Chapter 6 Flashcards

1
Q

interference pattern

A

when light passes through two closely spaced slits

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2
Q

constructive interference

A

result of adding waves that are in phase

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3
Q

destructive interference

A

result of adding waves that are out of phase

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4
Q

speed of light (c)

A

3.00e8 m/s

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5
Q

speed of light equation

A

c = (wavelength)(frequency)
- (wavelength) = meters
- (frequency) = s^-1

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6
Q

blackbody radiation

A

when a solid is heated, it emits electromagnetic radiation over a wide range of wavelengths

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7
Q

Max Planck

A

suggested that radiant energy is only emitted or absorbed in discrete quantities or bundles

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8
Q

quantum (of energy)

A

smallest quantity of energy that can be emitted (or absorbed)

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9
Q

quantum theory formula

A

E = h(nu)
- E = energy in Joules
- nu = frequency
- h = Planck’s constant = 6.63e-34 Jxs

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10
Q

photoelectric effect

A

Einstein; electrons are ejected from the surface of a metal exposed to light of a certain threshold frequency

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11
Q

photons

A

Einstein proposed; light is a stream of particles

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12
Q

photon quantum theory equation

A

Photon = h(nu)
- where nu is at the threshold frequency

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13
Q

Heisenberg uncertainty principle

A

it is impossible to know simultaneously both the momentum and the position of a particle with certainty

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14
Q

Heisenberg uncertainty principle formula

A

(delta)x x (delta)p >= h/4(pi)
- (delta)x = uncertainty in position in meters
- (delta)p = uncertainty in momentum (mass x velocity)

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15
Q

Planck’s constant

A

6.63e-34 Jxs

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16
Q

Pauli exclusion principle

A

no two electrons can have the same four quantum numbers

17
Q

Electron configuration

A

describes how the electrons are distributed in the atomic orbitals

18
Q

Aufbau principle

A

electrons are added to the lowest energy orbitals first before moving to higher energy orbitals

19
Q

Bohr’s Theory of the hydrogen atom

A

All wavelengths of visible light are present in the emission spectra of sun light and a heated solid

20
Q

Line spectra

A

emission of light only at specific wavelengths

21
Q

Bohr showed that the energies of the electron in a hydrogen atom are given by the equation

A

En = -2.18x10^18J(1/n^2)

22
Q

Lowest energy state (n=1)

A

ground state

23
Q

The stability of the electron decreases…

A

as n increases

24
Q

n>1

A

excited state

25
Louis De Broglie
if light can behave like a stream of particles (photons), then electrons could exhibit wavelike properties.
26
According to deBroglie, electrons behave like
standing waves
27
The particle and wave properties are related by the following expression:
lambda = h/mu - m = mass (kg) - u - velocity (m/s)
28
Quantum numbers describe
the distribution of electron density in an atom
29
Principal quantum number
(n) - specifies size
30
Angular moment quantum number
(l) - specifies shape
31
Magnetic quantum number
(ml) - specifies orientation
32
s orbitals
spherical
33
p orbitals
hourglass shaped
34
d orbitals
two hourglasses
35
f orbitals
christmas lights
36
electron spin quantum number
(ms) - used to specify an electrons spin - either +1/2 or -1/2