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Atomic Theory > Lesson 1 > Flashcards

Lesson 1 Flashcards

1
Q

Who introduced the concept that electrons behave both as particles and waves?

A

Louis de broglie

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2
Q

Which principles explain the filling order of electrons in atomic orbitals?

A

Aufbau principle

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3
Q

What shape is associated with the p-orbitals

A

Dumbbell-shaped

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4
Q

What quantum number specifies the orientation of an orbital in space

A

Magnetic quantum number ( ml)

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5
Q

According to the photoelectric effect, what determines the emission of electrons from a metal surface?

A

Frequency of light

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6
Q

The energy of an orbital in a hydrogen atom depends only on the principle quantum number (n).

A

True

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7
Q

Orbitals are fixed paths that electrons follow around the nucleus

A

False

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8
Q

According to Hund’s rule, electrons fill orbitals of the same energy single before pairing.

A

True

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9
Q

Diamagnetic substances have unpaired electrons

A

False

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10
Q

Quantum mechanics explains that the exact position of an electron cannot be determined.

A

True

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11
Q

Explain the key difference between Bohr’s model and the quantum mechanical model of the atom.

A

Bohr’s model proposed fixed circular orbits, while the quantum model describes probabilistic regions (orbitals)

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12
Q

Describe the significance of schrödinger’s wave equation in understanding atomic structures.

A

Schrödinger’s equation predicts the probability distribution of electrons

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13
Q

What is the madelung rule, and how does it apply to electron configuration.

A

Madelung’s rule explains the n+l, determining the orbital filling order.

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14
Q

What experimental observations led to the development of the photoelectric effect

A

Observations: electrons were emitted only above a certain light frequency.

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15
Q

Illustrate the process of writing the electron configuration for a transition metal ion (e.g. Fe 2+)

A

Remove electrons starting with the highest n: Fe [Ar] 4s2 3d6 —> Fe 2+: [Ar] 3d6

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16
Q

Which atomic model was the first to suggest that electrons have specific energy levels?

A

Bohr’s model

17
Q

What is the relationship between wavelength and frequency in electromagnetic waves?

A

Long wavelength corresponds to low frequency

18
Q

According to the relationship between wavelength and frequency, what happens to frequency as wavelength increases?

A

Frequency decreases

19
Q

What phenomenon does ultraviolet catastrophe illustrate?

A

Limitations of classical physics

20
Q

What is the relationship between energy and frequency and electromagnetic radiation?

A

Energy is directly proportional to frequency

21
Q

What type of radiation has a long wavelength?

A

Low frequency radiation

22
Q

What does the term ‘Quanta’ refer to in the context of energy?

A

Discrete packets of energy

23
Q

What happens to the energy of an object when it emits radiant energy?

A

It loses energy

24
Q

What statement is true regarding electromagnetic radiation?

A

All radiation has the same speed in a vacuum.

25
Q

What does the photoelectric affect demonstrate about energy transfer?

A

Energy is quantised

26
Q

What is the significance of the photoelectric effect in physics?

A

It led to the development of quantum mechanics

27
Q

What is the effect of increasing frequency on energy of radiation?

A

Energy increases

28
Q

Which of the following is a characteristic of electromagnetic radiation?

A

It can travel through a vacuum

29
Q

What does the term ultraviolet refer to in the electromagnetic spectrum?

A

Wavelength are shorter than visible light

30
Q

What does the atomic theory primarily describe?

A

The structure of subatomic particles

31
Q

Which theory describes the motion of electrons?

A

Wave theory

32
Q

What is the electromagnetic spectrum composed of?

A

Various wavelengths and frequencies

33
Q

What type of mechanics do subatomic particles are be?

A

Quantum mechanics

34
Q

What is the energetic content of electrons described as?

A

Quantised

35
Q

Which atomic model introduced the concept of electron clouds?

A

Modern atomic model

36
Q

What describes wave theory?

A

A model for electromagnetic radiation

37
Q

What do particles in the electromagnetic spectrum represent?

A

Different energies and frequencies

Atomic Theory (2 decks)

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