Q: A sodium vapor lamp emits yellow light with a wavelength of 589 nm. What is the frequency of this radiation? (Speed of light $$c = 3.00 \times 10^8$ m/s)

$$5.09 \times 10$$^{14}$$\ \text{s}^{-1}$$

Q: Calculate the energy of a single photon of light with a frequency of $$4.69 \times 10$$^{14}$$\ \text{s}^{-1}$$. ($$h = 6.626 \times 10$$^{-34}$$ J·s)

$$3.11 \times 10$$^{-19}$$\ \text{J}$$

Q: Which equation correctly gives the energy of an allowed orbit in the Bohr model for hydrogen?

$$E = -2.18 \times 10$$^{-18}$$\ \text{J}\ \frac{1}{n^2$}$$

Q: A laser emits light at 528 nm. What is the energy of one photon of this light? ($$h = 6.626 \times 10$$^{-34}$$ J·s, c = 3.00$$ \times $$10^8 m/s)$$

$$3.76 \times 10$$^{-19}$$\ \text{J}$$

Question 1

A sodium vapor lamp emits yellow light with a wavelength of 589 nm. What is the frequency of this radiation? (Speed of light $$c = 3.00 	imes 10^8$ m/s)

Accepted Answer

$$5.09 	imes 10$$^{14}$$\ 	ext{s}^{-1}$$

Question 2

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

Accepted Answer

As wavelength increases, frequency decreases.

Question 3

Calculate the energy of a single photon of light with a frequency of $$4.69 	imes 10$$^{14}$$\ 	ext{s}^{-1}$$. ($$h = 6.626 	imes 10$$^{-34}$$ J·s)

Accepted Answer

$$3.11 	imes 10$$^{-19}$$\ 	ext{J}$$

Question 4

Which phenomenon provided evidence that light behaves as both a wave and a particle?

Accepted Answer

The photoelectric effect

Question 5

A hydrogen atom electron transitions from $$n=6 to$$ $$n=2. $$What is the sign of $$\Delta E$$ and what does it indicate?

Accepted Answer

$$\Delta E is $$negative; energy is emitted as a photon.

Question 6

Which equation correctly gives the energy of an allowed orbit in the Bohr model for hydrogen?

Accepted Answer

$$E = -2.18 	imes 10$$^{-18}$$\ 	ext{J}\ \frac{1}{n^2$}$$

Question 7

Which transition in a hydrogen atom would emit a photon with the highest energy?

Accepted Answer

From $$n=3 to$$ $$n=1$$

Question 8

The de Broglie wavelength of an electron is given by $$\lambda = \frac{h}{mv}. $$What happens to the wavelength if the velocity of the electron increases?

Accepted Answer

The wavelength decreases.

Question 9

Which set of quantum numbers is NOT allowed for an electron in an atom?

Accepted Answer

$$n=3,\ l=0,\ m_l=1,\ m_s=+\frac{1}{2}$$

Question 10

How many electrons can occupy the $$n=3$$ shell in an atom?

Accepted Answer

18

Question 11

Which of the following electron configurations represents a transition metal in its ground state?

Accepted Answer

[Ar] 4s2 3d6

Question 12

Which principle states that no two electrons in an atom can have the same set of four quantum numbers?

Accepted Answer

Pauli exclusion principle

Question 13

What is the condensed (noble-gas) electron configuration for calcium (Ca)?

Accepted Answer

[Ar] 4s2

Question 14

Which of the following ions is isoelectronic with neon (Ne)?

Accepted Answer

Mg$$^{2+}$$

Question 15

Which of the following best describes Hund’s Rule?

Accepted Answer

Electrons occupy degenerate orbitals singly before pairing.

Question 16

Which quantum number defines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 17

A laser emits light at 528 nm. What is the energy of one photon of this light? ($$h = 6.626 	imes 10$$^{-34}$$ J·s, c = 3.00$$ 	imes $$10^8 m/s)$$

Accepted Answer

$$3.76 	imes 10$$^{-19}$$\ 	ext{J}$$

Question 18

Which of the following transitions in a hydrogen atom would absorb the most energy?

Accepted Answer

From $$n=1 to$$ $$n=3$$

Question 19

How many unpaired electrons are present in the ground state of a nitrogen atom?

Accepted Answer

3

Question 20

Which of the following is the correct set of quantum numbers for a 3p electron?

Accepted Answer

$$n=3,\ l=1,\ m_l=0,\ m_s=+\frac{1}{2}$$

Chapter 6: Electronic Structure of Atoms – Mini-Textbook Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards