Table of contents

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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

13. Liquids, Solids & Intermolecular Forces

Molecular Polarity

General Chemistry

13. Liquids, Solids & Intermolecular Forces

Molecular Polarity

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Multiple Choice

Is the molecule H2O polar or nonpolar?

Nonpolar

Polar

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Verified step by step guidance

Identify the molecular geometry of H2O. Water (H2O) has a bent shape due to the two lone pairs of electrons on the oxygen atom.

Consider the electronegativity of the atoms involved. Oxygen is more electronegative than hydrogen, which means it will attract the shared electrons more strongly.

Determine the direction of the dipole moments. In H2O, the dipole moments point from the hydrogen atoms towards the oxygen atom due to the difference in electronegativity.

Analyze the symmetry of the molecule. The bent shape of H2O means that the dipole moments do not cancel out, resulting in a net dipole moment.

Conclude that because of the net dipole moment and the asymmetrical shape, H2O is a polar molecule.