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BASCHEM Concepts > Quantum Theory, Quantum Mechanics > Flashcards

Quantum Theory, Quantum Mechanics Flashcards

1
Q

This theory states that that atoms or molecules emit energy in certain discrete quantities called “quanta or quantum.”

A

Quantum theory

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2
Q

Who proposed the quantum theory?

A

Max Planck

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3
Q

What is the equation for energy E of a single quantum of energy?

A

E = hv where (h) is called Planck’s constant and (v) is the frequency of radiation

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4
Q

A vibrating substance by which energy is transmitted

A

Wave

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5
Q

The distance between identical points on successive waves

A

Wavelength (λ ; lambda)

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6
Q

Number of waves that pass through a particular point in 1 s.

A

Frequency (ν ; nu)

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7
Q

Vertical distance from the midline of a wave to the peak or trough

A

Amplitude

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8
Q

The point at which the amplitude is zero

A

Node

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9
Q

It is defined as the product of wavelength and frequency (λν)

A

speed (u)

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10
Q

Defined as a wave with an electric and magnetic field components

A

Electromagnetic waves

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11
Q

Emission and transmission of energy in the form of electromagnetic waves

A

Electromagnetic radiation

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12
Q

What is the speed of electromagnetic waves (aka light)?

A

c = 2.99792458 × 10^8 / 3.0 x 10^8 m/s

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13
Q

Shortest waves with the highest frequency

A

Gamma rays

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14
Q

An interference that occurs when two waves are in phase/identical, resulting in a pattern made from the addition of the two waves

A

Constructive interference

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15
Q

An interference that occurs when two waves are out of phase, resulting in the perfect cancellation of the two waves

A

Destructive interference

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16
Q

Smallest quantity of energy that can be emitted or absorbed in the form of electromagnetic radiation

A

Quantum

17
Q

What is the value of Planck’s constant?

A

6.63 × 10^−34 J

18
Q

A phenomenon in which electrons are ejected from the surface of certain metals exposed to light of at least a certain minimum frequency

A

Photoelectric effect

19
Q

Below the threshold frequency no electrons were ejected no matter how intense the light

A

TRUE

20
Q

The number of electrons
ejected was proportional to the intensity (or brightness) of the light, but the energies of the
ejected electrons were not.

A

TRUE

21
Q

It is the particle of light, with an energy E using the same form as Planck’s equation

A

Photons

22
Q

The energy that binds the electrons in the metal

A

Work function Φ

23
Q

In the photoelectric effect, no electrons are ejected when the frequency of light is below the threshold frequency of a metal. When the frequency of light is above the threshold frequency, electrons are ejected with kinetic energy that increases with increasing frequency of light.

A

TRUE

24
Q

It is the state where an atom absorbs energy and its electrons form an orbit to another with a higher energy

A

Excited

25
Q

The state after an electron falls to an orbit of low energy / lowest energy state of a system

A

Ground state

26
Q

The more intense the light, the greater the
number of electrons emitted by the target metal; the higher the frequency of the light, the greater the kinetic energy of the ejected electrons

A

TRUE

27
Q

What is represented by the value 2.18 x 10^-18 J

A

Rydberg constant for the hydrogen atom

28
Q

How does Bohr’s model of the atom explain the line spectrum of hydrogen?

A

Bohr tells us that the electrons in the Hydrogen atom can only occupy discrete orbits around the nucleus (not at any distance from it but at certain specific, quantized, positions or radial distances each one corresponding to an energetic state of your H atom) where they do not radiate energy.

When the electron moves from one allowed orbit to another it emits or absorbs photons of energy matching exactly the separation between the energies of the given orbits (emission/absorption spectrum).

29
Q

The difference between the energies of the initial and final states is denoted by?

A

ΔE = Ef− Ei

30
Q

What is meant by the dual nature of an electron?

A

It can be considered both as a wave and as a particle

31
Q

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

A

Heisenberg Uncertainty Principle

32
Q

How does the Heisenberg principle contradict Bohr’s atomic model?

A

BASCHEM Concepts (4 decks)

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