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AP Chemistry > Chapter 7 > Flashcards

Chapter 7 Flashcards

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1
Q

Wavelength

A

distance between two consecutive peaks or troughs in a wave

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2
Q

Symbol for wavelength

A

λ

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3
Q

Frequency

A

number of waves that pass a given point per second

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4
Q

Energy is _______ and can occur only in discrete units of size called _______

A

quantized, hv

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5
Q

discrete units of size

A

hv

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6
Q

quantum

A

the smallest amount of energy

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7
Q

electrons can be viewed as a stream of “particles” called?

A

photons

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8
Q

phenomenon in which electrons are emitted from the surface of a metal when light strikes it

A

photoelectric effect

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9
Q

when are electrons emitted from the surface of a metal?

A

when light strikes it

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10
Q

when electromagnetic radiation exhibits wave properties and particulate properties is a phenomenon called?

A

dual nature of light

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11
Q

diffraction

A

when light is scattered from a regular array of points or lines

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12
Q

diffraction pattern

A

bright spots and dark areas on a photographic plate

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13
Q

when does a diffraction pattern occur?

A

scattered light interfere constructively to produce a bright area or destructively to produce a dark area.

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14
Q

interfere constructively

A

the peaks and troughs are in phase

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15
Q

interfere destructively

A

the peaks and troughs are out of phase

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16
Q

continuous spectrum results when?

A

white light is passed through a prism.

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17
Q

the energy of the electron is?

A

quantized

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17
Q

quantized

A

to subdivide energy into very small but measurable increments

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18
Q

what is significant of the line spectrum of hydrogen?

A

indicates only certain energies are allowed for the electron

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19
Q

what is the quantum model?

A

the electron in a hydrogen atom moves around the nucleus only in certain allowed circular orbitals

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20
Q

A hydrogen atom in its lowest possible energy state is called?

A

ground state

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21
Q

the electron bound to the nucleus is similar to?

A

standing wave

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22
Q

orbital

A

a specific wave function

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23
Q

Heisenberg uncertainty principle

A

there is a limitation to just how precisely we know the position and momentum of a particle at any time.

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24
Q

Probability distribution

A

the probability of finding the electron at points along a line drawn outwards from the nucleus.

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25
Q

frequency symbol

A

v

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26
Q

why do we see visible light?

A

the chemical reaction that takes place within our retina

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27
Q

how does all types of electromagnetic radiation travel?

A

at the speed of light

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28
Q

short waves have a ____ frequency

A

high

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29
Q

what is wavelength measured in?

A

meters

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30
Q

what is frequency measured in?

A

Hz (hertz)

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31
Q

symbol for speed?

A

c

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32
Q

symbol for planck’s constant?

A

h

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33
Q

long wavelengths have _____ frequencies.

A

low

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34
Q

Max Planck postulated what?

A

energy can be gained or lost only in whole number multiples of the quantity hz

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35
Q

a system can transfer energy only in?

A

whole quanta

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36
Q

Einstein proposed that electromagnetic radiation is itself?

A

quantized

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37
Q

electromagnetic radiation

A

stream of photons traveling in a wave like pattern at the speed of light.

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38
Q

photon

A

stream of “particles” suggested by electromagnetic radiation

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39
Q

Important conclusions of Planck and Einstein

A
  • Energy is quantized and can occur only in quanta
  • Electromagnetic radiation shows characteristics of particulate matter and wave properties. (dual nature of light)
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40
Q

all matter exhibits both?

A

particulate and wave properties.

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41
Q

when H2 molecules absorb energy what happens to the bonds?

A

the bonds are broken resulting in excited atoms

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42
Q

what is produced when excess energy is released from hydrogen atoms?

A

An emission spectrum

43
Q

Emission spectrum

A

a series of colored lines that correspond to wavelengths emitted by the glowing gas.

44
Q

what colors does a continuous spectrum possess?

A

rainbow

45
Q

Important points about the Bohr model (3)

A

-The model correctly fits the quantized energy levels of the hydrogen atom and only allows certain circular orbits for the electron
- As the electron becomes more tightly bound, its energy becomes more negative
- As the electron is brought closer to the nucleus, energy is released from the system

46
Q

wave function

A

a function of the coordinates (x,y,z) of the electrons position in 3-D space

47
Q

quantum wave mechanical model

A

the electron is able to move freely within its own home orbital and can gain energy and jump to a higher energy level

48
Q

Pauli Exclusion Principle

A

In a given atom no two electrons can have the same set of four quantum numbers.

49
Q

l=1

A

p

50
Q

l=0

A

s

51
Q

l=2

A

d

52
Q

l=3

A

f

53
Q

to Schrodinger and de Brigolie the electron bound to the nucleus seemed similar to?

A

standing wave

54
Q

In the quantum mechanical model, Specific electron motions are?

A

unknown

55
Q

In the quantum mechanical model, the specific electron motions help determine?

A

the most probable distance at which the electron is found

56
Q

Principle Quantum number has ____ values?

A

integer

57
Q

As n increases, what happens to the orbital and energy of the electron?

A

orbital becomes larger with more electrons away from nucleus. Energy is higher since electron less tightly bound to the nucleus.

58
Q

angular momentum quantum number symbol

A

l

59
Q

angular momentum quantum number has values from?

A

0 to n-1

60
Q

the angular momentum quantum number is related to?

A

the shape of atomic orbitals

61
Q

magnetic quantum number symbol

A

ml

62
Q

the magnetic quantum number has integer values between

A

l and -l including zero

63
Q

the value of ml is related to?

A

the orientation of the orbital in space

64
Q

l is also called?

A

subshell

65
Q

the number of nodes increases as?

A

n increases

66
Q

node

A

area of zero probability if finding an electron

67
Q

shape of the s orbital

A

spherical

68
Q

shape of p orbitals

A

2 lobes separated by a node at the nucleus

69
Q

electron spin quantum number symbol

A

ms

70
Q

ms can only have two values?

A

+.5 and -.5

71
Q

Since only 2 values of ms are allowed, an orbital?

A

can only hold two electrons and must have opposite spins

72
Q

poly electronic atoms

A

atoms with more than one electron

73
Q

3 energy contributions that must be considered of the description of poly electronic atoms?

A

-KE as move towards the nucleus
-PE of attraction btwn the nucleus & electrons
-PE of repulsion between 2 electrons

74
Q

Electron correlation problem

A

since electron pathways are unknown, the electron repulsion cannot be calculated

75
Q

electron repulsion

A

electrons staying as far apart from each other as possible due to their same charge

76
Q

2s orbital is lower than a _____ orbital in poly electronic atoms

A

2p

77
Q

the more effectively an orbital allows its electrons to penetrate the shielding electrons to be closer to the nuclear charge, what happens to the energy of the orbitals?

A

lowers

78
Q

Aufbau principle

A

as protons are added one by one to the nucleus to build up elements, electrons are similarly added to the hydrogen-like orbitals

79
Q

Hund’s rule

A

the lowest energy for an atom is one having the max number of unpaired electrons allowed in a particular set of degenerate orbitals

80
Q

inner elements are known as?

A

core elements

81
Q

elements on which the 4f orbitals are being filled

A

lanthanides

82
Q

elements on which the 5f orbitals are being filled

A

actinides

83
Q

Ionization energy

A

energy required to remove an electron from a gaseous ion or atom in gorund state

84
Q

In the process of ionization ______ energy electrons are removed first.

A

highest

85
Q

first ionization energy

A

energy required to remove the highest energy electron of an atom

86
Q

Second ionization energy

A

energy required to remove the highest energy electron of an ion

87
Q

trend in ionization across a period

A

increase

88
Q

why does ionization energy increase across a period?

A

due to increasing nuclear charge which results in electrons being more strongly bound to the nucleus

89
Q

trend in ionization down a group

A

decrease

90
Q

why does ionization decrease down a group?

A

due to the outermost electron being father from the nucleus

91
Q

atomic radius

A

the measure of size of an element

92
Q

trend in atomic radius across a period

A

decrease

93
Q

why does atomic radius decrease across a period

A

due to the increase in protons the nuclear charge attracts the electrons more strongly.

94
Q

trend in atomic radius down a group

A

increase

95
Q

why does atomic radius increase down a group?

A

the number of energy levels increases so there is a greater distance between the nucleus and outermost orbital

96
Q

group 1A

A

alkali

97
Q

group 2A

A

alkaline earth metals

98
Q

group 7A

A

halogens

99
Q

group 8A

A

noble gases

100
Q

metals tend to _____ electrons and form _____.

A

lose, cations

101
Q

metals tend to have ______ ionization energies

A

low

102
Q

where are most active metals located on the table?

A

bottom left corner

103
Q

nonmetals tend to ____ electrons and form ____.

A

gain, anions

104
Q

electron shielding

A

the blocking of valence shell electron attraction by the nucleus, due to the presence of inner-shell electrons.

AP Chemistry (16 decks)

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