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

Midterm 1- Chapters 1-4 Flashcards

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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
Q

vaporization

A

physical change from liquid to gas

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26
Q

condensation

A

gas to liquid

27
Q

sublimation

A

liquid to gas

28
Q

depostion

A

gas to solid

29
Q

Law of definite proportions

A

all samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements

30
Q

Law of Multiple Proportions

A

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
Q

Cathode Ray Experiment

A

determined the charge to mass ratio of electrons

32
Q

oil drop experiment

A

determined the charge to mass ratio of electrons

33
Q

Gold foil experiment

A

determined the location of protons in an atom

34
Q

Bombardment experiment

A

determined the presence of neutrons in an atom

35
Q

Electromagnetic radiation

A

oscillating electric and magnetic fields

36
Q

interference

A

addition of wave amplitudes when the waves overlap

37
Q

diffraction

A

waves bend when they encounter an obstacle that is about the same size as the wavelength

38
Q

photoelectric effect

A

electrons are sometimes ejected upon irradiation of a metal surface

39
Q

work function

A

the energy it takes for an electron to escape its binding energy to the atom

40
Q

de Broglie wavelength

A

the wavelength any matter has by virtue of its momentum

41
Q

Heisenberg’s uncertainty principle

A

the position and momentum of an object cannot both be known simultaneously with infinite precision

42
Q

Schrodinger Equation

A

describes the state (position and energy) of an atom’s electrons

43
Q

node

A

where the value of the wave function is zero

44
Q

Pauli Exclusion Principle

A

no two electrons in an atom may have the same set of four quantum numbers

45
Q

Coulomb’s law

A

potential energy associated with the attraction and repulsion of charged particles

46
Q

shielding

A

valence electrons “feel” less pull from the nucleus than core electrons do

47
Q

penetration

A

the possibility of high-energy electrons approaching areas closer to the nucleus

48
Q

Degenerate states

A

states that have the same energy as each other

49
Q

Core electrons

A

electrons in the inner “n” levels

50
Q

valence electrons

A

electrons in the outermost (highest) “n” level

51
Q

ground state

A

The configuration of electrons in which all electrons are in as low an energy orbital as possible

52
Q

excited state

A

any configuration in which at least one electron is in a higher-than-baseline energy orbital

53
Q

Aufbau principle

A

fill electrons from low energy to high energy

54
Q

Hund’s rule

A

Maximize spin alignment in degenerate orbitals and don’t pair spins unless necessary

55
Q

Isoelectronic

A

species containing the same electron configuration

56
Q

Effective nuclear charge

A

the amount of proton’s an orbiting electron “feels”

57
Q

paramagnetic

A

electron configuration with unpaired electrons

58
Q

diamagnetic

A

electrons configurations with no unpaired electrons

59
Q

ionization energy

A

amount of energy needed to remove an electron from an atom/ion, increases bottom to top, left to right

60
Q

electron affinity

A

amount of energy gained or released when an atom/ion gains an electron, increases left to right, bottom to top

61
Q

Pauling Electronegativity

A

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
Q

Atomic radius

A

increases top to bottom, right to left

63
Q

cation radius

A

smaller than a neutral atom, high valence shell=larger

64
Q

anion radius

A

larger than a neutral atom, higher valence shell=larger

Chem 142 (1 decks)

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