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 molecules is nonpolar but contains polar covalent bonds?

CHCl_3

H_2O

NH_3

CO_2

Previous problemNext problem

Verified step by step guidance

Step 1: Understand the difference between polar covalent bonds and molecular polarity. A polar covalent bond occurs when two atoms share electrons unequally due to differences in electronegativity, creating partial positive and negative charges within the bond.

Step 2: Recognize that molecular polarity depends on both the polarity of individual bonds and the geometry (shape) of the molecule. Even if a molecule has polar bonds, the overall molecule can be nonpolar if the bond dipoles cancel out due to symmetry.

Step 3: Analyze the molecular geometry of each molecule: CHCl_3 (trichloromethane) has a tetrahedral shape but with different atoms attached, leading to an overall polar molecule; H_2O (water) has a bent shape causing an overall polar molecule; NH_3 (ammonia) has a trigonal pyramidal shape, also polar.

Step 4: Examine CO_2 (carbon dioxide), which has two polar C=O bonds. However, CO_2 is linear and symmetrical, so the bond dipoles are equal in magnitude but opposite in direction, canceling each other out and making the molecule nonpolar overall.

Step 5: Conclude that CO_2 is the molecule that contains polar covalent bonds but is nonpolar as a whole due to its linear geometry and symmetrical distribution of bond dipoles.