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 ClF polar or nonpolar?

Polar

Nonpolar

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Verified step by step guidance

Step 1: Draw the Lewis structure of ClF. Chlorine (Cl) and Fluorine (F) are bonded by a single bond, with each atom having three lone pairs of electrons around it.

Step 2: Determine the molecular geometry. Since ClF is a diatomic molecule, its shape is linear with only two atoms.

Step 3: Consider the electronegativity values of Cl and F. Fluorine is more electronegative than chlorine, meaning it will attract the bonding electrons more strongly.

Step 4: Analyze the dipole moment. Because the two atoms have different electronegativities, the electron density is unevenly distributed, creating a dipole moment pointing toward fluorine.

Step 5: Conclude polarity. Since there is a net dipole moment due to the difference in electronegativity and the linear shape does not cancel it out, ClF is a polar molecule.