AP Chemistry Quiz: Types Of Chemical Bonds

20 questions · exam conditions

0:00

Types Of Chemical BondsQuestion 1 of 20

Which of the following molecules contains both polar covalent bonds and nonpolar covalent bonds?

H_2O

C_2H_4

H_2O_2

CH_2Cl_2

← Back to quizzes

AP Chemistry Quiz

AP Chemistry Quiz: Types Of Chemical Bonds

Practice Types Of Chemical Bonds in AP Chemistry with focused quiz questions that help you check what you know, review explanations, and build confidence with test-style prompts.

What this quiz covers

This quiz focuses on Types Of Chemical Bonds, giving you a quick way to practice the rules, question types, and explanations that matter most for AP Chemistry.

How to use this quiz

Try each quiz question before looking at the correct answer. Use the explanations to review missed ideas, then come back to similar questions until the pattern feels familiar.

All questions

Question 1

Which of the following molecules contains both polar covalent bonds and nonpolar covalent bonds?

$H_2O$
$C_2H_4$
$H_2O_2$ (correct answer)
$CH_2Cl_2$

Explanation: To have both polar and nonpolar covalent bonds, a molecule must contain bonds between different atoms with a significant electronegativity difference (polar) and bonds between identical atoms (nonpolar). Hydrogen peroxide ( $H_2O_2$ ) has the structure H-O-O-H. The O-H bonds are polar covalent due to the electronegativity difference between oxygen and hydrogen. The O-O bond is nonpolar covalent because the two oxygen atoms have identical electronegativity.

Question 2

In aluminum metal, Al atoms are bonded through delocalized valence electrons that move throughout the solid. What type of bonding best describes solid aluminum?

Polar covalent
Metallic (correct answer)
Nonpolar covalent
Ionic
London dispersion

Explanation: This question tests the ability to identify the type of chemical bond in elemental metals. In solid aluminum, Al atoms are bonded via delocalized valence electrons in a metallic structure, allowing properties like ductility. This 'electron sea' model defines metallic bonding among metal atoms. Metallic bonds are distinct from covalent or ionic. A tempting distractor is ionic, but it is incorrect without anions, misconceptions arise from lattice similarities to ionic solids. Recognize metallic bonds in pure metals by their conductivity and electron delocalization.

Question 3

Which of the following properties of aluminum is primarily explained by the delocalized nature of its valence electrons?

Its low density compared to other metals such as lead or gold.
Its ability to be drawn into wires without breaking, which is known as ductility. (correct answer)
Its chemical reactivity, such as the formation of a protective oxide layer on its surface.
Its existence as a solid with a specific crystal structure at room temperature.

Explanation: The delocalized 'sea of electrons' model of metallic bonding explains properties like electrical conductivity, malleability, and ductility. Ductility is the ability to be drawn into a wire. This is possible because the metal cations can slide past one another within the electron sea without disrupting the overall metallic bonding. The delocalized electrons continue to hold the repositioned cations together. Density is related to atomic mass and packing, while chemical reactivity relates to electron configuration and ionization energy.

Question 4

The bonds in a certain compound have significant ionic character but are best classified as polar covalent. Which of the following pairs of atoms is most likely to form such a bond?

Na and F
Al and Cl (correct answer)
Cl and F
C and S

Explanation: The character of a bond exists on a continuum. While bonds between metals and nonmetals are often considered ionic, the electronegativity difference provides a more nuanced view. The electronegativity difference between Al (EN ≈ 1.6) and Cl (EN ≈ 3.2) is approximately 1.6. This value falls in the range typically classified as polar covalent, but it is large enough to imply significant ionic character. In contrast, Na-F has a very large electronegativity difference and is clearly ionic. Cl-F is polar covalent, and C-S is nearly nonpolar covalent.

Question 5

In $\mathrm{CH_4(g)}$ , the electronegativity of C is 2.5 and that of H is 2.1, so $\Delta EN = 0.4$ . Which classification best describes a C–H bond in methane?

Nonpolar covalent bond (correct answer)
Polar covalent bond
Ionic bond
Metallic bond
Hydrogen bond

Explanation: This question tests the skill of classifying bonds based on electronegativity differences. The electronegativity difference between C and H is 0.4, which is at the boundary between nonpolar and polar covalent bonds, but is typically classified as nonpolar covalent. In CH₄, the small electronegativity difference means electrons are shared nearly equally between carbon and hydrogen atoms, resulting in minimal polarity in each C-H bond. Students might incorrectly choose polar covalent bond (B) by strictly applying the ΔEN = 0.4 cutoff, but C-H bonds are conventionally treated as nonpolar due to their minimal dipole moment. When ΔEN is exactly 0.4 or very close to it, especially for C-H bonds, classify as nonpolar covalent.

Question 6

In carbon dioxide, the C–O electronegativity difference is about $1.0$ (C $\approx 2.5$ , O $\approx 3.5$ ), meaning each C–O bond shares electrons unequally. What type of bond best describes a C–O bond in $\text{CO}_2$ ?

Metallic
Hydrogen bonding
Polar covalent (correct answer)
Nonpolar covalent
Ionic

Explanation: This question tests the ability to identify the type of chemical bond based on electronegativity in linear molecules. In CO₂, each C-O bond has ΔEN ≈ 1.0, leading to unequal electron sharing and polar covalent character. The oxygen atoms pull electrons more, creating partial charges, though the molecule is nonpolar overall due to symmetry. Polar covalent bonds are defined by 0.5 < ΔEN < 1.7 in covalent sharing. A tempting distractor is nonpolar covalent, but it is incorrect due to the ΔEN, misconceptions come from confusing molecular polarity with bond polarity. Distinguish bond types by focusing on individual bond ΔEN, not overall molecule symmetry.

Question 7

In $\mathrm{F_2(g)}$ , each F atom has electronegativity 4.0, so $\Delta EN = 0.0$ for the F–F bond. Which classification best describes the bond in $\mathrm{F_2}$ ?

Polar covalent bond
Metallic bond
Ionic bond
London dispersion force
Nonpolar covalent bond (correct answer)

Explanation: This question tests the skill of identifying bond types when identical atoms bond. In F₂, both fluorine atoms have the same electronegativity (4.0), resulting in ΔEN = 0, which definitively indicates a nonpolar covalent bond. The electrons in the F-F bond are shared perfectly equally because neither atom can attract electrons more strongly than the other. Students might incorrectly choose polar covalent bond (C) by focusing on fluorine's extremely high electronegativity value, but polarity requires different atoms with different electronegativities. Remember that bonds between identical atoms are always nonpolar covalent, regardless of how electronegative those atoms are.

Question 8

In $\mathrm{NH_3(g)}$ , the electronegativity of N is 3.0 and that of H is 2.1, giving $\Delta EN = 0.9$ . Which classification best describes an N–H bond in ammonia?

Ionic bond
Polar covalent bond (correct answer)
Nonpolar covalent bond
Metallic bond
Hydrogen bond

Explanation: This question tests the skill of classifying bonds based on electronegativity differences. The electronegativity difference between N and H is 0.9, which falls in the range of 0.4 to 1.7, indicating a polar covalent bond. In NH₃, nitrogen's higher electronegativity causes it to attract the shared electrons more strongly than hydrogen, creating partial charges and making each N-H bond polar. Students might incorrectly choose nonpolar covalent bond (C) by underestimating the effect of a 0.9 electronegativity difference, but this clearly exceeds the 0.4 threshold for polarity. When ΔEN falls between 0.4 and 1.7, the bond is polar covalent with unequal electron sharing.

Question 9

A bond forms between nitrogen and oxygen in NO. The electronegativity values are approximately $EN(\text{N})=3.0$ and $EN(\text{O})=3.4$ , so $\Delta EN \approx 0.4$ . Which classification best describes the N–O bond?

Nonpolar covalent
Polar covalent (correct answer)
Ionic
Metallic
London dispersion

Explanation: This question tests the skill of classifying chemical bonds based on electronegativity differences. The N-O bond has ΔEN = 3.4 - 3.0 = 0.4, indicating unequal electron sharing that creates a polar covalent bond. Despite the relatively small electronegativity difference, oxygen's higher electronegativity causes electrons to spend more time near the O atom, creating partial charges (δ+ on N and δ- on O). This unequal distribution distinguishes polar covalent bonds from nonpolar ones. Students might incorrectly choose nonpolar covalent (A), thinking the small ΔEN makes the bond nonpolar, but any measurable electronegativity difference creates polarity in the bond. Remember that polar covalent bonds exist whenever 0 < ΔEN < 1.7, regardless of how small the difference might be.

Question 10

In carbon dioxide, one C–O bond has $\chi_\text{C}=2.5$ and $\chi_\text{O}=3.5$ (so $\Delta\chi\approx1.0$ ). Which best classifies each C–O bond in CO $_2$ ?

Nonpolar covalent
Ionic
Polar covalent (correct answer)
Metallic
Dipole–dipole attraction

Explanation: This question tests the skill of classifying bonds based on electronegativity differences between nonmetal atoms. The C-O bond has an electronegativity difference of 1.0, which falls within the range of 0.4 to 1.7, characteristic of polar covalent bonds. In polar covalent bonds, electrons are shared between atoms but unequally, with oxygen (the more electronegative atom) pulling electron density toward itself, creating a partial negative charge on O and partial positive charge on C. The bond is not ionic because both elements are nonmetals and the electronegativity difference is less than 1.7. Students might incorrectly choose nonpolar covalent (A), perhaps thinking all bonds between nonmetals are nonpolar, but the significant electronegativity difference creates polarity. To classify covalent bonds correctly, always check the electronegativity difference: bonds between nonmetals with 0.4 ≤ Δχ < 1.7 are polar covalent.

Question 11

In a diatomic molecule of chlorine, $\text{Cl}_2$ , the two atoms have the same electronegativity ( $\Delta EN = 0.0$ ). Which type of bond is present between the two chlorine atoms?

Nonpolar covalent (correct answer)
Polar covalent
Ionic
Metallic
Hydrogen bonding

Explanation: This question tests the skill of identifying bond types based on electronegativity differences. When two chlorine atoms bond in Cl₂, they have identical electronegativity values, resulting in ΔEN = 0.0, which means the electrons are shared equally between the atoms. According to bond classification rules, when ΔEN < 0.5, the bond is considered nonpolar covalent, making answer A correct. Students might incorrectly choose polar covalent (B) by confusing this with other chlorine-containing compounds like HCl, failing to recognize that identical atoms always form nonpolar bonds. The key strategy is to remember that homonuclear diatomic molecules (same element) always have ΔEN = 0 and therefore form nonpolar covalent bonds.

Question 12

In solid sodium chloride, NaCl, sodium transfers an electron to chlorine to form $\text{Na}^+$ and $\text{Cl}^-$ . Which classification best describes the bond between Na and Cl?

Polar covalent
Ionic (correct answer)
Nonpolar covalent
Metallic
Dipole–dipole

Explanation: This question tests the skill of classifying chemical bonds based on electron transfer and ion formation. In NaCl, sodium completely transfers its valence electron to chlorine, forming Na⁺ and Cl⁻ ions, which is the defining characteristic of an ionic bond. The large electronegativity difference between Na (≈0.9) and Cl (≈3.0) gives ΔEN ≈ 2.1, well above the typical 1.7 threshold for ionic bonding. The resulting oppositely charged ions attract each other through electrostatic forces in a three-dimensional lattice structure. Students might incorrectly choose polar covalent (A), confusing partial charge separation with complete electron transfer, but the formation of discrete ions clearly indicates ionic bonding. To identify ionic bonds, look for metal-nonmetal combinations with large ΔEN values and evidence of complete electron transfer forming ions.

Question 13

In hydrogen chloride, HCl, the electronegativity values are approximately $EN(\text{H}) = 2.2$ and $EN(\text{Cl}) = 3.0$ (so $\Delta EN \approx 0.8$ ). Which classification best describes the H–Cl bond?

Ionic
Nonpolar covalent
Polar covalent (correct answer)
Metallic
London dispersion

Explanation: This question tests the skill of determining bond type from electronegativity differences. The H-Cl bond has ΔEN ≈ 0.8, which falls in the range of 0.5-1.7, indicating a polar covalent bond where electrons are shared unequally. The chlorine atom attracts the bonding electrons more strongly than hydrogen, creating a partial negative charge on Cl and partial positive on H. Students might incorrectly choose ionic (A) by overestimating the electronegativity difference or thinking all metal-nonmetal bonds are ionic, not recognizing that H behaves as a nonmetal in bonding. The key strategy is to calculate ΔEN and apply the standard ranges: polar covalent bonds have moderate ΔEN values where electrons are shared but unequally.

Question 14

In nitrogen monoxide, NO, the electronegativity values are approximately $\chi_\text{N}=3.0$ and $\chi_\text{O}=3.5$ (so $\Delta\chi\approx0.5$ ). Which best classifies the bond between N and O?

Nonpolar covalent
Ionic
Metallic
Hydrogen bonding
Polar covalent (correct answer)

Explanation: This question tests the skill of classifying bonds based on electronegativity differences between nonmetal atoms. The N-O bond has an electronegativity difference of 0.5, which falls within the range of 0.4 to 1.7, characteristic of polar covalent bonds. In this bond, electrons are shared between the atoms but unequally, with oxygen (the more electronegative atom) pulling electron density toward itself, creating a partial negative charge on O and partial positive charge on N. The bond cannot be ionic because both elements are nonmetals and the electronegativity difference is well below 1.7. Students might incorrectly choose nonpolar covalent (A), perhaps thinking the small electronegativity difference makes the bond nonpolar, but any Δχ ≥ 0.4 between different atoms creates measurable polarity. To classify bonds accurately, remember that polar covalent bonds occur when 0.4 ≤ Δχ < 1.7, regardless of how small the difference seems.

Question 15

A bond forms between aluminum and chlorine in aluminum chloride, AlCl $_3$ . The electronegativity values are approximately $EN(\text{Al}) = 1.6$ and $EN(\text{Cl}) = 3.0$ (so $\Delta EN \approx 1.4$ ). Which classification best describes an Al–Cl bond?

Metallic
Ionic
Polar covalent (correct answer)
Nonpolar covalent
Hydrogen bonding

Explanation: This question tests the skill of classifying bonds with intermediate electronegativity differences. The Al-Cl bond has ΔEN ≈ 1.4, which falls in the polar covalent range (0.5-1.7), indicating unequal electron sharing rather than complete transfer. Despite aluminum being a metal, the electronegativity difference is not large enough for ionic bonding, resulting in polar covalent character with chlorine attracting electrons more strongly. Students might incorrectly choose ionic (B) by assuming all metal-nonmetal bonds are ionic, not recognizing that moderate ΔEN values indicate electron sharing rather than transfer. The strategy is to rely on calculated ΔEN values rather than metal/nonmetal classifications alone when determining bond type.

Question 16

In magnesium oxide, MgO, magnesium forms $\text{Mg}^{2+}$ and oxygen forms $\text{O}^{2-}$ in an ionic lattice. Which classification best describes the bond between Mg and O?

Metallic
Polar covalent
Ionic (correct answer)
Nonpolar covalent
Dipole–dipole

Explanation: This question tests the skill of classifying chemical bonds based on ion formation and electron transfer. In MgO, magnesium loses two electrons to form Mg²⁺ while oxygen gains two electrons to form O²⁻, demonstrating complete electron transfer characteristic of ionic bonding. The electronegativity difference between Mg (≈1.3) and O (≈3.4) gives ΔEN ≈ 2.1, well above the 1.7 threshold typically associated with ionic bonds. The resulting ions arrange in a crystal lattice held together by strong electrostatic attractions. Students might incorrectly choose polar covalent (B), not recognizing that the formation of discrete ions with full charges indicates ionic rather than covalent bonding. To identify ionic bonds, look for evidence of complete electron transfer, ion formation, and typically a metal bonded to a nonmetal with large ΔEN.

Question 17

A bond forms between fluorine and fluorine in F $_2$ . Because the atoms are identical, the bonding electrons are shared equally ( $\Delta EN = 0.0$ ). What is the bond type?

Polar covalent
Ionic
Metallic
Hydrogen bonding
Nonpolar covalent (correct answer)

Explanation: This question tests the skill of recognizing nonpolar covalent bonds between identical atoms. When two fluorine atoms bond in F₂, they have exactly the same electronegativity, resulting in ΔEN = 0.0 and perfectly equal electron sharing. This equal sharing defines a nonpolar covalent bond, making answer E correct. Students might incorrectly choose polar covalent (A) by thinking fluorine's high electronegativity makes all its bonds polar, not recognizing that polarity requires a difference in electronegativity between bonding atoms. The strategy is to remember that bonds between identical atoms (homonuclear bonds) always have ΔEN = 0 and are therefore always nonpolar covalent.

Question 18

In sulfur dioxide, the electronegativity difference for each S–O bond is about $1.0$ (S $\approx 2.5$ , O $\approx 3.5$ ), so electrons are shared unequally. What type of bond best describes an S–O bond in $\text{SO}_2$ ?

Metallic
Nonpolar covalent
Polar covalent (correct answer)
Ionic
Hydrogen bonding

Explanation: This question tests the ability to identify the type of chemical bond in bent molecules like SO₂. In SO₂, S-O bonds have ΔEN ≈ 1.0, leading to unequal sharing and polar covalent classification. Oxygen's higher electronegativity creates partial charges. Polar covalent fits nonmetal bonds with moderate ΔEN. A tempting distractor is ionic, but it is incorrect as SO₂ is molecular, misconceptions arise from high ΔEN but ignoring covalent nature. Differentiate by noting molecular vs. ionic compound properties alongside ΔEN.

Question 19

In $\text{CH}_4$ , the electronegativity difference for each C–H bond is small (C $\approx 2.5$ , H $\approx 2.1$ , so $\Delta EN \approx 0.4$ ), and electrons are shared nearly equally. What type of bond best describes a C–H bond in methane?

Polar covalent
Nonpolar covalent (correct answer)
Dipole–dipole
Ionic
Metallic

Explanation: This question tests the ability to identify the type of chemical bond based on small electronegativity differences in organic compounds. In CH₄, the C-H bonds have ΔEN ≈ 0.4, indicating nearly equal electron sharing, classifying them as nonpolar covalent. This small difference means minimal polarity, common in bonds between carbon and hydrogen. Nonpolar covalent bonds are typical when ΔEN < 0.5, resulting in symmetrical charge distribution. A tempting distractor is polar covalent, but it is incorrect for such low ΔEN, misconceptions arise from overestimating slight differences as significant polarity. Use ΔEN calculations and thresholds to differentiate nonpolar from polar covalent bonds accurately.

Question 20

In calcium fluoride, Ca forms $\text{Ca}^{2+}$ and each F forms $\text{F}^-$ . The compound consists of ions arranged in a crystal lattice. What type of bond best describes CaF $_2$ ?

London dispersion
Ionic (correct answer)
Nonpolar covalent
Polar covalent
Metallic

Explanation: This question tests the ability to identify the type of chemical bond in ionic compounds with polyatomic ions. In CaF₂, calcium transfers electrons to fluorine, forming Ca²⁺ and F⁻ ions in a crystal lattice, indicative of ionic bonding. The metal-nonmetal combination and high ΔEN support electron transfer. Ionic bonds lead to strong electrostatic attractions in solids. A tempting distractor is polar covalent, but it is incorrect for complete transfer, misconceptions stem from high ΔEN but ignoring ionic character. Use ion formation and lattice structure to identify ionic bonds in metal-nonmetal compounds.