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Chemistry > Chapter 6 > Flashcards

Chapter 6 Flashcards

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1
Q

What is electromagnetic Radiation?

A

a form of energy that has wave characteristics and that propagates through a vauum at the speed of 3.00 X 10^8 m/s

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2
Q

What are the different types of waves?

A

radio waves, infrared radiation, ultraviolet radiation, x-rays

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3
Q

What is the wavelength?

A

the distance between identical points on sucessive waves

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4
Q

What is the frequency of a wave?

A

the number of complete wavelenghts, or cycles, that pass a given point

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5
Q

When wavelenght is long is frequency high or low?

A

low

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6
Q

When wavelenght is short is frequenecy high or low?

A

high

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7
Q

What is the equation to find wavelenght?

A

speed of light/frequency

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8
Q

What is the equation to find frequency?

A

speed of light/ wavelength

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9
Q

Order the different radiations by wavelength(longest to shortes?

A

radio frequency, microwaves, infrared, visible light ,ultraviolet, x-rays, gamma rays

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10
Q

Order the different radiations by frequency(highest to lowest)

A

Gamma rays, x-rays, ultraviolt, infrared, microwaves, radio frequency

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11
Q

Order the visible region by wavelenght(longest to shortes) by color?

A

red, yellow, green, blue, purple

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12
Q

Order the visble light by highest to lowest(freunecy) color?

A

purple, blue, green, yellow, red

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13
Q

What is the unit for frequency?

A

hertz(Hz) or s^-1

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14
Q

How to make nm to m?

A

times it by 10^-9

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15
Q

What is blackbody radiation?

A

the emission of light from hot objects

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16
Q

What is photoelelectric effect?

A

the emission of electrons from metal surfaces on which light shines

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17
Q

What is the emission spectr?

A

the emission of light from electroncially excited gas atoms

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18
Q

What did planck theorize about energy?

A

energy cna be either released or absorbed by atoms only in discrete chuncks of some minumum size

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19
Q

What is quantum?

A

the smallest quanity of energy that can be emitted or absorbed as electromagnetic radiation

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20
Q

How do you find Energy of a phton?

A

E=hv

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21
Q

What is h in the equation E=hv?

A

planck constant(6.626 x 10^-34 J-s)

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22
Q

When frequency increases what happnes to the photon energy and the kinetic energy?

A

photon energy will increase and kinetic energy of the ejected electrrons will increase

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23
Q

What is a photon?

A

the smallest increment of radiant energy

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24
Q

What happens to the emission of electrons when you increase the intensity light source?

A

doesn’t lead to emission of electrons

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25
Q

What happens to the emission of electrons when you increase the frequency of the light?

A

increases the emission of electrons

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26
Q

What happens to the number of photons when the intensity of light is increaseds?

A

number of photons increase but the energy doesn’t

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27
Q

What happenes to the excess energy of the photon?

A

it is converted into kinetic energy of the emitted electron

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28
Q

How to find Energy of a photon in J/mol

A

Times the energy by 6.022 x 10^23

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29
Q

When given the energy of the poton and then the pulse of the photon how do you find what the total energy is?

A

times the two

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30
Q

How do you find the number of photons emitted when given the energy of something and the energy of the photon?

A

enery during pulse/radiaton energy

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31
Q

What is monochromatic?

A

radiation composed of a single wavelenght

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32
Q

What is plychromatic radiation?

A

produces radiation containing many different wavelenghts

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33
Q

When is a spectrum produced?

A

when radiation from a polychromatic source is separated into its componet wavelenghts

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34
Q

What is the continous spectrum?

A

a spectrum that contains radiation distributed over all wavelenghts

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35
Q

What is a line spectrum?

A

a spectrum that contains radiation at only certain specifc wavelenghts

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36
Q

What is the wavelength of violet?

A

410nm

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37
Q

What is the wavelength of blue?

A

434 nm

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38
Q

What is the wavelenght of blue-green?

A

486nm

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39
Q

what is the wavelength of red?

A

656nm

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40
Q

What does rydberg equation allow us to calculate?

A

the wavelenghts of all the spectral lines of hydrogen

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41
Q

What is rydberg equation?

A

1/wavlenght=(RH(1/n1^2 - 1/n2^2

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42
Q

What is Rh in the rydberg equation?

A

rydberg constant which is 1.096776 x 10^7 m^-1)

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43
Q

How does bohr explain why an electron doens’t spiral into hydrogen?

A

only orbits of certain radii, corresponding to certian specific energies, are permitted for the elctron in a hydrogen atom

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44
Q

What an allowed energy state?

A

an electron permitted to obrit

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45
Q

Why does an electron in a allowed energy state doesn’t spiral into the nucleus?

A

does not radiate energy

46
Q

when is an electron emitted or absorbed?

A

as the electron changes from one allowed energy state to another

47
Q

What is the n quantum number?

A

orbits and energy levels

48
Q

How do you find energy of a electron?

A

∆E=(-2.18 x10^-18)(1/nf^2-1/ni^2)

49
Q

What numbers can the n quantum number be?

A

1,2,3,4… has to be a positive interger

50
Q

What happens to the radius as n increases?

A

the radius gets larger

51
Q

What happens to the stability of an atom as the energy increases?

A

becomes less stable teh lower(more negative) the energy the more stable

52
Q

What happens to the energy as n increases?

A

energy increaes

53
Q

What is n=1 called?

A

ground state

54
Q

When n= something higher than 1 what is it called?

A

the excited state

55
Q

How does an electron jump to a higher energy state?

A

the electron must absorb energy

56
Q

What happens to the energy when an electron jumps to a lower energy state?

A

the electron is emitted

57
Q

When ∆E is positive what must a photon do?

A

be abosrbed

58
Q

When ∆E is negative what must a photon do?

A

be emitted

59
Q

How do you find wavelength from Energy of a photon?

A

hc/-∆E

60
Q

How to go from m to nm?

A

times it by 10^9

61
Q

What is the number for the wavelength gamma rays radiation?

A

10^-11

62
Q

What is the number for the wavelength of the x-rays radiation?

A

10^-9

63
Q

What is the number for the wavelength of the ultraviolet radiation?

A

10^-7

64
Q

What is the number for wavelength of infrared rays?

A

10^-5

65
Q

What is the number for the wavelenght for the visible light radiation?

A

10^-4

66
Q

What is the number for the wavlenght of the microwaves radaition?

A

10^-3

67
Q

What is the number for the wavelenght of the radio radaiton?

A

10^1 and bigger

68
Q

What did De Broglie suggest about an electron moving about the nucleus?

A

it behaves like a wave and therefore has a wavlenght

69
Q

How do you find wavelength for an electron?

A

wavlenght= h/mv

70
Q

What is v in de broglie equation?

A

velocity

71
Q

What did de broglie equation apply to?

A

to all matter, any object of mass and velocity

72
Q

How to go from pico meters to nano meters?

A

times it by 10^-3

73
Q

What did heisenberg discover?

A

uncertainty princple?

74
Q

What is the uncertainty princple?

A

it is impossible for us to know both the exact momentum of an electron and its exact location in space

75
Q

What are wave functions?

A

a description of an allowed energy state for an electron in the quantum mechanical model of the atom

76
Q

What is the electron density?

A

the proabibilty of finding an electron at any particular poting in an atom

77
Q

As density increases what happens to the probability of find the electron?

A

increases

78
Q

As density decreases what happens to teh proabability of finding an electron?

A

decreases

79
Q

What are orbitals?

A

an allowed energy state of an electron in the quantum mechancial model of the atom

80
Q

What is the shape of the lowest energy orbital?

A

a spherical shape

81
Q

What are the three quantum number in the quantum mechanical model?

A

n, l, ml

82
Q

What is the l quantum number called?

A

angular momentum quantum number

83
Q

How do you find the l quantum number?

A

values from 0 (n-1)

84
Q

When l is 0 what letter do you use?

A

s

85
Q

When l is 1 what letter do you use?

A

p

86
Q

When l is 2 what letter do you use?

A

d

87
Q

When l is 3 what letter do you use?

A

f

88
Q

How do you find the ml value?

A

-l and l including zero

89
Q

What is the ml quantum number called?

A

magnetic quantum number

90
Q

What is an electron shell?

A

a collection of orbitals that have the same value of n

91
Q

What are subsells?

A

orbitals that have the same n and l value

92
Q

What does s orbitals look like?

A

spheres

93
Q

What happens to the peaks of the s orbitals as n increases?

A

gets larger and larger

94
Q

For an ns orbtial how do you find the number of peaks?

A

peaks= the n value

95
Q

How do you find the number of nodes for a s orbital?

A

nodes= n-1

96
Q

For an s orbital what happens to the probablity of finding the electron as n increases?

A

probabaility increases

97
Q

What kind of shape is the p orbital?

A

dumbell(two lobes0

98
Q

How do you find the number of nodes for a p orbital?

A

nodes= l value

99
Q

How do the p orbitals differ?

A

The ml number causes them to change what nodal plane they are on

100
Q

What happens to the size of the orbital in the p orbitals as n increases?

A

size increases

101
Q

What happens to the size of an orbital as n increases in the d orbitals?

A

size increases

102
Q

What do the d orbitals look like?

A

four leaf clovers(four lobes)

103
Q

How does the d orbitals change?

A

As the ml value changes it changes where the nodal plane is

104
Q

What happens to the energy of an orbital as l increases?

A

increases

105
Q

What are orbitals with the same energy called?

A

degenerate

106
Q

What is an electron spin?

A

a propert of the electron that makes it behave as though it were a tiny magnet

107
Q

What is the spin magnetic quantum numer?

A

associated with the electron spin

108
Q

What are the two values for the ms quantum number?

A

+1/2, -1/2

109
Q

What is the pauli exclusion principle?

A

no two electrons in an atom may have the same four quantum numbers(n,l,ml,and ms) can be no more than two electrons in any one atomic orbital

110
Q

What is hund’s rule?

A

when filling degenarte orbtials, the lowest energy is attained when the number of electrons have the same spin

Chemistry (13 decks)

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