Lesson 3.1.3.6

3.1.3.6 Bond polarity Quiz: AQA Chemistry, Unit 1

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.1.3.6, Bond polarity: 20 multiple choice questions for the AQA Chemistry (7405), Unit 1: Physical chemistry, written with Revision Ninja.

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The 20 questions

  1. What is electronegativity?

    • A measure of the atomic radius of an element
    • The energy needed to remove an electron from an atom
    • The tendency of an atom to lose electrons in a reaction
    • The power of an atom to attract the bonding pair of electrons in a covalent bond

  2. Which element is the most electronegative?

    • Chlorine
    • Nitrogen
    • Oxygen
    • Fluorine

  3. Which symbols are used to show partial charges in a polar bond?

    • Q and -Q
    • + and -
    • delta+ and delta-
    • 2+ and 2-

  4. In a hydrogen chloride molecule, which atom carries the partial negative charge?

    • Both equally
    • Chlorine
    • Hydrogen
    • Neither

  5. Which molecule has polar bonds but no permanent dipole?

    • CO2
    • HCl
    • H2O
    • NH3

  6. What causes a covalent bond to be polar?

    • A difference in electronegativity between the bonded atoms
    • The presence of a lone pair on each atom
    • A difference in atomic mass between the atoms
    • Both atoms having identical electronegativities

  7. Which statement describes a polar covalent bond?

    • The electrons are fully transferred to one atom
    • The electron distribution is unsymmetrical, giving partial charges on the atoms
    • The electrons are not shared at all
    • The electrons are shared equally between the two atoms

  8. Which of these molecules is non-polar overall?

    • CH4
    • H2O
    • NH3
    • HCl

  9. Why is CCl4 non-polar overall, even though each C-Cl bond is polar?

    • The polar bonds cancel out because the molecule is symmetrical
    • CCl4 has no polar bonds
    • CCl4 has a lone pair on carbon
    • Chlorine is not electronegative

  10. Which bond is the most polar?

    • C-C
    • H-F
    • O-H
    • C-H

  11. Predict whether BF3 has a permanent dipole.

    • No, because BF3 has no polar bonds
    • No, the polar bonds cancel because the shape is trigonal planar
    • Yes, because fluorine has lone pairs in the bonds
    • Yes, because boron is electronegative

  12. Which way does the bond dipole point in hydrogen fluoride, HF?

    • From F towards H
    • Equally in both directions
    • Upwards only
    • From H towards F

  13. Which molecule has a permanent dipole: NH3, CH4, CO2 or SF6?

    • CO2
    • SF6
    • CH4
    • NH3

  14. Which bond is the most polar: C-N, C-O or C-F?

    • C-C
    • C-N
    • C-F
    • C-O

  15. In water, why does the molecule have a permanent dipole?

    • Its bonds are ionic
    • Its bent shape means the O-H bond dipoles do not cancel
    • Its linear shape makes the two dipoles add
    • Its bonds have equal electronegativities

  16. Why does NH3 have a permanent dipole?

    • NH3 has no polar bonds
    • Its lone pair and polar N-H bonds are arranged asymmetrically, so the dipoles do not cancel
    • Nitrogen is less electronegative than hydrogen
    • The dipoles cancel because it is symmetrical

  17. Which statement about polar molecules is correct?

    • Polar molecules have no net dipole
    • A molecule can have polar bonds but no permanent dipole if the bond dipoles cancel
    • Every molecule with polar bonds has a permanent dipole
    • Non-polar bonds always create permanent dipoles

  18. Why is the bond in Cl2 non-polar?

    • Cl2 has no electrons in its bond
    • Chlorine is not electronegative
    • Both atoms have the same electronegativity, so the bonding pair is shared equally
    • Cl2 has ionic bonds

  19. Which hydrogen halide would have the largest permanent dipole: HI, HBr or HCl?

    • All would be equal
    • HI
    • HBr
    • HCl

  20. Which molecule is polar, given that its bonds are arranged asymmetrically?

    • BF3
    • CO2
    • CCl4
    • CH2Cl2

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