Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chem Quiz #1 > Chem Quix #4 > Flashcards

Chem Quix #4 Flashcards

1
Q

Octet Rule Exceptions

A

1) Odd e- molecules
2) Hypovalent (e- deficient molecules)
3) Hypervalent molecules (valence shell expansion)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Odd e- molecules

A

Moleulce w/ odd e- can’t have octet for every atom
ex. NO w/ 11 valence e- or NO2 w/ 17 valence e-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Hypovalent Molecules

A

atoms w/ less then octet configuration
ex. BH3 & BF3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Hypervalent Molecules/Valence Expansion

A

molecules APPEAR to have atoms w/ more then octet of e- in valence shells but it’s maintained
ex. XeF2 (8e- + 2e- = 10e-) or PF5 (5+5=10e-) or SF6 (6+6=12)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Formal Charge

A

charge on atom in molecule if e- pair bonds are hypothetically broken (homolyticially)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Heterolytically

A

breaking covalent bond so e- pair is transferred to 1 of the partners (usually more electron(-)…resulting charges = oxidation states

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

2 extremes of formal assignment of bonding e- pairs

A

formal charge & oxidation states

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Diff. between formal charge & oxidation #

A

FC = assuming equal sharing of e- VS Ox. # =assuming interaction is 100% ionic (transfer)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Neither FC or Ox # describe _____________ & actual charge is _____________

A

Neither FC or Ox # describe bonding in HETERNUCLEAR DIATOMIC MOLECULES & actual charge is INTERMEDIATE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Rules for Ox. #s

A

1) must add up to molecule charge
2) is always 0 in elemental form
3) nonmetals have (-) Ox. #s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Ox. # Rule Exceptions

A

1) Oxygen has Ox. # of -2 EXCEPT when combined w/ Flourine
2) Oxygen has Ox. # of -2 EXCEPT when combined w/ O-O bond
3) Ox. # of Hydrogen is +1 w/ nonmetals (EXCEPT B or Si)and -1 when bonded w/ metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

sum Ox. #s =

A

charge on molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

VESPR

A

don’t account for lone pairs (repulsion between e- lone pairs is minimized)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

In Ox. #s 1 valence e- pair =

A
  • 1 single bond
  • 1 double bond
  • 1 triple bond
  • 1 lone pair
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Steric #

A

atoms bonded
(coordination # + lone pair #)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

explain AXE notation

A

A: just is
X: coordination #
E: lone pair #

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

When is compound usually expressed w/ VESPR?

A

when X + E = steric #

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Lone Pair Size & effects

A

larger than bond pair & thus repulsions are greater resulting in decreasing bond angle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Molecules w/ steric #5

A

Trigonal Bipyramidal (AX4E)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Trigonal Bipyramidal sites for lone pairs

A

axial & equatorial

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Trigonal Bipyramidal isomers

A

has 2 depending on if lone pairs occupy axial or equatorial sites

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Trigonal Bipyramidal preferred bonding site

A

equatorial (more spacious w/ 2 90 angles instead of 3 90 angles)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Octahedral preferred bonding site

A

sites separated by 180

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Which is the most dominant & why?
lone pair-lone pair
lone pair-bond pair
bond pair-bond pair

A

lone pair-lone pair since they are closest to the central atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Molecular Orbital Theory
account for lone pairs
26
e- moving in circular orbit will
lose its energy and spiral into the nucleus
27
What will an electric charge that undergoes acceleration (changes in velocity & direction) emit?
electromagnetic radiation & will lose energy w/ every turn
28
Synchrotron
beam of e- spinning & changes path to emit radiation
29
Quantization
examines radiation emitted from materials
30
Light
wave, particle, or energy
31
most electronic structure of atoms comes from analysis of
light emitted/absorbed by substances
32
Newton's light discovery
light can be broken down into components w/ diff. color from red to violet w/ prism (ROYGBIV)
33
Wave lengths from longest to shortest (lowest frequency to highest)(lowest energy to highest)
Radio Waves Microwaves Infrared Radiation (ROY G BIV) Ultraviolet Gamma Rays Cosmic Radiation
34
3 Features of a Wave
1) Amplitude 2) Wavelength 3) Frequency
35
Wave Amplitude
max displacement (height above midline)
36
Wave Intensity
determines radiation levels (amplitude^2)
37
Wave Wavelength
peak-peak distance
38
Wave Frequency
wavelengths that pass through a given point in 1 second
39
1/s =
Hz
40
Speed eq.
distance frequency x wavelength ------------- = ------------------------------------ time 1
41
Distance eq.
frequency x wavelength
42
Sqeed eq. expanded
43
C in relation to frequency & wavelength
C = wavelength x frequency
44
Speed of Light in a vacuum (c)
3x10^8 - will have diff. speeds in diff. medians but never faster
45
Frequency in relation to C & wavelength
Frequency = c/wavelength
46
High Frequency has ____________ wavelength & ___________ energy?
Short wavelength High Energy ex. red light
47
Low frequency has ____________ wavelength & ___________ energy?
Long wavelength Low Energy ex. violet light
48
Node
where magnetic field & electric filed intersect at 0
49
light electromagnetic radiation
oscillating electric & magnetic field perpendicular to direction in which the light is propagating
50
Electric fields exert an influence on
particle changes
51
Magnetic fields exert an influence on
moving charged particles
52
Electromagnetic
has large range of wavelength & frequencies w/ no limit
53
Red light
Low frequency Long wavelength
54
Ultraviolet light
High frequency Short wavelength
55
Infrared light
corresponds to the heat we feel from a hot object
56
What did black body radiation, photoelectric effect, & atomic spectra prove?
Objects can't lose or gain energy in arbitrary or continuous amounts
57
Explain Black Body Radiation Experiment
put _______ into black body and w/ it bouncing off...examined color shift of BBR & demonstrated that the wavelength corresponds to the mas is INVERSELY proportional to the temp.
58
ex. of red hot and white hot heat
red hot = stove top burning white hot = incandescent bulb
59
Black body radiation is a function of
temp. & total intensity over all wavelengths is proportional to the power of temp.
60
max @ 1000K is shorter then that for
800K
61
Photons in a black box as an analogy for Oscillators
62
Black box
box that absorbs all photons incident upon it & re-radiates the photons till they reach thermal equilibrium
63
Ultraviolet Catastrophe
Any object @ non-zero temp. would emit intense ultraviolet radiation (even X-Rays) & would devastate the countryside - Breaks law of conservation of energy
64
Rayliegh's results
black body should emit an infinite amount of energy (breaks law of conservation of energy)
65
moles per unit frequency per unity volume eq.
8piv^2/c^3
66
increased frequencies you can fit _________ modes into the cavity
more because shorter wave lengths (2x frequency = 4x modes)
67
Basis for Classical Calculations
radiated photons (electromagnetic waves) can be considered to be produced by standing waves (resonant modes) in the cavity which is radiating
68
Standing waves
resonant modes
69
radiated photons
electromagnetic waves
70
BBR Classical Theory
intensity INCREASES as frequency INCREASES - that matter can absorb/emit any energy quantity - didn't predict region
71
BBR Experimental Results
max value of inensity exists as a function of wavelength
72
What would happen to humans in ultraviolet catastrophe?
Our bodies would glow in the dark but there wouldn't be any darkness to glow in
73
How must an oscillator gain & lose energy?
In quanta of magnitude h x frequency where H is plank's constant
74
Plank's Constant
6.63x10^-34 J s
75
Classical Oscillator
has CONTINUOUS values of energy and can gain or lose energy in arbitrary amounts (ramp)
76
Quantum Oscillator
has DISCRETE energy levels & can only gain & lose energy in discrete amounts (steps that can't be climbed if not enough energy to reach next level)
77
Low frequency oscillators have (occupied or unoccupied) levels?
Occupied energy levels
78
High frequency oscillators have (occupied or unoccupied) levels?
Unoccupied energy levels
79
What eq. shows radiation of frequency from oscillating atom releasing energy into its surroundings?
Frequency = energy / h
80
What is intensity of radiation?
energy packets generated by ind______ - measured in energy
81
Planks Hypothesis
radiation of frequency can only be generated if enough energy is available since atoms of a cool body don't have enough energy to generate a high frequency UV radiation (ultraV. cat. is avoided)
82
Planks Law deltaE: n: h: v: hv:
deltaE = nhv n: integer # h: 6.63x10^-34 v: radiation frequency hv: energy quanta
83
Photoelectric Cell (photocell) experiments by H. Hertz
ultraviolet radiation strikes a metal surface in vacuum & the ejected e- are attracted to (+) charged collector & a current flows
84
Photoelectric Effect Observations
1) max kinetic energy of e_ doesn't increase as intensity of light increases (more e- emitted) 2) no e- emitted unless radiation has frequency above threshold value characteristic of that meta 3) e- ejected immediately regardless of how low intensity of radiation 4) kinetic energy of ejected e- increase linearly w/ frequency of incident radiation
85
Red light shown onto metal: Low intensity purple light on metal: High intensity purple light on metal:
Red: frequency too low, no e- ejected from metal & no electric current flows Low purple: above threshold frequency so SOME e- ejected from metal; small current High purple: above threshold frequency so MANY e- ejected from metal; high current
86
Einstein said electromagnetic radiation consists of ___________?
Particles (photons) E=h x frequency
87
Photon
packets of energy related to frequency
88
Do photons of blue light or red light have higher energy?
Blue light photons
89
When energy of photon less the threshold, how does intensity effect e- ejection?
It doesn't...almost or far away are both not THERE
90
When energy of photons is more than threshold, what is excess energy and how does it effect ejected e-?
appears as Kinetic energy of the ejected e-
91
How does light eject e- from metal?
When light (photon particles) strikes metal, the energy is transferred to e-. If energy to e- is sufficient, it'll overcome the attractive forces & e- will be ejected.
92
How does light frequency effect photoelectron kinetic energy?
Linearly after threshold
93
How does light intensity effect photoelectron kinetic energy?
It's a constant
94
Work Function
barrier that e- must overcome to escape from surface (initial hv)
95
Kinetic Energy eq.
KE = hv - work function (initial hv) - intercept (work function) depends on metal but slope (h) is constant
96
hv in terms of KE & work function
hv = KE + work function
97
Kinetic energy of e-
.5m(sub e) v^2 + (initial hv)
98
E in terms of h and frequency
E = h/frequency
99

Chem Quiz #1 (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions