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General Chemistry 111 > Chapter 7 > Flashcards

Chapter 7 Flashcards

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1
Q

how has much of our understanding of the electronic structure of atoms came to be

A

as a result of the analysis of light emitted or absorbed by substances

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2
Q

what did Sir Isaac Newton discover about white light

A

that it can be broken down into components with different colors from red to violet by the action of a prism

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3
Q

properties of waves (maxwell)

A

suggested that light consists of “waves” and that the energy is spread over space like an oscillating liquid

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4
Q

amplitude

A

the max displacement (height of wave above the centerline)

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5
Q

wavelength

A

represented by lamda, is the peak-to-peak distance

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6
Q

frequency

A

represented by nu, the number of wavelengths that pass a given point in 1 second

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7
Q

units of frequency

A

are cycles per second (s-1) or hertz (Hz)

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8
Q

c

A

the speed of light (product of wavelength + frequency)

  • speed of a light wave in a vacuum is constant
  • c=3x10^8 ms-1
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9
Q

how are wavelength and frequency related

A

wavelength and frequency are inversly related

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10
Q

electromagnetic waves

A

all visible light consists of electromagnetic waves

  • there are oscillating electric and magnetic fields
  • these fields are perpendicular to the direction of the light
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11
Q

equation for electromagnetic radiation

A

c=(lamda)(nu)

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12
Q

electromagnetic spectrum

A

electromagnetic radiation has a large range of wavelengths and frequencies with no known limit

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13
Q

blue light

A

has a smaller wavelength but a smaller frequency

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14
Q

black body radiation

A

as a body is heated, it glows more brightly and the color of light it gives off changes from red through orange and yellow to white

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15
Q

incandescence

A

rhe emission of light (visible electromagnetic radiation) from a hot body due to its temperature

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16
Q

how did planck describe black body radiation

A
  • it is not possible to put any arbitrary amount of energy into an oscillator, the energy must be quantized
  • oscillator must gain and lose energy in “packets” or “quanta” of magnitude (hv) where h is plancks constant (6.63x10^-34
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17
Q

plancks constant

A

6.63x10^-34

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18
Q

oscillator

A

a machine that generated oscillating electric currents and voltages by nonchemical means

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19
Q

classical oscillator

A

has continuous valves of energy and can gain or lose energy in arbitrary amounts

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20
Q

formula for an oscillating atom releasing energy

A

E=hv

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21
Q

quantum oscillator

A

has discrete energy levels and can only gain or lose energy in discrete energy levels and can only gain or lose energy in discrete amounts

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22
Q

Heinrich Hertz

A

showed that electrons are ejected from a metal when it is exposed to ultraviolet radiation

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23
Q

photoelectric effect

A
  • if radiation frequency is less than the threshold value (Vo) of the metal, than no electrons are emitted no matter how intense
  • if radiation frequency is greater than or equal to the threshold value (Vo) than electrons are emitted
  • if increase intensity of light (more pockets of light) more electrons are emitted but there is no change to the max kinetic energy of the electron
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24
Q

Albert Einstein’s statements on light ect

A
  • light is quantizes as photons
  • light has properties of both waves and matter
  • neither the wave nor the particle view alone is a complete description of light (particle-wave duality of light)
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25
Q

particle-wave duality of light

A

neither the wave nor the particle view alone is a complete description of light

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26
Q

threshold value

A

a point in which a change is executed

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27
Q

can white light be seperated

A

yes, by a prism. and this produces a continuous range of colors which merge together

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28
Q

discharge tube

A

tube with a low pressure of gas, to which a high voltage is applied

29
Q

what happens when light is emitted from a gas in a discharge tube

A

the light is seperated by a prism but a continuous spectrum of colors is not observed and the spectrum consists of lines

30
Q

assumptions of the Bohr Model of the Atom

A
  • the electron moves in circular orbits about the nucleus with motion described by classical physics
  • only a fixed set of orbits are allowed and in these orbits, no energy is emitted (no death spiral) (electron falling into the nucleus)
31
Q

history of the principal quantum number (n)

A

bohrs theory gave the energies of these orbits as a function of a principal quantum number

32
Q

can electrons pass from one orbit to another

A

yes and when electrons pass from one orbit to another it is accompanied by discrete changes in energy (light is emitted or absorbed)

33
Q

why was the Bohr atom important

A

because it introduced the idea of quantized energy states for electrons in atoms

34
Q

3 shortcomings of Bohrs model of the atom

A
  • it cannot predict the energy levels and spectra of atoms and ions with more than one electron
  • it violates the heinsenberg uncertainty principle in that both position and momentum cannot be known exactly at the same time
  • bohrs theory was replaced by modern quantum mechanics in 1926
35
Q

behavior of electromagnetic radition as told by Einstein

A

suggested that electromagnetic radiation would behave like particles (photons) and eject electrons from a metal surface (photoelectric effect)

but

electromagnetic radiation also behaves like waves

36
Q

diffraction pattern

A

when 2 light waves interfere with eachother and may interfere constructively giving a bright line or destructively giving a dark region

37
Q

who proposed wave-particle duality

A

Louis de Broglie made a revolutionary proposition, saying that small particles of matter may at times display wave-like properties

38
Q

history of the circular standing wave

A

deBroglie recognized that the standing waves are examples of quantization and suggested that the electron in a Bohr orbit may be associated with a circular standing wave

39
Q

standing wave

A

also known as a stationary wave, is a wave which oscillates in time but whose peak amplitude does not move in space.

40
Q

circular standing wave

A

superimpose a sine wave on the radius r of your circle

41
Q

what 2 famous equations did de Broglie link to make his own equation

A

Einstein and Plancks, to show the relationship between the wavelength and momentum of the photon

42
Q

Louis de Broglie’s nobel prize

A

(1929) for his discovery of the wave nature of electrons and light=matter

43
Q

when are the wave properties of matter apparent

A

only for the very small masses of matter (electrons)

44
Q

Heisenberg’s Uncertainty Principle concluded . . .

A

-the wave-particle duality places a fundamental limitation on how precisely we can know the location and momentum of any object at the same instant in time

45
Q

why is the uncertainty principle important

A

because when the masses are as small as an electron. if not, the particles become fuzzy and cannot be localized`

46
Q

the schrodinger equation

A

wrote an equation that describes both the particle and wave nature of an electron (can only be used for the hydrogen atom)

47
Q

are there limits to wave function?

A

no, it stretches out to infinity so an atom has no boundaries

48
Q

boundaries of an atom

A

inside the “boundaries” of an atom, the electron has a specific probability of being located (typically 99%)

49
Q

the value of wave function is greatest . . .

A

nearest the nucleus, but rapidly decreases thereafter (never goes to zero tho)

50
Q

the probability of finding an electron in a shell is greatest

A

at some distance from the nucleus. this is the same difference that is calculated by Bohr for an electron orbit in his model

51
Q

atomic orbital

A

the wave function for an electron, it is described by 3 quantum numbers - n,l,m
-describes a region in space with a definite shape where there is a high probability of finding the electron

52
Q

n

A

principal quantum number (distance from nucleus)

53
Q

l

A

angular movement quantum number (shape of orbital)

54
Q

m1

A

magnetic quantum number (orientation of the orbital0

55
Q

4th quantum number

A

refers to the magnetic property of electrons

ms=spin quantum number

56
Q

principal quantum number (n)

A
  • quantum number in which the energy of an electron in an atom primarily depends
  • can have any positive value (1,2,3)
57
Q

the smaller the value of n

A

the lower the energy and the smaller the orbital

58
Q

orbitals with the same value for n

A

are said to be in the same shell (distance of e- from the nucleus)

59
Q

schrodinger equation

A

psi(wavefunction)= fn (n,l,m1)

60
Q

angular momentum quantum number (l)

A

distinguishes orbitals of a given shell, having different shapes
-shape of the volume of space that the electron occupies

61
Q

for every given value of n, l=

A

n-1

62
Q

l for n=1,2,3

A

=0 (s orbital)https://www.brainscape.com/decks/9348203/cards/quick?pack_id=16236168#
=1 (p orbital)
=2 (d orbital)

63
Q

why are orbitals labeled s,p,d,f

A

sharp, principal, diffuse, fundamentals (some poor darn fool)

64
Q

s orbital shape

A

spherical

65
Q

p orbital shape

A

has 2 lobes along a straight line through the nucleus, one lobe on either side

66
Q

d orbital shape

A

clover-shaped

67
Q

magnetic quantum number, m1

A

distinguishes orbitals of a given n and l, that is, of a given energy and shape but having different orientations

  • in each 1=1 subshell there are 3 p orbitals corresponding to m1=+1,0,-1
  • in each 1=2 subshell there are 5 d orbitals corresponding to m1=-2,-1,0,1,2
68
Q

spin quantum number, ms

A

refers to the 2 possible orientations of the spin axis of an electron
-ms=+1/2 or -1/2

69
Q

what does energy depend on in a single electron atom

A

energy only depends on principal quantum number n (En=-RH(1/n^2)

General Chemistry 111 (8 decks)

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