Question 1

Which of the following statements best explains why the energy of a photon is inversely proportional to its wavelength?

Accepted Answer

Because as the wavelength increases, the frequency decreases, and energy is directly proportional to frequency by $E = h 
u$.

Question 2

A hydrogen atom emits light with a wavelength of $486\ \mathrm{nm}$ as an electron transitions from a higher energy level to a lower one. Which equation would you use to calculate the energy of the emitted photon?

Accepted Answer

$E = h c / \lambda$

Question 3

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

The azimuthal (angular momentum) quantum number $l$

Question 4

Which of the following electron configurations is NOT possible for a neutral atom in its ground state?

Accepted Answer

$1s^2\ 2s^2\ 2p^6\ 3s^2\ 3p^6\ 3d^2$

Question 5

Which element is most likely to violate the octet rule by having fewer than eight electrons in its valence shell?

Accepted Answer

Boron

Question 6

Which of the following best describes the trend in atomic radius across a period from left to right in the periodic table?

Accepted Answer

Atomic radius decreases due to increasing effective nuclear charge.

Question 7

Which of the following ions has the largest radius?

Accepted Answer

$\mathrm{S}^{2-}$

Question 8

Which of the following statements about electronegativity is correct?

Accepted Answer

Electronegativity increases across a period and decreases down a group.

Question 9

Which of the following molecules is expected to have the largest dipole moment?

Accepted Answer

$\mathrm{HF}$

Question 10

Which of the following best explains why metals are good conductors of electricity?

Accepted Answer

Metals have delocalized valence electrons that can move freely throughout the lattice.

Question 11

Which of the following best describes the difference between ionic and covalent bonding?

Accepted Answer

Ionic bonding involves the transfer of electrons, while covalent bonding involves the sharing of electrons.

Question 12

Which of the following is the correct Lewis structure for carbon dioxide ($\mathrm{CO}_2$)?

Accepted Answer

O=C=O, with each O atom having two lone pairs

Question 13

A student is asked to write the formula for aluminum sulfate. Which of the following is correct?

Accepted Answer

$\mathrm{Al}_2(\mathrm{SO}_4)_3$

Question 14

Which of the following best describes the trend in ionization energy as you move down a group in the periodic table?

Accepted Answer

Ionization energy decreases because the outer electrons are farther from the nucleus and more shielded.

Question 15

Which of the following elements is most likely to form a $2+$ cation?

Accepted Answer

Magnesium

Question 16

Which of the following is the correct order of increasing metallic character?

Accepted Answer

O < Si < Mg < Na

Question 17

Which of the following best explains why noble gases are generally unreactive?

Accepted Answer

They have a complete valence shell, making them stable.

Question 18

Which of the following best describes the difference between a polar and a nonpolar covalent bond?

Accepted Answer

A polar covalent bond has unequal sharing of electrons due to a difference in electronegativity.

Question 19

Which of the following is the correct formal charge on the central atom in the Lewis structure of nitrate ion ($\mathrm{NO}_3^-$)?

Accepted Answer

Positive one (+1)

Question 20

Which of the following best explains why the second ionization energy of sodium is much higher than the first?

Accepted Answer

The second electron is removed from a stable, noble gas configuration.

General Chemistry Study Guide: Electronic Structure, Periodic Properties, and Chemical Bonding

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