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CHEM 130 > Chapter 1-3 Test > Flashcards

Chapter 1-3 Test Flashcards

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1
Q

What is matter?

A

Anything that occupies space and has mass (forms of energy aren’t matter)

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2
Q

What is a pure substance?

A

Uniform chemical composition

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3
Q

What is a mixture?

A

Composed of two or more pure substances and may or may not have uniform composition

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4
Q

Two different types of pure substances

A

Element and compound

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5
Q

What is an element?

A

Cannot be broken down

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6
Q

Different kinds of elements

A

Metals, metalloids, nonmetals

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7
Q

What is a compound?

A

Composed of 2 or more elements combine in definite proportions

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8
Q

Metal

A

Lustrous, malleable, ductile, conductor of heat and electricity, usually solid at room temperature

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9
Q

Nonmetal

A

Dull, brittle, insulator of heat and electricity, may be solid, liquid, gas, at room temperature

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10
Q

Metalloid

A

Has properties of both metal and nonmetal

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11
Q

Atom

A

Smallest unit of an element that retains the chemical properties of that element

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12
Q

Molecule

A

Smallest unit of a compound that retains the chemical properties of that compound

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13
Q

Different types of mixtures

A

Homogenous and heterogeneous

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14
Q

Homogeneous

A

Same composition throughout, dissolved, mixed properly

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15
Q

Heterogeneous

A

Don’t have uniform composition (ie potting soil)

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16
Q

Property

A

A characteristic that we can observe

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17
Q

Change

A

Process that changes the properties of a substance

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18
Q

Physical property

A

A characteristic we can observe

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19
Q

Qualitative physical property

A

Color, odor

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20
Q

Quantitative physical property

A

Mass, density

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21
Q

Physical change

A

A process in which no new substances are produced

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22
Q

Chemical property

A

A characteristic that can only be observed when a substance is converted

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23
Q

Density

A

D = m/v

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24
Q

Energy

A

Capacity to do work or transfer heat

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25
Q

Kinetic energy

A

Energy of motion

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26
Q

Potential energy

A

Energy possessed by an object because of its position

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27
Q

Exothermic process

A

Processes that release energy

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28
Q

Endothermic process

A

Processes that require energy input

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29
Q

Scientific method

A

Observation -> Hypothesis -> Experiment -> Conclusion (theory)

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30
Q

Scientific notation

A

Decimal to the right equals negative exponent, decimal to the left equals positive exponent

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31
Q

Laws of conservation of mass

A

Mass is not gained or lost in a chemical reaction

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32
Q

Law of definite proportions

A

A compound always has the same mass ratio of the elements that compose it

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33
Q

Dalton’s Atomic theory

A

All matter is composed of atoms, AL atoms of an element are identical in physical and chemical properties, atoms are not created or destroyed in reactions, atoms rearrange into new combinations, obeying the law of conservation of mass

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34
Q

Temp

A

Change in heat

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35
Q

Structure of an atom

A

Composed of subatomic particles and nucleus

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36
Q

Protons

A

Located in a tiny core at the center of the atom with a positive charge. Can count on right hand corner of element in periodic table

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37
Q

Neutrons

A

In nucleus, no charge. Can be counted by subtracting proton number from mass number

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38
Q

Electrons

A

Occupies empty space around nucleus, negative charge. Number is equal to proton number

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39
Q

Atomic number

A

Number of protons in an atom. Protons + neutrons

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40
Q

Isotope

A

An atom that contains a specific number of neutrons (will have number of protons from element)

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41
Q

Isotopic symbol

A
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42
Q

Ions

A

Differ from atoms in that they have a charge, the number of electrons do not equal protons

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43
Q

Cations

A

Positively charged ions, fewer electrons

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44
Q

Anions

A

Negatively charged, more electrons

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45
Q

Group or family

A

Elements in the same column behave similarly

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46
Q

Period

A

Horizontal row

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47
Q

Ionic compounds

A

Made of cation (the metal) and anion (the nonmetals)

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48
Q

Name of cation

A

Name of metal + “ion”

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49
Q

Roman numerals

A

Used to indicate the (+). (ie copper 2+ is copper (II) ion)

50
Q

Cations with predictable charges

A

Alkali metals (+1), alkaline metals (+2)

51
Q

Anions

A

One non-metal, monoatomic group of nonmetals, polyatomic

52
Q

N -3

A

Nitride

53
Q

P -3

A

Phosphide

54
Q

O -2

A

Oxide

55
Q

S -2

A

Sulfide

56
Q

F -1

A

Fluoride

57
Q

Cl -1

A

Chloride

58
Q

Br -

A

Bromide

59
Q

I -

A

Iodide

60
Q

Polyatomic ions

A

Consists of a group of atoms, usually nonmetals

61
Q

S -2

A

Sulfide

62
Q

SO3 -2

A

Sulfite

63
Q

SO4 -2

A

Sulfate

64
Q

Only common polyatomic cation

A

NH4 +

65
Q

CO3 -2

A

Carbonate

66
Q

NO2 -

A

Nitrite

67
Q

NO3 -

A

Nitrate

68
Q

PO3 -3

A

Phosphite

69
Q

PO4 -3

A

Phosphate

70
Q

SO3 -2

A

sulfite

71
Q

SO4 -2

A

Sulfate

72
Q

HCO3 -1

A

Hydrogen carbonate

73
Q

HPO4 -2

A

Hydrogen phosphate

74
Q

H2PO4 -

A

Dihydrogen phosphate

75
Q

Halogens have

A

One negative charge

76
Q

FO-

A

Hypofluorite

77
Q

FO2-

A

Fluorite

78
Q

FO3 -

A

Fluorate

79
Q

FO4 -

A

Perfluorate

80
Q

BrO -

A

Hypobromite

81
Q

BrO2 -

A

Bromite

82
Q

BrO3 -

A

Bromate

83
Q

BrO4 -

A

Perbromate

84
Q

MnMPO4

A

Permanganate ion

85
Q

CrO4 -2

A

Chromate ion

86
Q

OH-

A

Hydroxide ion

87
Q

C2H3O2 -

A

Acetate ion

88
Q

NH4 +

A

Ammonium ion

89
Q

Types of compounds

A

Metal first = ionic, H first = acid, NO metal at all = molecular

90
Q

Reactant

A

A substance that we start with that under goes a change

91
Q

Product

A

A new substance that forms during the reaction

92
Q

Evidence of reaction

A

Change in color, production of light, formation of solid or gas, change in heat

93
Q

Chemical equations

A

Subscript after formulas, (S) (g) (L)

94
Q

Relative atomic mass

A

(isotope mass of isotope 1) x (relative abundance of isotope 1) + (isotope mass of isotope 2) x (relative abundance of isotope 2)

95
Q

Alkali metals

A

Group 1 metals

96
Q

Alkaline metals

A

Group 2 metals

97
Q

Halogens

A

Group 17 nonmetals

98
Q

Noble gases

A

Group 18 nonmetals

99
Q

Main-group elements

A

Contain any element in the 8 groups designated with the letter A, groups 1, 2, and 13-18

100
Q

Transition metals

A

Groups 3-12

101
Q

7 elements that exist as diatomic molecules

A

N2, O2, F2, C12, Br2, I2, H2

102
Q

Metals tend to lose electrons

A

To become cations, to have the same number of electrons as the last noble gas

103
Q

Nonmetalls tend to gain electrons

A

To become anions, to have the same number of electrons as the next noble gas

104
Q

Acids

A

A substance that loses an H+ when reacting with water

105
Q

Bases

A

Substances that losee an OH- when reacting with water

106
Q

Binary acids

A

Made from hydrogen + one non-metal. Use hydro prefix and - ic

107
Q

HF (aq)

A

Hydrofluoric acid

108
Q

HCI (aq)

A

Hydrochloric acid

109
Q

HI (aq)

A

Hydroiodic acid

110
Q

H2S (aq)

A

Hydrosulfuric acid

111
Q

Oxyacids

A

Made from hydrogen and polyatomic anion. - ate becomes - ic, - ite becomes - ous, - ide

112
Q

Water

A

H2O

113
Q

Ammonia

A

NH3

114
Q

Methane

A

CH4

115
Q

Sodium chloride

A

NaCl

116
Q

Sodium nitrite

A

NaNO2

117
Q

Magnesium chloride

A

MgCl2

118
Q

Magnesium nitrate

A

Mg(NO3) 2

119
Q

Barium oxide

A

BaO

120
Q

Lithium nitride

A

Li3N

CHEM 130 (16 decks)

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