BOHR ATOM

Multiple Choice

Why is the Bohr model important for understanding how atoms create light?

• Because it explains how electrons move in quantized energy levels and emit light when transitioning between them.

• Because it shows that electrons can move freely between any energy levels.

• Because it describes the shape of the atom.

• Because it explains chemical bonding in detail.

Open Ended

How does the quantization of electron orbits affect the energy levels that electrons can occupy in an atom?

Multiple Choice

Which of the following statements about quantum leaps and energy exchange is correct?

• Jumping to a higher energy level releases energy.

• Falling to a lower energy level requires energy absorption.

• Falling to a lower energy level releases energy as a photon.

• Jumping to a higher energy level emits a photon.

Multiple Choice

What happens when an electron falls from a higher energy level to a lower one?

• It absorbs a photon.

• It emits a photon.

• It splits into two electrons.

• It loses its charge.

Open Ended

Explain how the energy of a photon emitted or absorbed by an electron is calculated using the initial and final energy levels.

Open Ended

Describe the process and significance of calculating the wavelength of the photon emitted when an electron falls from n=4 to n=2 in a hydrogen atom.

Multiple Choice

What is the frequency of a photon with energy 4.084 × 10⁻¹⁹ J?

• 6.16 × 10¹⁴ Hz

• 3.00 × 10⁸ Hz

• 4.87 × 10⁻⁷ Hz

• 2.18 × 10⁻¹⁸ Hz

Multiple Choice

An electron in the n=3 state absorbs a photon with a wavelength of 1283.45 nanometers. To what energy level will the electron jump?

• n=4

• n=5

• n=6

• n=2

Open Ended

Explain the steps required to determine the final energy level of an electron after it absorbs a photon, using the information provided in the case study.

Multiple Choice

Which of the following transitions releases the most energy when an electron falls to a lower energy level?

• n=2 → n=5

• n=6 → n=4

• n=1 → n=3

• n=3 → n=1

Multiple Choice

Which of the following spectral series corresponds to electron transitions that end at n=2?

• Lyman Series

• Balmer Series

• Paschen Series

• Brackett Series

Open Ended

Describe how the final state of an electron's transition determines the region of the electromagnetic spectrum in which light is emitted, using the hydrogen spectral series as an example.

Open Ended

How does the concept of quantized electron orbits help us understand atomic structure and spectra?

Multiple Choice

How does the Bohr model explain the emission of light from a single atom?

• Electrons absorb energy and move to higher orbits, emitting light as they do so.

• Electrons transition from higher to lower energy levels, releasing energy as light.

• Atoms split into smaller particles, releasing light in the process.

• Electrons remain in fixed orbits and do not emit light.