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0
Q

Mass of reactant = mass of product

A

Law of conservation of mass

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1
Q

Mass % of all elements is the same in a compound

A

Law of definite proportions

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2
Q

Ratio of elements in a compound is in whole number ratios

A

Law of multiple proportions

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3
Q

Atoms make up everything
Atoms cannot be created or destroyed
Atoms combine to form compounds

A

Dalton’s atomic theory

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4
Q

Amount of stuff

A

Mole

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5
Q

Energy of motion

A

Kinetic energy

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6
Q

Energy due to position

A

Potential energy

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7
Q

Kinetic energy formula

A

KE=1/2mv^2

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8
Q

Force of intersection; between charged particles when brought together

A

Electromagnetic force

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9
Q

2 particles with a charge q1 and q2 by distance r on force f

A

Coulomb’s law

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10
Q

When F is - when q1 and q2 have opposite signs

A

Attractive force

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11
Q

F is positive when q1 and q2 have the same sign

A

Repulsive force

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12
Q

Force exerted through distance

A

Energy

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13
Q

A

A

Mass number

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14
Q

Of protons and # of neutrons

A

Mass number

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15
Q

Z

A

Atomic number (number of protons)

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16
Q

Conducted the cathode ray experiment

A

JJ Thompson

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17
Q

Anode and cathode and high voltage ray through a tube deflect many directions

A

Cathode ray experiment

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18
Q

JJ Thompson discovered —

A

The electron

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19
Q

Millikan’s oil drop experiment found — and —

A

The charge of the electron and the mass of the electron

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20
Q

Oil drop experiment was conducted by whom?

A

Millikan

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21
Q

Alpha parties shot at gold foil, most passed through but some deflected

A

Rutherford’s gold foil experiment

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22
Q

In the gold foil experiment the — was found and it gave us the —

A

Nucleus
Nuclear model of the atom

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23
Q

Theory that states almost all mass and positive charge is found in the nucleus, most volume is empty space, and the number of protons equals the number of electrons making the atom neutral

A

Rutherford’s theory

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24
Q

Substance converted
Color change
Dissolving

A

Chemical properties

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25
Q

Retains identity
States of matter
Changes of shape
Density, melting point, malleability

A

Physical properties

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26
Q

3 experiments that were inconsistent w know physics

A

Black body radiation
Photoelectric effect
Atomic emission spectra

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27
Q

Cycles per second

A

Frequency

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28
Q

Distance between waves

A

Wavelength

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29
Q

Height of the wave crest, depth of the trough

A

Amplitude

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30
Q

High amplitude = — light

A

Bright

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31
Q

— wavelength = longer frequency = — energy

A

Shorter
Higher

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32
Q

— wavelength= shorter frequency = — energy

A

Longer
Lower

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33
Q

Sum of all colors

A

White light

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34
Q

Who said energy is quantized?

A

Planck

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35
Q

Solid object emits visible light when it is heated
First evidence of the quantum theory of energy

A

Black body radiation

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36
Q

UV light will eject electron from metal above threshold frequency
“Light is both a particle and and a wave”- Einstein

A

Photoelectric effect

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37
Q

Bohr model: electrons orbit bc it’s angular momentum is quantized (principal quantum numbers)
Excitation
Relaxation

A

Atomic line spectra

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38
Q

Absorbs energy, low to high level, change in E is positive

A

Excitation

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39
Q

Emits energy, high to low level, Change in E is negative

A

Relaxation

40
Q

E=mc^2
“Length of a wave must fit the circumference of orbit”- deBroglie
Verified by Davisson/ Germer w X-ray electron diffraction of aluminum foil scanning electron microscopy

A

Wave particle duality of matter and energy

41
Q

Matter is discontinuous and particulate, so is energy

A

Quantum theory

42
Q

You cannot know the position and speed of an electron at the same time. You can only know one

A

Heisenberg uncertainty principle

43
Q

shrodinger wave equation

A

Atomic orbital where the electron can/ might be

44
Q

You can never find an electron here (has to do with waves)

A

Node

45
Q

No 2 electrons will ever have the same 4 quantum numbers

A

Pauli exclusion principle

46
Q

Electrons fill up lowest orbitals first

A

Aufbau principle

47
Q

Most stable arrangement of electron in sub shells is parallel spins, not paired electron

A

Hunds rule

48
Q

When unpaired electrons spin the same way, makes it magnetic

A

Paramagnetic

49
Q

All electrons are paired, not magnetic

A

Diamagnetic

50
Q

Outermost shell; largest n value; bonding electrons

A

Valence electrons

51
Q

When Nuclear charge is greater , — is lower

A

Sublevel energy

52
Q

The larger the charger, the — it is to remove an electron

A

Harder

53
Q

Measure of atoms ability to attract bonding electrons

A

Electronegativity

54
Q

Bond between oppositely charged atoms, between a metal and a nonmetal, electrons are given up or taken

A

Ionic bond

55
Q

— give up electrons to achieve noble gas configurations

A

Metals

56
Q

Metals become —

A

Cations

57
Q

Nonmetals become —

A

Anions

58
Q

A bond between two Nonmetals
Polar or non- polar

A

Covalent bond

59
Q

Not equal sharing of electrons (have partial charges)

A

Polar

60
Q

Equal sharing of electrons

A

Nonpolar

61
Q

Cations are — than the original atom

A

Smaller

62
Q

Anions are — than the original atom

A

Larger

63
Q

Subshell energies are caused by —

A

Orbital penetration and it’s effects on shielding

64
Q

The minimum energy required to remove an electron from gaseous atoms in its ground state

A

Ionization energy

65
Q

Energy released when electrons are added
How much an atom wants electrons

A

Electron affinity

66
Q

In relative energy levels, the lower l value is the — energy

A

Lower

67
Q

Balanced chemical equations give —

A

Stoichiometric relationships

68
Q

Ability to do work

A

Energy

69
Q

Atoms of the same element with different numbers of neutrons in the nucleus

A

Isotopes

70
Q

Who came up with the modern periodic table?

A

Mendeleev

71
Q

Wave interference can be — or —

A

Constructive or destructive

72
Q

Interference between a large number of wave sources is called —

A

Diffraction

73
Q

All light has an — and a — component

A

Electric
Magnetic

74
Q

When a solid object emits visible light when it is heated to about 1000K

A

Black body radiation

75
Q

UV light will eject electrons from metal surfaces above a —

A

Threshold frequency

76
Q

How is light emitted?

A

When an electron moves from a high energy level to a lower energy level

77
Q

When an atom absorbs energy, an electron is excited to a — energy orbit

A

Higher

78
Q

The electron then relaxes back to a lower energy orbit, emitting —

A

A photon of light

79
Q

If n initial is greater than n final, a photon is — and the change energy is — than zero

A

Emitted
Less

80
Q

If n final is greater than n initial, a photon is —. Change in energy is — than 0

A

Absorbed
Greater

81
Q

— and — are alternate forms of the same entity

A

Matter
Energy

82
Q

All matter exhibits properties of both — and —

A

Particles
Waves

83
Q

Who said matter behaves as though it moves in a wave

A

DeBroglie

84
Q

Who said particles can be wave-like?

A

Davisson/ Germer

85
Q

Atoms with the same electron configuration

A

Isoelectric

86
Q

— reduces the full nuclear charge to an effective nuclear charge

A

Shielding by other electrons

87
Q

Formula for Z eff

A

Z- shielding constant

88
Q

Electrons in the same level lead to a — Z eff

A

Slightly lower

89
Q

Electrons in an inner level lead to a — Z eff

A

Much lower

90
Q

The nuclear charge that is actually experienced by a valence electron

A

Effective nuclear charge (Z eff)

91
Q

The electrostatic force that holds ions together in an ionic compound

A

Ionic bond

92
Q

Only trend that doesn’t apply to noble gases

A

Electronegativity

93
Q

Energy and wavelength are — related

A

Inversely

94
Q

Determined the charge of the electron

A

Milikans oil drop experiment

95
Q

His theory of the atom included fixed circular orbits for electrons

A

Bohr

96
Q

Showed that the nucleus is a dense region at the center of the atom

A

Rutherford’s gold foil experiment

97
Q

Explained the photoelectric effect in terms of the particle nature of light, photons.

A

Einstein

98
Q

Proposed that energy of a wave is quantized

A

Planck

From Flashcardlet (20 decks)

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