'Ion dipole' presentation slideshows

George Mason University General Chemistry 212 Chapter 13

George Mason University General Chemistry 212 Chapter 13 Properties of Mixtures: Solutions & Colloids Acknowledgements Course Text: Chemistry: the Molecular Nature of Matter and Change, 6 th ed , 2011, Martin S. Silberberg, McGraw-Hill

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You Ever Ask???

You Ever Ask???. Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature for such a small molecule? Why does ice float on water? Why do snowflakes have 6 sides? Why is I 2 a solid whereas Cl 2 is a gas? Why are NaCl crystals little cubes?.

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Phases of matter

Phases of matter. Energy and phases. Everything that has mass and volume is called matter. What is matter?. What kind of changes does matter undergo?. All matter can undergo changes in its state. These changes have to do with the amount of energy in the particles of matter. Kinetic theory.

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The Ties That Bind

The Ties That Bind. Chemical Bonding and Interactions. Chemical Bonding and Interactions. Stable Electron Configurations Electron-Dot (Lewis) Structures Drawing, Rules for Drawing The Octet Rule Some Exceptions to the Rule Ionic Bonding Naming ionic compounds Drawing Covalent Bonding

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The Ties That Bind

The Ties That Bind. Chemical Bonding and Interactions. Chemical Bonding and Interactions. Stable Electron Configurations Electron-Dot (Lewis) Structures Drawing, Rules for Drawing The Octet Rule Some Exceptions to the Rule Ionic Bonding Naming ionic compounds Drawing Covalent Bonding

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Chapter 11 Intermolecular Forces

Chapter 11 Intermolecular Forces. A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well-defined boundary. 2 Phases. Solid phase - ice. Liquid phase - water. 11.1.

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Intermolecular Forces

Concept Presentation By: Amarinder Sawhney Jeffrey Ip. Intermolecular Forces. Salt (NaCl) & Water (H 2 O). Why does salt dissolve in water?. Salt (NaCl) & Water (H 2 O). Water is a polar molecule: one end has a slightly positive charge, another has a slightly negative charge.

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Intermolecular Forces

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How I would study:

How I would study:. Look over exams Look over review sheets Difficulties? Work HW problems, examples from the text Start early: where are your problem spots?. Chapter 1: Introduction. Dimensional analysis Change among units (eg. feet vs. meters) Prefixes (1 kilogram/1000 grams)

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Intermolecular Forces

Chemical Bonding, Part 2. Intermolecular Forces. Honor Chemistry Only. A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well-defined boundary. 2 Phases. Solid phase - ice. Liquid phase - water.

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Chapter 14.3 Properties of Solutions

Chapter 14.3 Properties of Solutions. Adapted by SA Green from: John D. Bookstaver St. Charles Community College St. Peters, MO ? 2006, Prentice Hall, Inc. Solutions. Solutions are homogeneous mixtures of two or more pure substances.

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Experiment 1:

Experiment 1:. STRUCTURE, INTERMOLECULAR FORCES AND SOLUBILITY. OBJECTIVES. To learn how to identify which intermolecular forces exist between organic compounds. To investigate the relationship between structure, intermolecular forces and solubility using solubility testing.

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Experiment 1:

Experiment 1:. STRUCTURE, INTERMOLECULAR FORCES AND SOLUBILITY. OBJECTIVES. To learn how to identify which intermolecular forces (IMF) exist between organic compounds. To investigate the relationship between structure, intermolecular forces and solubility using solubility testing. ROLE OF IMF.

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Solution Formation

Solution Formation. Solutions. . . . the components of a mixture are uniformly intermingled (the mixture is homogeneous ). Solution Components. Solute Solvent. Steps in Solution Formation. Step 1 - Expanding the solute (endothermic, ?H 1 )

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20 B Week III Chapters 10 and 11

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FACTORS AFFECTING RATE OF DISSOLVING AND SOLUBILITY

FACTORS AFFECTING RATE OF DISSOLVING AND SOLUBILITY. SECTION 8.2. FACTORS AFFECTING RATE OF SOLUBILITY. TEMPERATURE High temp ? more kinetic energy Particles collide with each other This increases their rate of dissolving. FACTORS AFFECTING RATE OF SOLUBILITY. PARTICLE/ MOLECULE SIZE

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Intermolecular Forces

Intermolecular Forces . By: Michael London Ellie Kaplan Mike Ghen. Intermolecular Forces . Strengths of intermolecular forces of difference substances vary over a wide range, but they are generally much weaker than ionic or covalent bonds

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20 B Week IV Chapters 11

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Structure & properties

Structure & properties. INTERMOLECULAR FORCES. INTRAMOLECULAR FORCES. Ionic bonds, covalent bonds, metallic bonding are all examples of bonds within a molecule. intermolecular forces. Forces BETWEEN molecules Weaker than inTRAmolecular forces, but still very important.

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