Unit 9

• the fundamental difference between states of matter is

  distance between particles
• total disorder; much empty space; particles have complete freedom of motion; particles far apart

  gas
• ordered arrangement; particles are essentially in fixed position; particles close together

  crystalline solid
• comparison between states of matter

  A) conforms to shape and volume of container

  B) high

  C) high

  D) conform to shape of container volume limited by surface

  E) very low

  F) moderate

  G) maintains its own shape and volume

  H) almost none

  I) almost none

  
• forces that are found within a molecule

  intramolecular or bonding forces
• intramolecular or bonding forces are found within a molecule
• intermolecular or nonbonding forces are found between molecules
• forces that are found between molecules

  intermolecular or nonbonding forces
• intramolecular and intermolecular forces

  A) strong intramolecular attraction (covalent bond)

  B) weak intermolecular attraction

  
• arise from the attraction between molecules with partial charge, or between ions and molecules


  intermolecular forces
• intermolecular forces are relatively weak compared to bonding forces because they involve smaller charges that are farther apart
• properties of liquids such as boiling point and melting point reflect the strength of IMFs
• comparison between bonding (intramolecular) and nonbonding (intermolecular) forces

  A) ionic

  B) cation-anion

  C) 400-4000

  D) NaCl

  E) covalent

  F) nuclei-shared e- pair

  G) 150-1100

  H) H-H

  I) metallic

  J) cations-delocalized elecrons

  K) 75-100

  L) Fe

  
• what are examples of bonding forces?

  ionic

  covalent

  metallic
• nonbonding (intermolecular) forces

  A) ion-dipole

  B) h bond

  C) dipole-dipole

  D) ion-induced dipole

  E) dipole-induced dipole

  F) dispersion (london)

  G) ion charge - dipole charge

  H) polar bond to dipole charge (high in EN of N, O , F)

  I) dipole charges

  J) ion charge - polarizable e- cloud

  K) dipole charge - polarizable e- cloud

  L) polarizable e- cloud

  M) 40-600

  N) 10-40

  O) 5-25

  P) 3-15

  Q) 2-10

  R) 0.05-40

  
• example of intermolecular or nonbonding forces are

  ion-dipole

  h-bond

  dipole-dipole

  ion-induced dipole

  dipole-induced dipole

  dispersion (london)
• what are the four types of intermolecular or nonbonding forces?


  dispersion (london) forces

  dipole-dipole

  hydrogen bonding

  ion-dipole forces
• these intermolecular or nonbonding forces are called van der waals forces

  dispersion/london forces

  dipole-dipole forces
• a temporary attractive forces that result when electrons in two adjacent atoms occupy positions that make the atom form temporary dipoles

  london dispersion forces
• also called london dispersion forces

  dispersion forces
• weakest Intermolecular forces and present in all molecules

  london dispersion forces
• the only force found in nonpolar molecules

  london dispersion forces
• • a temporary attractive forces that result when electrons in two adjacent atom occupy positions that make the atoms form temporary dipoles
  • also called London Dispersion Forces
  • weakest intermolecular forces (IMF) present in all molecules
  • the only force found in nonpolar molecules


  london dispersion forces
• when atoms are apart they do not influence one another

  london dispersion forces
• when atoms are close together, the instantaneous dipole in one atom induces a dipole in the other

  london dispersion forces
• • when atoms are far apart they do not influence one another
  • when atoms are close together, the instantaneous dipole in one atom induces a dipole in the other
  • the process occurs throughout the sample

  london dispersion forces
• attractive forces between polar molecules

  dipole-dipole forces
• similar in orgin to hydrogen bonding but weaker

  dipole-dipole forces
• increases with increasing polarity

  dipole-dipole forces
• • attractive forces between polar molecules
  • similar in origin to hydrogen bonding but weaker
  • increases with increasing polarity


  dipole-dipole forces
• attraction between dipole molecules

  dipole-dipole forces
• for molecules of approximately equal mass and size the strength of intermolecular attraction increases with increasing polarity


  dipole-dipole forces
• • attraction between polar molecules
  • for molecules of approximately equal mass and size the strength of intermolecular attraction increases with increasing polarity

  dipole-dipole forces
• an intermolecular hydrogen bonding is the attraction between hydrogen atom of one molecule and a lone pair of the N, O, or F atom of another molecule

  hydrogen bonding
• what are the elements present in hydrogen bonding?

  hydrogen

  nitrogen

  oxygen

  fluorine
• it is the strongest intermolecular force (IMF)

  hydrogen bonding
• a special type of dipole-dipole attraction

  hydrogen bonding
• • an intermolecular hydrogen bonding is the attraction between the hydrogen atom of one molecule and a lone pair of the N, O, or F atom of another molecule
  • the strongest intermolecular force (IMF)
  • a special type of dipole-dipole attraction

  hydrogen bonding
• occurs when ionic compound is mixed with a polar compound


  ion-dipole forces
• the positively charged end of a polar molecule such as H2O is attracted to negative ions and the negatively charged end of the molecule is attracted to positive ions

  ion-dipole force