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Alexis Small > Chem Final Definitions > Flashcards

Chem Final Definitions Flashcards

1
Q

scientific method

A

approach to acquire knowledge through observation of phenomena

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2
Q

experiment

A

an observation of natural phenomena tested in a controlled and repeatable process and a rational conclusion can be made

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3
Q

hypothesis

A

a tentative and testable explanation for an observation or a series of observations

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4
Q

theory

A

a tested explanation of basic natural phenomena

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5
Q

law

A

a statement that summarizes a vast number of experimental observations, and describes or predicts some aspect of the natural world

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6
Q

precision

A

agreement among repeated measurements

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7
Q

accuracy

A

agreement between a measured value and the accepted or true value

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8
Q

chemistry

A

study of the composition and structure matter and of the changes that matter undergoes

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9
Q

matter

A

whatever occupies space and can be perceived by our senses

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10
Q

Law of Conservation of Mass

A

no mass is lost from the start of a process to the end

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11
Q

extensive property

A

depends on the amount of substance

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12
Q

intensive property

A

does not depend on the amount of substance

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13
Q

physical property

A

can be observed without doing a chemical reaction

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14
Q

chemical property

A

cannot be observed without doing a chemical reaction

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15
Q

pure substance

A

same physical and chemical properties throughout; cannot be separated into simpler substances by a physical process

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16
Q

mixture

A

combination of two or more pure substances; can be separated by physical processes

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17
Q

elements

A

a pure substance that cannot be separated into simpler substance by any chemical process

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18
Q

compounds

A

pure substance composed of two or more different elements bonded together in fixed proportions–> can be broken down into individual elements via chemical means

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19
Q

Law of Constant Composition

A

all samples of a particular compound contain the same elements combined in the same proportions

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20
Q

homogenous

A

components are distributed uniformly through the sample and have no visible boundaries or regions

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21
Q

heterogeneous

A

components are not distributed uniformly, and there may be distinct regions with different compositions

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22
Q

separating mixtures

A

distillation, filtration, chromatography

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23
Q

nucleus

A

positively charged at the center of the atom, contains the vast majority of the atom’s mass

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24
Q

nucleons

A

particles in the nucleus

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25
protons
positively charged subatomic particles
26
neutrons
electrically neutral subatomic particles
27
atomic mass
total number of nucleons in nucleus
28
atomic number
the number of protons in the nucleus
29
isotope
atoms of the same element that contains a different number of neutrons (diff mass)
30
average atomic mass
weighted average of the masses of ALL isotopes of an element (multiply natural abundance of each isotope by the mass)
31
ions
neutral atoms that gain/lose electrons
32
cations
ions with positive charges
33
anions
ions with negative charges
34
ionic compounds
made of a metal and a nonmetal (metals form cations, nonmetals from anions)
35
molecular compounds
composed of atoms held together in molecules by covalent bonds and are composed of nonmetals
36
covalent bonds
bond between two atoms created by sharing one or more pairs of electrons
37
empirical formula
shows the smallest whole number ration of elements in a compound
38
polyatomic ions
charged group of two or more atoms joined together by covalent bonds
39
oxyanion
polyatomic anions containing oxygen in combination with one or more other elements
40
Law of Conservation of Mass
the sum of the masses of the reactants in a chemical equation is qual to the sum of the masses of the products
41
percent composition
the mass percentage of each element in the compound
42
hydrocarbon
molecular compounds composed of only hydrogen and carbon
43
limiting reactant
substance that is completely consumed in the chemical reaction; determines the amount of product that can be formed during the reaction
44
theoretical yield
the calculated amount of product formed based on the amount of limiting reactant
45
actual yield
the measured amount of product fomred
46
chemical equation
describe ratios of reactants and products during a chemical reaction
47
coefficients
indicated ratio of reactants and products on molecular or molar level
48
solution
homogeneous mixtures of two or more substances
49
solvent
component of solution that is greatest in amount
50
solute
any component in a solution other than the solvent
51
aqueous solution
water is the solvent
52
concentrated solution
large amount of solute compared to solvent
53
dilute solution
small amount of solute compared to solvent
54
saturated solution
a solution that contains the max concentration of a solute possible at a given temperature
55
unsaturated solution
a solution that contains less than the maximum concentration of a solute possible at given temp (can dissolve more of solute into solution)
56
supersaturated solution
solution containing more than the maximum quantity of solute predicted to be soluble in a given volume of a solution at a given temperature
57
stock solution
a concentrated solution of a substance used to prepare solutions of lower concentration
58
dilution
the process of lowering the concentration of a solution by adding more solvent
59
electrolyte
dissolves in water to give an electrically conducting solution
60
acid
proton donor
61
base
proton acceptor
62
neutralization
reaction that takes place when an acid reacts with a base and produces a solution of salt in water
63
salt
cation of the base and anion of the acid
64
strong acids/bases
dissociate completely in aqueous solution (weak= dissociate partially)
65
titration
an analytical method to determine the concentration of a solute in a sample by reacting it with a standard solution
66
standard solution
a solution of known concentration
67
ionic equation
ionic species are represented as dissolved ions
68
net ionic equation
remove spectator ions
69
oxidation
loss of electrons
70
reduction
gain of electrons
71
diffusion
the process whereby a gas spreads out through another gas to occupy the space uniformly
72
effusion
the process by which a gas flows through a small hole in a container (ex: pinprick of a balloon)
73
thermodynamics
the study of energy and its transformations
74
thermochemistry
study of the relation between chemical reactions and changes in energy
75
thermochemical equilibrium
a condition in which temperature is uniform throughout a material and no energy flows from one point to another
76
energy
the capacity to do work
77
law of conservation of energy
energy can neither be created nor destroyed; can be converted from one form to another
78
system
the part of the universe that is the focus of a thermochemical study
79
surroundings
everything in the universe that is not part of the system
80
open system
can exchange matter and energy with surroundings
81
closed system
can exchange energy but not matter with surroundings
82
isolated system
does not exchange matter or energy with surroundings
83
heat
the energy transferred between objects because of a difference in their temperatures
84
extensive property
a property that depends on the amount of substance
85
molar heat capacity
the heat required to raise the temp of 1 mole of a substance by 1 degree C at constant pressure
86
specific heat capacity
the heat required to raise the temp of 1 gram of a substance by 1 degree C at constant pressure
87
calorimetry
measurement of heat
88
heat of reaction
the heat absorbed or released by a chemical reaction
89
wave
a contiuously repeating change or oscillation in matter
90
electromagnetic spectrum
the range of frequencies and wavelengths of electromagnetic radiation
91
wavelength
the distance between identical points on successive waves
92
amplitude
the vertical distance from the midline of a wave to the peak or trough
93
frequency
the number of waves that pass through a particular point in 1 second
94
refraction
bending of light waves when passing between media of different densities
95
diffraction
bending of light waves as they pass around the edge of an object or through narrow openings
96
interference
interaction of waves in which amplitudes either reinforce (constructive) or cancel (destructive)
97
quantized states
discrete energy levels
98
continuum states
smooth transition between levels
99
emission line spectra
consist of bright lines at discrete wavelengths on a dark background
100
absorption line spectra
consist of characteristic series of dark lines in continuous spectra
101
degenerate
orbitals that have the exact same energy level
102
isoelectronic
atoms/ions that have identical electron configurations
103
paramagnetic
weakly attracted to magnetic field, usually the result of unpaired electrons
104
diamagnetic
not attracted by a magnetic field generally because it has only paired electrons

Alexis Small (19 decks)

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