Chem Final Exam

Front 1

Chemistry

Back 1

study of science that deals with matter

Front 2

matter

Back 2

has mass and takes up space

Front 3

chemical change

Back 3

AKA chemical reaction

Front 4

Chemical properties

Back 4

the chemical reaction a substance overgoes

Front 5

physical properties

Back 5

properties that do not involve chemical reactions

Front 6

scientific method

Back 6

tool, testing theories

Front 7

fact

Back 7

statement based on direct experience

Front 8

hypothesis

Back 8

statement proposed to explain facts and relationships

Front 9

theory

Back 9

the formulation of apparent relationships among certain observed phenomenon

Front 10

serendipity

Back 10

chance observations leading to discoveries

Front 11

significant figures

Back 11

see Appendix II

Front 12

Length
5280 ft

Back 12

one mile

Front 13

Length
1760 yds

Back 13

one mile

Front 14

Length
3 ft

Back 14

1 yd

Front 15

Length
12 "

Back 15

1 ft

Front 16

length
1 KM

Back 16

1000 M

Front 17

1 cm

Back 17

.01 M

Front 18

Metric prefixes
giga G

Back 18

10e9, 1 billion

Front 19

Metric prefixes
Mega M

Back 19

10e6, 1 million

Front 20

Metric prefixes
Kilo K

Back 20

10e3, 1000

Front 21

Metric prefixes
deci d

Back 21

10e-1, .1 or 1/10

Front 22

Metric prefixes
centi c

Back 22

10e-2, .01 or 1/100

Front 23

Metric prefixes
milli m

Back 23

10e-3, 001 1/1000

Front 24

Metric prefixes
micro

Back 24

10e-6, .000001 1/1 million

Front 25

Metric prefixes
nano, n

Back 25

10e-9, .000000001 1/1 billion

Front 26

Conversion factors
Length
1 in =

Back 26

2.54 cm

Front 27

Conversion factors
Length
1 meter

Back 27

39.37 in

Front 28

Conversion factors
Length
1 mile

Back 28

1,609 km

Front 29

Conversion factors
Mass
1 oz

Back 29

28.35 g

Front 30

Conversion factors
Mass
1 lb

Back 30

453.6 g

Front 31

Conversion factors
mass
1 kg

Back 31

2.206 lb

Front 32

Conversion factors
mass
1 g

Back 32

15.43 grains

Front 33

Conversion factors
Volume
1 qt

Back 33

0.946 L

Front 34

Conversion factors
Volume
1 gal

Back 34

3.785 L

Front 35

Conversion factors
Volume
1 L

Back 35

33.81 fl oz

Front 36

Conversion factors
Volume
1 fl oz

Back 36

29.57 ml

Front 37

Conversion factors
Volume
1 L

Back 37

1.057 quart

Front 38

1 ml

Back 38

.001 L

Front 39

100 ml

Back 39

1 L

Front 40

1 ml

Back 40

1 cc

Front 41

1000 cc

Back 41

1 L

Front 42

1 kg

Back 42

1000 g

Front 43

1 mg

Back 43

.001 g

Front 44

Temp
F

Back 44

9/5 degrees C + 32

Front 45

Temp
C

Back 45

5/9 (degrees F -32)
ex: 5/9 (98.6-32) = 5/9 (66.6)= 37.0 degrees C

Front 46

Factor Label Method

Back 46

when multiplying/dividing numbers we also multiply/divide units

Front 47

denisity

Back 47

d = m/v
ex: 61.5 g/73.2 ml = .84 g/ml

Front 48

specific gravity

Back 48

dimensionless - defined as conparison of the denisty of a substance with the density of H20

Front 49

energy

Back 49

capacity to do work

Front 50

kinetic energy

Back 50

energy of motion; any moving object

Front 51

potential energy

Back 51

stored energy

Front 52

Law of Conservation of energy

Back 52

energy can't be created or destroyed

Front 53

Heat

Back 53

form of energy (temperature is not); measured in calories
1 Kilocalorie = 1000 cal = 1 Kcal

Front 54

1 cal =

Back 54

4.184 J

Front 55

specific heat

Back 55

amount of heat necessary to raise 1 g of any substance by 1 degree C

Front 56

element

Back 56

substance consisting of identical atoms; 116 known, 88 occur in nature

Front 57

compound

Back 57

pure substance made up of 2 or more elements in a fixed ratio by mass; 20 M known compounds

Front 58

mixture

Back 58

combination of 2 or more pure substances

Front 59

atoms

Back 59

make up all matter

Front 60

molecule

Back 60

combination of 2 or more atoms that act as a single unit

Front 61

Law of Conservation of Mass

Back 61

any compound is always made up of elements in the same proportion by mass

Front 62

monatomic elements

Back 62

single atoms not connected to each other

Front 63

diatomic elements

Back 63

H2, N2, F2, CL2, BR2, I2

Front 64

polyatomic elements

Back 64

diamonds; S8

Front 65

Proton

Back 65

subatomic particle with charge of +1 and a mass of approximately 1 amu, found in neucleus

Front 66

amu

Back 66

1 amu = 6.605 x 1-e-24 g; 1/2 the mass of a carbon atom containing 6 protons and 6 neutrons

Front 67

electron

Back 67

subatomic particle with charge of -1 and mass of approximately .0005 amu

Front 68

neutron

Back 68

subatomic particle with mass of approximately 1 amu and charge of 0; found in neucleus

Front 69

mass number

Back 69

number of protons and neutrons in the nucleus of an atom

Front 70

atomic number

Back 70

number of protons in the nucleus of an atom

Front 71

isotopes

Back 71

same number of protons but different numbers of neutrons; differ in radioactivity properties

Front 72

atomic weight

Back 72

weighted average of the masses (in amu) of its isotopes found on earth

Front 73

properties of metals

Back 73

solid (except mercury)
shiny
conduct electricity
malleable

Front 74

alloys

Back 74

solutions of 1 or more metals dissolved in another metal

Front 75

non-metals

Back 75

don't conduct electricity

Front 76

mettaloids

Back 76

boron, silicon, germanium, arsenic, antimony and tellurium

Front 77

halogens

Back 77

melting/boiling points increase as we go down the column

Front 78

alkali

Back 78

group 1A; can be cut with a knife

Front 79

noble gases

Back 79

group 8A

Front 80

ground state electron configuration

Back 80

electron configuration of the lowest energy state of an atom

Front 81

Distribution of electrons in Shells
Shell 4

Back 81

Shell can hold 32 electrons, subshell s

Front 82

Distribution of electrons in Shells
shell 3

Back 82

can hold 18 electrons, subshell p

Front 83

Distribution of electrons in Shells
shell 2

Back 83

can hold 8 electrons, subshell d

Front 84

Distribution of electrons in Shells
shell 1

Back 84

can hold 2 electrons, subshell f

Front 85

electron configuration

Back 85

description of the orbitals of an atom or ion occupied by electrons

Front 86

valence electron

Back 86

an electron in the outermost occupied (valence) shell of an atom

Front 87

valence shell

Back 87

the outermost occupied shell of an atom

Front 88

Lewis Dot Structure

Back 88

the symbol of the element surrounded by a number of dots equal to the number of electrons in their outer shell

Front 89

He and Ne - (noble gases)

Back 89

have filled valence shells

Front 90

Electrons in Periodic Table

Back 90

elements in same column have the same configuration of electrons in their outer shell

Front 91

2 kinds of chemical bonds

Back 91

ionic and covalent

Front 92

octet rule

Back 92

groups 1A - 7A - gains/loses or shares electrons to have 8 in the valence shell in chemical reaction - doesn't apply to 1B - 7B

Front 93

anion

Back 93

negatively charged ion

Front 94

cation

Back 94

positively charged ion

Front 95

monatonic cations:
Cu+

Back 95

Cuprous ion; Copper (I) ion

Front 96

monatonic cations:
Cu2+

Back 96

Cupric ion; copper (II) ion

Front 97

monatonic cations:
Fe 2+

Back 97

Ferrous ion; Iron (II) ion

Front 98

monatonic cations:
Fe 3+

Back 98

Ferric ion; Iron (III) ion

Front 99

monatonic cations:
Hg+

Back 99

Mercuric ion; Mercuey (II) ion

Front 100

monatonic cations:
Sn2+

Back 100

Stannic ion; Tin (ii) ion

Front 101

Monatomic anions:
F-

Back 101

fluoride

Front 102

Monatomic anions:
Cl-

Back 102

Chloride

Front 103

Monatomic anions:
Br-

Back 103

Bromide

Front 104

Monatomic anions:
I-

Back 104

Iodide

Front 105

Monatomic anions:
O2-

Back 105

Oxide

Front 106

Monatomic anions:
S 2-

Back 106

Sulfide

Front 107

Polyatomic ions (Common):
NH+

Back 107

ammonium

Front 108

Polyatomic ions (Common):OH4-

Back 108

Hydroxide

Front 109

Polyatomic ions (Common):NO2

Back 109

Nitrite

Front 110

Polyatomic ions (Common):N03 2-

Back 110

Nitrate

Front 111

Polyatomic ions (Common):
CH3 Coo-

Back 111

acetate

Front 112

Polyatomic ions (Common):
CN-

Back 112

cyanide

Front 113

Polyatomic ions (Common):MnO4-

Back 113

Permanganate

Front 114

Polyatomic ions (Common):CrO4 -2

Back 114

chromate

Front 115

Polyatomic ions (Common):
CO3 2-

Back 115

carbonate

Front 116

Polyatomic ions (Common):
HCO 3 -

Back 116

hydrogen carbonate

Front 117

Polyatomic ions (Common):
SO3 2-

Back 117

sulfite

Front 118

Polyatomic ions (Common):
HSO 3 -

Back 118

Hydrogen sulfite

Front 119

Polyatomic ions (Common):
SO4 2-

Back 119

Sulfate

Front 120

Polyatomic ions (Common):
HSO 4-

Back 120

hydrogen sulfate

Front 121

Polyatomic ions (Common):
PO4 2-

Back 121

phosphate

Front 122

Polyatomic ions (Common):
HPO4 2-

Back 122

hydrogen phosphate

Front 123

Polyatomic ions (Common):
H2 PO4 -

Back 123

dihydrogen phosphate

Front 124

ionic bond

Back 124

results from attraction between cation and anion

Front 125

covalent bond

Back 125

results from attraction between 2 atoms that share on or more pairs of electrons

Front 126

How to tell if ionic or covalent bond?

Back 126

ionic - usually forms between metal and non metal
covalent - usually forms between nonmetal/metalloid and nonmetal combine;
compare electronegativity

Front 127

electronegativity

Back 127

measure of an atom's attraction for the electrons it shares in a chemical bond with another atom

Front 128

How does ionic bond form?

Back 128

forms by transfer of 1 or mroe valence shell electrons from an atom of lower electr4onegativity to valence shell of an atom of higher electronegativity; more likely to occur if difference in electronegativity between 2 atoms is 1.9 or greater' covalent <1.9

Front 129

ionic compound

Back 129

formed by combination of + and - ions

Front 130

Predicting formulas of ionic compounds

Back 130

sum of ions and sum of + charges = sum of negative charges; subscripts represent ratio of the ions

Front 131

Naming Ionic compounds
binary compound -

Back 131

contains only 2 elements

Front 132

Naming Ionic compounds
binary ionic compound

Back 132

consists of name of metal (+ ion - cation) was formed, followed by name of anion (- ion; ignor subscripts in binary ionic compound naming

Front 133

How does covalent bond form?

Back 133

forms when electron bonds are shared between 2 atoms whose difference in electronegativity is < 1.9 (2 nonmetals or between nonmetal & metalloid)

Front 134

single bond

Back 134

sharing a pari of electrons (represented by a single line ex: H-H

Front 135

Chemical Bond Classification:
<.5

Back 135

Non-polar covalent - 2 non metals or a metal and a nonmetal

Front 136

Chemical Bond Classification:
0.5 to 1.9

Back 136

polar covalent; 2 non-metals or nonmetal & metalloid

Front 137

Chemical Bond Classification:
>1.9

Back 137

Ionic; a metal and a nonmetal

Front 138

bonding electrons

Back 138

valence elctrons involved in forming a covalent bond (shared electrons)

Front 139

non-bonding electrons

Back 139

valence elctrons not involved in forming covalent bonds (unshared electrons)

Front 140

Lewis structure

Back 140

formula for a molecule or ion showing all pairs of bonding electrons as single, double or triple bonds and all nonbonded electtrons as pairs of Lewis dots

Front 141

Structural formula

Back 141

formula showing how atoms in a molecule or ion were bonded to each other; similar to Leis structure expect shows only bonding pairs of electrons

Front 142

naming binary covalent compounds

Back 142

2 element compound with all covalent bonds:
1) name the less electronegative element (1st in formula)
2) name the more elctronegative element and add ide to the stem name
3) use di, tri, tetra to show number of atoms of each element

Front 143

How to predict bond angles (covalent molecules)

Back 143

use VSEPR; atoms spread out so eacfh is as far as possible from the others

Front 144

All H-C-H bond angles are

Back 144

109.5

Front 145

Methane bond angle

Back 145

tetrahedral

Front 146

water bond angle

Back 146

bent

Front 147

ammonia bond angle

Back 147

pyramidal

Front 148

ammonia molecule

Back 148

pyramidal

Front 149

formaldehyde & ethylene are

Back 149

120 degrees - trigonal planar

Front 150

carbon dioxide & acetylene

Back 150

linear and 180 degrees

Front 151

chemical reaction

Back 151

chemical change; reactants converted into products

Front 152

formula weight (FW)

Back 152

sum of atomic weights in amu of all atoms in compound's formula

Front 153

molecular weight

Back 153

strictly correct only when used for covalent compounds

Front 154

mole

Back 154

amount of substance that contains as many atoms, molecules or ions as there are atoms in exactly 12 g of Carbon -12

Front 155

Avogadro's number

Back 155

6.02 x 10e23 formula units per mole

Front 156

molar mass

Back 156

FW of substance expressed in grams

Front 157

combustion

Back 157

burning in air

Front 158

chemical equation

Back 158

a representation using chemical formulas of the process that occurs when reactants are convered to products

Front 159

balancing chemical equations

Back 159

1 - start with C or H
2 - balance free elements last
3 - change only coefficients in balancing equation

Front 160

actual yield

Back 160

mass of product formed in chemical reaction

Front 161

theoretical yield

Back 161

mass of product that should form in a chemical reaction according to stoichimetry of the balanced equation

Front 162

percent yield

Back 162

actual yield divided by theoretical yield X 100
% yield = actual yield/theoretical yield X 100

Front 163

dissociation -

Back 163

dissolved in H2) and the + and - ions become separated by H20 molecules

Front 164

aqueous solution

Back 164

solution in which the solvent is H20

Front 165

spectator ion

Back 165

ion that appears unchanged on both sides of a chemical equation

Front 166

net ionic equation

Back 166

chemical equation that does not contain spectator ions (show only ions that react)

Front 167

ions react only when

Back 167

1 - 2 ions form a solid in soluble H20 (most common)
2 - 2 ions form a gas that escapes from the reaction mixture as bubbles
3 - one of the ions can oxidize another
4 - an acid neutralizes a base

Front 168

most chlorides (Cl-) and sulfates (SO4 2-) are soluble in H20 (see back for exceptions)

Back 168

silver chloride (AgCl), lead (II) chloride (PbCl2)mercury (I) chloride (Hg2Cl2), barium sulfate (BaSO4) and lead sulfate (PbSO4) - NOT SOLUBLE IN H20

Front 169

Most carbonates (CO3 2-), phosphates (PO4 3-), sulfides (S 2-_and hydroxides (OH-_ are insoluble in H20

Back 169

exeptions LiOH, NaOHI, KOH, and aqueous NH3 ARE soluble in H20

Front 170

oxidation - reduction reaction

Back 170

AKA redox reaction; transfer of electrons from 2 species to another

Front 171

oxidizing agent

Back 171

an entity that accepts electrons in an oxidation-reduction reaction

Front 172

reducing agent

Back 172

an entity that donates electrons in an oxidation-reduction reaction

Front 173

oxidation

Back 173

gain of oxygen and/or loss of hydrogen

Front 174

reduction

Back 174

loss of oxygen and/or gain of hydrogen

Front 175

gas

Back 175

molecules far apart and disorganized; little interaction

Front 176

liquid

Back 176

intermediate situation

Front 177

solid

Back 177

molecules close together and ordered; strong interaction between molecules

Front 178

The number 12574.78 rounded to 3 significant figures will be

Back 178

1.25 x 10e4

Front 179

Which of the following changes is an example of a chemical change?
a - heating water
b - ice melting
c - cooking food
d - alcohol evaporating
e - condensing steam

Back 179

c - cooking of food

Front 180

When a strong magnet is brought near to a sample which is known to contain both iron and sulfur, the iron and sulfur are not separated from one another. Wha type of material is this sample?
a - a compound
b - a homogeneous mixture
c - a heterogeneous mixture
d - an element

Back 180

a - a compound

Front 181

A statement that is made to explain an observation is called
a - a hypothesis
b - a theory
c - a fact
d - a law
e - an equation

Back 181

a hypothesis

Front 182

Gasline is immiscible in water. The density of gasoline is 0.025 g/mL at 20 degrees C. When gasoline is added to water (denisty of water is 1.0 g/mL):
a - it will float on top
b - it will sink to the bottom
c - it will mix so you can't see it
d - the mixture will ijprove the running of the motor
c - none of these things will happen

Back 182

it will float on top

Front 183

A block of a material of mass 25 grams and volume of 1 cm3 is dropped in water. How much water would it displace?
a - 15 cc
b - 25 cc
c - 40 cc
d - 50 cc

Back 183

15 cc

Front 184

Which of the following elements is a halogen?
a - Ag
B - Br
c - B
d - N
e - Fe

Back 184

Br

Front 185

Which of the following postulates from Dalton's atomic theory are now known to be incorect?
i) matter is made up of atoms
ii) atoms are individisible and indestructible
iii) all atoms of a given element are identical

Back 185

(ii) and (iii)

Front 186

What is the name of the lement with a mass number 45 and 24 neutrons?
a - chromium
b - Scandium
c - Rhodium
D - Titanium
e - thulium

Back 186

b - Scandium

Front 187

The three common isotopes of hydrogen has
a - the same mass number and equal number of protons
b - the same atomic number and equal number of protons
c - the same atomic number and equal number of neutrons
d - the same mass number and equal number of electrons
e - the same mass number and equal number of protons

Back 187

the same atomic number and equal number of protons

Front 188

Which three elements are likely to have similar chemical and physical properties?
a nitrogen, oxygen, and neon
b. sodium, magnesium and alumininum
c. calcium, strontium and barium
d. nickel, copper and zinc
e. uranium, plutonium and americium

Back 188

calcium, strontium and barium

Front 189

Which of these is not a stable ion?
a. Ba+
b. Li+
c. Br-
d Se 2-
e. P3-

Back 189

Ba+

Front 190

Thelement aluminum is mostly likely to form which of these ions?
a. Al+
b. Al2+
c. Al3+
d. Al3-
e. Al5-

Back 190

Al3+

Front 191

A nitride ion has ____ electrons?

Back 191

10

Front 192

Vanadium (v) with 30 neutrons has an atomic number of ____ and _____ electrons. (V is a roman numeral)

Back 192

23, 18

Front 193

Elemments in which group are most likely o form ions with -3 charge?
Group I
Group II
Group II
Group IV
Group V

Back 193

Group V

Front 194

Which of the following pairs have the same number of electrons?
Cu2+ and Cu+
a2+ and Mg2+
Cl and Br-
F- and O2-
H+ and H-

Back 194

F- and O2-

Front 195

A good example of an ionic compound is
H20
C2H5OH
Dry ice solid Co2)
K2CO3
CH4

Back 195

K2CO3

Front 196

Which of the following pairs will form a polar covalent bond?Ca - CL
Cl - Cl
Mn - Cl
N - Cl
Ni - Cl

Back 196

N - Cl

Front 197

A battery stores chemical potential energy. Into what form of kinetic energy can this potntial energy be converted to play a radio?
a - thermal energy
b - electrical energy
c - radiant energy
d - electrostatic energy
e - mechanical energy

Back 197

electrical energy

Front 198

You an drive at a speed of 65 miles per hour whereas your spouse can drive at a speed of 35 meters per second. Explain with appropriate calculations who can drive faster.

Back 198

65 mph = ? meters per second
65 mi/hr x 1.609 km/1 mi x 1000 mi/km x 1 hr/60 min x 1 min/60 sec = 29 meters/second
Spouse can drive faster at a speed of 35 meters per second

Front 199

The temperature of Monday is 88 degrees F and that of Tuesday is 25 degrees C. Which day is hotter? Show your work

Back 199

C = 5/9 (F-32)
c = 5/9 (88-32)
c = 5/9 (56)
c = 31 degrees
Tuesday is hotter

Front 200

You can identify a metal by careful determining its density "d". An unknown piece of metal, wth a mass of 29.454 g, is 2.35 cm long, 1.34 cm wide, and 1.05 cm thick. Which of the following is the element?
Nickel, d = 8.91 g/cm3
Titanium, d = r.t0 g/cm3
Zinc, d = 7.14 g/cm3
Tin, d= 7.23 g/cm3

Back 200

d = m/v
29.454 g/2.35 cm x 1.34 cm x 1.05 cm = 29.454/3.306.45 = 8.90804337 g/cm3

Front 201

Complete the following. Show your work:

Back 201

Protons = electrons
atomic # = # of protons
mass # - protons = neutrons

Front 202

Compelte the formulas for the compounds formed and name each compound:

Fe 2+ and Br- =

Back 202

FeBr2

Front 203

Compelte the formulas for the compounds formed and name each compound:
Li+ and Br- =

Back 203

LiBr

Front 204

Compelte the formulas for the compounds formed and name each compound:
Li+ and O2- =

Back 204

Li2O

Front 205

Compelte the formulas for the compounds formed and name each compound:
Li+ and PO4 3- =

Back 205

Li3PO4

Front 206

Compelte the formulas for the compounds formed and name each compound:
Fe2+ and Br-

Back 206

FeBr2

Front 207

Compelte the formulas for the compounds formed and name each compound:
Fe2+ and O2-

Back 207

FeO

Front 208

Compelte the formulas for the compounds formed and name each compound:
Fe2+ and Po4 3-

Back 208

Fe3 (PO4)2
Ferrous Phosphate

Front 209

Compelte the formulas for the compounds formed and name each compound:
Al3+ and Br -

Back 209

AlBr3
Aluminium bromide

Front 210

Al3+ and O2-

Back 210

Al2O3
aluminium oxide

Front 211

Al3+ and PO4 3-

Back 211

Al(PO4)
aluminum phosphate

Front 212

A house is made of wood and glass. Assuming an equal amount of sunshine falls on a wooden wall and a piece of clean glass (of equal mass), which warms more? The specific heats of wood and glass are 1.76 J/g.K and 0.84 J/g.K respectively. Explain briefly.

Back 212

Wood is used i home bulding as insulation from heat and cold which would indicate it does nto doncut heat or cold as well as glass. The specific heat required to raise 1 g of wood is 1.87J/g.K whereas it only takes 0.84J/g.K to raise the temperature of 1 g of glass. This means that glass warms much easier than wood To raise the temperature of wood one degree requires more energy than the glass.

Front 213

The number 5 X 10e3 written in exponential notation, can be written in full as
a - .005
b - 0.05
c - 500
d - 5000

Back 213

0.005

Front 214

An example of a pure subsance is:
a - blood
b - salt
c - milk
d - air

Back 214

salt

Front 215

Which is a chemical change?
a - melting of snow
b - making tea from tea bag
c - distilling ocean water
d - dropping alka seltzer tablet in water

Back 215

dropping alka seltzer tablet in water

Front 216

The density of gsoline is 0.7025 g/mL at 20 degrees C. When gasoline is added to water denisty of water is 1.00 g/mL):
a - it will float on top
b - it will sink to the bottom
c - the mixture will improve the sunning of the motor
d - none of these

Back 216

it will float on top

Front 217

A battery operated power tool, such as cordless drill, converts
a - mechanical energy to thermal energy
b - thermal energy to mechanical energy
c - therman energy to chemical energy
d - chemical energy to mechanical energy

Back 217

chemical energy to mechanical energy

Front 218

1 kg = 2.205 lb; 1 lb = 16 oz. How many kilograms are prewsent in 125 ounces?

Back 218

125 oz/1 x 1 lb/16 oz x 1/kg/2.205 lb = 125/35.28 = 3.54 kg

Front 219

A rectangle block has dimensions 2.9 cm x 3.5 cm x 10.0 cm. The density of the block is 3.51 g/cm3. What is the mass of the block? (d=m/v)

Back 219

d = 3.5 g/cm3 =
m?/v+2.9 cm x 3.5 cm x 10.0 cm = 3.56265
m = 3.6 x 10e7 g

Front 220

Which of the following groups of the periodic table contains no metallic elements?
a - 4A
b - 5A
c - 6A
d - 7A

Back 220

7A

Front 221

An alkaline earth metal, a halogen, a transition metal and a noble gas are in the order:
a - Na, Cl, Fe, Ar
b - Ba, Br, Mn, Ar
c - Ba, N, Fe, He
d - Ba Br, Pb, Ne

Back 221

Ba, Br, Mn Ar

Front 222

Which three elements are likely to have similar cheical and physical properties?
a - nitrogen, oxygen, and neon
b - sodium, magnesium and aluminum
c - nickel, copper and zinc
d - oxygen, sulfur and selenium

Back 222

oxygen, sulfur, selenium

Front 223

How many electrons can be accommodated in the 3rd shell?
a - 8
b - 10
c - 18
d - 32

Back 223

18

Front 224

How many valence electrons are in the sulfur atom?
a 2
b 4
c 6
d 16

Back 224

6

Front 225

A student is preparing a sugar water solution to make rock candy. When the student continues to add sugar to the solution no additional sugar dissolves. Which kind of solution does the student have?

Back 225

saturated solution

Front 226

Which of the following solute will not dissolve in water?
a - KCl
b - MgCl2
c - HCl
d - CCl4

Back 226

CCl4

Front 227

A cucumber is placed in a concentrated salt solution. What will most likely happen?
a - wter will flow from the cucumber to the solution
b - water will flow from the solution to the cucumber
c - salt will flow into the cucumber
d - salt will precipitate out

Back 227

Water will flow from the cucumber

Front 228

Which of the following is the conjugate acid of NH3?
a. H+
b. H3O+
c NH2-
d. NH4+

Back 228

NH4+

Front 229

Which of the following solutions has the highest pH? a 0.1 M HCl
b 0.2 M HCl
c. pure H20
d 0.1 M NaOH
e. 0.2 M NaOH

Back 229

0.2 M NaOH

Front 230

What is the mass of salt in a 400 gram sample of salt water which is 2.50% (w/W)?

Back 230

400 g x 015/1 g = 6.00 g salt

Front 231

How many mL of pur alcohol are in 200 ml glass of wine that is 12% alcohol by volume. How much watrre is added?

Back 231

12% (v/v)
volume of solution = 200mL
12% = X mL solute (alcohol)/200 L wine X 100
x = 12/200/100 x 100
x = 24 mL alcohol
200 -24 = 176 mL H20

Front 232

a 50.0 g sample of a saline solution contains 1.75 g of NaCl. What is the % by weight concentration? (w/w)

Back 232

1.75 grams solute/50.0 grams solution x 100 = 3.50% w/w

Front 233

What is the mass of hydrogen peroxide in 250 grams of a 3.0% by weight solution? w/w

Back 233

grams of solute/grams of solution x 100
3.0% = x grams of hydrogen peroxide / 250 grms solution x 100
x = 3.0x250/100 = 750/100 = 7.5 grms hydrogen peroxide

Front 234

Calculate the molarity of a solution prepared by dissolving 5.844 g of NaCl in enough water to make a 200.0 mL solution.

Back 234

molarity = moles solute/volume of solution
5.844 g x 1 mol/58.44 (molar mass)g = 0.100 mol
0.1000 ol/.200 L - .500 mol/L or .50 M

Front 235

Calculate the moles of NaOH present in 500.0 mL of 0.25 M NaOH.

Back 235

.25 M NaOH = x moles solute/.50 L = 0.13 mol NaOH
0.25 mol x .5000 L = 0.13 mol

Front 236

Calculate the volume of 0.5 m HCl that would contain 2.0 mol HCl

Back 236

0.5 mol/L = 2.0 mol HCl/X = 2.0 ol/.5 mol/L = 4L
2.0 mol HCl/5 ol HCl vol (L) = 4.L