1 / 79

Gases, Liquids, and Solids: Characteristics and Intermolecular Forces

This chapter explores the characteristics of gases, liquids, and solids, including their volume, shape, and attractive forces. It also delves into the different types of intermolecular forces, such as London dispersion forces, dipole-dipole attraction, hydrogen bonding, and ion-dipole attraction, and their effects on boiling points and vapor pressure. In addition, the properties of ionic solids, including high melting points, strong electrostatic forces, and brittleness, are discussed.

mouser
Download Presentation

Gases, Liquids, and Solids: Characteristics and Intermolecular Forces

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Liquids & Solids Chapter 13

  2. Gases • Characteristics: -no definite volume or shape; takes on shape of container -virtually no attractive forces -can be compressed

  3. Liquids • Characteristics -definite volume but no definite shape; takes on shape of container -strong attractive forces -need to determine what kind!!! -really can’t be compressed

  4. Solids • Characteristics -definite volume -definite shape -strong attractive forces -need to determine what kind!!! -really can’t be compressed

  5. Quick Check • Has no definite shape, but has a definite volume = • Has a definite volume and a definite shape = • Gas =

  6. Intramolecular vs Intermolecular • Intramolecular - the attraction that results when electrons are given, taken or shared to form a bond.

  7. Intramolecular vs Intermolecular • Intermolecular - the attraction of a molecule or particle to another molecule or particle.

  8. Intramolecular vs. Intermolecular • Intramolecular forces are always much, MUCH stronger than intermolecular forces

  9. Types of Intermolecular Forces • London Dispersion Forces(LDF) - or Van der Waal’s forces. a) attraction between nonpolar molecules-nonpolar molecules. - how do you know if it’s nonpolar? b) Key word is Polarizable - how easy it is to distort a charge.

  10. Types of Intermolecular Forces Polarization Nonpolar - even distribution of charge

  11. Types of Intermolecular Forces Polarization - + Nonpolar Instant dipole

  12. Types of Intermolecular Forces Polarization - + - + Nonpolar Instant dipole Influences others around it

  13. Types of Intermolecular Forces London Dispersion Forces 1) Induced or “fake” charge. Molecules will line up + to -. Best stuff to induce a charge?

  14. Types of Intermolecular Forces • 1) Big nonpolar molecules (radius)- large electron clouds which induce easier. • A) Hydrocarbons?

  15. Types of Intermolecular Forces • 1) Big nonpolar molecules • A) Hydrocarbons? • B) Halogens?

  16. Types of Intermolecular Forces • 1) Big nonpolar molecules • A) Hydrocarbons? • B) Halogens? • C) Noble Gases

  17. Types of Intermolecular Forces • 2) Slow moving(large mass) - easier to induce charge when moving slow. -> small gases are almost impossible to induce charge

  18. Types of Intermolecular Forces Ways to Increase LDF: • Increase the size(radius and mass) • Bigger mass = MORE POLARIZABLE • More polarizable, bigger temporary diopole, holds together better

  19. Types of Intermolecular Forces Ways to Increase LDF: • In organic molecules, the longer the chain, the greater the opportunity to induce a charge. Long carbon chains vs isomers?

  20. Types of Intermolecular Forces • All molecules have LDF • In nonpolar molecules, LDF is the ONLY force • In other molecules, there are stronger IM forces. Such as…..

  21. Types of Intermolecular Forces • 2) Dipole-Dipole Attraction - polar molecules attracted to other polar molecules. • How do you know if it’s polar?

  22. Types of Intermolecular Forces • In general, dipole-dipole forces are stronger than LDF. • Why? • In what situation would LDF be stronger than dipole-dipole?

  23. Types of Intermolecular Forces • Hydrogen Bonding - not bonding! a) Attraction between Hydrogen and a very electronegative atom(upper right) F, O, N, S

  24. Types of Intermolecular Forces • Hydrogen Bonding - not bonding! a) Attraction between Hydrogen and a very electronegative atom(upper right) F, O, N b) Really a special dipole-dipole-> about 10 x stronger special. What does that mean? Increase in attraction!

  25. Types of Intermolecular Forces • Hydrogen Bonding - not bonding! c) Big 3: NH3, HF, H20 d) Alcohols show hydrogen bonding- get more attraction e) Dimers - a molecule that has two hydrogen bonds

  26. Types of Intermolecular Forces 1b) Ion-Dipole Attraction - attraction of ion and the partial charge of the molecule.

  27. Types of Intermolecular Forces 1b) Ion-Dipole Attraction - attraction of ion and the partial charge of the molecule. I) Important in solution making

  28. Types of Intermolecular Forces 1b) Ion-Dipole Attraction - attraction of ion and the partial charge of the molecule. i) Important in solution making. ii) Strength becomes greater when charge of ion is greater and/or the size of dipole is stronger.

  29. Types of Intermolecular Forces Strength? About 1% of ionic or covalent. Becomes weaker when the distance between molecules increase. Why?

  30. Intermolecular Forces • Look at how these forces will effect the following: -> Boiling Points -> Vapor Pressure

  31. SOLIDS Types of Solids and their properties

  32. Ionic Solids Ionic solids have ions at the points of the lattice. Ex: NaCl

  33. Ionic Solids • Characteristics: 1) High Melting Points

  34. Ionic Solids • Characteristics: 1) High Melting Points 2) Held together by strong electrostatic forces [Coulomb’s Law] a) the greater the charges of the ions, the greater the electrostatic forces. EX: CaCl2 vs NaCl b) The smaller the ions the greater the attraction. EX: KBr vs. LiF

  35. Ionic Solids • Characteristics: 3) Brittle

  36. Ionic Solids • Characteristics: 3) Brittle 4) Insulator-won’t conduct in solid state

  37. Ionic Solids • Characteristics: 3) Brittle 4) Insulator-won’t conduct in solid state 5) Will conduct in molten state or when dissolved

  38. Molecular Solids • Molecular solids have molecules at the points of lattice. EX: Ice, sugar • Held together by dipole-dipole, hydrogen bonding or London dispersion forces-Intermolecular forces

  39. Molecular Solids • Characteristics: 1) Stronger intramolecular than intermolecular

  40. Molecular Solids • Characteristics: 1) Stronger intramolecular than intermolecular 2) Most only have London dispersion- therfore they need to be big molecules.

  41. Molecular Solids • Characteristics: 3) Soft

  42. Molecular Solids • Characteristics: 3) Soft 4) Low melting points

  43. Molecular Solids • Characteristics: 3) Soft 4) Low melting points 5) Insulator

  44. Atomic Solids • Have atoms at the points of their lattice

  45. Atomic Solids • Two Types: 1) Metallic Solids - metal atoms at the points of lattice. A) Free moving(nondirectional) “sea” of valence electrons

  46. Atomic Solids Metallic Solids - metal atoms at the points of lattice. B) Close packing- arrangement that is most efficient use of space.

  47. Atomic Solids Metallic Solids - metal atoms at the points of lattice. B) Close packing- arrangement that is most efficient use of space. 1) Hexagonal close packing - 1st layer in line with 3rd layer

  48. Atomic Solids Metallic Solids - metal atoms at the points of lattice. B) Close packing- arrangement that is most efficient use of space. 1) Hexagonal close packing - 1st layer in line with 3rd layer 2) Cubic close packing - 1st layer in line with 4th layer

  49. Atomic Solids Metallic Solids - metal atoms at the points of lattice. C) Characteristics: 1. Wide range of melting points.

More Related