'London forces' diaporamas de présentation

Chapter 12: Intermolecular Attractions and the Properties of Liquids and Solids

Chapter 12: Intermolecular Attractions and the Properties of Liquids and Solids. Chemistry: The Molecular Nature of Matter, 6E Jespersen/Brady/Hyslop. Intermolecular Forces. Important differences between gases, solids, and liquids: Gases Expand to fill their container Liquids

1.38k views • 134 slides

Chapter 12: Intermolecular Attractions and the Properties of Liquids and Solids

Chapter 12: Intermolecular Attractions and the Properties of Liquids and Solids. Chemistry: The Molecular Nature of Matter, 6E Jespersen/Brady/Hyslop. Intermolecular Forces. Important differences between gases, solids, and liquids: Gases Expand to fill their container Liquids

1.88k views • 125 slides

Chapter 12: Intermolecular Attractions and the Properties of Liquids and Solids

Chapter 12: Intermolecular Attractions and the Properties of Liquids and Solids. Chemistry: The Molecular Nature of Matter, 6E Jespersen/Brady/Hyslop. Intermolecular Forces. Important differences between gases, solids, and liquids: Gases Expand to fill their container Liquids

2.28k views • 125 slides

Intermolecular Forces: State Changes, Solubility, and Cell Membranes

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Homework Private study work (bring notes to show me next lesson) ;

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Ch 11 States of Matter and Intermolecular Forces

Ch 11 States of Matter and Intermolecular Forces. Chapter 11 Preview. Intra molecular forces (bonds) govern molecular properties. Inter molecular forces are between molecules and determine the macroscopic physical properties of liquids and solids. This chapter:

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Dr. C. Yau Fall 2014

Intermolecular Forces (IMF) Part I: Types of IMF Effect of IMF on Physical Properties (based on Chap. 12 Sec 1-3 of Jespersen 6 th Ed). Dr. C. Yau Fall 2014. Review of the Postulates of the KMT. KMT = Kinetic Molecular Theory

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Intermolecular Forces: State Changes, Solubility, and Cell Membranes

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Intermolecular Forces, Liquids, and Solids

Intermolecular Forces, Liquids, and Solids. By: Ms. Buroker. 11.1: A Molecular Comparison of Liquids and Solids. There is a fundamental difference between the three states of matter and that is due to the space between the particles. Review of Gases

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Chemistry 11 Chemical Bonding

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Liquids and Solids

Liquids and Solids. Relative Magnitudes of Forces. The types of bonding forces vary in their strength as measured by average bond energy. Strongest Weakest. Covalent bonds ( 400 kcal/mol ). Hydrogen bonding ( 12-16 kcal/mol ). Dipole-dipole interactions ( 2-0.5 kcal/mol ).

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Chapter 12

Chapter 12 . Intermolecular Attractions and the Properties of Liquids and Solids. Gases, Liquids and Solids. Intermolecular Attractions. Intermolecular forces depend on distance Gases have very small attractive forces

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Part 08 Intermolecular Forces of Attraction

Part 08 Intermolecular Forces of Attraction. 1. IMFA Intermolecular forces of attraction are any attraction that exists in BETWEEN two or more molecules. They are NOT bonds. 2. Types of IMFA a. London Dispersion Forces

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AP unit 4-2 Intermolecular force and phase change

AP unit 4-2 Intermolecular force and phase change. States of Matter. Because in the solid and liquid states particles are closer together, we refer to them as condensed phases . Molecule distance: gas>liquid>gas. The States of Matter.

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14.1 Molecular Substances Intermolecular Forces

14.1 Molecular Substances Intermolecular Forces. Forces between molecules determine the melting and boiling point of substances. Ionic compounds have high melting and boiling points due to their electrostatic attraction. Molecular substances are held together by one of three forces. Dispersion

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Chapter 6 Reactions of Haloalkanes: S N 2

Chapter 6 Reactions of Haloalkanes: S N 2. Naming Haloalkanes Treat Halogen as a substituent to an alkane: chlorine = chloro- Name as in alkane nomenclature Physical properties of haloalkanes Bond Strength For RCH 2 X, F > Cl > Br > I bond strength F has best size for overlap

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Questions

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Explain the trend in the boiling points of the hydrogen halides:

Chapter 10 Worked Example 1. Explain the trend in the boiling points of the hydrogen halides: HCl, -85 o C; HBr, -67 o C; HI, -35 o C. - Electronegativity differences: HCl > HBr > HI. - Number of electrons and London forces: HCl < HBr < HI.

137 views • 7 slides