Chemistry 112 Sections 5-9 Please don’t sit in the last four rows. And, thanks

Chemistry 112 Sections 5-9

Please don’t sit in the last four rows.

And, thanks.

Chemistry 112Sections 5-9

Bill Vining232 PSCI436-2698

viningwj@oneonta.edu

You should have had:

• General Chemistry I– Up through drawing Lewis Structures and

Determining Molecular Structure and Polarity

General Chemistry I

• Basics of Atomic Structure• Chemical Reactions and Equations• Stoichiometry• Solution Chemistry, mainly in water• Thermochemistry• Electronic Structure of Atoms• Properties of Atoms• Ionic Bonding• Covalent Bonding of p-Block Elements• Properties of Gases

General Chemistry II

• IMFs and Properties of Liquids, Solids, and Solutions

• Control of Chemical Reactions and Stability– Thermodynamics– Kinetics

General Chemistry II

• Special Types of Chemical Systems:– Organic– Equilibrium– Acid-Base– Dissolution– Complexation– Electrochemical

Business

Class Rules

• Syllabus

Business I

• Class meetings:– Lecture MWF here– Lab once a week in Physical Sciences Bldg.– Recitation once a week in Physical Sci. Room

122.

• NO LABS or RECITATIONS this week- they start Monday

Business II

• Be here every single day• Be here on time• Don’t sit in back• Don’t talk when I’m talking• Don’t let me talk when you’re talking• It’s ok to get up and wander• Pick up handouts, generally in back• You are responsible• Be nice• Trust me

Classroom Rules

Business III

• 3 Hour Exams• OWL Homework• Labs• Final Exam

Grades

Business IV

If I fail the lab,

Recite After Me:

I fail the course.

Review: Bonding

When atoms stick together, that’s bonding.

Why do Covalent Bonds Form?

Electrons on oneatom attracted tonucleus of other atom

Nucleus on each atom repels other nucleus

Electron on each atom repels other electron

If new attractions > new repulsions, then a bond forms

Determining Molecular Geometry

Valence Lewis Electron-Pair MolecularElectrons Structure Geometry Geometry

Chapter 11Properties of Liquids and Solids

Formula Lewis Structure Electron Geometry

Molecular Geometry Polarity

Intermolecular Forces Properties

What happens when water boils. Draw pictures.

Bonding vs. Intermolecular Forces (IMFs):

Where do IMFs come from?

Types of forces between molecules: Intermolecular Forces (IMFs)

Enthalpy of hydration:

Trends:

Ion-Dipole Forces: Between dissolved ions and polar molecules

Dipole-Dipole Forces: Between polar molecules

Trends:

Dipole-Induced Dipole Forces: Between polar and nonpolar molecules

Trends:

Induced Dipole-Induced Dipole Forces: Between nonpolar molecules

Trends:

Hydrogen Bonding: Molecules with F-H, O-H, or N-H bonds

Hydrogen Bonding: Properties of water

Hydrogen Bonding: Properties of water

More on Boiling Points and Hydrogen Bonding

Identifying IMFs

Relative Contributions of Different IMFs

Properties of Liquids

• Vapor Pressure (volatility)

• Boiling Point

• Enthalpy of Vaporization

• Viscosity

• Surface Tension

Molecular interpretation of vapor pressure and boiling.

Enthalpy of vaporization:

Clausius-Clapyron Equation: Vapor Pressure, Hvap, and T

Graphical Method of Determining Enthalpy of Vaporization

Example 2.

What is the mass of water in the air in this lecture hall?

14 m x 5 m x 17 mT = 22 oCHumidity = 43%

Example 3.A 1-L flask of air is at 30 oC and relative humidity of 68%. The flask is put in a freezer and the temperature decreases to 5 oC. What happens?

Surface Tension