Quantum Mechanics Flashcards

1
Q

The amount of radiant energy emitted by an object at a certain temperature depends on ___

A

wavelength (E = hc/λ) and E = nhf

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2
Q

Formula for the kinetic energy of an ejected electron (photoelectric effect)

A

KE = hf - W

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3
Q

Why does an electron not spiral into the nucleus of an atom?

A

The electron is allowed to occupy only certain orbits of specific energies (the energies are quantized)

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4
Q

Relation between circumference of an allowed orbit and wavelength of an electron

A

2(pi)r = nλ

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5
Q

Relation between particle and wave properties

A

λ = h/mv

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6
Q

Heisenberg Uncertainty Principle

A

Cannot know simultaneously the momentum and position of a particle with certainty
ΔxΔp≥h/4π

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7
Q

Ψ vs Ψ^2

A

Ψ depends on the location in space of a system
Ψ^2 is proportional to the probability of finding a particle in a certain region of space
- Defines the distribution of electron density in 3-D space around the nucelus

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8
Q

Atomic orbital

A

Wave function of an electron in an atom

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9
Q

Quantum numbers

A

Four numbers that describe the distribution of electrons in H and other atoms
- Principal, angular, magnetic, spin

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10
Q

Principal quantum number (n)

A
  • Corresponds to energy of an orbital (only in H)
  • Relates to the average distance of the electron from the nucleus in an orbital
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11
Q

Angular momentum quantum number (l)

A

Tells us the “shape” of the orbitals, depends on n
- has values from 0 to (n-1)

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12
Q

Magnetic quantum number (m_l)

A

Describes the orientation of the orbitals in space, depends on l
- if l = 0, m_l = 0
- for a value of l, there are (2l+1) integral values of m_l

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13
Q

Electron spin quantum number (m_s)

A

A spinning charge generates a magnetic field, causing an electron to behave like a magnet
- m_s has values of +1/2 or -1/2

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14
Q

What does the energy of an electron in an atom depend on? (4)

A
  • Angular momentum quantum number
  • Principal quantum number
  • Sum of orbital energies
  • Repulsion between electrons in these orbitals
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15
Q

Simplified electron configuration notation

A

(n, l, m_l, m_s)

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16
Q

Pauli exclusion principle

A

No two electrons in an atom can have the same set of four quantum numbers

17
Q

Paramagnetic substances

A

Contain net unpaired spins and are attracted by a magnet

18
Q

Diamagnetic substances

A

Do not contain net unpaired spins and are slightly repelled by a magnet

19
Q

Shielding effect

A

Reduces the electrostatic attraction between protons in the nucleus and the electron in the 2s or 2p orbital

20
Q

Hund’s rule

A

The most stable arrangement of electrons in subshells is the one with the greatest number of parallel spins

21
Q

First rule for assigning electrons to orbitals

A

Each shell/principal level of quantum number n contains n subshells

22
Q

Second rule for assigning electrons to orbitals

A

Each subshells of quantum number l contains (2l + 1) orbitals

23
Q

Aufbau principle

A

As protons are added one by one to the nucleus to build up the elements, electrons are similarly added to the atomic orbitals