Unit3Day7-LaBrake. Important Information. Vanden Bout/LaBrake/Crawford CH301. WHY IS EVERYTHING SO DIFFERENT? Gas, Liquid or Solid?

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1 Unit3Day7-LaBrake Page 1 Unit3Day7-LaBrake Monday, October 28, :38 AM Vanden Bout/LaBrake/Crawford CH301 WHY IS EVERYTHING SO DIFFERENT? Gas, Liquid or Solid? UNIT 3 Day 7 Important Information HW09 DUE T 9AM Exam 3 NEXT Wed (11/6) CH301 Vanden Bout/LaBrake Spring 2013

2 Unit3Day7-LaBrake Page 2 What are we going to learn today? Properties of Liquids Think Some More Properties of Solids Different Types QUIZ: iclicker Question 1 Viscosity is a) Thickness b) Density c) Ability to flow d) Resistance to flow

3 Unit3Day7-LaBrake Page 3 Poll: iclicker Question 2 Studying chemistry with other students outside of class is helping me learn the material. A) I only study alone. B) My group is very helpful. C) My group is helpful. D) My group is only a little helpful. E) My group is not helpful at all. CH301 Vanden Bout/LaBrake Spring 2013 Study Groups are Effective When 2 or more students work collaboratively to solve the problem or engage in constructive dialogue, they Outperform those learning individually. Are exposed to different perspectives. Are required to negotiate to achieve understanding. Retain their knowledge longer. (Ding & Harskamp, 2011) CH301 Vanden Bout/LaBrake Spring 2013

4 Unit3Day7-LaBrake Page 4 Vapor Pressure We ve extensively discussed the relationship between boiling point and IMF. What is the relationship between boiling point and vapor pressure? Poll: iclicker Question 3 Which of the following has the highest vapor pressure? a) CH 3 OH b) CH 3 CH 2 OH c) CH 3 CH 2 CH 2 OH d) CH 3 CH 2 CH 2 CH 2 OH

5 Unit3Day7-LaBrake Page 5 Evaporation Boltzmann distribution explains evaporation Poll: iclicker Question 4 Which distribution is at higher T? A B C

6 Unit3Day7-LaBrake Page Poll: iclicker Question 5 What do you think will happen to the viscosity as the temperature is increased? A)It will go up B)It will go down C) It will stay the same CH302 Vanden Bout/LaBrake Fall 2012

7 Physical Properties Properties of Liquids based on intermolecular forces and shapes of molecules Properties of Solids based on intermolecular forces and the type of bonding Poll: iclicker Question 6 Diamonds are a) A bunch of C atoms held together by dispersion forces b) A bunch of C molecules held together by dipole dipole interactions c) A bunch of C atoms covalently bound together d) A bunch of C molecules held together by dispersion forces CH302 Vanden Bout/LaBrake Fall 2012 Poll: iclicker Question 7 Graphite is a) A bunch of C atoms held together by dispersion forces b) A bunch of C molecules held together by dipole dipole interactions c) A bunch of C atoms covalently bound together Unit3Day7-LaBrake Page 7

8 Poll: iclicker Question 7 Unit3Day7-LaBrake Page 8 Graphite is a) A bunch of C atoms held together by dispersion forces b) A bunch of C molecules held together by dipole dipole interactions c) A bunch of C atoms covalently bound together d) A bunch of C molecules held together by dispersion forces CH302 Vanden Bout/LaBrake Fall 2012 Poll: iclicker Question 8 Solids are classified into four different categories Ionic Covalent Metallic Molecular We ve already discussed two types of solids this semester. Which ones have we discussed? A. Ionic and Covalent B. Metallic and Covalent C. Molecular and Ionic D. Metallic and Molecular

9 Unit3Day7-LaBrake Page 9 Types of Solids Ionic Covalent or (Network) Metallic Molecular Types of Solids Class Examples Characteristics Ionic NaCl, KNO 3, CuSO 4 H 2 O Network B, C, black P, BN, SiO 2 Hard, rigid, brittle; high melting/boiling points; those soluble in water give conducting solutions Hard, rigid, brittle; very high melting points; insoluble in water Metallic s- and d- elements Malleable, ductile, lustrous; electrically and thermally conducting Molecular BeCl 2, S 8, P 4, I 2, ice, glucose Relatively low melting/boiling points; brittle if pure

10 Unit3Day7-LaBrake Page 10 Physical Properties of Solids Class Electrons Conductivity Ionic Localized Not a good conductor (only conducts electricity in aqueous solutions) Network Localized Not a good conductor Metallic Delocalized Good conductor Molecular Localized Not a good conductor Physical Properties of Solids Ionic Metallic

11 Physical Properties of Solids Molecular Network Predicting Melting Point Trends We can use melting points to distinguish between covalent and molecular solids Molecule Melting Point [K] Type of Solid Diamond 3823 SiO Gold 1337 NaCl 1074 Sugar 423 Naphthalene 353 Ice 273 CO Activity Recall Unit 3-Activity 1 (pg. 75) After discussing IMFs, shapes of liquids, and types of solids, can you now draw better pictures? Please complete the new Activity Unit3Day7-LaBrake Page 11

12 Activity Unit3Day7-LaBrake Page 12 Recall Unit 3-Activity 1 (pg. 75) After discussing IMFs, shapes of liquids, and types of solids, can you now draw better pictures? Please complete the new Activity IMF Unit- Constructing a Microscopic and Macroscopic View of Substances (ph. 81)

13 Unit3Day7-LaBrake Page 13 What have we learned today? Condensed phases exist because of IMFs Electrostatic Forces vary with shape, size, components of the compound, allowing for various phase transition temperatures Properties of liquids and solids depend on IMFs Learning Outcomes Recognize the four types of solids: ionic, covalent (network), metallic, and molecular Recognize how the macroscopic properties of solids (melting point, hardness, conductivity, etc.) can be explained by the microscopic model of solids