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Chem 101 - MidTerm > Mid Term > Flashcards

Mid Term Flashcards

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1
Q

Mixture

A

matter that can separated into it’s components by physical means

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2
Q

Compounds

A

pure substances that can be broken down by chemical changes

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3
Q

Elements

A

pure substances that can’t be broken down by chemical changes

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4
Q

Physical Change

A

change in the state or properties of matter that doesn’t involve a change in it’s chemical composition

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5
Q

Chemical Change

A

Change producing a different kind of matter from original matter

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6
Q

Mass

A

measure of the amount of matter

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7
Q

Weight

A

the force that gravity exerts on an object

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8
Q

Unit Conversion Factor

A

ratio of equivalent quantities expressed with different units: used to convert from one unit to another

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9
Q

Intensive property

A

Property of a substance that is independent of the amount of the substance

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10
Q

Extensive property

A

property of a substance that depends on the amount of the substance

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11
Q

Chemical Property

A

Behavior related to the change of one kind of matter into another kind of matter

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12
Q

Physical Property

A

Characteristic of matter that isn’t associated with any change in it’s chemical compound

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13
Q

Molecule

A

Bonded collection of two or more atoms of the same or different elements

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14
Q

Atom

A

smallest particle of an element that can enter into a chemical combination

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15
Q

Pure Substance

A

Has a constant composition

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16
Q

Law of Conservation of Matter

A

When matter converts from one type to another or changes form, there is no detectable change in the total amount of matter present

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17
Q

Matter

A

Anything that occupies space and has mass

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18
Q

Symbolic Domain

A

Contains Specialized language to represent components of macro and micro domains

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19
Q

Scientific Method

A

path of discovery that leads from question and observation to law or hypothesis ir theory, combined with experimental verification of the hypothesis and any necessary modification of the theory

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20
Q

Theory

A

well substantiated, comprehensive, testable explanations of particular aspects of nature

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21
Q

Laws

A

Summarize a vast number of experimental observations and describe or predict some facet of the natural world

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22
Q

Structural Isomers

A

Compounds in which the molecules differ in how the atoms are connected

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23
Q

Isomers

A

compounds with the same chemical formula but different molecular structures

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24
Q

Alpha Particles

A

2 protons and 2 neutrons, positively charged

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25
Q

Electron

A

Negatively charged, subatomic particle of relatively low mass located inside the nucleus

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26
Q

Law of Multiple Proportions

A

When two elements react to form more than one compound, a fixed mass of one element will react with masses of the other element in a ratio of small, whole numbers

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27
Q

Law of Definite Proportions or Law of Constant Composition

A

All samples of a pure compounds contain the same elements in the same proportion by mass

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28
Q

Anion

A

Negatively charged atom or molecule (contains more electrons than protons)

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29
Q

Atomic Mass Unit

A

unit of mass equal to 1/12 of the mass of 12g Carbon

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30
Q

Empirical Formula

A

Formula showing the composition of a compound given as the simplest whole number ratio

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31
Q

Ion

A

Electrically charged atom or molecule (contains unequal numbers of protons and electrons)

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32
Q

Nucleus

A

Massive, positively charged center of an atom made up of protons and neutrons

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33
Q

Isotopes

A

Atoms that contain the same number of protons but different numbers of neutrons

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34
Q

Hypothesis

A

A tentative explanation of observations that acts as a guide for gathering and chicken info

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35
Q

Structural Formula

A

Gives the same info as molecular formula (types and numbers of atoms in the molecule) but also shows how the atoms are connected in the molecule

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36
Q

Molecular Formula

A

A representation of a molecule that uses chemical symbols to indicate the types of atoms followed by subscripts to show the number of atoms of each type in the molecule

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37
Q

Atomic Mass

A

The atomic mass of a single atom is approximately equal to its mass number

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38
Q

Mass Number (A)

A

the total number of protons and neutrons in an atom

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39
Q

Atomic Number (Z)

A

The number of protons in the nucleus of an atom

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40
Q

Neutrons

A

Unchanged, subatomic particles with a mass approximately the same as that of protons, located in the nucleus

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41
Q

Spatial Isomers

A

The relative orientations of the atoms in space can be different

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42
Q

Cation

A

Positively charged atom of molecule (contains fewer electrons than protons)

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43
Q

Proton

A

positively charged subatomic particle in the nucleus

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44
Q

Covalent Bonds (Molecular Compound)

A

composed of molecules formed by atoms of two or more different elements

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45
Q

Binary Compounds

A

Compound containing two different elements

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46
Q

Binary Acid

A

Compound that contains hydrogen and one other element, bonded in a way that imparts acidic properties to the compound (Ability to release H+ ions when dissolved in water)

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47
Q

Nonmetals

A

Elements that appear dull, poor conductors of heat and electricity

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48
Q

Metalloids

A

Elements that conduct heat and electricity moderately well, possess some properties of metals and some nonmetals

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49
Q

Metals

A

elements that are shiny, malleable, good conductors of heat and electricity

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50
Q

Hydrates

A

Compound containing one or more water molecules bound within it’s crystals

51
Q

Ionic Bonds

A

Electrostatic forces of attraction between the oppositely charged ions of an ionic compound

52
Q

Ionic Compound

A

Compound composed of cations and anions combined in ratios, yielding an electrically neutral substance

53
Q

Molecular Compounds (Covalent Compound)

A

Compound of molecules formed by atoms of two or more different elements

54
Q

Monatomic Ions

A

Ion composed of a singular atom

55
Q

Oxyacids

A

Compound that contains hydrogen, oxygen, and 1 other element, bonded in a way that imparts acidic properties to the compound (ability to release H+ ions when dissolved in water)

56
Q

Oxyanions

A

polyatomic anion composed of a central atom bonded to oxygen atoms

57
Q

Polyatomic Ions

A

Ion composed of more than one atom

58
Q

Density

A

Mass Over Volume

59
Q

Volume

A

amount of space occupied by an object

60
Q

Gas

A

takes both the shape and volume of container

61
Q

Liquid

A

Flows and takes on shape of container; forms a flat or slightly curved upper surface when acted on by gravity

62
Q

Solid

A

Rigid and has definite shape

63
Q

Microscopic Domain

A

Often visited in imagination, some aspects are visible through standard optical microscopes

64
Q

Macroscopic Domain

A

Everyday things that are large enough to be sensed directly by human sight or touch

65
Q

Heterogenous Mixture

A

Combination of substances with a composition that varies from point to point

66
Q

Homogenous Mixture (Solution)

A

Combination of substances with a composition that is uniform throughout

67
Q

Empirical Formula Mass

A

Sum of average atomic masses for all atoms represented in an empirical formula

68
Q

Formula Mass

A

Sum of the average masses for all atoms represented in a chemical formula; for covalent compounds: this is also the molar mass

69
Q

Molar Mass

A

Mass in grams of one mole of a substance

70
Q

Mole

A

Amount of substance containing the same number of atoms, molecules, ions or other entities as the number of atoms in exactly 12 grams of Carbon

71
Q

Percent Composition

A

Percentage by mass of the various elements in a compound

72
Q

Aqueous Solution

A

Solution for which water is the solvent

73
Q

Concentration

A

Quantitative measure of the relative amounts of solute and solvent present in a solution

74
Q

Concentrated

A

a qualitative term for a solution containing solute at a relatively high concentration

75
Q

Dilute

A

Qualitative term for a solution containing solute at a relatively low concentration

76
Q

Dilution

A

Process of adding solvent to a solution in order to lower the concentration of solutes

77
Q

Dissolved

A

Describes the process by which solute components are dispersed in a solvent

78
Q

Mass Percentage

A

Ratio of a solute-to-solution mass expressed as a percentage

79
Q

Mass-Volume Percentage

A

ratio of solute mass to solution volume, expressed as a percentage

80
Q

Molarity (M)

A

Unit of concentration, defined as the number of moles of solute dissolved in 1L of solution

81
Q

Solvent

A

Solution component present in a concentration that is higher relative to other components

82
Q

Solute

A

Solution component present in a concentration less than that of the solvent

83
Q

Volume Percentage

A

Ratio of solute-to-solution volume expressed as a percentage

84
Q

Single-Displacement Reaction

A

Redox reaction involving the oxidation of an element substance by an ionic species

85
Q

Spectator Ions

A

Ion that doesn’t undergo a chemical or physical change during a reaction, but it’s presence is required to maintain charge neutrality

86
Q

Strong Acid

A

Acid that reacts completely when dissolved in water to yield hydronium ions

87
Q

Strong Base

A

Base that reacts completely when dissolved in water to yield hydroxide ions

88
Q

Weak Acid

A

Acid that reacts only to a slight extent when dissolved in water to release hydronium ions

89
Q

Weak Base

A

Base that reacts partially when dissolved in water to release hydroxide atoms

90
Q

Acid

A

Substance that produces H30+ when dissolved in water

91
Q

Acid Based Reactions

A

Reaction involving the transfer of a hydrogen ion between reactant species

92
Q

Base

A

Substance that produces OH- when dissolved in water

93
Q

Chemical Equation

A

Symbolic representation of a chemical reaction

94
Q

Coefficients

A

Number placed in front of symbols or formulas in a chemical equation to indicate their relative amount

95
Q

Combustion Reaction

A

Vigorous redox reaction producing significant amounts of energy in the form of heat, and sometimes light

96
Q

Complete Ionic Equation

A

Chemical equation in which all dissolved ionic reactants and products, including spectator ions, are explicitly represented by formulas for their dissociated ions

97
Q

Half-reaction

A

An equation that shows whether each reactant loses or gains electrons in a reaction

98
Q

Molecular Equation

A

Chemical Equation in which all reactants an products are represented as neutral substances

99
Q

Net Ionic Equations

A

Chemical equation in which only those dissolved ionic reactants and products that undergo a chemical or physical change are represented (excludes spectator ions)

100
Q

Neutralization Reaction

A

Reaction between an acid and a base to produce salt and water

101
Q

Oxidation

A

Process in which an element’s oxidation number is increased by the loss of electrons

102
Q

Oxidation Number

A

The charge each atom of an element would have in a compound if the compound were ionic

103
Q

Oxidation-Reduction Reaction (Redox)

A

Reaction involving a change in oxidation number for one or more reactant elements

104
Q

Oxidizing Agent

A

Substance that brings about the oxidation of another substance, and in the process becomes reduced

105
Q

Precipitation Reaction

A

Reaction that produces one or more insoluble products, when reactants are ionic compounds, sometimes called double-displacement or metathesis

106
Q

Reducing Agent

A

Substance that brings about the reduction of another substance and in the process becomes oxidized

107
Q

Actual Yield

A

Amount of product formed in a reaction

108
Q

Analyte

A

Chemical species of interest

109
Q

Buret

A

Device used for the precise delivery of variable liquid volumes, such as in titration analysis

110
Q

Combustion Analysis

A

Gravimetric technique used to determine the elemental composition of a compound win the collection and weighing of its gaseous combustion products

111
Q

End Point

A

Measured volume of titrant solution that yields the change in sample solution appearance or other property expected for stoichiometric equivalence

112
Q

Equivalence Point

A

Volume of titrant solution required to react completely with the analyze in titration analysis; provides a stoichiometric amount of titrant for the samples analyze according to the titration reaction

113
Q

Excess Reactant

A

Reactant present in an amount greater than required by the reaction stoichiometry

114
Q

Gravimetric Analysis

A

Quantitative chemical analysis method involving the separation of an analyze from a sample by a physical or chemical process and subsequent mass measurements of the analyze, reaction product, and/or sample

115
Q

Indicator

A

Substance added to the sample in a titration analysis to permit visual detection of the end point

116
Q

Limiting Reactant

A

Reactant present in an amount lower than required by the reaction stoichiometry, thus limiting the amount of product generated

117
Q

Percent Yield

A

Measure of the efficiency of a reaction, expressed as a percentage of the theoretical yield

118
Q

Quantitative Analysis

A

The determination of the amount or concentration of a substance in a sample

119
Q

Stoichiometric Factors

A

Ratio of coefficients in a balanced chemical equation, used in computations relating amounts of reactants and products

120
Q

Stoichiometry

A

Relationships between the amounts of reactants and products of a chemical reaction

121
Q

Theoretical Yield

A

Amount of product that may be produced from a given amount of reactants according to the reaction stoichiometry

122
Q

Titrant

A

Solution containing a known concentration of substance that will react with the analyze in a titration analysis

123
Q

Titration Analysis

A

Quantitative chemical analysis method that involves measuring the volume of a reactant solution

Chem 101 - MidTerm (1 decks)

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