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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 polarity of the molecule CH_4 (methane)?

CH_4 is a nonpolar molecule because its tetrahedral geometry causes the bond dipoles to cancel.

CH_4 is a polar molecule because it contains polar C–H bonds.

CH_4 is a nonpolar molecule because it contains only nonpolar bonds.

CH_4 is a polar molecule due to the presence of lone pairs on the central carbon atom.

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Verified step by step guidance

Step 1: Identify the molecular geometry of CH_4. Methane has a central carbon atom bonded to four hydrogen atoms arranged in a tetrahedral shape.

Step 2: Consider the polarity of each C–H bond. Although the C–H bond has a small difference in electronegativity, it is often considered slightly polar but close to nonpolar.

Step 3: Analyze the symmetry of the molecule. Because the molecule is tetrahedral and symmetrical, the individual bond dipoles point in different directions and can cancel each other out.

Step 4: Determine the overall molecular polarity by assessing if the bond dipoles cancel. In CH_4, the symmetrical arrangement causes the bond dipoles to cancel, resulting in no net dipole moment.

Step 5: Conclude that CH_4 is a nonpolar molecule due to its tetrahedral geometry causing the bond dipoles to cancel, despite the slight polarity of individual C–H bonds.