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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
Q

What is a spectrum?

A

produced when radiation from a polychromatic source is separated into component wavelengths

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26
Q

What is a line spectrum?

A

radiation of only specific wavelengths observed from energy emitted by atoms and molecules

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27
Q

What is the wavelength for VIOLET?

A

410 nm

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28
Q

What is the wavelength for BLUE?

A

434 nm

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29
Q

What is the wavelength for BLUE-GREEN?

A

486 nm

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30
Q

What is the wavelength for RED?

A

656 nm

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31
Q

Who is Johann Balmer?

A

discovered a simple formula relating the 4 wavelengths observed of the hydrogen spectrum to integers

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32
Q

Who is Johannes Rydberg?

A

Physicist that advanced Balmer’s formula

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33
Q

What is Balmer’s equation?

A

(1/lambda) = (Rh) ( (1/(nf^2)) - (1/(ni^2)) )

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34
Q

What is “Rh” in Balmer’s equation and what is its value?

A

Rydbergs constant | -2.18*10^-18 J

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35
Q

What are the 3 postulates that the Bohr atomic model is based on?

A

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

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36
Q

What are the 3 limitations of the Bohr model?

A

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
Q

What are the 2 ideas from the Bohr model that was incorporated into the current Atomic Model?

A

Electrons exist only in certain energy levels | Energy is involved when electron moves from one level to another

38
Q

What is Bohr’s model of the atom?

A

Visualizes the electron moving in a physical orbit, like planets around the sun

39
Q

What is the principal quantum number (n)

A

Describes the energy level of an orbital | n 1

40
Q

What is the principal quantum number for the 1st allowed orbit?

A

n = 1

41
Q

What is a ground state?

A

Lowest (most negative) energy state = where the electron is MOST STABLE

42
Q

What is the excited state?

A

The higher energy state that the electron moved into (less negative energy) = electron is NOT stable

43
Q

Who is Louis de Broglie?

A

Theorized that if light can have material properties, matter should exhibit wave properties = demonstrated the relationship between mass and wavelength

44
Q

What is the relationship between mass and wavelength that de Broglie demonstrated?

A

lambda = (h) / (mass*velocity)

45
Q

What is the equation for momentum?

A

mass*velocity

46
Q

What are matter waves?

A

Describes the wave characteristics of material particles

47
Q

Who is Werner Heisenberg?

A

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
Q

What was Heisenberg’s uncertainty principle?

A

States that it is impossible for us to know simultaneously both the exact momentum and the location of an electron in space

49
Q

Who is Erwin Schrödinger?

A

Developed quantum mechanics

50
Q

What is quantum mechanics?

A

equation that incorporates both the wave and particle nature of matter

51
Q

What is a wave function?

A

Math functions solving for Schrödinger’s equation for the hydrogen atom

52
Q

What is the symbol psi mean?

A

Solution for Schrödinger’s wave equation

53
Q

What is (psi)^2?

A

Gives the electron density

54
Q

What is electron density?

A

Probability of where an electron is likely to be at any given time

55
Q

What is an orbital?

A

A set of wave functions, each having a characteristic shape and energy visualized as electron clouds

56
Q

What are the 4 quantum numbers that the quantum mechanical model uses?

A

Principal quantum number | Angular momentum quantum number | Magnetic quantum number | Spin quantum number

57
Q

What is the relationship between the principal quantum number (n) and orbital size?

A

n increases = orbital size increases = electron-nucleus distance increases = electron’s energy increases

58
Q

What is the angular momentum quantum number (l)?

A

Defines the shape of the orbital

59
Q

What are the values for the angular momentum quantum number (l)?

A

l = n-1 | 0-s ; 1-p ; 2-d ; 3-f

60
Q

What is the magnetic quantum number (ml)?

A

each ml number describes a 3D orientation of the orbital

61
Q

What are the values for the magnetic quantum number (ml)?

A

-l ml l | ie: l = 2 ml = -2, -1, 0, 1, 2

62
Q

What is an electron shell?

A

Formed from orbitals with the same principal quantum number (n)

63
Q

What is an electron subshell?

A

Different orbital types (s, p, d, f) within a shell

64
Q

What is the spin magnetic quantum number (ms)?

A

Describes the orbital’s magnetic field which affects its energy; 2 electrons in the same orbital don’t have the same energy

65
Q

What are the values for the spin quantum number (ms)?

A

ms = -1/2 or +1/2

66
Q

What are the 3 observations due to the restrictions on possible values for n < 4?

A

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
Q

What is the shape and quantum numbers for an s-orbital?

A

Shape: sphere | l = 0 ; ml = 0

68
Q

What are nodes?

A

Where there is zero probability ( psi^2 = 0) of finding an electron

69
Q

What is radial probability density?

A

probability that the electron is at a specific distance from nucleus

70
Q

What is radial probabiltiy function?

A

graph showing radial probability densities as a function of r (distance from nucleus)

71
Q

What is the shape and quantum numbers for a p-orbital?

A

shape = dumbell (has 1 node in center) | l = 1 ; m = -1, 0, 1

72
Q

What is the shape and quantum number for a d-orbital?

A

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
Q

What is the shape and quantum number for a f-orbital?

A

shape = very complex | l = 3 ; ml = -3, -2, -1, 0, 1, 2, 3

74
Q

What are degenerate orbitals?

A

orbitals with the same energy (like 3p by itself is a degenrate orbital)

75
Q

What is the relationship between orbital energy and (l) for any given (n)?

A

as (l) increases = orbital energy increases

76
Q

Order the spdf orbitals from low to high orbital energy

A

s < p < d < f

77
Q

What is electron spin?

A

electron behaves as if it were spinning on an axis = creating a magnetic field

78
Q

What is the Pauli exclusion principle?

A

states that no 2 electrons in the same atom have the same quantum number combination

79
Q

Who discovered the Pauli exclusion principle?

A

Wolfgang Pauli

80
Q

What does the Pauli exclusion principal conclude?

A

an orbital can only hold 2 electrons that must have opposite spin

81
Q

What are the 3 things each component of an electron configuration must consist of?

A

n, l orbital letter, and superscript ml (ie: 4s^2)

82
Q

What is Hund’s Rule?

A

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
Q

What is the condensed electron configuration?

A

[noble gas] nl^(ml)

84
Q

What are valence electrons?

A

electrons of outermost shell, involved in bonding

85
Q

What are core electrons?

A

inner-shell electrons, noble gas core (noble gas before it)

86
Q

What (n) do d-orbitals begin with?

A

3d

87
Q

What (n) do f-orbitals begin with?

A

4f

88
Q

What is the electron configuration for Ag?

A

[Kr] 5s2 4d10

89
Q

What is the electron configuration for Cu?

A

[Ar] 4s2 3d10

Chemistry R120 (18 decks)

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