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Chem 142 > Midterm 1- Chapters 1-4 > Flashcards

Midterm 1- Chapters 1-4 Flashcards

1
Q

observation

A

knowledge about the world received through the senses or instrumentation

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2
Q

fact

A

something that is known to be consistent with reality

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3
Q

law

A

a brief statement that summarizes past observations and predicts future ones

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4
Q

hypothesis

A

a tentative interpretation that can be tested through observation

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5
Q

accurate

A

value that is closest to the actual “correct” value being measured

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6
Q

theory

A

an explanation of some aspect of the natural world that has been substantiated through repeated experiments or facts gathered over time

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7
Q

precise

A

measurement that is repeatable

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8
Q

matter

A

anything that has mass and takes up space

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9
Q

atom

A

the smallest possible component of matter capable of stable exsistence

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10
Q

element

A

a pure substance made of one type of atom

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11
Q

molecule

A

a chemical combination of two or more elements in fixed proportions

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12
Q

compound

A

a pure substance composed of two or more elements that are chemically combined

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13
Q

mixture

A

substances which can be physically separated into different substance

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14
Q

homogenous

A

a mixture with uniform appearance and properties throughout

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15
Q

heterogenous

A

a mixture with physically distinguishable components

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16
Q

solution

A

a homogenous mixture of two or more compounds

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17
Q

homonuclear

A

molecule composed of atoms of the same type

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18
Q

heteronuclear

A

molecule composed of multiple types of atoms

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19
Q

monatomic

A

molecule composed of one atom

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20
Q

diatomic

A

molecule composed of two atoms

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21
Q

triatomic

A

molecule composed of three atoms

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22
Q

polyatomic

A

molecule composed of more than three atoms

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23
Q

fusion

A

physical change from solid to liquid

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24
Q

freezing

A

physical change from liquid to solid

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25
vaporization
physical change from liquid to gas
26
condensation
gas to liquid
27
sublimation
liquid to gas
28
depostion
gas to solid
29
Law of definite proportions
all samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements
30
Law of Multiple Proportions
When two elements (a and b) form two different compounds, the masses of B that combine with 1 gram A can be expressed as a ratio of small whole numbers
31
Cathode Ray Experiment
determined the charge to mass ratio of electrons
32
oil drop experiment
determined the charge to mass ratio of electrons
33
Gold foil experiment
determined the location of protons in an atom
34
Bombardment experiment
determined the presence of neutrons in an atom
35
Electromagnetic radiation
oscillating electric and magnetic fields
36
interference
addition of wave amplitudes when the waves overlap
37
diffraction
waves bend when they encounter an obstacle that is about the same size as the wavelength
38
photoelectric effect
electrons are sometimes ejected upon irradiation of a metal surface
39
work function
the energy it takes for an electron to escape its binding energy to the atom
40
de Broglie wavelength
the wavelength any matter has by virtue of its momentum
41
Heisenberg's uncertainty principle
the position and momentum of an object cannot both be known simultaneously with infinite precision
42
Schrodinger Equation
describes the state (position and energy) of an atom's electrons
43
node
where the value of the wave function is zero
44
Pauli Exclusion Principle
no two electrons in an atom may have the same set of four quantum numbers
45
Coulomb's law
potential energy associated with the attraction and repulsion of charged particles
46
shielding
valence electrons "feel" less pull from the nucleus than core electrons do
47
penetration
the possibility of high-energy electrons approaching areas closer to the nucleus
48
Degenerate states
states that have the same energy as each other
49
Core electrons
electrons in the inner "n" levels
50
valence electrons
electrons in the outermost (highest) "n" level
51
ground state
The configuration of electrons in which all electrons are in as low an energy orbital as possible
52
excited state
any configuration in which at least one electron is in a higher-than-baseline energy orbital
53
Aufbau principle
fill electrons from low energy to high energy
54
Hund's rule
Maximize spin alignment in degenerate orbitals and don't pair spins unless necessary
55
Isoelectronic
species containing the same electron configuration
56
Effective nuclear charge
the amount of proton's an orbiting electron "feels"
57
paramagnetic
electron configuration with unpaired electrons
58
diamagnetic
electrons configurations with no unpaired electrons
59
ionization energy
amount of energy needed to remove an electron from an atom/ion, increases bottom to top, left to right
60
electron affinity
amount of energy gained or released when an atom/ion gains an electron, increases left to right, bottom to top
61
Pauling Electronegativity
The power of an atom in a molecule to attract electrons to itself, F is most electronegative, inc left to right, bottom to top
62
Atomic radius
increases top to bottom, right to left
63
cation radius
smaller than a neutral atom, high valence shell=larger
64
anion radius
larger than a neutral atom, higher valence shell=larger

Chem 142 (1 decks)

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