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PB Chemistry > The Electron and Exam Review > Flashcards

The Electron and Exam Review Flashcards

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1
Q

Light is made of…

A

Photons.

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2
Q

What are photons?

A

Tiny bundles of energy.

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3
Q

Light travels at…

A

The speed of light.

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4
Q

What is the speed of light?

A

3.00 x 10^8 m/s

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5
Q

What variable is used to represent the constant speed of light?

A

c

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6
Q

Light can be described as these two things:

A

Particles and waves.

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7
Q

What is the crest of a wave?

A

The highest point or the peak of the wave.

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8
Q

What is the trough of a wave?

A

The lowest point of the wave.

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9
Q

What is the wavelength?

A

How long the wave is.

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10
Q

Wavelength is measured in three ways:

A

Trough to trough, crest to crest, or node to node.

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11
Q

What is frequency?

A

The number of waves per second.

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12
Q

What are the units for wavelength?

A

Meters or nanometers.

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13
Q

How do you calculate speed?

A

Speed=distance/time

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14
Q

What is the unit for frequency?

A

Hertz (Hz) and 1/s.

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15
Q

If speed=distance/time, c=…

A

c = m x (1/s) = m/s

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16
Q

What is the relationship between wavelength and frequency?

A

Shorter wavelength=higher frequency. Longer wavelength=lower frequency.

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17
Q

How do you calculate wavelength?

A

Wavelength=c/f

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18
Q

How do you calculate frequency?

A

Frequency=c/wavelength

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19
Q

Negatively charged ions are called

A

Anions

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20
Q

Positively charged ions are called

A

Cations

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21
Q

In order from longest to shortest wavelength, list 7 types of electromagnetic radiation.

A

Radio waves, microwaves, infrared, visible light, ultraviolet light, x-rays, gamma rays.

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22
Q

Which color of visible light has the longest wavelength and lowest frequency?

A

Red.

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23
Q

Which color of visible light has the shortest wavelength and highest frequency?

A

Violet.

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24
Q

Who discovered the atomic nucleus through the gold-foil experiment?

A

Rutherford.

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25
Q

Rutherford also discovered that the nucleus contains…

A

All of the atom’s mass.

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26
Q

Rutherford found out that electrons orbit…

A

Outside, in the electron cloud.

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27
Q

What was the Bohr model also called?

A

The planetary model.

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28
Q

Bohr’s model was based on what three ideas?

A
  1. Electrons move outside the nucleus in specific energy levels
  2. Electrons are attracted to the nucleus (opposite charges attract)
  3. Electrons repel one another (like charges repel)
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29
Q

What letter is used to represent energy level?

A

n

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30
Q

Energy level can also be defined as…

A

The distance from the nucleus.

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31
Q

n=1 can hold how many electrons?

A

2

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32
Q

n=2 can hold how many electrons?

A

8

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33
Q

n=3 can hold how many electrons?

A

18

34
Q

n=4 can hold how many electrons?

A

32

35
Q

n=5 can hold how many electrons?

A

50

36
Q

The electrons are in the___energy levels, filling the levels___to the nucleus. This is called the___.

A

The electrons are in the lowest possible energy levels, filling the levels closest to the nucleus. This is called the ground state.

37
Q

What happens when an atom absorbs energy in the form of radiation, electricity, or heat?

A

The electrons can jump to an excited state, or higher energy levels.

38
Q

Can an atom remain in the excited state?

A

No.

39
Q

What happens since an atom cannot remain in the excited state?

A

The electrons fall back down to lower energy levels (ground state) and emit energy in the form of photons-light.

40
Q

Electron transitions between energy levels are connected to…

A

A specific frequency.

41
Q

Each frequency has a corresponding…

A

Wavelength.

42
Q

Each color or radiation type is identified by…

A

Its wavelength or frequency.

43
Q

Radio station Z107.7 broadcasts radiowaves. What do the numbers 107.7 represent?

A

The frequency of the waves in megahertz.

44
Q

What does c equal?

A

c=3.00 x 10^8 m/s

45
Q

What does h represent?

A

Planck’s constant.

46
Q

What is Planck’s constant?

A

6.63 x 10^-34 J x s

47
Q

What is the equation for energy?

A

E=hf

48
Q

How do you calculate the number of electrons per energy level?

A

2n^2. (n represents the energy level.)

49
Q

Nanometers to meters

A

1 nm= 1 x 10^-9 m or 1 m= 1 x 10^9 nm

50
Q

Megahertz to hertz

A

1 MHz= 1 x 10^6 Hz or 1 Hz= 1 x 10^-6 Hz

51
Q

Bohr’s planetary model worked well for hydrogen and helium, but it did not work well for…

A

Heavier elements.

52
Q

What did DeBroglie reason?

A

DeBroglie reasoned that if light, which seems like waves, could be treated as a particle, then electrons, which seem like particles, could be treated as waves.

53
Q

What did Schrodinger do?

A

Schrodinger developed Schrodinger Wave Equations, to describe the wavelike properties of electrons.

54
Q

What do Schrodinger Wave Equations describe?

A

The most probable location of the electron.

55
Q

If you have a 2 cation of calcium, what has happened to it?

A

It has a charge of 2+ because it lost 2 electrons.

56
Q

If you have a 2 anion of calcium, what has happened to it?

A

It has a charge of 2- because it gained 2 electrons.

57
Q

Which scientist reasoned that electrons reside in rings that get larger as you move away from the nucleus?

A

Bohr.

58
Q

Who explained that the world is made of empty space tiny, indivisible particles called “atomos?”

A

Democritus.

59
Q

Who conducted the gold-foil experiment, and what did that determine?

A

Rutherford; it determined that an atom is made of mostly empty space with a positively charged, dense central force.

60
Q

What is the nucleus like in Bohr’s atomic model?

A

Positively charged and dense.

61
Q

Is it possible to specify the exact location of an electron at a particular instant?

A

No.

62
Q

How are energy and region of an electron related?

A

Energy of an electron is inversely related to the volume of the region to which it is confined.

63
Q

The symbol for “principal” or “energy level” is…Principal is defined as…

A

Symbol=n, definition: distance electron is from nucleus.

64
Q

Symbol for sublevel:

Definition of sublevel:

A

Symbol: cursive lowercase “l”
Definition: shape of a region of the energy level

65
Q

Symbol for orbital:

Definition of orbital:

A

Symbol: M with subscript cursive lowercase “l”
Definition: 3D orientation of sublevel in space.

66
Q

Symbol for spin:

Definition of spin:

A

Symbol: M with subscript lowercase “s”
Definition: The spin of an electron (counter-clockwise or clockwise)

67
Q

Two rules for filling electron orbitals:

A
  1. Lowest energy level fills first (Aufbau principle)

2. No two electrons can have the same set of quantum numbers (Pauli exclusion principle)

68
Q

What do quantum numbers describe?

A

The distribution of the electrons.

69
Q

How many electrons can each orbital hold?

A

2 maximum.

70
Q

What letters represent the sublevels?

A

s, p, d, f

71
Q

How many orbitals are in each sublevel?

A

s=1 orbital. p=3 orbitals. d=5 orbitals. f=7 orbitals.

72
Q

How many electrons can fit in each sublevel?

A

s= up to 2 electrons. p= up to 6 electrons. d= up to 10 electrons. f= up to 14 electrons.

73
Q

What was Democritus’ contribution?

A

He said that reality is made of atoms and empty space. Atoms are indivisible particles.

74
Q

What was Dalton’s contribution?

A

He came up with the first atomic theory with five main points.

75
Q

What was J.J. Thomson’s contribution?

A

He discovered the negatively-charged electron through the cathode ray tube experiment and developed the plum pudding model.

76
Q

What was Robert Milikan’s contribution?

A

He discovered the charge and charge-to-mass ratio of the electron through the oil drop experiment.

77
Q

What was Ernest Rutherford’s contribution?

A

He discovered the atomic nucleus and that it is made of protons and neutrons, is dense (contains almost all of atom’s mass), and has a positive charge through the gold foil experiment. He also said that electrons occupy most of the atom’s volume. He created a model known as the nuclear model.

78
Q

What was Neils Bohr’s contribution?

A

He developed the Bohr model, AKA planetary model, in which electrons orbit the nucleus at fixed distances (energy levels).

79
Q

What was Dalton’s Atomic Theory?

A
  1. All matter is made of atoms.
  2. Atoms from the same element are identical; atoms from different elements differ in size, mass, etc.
  3. Atoms cannot be created, destroyed, or subdivided.
  4. Compounds form when atoms of different elements combine in whole-number ratios.
  5. In chemical reactions, atoms are separated, combined, or rearranged.
80
Q

What are the three changes that modern atomic theory made to Dalton’s atomic theory?

A

Atoms can be subdivided, atoms can be created or destroyed by changing them into different atoms using nuclear fission, and atoms from the same element are not necessarily identical due to isotopes and ions.

81
Q

On the periodic table, what are groups?

A

Vertical columns of elements that have like properties and characteristics because they have the same number of valence electrons.

82
Q

On teh periodic table, what are periods?

A

Horizontal rows of elements that have the same number of energy levels/electron shells.

PB Chemistry (9 decks)

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