Q: A sodium street lamp emits yellow light with a wavelength of $$589\ \mathrm{nm}. $$What is the energy of a single photon of this light? (Use $$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J \cdot s}$$ and $$c = 3.00 \times 10^8$\ \mathrm{m/s})$$

$$3.38 \times 10$$^{-19}$$\ \mathrm{J}$$

Q: A metal has a binding energy ($$\phi) of$$ $$2.50 \times 10$$^{-19}$$\ \mathrm{J}. $$What is the minimum frequency of light required to eject an electron from this metal? ($$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J \cdot s})$$

$$3.78 \times 10$$^{14}$$\ \mathrm{Hz}$$

Question 1

Which of the following best describes the relationship between the wavelength ($$\lambda) $$and frequency ($$
u) of $$electromagnetic radiation?

Accepted Answer

They are inversely proportional; as wavelength increases, frequency decreases.

Question 2

A sodium street lamp emits yellow light with a wavelength of $$589\ \mathrm{nm}. $$What is the energy of a single photon of this light? (Use $$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J \cdot s}$$ and $$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$3.38 	imes 10$$^{-19}$$\ \mathrm{J}$$

Question 3

Which phenomenon provides evidence for the wave nature of electrons?

Accepted Answer

Electron diffraction

Question 4

A metal has a binding energy ($$\phi) of$$ $$2.50 	imes 10$$^{-19}$$\ \mathrm{J}. $$What is the minimum frequency of light required to eject an electron from this metal? ($$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J \cdot s})$$

Accepted Answer

$$3.78 	imes 10$$^{14}$$\ \mathrm{Hz}$$

Question 5

Which transition in a hydrogen atom emits light with the shortest wavelength?

Accepted Answer

$$n=3 \rightarrow n=2$$

Question 6

According to the Heisenberg Uncertainty Principle, which of the following statements is true?

Accepted Answer

The more precisely the position of an electron is known, the less precisely its velocity is known.

Question 7

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 8

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

Accepted Answer

9

Question 9

Which of the following best explains why atoms are depicted as roughly spherical?

Accepted Answer

The sum of all orbital shapes in an atom results in a roughly spherical distribution.

Question 10

A student observes a bright yellow color in a flame test. Which element is most likely responsible for this color?

Accepted Answer

Sodium

Question 11

Which of the following sets of quantum numbers is NOT allowed for an electron in an atom?

Accepted Answer

$$n=2,\ l=2,\ m_l=0,\ m_s=+\frac{1}{2}$$

Question 12

Which of the following best describes the difference between constructive and destructive interference?

Accepted Answer

Constructive interference results in a larger amplitude, destructive results in cancellation.

Question 13

The emission spectrum of hydrogen contains several lines. What does each line in the spectrum represent?

Accepted Answer

A transition of an electron between two specific energy levels.

Question 14

Which of the following equations correctly relates the energy of a photon to its wavelength?

Accepted Answer

$$E = \dfrac{hc}{\lambda}$$

Question 15

A baseball follows a predictable path when thrown, but an electron does not. This is best explained by:

Accepted Answer

Electrons exhibit indeterminate behavior due to the uncertainty principle.

Question 16

Which of the following statements about the principal quantum number ($$n) is $$correct?

Accepted Answer

It determines the size and energy of the orbital.

Question 17

How many possible values of the magnetic quantum number ($$m_l) $$are there for $$l=3$$?

Accepted Answer

7

Question 18

Which of the following best describes the phase of an orbital?

Accepted Answer

It refers to the sign of the wave function, which can be positive or negative.

Question 19

Which of the following is a correct statement about the number of nodes in an atomic orbital?

Accepted Answer

The number of nodes is equal to $$n - l - 1.$$

The Quantum-Mechanical Model of the Atom: Light, Electrons, and Atomic Structure

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