Test 1

Front 1

How many significant figures are in the number 6.022 x 10^23?

Back 1

4

Front 2

In the product 1.04 x 0.31, the number of significant figures is

Back 2

2

Front 3

How many significant figures are in the number 60.02 x 10^5?

Back 3

4

Front 4

How many significant figures are in the number 0.020300?

Back 4

5

Front 5

Using the rules of significant figures, calculate the following: 12.67 + 13.005 =

Back 5

25.68

Front 6

If 1.000 kg equals 2.205 lb, what is the mass in pounds of a human who weighs 75.00 kg?

Back 6

165.4 lbs

Front 7

Convert 17.6 cm to inches (2.54 cm = 1 in)

Back 7

6.93

Front 8

Convert 692 m to decimeters.

Back 8

6920 dm

Front 9

The number of milligrams in 100 g is:

Back 9

1 x 10^5 mg

Front 10

Convert 258 L to milliliters.

Back 10

2.58 x 10^5 mL

Front 11

Correctly rounded, the result of (23.1000 g - 22.0000 g) /(25.10 mL - 25.00 mL) is

Back 11

11.0 g/mL

Front 12

The number 2.00152 rounded to four significant figures is:

Back 12

2.002

Front 13

In the product 1.04 x 0.31, the number of significant figures is:

Back 13

2

Front 14

When the calculation (32.8070 × 1.0200) x 0.000201 is carried out, the number of significant figures in the answer is:

Back 14

3

Front 15

What is the result of this calculation expressed to the correct number of significant digits? (42.785 - 41.808) / 25.56

Back 15

0.0382

Front 16

When the calculation (4.60 × 9.315) - 1.0 × 10^2 is carried out, the number of significant figures in the answer is:

Back 16

3

Front 17

What is the result of this calculation expressed to the correct number of significant digits? 72.1 + 1.684 = ?

Back 17

73.8

Front 18

Convert 6.0 kg to pounds (1 kg = 2.205 lb).

Back 18

13 lb

Front 19

How many milliliters are in 0.0020 L?

Back 19

2.0 mL

Front 20

The fundamental unit of mass in the metric system is the:

Back 20

Gram

Front 21

The answer that should be reported for the total number of milliliters of solution when 19.10 mL of ethanol is added to 1.52 L of methanol is:

Back 21

1.54 x 10^3 mL.

Front 22

Convert 9.83 kg to pounds (1 lb = 453.6 g).

Back 22

21.7 lb

Front 23

The measurements of three different masses on three different balances are 1.21 kg, 536 mg, and 23.14 g. The total mass should be reported as:

Back 23

1.23 x 10^3 g.

Front 24

A cubic centimeter (cm3) is equivalent to what other metric volume unit?

Back 24

mL

Front 25

The measurement 4.3 x 10^3 g also could be written as ______ kg:

Back 25

4.3 kg

Front 26

The density of copper metal is 8.9 g/mL. What is the mass of 1.00 L of this metal?

Back 26

8.9 x 10^3 g

Front 27

If a 100.-g sample of platinum metal has a volume of 4.67 mL, what is the density of platinum in g/cm3?

Back 27

21.4 g/cm3

Front 28

The density of copper metal is 8.9 g/mL. What is the volume of 55.0 mg of this metal?

Back 28

0.0062 cm3

Front 29

The density of an object that has a mass of 2.50 g and occupies a volume of 1.20 cm3 equals:

Back 29

2.08 g/cm3

Front 30

The density of lead metal is 11.3 g/cm3. What is the volume of 15.0 g of this metal?

Back 30

1.33 cm3

Front 31

What is the mass of a substance that has a volume of 16.0 mL. The density of this substance is 8.50 g/mL.

Back 31

136.0 g

Front 32

The density of alcohol is 0.780 g/mL. What is the mass of 20.0 mL of the alcohol?

Back 32

15.6 g

Front 33

What is the volume occupied by 56.0 g of a substance, which has a density of 0.940 g/mL?

Back 33

59.6 mL

Front 34

If 1 mi = 1.61 km, what is a speed of 1.0 km/min in mi/hr?

Back 34

37 mi/hr

Front 35

The recommended daily allowance (RDA) of calcium is 1200 mg. Calcium carbonate contains 12 % calcium by mass. How many grams of calcium carbonate are needed to provide the RDA of calcium?

Back 35

10.0 g

Front 36

If a person can comfortably carry 20 kg (44 lbs) and gold has a density of 19.6 g/cm3, what is the volume of the largest piece of solid gold a person can carry?

Back 36

1020 cm3

Front 37

A car averages 35 miles per gallon of gasoline. How many liters of gasoline will be needed for a trip of 450 km? Some conversion factors which may be helpful are the following:

Back 37

3.0 x 10^1 L

Front 38

A sample of milk is found to have arsenic at a concentration of 1.31 μg/L (microgram/liter). What is the concentration in ounces per gallon?

Back 38

1.7 x 10^7 oz/gal

Front 39

Two types of pure substances are:

Back 39

Compounds and elements.

Front 40

Ice floating in soda water is classified as:

Back 40

A heterogenous mixture.

Front 41

Which property of a sample of a substance would not be characteristic of the substance and hence would not be useful in identifying the substance?

Back 41

Mass of the sample.

Front 42

Gasoline is classified as:

Back 42

A homogenous mixture.

Front 43

In a chemical change, the products:

Back 43

are different substances from the starting materials.

Front 44

Water is an example of:

Back 44

A compound.

Front 45

If a solution of silver perchlorate is added to a solution of sodium iodide, solid silver iodide forms. The silver iodide is called a:

Back 45

precipitate.

Front 46

Muddy water is placed on a porous surface and clear water allowed to seep through. This process is called:

Back 46

Filtration

Front 47

A pure substance made up of more than one kind of atom is called:

Back 47

An element

Front 48

The fact that gold does not rust is a: PHYSICAL or CHEMICAL property?

Back 48

Chemical property

Front 49

275°F is equivalent to _________ C?

Back 49

135°C

Front 50

The temperature of a liquid is 247 K. The temperature in ºC would be:

Back 50

-26

Front 51

423 K equals ______ ºC?

Back 51

150.°C

Front 52

507.1 K is equal to ______ ºF.

Back 52

453.4

Front 53

22.4 ºC is equal to ______ ºF.

Back 53

72.3

Front 54

-105 oC is equal to ______ K.

Back 54

168

Front 55

-53.6 oC is equal to ______ oF.

Back 55

-64.5

Front 56

What is the change in temperature of 25.0 g of silver (specific heat = 0.240 J/g ºC) if 85.0 J of heat is added to the silver sample?

Back 56

14.2 C

Front 57

How much heat energy is needed to warm 50.0 g of carbon (specific heat = 0.71 J/g ºC) from 25 ºC to 75 ºC ?

Front 58

Heat is typically measured in:

Back 58

Joules

Front 59

How many kilojoules are there in 15.4 kilocalories?

Back 59

64.4 kJ

Front 60

What is the mass of a copper sample (specific heat = 0.384 J/gºC) if addition of 30.0 J of heat causes the temperature to change from 15.2ºC to 35.0ºC

Back 60

3.95 g

Front 61

Which of the following is a valid unit for specific heat (or specific heat capacity)?

Back 61

cal/g °C

Front 62

If 85.1 cal of heat are added to 10.0 g of water (specific heat = 4.184 J/g oC) at 30.0 oC, what is the final temperature of the water sample?

Back 62

38.5 ºC

Front 63

A 6.75-g sample of gold (specific heat capacity = 0.130 J/g °C) is heated using 50.6 J of energy. If the original temperature of the gold is 25.0°C, what is its final temperature?

Back 63

82.7 C

Front 64

How many kilojoules are there in 3.37 X 10^4 calories?

Back 64

141 kJ

Front 65

How many calories are there in 57.0 joules of energy?

Back 65

13.6 cal

Front 66

The quantity of heat required to change the temperature of 1 g of a substance by 1°C is defined as:

Back 66

Specific heat capacity

Front 67

A 13.1 g sample of a liquid changes from 35.0 ºC to 25.0ºC upon removal of 85.0 J of heat. What is the specific heat of this liquid in J/gºC?

Back 67

0.649

Front 68

An atom that has the same number of neutrons as 59Co has ____ neutrons.

Back 68

59

Front 69

The mass number of any atom is equal to its:

Back 69

number of protons plus neutrons

Front 70

The first scientist to show that atoms emit tiny negative particles was:

Back 70

JJ Thompson

Front 71

Which atomic particle determines the chemical behavior of an atom?

Back 71

Electron

Front 72

How many atoms of hydrogen are in one molecule of Ca(OH)2?

Back 72

2

Front 73

The atom with 68 neutrons and 50 protons has a mass number of:

Back 73

118

Front 74

Common table salt is sodium chloride. When table salt is dissolved in water, the solution conducts electricity because:

Back 74

There are ions in the solution

Front 75

What is the name of the element in Group IIA and period 3 in the periodic table?

Back 75

Magnesium

Front 76

An atom with 45 protons has a mass number of 100. It must contain how many neutrons?

Back 76

55

Front 77

In the atomic symbol 31P 3-, how many electrons are represented?

Back 77

18

Front 78

How many protons, electrons, and neutrons, respectively, does O have?

Back 78

8, 8, 8

Front 79

An atom with 15 protons and 16 neutrons is an atom of:

Back 79

P - Phosphorus

Front 80

Which subatomic particles must always be of equal numbers in any atom?

Back 80

Electrons and protons

Front 81

Atoms of the same element that have different masses are called:

Back 81

Isotopes

Front 82

How many phosphorus atoms are represented by one formula unit of calcium phosphate, Ca3(PO4)2?

Back 82

2

Front 83

How many electrons are present in a bromine atom with a mass number of 87?

Back 83

35

Front 84

What is the name of the Group IA metals?

Back 84

Alkali metals

Front 85

An element's most stable ion forms an ionic compound with chlorine having the formula XCl2. If the ion of element X has a mass of 89 and 36 electrons, what is the identity of the element, and how many neutrons does it have?

Back 85

Sr, 51 neutrons

Front 86

What is the symbol of the ion having 12 protons and 10 electrons?

Back 86

Mg2+

Front 87

Which parts of the atom have approximately the same mass?

Back 87

Proton and nutron.

Front 88

Which particle has the least mass? Proton or electron.

Back 88

Electron (mass is negligible)

Front 89

35.0 pounds of U.S. nickels contain 8.8 pounds of copper. What is the percentage copper in these coins?

Back 89

25%

Front 90

At PCC the student body is 56.3% female. If there are 39 students, on average, in each class at PCC, approximate how many women are there in each class?

Back 90

22

Front 91

An alloy is made by mixing 40.0 grams of tin, 35.6 grams of lead, and 50.0 grams of copper. What is the percentage of lead in this alloy?

Back 91

28.3

Front 92

If Sterling silver is 90.0% silver and 10.0% copper, what is the maximum amount of Sterling silver that can be made if you have 49.7 grams of silver metal and an unlimited amount of copper?

Back 92

55.2

Front 93

It is well known that the element magnesium has three naturally occurring isotopes. Mg-24 represents 79.0% of all magnesium atoms, Mg-25 accounts for 10.0%, and Mg-26 is the remaining 11.0%. If you have 226. atoms of magnesium, how many should be Mg-24?

Back 93

179

Front 94

It is generally recognized that a "balanced" diet should contain 30.0% fat. If the average individual requires 2388 Calories of energy from the foods ingested each day, how many Calories should come from fat?

Back 94

716

Front 95

You wish to buy enough honey to fill a 5.35 quart honey jar. At the grocery story you find that honey costs $3.00 per kilogram and it has a density of 1.50 grams per milliliter. How much will it cost in $ to buy enough honey to fill your 5.35 quart jar? (1 qt = 946 mL)

Back 95

22.8

Front 96

An iron ore was found to contain 92.0% pyrite (fool's gold). Pyrite has the formula FeS2and is 46.5% iron. How many grams of iron are there in 65.8 grams of iron ore?

Back 96

28.1

Front 97

Methane molecules (the overwhelming majority of the molecules in natural gas) are composed of 25.1% hydrogen and 74.9% carbon, by mass. If there is a reaction between 115.1 g of carbon with 28.3 grams of hydrogen, how many grams of methane could be produced?(Give only the numerical value for answer in the box)

Back 97

113.0

Front 98

How many electrons are in the third principal energy level (n = 3) of one atom of Fe?

Back 98

14

Front 99

As the principal energy level increases in an atom's orbitals, the average distance of an electron energy level from the nucleus ______________.

Back 99

Increases

Front 100

What element has the electron configuration 1s22s22p63p64s23d104p5?

Back 100

Br

Front 101

Which of the following is a reasonable criticism of the Bohr model of the atom?

Back 101

It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen.

Front 102

The shape of an s orbital is:

Back 102

Spherical

Front 103

An element which has the similar valence electron configuration as tellurium (Te) is:

Back 103

S

Front 104

Which subshell can hold the greatest number of electrons?

Back 104

4f

Front 105

The maximum number of electrons that can occupy the 5f orbitals is:

Back 105

14

Front 106

The number of unpaired electrons in an oxygen atom is:

Back 106

2

Front 107

The principal quantum number of the valence electrons in an atom of tin (Sn) is:

Back 107

4

Front 108

How many d electrons are there in a vanadium atom?

Back 108

3

Front 109

The maximum number of electrons allowed in the fourth energy level is:

Back 109

32

Front 110

The number of p orbitals in the fourth principal energy level is:

Back 110

3

Front 111

The Group 3 (III A) elements through the Group 8 (VIII A) elements form an area of the periodic table where the electron sublevels being filled are:

Back 111

P Orbitals

Front 112

Which of the following properties generally increases as we go from the left to the right of the periodic table?

Back 112

Ionization energy

Front 113

What main group element forms a positive ion having the ground-state electron configuration [Ar]?

Back 113

Calcium

Front 114

Order the elements S, Cl, and F in terms of increasing atomic radii.

Back 114

F, Cl, S

Front 115

What is ionization energy?

Back 115

The energy required to remove an electron from an atom.

Front 116

Which of the following pairs are isoelectronic (same number of electrons)?

Back 116

K+ and Ca2+

Front 117

What is the formula used to calculate specific heat?

Back 117

q = (m) ⋅ (c) ⋅ (Δt)

(q) heat added = (m) mass ⋅ (c) specific heat capacity ⋅ (Δt) change in temp.

Front 118

What is the formula to calculate density?

Back 118

d = m / v

Front 119

What is the formula for calculating mass?

Back 119

m = d ⋅ v

Front 120

What is the formula for calculating volume?

Back 120

v = m / d

Front 121

Atoms get excited and give off _____________ in the form of light as they return back to their ground state.

Back 121

Photon energy

Front 122

If an elemental atom loses 2 electrons, will it have a positive or negative charge?

Back 122

Positive

Front 123

If an elemental atom gains 2 electrons, will it have a positive or negative charge?

Back 123

Negative

Front 124

A _______ consists of atoms of 2 or more different elements bound together my chemical means.

Back 124

Compound

Front 125

A _________ consists of two or more elements or compounds that are physically intermingled. Often retains many properties of its components.

Back 125

Heterogenous mixture

Front 126

A _______ often retains many properties of its components.

Back 126

Mixture

Front 127

A _______ often takes on properties different than its component elements.

Back 127

Compound

Front 128

A ________ is a mixture of two or more substances (solute and solvent).

Back 128

Solution

Front 129

A compound can me physically separated: True or False?

Back 129

False

Front 130

Name 5 examples of heterogenous mixtures:

Back 130

1.) sandy water

2.) cereal in milk

3.) ice in soda water

4.) oil and water

5.) chicken noodle soup

Front 131

Name 5 examples of homogenous mixtures:

Back 131

1.) gasoline

2.) air

3.) blood

4.) brass

5.) cough medicine

Front 132

Name 5 physical properties:

Back 132

1.) physical state (s,l,g)

2.) color

3.) smell

4.) solubility

5.) melting / boiling points

6.) conductivity

7.) hardness

Front 133

Name 5 chemical properties:

Back 133

1.) corroding

2.) reacting

3.) tarnishing

4.) decomposing

5.) fermentation

Front 134

℃ to ℉ conversion equation

Back 134

℉ = 1.8 (℃) + 32

Front 135

℉ to ℃ conversion equation

Back 135

℃ = (℉ - 32) / 1.8

Front 136

℃ to K conversion equation

Back 136

K = ℃ + 273.15

Front 137

K to ℃ conversion equation

Back 137

℃ = K - 273.15

Front 138

1 calorie = __________ joules

Back 138

4.184

Front 139

What is the specific heat measurement of water?

Back 139

4.184

Front 140

How many electrons are present in a Fe 3+ atom?

Back 140

23 e-

Front 141

How many "f" orbitals are present in the third energy level?

Back 141

None

Front 142

What is the maximum amount of electrons in an "s" orbital?

Back 142

2

Front 143

What is the maximum amount of electrons in a "p" orbital?

Back 143

6

Front 144

What is the maximum amount of electrons in a "d" orbital?

Back 144

10

Front 145

What is the maximum amount of electrons in a "f" orbital?

Back 145

14

Front 146

A sample of pure iron requires 142 cal of energy to raise itstemperature from 23ºC to 92ºC. What is the mass of the sample?(The specific heat capacity of iron is 0.45 J/gºC.)

Back 146

19?

Front 147

7 Diatomic Elements:

Back 147

Hydrogen H2

Nitrogen N2

Oxygen O2

Fluorine F2

Chlorine Cl2

Bromine Br2

Iodine I2

Front 148

Define wavelength:

Back 148

the distance between two peaks in a wave

Front 149

Define frequency (v):

Back 149

the number of waves (cycles) per second that pass a given point

Front 150

Define speed (c):

Back 150

the speed of light (2.9979×108 m/s)

Front 151

In a chemical reaction, matter is:

Back 151

Neither created or destroyed.

Front 152

Energy is:

Back 152

the capacity to do work

Front 153

Work is defined as:

Back 153

the result of force acting on a distance

Front 154

The behavior of matter is driven by:

Back 154

Energy

Front 155

The energy needed to raise the temperature of 1 gram of water through 1 °C (now usually defined as 4.1868 joules).

Back 155

1 calorie

Front 156

1 calorie equals ________ joules.

Back 156

4.184

Front 157

1 Cal = ______ cal

Back 157

1000

Front 158

1 kcal = _______ cal

Back 158

1000

Front 159

1 Calorie equals ________ joules.

Back 159

4184

Front 160

60.1 cal to joules

Back 160

251j

Front 161

105.8 F = ________ C

Back 161

41 C

Front 162

37 C = _________ K

Back 162

310.15 K

Front 163

JJ Thompson

Back 163

Credited with the discovery and identification of the electron; and with the discovery of the first subatomic particle. He proposed that atoms must contain positive charge that balanced the negative charge of electrons.

Front 164

Dalton's Atomic Theory

Back 164

1) All matter is made of atoms. Atoms are indivisible and indestructible.

2) All atoms of a given element are identical in mass and properties

3) Compounds are formed by a combination of two or more different kinds of atoms.

4) A chemical reaction is a rearrangement of atoms.

Front 165

Bohr Atomic Model

Back 165

Depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus—similar in structure to the solar system, but with attraction provided by electrostatic forces rather than gravity.

Front 166

Rutherford Atomic Model

Back 166

Correctly explained nuclear atom: nucleus, protons (+) and electrons (-).

Front 167

Name group 1A:

Back 167

Alkali Metals

Front 168

Name group 2A:

Back 168

Alkaline Earth Metals

Front 169

List the 7 metalloids:

Back 169

B

Si

Ge

As

Sb

Te

At

Front 170

Name group 7A:

Back 170

Halogens

Front 171

Name group 8A:

Back 171

Noble gasses

Front 172

Most reactive group (1A-8A):

Back 172

1A

Front 173

Least reactive group (1A-8A):

Back 173

8A

Front 174

Positive ions are called:

Back 174

Cations

Front 175

Negative Ions are called:

Back 175

Anions

Front 176

If an atom loses a(n) electron(s), its charge becomes:

Back 176

Positive

Front 177

If an atom gains a(n) electron(s), its charge becomes:

Back 177

Negative

Front 178

An ______ chemical element is an atom that has a different number of neutrons (that is, a greater or lesser atomic mass) than the standard for that element.

Back 178

Isotope

Front 179

Calculate the atomic mass of Ga:

Ga-69 (60.11% mass 68.9256 amu)

Ga- 71 (39.89% mass 70.9247 amu)

Back 179

69.72 amu

Front 180

A _________ is a statement based on repeated experimental observations that describes some aspects of the universe.

Back 180

Scientific law

Front 181

A _______ always applies under the same conditions, and implies that there is a causal relationship involving its elements.

Back 181

Scientific law

Front 182

A __________ is a well-substantiated explanation of some aspect of the natural world, based on a body of facts that have been repeatedly confirmed through observation and experiment. Such

Back 182

Scientific theory

Front 183

Fact-supported ________ are not "guesses" but reliable accounts of the real world.

Back 183

Scientific theories

Front 184

________ is the active acquisition of information from a primary source.

Back 184

Observation

Front 185

In living beings, _________ employs the senses.

Back 185

Observation

Front 186

In science, ________ involves the recording of data via the use of instruments. The term may also refer to any data collected during the scientific activity.

Back 186

Scientific observation

Front 187

The _________ is the energy carried by a single photon with a certain electromagnetic wavelength and frequency.

Back 187

Photon energy

Front 188

The higher the photon's ________, the higher its energy.

Back 188

Frequency

Front 189

How many significant figures are counted when multiplying or dividing?

Back 189

The least amount of figures used in the initial equation.

Front 190

How many decimals are counted when adding or subtracting?

Back 190

The least amount of decimals used in the initial equation.

Front 191

Convert a 10 cm x 12 cm x 15 cm box to cubic inches.

Back 191

109.8 in3

Front 192

How many cubic inches is in 3.25 yard 3?

Front 193

If 75.0 g of copper is added to 50.0 mL of water in a graduated cylinder and the water lever rose to 58.4 mL, what is the density of the copper

Back 193

8.4 cm3

Front 194

What is the mass in grams of a cube of gold (density= 19.32 g/cm3) if the length of the cube is 2 feet.

Front 195

A ________ has definite volume and maintains its shape.

Back 195

Solid

Front 196

Particles vibrate and oscillate but to not change position.

Back 196

Solid state

Front 197

A _______ has definite volume but no definite shape.

Back 197

Liquid

Front 198

A ______ assumes the shape of its container

Back 198

Liquid

Front 199

A _______ has no fixed volume or shape.

Back 199

Gas

Front 200

A _______ takes the shape and volume of its container and are compressible.

Back 200

Gas

Front 201

Two types of pure substances:

Back 201

Elements and compounds

Front 202

A _________ is formed when two or more atoms join together chemically.

Back 202

molecule

Front 203

Define molecule:

Back 203

A molecule is formed when two or more atoms join together chemically.

Front 204

Define pure substance:

Back 204

Composed of only 1 type of atom or molecule.

Front 205

A ___________ is a molecule that contains at least two different elements.

Back 205

Compound

Front 206

All __________ are molecules but not all molecules are _________.

Back 206

Compounds

Front 207

All compounds are __________ but not all _________ are compounds.

Back 207

Molucules

Front 208

A ______ is a substance composed of a given combination of elements, that can be broken down into individual elements by chemical methods.

Back 208

Compound

Front 209

Define compound:

Back 209

A substance composed of a given combination of elements, that can be broken down into individual elements by chemical methods.

Front 210

The H atom has a volume in approximately 6.2 x 10 -31 m3. What is its volume in nm3?

Front 211

Cu-63 (69.17% at 62.93 amu)

Cu-65 (30.83% at 64.93 amu)

Back 211

62.55 amu

Front 212

The greater the energy, the larger the _________.

Back 212

Frequency

Front 213

The higher the frequency, the shorter the __________.

Back 213

Wavelength

Front 214

The higher the energy, the shorter the ___________.

Back 214

Wavelength