GENCHEM

• The theory that assumes that gases consist of widely separated molecules of negligible volume that are in constant motion, colliding elastically with one another and the walls of their container with average velocities determined by their absolute temperatures.


  Kinetic Molecular Theory
• When solids or liquids are heated up, the kinetic energy of their particles increases causing them to move faster.
• Intramolecular forces are the forces that hold atoms together within a

  molecule. Intermolecular forces are forces that exist between molecules.
• Kinetic Energy is the energy of particles in motion. It keeps the particles apart from each other. It counters the effect of intermolecular forces and it is proportional to the increase in temperature.
• This bond is formed by the complete transfer of valence

  electron(s) between atoms.

  Ionic bond
• This bond is formed by the complete transfer of valence

  electron(s) between atoms.

  Ionic bond
• In ionic bonds, the metal loses electrons to become a positively charged cation, whereas the nonmetal accepts those electrons to become a negatively charged anion.
• This bond is formed between atoms that have similar

  electronegativities—the affinity or desire for electrons.


  Covalent bond
• Because both atoms have similar affinity for electrons and neither has a tendency to donate them, they share electrons in order to achieve octet configuration and become more stable.


  Covalent bond
• A nonpolar covalent bond is formed between same atoms or

  atoms with very similar electronegativities—the difference in

  electronegativity between bonded atoms is less than 0.5.
• A polar covalent bond is formed when atoms of slightly different electronegativities share electrons. The difference in electronegativity between bonded atoms is between 0.5 and 1.9.
• This type of covalent bonding specifically occurs between atoms of metals, in which the valence electrons are free to move through the

  lattice.


  Metallic bond
• This bond is formed via the attraction of the mobile electrons—referred to as sea of electrons—and the fixed positively charged metal ions.


  Metallic bond
• What are the 3 types of intramolecular forces?

  Ionic, Covalent, Metallic
• What are the 3 types of Intermolecular forces?

  London dispersion forces, dipole-dipole interactions, hydrogen bonding
• result from the coulombic interactions between instantaneous dipoles. Dispersion forces are present between all molecules (and atoms) and are typically greater for heavier, more polarizable molecules and molecules with larger surface areas.


  London Dispersion Forces
• occur between molecules with permanent dipoles (i.e., polar

  molecules). For molecules of similar size and mass, the strength

  of these forces increases with increasing polarity. Polar

  molecules can also induce dipoles in nonpolar molecules,

  resulting in dipole–induced dipole forces.

  Dipole-dipole forces
• is a special type of dipole-dipole interaction that occurs between the lone pair of a highly electronegative atom (typically N, O, or F) and the hydrogen atom in a N–H, O–H, or F–H bond.


  Hydrogen Bonding
• The weakest intermolecular force, a distance-dependent interaction between atoms or molecules, and consists of dipole-dipole forces and dispersion forces.


  Van der Waals force
• Van der Waals force was named after a Dutch physicist named...


  Johannes Diderik van der Waals
• have definite volume but no definite shape


  Liquid
• Their particles are held closely together by the strong intermolecular forces but not strong enough to keep them in a rigid position. The

  particles are then free to slide over one another.


  Liquid
• have definite volume and shape


  Solid
• They are denser than liquids and are not easily compressed because their particles are tightly packed. The intermolecular forces between their particles are stronger than those in liquids, enough to make the solids rigid. 


  Solid
• Solid to liquid


  Melting
• Liquid to solid


  Freezing
• Liquid to Gas


  Vaporization
• Gas to Liquid

  Condensation
• Gas to Solid

  Deposition
• Solid to Gas


  Sublimation
• Gas to Plasma

  Ionization
• Plasma to Gas

  Deionization
• The resistance of a liquid to flow.


  Viscosity
• The pressure exerted by gas molecules above a liquid.

  Vapor Pressure
• Attraction between surface molecules in a liquid. Attractive forces at the surface pull molecules inward causing surface molecules to be held more tightly.


  Surface Tension
• Temperature at which a liquid changes to gas.


  Boiling point
• the amount of heat required to vaporize one mole of a substance at its boiling point.

  Molar heat of vaporization
• Boiling point generally increases as molar heat of vaporization increases.
• Solutions are mixtures of two or more substances evenly distributed throughout a single phase.
• Solutions are composed of solute and solvent.