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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

Which of the following best describes the molecular polarity of SO_2?

SO_2 is a nonpolar molecule because it contains only nonpolar bonds.

SO_2 is a polar molecule because it has a symmetrical structure.

SO_2 is a nonpolar molecule because its shape is linear and the dipoles cancel out.

SO_2 is a polar molecule because it has a bent shape and an uneven distribution of electrons.

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Verified step by step guidance

Identify the molecular geometry of SO\_2 by considering the Lewis structure. Sulfur (S) is the central atom bonded to two oxygen (O) atoms, and there is a lone pair of electrons on the sulfur atom.

Determine the shape of the molecule using VSEPR theory. With two bonded atoms and one lone pair on the central atom, the shape of SO\_2 is bent (angular), not linear.

Analyze the polarity of the bonds. The S–O bonds are polar because oxygen is more electronegative than sulfur, creating bond dipoles pointing towards the oxygen atoms.

Consider the molecular shape and how the bond dipoles combine. Because the molecule is bent, the bond dipoles do not cancel out, resulting in a net dipole moment.

Conclude that SO\_2 is a polar molecule due to its bent shape and uneven distribution of electron density, which leads to an overall molecular polarity.