Chem Exam 1, 2, 3, 4 Occc

Front 1

Volume

Back 1

The amount of space a substance occupies. Metric: liter (L)

SI: cubic meter (m³)

Front 2

Length

Back 2

Metric: meter (m)

SI: meter (m)

Front 3

Mass

Back 3

The mass of an object is a measure of the quantity of material it contains.

Metric: gram (g)

SI: kilogram (kg)

Front 4

Temperature

Back 4

Metric: degree Celsius (°C)

SI: kelvin (K)

Front 5

Time

Back 5

Metric: second (s)

SI: second (s)

Front 6

1 L =

Back 6

1000 mL

Front 7

1 m =

Back 7

100 cm

Front 8

1 kg =

Back 8

1000 g

Front 9

Kilo

Back 9

Symbol: k

Number: 1000

Scientific notatiin: 10³

Front 10

Centi

Back 10

Symbol: c

Number: 0.01

Scientific notation: 10-²

Front 11

Milli

Back 11

Symbol: m

Number: 0.001

Scientific notation: 10-³

Front 12

1 m =

Back 12

1000 mm

Front 13

1 cm =

Back 13

10 mm

Front 14

1 g =

Back 14

1000 mg

Front 15

1 mg =

Back 15

1000 mcg

Front 16

C

Back 16

Carbon

Front 17

H

Back 17

Hydrogen

Front 18

Na

Back 18

Sodium

Front 19

Mg

Back 19

Magnesium

Front 20

K

Back 20

Potassium

Front 21

Ca

Back 21

Calcium

Front 22

Cr

Back 22

Chromium

Front 23

Mn

Back 23

Manganese

Front 24

Fe

Back 24

Iron

Front 25

Co

Back 25

Cobalt

Front 26

Cu

Back 26

Copper

Front 27

Zn

Back 27

Zinc

Front 28

N

Back 28

Nitrogen

Front 29

O

Back 29

Oxygen

Front 30

F

Back 30

Fluorine

Front 31

P

Back 31

Phosphorus

Front 32

S

Back 32

Sulfur

Front 33

Cl

Back 33

Chlorine

Front 34

Se

Back 34

Selenium

Front 35

I

Back 35

Iodine

Front 36

Mo

Back 36

Molybdenum

Front 37

Pure substance

Back 37

A pure substance is matter that has a fixed or definite composition

Front 38

Element

Back 38

Elements are composed of only one type of material

Front 39

A compound

Back 39

A compound consists of 2 or more elements always chemically combined in the same proportion

Front 40

Mixtures

Back 40

A mixture is 2 or more different substances physically mixed but not chemically combined

Front 41

1 cm³ or 1 cc =

Back 41

1 mL

Front 42

1 km =

Back 42

1000m

Front 43

1 inch =

Back 43

2 54 cm (exact)

Front 44

1 m =

Back 44

100 cm

Front 45

1 L =

Back 45

1000 mL

Front 46

1 kg =

Back 46

1000 g

Front 47

Metric to U.S. units are ?

Back 47

Measured

Front 48

Metric unites are ?

Back 48

Exact

Front 49

Complete dimensional analysis

Back 49

Conversion factors

Front 50

Chemical

Back 50

A substance that has the same composition and properties wherever it is found

Front 51

Chemistry

Back 51

The study of the composition, structure, properties, and reactions of matter

Front 52

Conclusion

Back 52

An explanation of an observation that has been validated by repeated experiments that support a hypothesis

Front 53

Experiment

Back 53

A procedure that test the validity of a hypothesis

Front 54

Hypothesis

Back 54

In and verified explanation of a natural phenomenon

Front 55

Hypothesis

Back 55

In and verified explanation of a natural phenomenon

Front 56

Observation

Back 56

Information determined by noting and recording a natural phenomenon

Front 57

Scientific method

Back 57

The process of making observations, proposing a hypothesis, and testing the hypothesis. After repeating experiments validate the hypothesis, it may become a theory

Front 58

Scientific notation

Back 58

A form of writing large and small numbers using a coefficient that is at least one but less than 10 followed by a power of 10

Front 59

Theory

Back 59

An explanation for an observation supported by additional experiments that confirmed the

Front 60

Density

Back 60

The relationship of the mass of an object to its volume expressed as grams per cubic centimeter , grams per milliliter, or grams per liter

Front 61

International system of units

Back 61

The official system of measurement throughout the world except for the United States that modifies the metric system

Front 62

Prefix

Back 62

All prefixes are related on a decimal scale

Front 63

Specific gravity

Back 63

A relationship between the density of a substance and the density of water.

Front 64

Compound

Back 64

Appear substance consisting of 2 or more elements with a definite composition that can be broken down into simpler substances only by chemical methods

Front 65

Element

Back 65

A pure substance containing only one type of matter which cannot be broken down by chemical methods

Front 66

Deposition

Back 66

The change of a gas directly into a solid

Front 67

Energy value

Back 67

The kilo calories obtained per gram of the food types carbohydrate, fat, and protein

Front 68

Heat of fusion

Back 68

The energy required to melt exactly one g of a substance at its melting point

Front 69

Heat of vaperation

Back 69

The energy required to vaporize exactly one g of a substance at its boiling point

Front 70

Joule

Back 70

The SI unit of heat energy

Front 71

Kinetic energy

Back 71

The energy of moving particles

Front 72

Specific heat

Back 72

A quantity of heat that changes the temperature of exactly one g of a substance by exactly 1ﾟC

Front 73

Sublimated

Back 73

The change of state in which a solid is transformed directly to a gas without forming a liquid 1st

Front 74

Chemical symbol

Back 74

In abbreviation that represents the name of an element

Front 75

Homogenous Mixture

Back 75

The composition is uniform throughout the different parts of the mixture are not visible

Front 76

Heterogeneous mixture

Back 76

The composition berries from one part of the mixture to another it is not uniform the different parts of the mixture are visible

Front 77

Classification Of matter

Back 77

Front 78

Addition and subtraction rule

Back 78

The final answer must have the same number of decimal places as the measurement with the fewest decimal places

Front 79

Multiplication and division rule

Back 79

The final answer must have the same number of significant figures as the measurement with the fewest significant

Front 80

A prefix

Back 80

Makes units larger or smaller than the base unit by factors of 10

Front 81

1 cc =

Back 81

1 cm³ = 1 mL

Front 82

Finding density

Back 82

Density = mass divided by volume. g/mL OR g/cm³

Front 83

1 mL =

Back 83

1 cm³

Front 84

Groups on the periodic table

Back 84

All vertical columns are groups of elements that have similar properties

Front 85

Periods on the periodic table

Back 85

Each horizontal row is a period

Front 86

Alkali metals

Back 86

Group 1A. Lithium(Li), sodium(Na), potassium(K), rubidium(Rb), cesium(Cs), and francium(Fr).

Front 87

Alkaline earth metals

Back 87

Group 2A. Beryllium(Be), magnesium(Mg), calcium(Ca), strontium(Sr), barium(Ba), and radium(Ra).

Front 88

Halogens

Back 88

Group 7A. Fluorine(F), chlorine(Cl bromine(Br), iodine(I), astatine(At), and tennessine(Ts).

Front 89

Noble gases

Back 89

Group 8A. Helium(He), neon(Ne), argon(Ar), krypton(Kr), xenon(Xe), radon(Rn) and oganesson(Og).

Front 90

Metals

Back 90

Shiny solids that can be shaped into wires or hammered into a flat sheet. Metals are good constructs of heat and electricity. They usually melt at higher temps than non-metals. Examples: copper(Cu), gold(Au), and silver (Ag).

Front 91

Nonmetals

Back 91

Not especially shiny, or malleable. Often poor conductors of heat and electricity. Low melting points and low densities. Examples: hydrogen(H), carbon(C), nitrate(N), oxygen(O), chlorine(Cl), and sulfur(S).

Front 92

Metalloids

Back 92

Elements that exhibit some properties of metal and some properties of nonmetals. Better at conducting heat and electricity than non metals, but not as good as metals. Nonmetals are semiconductors. Metalloids include: boron(B), silicon(S), arsenic(As), tellurium(Te), astatine(At), and tennessine(Ts).

Front 93

Major elements in the human body

Back 93

Hydrogen(H), carbon(C), nitrate(N), and oxygen(O).

Front 94

Macrominerals

Back 94

Sodium(Na), magnesium(Mg), potassium(K), calcium(Cl), phosphorus(P), sulfur(S), and chlorine(Cl).

Front 95

Microminerals

Back 95

Vanadium(V), chromium(Cr), manganese(Mn), iron(Fe), cobalt(Co), copper(Cu), zinc(Zn), molybdenum(Mo), silicon(Si), arsenic(As), selenium(Se), and iodine(I).

Front 96

An atom

Back 96

The smallest particle of an element that retains characteristics of the element.

Front 97

Dalton's atomic theory

Back 97

Atoms

•are tiny particles of matter.

•of the same element have the same properties.

•of different elements have different properties.

•of two or more different elements combine to form compounds.

•are rearanged in a chemical reaction to form new combinations in whole number ratios.

Front 98

3 major Subatomic particles

Back 98

Protons, neutrons, and electrons.

Front 99

An atom consists of

Back 99

•a nucleus: containing protons and neutrons.

•electrons in a "cloud" around the nucleus.

•and mostly, empty space.

Front 100

Atomic number

Back 100

Number of protons in an atom

Front 101

Mass number

Back 101

Number of protons + number of neutrons

Front 102

Isotopes

Back 102

Are atoms of the same same element that have the same atomic number but different numbers of neutrons.

Front 103

Example of an isotope of Magnesium

Back 103

Mass number--> | ²⁴ |

Mg <-- symbol

Atomic number-->|¹² |

Front 104

Atomic mass

Back 104

Included on the periodic table. It is the number with a decimal. Atomic mass is a average calculation.

Front 105

Electron energy levels

Back 105

Principal quantum numbers. Generally elections in the lower energy levels are closer to the nucleus. Values are quantized, which means the electron can only have a specific energy level and nothing in between.

Front 106

Changes in election energy levels

Back 106

An electron can move to higher energy levels only if it absorbs the energy equal to the difference in energy levels.

When an electron drops to a lower energy level it emits energy equal to the difference in levels.

Front 107

Electron arrangements.

Back 107

Level 1: holds up to 2.

Level 2: holds up to 8.

Level 3: holds up to 18.

Front 108

Valence electrons

Back 108

Are electrons in the outermost energy level.

Element groups 1A-8A have an equal number of valence electrons as the digit in their group number

Front 109

Lewis dot symbols

Back 109

Represents the number of valence electrons in an element

Front 110

Cation

Back 110

A positively charged ion of a metal.

Front 111

Anion

Back 111

A negatively charged ion.

Front 112

Octet

Back 112

Atoms lose, gain, or share valence electrons to acquire an octet of eight(8) valence electrons. To gain a stable electron arrangement is know as the octet rule.

Front 113

Gaining and losing valence electrons.

Back 113

Metals lose electrons to form positive ions. Nonmetals gain electrons to form negative ions.

Front 114

An ionic compound

Back 114

When one or more electrons are transferred from metals to nonmetals and form + or - ions. The attra ton is called an ionic bond.

Front 115

Chemical formula

Back 115

Represents the symbols and subscripts in the lowest whole number ratio of atoms to ions.

Front 116

Naming an ionic compound

Back 116

•metal ion first as whole name

•nonmetal ion second ending in "ide"

Subscripts are not used

Front 117

Variable charges

Back 117

Most transition elements have variable positive charges and are expressed using a Roman numerical to represent its subscript.

Front 118

Writing ionic formulas

Back 118

Starts with the name that describes the metal ion, including the charge, followed by the non-metal

Front 119

Polyatomic ions

Back 119

An ionic compound may contain a polyatomic ion as one of its cations or anions. A polyatomic ion is a group of covalently bonded atoms that have an overall ionic charge. Most examples are phosphorus(P), sulfur(S), carbon(C), and nitrogen(N) bonded to oxygen.

Front 120

Naming polyatomic ions

Back 120

Most end in "ate". When one less Oxygen(O) atom is used, "ite" is used to name it.

Front 121

Halogens and polyatomic ions.

Back 121

Halogens form 4 different polyatomic ions with oxygen(O). The prefix "per" is used for one more oxygen(O) than the "ate" ion, and the prefix "hypo" is used for one less oxygen(O) than the "ite" ion.

Front 122

Naming molecular compounds

Back 122

•nonmetal element name

•second nonmetal is named by forst syllable followed by "ide".

•if a subscript is know, a prefix is placed befor the name.

Front 123

Prefixes used to name molecular compounds

Back 123

1=Mono

2=Di

3=Tri

4=Tetra

5=penta

6=hexa

7=hepta

8=Octa

9=nona

10=deca

Front 124

Chloride ion

Back 124

Cl-

Front 125

Fluoride ion

Back 125

F-

Front 126

Oxide ion

Back 126

O²-

Front 127

Sulfide ion

Back 127

S²-

Front 128

Nitride ion

Back 128

N³-

Front 129

Phosphide ion

Back 129

P³-

Front 130

Ammonium formula

Back 130

NH4+

Front 131

Hydroxide

Back 131

OH-

Front 132

Mono

Back 132

1

Front 133

Di

Back 133

2

Front 134

Tri

Back 134

3

Front 135

Tetra

Back 135

4

Front 136

Penta

Back 136

5

Front 137

Hexa

Back 137

6

Front 138

Hepta

Back 138

7

Front 139

Octa

Back 139

8

Front 140

Nona

Back 140

9

Front 141

Deca

Back 141

10

Front 142

Describe the biological functions and dietary sources of the following trace elements.

Back 142

Fe (Iron): carrier of oxygen hemoglobin.

Cu (Copper): needed for blood vessels, blood pressure, and immune system.

Zn (Zinc): needed for metabolic reactions in cells, DNA synthesis, growth of bones, teeth, connective tissue and immune system.

Mn (Manganese): needed for growth of bones, blood clotting and metabolic reactions.

I (Iodine): needed for proper thyroid funtions.

Front 143

States of matter

Back 143

Solid, liquid, and gas.

Front 144

Solid

Back 144

Has a definite shape and volume

Front 145

Liquid

Back 145

Has a definite volume but not a definite shape

Front 146

Gas

Back 146

Does not have a definite shape or volume

Front 147

Physical properties

Back 147

Are the characteristics that can be observed or measured without affecting the identity of a substance

Front 148

Physical change

Back 148

The state, size, or appearance will change, but its composition remains the same.

Front 149

Chemical properties

Back 149

Chemical properties are those that describe the ability of a substance to change into new substances

Front 150

Chemical change

Back 150

When a chemical change takes place, the original substance is converted into one or more new substances, which have new physical or chemical properties.

Front 151

Melting

Back 151

Changing from a solid to a liquid. When he is added to a solid, the particles move faster. Requires heat, endothermic.

Front 152

Freezing

Back 152

A liquid changes to a solid. The particles slow down, and attractive forces pulled a particles close together. Loses heat, exothermic.

Front 153

Heat of fusion

Back 153

During melting, the heat of fusion is the energy that must be added to convert exactly one g of solid to liquid at the melting point.

Front 154

Sublimation

Back 154

When a solid turns into a gas without becoming a liquid first. Requires heat, endothermic.

Front 155

Deposition

Back 155

When a gas becomes a solid. Takes heat away, exothermic.

Front 156

Evaporation

Back 156

When a liquid becomes a gas. Requires heat, endothermic.

Front 157

Condensation

Back 157

Water vapor converting back to a liquid. Takes heat away, exothermic.

Front 158

Heat of vaporation

Back 158

The energy that must be added to convert exactly one g of a liquid to a gas

Front 159

Radiation

Back 159

An unstable nucleus is radioactive, which means that it spontaneously amidst small particles of energy called radiation to become more stable.

Front 160

Types of radiation

Back 160

1-Alpha particles

2-Beta particles

3-Positron

4-Gamma rays

Front 161

Alpha particles

Back 161

Identical to a helium nucleus which has 2 protons and 2 neutrons. An alpha particle has a mass number of 4, an atomic number of 2, and a charge of 2+. a ( ⁴He )

²

Front 162

Beta particle

Back 162

A high energy Elektron, has a charge of 1-, and because its mass is so much less than the mass of a proton, it has a mass number of zero. ß ( ⁰e )

-¹

Front 163

A positron

Back 163

Similar to a Beta particle, has a 1+ charge with a mass number of 0. ß+ ( ⁰ e )

+¹

Front 164

Gamma rays

Back 164

Gamma rays are high energy radiation, released when unstable nucleus undergoes a rearrangement of its particles. Often emitted along with other types of radiation.

Gamma rays have no mass or charge.

( ⁰ y ) or y

⁰

Front 165

Radioactive decay

Back 165

The nucleus spontaneously breaks down by a mitting radiation

Front 166

Alpha decay

Back 166

When an unstable nucleus emits an alpha particle the mass of the radioactive nucleus decreases.

Front 167

Beta decay

Back 167

In the nuclear equation for Beta decay, the mass number of the new nucleus remains the same and its atomic number increases by one.

Front 168

Positron emission

Back 168

And the nuclear equation for positron emission, the mass number of the radioactive nucleus and the mass number of the new nucleus are the same. However, the atomic number of the new nucleus decreases by one, indicating a change of 1 element into another.

Front 169

Gamma emission

Back 169

Pure gamma emitters are rare, although gamma radiation accompanies most Alpha and Beta radiation.

Front 170

Back 170

Remember

Front 171

Measuring radiation

Back 171

The activity is measured in terms of the number of nuclear disintegrations per second.

Front 172

Curie (Ci)

Back 172

Original unit of activity, defined as the number of disintegrations that occur in 1 second for one g of radium. 3.7 X 10¹⁰

Front 173

Becquerel

Back 173

1 disintegration/ s

Front 174

RAD

Back 174

Radiation Absorbed Dose.

The SI unit for absorbed dose is the Gray (Gy) which is defined as the joules of energy absorbed by one kg of body tissue. 1 Gray = 100 RAD

Front 175

REM

Back 175

Radiation Equivalent in Man.

The unit that measures the biological effects of different kinds of radiation.

Front 176

Equivalent dose or rem dose

Back 176

Biological damage=absorbed dose X factor

Front 177

Avogadro's number

Back 177

6.02 X 10²³/ 1 mole

Front 178

Molar mass

Back 178

Quantity in mass that equals the atomic mass of the element

Front 179

A chemical reaction always involves ?

Back 179

Chemical change

Front 180

Evidence of a chemical

Back 180

1- Change in color

2-Formation of gas or bubbles

3-Formation of a solid

4-Heat produced or absorbed

Front 181

Writing a chemical equation

Back 181

•Reactant on the left

•Arrow in the middle

•Products on the right

Front 182

Types of chemical reactions

Back 182

•Combination

•Decomposition

•Single replacement

•Double replacement

•Combustion

Front 183

Combination reaction

Back 183

2 or more elements or compounds bind to form one product.

Front 184

Decomposition reaction

Back 184

A reactant splits into 2 or more simpler products.

Front 185

Replacement reactions

Back 185

Single replacement - A reactive elements switches places with an element on the other reacting compound.

Double replacement reaction - The positive ions in the reacting compounds switch places.

Front 186

Oxidation reduction reaction

Back 186

When electrons are transferred from one substance to another. If 1 substance loses electron's, another substance must again Elektron

Front 187

Oxidation

Back 187

Oxidation is loss of electrons

Front 188

Reduction

Back 188

Reduction is gain of electrons

Front 189

1 kcal =

Back 189

1000 cal

Front 190

1 kJ =

Back 190

1000 J

Front 191

3 biological effects of radiation

Back 191

Birth defects, anemia, cancer

Front 192

Radiation protection

Back 192

Limiting amount of time spent near radioactive sources. Increasing distance from the source.

Front 193

Medic molecular theory of gasses

Back 193

1) A gas consists of small particles that move randomly with high velocities.

2) The attraction between the particles of a gas are very small.

3) The volume occupied by gas molecules is extremely small compared to the volume that the gas occupies.

4) Gas particles are in constant motion moving rapidly in straight paths.

5) The average kinetic energy of gas is proportional to the Kelvin temperature.

Front 194

Pressure

Back 194

Gas particles moving and straight lines within a container exert pressure when they collide with the walls of the container

Front 195

Volume of gas

Back 195

The volume of gas equals the size of the container in which it is placed

Front 196

Temperature of gas

Back 196

The temperature of a gas is related to the kinetic energy of its particles

Front 197

Amount of gas

Back 197

Gas is measured by its mass in grams. Grams must be changed to moles

Front 198

Measuring gas pressure

Back 198

Pressure equals force divided by area

Front 199

Boyle's law. Pressure and volume

Back 199

A gas law stating that the pressure of the gas is inversely related to the volume when temperature and moles of the gas do not change.

P1V1=P2V2

Front 200

Charles's law. Temperature in volume

Back 200

A gas law stating that the volume of a gas is directly related to the Kelvin temperature when pressure and moles of the gas do not change.

V1/T1 = V2/T2

Front 201

Gay-Lussac's law. Temperature and pressure.

Back 201

A gas law stating that the pressure of a gas is directly related to the Kelvin temperature when the number of moles of a gas and its volume do not change.

P1/T1 = P2/T2

Front 202

Avogadros law. Volume and moles

Back 202

A gas law stating that the volume of a gas is directly related to the number of moles of gas when pressure and temperature do not change.

V1/n1 = V2/n2

Front 203

Standard pressure and molar volume

Back 203

Standard temperature is exactly 0ﾟC this period standard pressure is exactly one atmosphere (atm).

Front 204

Dalton's law. Partial pressures.

Back 204

A gas law stating that the total pressure exerted by a mixture of gasses in a container is the some of the partial pressures that each gas would exert alone.

Ptotal = P1+P2+P3 ••••

Front 205

Atmosphere (atm)

Back 205

A unit equal to the pressure exerted by a column of Mercury 760 MM high.

Front 206

Atmospheric pressure

Back 206

The pressure exerted by the atmosphere

Front 207

Combined gas law

Back 207

A relationship that combines several gas laws relating pressure, volume, and temperature when the amount of gas does not change.

Front 208

Direct relationship

Back 208

A relationship in which 2 properties increase or decrease together

Front 209

Inverse relationship

Back 209

A relationship in which 2 properties change in opposite directions

Front 210

Kinetic molecular theory of gasses

Back 210

A model used to explain to behavior of gasses

Front 211

Partial pressure

Back 211

The pressure exerted by a single gas in a gas mixture

Front 212

Pressure

Back 212

The force exerted by gas particle that hits the walls of a container