Question 1

Which of the following best explains why Rutherford’s model of the atom was ultimately considered incomplete?

Accepted Answer

It predicted that electrons would continuously emit energy and spiral into the nucleus, causing atoms to collapse, which is not observed.

Question 2

What is the main difference between a continuous spectrum and a line spectrum as observed in atomic spectroscopy?

Accepted Answer

A continuous spectrum contains all wavelengths in a region, while a line spectrum contains only discrete wavelengths characteristic of an element.

Question 3

Why is the emission spectrum of hydrogen significant in the development of atomic theory?

Accepted Answer

It demonstrated that the energy of electrons in hydrogen is quantized, supporting Bohr’s model.

Question 4

Which of the following statements about Bohr’s model of the atom is correct?

Accepted Answer

Electrons travel in circular orbits with quantized energy levels around the nucleus.

Question 5

When an electron in a hydrogen atom transitions from a higher energy level to a lower one, what happens?

Accepted Answer

A photon of a specific energy (and wavelength) is emitted.

Question 6

Why can line spectra be used as 'fingerprints' to identify elements in unknown samples?

Accepted Answer

Each element has a unique line spectrum due to its specific electron energy levels.

Question 7

Which of the following best describes the process of spectroscopy?

Accepted Answer

The study of the absorption and emission of light by matter to determine properties of the source.

Question 8

A sodium atom and a magnesium atom both have electrons in the first, second, and third energy levels. Why do their emission spectra differ?

Accepted Answer

They have different numbers of protons, which affects the energy levels and electron transitions.

Question 9

Which of the following equations correctly represents the energy of a photon emitted during an electron transition in the Bohr model?

Accepted Answer

$$E = h 
u$$

Question 10

In the Bohr model, what is the maximum number of electrons that can occupy the second energy level of an atom?

Accepted Answer

8

Question 11

Which real-world application relies on the use of atomic line spectra?

Accepted Answer

Identifying the composition of stars using astronomical spectroscopy.

Question 12

What is the ground state of an atom?

Accepted Answer

The lowest possible energy state for an atom, with no excited electrons.

Question 13

Which of the following is a limitation of the Bohr model?

Accepted Answer

It cannot explain the line spectra of atoms with more than one electron.

Question 14

A student observes a spectrum with only a few bright lines at specific wavelengths. What type of spectrum is this, and what does it indicate?

Accepted Answer

A line spectrum, indicating the presence of specific elements.

Question 15

Which statement best summarizes the historical importance of the Bohr model?

Accepted Answer

It was the first model to include the quantization of energy in atoms, paving the way for modern atomic theory.

Question 16

Which of the following best describes what happens when an atom absorbs light?

Accepted Answer

An electron moves from a lower to a higher energy level.

Question 17

Why did Bohr–Rutherford diagrams become less useful for elements beyond the first 20 in the periodic table?

Accepted Answer

The diagrams became too complex due to the increasing number of electrons and energy levels.

Question 18

Which of the following is a correct statement about electron transitions and the emission of light?

Accepted Answer

Electrons emit light when they move from a higher to a lower energy level.

Question 19

Which equation represents the relationship between the energy of a photon and its frequency?

Accepted Answer

$$E = h 
u$$

Question 20

Which of the following best explains why the Bohr model was eventually replaced by more advanced atomic models?

Accepted Answer

It could not accurately predict the spectra of atoms with more than one electron.

Lesson 3.2: Bohr’s Model of the Atom and Atomic Spectra

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