Chapter 8-11 Flashcards
1
Q
Define quantum
A
Absolutely small
2
Q
define macroscopic
A
large
3
Q
quantum particles can be in how many states at one time?
A
2 states
4
Q
what is Schrodinger’s cat?
A
while unknown, something can be in two states
5
Q
light is what type of radiation?
A
electromagnetic
6
Q
True of false: electromagnetic radiation is a wave
A
true
7
Q
what is the speed of light?
A
c=3*10^8 m/s
8
Q
what is amplitude?
A
vertical height of a wave
9
Q
what is wavelength
A
distance between adjacent crests
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
11
Q
frequency of a wave is proportional to what of a wave
A
speed and energy
12
Q
frequency is inversely proportional to what of a wave
A
wavelenth
13
Q
what color of visible light has the longest wavelength
A
red (750nm)
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
15
Q
what is constructive interference of waves
A
combining and building of two waves
16
Q
define defraction
A
wave bending around obstacle
17
Q
many metals emit what when light shines on them
A
electrons
18
Q
define threshold value
A
minimum value required to eject electrons from surface of metal
19
Q
Albert Einstein developed what theory
A
the photoelectric affect and photons
20
Q
what are photons
A
packets of light
21
Q
what is Plank’s constant
A
h=6.626*10^-34 J… measure of energy
22
Q
modern electromagnetic theory
A
light is lumpy; a shower of particles
23
Q
what is atomic spectroscopy
A
sutdy of electromagnetic radiation emitted and absorbed by atoms
24
Q
when an atom absorbs energy, it does what with that energy
A
re-emits it as light
25
emission spectrum can be used to identify what
specific elements
26
what is Bohr known for
dorming model with fixed electron orbit
27
radiation is emitted or absorbed only when what happens
electrons jump from different orbits
28
what is the equation for speed of light
frequency x wavelength
29
what is the equation for energy of light
Plank's constant x frequency
30
who proposed wave nature of electrons
Louis De Broglie
31
true/false: wavelength is proportional to velocity
true
32
interference is associated with what nature of electrons
wave nature
33
wave nature and electron nature are what kind of properties
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
34
what is the Heisenburg Uncertainty Principle
impossible to know both position and speed of particle accurately
35
electron beams carry similar but different BLANK as light
diffraction patterns
36
what is a probabilty distribution map
statistical map that shows where an electron is likely to be found
37
what is an orbital
a probabilty distribution map
38
what are the 4 quantum numbers
n, l, ml, ms
39
what is the principle quantum number and what does it show
n; determines size and energy of orbital; is the shell; infinite number of shells
40
what is l
angular momentum; determines shape of orbital; letters assigned sdpf
41
what is ml
magnetic quantum number; orientation of orbital (planes); values between -l and +l
42
what is ms
spin orientation; only +1/2 or -1/2
43
how many sublevels in n=2
2 sublevels
44
how many orbitals of l=2
l=2 is d sublevel, therefore there are 5 orbitals
45
the energy of a photon is always positive or negative?
positive
46
wavelength of photon equals
(plank's constant x speed of light) / energy
47
probability density
probability (per unit volume) of find e- at point in space
48
radial distribution function
probability of finding e- within thing spherical shell at a distance of r from nucleus
49
probability density is at maximum where
nucleus
50
RDF is what value at nucleus
zero
51
what is a node
point where wave function is zero
52
what is the probabilty of finding an electron at a node?
zero
53
what was Balmer/Rydberg contribution
relating the wavelength of an atome to the energy of the atom
54
Mendeleev contribution
organized periodic table based on increasing atomic mass and recognized patterns in properties of elements
55
Mendeleev's model didn't explain what
why
56
what is electron configuraiton
notation that shows paticular orbitals occupied by eletrons in an atom
57
what is ground state
lowest energy state
58
what is an orbital diagram
gives information similar to electron configuration but symbolizes eletrons with boxes and arrows
59
what is Pauli exclusion principle
no 2 electrons can have same 4 QN, they must have different spins, and only 2 electonrs can occupy a given orbital
60
Coulumbs law
potential energy of 2 charged particles dpeneds on charges and separation
61
potential energy does what as particles get further apart
increases
62
for opposite charges, potential energy is what value and does what as particles get closer
energy is negative and gets more negative as particles get closer
63
what is shielding
repulsion of one electron by the other
64
what is effective nuclear charge
actualy nuclear charge experience by an elecron; charge of nucleus minus charge of shielding electron
65
Aufbau principle
electrons fill one orbital at a time starting with the lowest energy available
66
Hund's rule
elecrons fill orbitals in a level singly first with parallel spins
67
orbitals can hold no more than how many electrons
2 electrons
68
atomic radius periodic pattern
increases down a column, decreases across a row (atoms become more tightly bundled)
69
removal of electrons in reverse order of filling EXCEPT for what elements
transition elements
70
what is a paramagnetic atom
atom or ion that has unpaired electrons and is attracted to magnetic field
71
what is diamagnetic atom
atom or electron which all electrons are paired
72
losing electrons has what effect on atomic radii
it get smaller
73
what is ionization energy
energy requird to remove an electron; always positive
74
ionization energy periodic pattern
increases up a column and to the right; inverse of size
75
exceptions to ionization energy include what 2 elements
boron and oxygen
76
core electrons are equal to what elements
noble gases
77
define electron affinity
energy required to add an electron to nuetral gas atom
78
how are core electrons found
subtract valence electrons from total number of electrons
79
electron affinities are generally what value
negative, exothermic
80
electron affinity trend
becomes more negative across rows
81
why do chemica bonds form
they lower potential energy between charged particles
82
which bonds are stronger: ionic or covalent
ionic bonds
83
octet rule
stable configuration with 8 valence electrons
84
which bond are generally the shortest and strongest
triple bonds
85
polarity is based on what
electron density
86
what is electronegativity
ability of atom to attract electron to itself; results in polarity
87
electronegativity trend
increases across a row, decreases down a column
88
what are the 4 most electronegative elements?
fluorine, oxygen, nitrogen, chlorine
89
higher electronegativity indicates greater what
polarity
90
what is dipole moment
measure of separation of positive and negative charge in a molecule; shows polarity
91
how do you know which elements is central in lewis structure
least electronegative element is the center; terminal atoms are most electronegative
92
what is a resonance structure
a structure that represents a molecule with multiple correct lewis structures
93
in nature atoms are acutally delocalized or localized
delocalized: spread out with lower energies
94
define formal charge
fictitious charge assigned to each atom in a lewis structure that helps distinguish among competing lewis structures
95
according to formal charge rules, the sum of all formal charges in a molecule must equa what
zero
96
according to formal charge rules, the sum of all formal charges in an ion must equal what
the charge of the ion
97
true/false: large formal charges for individual ions are better than small charges
false
98
negative formal charges should reside on which kind of ion
the most electronegative atom
99
two elements that often form incomplete octets are
Boron and Beryllium
100
3rd row elements and on often form what
exanded octets
101
what is bond energy
energy required to break 1 mole of bond in gas statebon
102
bond energies are endothermic and therefore always what
positive
103
What type of bonds have the greates bond energy
stable bonds, noble gases
104
forming bonds is BLANK while breaking bonds is BLANK
exothermic, endothermic
105
formula for bond energy
bonds broken minus bonds formed
106
VSEPR Theory states
electron groups repel each other through coulombic forces
107
what are the five electron geometries
linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral
108
bond angle for linear
180°
109
bond angle for trigonal planar
120°
110
tetrahedyl bond angle
~109°
111
trigonal pyramidal bond angle
90° and 120°
112
octahedral bond angle
90°
113
presence of lone pair changes what two things
molecular geometry and bond angle
114
for any trigonal bipyramidal, place lone pairs in BLANK positions
equatorial
115
for octahedral, place lone pairs in BLANK positions
axial
116
what is the pattern for Carboxylic acids
RCO2H
117
most acids are what kind of acid
oxoacids
118
in oxoacids, what two elements are bonded together
hydrogen and oxygen
