We think you have liked this presentation. If you wish to download it, please recommend it to your friends in any social system. Share buttons are a little bit lower. Thank you!
Presentation is loading. Please wait.
Published byRosamond Sparks
Modified over 4 years ago
I. Intermolecular Forces (Ch. 6, p.189-193)Ch Liquids & Solids I. Intermolecular Forces (Ch. 6, p )
A. Definition of IMF Attractive forces between molecules.Much weaker than chemical bonds within molecules.
B. Types of IMF
B. Types of IMF London Dispersion Forces View animation online.
B. Types of IMF Attractive forces that arise as a result of temporary dipoles induced in atoms or molecules ion-induced dipole interaction dipole-induced dipole interaction 11.2
B. Types of IMF Dipole-Dipole Forces + - View animation online.
B. Types of IMF Hydrogen Bonding
C. Determining IMF NCl3 polar = dispersion, dipole-dipole CH4nonpolar = dispersion HF H-F bond = dispersion, dipole-dipole, hydrogen bonding
II. Physical Properties (p. 363 - 371)Ch Liquids & Solids II. Physical Properties (p )
A. Liquids vs. Solids IMF Strength Fluid Density CompressibleDiffusion LIQUIDS Stronger than in gases Y high N slower than in gases SOLIDS Very strong N high extremely slow
A. Liquids vs. Solids A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well-defined boundary.
B. Liquid Properties Surface Tensionattractive force between particles in a liquid that minimizes surface area
B. Liquid Properties Capillary Actionattractive force between the surface of a liquid and the surface of a solid water mercury
B. Liquid Properties Adhesion Cohesion
Water is a Unique SubstanceMaximum Density 40C Density of Water Water is a Unique Substance 11.3
C. Types of Solids Crystalline - repeating geometric patterncovalent network metallic ionic covalent molecular Amorphous - no geometric pattern decreasing m.p.
C. Types of Solids Ionic (NaCl) Metallic
C. Types of Solids Covalent Molecular Covalent Network Amorphous (H2O)(SiO2 - quartz) Amorphous (SiO2 - glass)
C. Types of Solids Diamond Graphite
C. Types of Solids
III. Changes of State (p. 372 - 382)Ch Liquids & Solids III. Changes of State (p )
A. Phase Changes
A. Phase Changes Evaporationmolecules at the surface gain enough energy to overcome IMF Volatility measure of evaporation rate depends on temp & IMF
Greatest Order Least T2 > T1 Evaporation Condensation
A. Phase Changes temp volatility IMF volatility Boltzmann Distribution# of Particles volatility IMF volatility Kinetic Energy
A. Phase Changes Equilibriumtrapped molecules reach a balance between evaporation & condensation
A. Phase Changes Vapor Pressurepressure of vapor above a liquid at equilibrium depends on temp & IMF directly related to volatility
A. Phase Changes IMF v.p. v.p. temp
A. Phase Changes Patm b.p. IMF b.p. Boiling Pointtemp at which v.p. of liquid equals external pressure depends on Patm & IMF Normal B.P. - b.p. at 1 atm Patm b.p. IMF b.p.
A. Phase Changes IMF m.p. Melting Point equal to freezing pointWhich has a higher m.p.? polar or nonpolar? covalent or ionic? polar ionic
A. Phase Changes Sublimation solid gasv.p. of solid equals external pressure EX: dry ice, mothballs, solid air fresheners
B. Heating Curves Gas - KE Boiling - PE Liquid - KE Melting - PE Solid - KE
B. Heating Curves Heat of Vaporization (Hvap)energy required to boil 1 gram of a substance at its b.p. usually larger than Hfus…why? EX: sweating, steam burns, the drinking bird
B. Heating Curves Temperature Change change in KE (molecular motion)depends on heat capacity Heat Capacity energy required to raise the temp of 1 gram of a substance by 1°C
B. Heating Curves Phase Change change in PE (molecular arrangement)temp remains constant Heat of Fusion (Hfus) energy required to melt 1 gram of a substance at its m.p.
C. Phase Diagrams Show the phases of a substance at different temps and pressures.
C. Phase Diagrams
III. Changes of State (p )
II. Physical Properties (p )
Liquids and Solids Chapter 13.
Intermolecular Forces and
I. Kinetic Molecular Theory KMT
States of Matter Newport High School Academic Chemistry Modified from a PowerPoint found at
I. Kinetic Molecular Theory KMT. Assumptions of KMT All matter is composed of tiny particles These particles are in constant, random motion. Some particles.
Unit 11: States of Matter Ch. 13, Sections 2-4. ++ -- Types of Covalent Bonds Polar Covalent Bond –e - are shared unequally –asymmetrical e - density.
LIQUIDS AND SOLIDS. LIQUIDS: Why are they the least common state of matter? 1. Liquids and K.M.T. Are particles in constant motion? Spacing? Kinetic.
Liquids and Solids.
H 2 O (s) H 2 O ( ) H 2 O (g). The state (or phase) of matter is determined by the arrangement and motion of particles. The motion of particles is governed.
Chapter 14: Liquids and Solids
Ch. 12 – States of Matter I. Intermolecular Forces.
1 Intermolecular Forces and Liquids and Solids Chapter 12 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Ch. 10 – Changes of State (p. 324 – 330). Phases The phase of a substance is determined by three things. The temperature. The pressure. The strength.
Intermolecular Forces and Liquids and Solids Chapter 14.
Intermolecular Forces and Liquids and Solids Chapter 11.
© 2020 SlidePlayer.com Inc. All rights reserved.