Textbook Question
Compare the Lewis structures of CF4 and NF3 Why do these molecules have different shapes?
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Ch.6 Ionic and Molecular Compounds
Timberlake14thChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249
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Table of contents
- Ch.1 Chemistry in Our Lives19
- Ch.2 Chemistry and Measurements80
- Ch.3 Matter and Energy53
- Ch.4 Atoms and Elements58
- Ch.5 Nuclear Chemistry42
- Ch.6 Ionic and Molecular Compounds57
- Ch.7 Chemical Quantities and Reactions38
- Ch.8 Gases30
- Ch.9 Solutions50
- Ch.10 Acids and Bases and Equilibrium64
- Ch.11 Introduction to Organic Chemistry: Hydrocarbons77
- Ch.12 Alcohols, Thiols, Ethers, Aldehydes, and Ketones82
- Ch.13 Carbohydrates54
- Ch.14 Carboxylic Acids, Esters, Amines, and Amides91
- Ch.15 Lipids61
- Ch.16 Amino Acids, Proteins, and Enzymes84
- Ch.17 Nucleic Acids and Protein Synthesis86
- Ch.18 Metabolic Pathways and ATP Production73
Timberlake14thChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249Not the one you use?Change textbook
Chapter 6, Problem 86b
Identify the major type of intermolecular forces between the particles of each of the following:
b. HCl
Verified step by step guidance1
Step 1: Begin by identifying the type of molecule HCl is. HCl is a polar covalent molecule because the electronegativity difference between hydrogen (H) and chlorine (Cl) is significant, causing an uneven distribution of electron density.
Step 2: Recognize that polar molecules exhibit dipole-dipole interactions as their major type of intermolecular force. This occurs because the partial positive charge on the hydrogen atom is attracted to the partial negative charge on the chlorine atom of neighboring molecules.
Step 3: Consider whether hydrogen bonding is possible. Hydrogen bonding occurs when hydrogen is directly bonded to highly electronegative atoms like oxygen (O), nitrogen (N), or fluorine (F). Since HCl does not meet this criterion, hydrogen bonding is not present.
Step 4: Note that London dispersion forces (induced dipole-induced dipole interactions) are present in all molecules, but they are not the major intermolecular force in polar molecules like HCl. Dipole-dipole interactions dominate in this case.
Step 5: Conclude that the major type of intermolecular force in HCl is dipole-dipole interactions, which arise due to the polarity of the molecule.
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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 forces of attraction or repulsion between neighboring particles (atoms, molecules, or ions). They are crucial in determining the physical properties of substances, such as boiling and melting points. The main types of intermolecular forces include hydrogen bonding, dipole-dipole interactions, and London dispersion forces.
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Dipole-Dipole Interactions
Dipole-dipole interactions occur between polar molecules, where positive and negative ends of the molecules attract each other. In the case of HCl, the molecule has a permanent dipole due to the difference in electronegativity between hydrogen and chlorine, leading to significant dipole-dipole interactions that influence its physical properties.
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Hydrogen Bonding
Hydrogen bonding is a specific type of strong dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative atoms like nitrogen, oxygen, or fluorine. While HCl does not form hydrogen bonds, understanding this concept is essential for comparing it with other molecules that do, as it highlights the strength and significance of intermolecular forces in molecular interactions.
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