Enter your Sign on user name and password.

Forgot password?
Sign In | Subscribe
Start learning today, and be successful in your academic & professional career. Start Today!
Loading video...
This is a quick preview of the lesson. For full access, please Log In or Sign up.
For more information, please see full course syllabus of Chemistry
  • Discussion

  • Study Guides

  • Download Lecture Slides

  • Table of Contents

  • Related Books & Services

Lecture Comments (6)

0 answers

Post by Zachary McCoy on January 4, 2014

Please note: The far more common term used in America for the phase change of gas to solid is "deposition," not "condensation." Alternatively, "desublimation."

2 answers

Last reply by: Zachary McCoy
Sat Jan 4, 2014 8:48 PM

Post by Su Jung Leem on July 24, 2012

why is there a trinagle in front of the abbreviated letters for things like condensation and evaporation?

1 answer

Last reply by: Zachary McCoy
Sat Jan 4, 2014 9:43 PM

Post by Alysha Haeems on November 6, 2011

at 45:09 he says "ass lore"

Related Articles:

States of Matter, Intermolecular Forces, Gases and Gas laws

  • States of matter are solid (s), liquid (l), and gas (g)

  • Phase changes have names: freezing/melting; boiling/condensing

  • Solid going directly to gas: subliming; example dry ice, CO2(g)

  • Forces between particles in decreasing order of strength are: ionic; ion/dipole; hydrogen bonding; dipole/dipole; London (dispersion)

  • H-bonding only for O…H; N…H; F…H

  • H-bonding very important in proteins, nucleic acids

  • The atmosphere: nitrogen, oxygen and 1% argon

  • Pressure = F/A

  • Units of pressure can be Pascals (SI); atmospheres (1 atm. = 760 mm Hg = 760 torr)

  • Kinetic molecular theory models gases as rapidly randomly moving molecules

  • Ideal gas law (includes other gas laws) PV = nRT; watch for consistency of units.

  • Molar mass of gas from gas density measurements: PV = (m/M)RT

States of Matter, Intermolecular Forces, Gases and Gas laws

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

  • Intro 0:00
  • States of Matter: Solid, Liquid, Gas 0:43
    • Solid
    • Liquid
    • Gas
  • Phase Transitions 4:36
    • Melting, Freezing, Boiling, Condensing
    • Sublimation, Condensation
    • Example: Dry Ice
  • Ionic Forces and Ion Dipole Forces 8:42
    • Example: Ionic Forces
    • Example: Ion Dipole Forces (Polar)
  • Dipole-Dipole Forces and Hydrogen Bonding 15:51
    • Example: Water Molecules
    • Example: Liquid Hydrogen Chloride
    • Strong Dipole-Dipole, Hydrogen Bonds
    • Boiling Points
  • Dispersion or London Forces 22:36
    • Boiling Points of Noble Gases
  • Hydrogen Bonding in Water and Biological Systems 28:17
    • Example: Crystalline Water (Open Structure)
    • Example: Protein
    • Example: DNA Double Helix
  • Gaseous State: Kinetic Molecular Model 31:00
  • Gases of the Atmosphere 33:31
    • Percentage by Volume
  • Pressure 33:15
    • Mercury Barometer
  • Units of Pressure 38:33
    • Pascal
    • Bar, Torr, Atm
  • Gas Laws and the Ideal Gas Law 41:47
    • Boyle's Law
    • Charles' Law
    • Ideal Gas Law (Combined Law)
    • Gas Constant R
  • Example: Gas Law Calculations 45:02
  • Molar Mass from Gas Law Calculations 47:21
    • Example: Experimental Gas
  • Additional Example 1
  • Additional Example 2