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HChem vocab Flashcards

1
Q

Chemistry

A

The study of matter, its properties, composition, and the changes it undergoes.

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2
Q

Matter

A

Anything that has mass and takes up space.

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3
Q

Mass

A

A measurement that reflects the amount of matter (does not change with location like weight)

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4
Q

Volume

A

The amount of space matter occupies

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5
Q

Weight

A

A force due to gravity can change with distance from the center of the Earth. (altitude)

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6
Q

Organic Chemistry

A

Focuses on most carbon-containing chemicals. (ex. Pharmaceuticals, plastics)\

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7
Q

Inorganic Chemistry

A

Focuses on materials that, in general, do not contain carbon. (Minerals, metals, non-metals, and semiconductors)

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8
Q

Physical Chemistry

A

Focuses on the behavior and changes in matter and the related energy changes

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9
Q

Analytical Chemistry

A

Focuses on the components and composition of substances. (Food, nutrients, quality control)

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10
Q

Biochemistry

A

Focuses on the matter and processes of living organisms (ex Metabolism, fermentation)

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11
Q

Alchemy/Alchemists

A

Heavily interested in the transmutation of metals. Wanted to change common metals into gold. Wanted to find a cure for diseases and internal life.

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12
Q

Practical Alchemy

A

Developing techniques for working with metals, glass, and dyes

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13
Q

Mystical Alchemy

A

Focused on concepts like perfection, eternal life, and sorcery.

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14
Q

Qualitative date

A

Information that describes color, odor, shape, or some other physical characteristics

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15
Q

Quantitative data

A

Information that is numerical based (data, charts, volume, mass)

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16
Q

Hypothesis

A

A tentative explanation for what has been observed, cannot be proven by an experiment, but it can be disproven

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17
Q

Scientific Law

A

A summary of accepted facts of nature

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18
Q

Theory

A

A hypothesis supported by many experiments

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19
Q

Pure Research

A

Research motivated by pure curiosity

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20
Q

Applied Research

A

Research undertaken to solve a specific problem

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21
Q

International System of Units (SI)

A

A revised version of the metric system. (meter, kilogram, kelvin, second, and mole)

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22
Q

Kelvin Scale

A

the freezing point of water is 273.15k and the boiling point is 373.15k

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23
Q

Accuracy

A

A measure of how close a measurement comes to the actual or true value of whatever is measured.

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24
Q

Precision

A

A measurement of how close a series of measurements are to one another

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25
Error
Can be positive or negative depending on whether the experimental value is greater than or less than the accepted value.
26
Significant figures
a measurement that includes all of the digits that are known, plus an estimated last digit.
27
Extensive properties
A property that depends on the amount of matter in a sample (ex. Mass and volume)
28
Intensive properties
a property that depends on the type of matter.
29
Uniform substance
A substance that is the same, not varying throughout
30
Definite substance
A substance that is established, unchanging
31
Physical property
A quality or condition of substance that can be observed or measured without changing the substance composition
32
Solids
A form of matter that has an indefinite shape and volume. Particles are closely packed, often in orderly arrangements, incompressible, and expand slightly when heated.
33
Liquid
A form of matter that has an indefinite shape, and flows, yet has a fixed volume, particles are in close contact with one another but aren't as rigid or orderly, the volume doesn't change as the shape does, expands slightly when heated
34
Gaases
A form of matter that takes both the shape and volume of its container, particles are far apart, they are easily compressed into smaller volumes, and they expand greatly upon heating.
35
Vapor
Describes that gaseous state if a substance that is generally liquid or solid at room temperature
36
Physical Change
A change in which some properties of a material change, but the composition of the material does not change.
37
Reversible physical change
All changes in state, including boiling, freezing, melting, and condensing
38
Irreversible physical change
Breaking, splitting, grinding, cutting, and crushing.
39
Mixture
A physical blend of two or more compounds
40
Heterogenous Mixture
A mixture in which the composition is not uniform. Components are unevenly distributed, two or more phases.
41
Homogenous Mixture
A mixture in which the composition is uniform throughout. Components are evenly distributed and the particles of these components are about 1nm. One phase.
42
Solution
Another name for a homogenous mixture can be a solid, liquid, or gas mixture.
43
Phase
A term used to describe any part of a sample with uniform composition.
44
Filtration
A process that separates a solid from the liquid in a heterogenous mixture based on particle size
45
Distillation
a separation method in which a liquid is boiled to produce a vapor that is then condensed into a liquid, based on different boiling points of the components in a mixture
46
Substance
A material with a fixed composition can be classified as an element or compounds
47
Element
The simplest form of matter that has a unique set of properties
48
Compound
A substance that contains two or more elements chemically combined in a fixed proportion. Only can be separated into simpler substances through a chemical change.
49
Chemical change
A change that produces matter with a different composition than the original matter
50
Chemical symbols
Used by chemists to represent elements
51
Chemical formulas
Used to represent compounds
52
Subscripts
Used in chemical formulas to indicate the relative proportions of the elements in the compound.
53
Chemical property
The ability of a substance to undergo a specific chemical change
54
Reactant
A substance present at the start of the reaction
55
Product
A substance produced in the reation
56
Protons
Positively charged particles that have an atomic mass of 1 amu. Carries exactly one unit of positive charge. Discovered by Ernest Rutherford in his gold experiment.
57
Electrons
Negatively charged particles were discovered by J.J. Thomson through his cathode ray experiment. Mass is 1/1840, which is also the mass of a hydrogen atom, which is discovered by Robert Millikan in his oil drop experiment.
58
Neutrons
Particles that do not carry a positive or negative charge. Discovered by James Chadwick. The atomic mass of 1 amu.
59
Amplitude
The wave height from zero to the crest
60
Wavelength
λ (lambda), the distance between crests
61
Frequency
v (nu), the number of wave cycles to pass a given point per unit time.
62
Hertz (Hz)
Units of frequency, other being cycles/seconds (1/s, or s^-1)
63
Speed of light (c)
The product of the frequency and wavelength. (c= 3.00 x 10^8m/s) (c= λν)
64
Electron magnetic radiation
Waves include radio waves, microwaves, infrared waves, ultraviolet waves, X-rays, and gamma waves.
65
Spectrum
When sunlight passes through a prism, the different frequencies of light separate into colors, forming this.
66
Atomic emission spetrum
Specific, individual lines of the rainbow of an element that are produced by the light emitted by energized electrons in atoms.
67
Ground state
The lowest possible energy an electron in the atom can possess
68
Principle quantum number
The numbered energy levels from the nucleus outward (n)
69
Excited state
The raising of an electron from the ground state to a new energy level by absorbing energy
70
Electron configuration
The ways in which electrons are arranged in various orbitals around the nuclei of atoms.
71
Aufbau Principle
Electrons occupy the orbitals of lowest energy first.
72
Pauli exclusion principle
An atomic orbital may describe at most 2 electrons
73
Hund's rule
Electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible

Midterms (3 decks)

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