Q: A photon of green light has a wavelength of $$522\ \mathrm{nm}. $$What is its frequency? (Speed of light $$c = 3.00 \times 10^8$\ \mathrm{m/s})$$

$$5.75 \times 10$$^{14}$$\ \mathrm{Hz}$$

Q: What is the energy (in joules) of a photon with a wavelength of $$5.00 \times 10$$^{-2}$$\ \mathrm{nm}$$? (Planck's constant $$h = 6.63 \times 10$$^{-34}$$\ \mathrm{J\cdot s}$$, $$c = 3.00 \times 10^8$\ \mathrm{m/s})$$

$$3.98 \times 10$$^{-15}$$\ \mathrm{J}$$

Question 1

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 2

A photon of green light has a wavelength of $$522\ \mathrm{nm}. $$What is its frequency? (Speed of light $$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$5.75 	imes 10$$^{14}$$\ \mathrm{Hz}$$

Question 3

According to the Aufbau principle, which orbital will be filled first in a multi-electron atom?

Accepted Answer

$$1s$$

Question 4

Which of the following transitions in a hydrogen atom would emit light of the shortest wavelength?

Accepted Answer

$$n_i = 4 \rightarrow n_f = 2$$

Question 5

What is the maximum number of electrons that can be present in the principal level for which $$n = 3$$?

Accepted Answer

18

Question 6

Which of the following is a correct set of quantum numbers for an electron in a $$3d$$ orbital?

Accepted Answer

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

Question 7

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 8

A sodium atom ($$\mathrm{Na}) $$loses one electron to form $$\mathrm{Na}^+. $$What is the electron configuration of $$\mathrm{Na}^+$$?

Accepted Answer

$$1s^2$$ $$2s^2$$ $$2p^6$$

Question 9

Which of the following best describes the difference between a continuous spectrum and a line spectrum?

Accepted Answer

A continuous spectrum contains all wavelengths without gaps, while a line spectrum contains only specific wavelengths.

Question 10

What is the energy (in joules) of a photon with a wavelength of $$5.00 	imes 10$$^{-2}$$\ \mathrm{nm}$$? (Planck's constant $$h = 6.63 	imes 10$$^{-34}$$\ \mathrm{J\cdot s}$$, $$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$3.98 	imes 10$$^{-15}$$\ \mathrm{J}$$

Question 11

Which of the following ions is isoelectronic with neon ($$\mathrm{Ne}$$)?

Accepted Answer

$$\mathrm{Na}^+$$

Question 12

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

Accepted Answer

Hund's Rule

Question 13

What is the total number of orbitals associated with the principal quantum number $$n = 3$$?

Accepted Answer

9

Question 14

Which of the following elements has an anomalous electron configuration due to increased stability of half-filled or fully-filled $$d$$ orbitals?

Accepted Answer

Chromium (Cr)

Question 15

Which of the following statements about the quantum mechanical model of the atom is correct?

Accepted Answer

Electrons are found in orbitals, which are regions of high probability.

Question 16

How many electrons can be placed in the $$3d$$ subshell?

Accepted Answer

10

Question 17

Which of the following ions has the electron configuration $$[\mathrm{Ar}]3d$$^{10}$$?

Accepted Answer

$$\mathrm{Zn}^{2+}$$

Question 18

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

Accepted Answer

Magnetic quantum number ($$m_l)$$

Question 19

Which of the following substances is paramagnetic?

Accepted Answer

A substance with unpaired electrons

Quantum Theory and the Electronic Structure of Atoms: Study Notes

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