Domanda del libro di testo
When lithium iodide (LiI) is dissolved in water, the solution becomes hotter. c. Sketch a qualitative energy diagram similar to Figure 13.7 for the dissolution of LiI.
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Ch.14 - Solutions
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Capitolo 14, Problema 34
For each compound, would you expect greater solubility in water or in hexane? Indicate the kinds of intermolecular forces that would occur between the solute and the solvent in which the molecule is most soluble. d. ethylene glycol
Guida verificata passo dopo passo1
Identify the molecular structure of ethylene glycol, which is HOCH2CH2OH. Note that it contains hydroxyl groups (-OH) which are polar.
Recognize that water is a polar solvent and hexane is a non-polar solvent. Polar solutes generally dissolve better in polar solvents due to similar types of intermolecular forces.
Analyze the intermolecular forces in ethylene glycol. The presence of -OH groups allows it to form hydrogen bonds, which are strong intermolecular forces.
Predict the solubility of ethylene glycol in water by considering its ability to form hydrogen bonds with water molecules, which also contain polar O-H bonds.
Conclude that ethylene glycol would have greater solubility in water due to the hydrogen bonding between the -OH groups of ethylene glycol and the water molecules, compared to weaker dispersion forces that would be present in hexane.
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Polarity of Molecules
Polarity refers to the distribution of electrical charge over the atoms in a molecule. Polar molecules, which have a significant difference in electronegativity between their atoms, tend to dissolve well in polar solvents like water. In contrast, nonpolar molecules, which have an even distribution of charge, are more soluble in nonpolar solvents like hexane.
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02:38
Molecular Polarity
Intermolecular Forces
Intermolecular forces are the forces of attraction or repulsion between neighboring particles (atoms, molecules, or ions). The main types include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. The strength and type of these forces influence a compound's solubility in a given solvent, as similar types of intermolecular forces between solute and solvent enhance solubility.
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01:59Intermolecular vs Intramolecular Forces
Hydrogen Bonding
Hydrogen bonding is a strong type of dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine. Ethylene glycol, which contains hydroxyl (-OH) groups, can form hydrogen bonds with water, significantly increasing its solubility in polar solvents. This interaction is crucial for understanding why certain compounds dissolve better in water than in nonpolar solvents.
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01:22Hydrogenation Reactions
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For each compound, would you expect greater solubility in water or in hexane? Indicate the kinds of intermolecular forces that occur between the solute and the solvent in which the molecule is most soluble. a. glucose
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Domanda del libro di testo
When lithium iodide (LiI) is dissolved in water, the solution becomes hotter. a. Is the dissolution of lithium iodide endothermic or exothermic?
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When lithium iodide (LiI) is dissolved in water, the solution becomes hotter. b. What can you conclude about the relative magnitudes of the lattice energy of lithium iodide and its heat of hydration?
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Which molecule would you expect to be more soluble in water: CH3CH2CH2OH or HOCH2CH2CH2OH?
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