2.solid ionics in the molten state will conduct an electric current
3.ionic solids have relitively high melting points
4.ionic solids are brittle and easily broken
5.ionic solids soluability depends on how strong the bond is b/w cation and anions- stronger the bond the harder to break; type of solvent used-like dissolves like
endothermic
absorbs energy
exothermic
releases energy
ionization energy
the energy require to remove the least tightly held electron from the atom
the larger the atom the easier it is to take an electron off
Electron affinity
the energy released when an atom in its vapor states gains an electron
Naming binary compounds
Name cation+stem of anion+ide
ex.MgI2= magnesium iodide
KBr= potassium bromide
Bond angle
desired angle is 109.5 degrees; tetrahedral
the affect of unbonded pairs decreases the bond angle
104.5 is the accepted value; angular
107 is another pyramid
Angular shape
if 2 atoms are bonded to the central atom the resulting molecule will be angular in shape a bond angle of 104.5 if you have 2 bonded electron pairs and 2 unbonded
Pyramid Shape
if you have 3 atoms bonded to a central atom the resulting molecule will be in the shape of a pyramid with a 107 degree angle
Tetrahydren shape
if you have 4 atoms bonded to a central atom the resulting molecule will be in the shape of a tetrahydren w/ a bond angle of 109.5
if you have 4 bonded pairs 0 will be unbonded
Resonance
there maybe 2 or more lewis structures of a single compound
characteristics of covalent bonding
1.covalent compounds dont normally conduct an electric current
2.they have relitively low melting and boiling points
3.tend to be waxy type solids and relitivly soft
Characteristics of metallics
1. excellent conductors of heat and electricity- to be a conductor you must have charged particles and must be free to move
Look over naming colvant compounds
Van der Waal's Forces
1.London Dispusion force (LDF)
found b/w all molecules
if it werent for LDF you could push molecules together but they wouldnt stay that way