Q: A hydrogen atom undergoes a transition from $n = 7$ to $n = 2$. Which formula would you use to calculate the energy of the photon emitted?

$\Delta E = -2.18 \times 10^{-18} (1/n_f^2 - 1/n_i^2)$

Question 1

Which statement best describes the concept of wave–particle duality as it applies to electrons?

Accepted Answer

Electrons can behave as both particles and waves, depending on the experimental conditions.

Question 2

According to quantum mechanics, what does the principal quantum number $n$ primarily determine for an electron in an atom?

Accepted Answer

The energy level and size of the orbital.

Question 3

Which equation correctly relates the energy of a photon to its frequency?

Accepted Answer

$E = h 	imes v$

Question 4

A sodium metal surface requires $2.28 	imes 10^{-19}$ J of energy to eject an electron via the photoelectric effect. What is the minimum wavelength of light (in nm) that can cause this effect? (Use $h = 6.626 	imes 10^{-34}$ J·s and $c = 3.00 	imes 10^8$ m/s)

Accepted Answer

$\lambda = 873$ nm$

Question 5

Which phenomenon provides direct evidence for the wave nature of electrons?

Accepted Answer

Electron diffraction

Question 6

If the frequency of light is doubled, what happens to the energy of each photon?

Accepted Answer

It is doubled.

Question 7

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($l$)

Question 8

A green laser emits light with a wavelength of $515$ nm. What is the frequency of this light? ($c = 3.00 	imes 10^8$ m/s)

Accepted Answer

$5.83 	imes 10^{14}$ Hz

Question 9

Which statement about the emission spectrum of hydrogen is correct?

Accepted Answer

It consists of a few distinct lines, each corresponding to a specific electron transition.

Question 10

According to the Heisenberg uncertainty principle, which of the following is true?

Accepted Answer

Increasing the accuracy of position measurement decreases the accuracy of velocity measurement.

Question 11

Which equation gives the de Broglie wavelength of a particle?

Accepted Answer

$\lambda = h / (mv)$

Question 12

How many orbitals are present in the $n = 3$ principal energy level?

Accepted Answer

9

Question 13

Which quantum number is responsible for specifying the orientation of an orbital in space?

Accepted Answer

Magnetic quantum number ($m_l$)

Question 14

What is the maximum number of electrons that can occupy the $n = 2$ principal energy level?

Accepted Answer

8

Question 15

Which of the following best explains why ultraviolet light can eject electrons from a metal surface with greater kinetic energy than yellow light?

Accepted Answer

Ultraviolet light has a higher frequency and therefore higher photon energy.

Question 16

Which of the following is NOT a consequence of the quantum mechanical model of the atom?

Accepted Answer

It allows for the exact prediction of an electron's path around the nucleus.

Question 17

What is the total number of sublevels in the $n = 4$ principal energy level?

Accepted Answer

4

Question 18

Which quantum number describes the spin orientation of an electron?

Accepted Answer

Spin quantum number ($m_s$)

Question 19

A hydrogen atom undergoes a transition from $n = 7$ to $n = 2$. Which formula would you use to calculate the energy of the photon emitted?

Accepted Answer

$\Delta E = -2.18 	imes 10^{-18} (1/n_f^2 - 1/n_i^2)$

Question 20

Which statement about atomic orbitals is correct?

Accepted Answer

p orbitals have a dumbbell shape and are oriented along different axes.

The Quantum Mechanical Model of the Atom: Structure, Behavior, and Implications

Study Guide - Practice Questions

Study Guide - Flashcards