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Chemistry I > Unit 2 Test > Flashcards

Unit 2 Test Flashcards

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0
Q

what is electromagnetic radiation?

A

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

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1
Q

what are the 2 other names for electromagnetic radiation?

A
  1. electromagnetic spectrum

2. light

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2
Q

what kind of relationship is between freq. & wavelength?

A

inverse relationship

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3
Q

what kind of relationship is between freq. & energy?

A

direct relationship

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4
Q

what are radio waves on the electromagnetic spectrum?

A

LIGHT, not sound

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5
Q

what is the diff. between light & sound?

A

sound requires matter to travel, light does not

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6
Q

what are microwaves used in?

A

microwaves (the kitchen appliance)

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7
Q

what is infrared?

A

heat radiation, what’s given off w/ high temp.

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8
Q

what is visible light?

A

what we see (we see what isn’t absorbed (what is reflected))

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9
Q

what color is something when all the light is absorbed?

A

black

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10
Q

what color is something when all the light is reflected?

A

white

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11
Q

tell about ultraviolet light

A
  • very bad for us, what we use sunscreen to block

- only about 1% comes down to earth

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12
Q

what is wavelength?

A

distance between 2 same spots on neighboring waves (corresponding points on adjacent waves)

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13
Q

what is the name of the symbol for wavelength & what does it look like?

A

lamba; upside down y

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14
Q

what is the preferable unit for wavelength?

A

nm (nanometer)

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15
Q

what is frequency?

A
  • the “how often” factor

- the # of waves that pass a given point in a specific time, usually 1 second

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16
Q

what is the symbol for frequency?

A

v

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17
Q

what is the unit for freq.?

A

Hz (hertz) – means: waves/sec

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18
Q

what is the symbol for speed?

A

C

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19
Q

what is the speed of light?

A

3.0 X 10^8 m/sec

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20
Q

what does the speed of each light form depend on?

A

TRICK QUESTION ALL FORMS OF LIGHT TRAVEL AT THE SAME SPEED

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21
Q

what is the equation/formula for speed of light?

A

speed of light = wavelength X freq.

C = (upside down)y X v

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22
Q

what is the symbol for energy?

A

E

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23
Q

what is energy measured in?

A

Kilojoules (KJ)

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24
Q

what is the formula for energy?

A

E=hv

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25
Q

what is h? (E=hv)

A

Plank’s constant

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26
Q

what is the “formula” for Plank’s constant?

A

h = E/v

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27
Q

what does a constant mean?

A

direct relationship

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28
Q

what is a quanta?

A

a small amount of energy

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29
Q

what is a photon?

A

a small amount of energy?

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30
Q

who named the quanta?

A

Plank

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31
Q

who named the photon?

A

Einstein

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32
Q

what is the difference between a quanta & a photon?

A

NOTHING - INTERCHANGEABLE, SAME THING

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33
Q

is quanta or photon used more often?

A

photon is used more often, it’s more common

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34
Q

what did scientists used to think energy was like?

A

connected, never-ending (like a long, curvy continuous line)

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35
Q

what do scientists now know energy is like?

A

short bursts of energy (imagine a string of pearls)

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36
Q

what does the duel wave particle nature deal with?

A

photon (quanta) vs. electron

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37
Q

what is a photon (quanta) & what is an e-?

A

photon (quanta) –> energy

electron –> matter

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38
Q

how does a photon (quanta) travel?

A

travels in waves

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39
Q

what does an e- have that the photon (quanta) doesn’t?

A

mass & volume

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40
Q

how is a photon like matter & how is an e- like energy?

A
  • photon –> like matter in small packets (like a particle)

- electron –> like energy in their movement which is in waves

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41
Q

what is the photoelectric effect?

A
  • “what happens w/ light & electrons”

- the response of e- in a material when light is directed/absorbed to/into it

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42
Q

what is ground state?

A

lowest energy state –> naturally

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43
Q

what is excited state?

A

higher energy state –> after absorbed # photons (of light)

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44
Q

what happens to the e- in a material when light is directed/absorbed to/into it?

A

they go from G.S. –> E.S. –> G.S.

+energy -energy

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45
Q

what can be measured in the photoelectric effect?

A

can measure & can see what is released (the color of visible light)

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46
Q

do the e- stay in the excited state?

A

no - cannot sustain self in excited state, must go back to ground state

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47
Q

how is a spectrum produced?

A

using spectroscope

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48
Q

what does a spectroscope need to contain?

A

prism or diffraction lens

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49
Q

what does a spectrum do?

A

breaks light up into diff. parts

50
Q

what is a spectrum based on?

A

range of nm & freq.

51
Q

basically, what’s a spectrum?

A

visible light

52
Q

what are the 3 types of spectrums?

A
  1. continuous spectrum
  2. emission spectrum
  3. absorption spectrum
53
Q

what is a continuous spectrum?

A

where the bonds of light have no gaps, no divisions, no breaks - 1 color blends into the next

54
Q

what are continuous spectrums produced by?

A

light sources (i.e. the sun, lightbulbs (white ones))

55
Q

what is an emission spectrum?

A

have separate bands of colors

56
Q

what are the the other names for an emission spectrum?

A

Bright-light / Line spectrum

57
Q

what are emission spectrums produced by?

A

individual elements

58
Q

what is an absorption spectrum?

A

has dark lines where they responded to light

59
Q

what is an absorption spectrum also known as?

A

Dark-line spectrum

60
Q

what are the colors of visible light?

A

red, orange, yellow, green, blue, indigo, violet

61
Q

what is the range of visible light?

A

700 nm - 400 nm

62
Q

at the end where radio waves are, are wavelengths longer or shorter?

A

longer

63
Q

at the end where radio waves are, is freq. low or high?

A

low

64
Q

at the end where radio waves are, is energy low or high?

A

low

65
Q

at the end where gamma rays are, are wavelengths short or long?

A

shorter

66
Q

at the end where gamma rays are, is freq. high or low?

A

high

67
Q

at the end where gamma rays are, is energy high or low?

A

high

68
Q

in Bohr’s model, what was the problem?

A

mathematically, it only worked for 1 e- (hydrogen), not any other elements

69
Q

what did most scientists during Bohr’s time think the atom was set up like?

A

the solar system

70
Q

what is Bohr’s model referred to as?

A

the “planetary model”

71
Q

what did Bohr determine from his failed model?

A

each location (orbital) within the e- cloud can hold more than 1 e-

72
Q

what did DeBroglie do?

A

tell us the e- moves around nucleus in waves (unlocked movement of e-)

73
Q

what did Heisenberg give us?

A

the Heisenberg Uncertainty Principle

74
Q

what is the Heisenberg Uncertainty Principle?

A

cannot look at speed & location (velocity & position) at the same time - can pick one, can’t do both

75
Q

what was Schrödinger’s contribution?

A

gave us probable location of e-, mathematically calculated

76
Q

how did Schrödinger find the probable location of the e-?

A

used equations called quantum theory

77
Q

what was Schrödinger’s quantum theory?

A

probable location = (# e-) (v) (h)

78
Q

what is an orbital?

A

3D region located above & around nucleus

79
Q

what do orbitals max out at?

A

2 e-

80
Q

what are the 4 diff. types of quantum #s?

A
  1. Principal QN
  2. Angular Momentum QN
  3. Magnetic QN
  4. Spin QN
81
Q

what does the principal QN indicate?

A

distance from nucleus

82
Q

what is the symbol for principal QN?

A

n

83
Q

what are the # values for principal QN?

A

1 to 7 (whole #s)

84
Q

what do the # values for principal QN actually represent?

A 
energy levels (aka energy shells which use letters K-Q)
*also are periods on PT
85
Q

what does angular momentum QN indicate?

A

shape of orbital

86
Q

what is the symbol for angular momentum QN?

A

scripted/cursive l (L)

87
Q

what are the # values for angular momentum QN?

A

0 to 3 (whole #s)

88
Q

what do the # values for angular momentum QN actually represent?

A

sublevels (s-p-d-f)

89
Q

what does the angular momentum QN 0 tell about that sublevel?

A
  • aka s
  • electron capacity of 2 e-
  • sphere shape
90
Q

what does the angular momentum QN 1 tell about that sublevel?

A
  • aka p
  • electron capacity of 6 e-
  • dumb bell shape
91
Q

what does the angular momentum QN 2 tell about that sublevel?

A
  • aka d
  • electron capacity of 10 e-
  • double dumb bell / donut w/ dumb bell shape
92
Q

what does the angular momentum QN 3 tell about that sublevel?

A
  • aka f
  • electron capacity of 14 e-
  • complex shape (see book)
93
Q

what does the magnetic QN indicate?

A

orientation around nucleus on x-y-z axes

94
Q

what is the symbol for magnetic QN?

A

m

95
Q

what are the # values for magnetic QN?

A

+3 to 0 to -3 (whole #s)

96
Q

what do the # values for magnetic QN actually represent?

A

orbital (max of 2 e-), used in arrangment as x-y-z

97
Q

what is the magnetic QN range & # of orbitals for the s sublevel?

A 
range: 0
# orbitals: 1
98
Q

what is the magnetic QN range & # of orbitals for the p sublevel?

A 
range: +1 / 0 / -1
# orbitals: 3
99
Q

what is the magnetic QN range & # of orbitals for the d sublevel?

A 
range: +2 / +1 / 0 / -1 / -2
# orbitals: 5
100
Q

what is the magnetic QN range & # of orbitals for the f sublevel?

A 
range: +3 / +2 / +1 / 0 / -1 / -2 / -3
# orbitals: 7
101
Q

what does spin QN indicate?

A

-spin direction of e- (rotation around its axis of e-)

102
Q

what is the symbol for spin QN?

A

s

103
Q

what are the # values for spin QN?

A

+1/2 , -1/2

104
Q

in spin QN, what # value is clockwise & what # value is counterclockwise?

A

+1/2 –> clockwise

-1/2 –> counterclockwise

105
Q

what do the # values for spin QN actually represent?

A

spin on its axis

106
Q

how is spin QN represented in a written arrangement?

A

arrows (going up or down)

*up = positive, down = neg.

107
Q

what is the Pauli Exclusion Principle?

A

-no 2 e- for the same atom can have the same 4 QNs
so…
only can have 2 e- per orbital w/ opposite spins

108
Q

what do opposite spins do?

A

keep e- apart

109
Q

when was the Pauli Exclusion Principle developed?

A

1925

110
Q

what is the Aufbau Principle?

A

e- must fill lowest energy orbitals

111
Q

what are the exceptions to the Aufbau principle?

A

groups 6 & 11

112
Q

what is done when filling group 6 element’s e- arrangements?

A

always put 1 half arrow in each of the 5 d orientations (take arrow out of 4s orbital)

113
Q

what is the reason behind the special rule in group 6?

A

balance d- orbital w/ one in each orbitals place & only 1 in s orbital

114
Q

what is the rule for group 11 element’s e- arrangements?

A

always fill d sublevel completely (2 arrows in each)

115
Q

what is the reason behind the exception with group 11?

A

balance d- orbitals w/ 2 in each orbital place & only 1 in s orbital

116
Q

what is Hund’s Rule?

A

orbitals w/ the same energy (in same sublevel) are filled w/ one e- each before 2nd e- is added to oribtal

117
Q

what are the 3 types of e- arrangements?

A
  1. orbital notation
  2. electron configuration notation
  3. noble gas notation
118
Q

what does orbital notation use to represent the orbital?

A

a line

119
Q

in orbital notation, what goes underneath the line (orbital)?

A

label under line w/ principal QN & sublevel letter for angular momentum QN & letter for magnetic QN

120
Q

what goes above the line (orbital) in orbital notation?

A

arrow(s) showing e- spin QN (max. 2 arrows in opposite directions)

121
Q

describe electron configuration notation

A

uses principal QN & sublevel letter for angular momentum QN && superscript for # of e-

*add superscripts to get total # e-

122
Q

describe noble gas notation

A

used chem. symbol of noble gas in [brackets] for filled energy levels (use noble gas in 1 period before the element)
cont. w/ principal QN & sublevel letter for angular momentum QN && superscript for # of e-

123
Q

describe electron dot diagram

A

used chem. symbol & dots (for valence e- only)

Chemistry I (5 decks)

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