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CHE 1211 Gen > Ch.6 Quantum Theory and Electronic Structure of Atoms > Flashcards

Ch.6 Quantum Theory and Electronic Structure of Atoms Flashcards

1
Q

What we commonly refer to as “light” is actually the visible portion of the ____ ___

A

Electromagnetic Spectrum

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2
Q

All light has certain common characteristics including…

A
  1. Wavelength
  2. Frequency
  3. Amplitude
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3
Q

This is the distance between two crests or two troughs of a wave.

A

Wavelength (λ)

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4
Q

This is the number of waves that pass a point per unit time.

A

Frequency (ν)

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5
Q

This is the distance between the midpoint and crest or trough of a wave.

A

Amplitude

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6
Q

Electromagnetic waves have both ____ and ____ components that are both mutually perpendicular and in phase.

A

electric

magnetic

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7
Q

When energy moves through space away from a source.

A

Radiation

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8
Q

What are the 2 types of radiation?

A

Ionizing from radioactive materials

Electromagnetic or light.

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9
Q

What is the unit of measure for frequency?

A

Reciprocal seconds s-1

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10
Q

This is a wave consisting of oscillations occurring perpendicular to the direction of energy transfer.

A

Transverse

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11
Q

What is the speed of light constant?

A

C= 3.00x10^8 m/s

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12
Q

Wavelength is expressed in what unit of measure?

A

m (meter)

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13
Q

How do you find wavelength? What’s the formula?

A

Wavelength=c/v
C= speed of light
V= frequency

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14
Q

Which type of wave has an electric field component and a magnetic field component?

A

Electromagnetic wave

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15
Q

The electric field component and magnetic field component of an electromagnetic wave have what two same components?

A
  1. The same wavelength and frequency
  2. The same speed
  3. Travel in mutually perpendicular planes
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16
Q

What does orthogonal mean?

A

Two things are 90 degrees to each other.

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17
Q

When identical waves having common origin, corresponding peaks and troughs at any instant are _____.

A

In phase

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18
Q

The double slit experiment was performed by whom? And what did it demonstrate?

A

Thomas Young

That light is a wave

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19
Q

A particle oscillating about an equilibrium point has energy levels that are continuous.

A

Classical Mechanics

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20
Q

Energy levels are quantized and they have discrete values.

A

Quantum mechanics

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21
Q

What is planks constant?

A

h= 6.63x10^-34 J/s

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22
Q

What is the formula for energy using planks constant?

A 
Energy= h * v
H= planks constant
V= frequency
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23
Q

Who is the originator of quantum theory?

A

Max Planck

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24
Q

An idealized solid emits electromagnetic radiation over a wide range of wavelengths when heated.

A

Blackbody radiation

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25
Q

Electrons are emitted from solids, liquids, or gases when they absorb energy from light.

A

The photoelectric effect.

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26
Q

Who discovered the photoelectric effect?

A

Heinrich Hertz

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27
Q

The minimum frequency at which electrons are ejected is called the what?

A

Threshold frequency

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28
Q

Photons behave as?

A

Waves and particles

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29
Q

What is the formula for energy of a photon?

A

Ephonton= hv/wavelength

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30
Q

Who proposed the special theory of relativity? And what is the formula?

A

Einstein

E=mc^2

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31
Q

E=mc^2 is called what?

A

Mass energy equivalence.

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32
Q

This is the concept that the mass of an object is a measure of its energy content.

A

mass energy equivalence

33
Q

Electromagnetic radiation exhibits wave properties and particulate properties.

A

The dual nature of light

34
Q

These are the emission of light only at specific wavelengths.

A

Line spectra

35
Q

This consists of bright lines in distinct parts of the electromagnetic spectrum.

A

Atomic spectra

36
Q

What was Bohrs experiment called?

A

Atomic line spectra.

37
Q

The electrons moves around the nucleus only in certain allowed circular orbits. It explains the experimental hydrogen line spectrum.

A

Bohrs Model

38
Q

This is the lowest possible energy state n=1

A

Ground state

39
Q

Excited states have n values of what?

A

2,3,4 etc.

40
Q

What is the formula for Bohrs ground state? It shows that the electron in the hydrogen atom can have energies given by this formula.

A

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

41
Q

n=1 is called ____ and is lowest in energy.

A

Ground state

42
Q

n=2,3,4 is called _____ and is highest in energy.

A

Excited States.

43
Q

Radiant energy absorbed by the atom causes the electron to move from the ground state to an excited state is called?

A

Absorption

44
Q

Radiant energy, a photon, is emitted when the electron moves from a higher energy excites state to a lower energy excites state, including the ground state. This is called?

A

Emission

45
Q

The electron gains energy and moves from a lower state to a higher state. This is?

A

Absorption

46
Q

The electron loses energy and moves from a higher stage to a lower state this is called?

A

Emission

47
Q

This shows the transitions that correspond to the experimental emission spectrum of hydrogen.

A

Orbit-Transition Diagram

48
Q

What is the formula used for emission or absorption of an electron?

A

E= -2.18x10^-18J(1/nf^2 - 1/ni^2)/hc

49
Q

This mans theory states that if waves of light act like particles, do particles act like waves? His equation replaces the speed of light (c) with the speed of the particle (v)

A

Broglie

50
Q

What is the formula for Broglie wavelength?

A

Wavelength= h/mu

M= mass of the electron
U= electrons velocity
51
Q

This principle states that there is a fundamental limitation to just how precisely we can know both the position, x, and momentum ,p=mu, of a particle at a given time.

A

Heisenberg uncertainty principle

52
Q

What is the formula for the u certainty principle?

A

Delta x= h/ 4(pie) x (m)(delta.u)

53
Q

This equation specified the possible energy states the electron can occupy in a hydrogen atom and identifies the corresponding wave functions.

A

Shrodingers equation

54
Q

Regions of high electron density represent what?

A

A high probability of locating the electron

55
Q

The energy states and wave functions are characterized by a set of______ _____, with which a comprehensive model of the hydrogen atom is constructed.

A

Quantum numbers.

56
Q

An atomic orbital has these three characteristics?

A
  1. Energy
  2. Distribution of electron density
  3. Probability of locating an electron
57
Q

In quantum mechanics, three quantum numbers are required to describe what in an atom?

A

The distribution of electron density

58
Q

This quantum number has integer values of n=1,2,3…. like Bohr model.

A

Principal quantum number

59
Q

As n, the principal quantum number, increases what 3 things happen to the atom.

A
  1. The orbital becomes larger,
  2. The electron spends more time farther from the nucleus,
  3. The energy increases because the electron is less tightly bound.
60
Q

This quantum number describes the type and shape of the atomic orbital. It is given the letter l.
The l values are integers that depend on the value of the principal quantum number, n.

A

Angular momentum quantum number (l)

61
Q

For a given value if n, l ranges from 0 to what?

A

N-1

62
Q

The values of l are assigned letters… what are they? And how many orbitals are in each?

A

S- 1
P- 3
D- 5
F-7

63
Q

Where do the designations of s, p, d, and f come from?

A

Sharp
Principal
Diffuse
Fine

64
Q

A collection of orbitals with the same value of n is frequently called a ____?

A

Shell

65
Q

One or more orbitals with the same n and l values are referred to as a _____?

A

Subshell

66
Q

This quantum number describes the orientation of the orbital in space. Ml
Within the subshell the allowed values of m, range from -l to +l including 0.

A

Magnetic Quantum Number (Ml)

67
Q

What are the values of Ml?

A

2l+1

68
Q

What does ml determine?

A

How much the energy of an electron is changed when a magnetic field is present.

69
Q

This quantum number is necessary to describe electrons that occupy the orbital. Electrons possess a magnetic field as if they were spinning. Ms

A

Electron spin quantum number.

70
Q

There are ___ possible directions of electron spin. So Ms has ___ values.

A

2

2

71
Q

What are the two values of Ms referred to as?

A

+1/2 and -1/2 or spin-up and spin-down

72
Q

Two electrons in the same orbital with opposite spins are referred to as ______.

A

Paired.

73
Q

No two electrons in the same atom can have the same 4 quantum number according to what principle?

A

Pauli exclusion principle

74
Q

This principle makes it possible to “build” the periodic table of the elements and determine their electron configurations in a stepwise manner. Each step involves adding one proton to the nucleus and one electron to the appropriate atomic orbital.

A

Aufbau principle

75
Q

1s^1

Which does each denote?

A

1- principle quantum number, n
S- angular momentum quantum number,l
^1- number of electrons in the orbital or subshell

76
Q

According to _____ rule, the most stable arrangement of electrons in orbitals of equal energy is the one in which the number of electrons with the same spin is maximized.

A

Hund’s Rule

77
Q
  1. Electrons will reside in the available orbitals of the lowest possible energy.
  2. Each orbital can accommodate a maximum of 2 electrons
  3. Electrons will not have paired spins in degenerate orbitals (orbitals with the same energy) if an empty orbital is available.
  4. Orbitals will fill in order
A

Electron configuration rules

78
Q

The electron configuration where the noble gas in brackets represents the electron configuration of the noble gas that most recently preceded the element in question.

A

Noble Gas Electron Configuration

CHE 1211 Gen (8 decks)

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