Lecture 8: Electrons as Waves, Quantum Numbers Flashcards

1
Q

Limitations of the bohr model

A

-only works for 1 electron
-doesn’t explain quantized energy just assumes it true
-doesn’t explain why electrons don’t fall into nucleus

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2
Q

de broglie hypothesis

A

if light can have
wave/particle duality, can matter exhibit
wave/particle duality?

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3
Q

de broglie wavelength

A

Any moving mass has a wavelength λ =ℎ/𝑚v

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4
Q

Electron diffraction

A

electrons through crystal showed diffraction proving they are waves not just particles

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5
Q

electrons don’t fall into the nucleus because

A

they are waves

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6
Q

Waves that are bounded can form

A

standing waves

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7
Q

Heisenberg Uncertainty Principle

A

There is a fundamental limit on how accurately we can measure position and momentum simultaneously

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8
Q

Solutions to SCHRÖDINGER’s Wave Equation describe

A

allowed energy states of an electron in H

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9
Q

SCHRÖDINGER’s Wave Equation is the theoretical foundation for

A

quantizing the energy of electrons
= wave-particle duality

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10
Q

ψ describes

A

an allowed energy state

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11
Q

ψ2 describes

A

probability density (Orbital)

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12
Q

n

A

principle quantum number

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13
Q

L (special L)

A

angular momentum quantum number

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14
Q

ml (m subscript L)

A

magnetic quantum number

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15
Q

principle quantum number determines

A

size and energy of an orbital (shell)

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16
Q

angular momentum number describes

A

shape of an orbital (subshell)

17
Q

magnetic quantum number describes

A

orientation of an orbital

18
Q

ms (m subscript s)

A

spin quantum number

19
Q

spin quantum number describes

A

up or down spin of an electron