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Chemistry > CH 5 Electrons in Atoms > Flashcards

CH 5 Electrons in Atoms Flashcards

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1
Q

Bohr’s atomic model

A
  • physical model, upgrade from planetary
  • incorporated new discoveries into Rutherford’s nucleic model (like photoelectric effect)
  • based off of the simplest element, HYDROGEN**, didn’t explain those with more than one electron

theorized that…

  • electron is only found in specific orbits
  • each possible electron is quantized (has specific amount of energy
  • they must give off or gain a quantum in order to change their orbit
  • the electrons CLOSEST TO THE NUCLEUS ARE LOWER ENERGY, THE ELECTRONS FURTHEST ARE HIGH ENERGY
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2
Q

Schrödinger

A

*takes Bohr’s model from HYDROGEN to everything else

  • created quantum mechanical model EQUATIONS based off of later inconsistent evidence with Bohr’s model
  • ‘quantum mechanical model’ derived from equations
  • mathematical rather than physical
  • most modern description of atoms and their electrons
  • if you GRAPH equation, you make orbital shapes
  • like Bohr’s, electrons are quantized
  • UNLIKE Bohr’s, the path an electron takes around the nucleus is non-exact, and uses PROBABILITY that an electron is in any location (like windmill blades)
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3
Q

what are Bohr’s quantized orbits similar to?

A

PRIMARY ENERGY LEVELS, rungs on a ladder, unevenly spaced at times (need different quantums)

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4
Q

what couldn’t Rutherfords’ model explain?

A

the changing of physical properties elements underwent in fire, etc. (what we now know as chemical reactions, interaction of electrons)

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5
Q

electron cloud

A

represents the locations where an electron is likely to be found in a certain volume of space; it is not possible to know where one is in the cloud at any moment

  • high density= higher probability, low density= low probability
  • no boundary, as electron COULD be very far from nucleus, usually limited to location 90% of the time
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6
Q

solutions to schrödinger’s equation give…

A

the energy level an electron can have

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7
Q

Light calcs

A

E=hv

C=lambda v

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8
Q

Aufbau principle

A

electrons fill from lowest to highest energy level
(lowest energy first)
sublevel orbitals always equal (4s #1 = 4s #2)

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9
Q

Pauli Exclusion Principle

A

each orbital describes 2 electrons

must have opposite spins

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10
Q

Hund’s Rule

A

everyone gets one electron before anybody at the same energy level gets 2

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11
Q

issues w/ Rutherford’s model

A

doesn’t account for:

  • proton/e- attractions
  • metals changing color when heated (iron which is brown going from red to white)
  • solutions showing bright line spectrums when heated
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12
Q

define energy level

A

an area around the nucleus where orbitals exist

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13
Q

define orbitals

A

a place in an energy level where there is a chance of locating two electrons (technically electron cloud OF the nrg level)

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14
Q

define orientation

A

a different location of the orbital and their electrons

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15
Q

what is the difference between 1s v. 2s

A

2s occupies more volume, but can hold same number of electrons

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16
Q

what is the purpose of electron configuration exceptions?

A

to create a more stable atom

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17
Q

number of orbitals formula

A

n^2

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18
Q

number of electrons formula

A

2n^2

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19
Q

Hantaro Nagaoka

A

suggests that an atom has a central nucleus and that electrons move in rings like those of Saturn

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20
Q

Louis de Broglie

A

proposes that moving particles like electrons have some properties of waves

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21
Q

In a atom, electrons and the nucleus interact to…

A

make the most stable arrangement possible

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22
Q

the y axis of an aufbau diagram is

A

increasing energy

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23
Q

exceptions

A

column 6, 11

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24
Q

Isaac Newton

A

tried to explain behavior of light by assuming it consists of particles

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25
Q

by 1900, scientists had evidence that light was made of

A

WAVES

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26
Q

waves of light have certain properties

A

amplitude, wavelength, frequency

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27
Q

amplitude

A

height from zero to crest

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28
Q

frequency

A

m/s also Hz or s-1

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29
Q

wavelength

A

m

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30
Q

electromagnetic radiation

A

includes visible light, UV, X-rays, gamma

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31
Q

3.00 x 10^8 m/s (C)

A

speed of light

32
Q

when sunlight (white) passes through a prism…

A

it separates into a spectrum of colors

33
Q

violet light

A

400 nm -470 nm

34
Q

blue light

A

470 nm - 530 nm

35
Q

green light

A

530 nm - 580 nm

36
Q

yellow light

A

580 nm - 620 nm

37
Q

orange light

A

620 nm - 700 nm

38
Q

red light

A

700 nm

39
Q

radio

A

100-1 m

40
Q

micro

A

1^-1 to 1^-3

41
Q

infared

A

10^-4 to 10^-6

42
Q

UV

A

10^-7 to 10^-10

43
Q

x-rays

A

10^-11 to 10^-12

44
Q

gamma

A

10^-13

45
Q

atomic emission spectra

A 
BRIGHT LINE
(when an electric current is passed through an element, the electrons are energized, then emit light)
46
Q

when electrons gain energy

A

they move up to higher energy levels

47
Q

when electrons lose energy by emitting light

A

they return to lower energy levels

48
Q

regular light put through a prism creates a…

A

rainbow

49
Q

energized light (helium lamp) put through a prism creates an…

A

atomic emission spectrum made up by several specific lines of color

50
Q

no two element’s atomic emission spectra are

A

the same; therefore they can be used to identify elements (often used to analyze stars/astronomical bodies)

51
Q

scientists who discovered E=hv

A

Max Planck;
trying to understand color changes while heated, could explain if he assumed energy of a body changes in small discrete units (quanta)

*quantization of energy

52
Q

h, or 6.626 x 10-34 JxS is called

A

Planck’s constant

53
Q

the energy of a quantum equals

A

hv

54
Q

a small energy charge discharges or absorbs

A

low-frequency radiation

55
Q

a large energy change discharges or absorbs

A

high-frequency radiation

56
Q

_______ used Planck’s quantum theory to explain ____

A

Albert Einstein; the photoelectric effect

57
Q

the photoelectric effect

A

electrons are emitted when a specific light, at or above the threshold frequency, shines on a metal; classical physics (light=energy in waves) could not explain

58
Q

threshold frequency

A

the frequency a light must reach to emit electrons from a metal (photoelectric effect);
above it, the electrons travel faster

59
Q

Albert Einstein’s explanation of the photoelectric effect

A

he proposed that light could be described as quanta of energy that behave like particles, or PHOTONS quantized according to Planck’s forumla

60
Q

photons in a monochromatic (same frequency) beam have

A

the same energy

61
Q

electrons are ejected when

A

freuquency/energy are too low

62
Q

light behaves as

A

waves and particles

63
Q

when an electron has its lowest possible energy it is in its

A

ground state

64
Q

the step of an emission of an electron is also known as

A

electronic transition

65
Q

the light emitted by an electron moving from a HIGHER to a LOWER energy level has frequency ______ to the energy change of an electron.

A

DIRECTLY PROPORTIONAL

66
Q

this causes

A

the lines of specific frequency in an atomic emission spectrum

67
Q

Warner Heisenberg

A 
uncertainty principle
(we can know either velocity or location of electron, not either, since we must trap it an a magnetic field to find location)
68
Q

Bohr’s model explains the _______ of all atoms because______

A

atomic emission spectra; it predicts the quanta of energy (light) atoms give off as they jump between energy levels (energized)

69
Q

more closely spaced spectral lines mean

A

energy levels are closer together, occurs at increased values of n

70
Q

there is a limit to the frequency of emitted light because

A

with a high enough energy, the e- completely escapes atom

71
Q

Clinton Davisson and Lester Germer

A

confirmed de Broglie’s theory of matter waves by showing the reflections of electrons off of metals that acted like waves (caused by X-rays)

72
Q

wavelike properties of electrons are useful because_____

A

they are used in electron microscopes to show very small objects

73
Q

de Broglie’s equation

A

predicts that all moving objects have wavelike behavior, but mass must be very small for the wavelength to be large enough to observe (must travel at much higher velocity)
-set stage for new way to describe motion of subatomic particles…QUANTUM MECHANICS versus classical mechanics for big things, quantum is used on small things which act like waves and particles)

74
Q

atomic spectra are produced as

A

atoms emit light as excited electrons DROP DOWN in energy levels

75
Q

the leftmost atomic emission band show the

A

GREATEST energy change

76
Q

electromagnetic light in order of biggest to smallest wavelength

A

radio, micro, infared, UV, X-rays, gamma

Chemistry (9 decks)

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