Table of contents

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

2. Molecular Representations

Intermolecular Forces

Organic Chemistry

2. Molecular Representations

Intermolecular Forces

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Multiple Choice

Which molecule is nonpolar?

The figure illustrates a Lewis structure. A central C atom is single bonded to H above, H below, H on the left, and I on the right. The I atom has 3 lone pairs of electrons.

The figure illustrates a Lewis structure. C, double bond, C. C 1 is single bonded to H on the upper left and H on the lower left. C 2 is single bonded to B r on the upper right and B r on the lower right. Each B r atom has 3 lone pairs of electrons.

The figure illustrates a Lewis structure. C, double bond, C. C 1 is single bonded to F on the upper left and F on the lower left. C 2 is single bonded to F on the upper right and F on the lower right. Each F atom has 3 lone pairs of electrons.

The figure illustrates a Lewis structure. A central C atom is single bonded to C l above, C l below, H on the right, and H on the left. Each C l atom has 3 lone pairs of electrons.

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Verified step by step guidance

Identify the molecular geometry of each molecule. For example, the first molecule (CH3F) is tetrahedral, the second molecule (C2H2Br2) is planar, the third molecule (C-N) is linear, and the fourth molecule (CH2Cl2) is tetrahedral.

Determine the electronegativity of the atoms involved in each molecule. Fluorine, bromine, nitrogen, and chlorine are more electronegative than carbon and hydrogen, which can lead to polar bonds.

Analyze the symmetry of each molecule. A nonpolar molecule typically has a symmetrical distribution of charge, which means the dipole moments cancel each other out.

For the first molecule (CH3F), the presence of a highly electronegative fluorine atom creates a dipole moment, making it polar.

For the second molecule (C2H2Br2), if the bromine atoms are on opposite sides, the dipole moments can cancel out, making it nonpolar. However, if they are on the same side, it would be polar. The third molecule (C-N) is polar due to the difference in electronegativity between carbon and nitrogen. The fourth molecule (CH2Cl2) is polar because the dipole moments do not cancel out due to its geometry.