Mid Term Flashcards
(123 cards)
1
Q
Mixture
A
matter that can separated into it’s components by physical means
2
Q
Compounds
A
pure substances that can be broken down by chemical changes
3
Q
Elements
A
pure substances that can’t be broken down by chemical changes
4
Q
Physical Change
A
change in the state or properties of matter that doesn’t involve a change in it’s chemical composition
5
Q
Chemical Change
A
Change producing a different kind of matter from original matter
6
Q
Mass
A
measure of the amount of matter
7
Q
Weight
A
the force that gravity exerts on an object
8
Q
Unit Conversion Factor
A
ratio of equivalent quantities expressed with different units: used to convert from one unit to another
9
Q
Intensive property
A
Property of a substance that is independent of the amount of the substance
10
Q
Extensive property
A
property of a substance that depends on the amount of the substance
11
Q
Chemical Property
A
Behavior related to the change of one kind of matter into another kind of matter
12
Q
Physical Property
A
Characteristic of matter that isn’t associated with any change in it’s chemical compound
13
Q
Molecule
A
Bonded collection of two or more atoms of the same or different elements
14
Q
Atom
A
smallest particle of an element that can enter into a chemical combination
15
Q
Pure Substance
A
Has a constant composition
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
17
Q
Matter
A
Anything that occupies space and has mass
18
Q
Symbolic Domain
A
Contains Specialized language to represent components of macro and micro domains
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
20
Q
Theory
A
well substantiated, comprehensive, testable explanations of particular aspects of nature
21
Q
Laws
A
Summarize a vast number of experimental observations and describe or predict some facet of the natural world
22
Q
Structural Isomers
A
Compounds in which the molecules differ in how the atoms are connected
23
Q
Isomers
A
compounds with the same chemical formula but different molecular structures
24
Q
Alpha Particles
A
2 protons and 2 neutrons, positively charged
25
Electron
Negatively charged, subatomic particle of relatively low mass located inside the nucleus
26
Law of Multiple Proportions
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
27
Law of Definite Proportions or Law of Constant Composition
All samples of a pure compounds contain the same elements in the same proportion by mass
28
Anion
Negatively charged atom or molecule (contains more electrons than protons)
29
Atomic Mass Unit
unit of mass equal to 1/12 of the mass of 12g Carbon
30
Empirical Formula
Formula showing the composition of a compound given as the simplest whole number ratio
31
Ion
Electrically charged atom or molecule (contains unequal numbers of protons and electrons)
32
Nucleus
Massive, positively charged center of an atom made up of protons and neutrons
33
Isotopes
Atoms that contain the same number of protons but different numbers of neutrons
34
Hypothesis
A tentative explanation of observations that acts as a guide for gathering and chicken info
35
Structural Formula
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
36
Molecular Formula
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
37
Atomic Mass
The atomic mass of a single atom is approximately equal to its mass number
38
Mass Number (A)
the total number of protons and neutrons in an atom
39
Atomic Number (Z)
The number of protons in the nucleus of an atom
40
Neutrons
Unchanged, subatomic particles with a mass approximately the same as that of protons, located in the nucleus
41
Spatial Isomers
The relative orientations of the atoms in space can be different
42
Cation
Positively charged atom of molecule (contains fewer electrons than protons)
43
Proton
positively charged subatomic particle in the nucleus
44
Covalent Bonds (Molecular Compound)
composed of molecules formed by atoms of two or more different elements
45
Binary Compounds
Compound containing two different elements
46
Binary Acid
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)
47
Nonmetals
Elements that appear dull, poor conductors of heat and electricity
48
Metalloids
Elements that conduct heat and electricity moderately well, possess some properties of metals and some nonmetals
49
Metals
elements that are shiny, malleable, good conductors of heat and electricity
50
Hydrates
Compound containing one or more water molecules bound within it's crystals
51
Ionic Bonds
Electrostatic forces of attraction between the oppositely charged ions of an ionic compound
52
Ionic Compound
Compound composed of cations and anions combined in ratios, yielding an electrically neutral substance
53
Molecular Compounds (Covalent Compound)
Compound of molecules formed by atoms of two or more different elements
54
Monatomic Ions
Ion composed of a singular atom
55
Oxyacids
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
Oxyanions
polyatomic anion composed of a central atom bonded to oxygen atoms
57
Polyatomic Ions
Ion composed of more than one atom
58
Density
Mass Over Volume
59
Volume
amount of space occupied by an object
60
Gas
takes both the shape and volume of container
61
Liquid
Flows and takes on shape of container; forms a flat or slightly curved upper surface when acted on by gravity
62
Solid
Rigid and has definite shape
63
Microscopic Domain
Often visited in imagination, some aspects are visible through standard optical microscopes
64
Macroscopic Domain
Everyday things that are large enough to be sensed directly by human sight or touch
65
Heterogenous Mixture
Combination of substances with a composition that varies from point to point
66
Homogenous Mixture (Solution)
Combination of substances with a composition that is uniform throughout
67
Empirical Formula Mass
Sum of average atomic masses for all atoms represented in an empirical formula
68
Formula Mass
Sum of the average masses for all atoms represented in a chemical formula; for covalent compounds: this is also the molar mass
69
Molar Mass
Mass in grams of one mole of a substance
70
Mole
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
Percent Composition
Percentage by mass of the various elements in a compound
72
Aqueous Solution
Solution for which water is the solvent
73
Concentration
Quantitative measure of the relative amounts of solute and solvent present in a solution
74
Concentrated
a qualitative term for a solution containing solute at a relatively high concentration
75
Dilute
Qualitative term for a solution containing solute at a relatively low concentration
76
Dilution
Process of adding solvent to a solution in order to lower the concentration of solutes
77
Dissolved
Describes the process by which solute components are dispersed in a solvent
78
Mass Percentage
Ratio of a solute-to-solution mass expressed as a percentage
79
Mass-Volume Percentage
ratio of solute mass to solution volume, expressed as a percentage
80
Molarity (M)
Unit of concentration, defined as the number of moles of solute dissolved in 1L of solution
81
Solvent
Solution component present in a concentration that is higher relative to other components
82
Solute
Solution component present in a concentration less than that of the solvent
83
Volume Percentage
Ratio of solute-to-solution volume expressed as a percentage
84
Single-Displacement Reaction
Redox reaction involving the oxidation of an element substance by an ionic species
85
Spectator Ions
Ion that doesn't undergo a chemical or physical change during a reaction, but it's presence is required to maintain charge neutrality
86
Strong Acid
Acid that reacts completely when dissolved in water to yield hydronium ions
87
Strong Base
Base that reacts completely when dissolved in water to yield hydroxide ions
88
Weak Acid
Acid that reacts only to a slight extent when dissolved in water to release hydronium ions
89
Weak Base
Base that reacts partially when dissolved in water to release hydroxide atoms
90
Acid
Substance that produces H30+ when dissolved in water
91
Acid Based Reactions
Reaction involving the transfer of a hydrogen ion between reactant species
92
Base
Substance that produces OH- when dissolved in water
93
Chemical Equation
Symbolic representation of a chemical reaction
94
Coefficients
Number placed in front of symbols or formulas in a chemical equation to indicate their relative amount
95
Combustion Reaction
Vigorous redox reaction producing significant amounts of energy in the form of heat, and sometimes light
96
Complete Ionic Equation
Chemical equation in which all dissolved ionic reactants and products, including spectator ions, are explicitly represented by formulas for their dissociated ions
97
Half-reaction
An equation that shows whether each reactant loses or gains electrons in a reaction
98
Molecular Equation
Chemical Equation in which all reactants an products are represented as neutral substances
99
Net Ionic Equations
Chemical equation in which only those dissolved ionic reactants and products that undergo a chemical or physical change are represented (excludes spectator ions)
100
Neutralization Reaction
Reaction between an acid and a base to produce salt and water
101
Oxidation
Process in which an element's oxidation number is increased by the loss of electrons
102
Oxidation Number
The charge each atom of an element would have in a compound if the compound were ionic
103
Oxidation-Reduction Reaction (Redox)
Reaction involving a change in oxidation number for one or more reactant elements
104
Oxidizing Agent
Substance that brings about the oxidation of another substance, and in the process becomes reduced
105
Precipitation Reaction
Reaction that produces one or more insoluble products, when reactants are ionic compounds, sometimes called double-displacement or metathesis
106
Reducing Agent
Substance that brings about the reduction of another substance and in the process becomes oxidized
107
Actual Yield
Amount of product formed in a reaction
108
Analyte
Chemical species of interest
109
Buret
Device used for the precise delivery of variable liquid volumes, such as in titration analysis
110
Combustion Analysis
Gravimetric technique used to determine the elemental composition of a compound win the collection and weighing of its gaseous combustion products
111
End Point
Measured volume of titrant solution that yields the change in sample solution appearance or other property expected for stoichiometric equivalence
112
Equivalence Point
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
Excess Reactant
Reactant present in an amount greater than required by the reaction stoichiometry
114
Gravimetric Analysis
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
Indicator
Substance added to the sample in a titration analysis to permit visual detection of the end point
116
Limiting Reactant
Reactant present in an amount lower than required by the reaction stoichiometry, thus limiting the amount of product generated
117
Percent Yield
Measure of the efficiency of a reaction, expressed as a percentage of the theoretical yield
118
Quantitative Analysis
The determination of the amount or concentration of a substance in a sample
119
Stoichiometric Factors
Ratio of coefficients in a balanced chemical equation, used in computations relating amounts of reactants and products
120
Stoichiometry
Relationships between the amounts of reactants and products of a chemical reaction
121
Theoretical Yield
Amount of product that may be produced from a given amount of reactants according to the reaction stoichiometry
122
Titrant
Solution containing a known concentration of substance that will react with the analyze in a titration analysis
123
Titration Analysis
Quantitative chemical analysis method that involves measuring the volume of a reactant solution
