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Chemistry 11 > Chapter 5: A Closer Look at Matter > Flashcards

Chapter 5: A Closer Look at Matter Flashcards

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1
Q

why is hydrogen so different from other elements?

A

it has only one electron so there is no electron interation within the atom

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2
Q

which subshell is this?

A

p

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3
Q

which subshell is this?

A

s

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4
Q

in the late 17th century, who proposed that elements were any material that a single substance that could not be broken down anymore

A

Robert Boyle

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5
Q

what do you call the magnetic orientation of an electron?

A

it’s magnetic moment

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6
Q

what could Thomson conclude about the cathode particles and hydrogen ions?

A

that they have the same charge and the cathode particles are significantly smaller than H+

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7
Q

if orbitals have the same angular momentum quantum number, they are in the same ______?

A

subshell

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8
Q

once the air from the Crookes tube was vacuumed out, what happened?

A

the pink glow faded and the opposite cathode was glowing a vibrant green

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9
Q

who came up with the plum-pudding model

A

Thomson

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10
Q

what are the two possible values that ms can hold?

A

ms = -1/2 and ms = 1/2

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11
Q

whose mathematical equation describing frequencies given off by a black body at a given temperature did not work at high temps?

A

Lord Rayleigh and Sir James Jeans

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12
Q

who proved Einstein’s theory of light behaving like a particle?

A

Robert Millikan

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13
Q

in a system with a fixed distance, what will happen to the frequency?

A

the frequency will change to keep the distance fixed

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14
Q

Thomson discovered the cathode ray was always deflected towards the ______ plate

A

positive

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15
Q

Who thought to think of energy as a particle, rather than as a wave?

A

Planck

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16
Q

def: the number of neutrons in a nucleus (N)

A

neutron number

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17
Q

what is the frequency below which the light no longer generates an electric current called?

A

a threshold frequency

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18
Q

who predicted the neutron?

A

Rutherford

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19
Q

def: a quantum number that descirbes an electron’s magnetic orientation, created as a result of being a moving charge

A

spin quantim number (ms)

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20
Q

def: a visual representaiton of an atom’s electron configuration using: boxes or lines for the atomic orbitals, arrows for the electrons and the arrow direction indidcation the spin

A

orbital diagram

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21
Q

def: a notation that identifies the organization of electrons in an atom, indication the sehll they’re in, the subshell they’re in and how many in that subshell

A

electron configuration

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22
Q

def: whole number representing the number of protons, the charge of an atom or ion and the number of electrons in a neutral atom (Z)

A

atomic number

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23
Q

what are the two types of waves?

A

travelling waves and standing waves

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24
Q

def: a device that separates light into its component wavelengths, allowing the measurement of those wavelenghts

A

spectroscope

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25
Q

what does AZE notation include?

A

atomic number, mass number and element

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26
Q

who discovered the neutron?

A

James Chadwick

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27
Q

what did aristotle propose about matter?

A

that it’s made of earth, water, air and fire

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28
Q

def: a unique pattern of spectral line given off by each element, representing specific frequencies and wavelengths, and therefore specific energies

A

bright-line spectrum

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29
Q

who discovered that every element has a different bright-line spectrum?

A

Niels Bohr

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30
Q

if light is a particle, and quanta are made of particles, increasing the light’s intensity is equivalent to producing ________

A

more quanta

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31
Q

def: refers to neurtal atoms and charged ions who have the same number of electrons occupying the same orbitals, giving them the same electron configuration

A

isoelectronic

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32
Q

def: a 3D representation of the square of an electron’s wave function, representing where in space around the nucleus we have the highest probability of finding that electron

A

atomic orbital

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33
Q

applying a high voltage across the electrodes in a Crookes tube cause what to happen?

A

the air inside the tube glowed pink

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34
Q

what are the two ways you can change a wave system?

A
  • fixed distance and a variable wavelength - fixes wavelength and a variable distance
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35
Q

is light a wave or a particle?

A

both

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36
Q

what are the key points of Bohr’s atomic model for hydrogen?

A
  1. the hydrogen atoms has a specific allowed energy levels or stationary states 2. as long as electrons are in the allowed energy levels, they do not give off or absorb energy 3. electrons can only move between the allowed energy levels if they absorb or give off the amount of energy needed to go between levels
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37
Q

what did Werner Heisenberg say about subatomic particles?

A

that you can know their position or momentum but not both

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38
Q

how did Thomson modify the Crooke’s tube?

A
  1. employed a better vacuum pump 2. modified the anode, creating a focused cathode ray 3. coated the inside of the glass with phosphorescent compound that lit up when cathode rays struck it 4. added a pair of metal plates between the anode and the end of the tube, creating a controllable electric field
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39
Q

how did Schrödinger treat electrons? waves or particles?

A

waves

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40
Q

T or F: electrons can’t hold the same ms number

A

True, only one spin up and one spin down

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41
Q

def: in the same atom, no two electrons can have the same combination of four quantum numbers, n, ℓ, ml, and ms

A

Pauli exclusion principle

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42
Q

Thomson believed the Crookes tube contained _________, not letting scientists observe any interactions

A

residual air

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43
Q

the bigger the n value…?

A

the bigger the orbital, more energy, larger distance from nucleus

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44
Q

def: when multiple orbitals of equal energy are available in a subshell, electrons will fill the orbital’s individually before pairing up

A

Hund’s rule

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45
Q

which subshells are these?

A

f

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46
Q

def: a quantum number that determines an orbital’s shape for which we use a corresponding letter to distinguish it form the principal quantum number

A

angular momentum quantum number (𝓁)

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47
Q

can an element be its own core?

A

no

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48
Q

J.J. Thomson believed that an _______ would cause the cathode rays to be deflected

A

electric field

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49
Q

scientist understood that cathode rays are made up of _________

A

charged particles

50
Q

what range of values can 𝓁 have?

A

𝓁 = 0 to 𝓁 = n-1

51
Q

def: the concept that quantized entities and elementary particles, like light and electrons, display both wave and particle natures, requiring both to properly describe them

A

wave-particle duality

52
Q

def: the set of orbitals of the same type, each having the same angular momentum quantum number

A

electron subshell

53
Q

what does the energy of a given quantum depend on ?

A

the oscillators’ speed, the faster the oscillator the more likely to vibrate

54
Q

def: gas-discharge tube that has two electrode, a negative cathode at on end and a positive anode about halfway down, and a flat cross about two thirds of the way along

A

Crookes tube

55
Q

the only way an electron can carry a charge and have a mass is if it’s a _______

A

particle

56
Q

what is the difference between the mass number and the atomic mass?

A

atomic mass is the average of all element’s atoms while mass number describes the composition of a specific atom

57
Q

T or F: Electrons occupy the specific orbits around the nucleus allow them to form circular standing waves

A

True

58
Q

who named beta decay and gamma decay?

A

Rutherford

59
Q

T or F: using math, we can tell exactly where electrons will be and what momentum they’ll have

A

False, we can only know where they are likely to be and how they’re likely to be moving

60
Q

how did the charge-to-mass ratio that Thomson found compare to that of a hydrogen ion

A

it was 2000 times bigger

61
Q

orbitals with the same “n” number are called _______

A

shells

62
Q

what are the first four subshells?

A

s, p, d, f

63
Q

T or F: electrons can hold the same n, ℓ and ml numbers

A

True

64
Q

what were two points of Rutherford’s atomic model?

A
  1. the nucleus represented most of the atom’s mass, but little volume 2. the electrons outside the nucleus represented most of the atom’s volume but very little mass
65
Q

def: a whole number representing the sum of the number of protons and neutrons in the nucleus (A)

A

mass number

66
Q

which student of Rutherford believed that the atom had a positively charged nucleus?

A

Niels Bohr

67
Q

what were some of Bohr’s points on energy levels and stationary states?

A
  • each energy level is a circular orbit - the further the orbit from the nucleus, the higher the energy - each level has a quantum number, whole number starting at 1 - lowest energy level orbit is the ground state - larger orbits of higher energy are excited states
68
Q

what offers the best evidence for light as a wave?

A

diffraction

69
Q

how can you find the neutron number?

A

neutron number = mass number - atomic number

70
Q

def: mysterious agent causing a green glow in the Crookes tube

A

cathode ray

71
Q

with the concept of quanta, what was Planck doing to energy?

A

he was quantizing it

72
Q

Scientists knew that energy _______________ then _____________

A

increased to a maximum then decreased as frequency continued to increase

73
Q

law of classical physics would lead to the electrons __________

A

losing energy and rapidly spiralling inwards toward the nucleus. making unstable atoms

74
Q

who legitimized Planck’s Postulate?

A

Albert Einstein

75
Q

T or F: low frequency light, no matter it’s intensity does not generate an electric current

A

True

76
Q

T or F: quanta are divisible

A

False, you can only have whole quanta

77
Q

what did De Broglie’s equation say about particle wavelength?

A

that wavelength is inversely proportional to the particle’s mass and velocity

78
Q

who proposed the proton?

A

Rutherford

79
Q

T or F: electrons can only take two possible orientations

A

True

80
Q

what did Planck call the bundles of energy her proposed?

A

quanta

81
Q

what was the name of the disagreement between classical prediction and experimental observation concerning radiation?

A

the ultraviolet catastrophe

82
Q

def: electrons tend to full to maximum any orbitals in the lowest available subshell first, before filling a higher-energy orbital

A

Aufbau principle

83
Q

T or F: 𝓁 is dependent on n

A

True

84
Q

def: an experiment involving an alpha particle source, fluorescent screen and gold foil?

A

Rutherford gold foil experiments

85
Q

what did aristotle’s idea of matter lead to?

A

alchemy

86
Q

what two predictions in Rutherford’s atomic model were proven false?

A
  1. matter should be unstable 2. light given off by atoms should be a continuous spectrum
87
Q

who discovered alpha decay?

A

Rutherford

88
Q

how did Heisenberg treat electrons? waves or particles?

A

particles

89
Q

by comparing similar measurements using a magnetic field, Thomson was able to determine the ______ of the cathode-ray particles

A

charge-to-mass ratio

90
Q

in a system with a variable distance, what will happen to the frequency?

A

the frequency will stay the same as the distance changes

91
Q

what did democritus call the small indivisible particles of matter?

A

atomos means indivisible

92
Q

what happened to alpha particles when Rutherford shot them at gold foil?

A

they were deflected

93
Q

def: the more precisely you know a particle’s position, the less precisely you can know it’s momentum, and vice versa

A

Heisenberg’s uncertainty principle

94
Q

def: a shotened electron configuration that simplifies the reporting of inner core electrons while fully reporting valence electrons

A

core notation

95
Q

how do we represent the core electrons in core notation?

A

using the symbol of the noble gas from the previous row

96
Q

def: an elementary particle, whose substructure is unknown, representing a quantum electromagnetic radiation

A

photon

97
Q

the principal quantum number refers to the ______

A

electron shell

98
Q

def: the set of all the orbitals described by the same principal quantum number

A

electron shell

99
Q

T or F: in a hydrogen atom, all the orbiatals have different amounts of energy

A

False, in hydrogen atoms, all orbitals have the same amount of energy

100
Q

what were the 4 main points of dalton’s atomic theory?

A
  1. all matter is composed of tiny particles, which can’t be broken down, created or destroyed 2. atoms of a given element are identical to each other, but different from other elements 3. atoms if different elements combine in specific ratios to form compounds 4. in a chemical reaction, atoms separate or rearrange to form new compounds
101
Q

“Cathode rays are made up of streams of ________ charged particles who are ______ in size.”

A

negatively subatomic

102
Q

Bohr’s model accurately explained and predicted _______________ and was lacking ________

A

most of hydrogens bright line spectrum, but not all of it and was lacking theoretical basis

103
Q

def: Bohr’s original quantum number, indicating the orbital’s size and energy relative to other orbitals, and it’s distance from the nucleus

A

principal quantum number (n)

104
Q

what did Bohr call the distances in which the electrons orbited the nucleus?

A

stationary orbits

105
Q

what is the equation for 𝓁

A

𝓁 = n-1

106
Q

def: the study of energy given off by hot objects

A

black-body radiation

107
Q

a high frequency quantum has lots of energy, but in an actual system, _________

A

is less likely to exist

108
Q

T or F: Bohr thought electrons emitted electromagnetic waves

A

False

109
Q

Bohr’s theory behind his math could not explain why some lines on the spectrum where _____ than others

A

brighter

110
Q

T or F: ml is related to 𝓁?

A

True

111
Q

In 1897, J.J Thomson set about characterizing ________

A

cathode rays

112
Q

how many electrons can one orbital hold?

A

two electrons

1 spin up, 1 spin down

113
Q

what did the ancient greeks propose about matter?

A

that solid matter could be cut into smaller and smaller pieces until there was a piece that you could no longer cut up. there is also empty space between matter, in different proportions

114
Q

what range of values can ml have?

A

values ranging from -𝓁 to 𝓁, including 0

115
Q

Thomson could conclude what about cathode rays?

A

that they are made up of streams of negatively charged particles

116
Q

which subshells are these?

A

d

117
Q

who proposed the nucleus?

A

Rutherford

118
Q

def: atoms of a given element that have the same atomic number but different neutron numbers and therefore different mass numbers

A

isotopes

119
Q

T or F: the energy levels in hydrogen atoms are simple

A

True

120
Q

who provided the theoretical foundation that was missing in Bohr’s model?

A

de Broglie

121
Q

def: a quantum number that describes an orbital’s orientation in space, leading to a specific number of orbital’s in each subshell

A

magnetic quantum number (ml)

Chemistry 11 (6 decks)

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