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

$$5.09 \times 10$$^{14}$$\ \mathrm{Hz}$$

Question 1

Which of the following statements best describes the relationship between wavelength ($$\lambda) $$and frequency ($$
u) $$for electromagnetic radiation traveling at the speed of light ($$c$$)?

Accepted Answer

$$c = \lambda 
u$$

Question 2

A sodium street lamp emits yellow light with a wavelength of $$589\ \mathrm{nm}. $$What is the frequency ($$
u) of $$this light? ($$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$5.09 	imes 10$$^{14}$$\ \mathrm{Hz}$$

Question 3

Which phenomenon could NOT be explained by the classical wave theory of light, but was explained by the quantum theory?

Accepted Answer

The photoelectric effect

Question 4

According to Planck’s hypothesis, the energy of a photon is given by which equation?

Accepted Answer

$$E = h 
u$$

Question 5

Which of the following best describes the Bohr model’s explanation for the emission of light by hydrogen atoms?

Accepted Answer

Electrons emit photons when they transition from higher to lower energy levels.

Question 6

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 7

How many possible values of the magnetic quantum number ($$m_l) $$are there for a $$d$$ orbital?

Accepted Answer

5

Question 8

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 9

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 10

Which of the following electron configurations represents a violation of Hund’s Rule?

Accepted Answer

$$1s^2$$\ $$2s^2$$\ $$2p^4$$\ with\ paired\ electrons\ in\ one\ 2p\ orbital\ and\ empty\ 2p\ orbitals

Question 11

Which of the following elements has the ground-state electron configuration $$[\mathrm{Ar}]\ 4s^2$\ 3d^6$?

Accepted Answer

Iron (Fe)

Question 12

Which of the following best describes the difference between core electrons and valence electrons?

Accepted Answer

Core electrons are in filled inner shells; valence electrons are in the outermost shell.

Question 13

Which of the following is a correct condensed electron configuration for bromine (Br, atomic number 35)?

Accepted Answer

$$[\mathrm{Ar}]\ 4s^2$\ 3d$$^{10}$$\ 4p^5$

Question 14

Which quantum number is associated with the orientation of an orbital in space?

Accepted Answer

Magnetic quantum number ($$m_l)$$

Question 15

Which of the following statements about the Heisenberg Uncertainty Principle is correct?

Accepted Answer

It is impossible to know both the exact position and exact momentum of an electron simultaneously.

Question 16

Which of the following elements is a lanthanide?

Accepted Answer

Cerium (Ce)

Question 17

Which orbital will fill first according to the Aufbau principle: $$4s or$$ $$3d$$?

Accepted Answer

$$4s$$

Question 18

Which of the following best describes the shape of a $$p$$ orbital?

Accepted Answer

Two lobes with a node between them

Question 19

A photon is emitted when an electron in a hydrogen atom transitions from $$n=4 to$$ $$n=2. $$Which of the following statements is true?

Accepted Answer

The energy of the photon equals the difference in energy between the two levels.

Electronic Structure of Atoms: Quantum Theory and Atomic Orbitals

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