AP Chemistry Unit 2 Practice Test 2025 (Compound Structure and Properties)

Last Updated on January 15, 2025

AP Chemistry Unit 2 Practice Test 2025 (Compound Structure and Properties). These are the sample questions and answers on the Unit 2: Compound Structure and Properties AP Chemistry exam. You can try both Multiple Choice Questions and Answers and Free-Response Questions. This unit is 7–9% of the Advanced Placement (AP) Exam score.

These multiple-choice questions are about Types of chemical bonds, Intramolecular force and potential energy, Structure of ionic solids, Structure of metals and alloys, Lewis diagrams, Resonance and formal charge, VSEPR and hybridization.

Table of Contents

AP Chemistry Unit 2 Practice Test

AP Chemistry Unit 2: Compound Structure and Properties

Total Items: 20 (Multiple Choice Questions)

Unit 2: Compound Structure and Properties

You’ll discover the range of chemical bonds and how their structure can affect the properties of the molecules created.

Topics may include:

Types of chemical bonds
Intramolecular force and potential energy
Structure of ionic solids
Structure of metals and alloys
Lewis diagrams
Resonance and formal charge
VSEPR and hybridization

On The Exam

7%–9% of exam score

1 / 20

Which of these molecules has a shape related to a tetrahedron (or has sp3 bonding)?

(A) CBr₄ and NH₃

(B) PF₅

(D) SO₃

2 / 20

Which of these molecules has the largest bond angle?

(A) HCN

(B) PF₅

(D) SO₃

3 / 20

The observation that the bond lengths found in the nitrate ion are equal is due to

(A) resonance structures

(B) hybridization of the central atom

(D) the existence of lone pairs of electrons

4 / 20

Which of these molecules have all atoms lying in the same plane?

(A) CBr₄ and NH₃

(B) PF₅

(D) SO₃ and HCN

5 / 20

Which of the following molecules are paired correctly with their molecular geometry?

(A) PF₅, tetrahedron

(B) XeF₄, square planar

(D) SF₆, square pyramid

6 / 20

In which of the following are the elements listed in order of increasing electronegativity?

(A) Ba, Zn, C, Cl

(B) N, O, S, Cl

(D) K, Ba, Si, Ga

7 / 20

The difference in bond angles for SBr₂, PBr₃, and CBr₄ is due to

(A) the dissimilarity in bond polarity between the central atom and bromine

(B) the size of the central atom

(D) the variance in bond length and strength

8 / 20

Which of the following is a nonpolar molecule containing polar bonds?

(A) H—C ☰ C—H

(B) H—H

(D) F—Be—F

9 / 20

The following diagram is an incomplete Lewis structure

What does the complete Lewis structure for the diagram have?

(A) Both polar and nonpolar bonds

(B) At least one double bond

(D) At least one lone pair of electrons on each atom

10 / 20

Which of the following is NOT a linear structure?

(A) I₂

(B) I‾₃

(D) H₂S

11 / 20

The Lewis structure of the cyanide ion most closely resembles

(A) N₂

(B) O₂

(D) NO

12 / 20

In which of the following pairs are the two items NOT properly related?

(A) sp³ and 109.5°

(B) Trigonal planar shape and 120°

(D) Square planar shape and 120°

13 / 20

The nitrate ion, can be described by the following Lewis structures:

What does this diagram mean?

(A) Two nitrogen to oxygen bonds are single bonds and a third is a double bond.

(B) The nitrate ion can exist as three equal forms in equilibrium.

(D) The electrons are rapidly exchanged among the three forms.

14 / 20

Which of the following has a nonbonding pair of electrons on the central atom?

(A) BCl₃

(B) NH₃

(D) PF₅

15 / 20

Which of the following is true when the C=C and C≡C bonds are compared?

(A) The triple bond is shorter than the double bond.

(B) The double bond vibrates at a lower frequency than the triple bond.

(D) All of the above are true.

16 / 20

Why does a molecule of BF₃ have no overall dipole moment but a molecule of PF₃ does?

(A) The overall structure of BF3 is linear.

(B) The atomic radius of phosphorus is larger than the atomic radius of boron.

(D) BF3 does not have a symmetrical structure but PF3 does.

17 / 20

There are ___ sigma bonds and ___ pi bonds in the following compound

(A) 7, 2

(B) 6, 3

(D) 9, 0

18 / 20

The molecular shape (geometry) of a Cl₂CO molecule is ________.

(A) trigonal planer

(B) tetrahedron pyramidal

(D) bent

19 / 20

Sulfur forms the following compounds: SO₂, SCl₂, and SO $\frac23$ . Which form of hybridization is NOT represented by these molecules?

(A) sp

(B) sp²

(D) None of these

20 / 20

Which of the following is least related to the strength of a covalent bond?

(A) vibrational frequency

(B) bond order

(D) bond direction

Your score is

Free-Response Questions

Answer the following questions regarding the concepts and properties concerning the structure and geometry of molecular compounds.

(a) Diethyl ether, CH₃CH₂OCH₂CH₃, is a highly flammable liquid. It is a common solvent in many laboratories.

(i) Draw the Lewis structure for this compound. Identify the electron pairs and molecular geometry of the oxygen. Explain your response.

(ii) Explain using VSEPR theory why the bond angle for the C–O–C bonds are not at 180°.

(iii) Are there any polar bonds in this molecule? If so, indicate the positive and negative poles of each bond. Is this molecule polar or nonpolar? Defend your answer.

(b)

(i) Draw the Lewis structure for nitrogen trichloride, and determine its molecular geometry. Explain what hybrid orbitals are required to produce this structure.

(ii) Based on the structure of nitrogen trichloride, are the bonds in this molecule polar? If so, indicate the positive and negative poles in an appropriate manner. Explain your reasoning.

(iii) As seen in part (i), a molecule of nitrogen trichloride is possible. Is a molecule of nitrogen pentachloride possible? Justify your answer.

See also:

FREE AP Chemistry Practice Test 2025 Study Guide (PDF)

Unit Wise Practice Test