SALT
*NOT ACID B/C NO CHARGES
*NO CHARGED PARTICLES B/C NO METALS
*NO ELECTRICITY

Front 6

POLAR COVALENT BOND

Back 6

UNEQUAL SHARING OF E-

Front 7

VALENCE SHELL ELECTRON PAIR REPULSION MODEL (VSEPR MODEL)

Back 7

IMPLIED SHAPE OF E- PAIRS
NOT MOLECULAR SHAPE

LINEAR SHAPE - 2 ATOMS
TRIANGULAR
TETRAHEDRON
NON LINEAR OF V SHAPED

Front 8

LONE PAIRS

Back 8

NOT ATOMS
JUST 2E- THAT STILL NEED SPACE

Front 9

DIPOLE

Back 9

MOLECULE HAS POS AND NEG SIDE
IS CONSIDERED POLAR
TEND TO DISSOLVE IN OTHER DIPOLE SPECIES

EX) OIL NOT DISSOLVE IN WATER

Front 10

NOMENCLATURE OF SALTS

*note for transition metals

Back 10

*METAL CATION = ELEMENT NAME
*NON METAL ANION = ELEMENT NAME + IDE SUFFIX

TRANSITION METALS DONT HAVE VALENCE E- SO USE NUMBER F/ VALENCE E- OF OTHER NON TRANSITIONAL ELMENT

Front 11

GREEK NUMBER PREFIX

Back 11

1 NO PREFIX
2 DI
3 TRI
4 TETRA
5 PENTA
6 HEXA
8 OCTA
10 DECA

Front 12

NOMENCLATURE OF COVALENTLY BONDED COMPOUNDS

NON METAL + (NONMETAL or METALLOID)

Back 12

LEAST X ELEMENT W/ ATOM # PREFIX
MOST X ELEMENT WITH IDE SUFFIX & # PREFIX

Front 13

ELECTRONEGATIVITY (X) TRENDS

Back 13

X INCR (UP) AND -->

Front 14

H3O+

Back 14

HYDRONIUM

Front 15

NH4+

Back 15

AMMONIUM

Front 16

OH–

Back 16

HYDROXIDE

Front 17

O2 2–

Back 17

PEROXIDE

Front 18

O2 –1

Back 18

SUPEROXIDE

Front 19

CO3 2–

Back 19

CARBONATE

Front 20

H2CO3

Back 20

CARBONIC ACID

Front 21

HCO3–

Back 21

HYDROGEN CARBONATE

Front 22

NO3–

Back 22

NITRATE

Front 23

HNO3

Back 23

NITRIC ACID

Front 24

NO2 –1

Back 24

NITRITE

Front 25

HNO2

Back 25

NITROUS ACID

Front 26

PO4 3–

Back 26

PHOSPHATE

Front 27

H3PO4

Back 27

PHOSPHORIC ACID

Front 28

HPO4 2–

Back 28

HYDROGEN PHOSPHATE

Front 29

H2PO4 –1

Back 29

DIHYDROGEN PHOSPHATE

Front 30

SO4 2–

Back 30

SULFATE

Front 31

H2SO4

Back 31

SULFURIC ACID

Front 32

SO3 2–

Back 32

SULFITE

Front 33

H2SO3

Back 33

SULFUROUS ACID

Front 34

HSO4 –1

Back 34

HYDROGEN SULFATE

Front 35

HSO3 –1

Back 35

HYDROGEN SULFITE

Front 36

CN–

Back 36

CYANIDE

Front 37

MnO4 –1

Back 37

PERMANGANATE

Front 38

CrO4 2–

Back 38

CHROMATE

Front 39

SCN–

Back 39

thiocyanate

Front 40

TREND IN ACID NAMES

Back 40

*if oxy-anion name ends in -ate the acid ends in -ic
*if oxy-anion name ends in -ite the acid ends in -ous

Front 41

SOLUBILITY FOR NITRATES

Back 41

*NITRATES ALL SOLUBLE

Front 42

SOLUBILITY FOR AMMONIUM

Back 42

ALL SOLUBLE

Front 43

SOLUBILITY FOR

CHLORIDES
BROMIDES
IODIDES

Back 43

All are soluble except their Ag+, Pb 2+ and Hg2 2+ salts.

Front 44

SOLUBILITY FOR

HYDROXIDES
OXIDES

Back 44

All hydroxides and oxides: insoluble with exception of alkalai metals & Ca2+, Sr2+ and Ba2+.

Front 45

SOLUBILITY FOR SULFIDES

Back 45

All sulfides: insoluble with the exception of
alkalai & alkaline earth metals (Group I & II metals).

Front 46

H2SO4

Back 46

SULFURIC ACID

Front 47

SO3 2–

Back 47

SULFITE

Front 48

H2SO3

Back 48

SULFUROUS ACID

Front 49

HSO4 –1

Back 49

HYDROGEN SULFATE

Front 50

HSO3 –1

Back 50

HYDROGEN SULFITE

Front 51

CN–

Back 51

CYANIDE

Front 52

MnO4 –1

Back 52

PERMANGANATE

Front 53

CrO4 2–

Back 53

CHROMATE

Front 54

SCN–

Back 54

thiocyanate

Front 55

TREND IN ACID NAMES

Back 55

*if oxy-anion name ends in -ate the acid ends in -ic
*if oxy-anion name ends in -ite the acid ends in -ous

Front 56

SOLUBILITY FOR NITRATES

Back 56

*NITRATES ALL SOLUBLE

Front 57

SOLUBILITY FOR AMMONIUM

Back 57

ALL SOLUBLE

Front 58

SOLUBILITY FOR

CHLORIDES
BROMIDES
IODIDES

Back 58

All soluble EXCEPT their Ag+, Pb 2+ and Hg2 2+ salts.

Front 59

SOLUBILITY FOR

HYDROXIDES
OXIDES

Back 59

All hydroxides and oxides: INSOLUTLBE with EXCEPTION of alkalai metals & Ca2+, Sr2+ and Ba2+.

Front 60

SOLUBILITY FOR SULFIDES

Back 60

All sulfides: INSOLUBLE with the EXCEPTION of
alkalai & alkaline earth metals (Group I & II metals).

Front 61

SOLUBILITY FOR

PHOSPHATES
CARBONATES

Back 61

ALL phosphate & carbonates: INSOLUBLE with EXCEPTION of alkalai metals and ammonium.

Front 62

SOLUBILITY FOR SULFATES

Back 62

All sulfates are soluble with the exception of Ca2+, Sr2+, Ba2+ & Pb2+.

Front 63

PROCESS OF BALANCING A CHEMICAL REACTION IS JUSTIFIED BY:

Back 63

LAW OF CONSERVATION OF MASS
*ASSURES EQUAL # ATOMS BOTH SIDES
*EQUAL CHARGES LEFT AND RIGHT

Front 64

LIMITING REAGENT

Back 64

*WILL BE USED UP FIRST
*DEFINES THEORETICAL YIELD
*NOT CALCULATED BY MASS PROPORTIONS
*CHANGE F/ GRAMS->MOL AND COMPARE TO MOLES FROM BALANCED EQN

Front 65

PERCENT YIELD

Back 65

(ACTUAL YIELD)/(THEORETICAL YIELD) ALL X 100 %

Front 66

STOCHIOMETRY

Back 66

MASS RELATIONS APPLIED TO BALANCE CHEMICAL REACTIONS

Front 67

SOLUTION

Back 67

*HOMOGENEOUS MIXTURE OF 2OR MORE SUBSTANCES
*AKA ALLOYS (METAL + SOLID)
*USU DISSOLVED IN WATER
*AQUEOUS SOLUTION

Front 68

SOLVENT

Back 68

*ALWAYS ASSUME ITS WATER
*MAJOR COMPONENT
*DISSOLVING MEDIUM

Front 69

SOLUTE

Back 69

*MINOR COMPONENT
*PLACED ON SOLVENT

Front 70

SATURATION

Back 70

ACHIEVED WHEN LIMIT TO HOW MUCH SOLUTE CAN BE DISSOLVED IN WATER IS REACHED.

Front 71

UNSATURATION

Back 71

BEFORE LIMIT IS REACHED

Front 72

SATURATION TREND

Back 72

COMPOUNDS: SIMILAR -> MIXED IN ANY PROPORTIONS
ALSO TEMP DEPENDENT

Front 73

MISCIBLE

Back 73

NO LIMIT TO SOLUBILITY

Front 74

SUPER SATURATION SOLUTION

Back 74

*UNSTABLE SOLUTION
*WHEN SOLUBILITY LIMIT OF SUBSTANCE HAS BEEN EXCEEDED

Front 75

NaC2H3O2

Back 75

SODIUM ACETATE

Front 76

MOLARITY (M)

Back 76

[MOLES SOLUTE (DISSOLVED MATERIAL)] / [LITERS SOLUTION (VOLUME)]

HIGH MOLARITY = LOTS OF SOLUTE IN SOLUTION

[ACETONE] = MOLARITY OF ACETONE

Front 77

C12H22O11

Back 77

SUGAR

Front 78

TYPES OF REACTIONS (3)

Back 78

1.DISSOLUTION/PRECIPITATION
2.OXIDATION REDUCTION (REDOX)
3.ACID BASE

Front 79

PRECIPITATION

Back 79

PARTICLES F/ SOLUTION FORM A SOLID

Front 80

DISSOLUTION

Back 80

*GOES F/ SOLID TO LIQUID
*FORMS A CONDUCTING SOLUTION

Front 81

SPECTATOR ION

Back 81

NON PARTICIPANT IN PRECIP RXN

Front 82

ELECTROLYTE

Back 82

*SUBSTANCE DISSOLVED IN H20
*PRODUCED BY DISSOLUTIN RXN
*FORMS SEPARATE CATIONS/ANIONS

Front 83

DIFFERENCE B/W PRECIPITATION IN SALTS

Back 83

SOLUBILITY

Front 84

SOLUBLE SALT

Back 84

*WILL DISSOLVE IN AQUEOUS SOLUTION
*IF >1 GRAM DISSOLVE IN 1 LITER

Front 85

ACID

Back 85

*"DISSOLVES" METALS (PREATOMIC)
*SOUR TASTE
*DYE LITMUS = RED
*HAS IONIC BOND (HAS CHARGES = NOT COVALENT)
*ELEMENT Y MUST HAV >X THAN H
*IF =ELECT X,NOT POLAR, NOT ACID
*H+ DONOR
*NOT ACID UNLES H IS PRESENT

Front 86

BASE

Back 86

*H+ ACCEPTOR
*BITTER TASTE
*TURN LITMUS BLUE
*LONE PAIR OF E- MUST BE PRESENT

Front 87

CONJUGATE BASE OF ACID

Back 87

FRAGMENT LEFT AFTER H+ IS ACCEPTED

*TO GET IT REMOVE H+ FROM ACID

Front 88

CONJUGATE ACID OF BASE

Back 88

*SPECIE PRODUCED WHEN H+ IS ACCEPTED
*TO GET IT ADD H+ TO BASE

Front 89

DISSOLUTIN REACTION OF SALT AND WATER

Back 89

ANIONS AND CATIONS BREAK APART (PHYSICAL PROCESS NO CHEM CHANGE)
FORMULA IS CHEM CHANGE B/C SOMETHING NEW HAS BEEN CREATED.

Front 90

HC2H3O2

Back 90

VINEGAR

Front 91

TREND IN SALT/ELECTROLYTES

Back 91

ALL SALTS ARE STRONG ELECTROLYTES CUS THEY GO 100% INTO ION FORMATION AS IT DISSOLVES.
*FEW IONS LOW CONDUCTIVITY.

Front 92

EXAMPLES OF WEAK ACIDS

Back 92

VITAMIN C, ASPIRIN, CITRIC ACID

Front 93

EX) OF STRONG ACIDS

Back 93

HCL, SULFURIC ACID , NITRIC ACID

Front 94

H2SO4

Back 94

SULFURIC ACID

Front 95

HNO3

Back 95

NITRIC ACID

Front 96

OXIDES OF ELEMENTS

Back 96

*THEY ARE ANHYDRIDES OF ACIDS AND BASES.
*ADDING MORE OXYGEN TO AN ELEMENT MAKES IT MORE ACIDIC OR BASIC.

Front 97

METAL OXIDE

Back 97

*BASE ANHYDRIDES
*MORE METTALLIC = STRONGER BASE

Front 98

METAL OXIDES

Back 98

*BASE ANHYDRIDES
*MORE METALLIC = STRONGER BASE

Front 99

NON METALLIC OXIDES

Back 99

*ACID ANHYDRIDES
*MORE NONMETALLIC = STRONGER ACID

Front 100

AMPHOTERIC SUBSTANCE

Back 100

FUNCTIONS AS ACID AND BASE
EX) WATER CAN FUNCTION AS BOTH
IT IS ALSO NEUTRAL

Front 101

HALOGEN-HYDROGEN COMPOUNDS

Back 101

SPECIAL CLASS OF NON OXYGEN CONTAINING ACIDS
EX)HF, HCL, HBr, HI

Front 102

H2CO3

Back 102

CARBONIC ACID

Front 103

NEUTRALIZATION REACTION

Back 103

WHEN A STRONG ACID REACTS WITH A STRONG BASE

Front 104

REDOX RXN FOR GRP 1 METALS

Back 104

+1

Front 105

REDOX RXN FOR GRP 2 METALS

Back 105

+2

Front 106

REDOX RXN FOR FLUORINE

Back 106

-1

Front 107

REDOX RXN FOR GRP 7

Back 107

-1 EXCEPT FOR COMPOUNDS WITH F OR O : FLUORINE OR OXYGEN WHERE IT CAN BE POSITIVE

Front 108

REDOX RXN FOR HYDROGEN

Back 108

+1 IN COMPOUNDS

-1 IN GRP 1 AND 2 METALS

Front 109

REDOX RXN FOR OXYGEN

Back 109

-2 UNLESS W/ F (F TAKES PRECEDENCE)

-1 IN PEROXIDES LIKE H202

Front 110

REDUCTION

Back 110

*GAIN OF E-
*REDUCTION IN OXIDATION #

Front 111

OXIDATION

Back 111

*LOSS OF E-
*INCREASE IN OXIDATIN #

Front 112

REDUCIING AGENT

Back 112

*THE SUPPLIER/DONOR OF E-
*LOSING ELECTRONS
*BEING OXIDIZED

Front 113

OXIDIZING AGENT

Back 113

*THE ACCEPTOR OF E-
*GAINING ELECTRONS
*BEING REDUCED

Front 114

AVOGADRO'S LAW

Back 114

V IS PROP TO N (MOLES)

Front 115

CHARLES LAW

Back 115

V IS PROP TO T

Front 116

BOYLE'S LAW

Back 116

V IS INVERSLY PROP TO P

Front 117

IDEAL GAS LAW

Back 117

*PV=NRT
*PV = (G/MW)RT

Front 118

DALTON'S LAW OF PARTIAL PRESSURE

Back 118

TOTAL PRESSURE = SUM OF INDIVIDUAL PRESSURES OF EACH GAS BY ITSELF

Front 119

PARTIAL PRESSURE

Back 119

PRESSURE EXERTED IF THE GAS WERE ALONE IN THE CONTAINER W/O OTHER GASES

Front 120

UNITS OF PRESSURE (3)

Back 120

*SI UNIT Pa
* 1 ATM = 101325 Pa = 760 mm Hg
*TORR = mm Hg

Front 121

UNITS OF VOLUME

Back 121

SI UNIT m3 BUT USU LITERS

Front 122

R: GAS LAW CONSTANT

Back 122

R = .08206 L ATM
_____________
MOL K

Front 123

STP

Back 123

* STANDARD TEMP AND PRESSURE
* T = 273 K OR 0*C
* P = 1 ATM

Front 124

UNIT OF TEMP

Back 124

KELVIN

K = C + 273`