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Chemistry R120 > Chapter 6 > Flashcards

Chapter 6 Flashcards

1
Q

What is an electronic structure?

A

arrangement and energy of electrons

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2
Q

What is electromagnetic radiation?

A

form of energy that has wave characterisitics and that propagates through a vacuum at the speed of light

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3
Q

What is the value for the speed of light?

A

c = 3.00 * 10^8 m/s

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4
Q

What are the 3 characteristics of waves?

A

peak | trough | wavelength

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5
Q

What is a wavelength (lambda)?

A

distance between 2 adjacent peaks or troughs

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6
Q

What is frequency (v)?

A

number of complete wavelengths, or cycles that pass a given point each second

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7
Q

What is the unit for frequency?

A

Hertz (Hz) = cycles per second

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8
Q

What velocity do all electromagnetic radiation travels at?

A

speed of light! 3.00*10^8 m/s

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9
Q

What length and unit does X-ray radiation have?

A

e-10 | Å angstroms

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10
Q

What length and unit do ultraviolet/visible radaition have?

A

e-9 | nanometer (nm)

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11
Q

What length and unit do infrared radiation have?

A

e-6 | micrometer (um)

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12
Q

What length and unit do microwaves have?

A

e-3 to e-2 | milimeter (mm) to centimeters (cm)

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13
Q

What length and unit do television/radio waves have?

A

1 meter (m)

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14
Q

What length and unit do radio waves have?

A

e3 | kilometer (km)

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15
Q

What are the 3 phenomenons of light?

A

blackbody radiation | photoelectric effect | emission spectra

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16
Q

What is blackbody radiation?

A

emisison of light from hot objects

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17
Q

Who is Max Planck?

A

explained energy by assuming that it comes in packets called “quanta”

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18
Q

What is quantum?

A

smallest quantity of energy that can be emitted or absorbed as electromagnetic radiation

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19
Q

What is the equation Planck proposed about energy?

A

E = h(Planck’s constant) v(frequency)

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20
Q

What is the value of Planck’s constant?

A

h = 6.626*10^-23 Js

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21
Q

Who explained the photoelectric phenomenon?

A

Einstein using quanta

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22
Q

What is the photoelectric effect?

A

the light (photon) has an energy (E=hv) that makes the electrons on the metal surface emit off of it

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23
Q

What is a photon?

A

particle of energy

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24
Q

What is a continuous spectrum?

A

continuous range of rainbow colors containing light of all wavelengths

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25
What is a spectrum?
produced when radiation from a polychromatic source is separated into component wavelengths
26
What is a line spectrum?
radiation of only specific wavelengths observed from energy emitted by atoms and molecules
27
What is the wavelength for VIOLET?
410 nm
28
What is the wavelength for BLUE?
434 nm
29
What is the wavelength for BLUE-GREEN?
486 nm
30
What is the wavelength for RED?
656 nm
31
Who is Johann Balmer?
discovered a simple formula relating the 4 wavelengths observed of the hydrogen spectrum to integers
32
Who is Johannes Rydberg?
Physicist that advanced Balmer’s formula
33
What is Balmer’s equation?
(1/lambda) = (Rh) ( (1/(nf^2)) - (1/(ni^2)) )
34
What is “Rh” in Balmer’s equation and what is its value?
Rydbergs constant | -2.18*10^-18 J
35
What are the 3 postulates that the Bohr atomic model is based on?
Electrons can only occupy certain orbits corresponding to certain energies | Electron in an orbit has an “allowed” energy won’t be radiated from the atom | Electron emits/absorbs energy when it moves energy states
36
What are the 3 limitations of the Bohr model?
Only works for hydrogen | Bohr assumed electron won’t fall into (+)nucleus when physics says it would | Circular motion is not wave-like in nature
37
What are the 2 ideas from the Bohr model that was incorporated into the current Atomic Model?
Electrons exist only in certain energy levels | Energy is involved when electron moves from one level to another
38
What is Bohr’s model of the atom?
Visualizes the electron moving in a physical orbit, like planets around the sun
39
What is the principal quantum number (n)
Describes the energy level of an orbital | n 1
40
What is the principal quantum number for the 1st allowed orbit?
n = 1
41
What is a ground state?
Lowest (most negative) energy state = where the electron is MOST STABLE
42
What is the excited state?
The higher energy state that the electron moved into (less negative energy) = electron is NOT stable
43
Who is Louis de Broglie?
Theorized that if light can have material properties, matter should exhibit wave properties = demonstrated the relationship between mass and wavelength
44
What is the relationship between mass and wavelength that de Broglie demonstrated?
lambda = (h) / (mass*velocity)
45
What is the equation for momentum?
mass*velocity
46
What are matter waves?
Describes the wave characteristics of material particles
47
Who is Werner Heisenberg?
Proposed that the dual nature of matter places a fundamental limitation on how precisely we can know both the location AND momentum of an object at a give instant
48
What was Heisenberg’s uncertainty principle?
States that it is impossible for us to know simultaneously both the exact momentum and the location of an electron in space
49
Who is Erwin Schrödinger?
Developed quantum mechanics
50
What is quantum mechanics?
equation that incorporates both the wave and particle nature of matter
51
What is a wave function?
Math functions solving for Schrödinger’s equation for the hydrogen atom
52
What is the symbol psi mean?
Solution for Schrödinger’s wave equation
53
What is (psi)^2?
Gives the electron density
54
What is electron density?
Probability of where an electron is likely to be at any given time
55
What is an orbital?
A set of wave functions, each having a characteristic shape and energy visualized as electron clouds
56
What are the 4 quantum numbers that the quantum mechanical model uses?
Principal quantum number | Angular momentum quantum number | Magnetic quantum number | Spin quantum number
57
What is the relationship between the principal quantum number (n) and orbital size?
n increases = orbital size increases = electron-nucleus distance increases = electron’s energy increases
58
What is the angular momentum quantum number (l)?
Defines the shape of the orbital
59
What are the values for the angular momentum quantum number (l)?
l = n-1 | 0-s ; 1-p ; 2-d ; 3-f
60
What is the magnetic quantum number (ml)?
each ml number describes a 3D orientation of the orbital
61
What are the values for the magnetic quantum number (ml)?
-l ml l | ie: l = 2 ml = -2, -1, 0, 1, 2
62
What is an electron shell?
Formed from orbitals with the same principal quantum number (n)
63
What is an electron subshell?
Different orbital types (s, p, d, f) within a shell
64
What is the spin magnetic quantum number (ms)?
Describes the orbital’s magnetic field which affects its energy; 2 electrons in the same orbital don't have the same energy
65
What are the values for the spin quantum number (ms)?
ms = -1/2 or +1/2
66
What are the 3 observations due to the restrictions on possible values for n < 4?
Shell with (n) consists of exactly (n) subshells | Each subshell has a specific number of orbitals | The number of orbitals in a shell is (n)^2
67
What is the shape and quantum numbers for an s-orbital?
Shape: sphere | l = 0 ; ml = 0
68
What are nodes?
Where there is zero probability ( psi^2 = 0) of finding an electron
69
What is radial probability density?
probability that the electron is at a specific distance from nucleus
70
What is radial probabiltiy function?
graph showing radial probability densities as a function of r (distance from nucleus)
71
What is the shape and quantum numbers for a p-orbital?
shape = dumbell (has 1 node in center) | l = 1 ; m = -1, 0, 1
72
What is the shape and quantum number for a d-orbital?
shape = four are a 4-leaf clover with one lobe in center, one is a dumbell with a donut on the middle near the node | l = 2 ; ml = -2, -1, 0, 1, 2
73
What is the shape and quantum number for a f-orbital?
shape = very complex | l = 3 ; ml = -3, -2, -1, 0, 1, 2, 3
74
What are degenerate orbitals?
orbitals with the same energy (like 3p by itself is a degenrate orbital)
75
What is the relationship between orbital energy and (l) for any given (n)?
as (l) increases = orbital energy increases
76
Order the spdf orbitals from low to high orbital energy
s < p < d < f
77
What is electron spin?
electron behaves as if it were spinning on an axis = creating a magnetic field
78
What is the Pauli exclusion principle?
states that no 2 electrons in the same atom have the same quantum number combination
79
Who discovered the Pauli exclusion principle?
Wolfgang Pauli
80
What does the Pauli exclusion principal conclude?
an orbital can only hold 2 electrons that must have opposite spin
81
What are the 3 things each component of an electron configuration must consist of?
n, l orbital letter, and superscript ml (ie: 4s^2)
82
What is Hund's Rule?
states that when filling degenerate orbitals, LOWEST energy is attained when the orbital has both arrows (electrons) filled in | Fill up position first then down
83
What is the condensed electron configuration?
[noble gas] nl^(ml)
84
What are valence electrons?
electrons of outermost shell, involved in bonding
85
What are core electrons?
inner-shell electrons, noble gas core (noble gas before it)
86
What (n) do d-orbitals begin with?
3d
87
What (n) do f-orbitals begin with?
4f
88
What is the electron configuration for Ag?
[Kr] 5s2 4d10
89
What is the electron configuration for Cu?
[Ar] 4s2 3d10

Chemistry R120 (18 decks)

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