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Chemistry I > Chapter 8-11 > Flashcards

Chapter 8-11 Flashcards

1
Q

Define quantum

A

Absolutely small

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2
Q

define macroscopic

A

large

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3
Q

quantum particles can be in how many states at one time?

A

2 states

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4
Q

what is Schrodinger’s cat?

A

while unknown, something can be in two states

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5
Q

light is what type of radiation?

A

electromagnetic

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6
Q

True of false: electromagnetic radiation is a wave

A

true

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7
Q

what is the speed of light?

A

c=3*10^8 m/s

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8
Q

what is amplitude?

A

vertical height of a wave

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9
Q

what is wavelength

A

distance between adjacent crests

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10
Q

define frequency

A

number of cycles that pass through a stationary point at a given time; cycle per second; units are Hertz or s^-1

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11
Q

frequency of a wave is proportional to what of a wave

A

speed and energy

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12
Q

frequency is inversely proportional to what of a wave

A

wavelenth

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13
Q

what color of visible light has the longest wavelength

A

red (750nm)

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14
Q

name the parts of a wave spectrum in order of increasing wavelength

A

gamma, x-ray, uv, visible light, infrared light, micro, radio

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15
Q

what is constructive interference of waves

A

combining and building of two waves

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16
Q

define defraction

A

wave bending around obstacle

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17
Q

many metals emit what when light shines on them

A

electrons

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18
Q

define threshold value

A

minimum value required to eject electrons from surface of metal

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19
Q

Albert Einstein developed what theory

A

the photoelectric affect and photons

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20
Q

what are photons

A

packets of light

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21
Q

what is Plank’s constant

A

h=6.626*10^-34 J… measure of energy

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22
Q

modern electromagnetic theory

A

light is lumpy; a shower of particles

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23
Q

what is atomic spectroscopy

A

sutdy of electromagnetic radiation emitted and absorbed by atoms

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24
Q

when an atom absorbs energy, it does what with that energy

A

re-emits it as light

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25
Q

emission spectrum can be used to identify what

A

specific elements

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26
Q

what is Bohr known for

A

dorming model with fixed electron orbit

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27
Q

radiation is emitted or absorbed only when what happens

A

electrons jump from different orbits

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28
Q

what is the equation for speed of light

A

frequency x wavelength

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29
Q

what is the equation for energy of light

A

Plank’s constant x frequency

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30
Q

who proposed wave nature of electrons

A

Louis De Broglie

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31
Q

true/false: wavelength is proportional to velocity

A

true

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32
Q

interference is associated with what nature of electrons

A

wave nature

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33
Q

wave nature and electron nature are what kind of properties

A

complimentary; the more we know about one the less we now about the other; the more we know of location the less we know of speed

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34
Q

what is the Heisenburg Uncertainty Principle

A

impossible to know both position and speed of particle accurately

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35
Q

electron beams carry similar but different BLANK as light

A

diffraction patterns

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36
Q

what is a probabilty distribution map

A

statistical map that shows where an electron is likely to be found

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37
Q

what is an orbital

A

a probabilty distribution map

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38
Q

what are the 4 quantum numbers

A

n, l, ml, ms

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39
Q

what is the principle quantum number and what does it show

A

n; determines size and energy of orbital; is the shell; infinite number of shells

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40
Q

what is l

A

angular momentum; determines shape of orbital; letters assigned sdpf

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41
Q

what is ml

A

magnetic quantum number; orientation of orbital (planes); values between -l and +l

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42
Q

what is ms

A

spin orientation; only +1/2 or -1/2

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43
Q

how many sublevels in n=2

A

2 sublevels

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44
Q

how many orbitals of l=2

A

l=2 is d sublevel, therefore there are 5 orbitals

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45
Q

the energy of a photon is always positive or negative?

A

positive

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46
Q

wavelength of photon equals

A

(plank’s constant x speed of light) / energy

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47
Q

probability density

A

probability (per unit volume) of find e- at point in space

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48
Q

radial distribution function

A

probability of finding e- within thing spherical shell at a distance of r from nucleus

49
Q

probability density is at maximum where

A

nucleus

50
Q

RDF is what value at nucleus

A

zero

51
Q

what is a node

A

point where wave function is zero

52
Q

what is the probabilty of finding an electron at a node?

A

zero

53
Q

what was Balmer/Rydberg contribution

A

relating the wavelength of an atome to the energy of the atom

54
Q

Mendeleev contribution

A

organized periodic table based on increasing atomic mass and recognized patterns in properties of elements

55
Q

Mendeleev’s model didn’t explain what

A

why

56
Q

what is electron configuraiton

A

notation that shows paticular orbitals occupied by eletrons in an atom

57
Q

what is ground state

A

lowest energy state

58
Q

what is an orbital diagram

A

gives information similar to electron configuration but symbolizes eletrons with boxes and arrows

59
Q

what is Pauli exclusion principle

A

no 2 electrons can have same 4 QN, they must have different spins, and only 2 electonrs can occupy a given orbital

60
Q

Coulumbs law

A

potential energy of 2 charged particles dpeneds on charges and separation

61
Q

potential energy does what as particles get further apart

A

increases

62
Q

for opposite charges, potential energy is what value and does what as particles get closer

A

energy is negative and gets more negative as particles get closer

63
Q

what is shielding

A

repulsion of one electron by the other

64
Q

what is effective nuclear charge

A

actualy nuclear charge experience by an elecron; charge of nucleus minus charge of shielding electron

65
Q

Aufbau principle

A

electrons fill one orbital at a time starting with the lowest energy available

66
Q

Hund’s rule

A

elecrons fill orbitals in a level singly first with parallel spins

67
Q

orbitals can hold no more than how many electrons

A

2 electrons

68
Q

atomic radius periodic pattern

A

increases down a column, decreases across a row (atoms become more tightly bundled)

69
Q

removal of electrons in reverse order of filling EXCEPT for what elements

A

transition elements

70
Q

what is a paramagnetic atom

A

atom or ion that has unpaired electrons and is attracted to magnetic field

71
Q

what is diamagnetic atom

A

atom or electron which all electrons are paired

72
Q

losing electrons has what effect on atomic radii

A

it get smaller

73
Q

what is ionization energy

A

energy requird to remove an electron; always positive

74
Q

ionization energy periodic pattern

A

increases up a column and to the right; inverse of size

75
Q

exceptions to ionization energy include what 2 elements

A

boron and oxygen

76
Q

core electrons are equal to what elements

A

noble gases

77
Q

define electron affinity

A

energy required to add an electron to nuetral gas atom

78
Q

how are core electrons found

A

subtract valence electrons from total number of electrons

79
Q

electron affinities are generally what value

A

negative, exothermic

80
Q

electron affinity trend

A

becomes more negative across rows

81
Q

why do chemica bonds form

A

they lower potential energy between charged particles

82
Q

which bonds are stronger: ionic or covalent

A

ionic bonds

83
Q

octet rule

A

stable configuration with 8 valence electrons

84
Q

which bond are generally the shortest and strongest

A

triple bonds

85
Q

polarity is based on what

A

electron density

86
Q

what is electronegativity

A

ability of atom to attract electron to itself; results in polarity

87
Q

electronegativity trend

A

increases across a row, decreases down a column

88
Q

what are the 4 most electronegative elements?

A

fluorine, oxygen, nitrogen, chlorine

89
Q

higher electronegativity indicates greater what

A

polarity

90
Q

what is dipole moment

A

measure of separation of positive and negative charge in a molecule; shows polarity

91
Q

how do you know which elements is central in lewis structure

A

least electronegative element is the center; terminal atoms are most electronegative

92
Q

what is a resonance structure

A

a structure that represents a molecule with multiple correct lewis structures

93
Q

in nature atoms are acutally delocalized or localized

A

delocalized: spread out with lower energies

94
Q

define formal charge

A

fictitious charge assigned to each atom in a lewis structure that helps distinguish among competing lewis structures

95
Q

according to formal charge rules, the sum of all formal charges in a molecule must equa what

A

zero

96
Q

according to formal charge rules, the sum of all formal charges in an ion must equal what

A

the charge of the ion

97
Q

true/false: large formal charges for individual ions are better than small charges

A

false

98
Q

negative formal charges should reside on which kind of ion

A

the most electronegative atom

99
Q

two elements that often form incomplete octets are

A

Boron and Beryllium

100
Q

3rd row elements and on often form what

A

exanded octets

101
Q

what is bond energy

A

energy required to break 1 mole of bond in gas statebon

102
Q

bond energies are endothermic and therefore always what

A

positive

103
Q

What type of bonds have the greates bond energy

A

stable bonds, noble gases

104
Q

forming bonds is BLANK while breaking bonds is BLANK

A

exothermic, endothermic

105
Q

formula for bond energy

A

bonds broken minus bonds formed

106
Q

VSEPR Theory states

A

electron groups repel each other through coulombic forces

107
Q

what are the five electron geometries

A

linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral

108
Q

bond angle for linear

A

180°

109
Q

bond angle for trigonal planar

A

120°

110
Q

tetrahedyl bond angle

A

~109°

111
Q

trigonal pyramidal bond angle

A

90° and 120°

112
Q

octahedral bond angle

A

90°

113
Q

presence of lone pair changes what two things

A

molecular geometry and bond angle

114
Q

for any trigonal bipyramidal, place lone pairs in BLANK positions

A

equatorial

115
Q

for octahedral, place lone pairs in BLANK positions

A

axial

116
Q

what is the pattern for Carboxylic acids

A

RCO2H

117
Q

most acids are what kind of acid

A

oxoacids

118
Q

in oxoacids, what two elements are bonded together

A

hydrogen and oxygen

Chemistry I (16 decks)

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