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Quizzes > Science > Chemistry

Ready to Master Polar vs Nonpolar Molecules? Take the Quiz!

Think you can solve these polarity practice problems? Jump in and find out!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art illustration for molecular polarity quiz on a golden yellow background

Are you curious whether propane carries a dipole? Ready to sharpen your chemistry skills? Dive into our polar vs nonpolar quiz and challenge yourself as you spot polar and nonpolar molecules! From answering "is propane a polar molecule" to tackling fun polarity practice problems, this interactive test reinforces electronegativity and molecular geometry, offering targeted polarity practice to cement skills in molecular shape and solubility applications. Perfect for students and future chemists, our friendly quiz turns learning into an adventure. Explore the molecular structure quiz and jump into this polar or nonpolar quiz now to boost your skills!

Which of the following is a polar molecule?
BeH2
CH4
CO2
H2O
Water (H2O) has a bent geometry and a significant electronegativity difference between oxygen and hydrogen, resulting in a net dipole moment. The two O - H bond dipoles do not cancel out. This makes H2O polar. For more details, see Electronegativity and Polar Bonds.
Which molecule is nonpolar?
HCl
NH3
CO2
H2O
Carbon dioxide (CO2) is linear with two equal C=O bond dipoles that point in opposite directions and cancel each other. This symmetry yields a net dipole moment of zero, making it nonpolar. Learn more at Molecular Polarity.
CH4 is classified as:
A nonpolar molecule
A polar molecule
An ionic compound
A metallic compound
Methane (CH4) has a tetrahedral shape with four identical C - H bonds symmetrically arranged around the central carbon. The equal sharing of electrons in these bonds results in no net dipole moment, making it nonpolar. See why CH4 is nonpolar.
Which central atom property largely influences molecular polarity?
Bond angles
Electronegativity difference
Atomic number
Molecular weight
Electronegativity difference between atoms determines how strongly electrons are pulled toward one atom, creating bond dipoles. Larger differences yield more polar bonds, which influence the overall molecular polarity based on geometry. Review at Electronegativity and Bond Polarity.
In a diatomic molecule of F2, how would you classify the bond?
Metallic
Polar covalent
Nonpolar covalent
Ionic
In F2, both atoms have identical electronegativity, so electrons are shared equally. This equal sharing of electrons characterizes a nonpolar covalent bond. For more info, see Nonpolar Covalent Bonds.
Which of the following molecules is polar?
CO2
CCl4
NH3
CH4
Ammonia (NH3) has a trigonal pyramidal shape due to its lone electron pair on nitrogen, which leads to an asymmetrical charge distribution and a net dipole moment. The lone pair also contributes to polarity. See NH3 Geometry and Polarity.
In HCl, which atom carries the partial negative charge (?-)?
H
Neither
Cl
Both equally
Chlorine is more electronegative than hydrogen and thus pulls the shared electron pair closer to itself, acquiring a partial negative charge. Hydrogen becomes ?+. More at Electronegativity Effects.
What is the molecular shape of ammonia (NH3)?
Tetrahedral
Bent
Trigonal planar
Trigonal pyramidal
Ammonia has three N - H bonds and one lone pair on nitrogen, resulting in a trigonal pyramidal shape under VSEPR theory. This geometry leads to a net dipole moment. Details at VSEPR and Shape.
Which molecule has a net dipole moment?
C2H2
CO2
C2H4
C2H5Cl
Chloroethane (C2H5Cl) is asymmetrical since one hydrogen is replaced by chlorine, creating an uneven electron distribution and a net dipole moment. Symmetrical molecules like CO2 and C2H2 have no net dipole. See Molecular Polarity in Organic Molecules.
What is the approximate H - O - H bond angle in a water molecule?
120°
104.5°
109.5°
90°
The bent geometry of water, due to two lone pairs on oxygen, compresses the bond angle from the tetrahedral 109.5° to about 104.5°. This contributes to its strong polarity. For more, visit Water Bond Angles.
Considering molecular geometry and bond polarity, which molecule is nonpolar?
CCl3F
CH3OH
CH2Cl2
CCl4
Carbon tetrachloride (CCl4) is tetrahedral with four identical C - Cl bond dipoles that symmetrically cancel out, resulting in no net dipole moment. Other listed molecules are asymmetrical and thus polar. Learn more at Polarity and Geometry.
Which of the following molecules is polar despite having two identical bonds on the central atom?
CCl4
CH2O
CO2
BeH2
Formaldehyde (CH2O) has two C - H bonds and one C=O bond. The double bond to oxygen is more polar than the C - H bonds, and the molecule is trigonal planar but asymmetrical in its substituents, yielding a net dipole. See Formaldehyde Polarity.
Among the following, which molecule has a net dipole moment approximately zero due to its symmetry?
CH2Cl2
SF6
H2S
NF3
Sulfur hexafluoride (SF6) has an octahedral geometry with six identical S - F bonds arranged symmetrically, so all bond dipoles cancel out. This results in no overall dipole moment. More at Octahedral Symmetry.
Which of the following phosphorus halides is nonpolar?
PCl3
PF5
PBr3
PF3
Phosphorus pentafluoride (PF5) adopts a trigonal bipyramidal geometry with five equivalent P - F bonds symmetrically arranged, leading to cancellation of bond dipoles. The other phosphorus halides listed are trigonal pyramidal and thus polar. Reference: PBery Symmetry Effects.
Which of the following molecules exhibits a seesaw molecular geometry and is polar?
PCl5
SF4
SF6
CH4
Sulfur tetrafluoride (SF4) has five regions of electron density: four bonding pairs and one lone pair, resulting in a seesaw shape. The asymmetry introduced by the lone pair gives SF4 a net dipole moment. More detail at Seesaw Geometry and Dipole.
Which stereoisomer of 2,3-dichlorobutane exhibits no net dipole moment due to an internal plane of symmetry?
(2R,3R)-2,3-dichlorobutane
(2R,3S)-2,3-dichlorobutane (meso)
(2S,3S)-2,3-dichlorobutane
Racemic mixture of enantiomers
The meso form ((2R,3S)-) of 2,3-dichlorobutane has an internal plane of symmetry that causes the two C - Cl bond dipoles to cancel. The enantiomeric pair ((2R,3R) and (2S,3S)) lacks this symmetry and is polar. See Meso Compounds and Polarity for a full discussion.
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Study Outcomes

  1. Understand Molecular Polarity Principles -

    Learn the fundamental concepts of electronegativity differences and molecular geometry that govern whether a molecule is polar or nonpolar.

  2. Analyze Molecular Structures -

    Examine various molecular shapes and bond orientations to predict the distribution of charge within a molecule.

  3. Apply Electronegativity to Predict Polarity -

    Use electronegativity values and bond dipoles to determine the overall polarity of compounds like propane and beyond.

  4. Distinguish Polar vs Nonpolar Molecules -

    Develop the ability to categorize molecules accurately by evaluating symmetry and dipole moments.

  5. Solve Polarity Practice Problems -

    Tackle a variety of polarity practice problems and quiz questions to reinforce your understanding and test your skills.

  6. Build Confidence in Identifying Molecule Polarity -

    Gain hands-on experience through a scored, interactive polar vs nonpolar quiz that sharpens your chemistry knowledge.

Cheat Sheet

  1. Electronegativity Difference Thresholds -

    The difference in electronegativity between two bonded atoms dictates bond polarity: <0.5 is nonpolar covalent, 0.5 - 1.7 is polar covalent, and >1.7 often indicates ionic character. For example, the O - H bond in water has a ΔEN of about 1.4, classifying it as polar (American Chemical Society resources). Memorize these ranges to tackle polarity practice problems confidently in your polar vs nonpolar quiz.

  2. VSEPR & Molecular Symmetry -

    VSEPR theory from university chemistry departments predicts shapes by electron-pair repulsions, revealing symmetry that can cancel dipoles. Linear CO₂ and tetrahedral CH₄ are nonpolar despite polar bonds, whereas bent H₂O maintains a net dipole. Practicing these geometries will help you answer "is propane a polar molecule?" and similar quiz questions with ease.

  3. Net Dipole Moment Concept -

    A molecule's overall polarity depends on the vector sum of individual bond dipoles: if vectors cancel, the molecule is nonpolar. The net dipole moment (μ, in Debye units) is zero for nonpolar molecules like N₂ and nonzero for polar ones like HCl. Mastering vector addition is essential for solving polarity practice problems in academic and ACS-certified assessments.

  4. Real-World Molecule Examples -

    Propane (C₃H₈) is nonpolar because its C - H bonds have minimal electronegativity difference and the hydrocarbon skeleton lacks a strong dipole (University of Minnesota Chem Dept). In contrast, ethanol (C₂H₅OH) is polar due to its O - H bond and bent hydroxyl group, highlighting how functional groups influence polarity. Use these examples to solidify your grasp of polar vs nonpolar molecules in quizzes and lab reports.

  5. Mnemonics & Polarity Practice Tips -

    Use the "FONClBrIS" mnemonic to recall the most electronegative elements (F, O, N, Cl, Br, I, S), spotting bond polarity swiftly (Royal Society of Chemistry). Combine flashcards of VSEPR shapes with dipole vector diagrams to reinforce your understanding of molecular symmetry and net dipole moments. Regularly challenge yourself with polarity practice problems to boost confidence before any polar or nonpolar quiz.

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