Unit3Day7-LaBrake Monday, October 28, 2013 9:38 AM Vanden - - PDF document

CH301 Vanden Bout/LaBrake Fall 2013

Vanden Bout/LaBrake/Crawford CH301 WHY IS EVERYTHING SO DIFFERENT? Gas, Liquid or Solid? UNIT 3 Day 7

CH301 Vanden Bout/LaBrake Spring 2013

Important Information

HW09 DUE T 9AM Exam 3 NEXT Wed (11/6)

Unit3Day7-LaBrake

Monday, October 28, 2013 9:38 AM Unit3Day7-LaBrake Page 1

CH301 Vanden Bout/LaBrake Fall 2013

What are we going to learn today?

Properties of Liquids – Think Some More Properties of Solids – Different Types

CH301 Vanden Bout/LaBrake Fall 2013

Viscosity is… a) Thickness b) Density c) Ability to flow d) Resistance to flow

QUIZ: iClicker Question 1

Unit3Day7-LaBrake Page 2

CH301 Vanden Bout/LaBrake Spring 2013

Studying chemistry with other students outside

• f 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.

Poll: iClicker Question 2

CH301 Vanden Bout/LaBrake Spring 2013

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)

Study Groups are Effective

Unit3Day7-LaBrake Page 3

CH301 Vanden Bout/LaBrake Fall 2013

We’ve extensively discussed the relationship between boiling point and IMF. What is the relationship between boiling point and vapor pressure?

Vapor Pressure

CH301 Vanden Bout/LaBrake Fall 2013

Which of the following has the highest vapor pressure? a) CH3OH b) CH3CH2OH c) CH3CH2CH2OH d) CH3CH2CH2CH2OH

Poll: iClicker Question 3

Unit3Day7-LaBrake Page 4

CH301 Vanden Bout/LaBrake Fall 2013

Boltzmann distribution explains evaporation

Evaporation

CH301 Vanden Bout/LaBrake Fall 2013

Which distribution is at higher T?

Poll: iClicker Question 4

A B C

Unit3Day7-LaBrake Page 5

CH301 Vanden Bout/LaBrake Fall 2013

• 100

20 600

CH302 Vanden Bout/LaBrake Fall 2012

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

Poll: iClicker Question 5

Unit3Day7-LaBrake Page 6

CH301 Vanden Bout/LaBrake Fall 2013

Properties of Liquids based on intermolecular forces and shapes of molecules Properties of Solids based on intermolecular forces and the type of bonding

Physical Properties

CH302 Vanden Bout/LaBrake Fall 2012

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

Poll: iClicker Question 6

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

Poll: iClicker Question 7

Unit3Day7-LaBrake Page 7

CH302 Vanden Bout/LaBrake Fall 2012

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

Poll: iClicker Question 7

CH301 Vanden Bout/LaBrake Fall 2013

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

Poll: iClicker Question 8

Unit3Day7-LaBrake Page 8

Ionic Covalent or (Network) Molecular Metallic

Types of Solids

CH301 Vanden Bout/LaBrake Fall 2013

Types of Solids

Class Examples Characteristics Ionic NaCl, KNO3, CuSO4•H2O Hard, rigid, brittle; high melting/boiling points; those soluble in water give conducting solutions Network B, C, black P, BN, SiO2 Hard, rigid, brittle; very high melting points; insoluble in water Metallic s- and d- elements Malleable, ductile, lustrous; electrically and thermally conducting Molecular BeCl2, S8, P4, I2, ice, glucose Relatively low melting/boiling points; brittle if pure

Unit3Day7-LaBrake Page 9

CH301 Vanden Bout/LaBrake Fall 2013

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

Unit3Day7-LaBrake Page 10

CH301 Vanden Bout/LaBrake Fall 2013

Physical Properties of Solids

Molecular Network

CH301 Vanden Bout/LaBrake Fall 2013

We can use melting points to distinguish between covalent and molecular solids

Predicting Melting Point Trends

Molecule Melting Point [K] Type of Solid Diamond 3823 SiO2 1900 Gold 1337 NaCl 1074 Sugar 423 Naphthalene 353 Ice 273 CO2 190 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

Activity

Unit3Day7-LaBrake Page 11

CH301 Vanden Bout/LaBrake Fall 2013

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)

Activity

Unit3Day7-LaBrake Page 12

CH301 Vanden Bout/LaBrake Fall 2013

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

CH301 Vanden Bout/LaBrake Fall 2013

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

Learning Outcomes

Unit3Day7-LaBrake Page 13