Quantum Theory & Electron Structure

Multiple Choice

Which of the following is NOT an example of electromagnetic radiation?

• Visible light

• Ultraviolet light (UV)

• Infrared (IR)

• Sound waves

Open Ended

Why is the study of quantum theory and the electronic structure of atoms significant in understanding modern technology and scientific advancements?

Multiple Choice

Which property of a wave is defined as the distance between identical points on successive waves?

• Amplitude

• Frequency

• Wavelength

• Speed

Open Ended

Explain how the speed of electromagnetic waves in vacuum is related to their wavelength and frequency.

Multiple Select

Select all the correct steps involved in converting frequency (ν) to wavelength (λ) for electromagnetic waves.

• Multiply frequency by speed of light

• Divide speed of light by frequency

• Multiply wavelength by frequency

• Convert meters to nanometers

Open Ended

A photon has a frequency of 6.0 x 10^4 Hz. Does this frequency fall in the visible region? Justify your answer.

Open Ended

Explain why classical physics could not explain the phenomena of black body radiation.

Multiple Choice

Which statement best describes black body radiation?

• It is the emission of light by heated objects, with energy dependent on frequency.

• It is the emission of light by cold objects, with energy independent of frequency.

• It is the emission of light by heated objects, with energy independent of frequency.

• It is the emission of light by cold objects, with energy dependent on frequency.

Multiple Choice

According to Planck's study of black body radiation, what two assumptions did he make to explain the energy spectrum?

• Energy is quantized and light has particle character (photons).

• Energy is continuous and light has wave character only.

• Energy is quantized and light has wave character only.

• Energy is continuous and light has particle character (photons).

Open Ended

What is the energy, in joules, of a single photon associated with a frequency of 7.5 x 10^14 Hz?

Multiple Choice

Which of the following equations can be used to calculate the wavelength of electromagnetic radiation given its frequency?

• λ = c / ν

• λ = h / ν

• λ = ν / c

• λ = h × ν

Multiple Choice

Which equation describes the relationship between the energy of a photon, the kinetic energy of an ejected electron, and the work function in the photoelectric effect?

• KE = hv + W

• hv = KE + W

• KE = hv × W

• hv = KE - W

Open Ended

Explain why cesium (Cs) will not emit electrons when exposed to light with a frequency less than 4.60 x 10^14 s^-1.

Multiple Choice

What is the photoelectric effect an evidence of?

• Wave nature of light

• Particle nature of light

• Continuous spectrum of light

• Refraction of light

Multiple Choice

Which of the following statements about continuous spectra is correct?

• Only a few wavelengths are present in continuous spectra.

• All wavelengths from 400 nm to 700 nm are present in continuous spectra.

• Continuous spectra only occur in cold objects.

• The intensity of all wavelengths is always the same in continuous spectra.

Open Ended

Compare and contrast continuous spectra and line spectra in terms of their origin and appearance.

Multiple Choice

Calculate the energy (in joules) associated with the photons if the wavelength of the X rays is 0.154 nm.

• 1.29 x 10^-15 J

• 2.00 x 10^-16 J

• 8.50 x 10^-14 J

• 6.63 x 10^-34 J

Open Ended

Explain how absorption spectra are formed and what information they provide about the sample being studied.

Multiple Select

Which of the following statements are true about atomic spectra?

• Every element has a unique spectrum.

• Spectra can be used to identify elements.

• All elements have the same spectrum.

• Spectra cannot be observed in stars.

Multiple Choice

Which group of elements in the bright-line spectra chart are classified as divalent metals?

• Alkaline Earth Elements

• Alkali Metals

• Gases

• Transition Metals

Open Ended

Describe the difference between the ground state and excited state of an electron in a hydrogen atom, and explain what happens when the electron returns to the ground state.

Multiple Choice

Which scientist is credited with the development of the orbitals in the Quantum Mechanical Model?

• Bohr

• Schrodinger

• Heisenberg

• Rutherford

Multiple Choice

How many orbitals does the p sublevel have?

• 1

• 3

• 5

• 6

Multiple Choice

Which orbital shows a violation of the Pauli Exclusion Principle?

• A
• B
• C
• D

Multiple Choice

Which orbital shows a violation of the Pauli Exclusion Principle?

• A

• B

• C

• D

Multiple Choice

Which energy level is higher than 5d?

• 7s

• 3d

• 3f

• 2d

Open Ended

How do you think the ability of electromagnetic radiation to travel through a vacuum impacts our daily lives or technology?

Multiple Choice

What are some examples of electromagnetic radiation mentioned in the lesson?

• Visible light, ultraviolet light (UV), and infrared (IR)

• X-rays, gamma rays, and microwaves

• Sound waves, water waves, and seismic waves

• Radio waves, microwaves, and sound waves