DIFFERENT? Gas, Liquid or Solid? UNIT 3 Day 7 What are we going to - - PowerPoint PPT Presentation

Sparks CH301 WHY IS EVERYTHING SO DIFFERENT? Gas, Liquid or Solid? UNIT 3 Day 7

What are we going to do today?

Discuss types of intermolecular forces. Compare intermolecular forces for different molecules. Discuss the effect of these forces on properties of substances.

INTERMOLECULAR FORCES: fact check

Water and Ethanol attracted to charged rod. Hexane and Carbon Tetrachloride NOT attracted to charged rod. Explanation: presence of dipole moment How is it possible for Hexane and Carbon Tetrachloride to exist as liquids?

INTERMOLECULAR FORCES: fact check

How is it possible for Hexane and Carbon Tetrachloride to exist as liquids? THERE MUST BE AN ELECTROSTATIC ATTRACTION! EXPLANTION: INDUCED DIPOLE – INDUCED DIPOLE

INTERMOLECULAR FORCES: Induced dipole – Induced dipole

Exist in all condensed substances Caused by induced dipoles, which come and go in nonpolar molecules and atoms E  1 r6

Look at the table on p. 73 of your course packet.

• 1. Comment on the correlation of molecular weight and

boiling point for the first four substances (methane –

• ctane).
• What do you think this says about the strength of the

induced dipole-induced dipole interactions as MW increases?

• 2. Now look at the last value on the table – carbon
• tetrachloride. Does this fit with your MW:interaction

strength correlation?

• Suggest another factor you think might be important in

determining strength of interactions.

INTERMOLECULAR FORCES: Induced dipole – Induced dipole

Strength depends on polarizability

INTERMOLECULAR FORCES: fact check

STRENGTH DEPENDENT ON POLARIZABILITY CCl4, (154 g/mol) boiling point = 77°C C8H18 (114 g/mol) boiling point = 126°C Strength also depends on SHAPE of molecule

Hard question…..

Why can’t the charged glass rod induce a dipole? Lots of common examples: oils versus fats plastic wrap vs milk jugs FAVORITE ANALOGY - VELCRO

INTERMOLECULAR FORCES Induced dipole – induced dipole

This type of intermolecular force goes by several different names: Induced dipole – Induced dipole Dispersion Forces London Forces Van der Waal’s Forces

Answer question #3 on page 74 using data from your chart. Why do you think this is true?

Hydrogen bonding*

Subset of dipole-dipole interactions Molecules with H attached to F, O, or N *“Hydrogen Bond” a misnomer – implies a chemical bond; just a very strong dipole-dipole interaction.

Hydrogen bonding*

Strength depends on distance and dipole moment.

Draw dot structures for ethyl alcohol, CH3CH2OH and consider if hydrogen bonding would occur in a sample of this substance.

• A. Yes, this molecule would exhibit hydrogen bonding.
• B. No, this molecule would not exhibit hydrogen bonding.

Quiz: CLICKER QUESTION

Would hydrogen bonding occur in a sample of CH3CH2OCH2CH3?

A.Yes. B.No.

Quiz: CLICKER QUESTION

WHAT HAVE WE LEARNED TODAY?

PHYSICAL PROPERTIES DEPEND ON COMPOSITION & SHAPE OF COMPOUND CLASSIFY INTERMOLECULAR FORCES ION-ION vs. DIPOLE-DIPOLE vs. INDUCED DIPOLE – INDUCED DIPOLE PREDICT WHAT TYPE OF IMFs EXIST FOR A PARTICULAR COMPOUND

Learning Outcomes

Define the three major types of intermolecular forces (IMF) discussed in class:

• dipole-dipole,
• H-bonding, and
• dispersion (London, van der Waals,
• induced dipole-induced dipole)

Explain how molecular size and shape affect the magnitude of the dispersion forces