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Marine Chemistry > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

wave motion

A

frequency and wavelength

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2
Q

wavelength

A
  • the distances between corresponding points on a wave
  • Units: meters/nanometers
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3
Q

frequency

A
  • the number of waves that pass a given point in a specific time
  • Units: Hz or 1/s
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4
Q

relation of wavelength and frequency

A

inversely proportional

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5
Q

relation of wavelength and energy

A

inversely proportional

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6
Q

relation of frequency and energy

A

directly proportional

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7
Q

electromagnetic radiation

A

form of energy that exhibits wavelength behavior as it travels through space

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8
Q

electromagnetic spectrum

A

all forms of electromagnetic radiation combined

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9
Q

constant velocity

A

what all types of electromagnetic radiation travel at

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10
Q

speed of light(c)

A

3.00 x 10^8 m/s

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11
Q

formula for speed of light

A

c = wavelength x frequency

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12
Q

formula for energy (using frequency)

A

E = planks constant x frequency

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13
Q

formula for energy (NOT using frequency)

A

E = (Plancks x speed of light) / wavelength

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14
Q

electromagnetic spectrum in order from least to most energy

A

Radio
Microwave
Infared
Visible
Ultraviolet
X-ray
Gamma Ray

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15
Q

Visible light travels at what speed

A

speed of light(c)

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16
Q

Photoelectric effect

A
  • shine light at different metals and they emit electricity
  • electricity is only emitted when the frequency of light is high enough
  • Light is acting like a particle
  • Max Planck came up with it
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17
Q

Who came up with the dual-wave particle theory

A

Albert Einstein

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18
Q

why were scientists surprised from the photoelectric effect?

A

They expected that eventually you could shine lower frequency light long enough that enough energy would accumulate but you can’t

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19
Q

quanta

A

small amounts of energy

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20
Q

photon

A

a particle of electromagnetic radiation that has zero mass and carries a quantum of energy

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21
Q

planks constant

A

6.626 x 10^-34 Joules

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22
Q

frequency units

A

Hz or 1/s

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23
Q

energy unit

A

Joules or J

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24
Q

ground state

A

the lowest energy state of an atom

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25
Q

excited state

A

the higher energy when atoms gain energy, and have a higher potential energy than the ground state

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26
Q

when an excited atom returns to the ground state, it gives off energy in the form of…

A

electromagnetic radiation

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27
Q

line-emission spectrum

A

the bands of light that are visible

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28
Q

how are atoms like a fingerprint?

A

excited atoms exhibit a specific portion of the visible spectrum; unique.

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29
Q

Why do we see distinct colors or different elements?

A

There are different amounts of energy that is released depending on the frequency

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30
Q

what does Niels Bohr suggest about electrons?

A
  • electrons could circle the nucleus in a fixed path
  • electrons could move up and down to higher or lower orbits
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31
Q

absorption

A

photon is absorbed
electron is emitted

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32
Q

emission

A

photon is emitted
electron is absorbed

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33
Q

what has to happen for an electron to “jump” from the ground state to an excited state?

A

Absorption of energy leads to photon getting excited and released a proton

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34
Q

1 meter = ? nanometers

A

1 x 10^-9 nm

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35
Q

1 kJ = ? J

A

1000 J

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36
Q

quanta = (Planck constant)(frequency)

A

TRUE

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37
Q

According to Bohrs model of the atom, which particles are allowed to exist in any one of a number of energy levels?

A

Electrons

38
Q

The line-emission spectrum of an atom is caused by the energies released when electrons…

A

“jump” from a higher energy level to a lower energy level

39
Q

because excited hydrogen atoms always produced the same line-emission spectrum, scientists concluded that hydrogen…

A

releases energy of only certain values

40
Q

color of light from longest to shortest wavelength

A

Red
Orange
Yellow
Green
Blue
Purple

41
Q

When light is envisioned as a particle, it is called what?

A

a photon

42
Q

In the equation E = hf, what does h represent

A

Planck’s constant

43
Q

What form of energy exhibits wave behavior as it travels through space

A

all types of electromagnetic radiation

44
Q

the photoelectric effect is when…

A

light is shone at a substance and the element emits electrons

45
Q

In the Bohr model of the atom, in which orbit is an electron in its lowest energy level?

A

the orbit closest to the nucleus

46
Q

wave theory of The atom was created by who?

A

de Broglie and
Schrodinger

47
Q

Wave theory of an atom

A
  • described electrons as particles that behave like waves
  • knew electrons had a certain amount of energy and NOTHING in between
    *still didn’t explain everything
48
Q

quantum theory of an atom

A

describes mathematically the LIKELY behavior of electrons

Uses the 4 quantum numbers to describe them in their MOST LIKELY location in an atom

49
Q

Heisenberg uncertainty principle

A

you can’t know the exact position of an electron at the same time as the velocity of an electron

50
Q

velocity

A

speed and direction

51
Q

the exact position and motion of an electron is…

A

unknowable

52
Q

you can only describe the probable places to find electrons using:

A

orbitals

53
Q

orbital

A

a 3D region around the nucleus where an electron will likely be

54
Q

what is the name of the first quantum number?

A

Principle quantum number

55
Q

Principle Quantum number

A
  • Abbreviation: n
  • Tells us the energy level the electrons are
56
Q

what is the highest energy level they go up to?

A

7 energy levels

57
Q

As n increases:

A

electrons energy and average distance from nucleus increase too

58
Q

what is the name of the second quantum number?

A

Angular momentum quantum number

59
Q

Angular momentum quantum number

A
  • Abbreviation: l
  • Tells us the sub level the electron is in within the energy levels
60
Q

are sub levels equal in size?

A

NO

61
Q

What number do sublevels start at?

A

0
Go up by 1

62
Q

1st sub level = ?

A

0

63
Q

Sublevel 1 = ?

A

p or 2nd sublevel

64
Q

what 2 things does the 2nd quantum number tell us?

A
  • shape of orbital
  • sublevel it is in
65
Q

what is the name of the 3rd quantum number?

A

Magnetic quantum number

66
Q

Magnetic quantum number

A
  • Abbreviation: m
  • Tells us the designation for which specific orbital within the sublevel
    *Tells us the the orientation of orbital around the nucleus
67
Q

what are orbitals labeled as?

A

(- l … + l )

68
Q

p sublevel has how many orbitals?

A

3 orbitals

69
Q

d sublevel has how many orbitals?

A

5 orbitals

70
Q

s sublevel has how many orbitals?

A

1 orbital

71
Q

possible orbitals (m values) equation:

A

2l + 1

72
Q

what is the name of the 4th quantum number?

A

Spin Quantum Number

73
Q

Spin Quantum Number

A
  • Abbreviation: s
  • Tells us the one of two possible spin states
74
Q

what are the two possible spin states?

A

+ 1/2
- 1/2

75
Q

if the electron is spinning in a positive direction, does it mean it has a positive charge?

A

NO

76
Q

electron configuration

A

electrons will fill up rows various spots in the atom from least to most energy

77
Q

ground state configuration

A

natural state at lowest energy

78
Q

valence electrons

A

outermost electrons in the highest energy levels

79
Q

orbital filling notation

A
  • based on energy of orbitals, filling the lowest first
  • every orbital is designated with a horizontal line
  • arrows on top are electrons pointing up and down
80
Q

electron configuration notation

A

shortened notation
all sublevel superscripts should be full UNLESS its the last one

81
Q

noble gases

A

the gaseous elements on the periodic table that have full outer electron shells

82
Q

noble gases are what orbitals?

A

s and p

83
Q

noble gases DO NOT react with other elements to form compounds

A

TRUE

84
Q

what are the noble gases

A

Helium
Neon
Argon
Krypton
Xenon
Radon

85
Q

aufbrau principle

A

lowest energy orbitals will be first filled

86
Q

Hunds rule

A
  • when orbitals of identical energy are available, electrons enter these orbitals singly before a second electron will fill each orbital
  • orbitals in the same sublevel are degenerate
87
Q

degenerate

A

have identical energy

88
Q

Pauli Exclusion Principle

A
  • orbitals can only contain a maximum of two electrons and when two electrons enter the same orbital they must have opposite spins so that each electron has a unique set of quantum numbers.
89
Q

how many electrons are in each orbital?

A

2 electrons

90
Q

Why do we see colored lights during the flame test experiment?

A
  • The flame adds energy to the electrons
  • They get excited and jump to higher energy levels
  • Then, they get pulled back towards the nucleus and the extra energy gets emitted as light.

Marine Chemistry (11 decks)

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