$$\nu = \frac{c}{\lambda} = \frac{2.998 \times 10^8$}{725 \times 10$$^{-9}$$} = 4.14 \times 10$$^{14}$$\ \mathrm{s}^{-1}$$

Question 1

Which principle explains why fireworks display different colors when different elements are heated in a flame?

Accepted Answer

Each element emits photons of specific energies due to its unique electronic structure.

Question 2

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

Accepted Answer

$$E = h 
u$$

Question 3

A photon of red light has a wavelength of $$725\ \mathrm{nm}. $$What is its frequency? (Speed of light $$c = 2.998 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$
u = \frac{c}{\lambda} = \frac{2.998 	imes 10^8$}{725 	imes 10$$^{-9}$$} = 4.14 	imes 10$$^{14}$$\ \mathrm{s}^{-1}$$

Question 4

Which statement best describes the difference between a continuous and a line atomic spectrum?

Accepted Answer

A continuous spectrum contains all wavelengths, while a line spectrum contains only specific wavelengths emitted by atoms.

Question 5

According to Bohr’s model, what happens when an electron in a hydrogen atom absorbs a photon of energy $$E$$?

Accepted Answer

The electron moves to a higher energy orbit (excited state).

Question 6

Which of the following is NOT a limitation of the Bohr model of the atom?

Accepted Answer

It accurately predicts the line spectrum of hydrogen.

Question 7

De Broglie’s hypothesis states that particles such as electrons have wave-like properties. What is the equation for the wavelength of an electron?

Accepted Answer

$$\lambda = \frac{h}{mv}$$

Question 8

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 9

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

Accepted Answer

5

Question 10

Which statement about the Pauli Exclusion Principle is correct?

Accepted Answer

No two electrons in an atom can have the same set of all four quantum numbers.

Question 11

What is the condensed electron configuration for sodium ($$Z=11$$)?

Accepted Answer

$$[Ne] 3s^1$

Question 12

Which rule states that electrons fill degenerate orbitals singly before pairing up?

Accepted Answer

Hund’s Rule

Question 13

How many electrons can occupy the $$3d$$ subshell?

Accepted Answer

10

Question 14

Which quantum number describes the orientation of an orbital in space?

Accepted Answer

Magnetic quantum number ($$m_l)$$

Question 15

What is the maximum number of electrons that can occupy a single orbital?

Accepted Answer

2

Question 16

Which of the following electron configurations represents the ground state of carbon ($$Z=6$$)?

Accepted Answer

$$1s^2$$ $$2s^2$$ $$2p^2$$

Question 17

Which orbital diagram correctly represents the electron configuration of oxygen ($$Z=8) $$according to Hund’s Rule?

Accepted Answer

Two electrons paired in each of the $$1s$$ and $$2s$$ orbitals, and four electrons in $$2p$$ with two paired and two unpaired.

Question 18

Which of the following statements about $$s$$ orbitals is true?

Accepted Answer

$$s$$ orbitals are spherically symmetric and increase in size with increasing principal quantum number $$n.$$

Question 19

Which quantum number is responsible for the spin of an electron?

Accepted Answer

Spin magnetic quantum number ($$m_s)$$

Question 20

Which of the following best describes the uncertainty principle?

Accepted Answer

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

Electronic Structure of Atoms: Wave-Particle Duality, Quantum Mechanics, and Atomic Orbitals

Study Guide - Practice Questions