Table of contents

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

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Which of the following Lewis structures best represents a polar molecule?

A bent molecule with two different atoms and lone pairs on the central atom, such as H_2O

A linear molecule with two identical atoms, such as O_2

A tetrahedral molecule with four identical atoms around the central atom, such as CH_4

A trigonal planar molecule with three identical atoms around the central atom, such as BF_3

Previous problemNext problem

Verified step by step guidance

Step 1: Understand that molecular polarity depends on both the polarity of individual bonds and the overall molecular geometry. A molecule is polar if it has polar bonds arranged asymmetrically, resulting in a net dipole moment.

Step 2: Analyze each molecular shape and its symmetry: linear molecules with identical atoms (like O_2) are nonpolar because the bond dipoles cancel out; tetrahedral molecules with four identical atoms (like CH_4) are also nonpolar due to symmetrical charge distribution; trigonal planar molecules with three identical atoms (like BF_3) are nonpolar because the dipoles cancel out in a symmetrical plane.

Step 3: Consider the bent molecule with two different atoms and lone pairs on the central atom (like H_2O). The presence of lone pairs creates an asymmetrical shape, and the different atoms create polar bonds that do not cancel out, resulting in a net dipole moment.

Step 4: Conclude that the bent molecule with lone pairs and different atoms is polar because its molecular geometry and bond polarity combine to produce an overall dipole moment.

Step 5: Therefore, the Lewis structure that best represents a polar molecule is the bent molecule with two different atoms and lone pairs on the central atom, such as H_2O.