Molecular and Ionic Bonding Practice Questions
AP (Advanced Placement) · AP Chemistry · 141 free MCQs with instant results and detailed explanations.
141
Total
42
Easy
72
Medium
27
Hard
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Sample Questions from Molecular and Ionic Bonding
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Q1
Easy
Which of the following bonds is primarily ionic?
A.
NaCl
B.
H2
C.
CH4
D.
CO2
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Correct Answer: A
NaCl is primarily ionic because it forms from the transfer of an electron from sodium (Na) to chlorine (Cl), creating charged ions that attract each other.
Q2
Easy
Which of the following compounds contains both ionic and covalent bonds?
A.
NaHCO3
B.
H2O
C.
CH4
D.
CaO
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Correct Answer: A
NaHCO3 (sodium bicarbonate) contains ionic bonds between Na+ and HCO3- ions, and covalent bonds within the HCO3- ion itself. This makes it the only compound listed that exhibits both types of bonding.
Q3
Easy
What is the shape of a molecule with a central atom that has two bonded pairs and one lone pair of electrons?
A.
Trigonal planar
B.
Bent
C.
Linear
D.
Tetrahedral
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Correct Answer: B
A central atom with two bonded pairs and one lone pair results in a bent molecular shape due to the repulsion of the lone pair, which pushes the bonded pairs closer together.
Q4
Medium
Which of the following compounds has the highest ionic character?
A.
NaCl
B.
CH4
C.
H2O
D.
CO2
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Correct Answer: A
NaCl has the highest ionic character due to the large difference in electronegativity between sodium and chlorine, leading to significant ionic bonding.
Q5
Medium
What is the hybridization of the central atom in SF6?
A.
sp3d2
B.
sp3
C.
d2sp3
D.
sp2
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Correct Answer: A
The central atom sulfur in SF6 undergoes sp3d2 hybridization because it forms six sigma bonds with fluorine atoms, requiring six hybrid orbitals.
Q6
Medium
Which of the following molecules exhibits resonance?
A.
O3
B.
CH4
C.
NH3
D.
H2O
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Correct Answer: A
O3 (ozone) exhibits resonance because it can be represented by two different Lewis structures that contribute to its overall hybrid structure.
Q7
Medium
Which type of bond is primarily responsible for the high boiling point of water?
A.
Ionic bonds
B.
Covalent bonds
C.
Hydrogen bonds
D.
Metallic bonds
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Correct Answer: C
Hydrogen bonds are primarily responsible for the high boiling point of water, as they are strong intermolecular forces that require considerable energy to break.
Q8
Hard
When considering the molecular geometry of SF6, what hybridization is present in the sulfur atom?
A.
sp
B.
sp2
C.
sp3d2
D.
d2sp3
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Correct Answer: C
In SF6, the sulfur atom is surrounded by six fluorine atoms, leading to an octahedral shape. This requires hybridization involving six orbitals, which corresponds to sp3d2 hybridization.
Q9
Hard
Which of the following compounds has the highest lattice energy?
A.
LiBr
B.
NaCl
C.
MgO
D.
KCl
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Correct Answer: C
Lattice energy increases with the charge of the ions and decreases with the size of the ions. MgO has a higher charge (Mg²⺠and O²â») compared to LiBr, NaCl, and KCl, thus it possesses the highest lattice energy.
Q10
Hard
In which scenario would the molecular polarity of a molecule be affected the most?
A.
Changing the electronegativity of a central atom.
B.
Altering the molecular geometry from tetrahedral to trigonal planar.
C.
Increasing the number of non-bonding electron pairs on the central atom.
D.
Reducing the number of bonds in the molecule.
Show Answer & Explanation
Correct Answer: C
Increasing the number of non-bonding electron pairs on the central atom can significantly affect the shape of the molecule and thus its dipole moment, making it more polar. Non-bonding pairs repel more than bonding pairs, distorting the geometry.
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Molecular and Ionic Bonding â AP (Advanced Placement) AP Chemistry Practice Questions Online
This page contains 141 practice MCQs for the chapter Molecular and Ionic Bonding in AP (Advanced Placement) AP Chemistry. The questions are organized by difficulty â 42 easy, 72 medium, 27 hard â so you can choose the right level for your preparation.
Every question includes a detailed explanation to help you understand the concept, not just memorize answers. Take a timed quiz to simulate exam conditions, or practice at your own pace with no time limit.