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Principles of Chemistry (Lecture) > Module 6: Quantum Mechanics > Flashcards

Module 6: Quantum Mechanics Flashcards

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1
Q

He extended the wave-particle duality of light that Einstein used to resolve the photoelectric-effect paradox to material particles

A

Louis de Broglie

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2
Q

he predicted that a particle should also exhibit the behavior of a wave

A

Louis de Broglie

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3
Q

Formula for de Broglie wavelength

A

λ = h / mV

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4
Q

Is de Broglie wavelength not a characteristic of particles?

A

No

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5
Q

two scientists that demonstrated experimentally that electrons can exhibit wavelike behavior

A

C.J. Davisson and L.H. Germer

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6
Q

Field of study that includes quantization of energy, wave-particle duality, and the Heisenberg uncertainty principle to describe matter

A

Quantum Mechanics

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7
Q

This principle states that it is fundamentally impossible to determine simultaneously and exactly both the momentum and the position of a particle

A

Heisenberg Uncertainty Principle

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8
Q

Unlike de Broglie who thought of the electron in terms of circular stationary waves, this person properly though in terms of three-dimensional stationary waves

A

Schrodinger

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9
Q

three-dimensional stationary waves that Schrodinger thought of

A

Wavefunction (ψ)

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10
Q

Who proposed the interpretation of wavefunction?

A

Max Born

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11
Q

he said that electrons are still particles and so the waves represented by ψ are not physical waves but are complex probability amplitudes

A

Max Born

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12
Q

the square of this describes the probability of the quantum particle being present near a certain location in space

A

Wavefunction (ψ)

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13
Q

It can be used to determine the distribution of the electron’s density

A

Wavefunction (ψ)

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14
Q

This describe the location or general description of an electron

A

Quantum numbers

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15
Q

A general region in an atom within which an electron is most probable to reside

A

Atomic orbital

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16
Q

The four quantum numbers

A

principal
angular momentum
magnetic
spin

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17
Q

this quantum number specify the shell an electron occupies in an atom

A

Principal quantum number (n)

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18
Q

this quantum number defines the location of the energy level and general size and energy of the orbital

A

Principal quantum number (n)

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19
Q

this quantum number determines the average distance form nucleus

A

Principal quantum number (n)

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20
Q

This quantum number’s values are 1, 2, 3, 4, ..

A

Principal quantum number (n)

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21
Q

As the principal quantum number (n), what happens to the distance from the nucleus and energy?

A

Increases

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22
Q

This quantum number defines the shape of the orbital which is dependent on where you can probably find electrons

A

Angular Momentum Quantum Number (l)

23
Q

This quantum number is also known as the subshell

A

Angular Momentum Quantum Number (l)

24
Q

This quantum number’s values are 0, 1, 2, (n-1)

A

Angular Momentum Quantum Number (l)

25
Q

This quantum number describes the orientation of the orbital in space

A

Magnetic Quantum Number (ml)

26
Q

This quantum indicates the region that an electron occupies within a subshell based on the shape of the subshell

A

Magnetic Quantum Number (ml)

27
Q

This quantum number’s values are 0, +1, -1, +2, -2, (-l to +l)

A

Magnetic Quantum Number (ml)

28
Q

This quantum number describes the orientation of electron spin

A

Spin Quantum Number (s)

29
Q

A completely quantum phenomenon with no analogous in the classic al realm

A

Electron spin

30
Q

Describes an intrinsic electron “rotating” or “spinning”

A

Electron Spin

31
Q

This quantum number states that each electron acts as atiny magnet with an angular momentum, even though this rotation cannot be observed in terms of the spatial coordinates

A

Spin Quantum Number (s)

32
Q

This quantum number’s values are either +1/2 or -1/2

A

Spin Quantum Number (s)

33
Q

Value of spin quantum number (s) with a slightly higher energy in an external field than the other

A

s = -1/2

34
Q

Principle that states no two electrons in the same atom can have exactly the same set of all the four quantum number

A

Pauli Exclusion Principle

35
Q

Which orbital have the lowest energy

A

Orbitals closest to the nucleus of an atom

36
Q

lowest to highest energy of subshells

A

s < p < d < f

37
Q

This is the arrangement of electrons in the orbitals of an atom

A

Electron Configuration

38
Q

Three information that an electron configuration have

A

Principal quantum number (n)
Orbital type (subshell ,l)
number of electrons in a particular subshell

39
Q

unpaired electrons that behave like a magnet and attract others

A

Paramagnetic

40
Q

Principle that states that the procedure in which the electron configuration of the elements is determined by “building” them in order of atomic number

A

Aufbau Principle

41
Q

Principle that states that lowest energy level should be filled up first before the higher energy levels

A

Aufbau Principle

42
Q

writing the electron configuration by abbreviation using the noble gas closest to the atom

A

Abbreviated Electron Configuration

43
Q

the electron occupying the inner shell orbitals

A

Core Electrons

44
Q

outer-shell electrons

A

Valence Electrons

45
Q

type of electrons that correspond to noble gases electron configuration

A

Core Electrons

46
Q

type of electrons that heavily contribute to an element’s properties and they are the electrons involved in chemical bonding

A

Valence Electrons

47
Q

pictorial representations of the electron configuration, showing the individual orbitals and the pairing arrangement of electrons

A

Orbital diagrams

48
Q

Electron configuration that is exceptions to the order of filling of orbitals that are indicated by Aufbau principle

A

Anomalous Electron Configuration

49
Q

for this type of electron configuration, half-filled and completely-filled subshells apparently represent conditions of preferred stability

A

Anomalous Electron Configuration

50
Q

electron configuration exceptions because the magnitude of the repulsion between electrons is greater than the differences in energy between subshells

A

Anomalous Electron Configuration

51
Q

meaning of s, p, d and f?

A

sharp
principal
diffused
fundamental

52
Q

formula for number of orbitals in a subshell

A

2l + 1

53
Q

formula for total number of orbital

A

n e2 (n squared)

54
Q

formula for maximum number of electrons

A

2n e2 ( 2 n squared)

Principles of Chemistry (Lecture) (7 decks)

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