Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

16. Carboxylic Acids and Their Derivatives

Naming Amides

GOB Chemistry

16. Carboxylic Acids and Their Derivatives

Naming Amides

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Problem 35b

Textbook Question

Arrange these compounds in order of increasing boiling points and explain your rationale for the order.
(i) formic acid
(ii) methyl formate
(iii) formamide.

Verified step by step guidance

Identify the intermolecular forces present in each compound. Common forces include London dispersion forces, dipole-dipole interactions, and hydrogen bonding. Stronger intermolecular forces generally lead to higher boiling points.

Consider the molecular weight of each compound. Larger molecules with greater molecular weights tend to have higher boiling points due to increased London dispersion forces.

Examine the molecular structure of each compound. Linear molecules often have stronger London dispersion forces compared to branched molecules of similar molecular weight, which can influence boiling points.

Check for the presence of functional groups capable of hydrogen bonding (e.g., -OH, -NH). Compounds with hydrogen bonding typically have significantly higher boiling points than those without.

Arrange the compounds in order of increasing boiling points based on the strength of their intermolecular forces, molecular weight, and structural considerations. Provide a rationale for the order based on these factors.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Intermolecular Forces

Intermolecular forces are the attractions between molecules that influence physical properties like boiling points. The main types include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Compounds with stronger intermolecular forces typically have higher boiling points because more energy is required to separate the molecules during the phase change from liquid to gas.

Molecular Weight

Molecular weight, or molar mass, refers to the mass of a molecule based on the sum of the atomic weights of its constituent atoms. Generally, as molecular weight increases, the boiling point also tends to increase due to the greater number of electrons, which enhances London dispersion forces. However, this trend can be influenced by the presence of functional groups and molecular structure.

Polarity

Polarity describes the distribution of electrical charge over the atoms in a molecule. Polar molecules have a significant difference in electronegativity between bonded atoms, leading to dipole-dipole interactions that can elevate boiling points. In contrast, nonpolar molecules primarily exhibit weaker London dispersion forces, resulting in lower boiling points. Understanding polarity is crucial for predicting the boiling point order of compounds.

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