Q: A Mehrium atom has energy levels at $$1 \, \text{eV}$$, $$4 \, \text{eV}$$, and $$9 \, \text{eV}. $$What photon energies can be emitted by this atom?

$$3 \, \text{eV}$$, $$5 \, \text{eV}$$, and $$8 \, \text{eV}$$

Question 1

According to the Bohr model, why do electrons in atoms not spiral into the nucleus despite being attracted by the positive charge?

Accepted Answer

Because electrons occupy quantized energy levels and cannot exist between them.

Question 2

Which of the following best describes the emission spectrum of an element?

Accepted Answer

A unique set of bright lines at specific wavelengths corresponding to electron transitions.

Question 3

If an electron in an atom absorbs a photon and jumps from the ground state (1 eV) to the second excited state (9 eV), what is the energy of the absorbed photon?

Accepted Answer

$$ 8 \, 	ext{eV} $$

Question 4

Which color of visible light has the highest energy per photon?

Accepted Answer

Blue

Question 5

A heated gas emits photons at discrete frequencies. What would you observe if white light were shone through the same gas?

Accepted Answer

A continuous spectrum with dark lines at the same frequencies.

Question 6

Which process describes the emission of light by a material after it has absorbed energy and continues to emit light even after the excitation source is removed?

Accepted Answer

Phosphorescence

Question 7

Why do incandescent objects, like stars or bulbs, emit a continuous spectrum rather than discrete lines?

Accepted Answer

Because the interactions between neighboring atoms in a solid smear out the energy levels.

Question 8

Which lamp is more efficient for emitting visible light?

Accepted Answer

Fluorescent lamp

Question 9

A Mehrium atom has energy levels at $$1 \, 	ext{eV}$$, $$4 \, 	ext{eV}$$, and $$9 \, 	ext{eV}. $$What photon energies can be emitted by this atom?

Accepted Answer

$$3 \, 	ext{eV}$$, $$5 \, 	ext{eV}$$, and $$8 \, 	ext{eV}$$

Question 10

Which of the following best explains why each element has a unique emission spectrum?

Accepted Answer

Each element has a unique arrangement of quantized electron energy levels.

Question 11

Which of the following is NOT a source of excitation energy for electrons in an atom?

Accepted Answer

Spontaneous emission

Question 12

If a gas absorbs high-energy ultraviolet (UV) light, will it always emit UV light when it returns to lower energy levels?

Accepted Answer

No, because the atom can emit several lower-energy photons instead.

Question 13

Which of the following best describes fluorescence?

Accepted Answer

Emission of visible light after absorbing higher-frequency radiation such as UV.

Question 14

Which of the following statements about absorption and emission spectra is correct?

Accepted Answer

The absorption spectrum shows dark lines at the same wavelengths as the emission spectrum's bright lines.

Question 15

Which of the following is a real-world application of emission spectra?

Accepted Answer

Identifying elements in distant stars using their spectral lines.

Question 16

A light-emitting diode (LED) produces light when:

Accepted Answer

Electrons drop from a higher energy state to a lower energy state, releasing photons.

Question 17

Which of the following is an example of bioluminescence?

Accepted Answer

A firefly producing light through a chemical reaction.

Question 18

If an electron in an atom drops from the second excited state (9 eV) to the first excited state (4 eV), what is the energy of the emitted photon?

Accepted Answer

$$ 5 \, 	ext{eV} $$

Question 19

Which of the following photons is most likely to excite an electron from the ground state to the second excited state?

Accepted Answer

Blue photon

Light Emission and the Bohr Model: Atomic Spectra, Excitation, and Modern Light Sources

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