Gen.chemistry Chapters 4, 10 & 11

Front 1

Rb

Back 1

rubidium

Front 2

Sr

Back 2

strontium

Front 3

Mo

Back 3

molybdenum

Front 4

Ag

Back 4

silver

Front 5

Cd

Back 5

cadium

Front 6

Sn

Back 6

tin

Front 7

Sb

Back 7

antimony

Front 8

I

Back 8

iodine

Front 9

Xe

Back 9

xenon

Front 10

Ca

Back 10

calcium

Front 11

Ba

Back 11

barium

Front 12

W

Back 12

tungsten

Front 13

Pt

Back 13

platinum

Front 14

Au

Back 14

gold

Front 15

Hg

Back 15

mercury

Front 16

Pb

Back 16

lead

Front 17

Rn

Back 17

radon

Front 18

U

Back 18

uranium

Front 19

Pu

Back 19

plutonium

Front 20

H

Back 20

hydrogen

Front 21

He

Back 21

helium

Front 22

Li

Back 22

lithium

Front 23

Be

Back 23

berrylium

Front 24

B

Back 24

boron

Front 25

C

Back 25

carbon

Front 26

N

Back 26

nitrogen

Front 27

O

Back 27

oxygen

Front 28

F

Back 28

flourine

Front 29

Ne

Back 29

neon

Front 30

Na

Back 30

sodium

Front 31

Mg

Back 31

magnesium

Front 32

Al

Back 32

aluminum

Front 33

Si

Back 33

silicon

Front 34

P

Back 34

phosphorous

Front 35

S

Back 35

sulfur

Front 36

Cl

Back 36

chlorine

Front 37

Ar

Back 37

argon

Front 38

K

Back 38

potassium

Front 39

Ca

Back 39

calcium

Front 40

Sc

Back 40

scandium

Front 41

Ti

Back 41

titanium

Front 42

V

Back 42

vanadium

Front 43

Cr

Back 43

chronium

Front 44

Mn

Back 44

manganese

Front 45

Fe

Back 45

iron

Front 46

Co

Back 46

cobalt

Front 47

Ni

Back 47

nickel

Front 48

Cu

Back 48

copper

Front 49

Zn

Back 49

zinc

Front 50

Ga

Back 50

gallium

Front 51

Ge

Back 51

germanium

Front 52

As

Back 52

arsenic

Front 53

Se

Back 53

selenium

Front 54

Br

Back 54

bromine

Front 55

Kr

Back 55

krypton

Front 56

Binary Ionic Compounds are named how?

Back 56

1. name of the metal as it appears in the periodic table
2. name of the nonmetal with ending changed to "ide"

Front 57

Group IA charge?
Group 2A charge?
Group 3A charge?
Group 5A charge?
Group 6A charge?
Group 7A charge?

Back 57

Group IA +1
Group 2A +2
Group 3A +3
Group 5A -3
Group 6A -2
Group 7A -1

Front 58

Name binary ionic compound:

PtCl2 =?

Back 58

platinum (II) chloride

Front 59

Name binary ionic compound:


Au2S

Back 59

gold (I) sulfide

Front 60

Name binary ionic compound:


Fe2S3

Back 60

iron (III) sulfide

Front 61

Name binary ionic compound:


Cu2O

Back 61

copper (I) oxide

Front 62

Name binary ionic compound:


AgCl

Back 62

silver chloride

Front 63

Name binary ionic compound:


Zn3N2

Back 63

zinc nitride

Front 64

Name binary ionic compound:


CdS

Back 64

cadmium sulfide

Front 65

group or family

Back 65

vertical columns

Front 66

periods

Back 66

horizontal rows

Front 67

Group 1A

Back 67

alkali metals

Front 68

Group 2A

Back 68

alkaline earth metals

Front 69

Group 6A

Back 69

chalogens

Front 70

Group 7A

Back 70

halogens

Front 71

Group 8A

Back 71

noble or inert gases

Front 72

Group 3B-3A

Back 72

transition metals

Front 73

nonmetals

Back 73

to the right of the stairstep

Front 74

metals

Back 74

to the left of the stairstep

Front 75

metalloids (7)

Back 75

B, Si, Ge, As, Sb, Te and At

Front 76

diatomic molecules (7)

Back 76

H, N, O, F, Cl, Br & I

Front 77

binary ionic compounds

Back 77

metal + nonmetal

Front 78

psuedo-binary ionic compounds

Back 78

-one of both of the parks will be polyatomic ions

Front 79

how to name psuedo-binary ionic compounds

Back 79

1st word- name of metal as it appears in the periodic table or the name of the polyatomic cation

2nd word- name of nonmetal with the ending changed to "ide" or the name of the polyatomic anion

Front 80

Name pseudo-binary compound:

NaOH

Back 80

sodium hydroxide

Front 81

Name pseudo-binary compound:

NH4SCN (use common polyatomic ions list)

Back 81

ammonium thiocyanate

Front 82

Name pseudo-binary compound:

CuCN (use common polyatomic ions list)

Back 82

Copper (I) cyanide

Front 83

Name pseudo-binary compound:

CuSO4 (use common polyatomic ions list)

Back 83

copper (II) sulfate

Front 84

Name pseudo-binary compound:

k2s2o3 (use common polyatomic ions list)

Back 84

potassium thiosulfate

Front 85

Name pseudo-binary compound:

CaC2O4 (use common polyatomic ions list)

Back 85

calcium oxylate

Front 86

covalent binary compounds

Back 86

usually contain 2 different nonmetals

Front 87

how to name covalent binary compound

Back 87

1st word- name of the first nonmetal as it appears in the periodic table with a prefix added

2nd word- name of the second nonmetal with the ending changed to "ide" and a prefix added

Front 88

name covalent binary:

PCL3

Back 88

phosphorous trichloride

Front 89

name covalent binary:

IF3

Back 89

iodine pentafluoride

Front 90

name covalent binary:

PCl5

Back 90

phosphorous pentachloride

Front 91

Name Covalent Binary Compound:

N2O4

Back 91

dinitrogen tetroxide

Front 92

Name Covalent Binary Compound:

Cl2O7

Back 92

dichlorine deptoxide

Front 93

Name Covalent Binary Compound:

I4O9

Back 93

tetraiodine nonoxide

Front 94

Name Covalent Binary Compound:

NO2

Back 94

nitrogen dioxide

Front 95

Name Covalent Binary Compound:

S2F10

Back 95

disulfurdecafluoride

Front 96

Name Covalent Binary Compound:

NaH

Back 96

sodium hydride

Front 97

Name Covalent Binary Compound:

HBr

Back 97

hydrogen bromide

Front 98

Name Covalent Binary Compound:

HCN

Back 98

hydrogen cyanide

Front 99

Name Covalent Binary Compound:

H2S

Back 99

hydrogen sulfide

Front 100

Name Covalent Binary Compound:

HCl

Back 100

hydrogen chloride

Front 101

binary acid

Back 101

covalent compounds

-Hydrogen plus a more electronegative element

-mono/di/tri/etc never use with acids

Front 102

how do you name a binary acid?

Back 102

1st word- name of the more electronegative element or polyatomic ion with the ending changed to "ic" and a hydro prefix added

2nd word- the word acid

Front 103

name the binary acid:

HCl

Back 103

hydrochloric acid

Front 104

name the binary acid:

HBr

Back 104

hydrobromic acid

Front 105

HCN

Back 105

hydrocyanic acid

Front 106

H2S

Back 106

hydrosulfuric acid

Front 107

ternary acids

Back 107

-acids consist of a more electronegative element, hydrogen and oxygen

-also known as oxyacids, b/c they contain oxygen

-mono/di/tri/etc never used with acids

-named using common acid root names known as "ic" acids

Front 108

how do you name ternary acids?

Back 108

1st word- determined systematically using the rules in the table

2nd word- the word acid

Front 109

number of oxygen atoms compared to corresponding"ic" acid= A

name change= B

Back 109

A B

+1 a "per" prefix is added
-1 the "ic" ending is changed to "ous"
-2 the "ic" ending is changed to "ous" and a "hypo" prefix is added

Front 110

using common ternary "ic" acid list, name ternary acid:

HBrO4

Back 110

bromic acid to

perbromic acid

Front 111

using common ternary "ic" acid list, name ternary acid:

HNO2

Back 111

derived from nitric acid

.... nitrous acid

Front 112

using common ternary "ic" acid list, name ternary acid:

H3PO2

Back 112

derived from phosphoric acid

..... hypophosphorous acid

Front 113

using common ternary "ic" acid list, name ternary acid:

HIO2

Back 113

derived from iodic acid

....iodous acid

Front 114

using common ternary "ic" acid list, name ternary acid:

HClO

Back 114

derived from chloric acid

.....hypochlorous acid

Front 115

ternary salts

Back 115

-result when acidic hydrogen atoms are replaced with other cations

-first word is named like other ionic compounds (name of metal or polyatomic cation)

-second word is name of the polyatomic anion derived from the ternary acid name

**if polyatomic anion is derived from IC changes to ATE
**if polyatomic anion is derived from OUR changes to ITE

Front 116

name ternary salt:

Na2CO3

Back 116

polyatomic anion derived from CARBONIC ACID (H2CO3).....

same number of oxygen atoms, the name is

sodium carbonate

Front 117

name ternary salt:

(NH4)2SO3

Back 117

derived from sulfuric acid (SO4)

.... one less O atom

sulfurous acid


=AMMONIUM SULFITE

Front 118

name ternary salt:

KIO

Back 118

derived from iodic acid (IO3)

... two less O atoms (hypoiodous acid)

same number of oxygens, name is

POTASSIUM HYPOIODITE

Front 119

name ternary salt:

LiClO4

Back 119

derived from chloric acid (ClO3)

.... one additional O atom= perchloric acid

... same number of O atoms, name is

LITHIUM PERCHLORATE

Front 120

name ternary salt:

Au(NO3)3

Back 120

derived from nitric acid (NO3)

same number of oxygen atoms...

gold (III) nitrate

Front 121

ternary acid salts

Back 121

-result from replacement of only some of the acidic hydrogen atoms in ternary acids with another cation

-endings are like ternary salts

Front 122

how you name ternary acid salts?

Back 122

1st word- name of metal or polyatomic cation

2nd word- hydrogen

3rd word- name of the polyatomic anion which is an acid derivative

**IC to ATE
**OUS to ITE

Front 123

name the ternary acid salt:

NaHCO3

Back 123

derived from carbonic acid (CO3)

same number of O atoms, the name is

SODIUM HYDROGEN CARBONATE

Front 124

name the ternary acid salt:

NaHSO4

Back 124

derived from sulfuric acid (SO4)

same number of O atoms, the name is

SODIUM HYDROGEN SULFATE

Front 125

name the ternary acid salt:

K2HPO3

Back 125

derived from phosphoric acid (PO4)

one less O atom= phosphorous acid

same number of O atoms, name is

POTASSIUM HYDROGEN PHOSPHITE

Front 126

name the ternary acid salt:

KH2PO3

Back 126

derived from phosphoric acid (PO4)

one less O atom= phosphorous acid

...name is
POTASSIUM DIHYDROGEN PHOSPHITE

Front 127

what is a combination or synthesis reaction?

Back 127

two or more substances react to form one product

Front 128

combination or synthesis reaction (A and B stuff) looks like?

Back 128

A + B --> AB

Front 129

what are the three possibilities for reactions with combination or synthesis reaction?

(element/compound)

Back 129

1. element + element = compound

2. compound + element = compound

3. compound + compound = compound

Front 130

what is

Mg + O2 --> 2MgO

and example of?

Back 130

combination or synthesis reaction

Front 131

these are all what?

2Na + O2 --> Na2O2

N2 + 3H2 --> 2NH3

CaO + H2) --> Ca(OH)2

Back 131

combination or synthesis reaction

Front 132

what is a decomposition reaction?

Back 132

conceptually, the opposite of the combination reaction, a compound breaks down into simpler substances

Front 133

what does decomposition reaction look like? (A and B stuff)?

Back 133

AY --> A + Y

Front 134

what are the three possibilities for reactions with decomposition reaction?

(element/compound)

Back 134

1. compound --> element + element

2. compound --> compound + element

3. compound --> compound + compound

Front 135

what are the three different types of reactions in aqueous solutions?

Back 135

combination or synthesis reaction

decomposition reaction

complete oxidation or combustion reaction

Front 136

what are these examples of?

CaCO3 --> CaO + CO2

2H2O --> 2H2 + O2

2KClO --> 2KCl + 3O2

PbCO3 --> PbO + CO2

Back 136

decomposition reactions

Front 137

what is a complete oxidation or combustion reaction?

Back 137

-rapid reaction which produce a flame

-this is called oxidation because of the reaction of a hydrocarbon plus environmental oxygen

-these hydrocarbons include petroleum products, alcohols, some acids, and sugars

Front 138

what does a hydrocarbon contain?

Back 138

C and H

OR

C, H and O

Front 139

what are the products of a complete oxidation or combustion reaction?

Back 139

products are ALWAYS CO2 and H2O

Front 140

what are these examples of?

C3H8 + 5O2 --> 3CO2 + 4H2)

C3H9OH + 6O2 --> 4CO2 + 5H2)

Back 140

complete oxidation or combustion reactions

Front 141

what is a solution?

Back 141

homogeneous mixture of 2 or more substances, in the liquid phase

Front 142

what is a solvent?

Back 142

major component of a solution

Front 143

what is a solute?

Back 143

minor component of the solution

Front 144

what are strong electrolytes?

Back 144

--good conductors

--form many of the IONS in aqueous solution (about 100%)

Front 145

what are weak electrolytes?

Back 145

--poor conductors

--form few IONS in aqueous solution (less than 5%)

Front 146

what are non electrolytes?

Back 146

--nonconductors

--form no ions in aqueous solutions

Front 147

what are acids?

Back 147

-covalent compounds

-substances that produce H+ ions, hydrogen ions or protons when dissolved in water

Front 148

what is ionization?

Back 148

physical process of converting an atom or molecule into an ion by adding or removing charged particles such as electrons or other ions

Front 149

What is HCL?

Back 149

HYDROCHLORIC ACID

Front 150

are strong acids strong or weak electrolytes?

are strong acids double or single arrow forward?

are strong acids reversible reactions?

Back 150

STRONG electrolytes

SINGLE arrow forward

NON-REVERSIBLE reactions

Front 151

What is HBR?

Back 151

hydrobromic acid

Front 152

What is HI?

Back 152

hydroiodic acid

Front 153

What is HNO?

Back 153

nitric acid

Front 154

What is H2SO4

Back 154

sulfuric acid

Front 155

What is HCLO3

Back 155

chloric acid

Front 156

What is HCLO4

Back 156

perchloric acid

Front 157

are weak acids strong or weak electrolytes?

are weak acids reversible reactions?

are weak acids SINGLE or DOUBLE froward arrows?

Back 157

weak acids are WEAK electrolytes

weak acids are REVERSIBLE reactions that do not go into completion

weak acids are DOUBLE arrow forward and reverse

Front 158

What is a monoprotic acid?

Back 158

yields 1 mole of H+ per mole of acid

Front 159

What is this an example of?

H2O + HCL --> H3O+ + CL-

Back 159

a MONOPROTIC acid

Front 160

What is a diprotic acid?

Back 160

yields 2 moles of H+ per mole of acid

occurs in TWO steps

Front 161

What is this an example of?

H2O + H2SO4 --> H3O+ + HSO4-
H2O + HSO4- --> H3O+ + SO42-

Back 161

a DIPROTIC acid

Front 162

What is a triprotic acid?

Back 162

yields 3 moles of H+ per mole of acid

occurs in THREE steps

Front 163

What is this an example of?

H2O + H3PO4 ---> H3O + + H2PO4-
<--

H2O + H2PO4- --> H3O+ + HPO42-
<--

H2O + HPO42- --> H3O+ + PO43-
<--

Back 163

a TRIPROTIC acid

Front 164

HCL ----> H+ + CL-

what is this? dissociation or ionization?

Back 164

BOTH

Front 165

What is a base?

Back 165

-substance that produces OH- ions, hydroxide ions when dissolved in aqueous solution

Front 166

is a strong base a strong electrolyte or weak?

is a strong base reversible?

is a strong base single or double arrow forward?

Back 166

strong base is STRONG electrolyte

strong base is NON-REVERSIBLE reaction that goes to completion

strong base is SINGLE arrow forward

Front 167

strong, soluble base

LiOH

Back 167

lithium hydroxide

Front 168

strong, soluble base

NaOH

Back 168

sodium hydroxide

Front 169

strong, soluble base

KOH

Back 169

potassium hydroxide

Front 170

strong, soluble base

RbOH

Back 170

rubidium hydroxide

Front 171

strong, soluble base

CsOH

Back 171

caesium hydroxide

Front 172

strong, soluble base

Ca(OH)2

Back 172

calcium hydroxide

Front 173

strong, soluble base

Sr(OH)2

Back 173

strontium hydroxide

Front 174

strong, soluble base

Ba(OH)2

Back 174

barium hydroxide

Front 175

Is a weak base a weak or strong electrolyte?

is a weak base reversible or non-reversible reaction?

is a weak base a single or double arrow?

Back 175

weak base is WEAK electrolyte

weak base is REVERSIBLE reaction that does not go into completion

weak base is DOUBLE arrow forward/reverse reaction

Front 176

is ammonia a weak or strong base?

Back 176

weak base. (not a salt)

Front 177

What is a salt?

Back 177

-ionic compound
-cationic portion comes from base
-anionic portion comes from acid
-if soluble, then STRONG electrolyte

Front 178

is a salt is soluble, what is it?

Back 178

STRONG electrolyte

Front 179

where does the cationic portion of a salt come from?

Back 179

a BASE

Front 180

where does the anionic portion of a salt come from?

Back 180

an ACID

Front 181

what is this an example of?

NaCL --> Na+ + CL-

MgSO4 --> Mg2+ + SO42-

Ca(NO3)2 --> Ca2+ + 2NO3-

Back 181

SALT dissociation

Front 182

what is an oxidation number or oxidation state?

Back 182

number of electrons gained or lost when an atom or group of atoms become ionized

Front 183

if something is a free element or molecule what is the oxidation state?

Back 183

oxidation state ZERO

Front 184

example of a free molecule with zero oxidation state?

Back 184

Fe
C
H2
S8

Front 185

if something is a monatomic ion what is the oxidation state?

Back 185

the CHARGE

Front 186

what is an example of a monatomic ion?

Back 186

Cl-
O2-
Fe3+
Mg2+

Front 187

what is the oxidation state of a polyatomic ion?

Back 187

the CHARGE

Front 188

what is an example of a polyatomic ion?

Back 188

NH4+
SO42-

Front 189

what is the oxidation state of a neutral compound?

Back 189

ZERO

Front 190

what is an example of a neutral compound?

Back 190

ZnSO4
NaCL

Front 191

what is the charge for
group1
group2
group3
group5
group6
group7

Back 191

group 1- +1
group 2- +2
group 3- +3
group 5- -3
group 6- -2
group 7- -1

Front 192

what is usually the charge for a hydrogen atom?

Back 192

+1

Front 193

what is usually the charge for an oxygen atom?

Back 193

-2

Front 194

what is the oxidation number for N, H and overall in...?

NH3

Back 194

N is -3
H is 1 (times 3)

overall= 0 charge

Front 195

What is the charge of N in

HNO2

Back 195

H= +1
O= -2 (times 2)= -4

1 + -4 + N= 0

N=3

Front 196

What is the charge of N in
N2O4

Back 196

N = 4

Front 197

What is the charge of N in

NO3-

Back 197

N= +5

Front 198

What is REDOX?

Back 198

OILRIG

Oxidation Involves Loss of electrons
Reductions Involves Gain of electrons

Front 199

oxidation is?

Back 199

LOSS of electrons

Front 200

reduction is?

Back 200

GAIN of electrons

Front 201

What is this an example of?

Zn --> Zn2+ + 2e-

(LOSS of electron)

Back 201

OXIDATION

Front 202

What is this an example of?

Cu2+ + 2e- --> Cu

(GAIN of electron)

Back 202

REDUCTION

Front 203

oxidations and reductions always occur __________, one chemical species GAINS electrons and the other chemical species LOSES electrons

Back 203

TOGETHER

Front 204

two half-reactions combine into a what?

Back 204

NET ionic equation

Front 205

what is this an example of?

Zn --> Zn2+ + 2e-
Cu2+ + 2e- --> Cu
________________
Zn + Cu2+ + 2e- (crossed out) -->
Zn2+ + Cu + 2e- (crossed out)

Back 205

NET IONIC EQUATION

Front 206

what is a reducing agent?

Back 206

OXIDIZED causing another substance to be reduced

Front 207

what is an oxidizing agent?

Back 207

REDUCED causing another substance to be oxidized

Front 208

reducing agent goes from one side of the equation with no charge to the other side being charged

true or false?

Back 208

TRUE

Front 209

oxidizing agent goes from one side of the equation with a charge to the other side being not charged

true or false?

Back 209

TRUE

Front 210

what is another term for REDOX?

Back 210

SINGLE-REPLACEMENT
SINGLE-DISPLACEMENT
OXIDATION-REDUCTION
or
REDOX

Front 211

oxidation

Back 211

reductant --> product + e-
(loss of e) --> (oxidation # increases)

Front 212

reduction

Back 212

oxidant + e- --> product
(gain of e) --> (oxidation # decreases)

Front 213

What is a redox reaction?

Back 213

-one element is replacing another in a compound

Front 214

what is this?
A + BC --> AC + B

A= more active metal
BC= less active metal salt
AC= more active metal salt
B= less active metal

Back 214

REDOX. TYPE ONE METAL

A + BC --> AC + B

A= more active metal
BC= less active metal salt
AC= more active metal salt
B= less active metal

Front 215

what is a more active metal?

Back 215

one that is higher in the activity series than the less active metal

Hint 215

type ONE metal

Front 216

what is a more active metal salt?

Back 216

one that contains a metal that is higher in the activity series than the metal in the less active metal salt

Hint 216

type ONE metal

Front 217

what does a type 2 metal REDOX look like?

Back 217

A + HX --> H2 + AX

Front 218

type 2 metal redox what is A, HX, H2 and AX?

Back 218

A= active metal
HX= acid
H2= hydrogen gas
AX= metal salt

Front 219

in type 2 metal redox what is an active metal?

Back 219

any metal above H in the activity series

Front 220

what does a type 3 metal REDOX look like?

Back 220

A + H20 --> H2 + AOH

Front 221

type 3 metal redox what is A and AOH?

Back 221

A=active metal
AOH= metal salt of water

Front 222

in order to react with water in a redox what must be true?

Back 222

it must be one of SIX top metals on activity series to react with water