Chemistry Chapter 4

• b/w atoms; very strong
• ionic bonds
• covalent bonds
• metallic bonds

• formed by the transfer of electrons
• produce ions
• form cation or anion
• salts

• sharing of electrons
• form molecules
• 1.single covalent bond
• 2.double covalent bond
• 3.triple covalent bond
• 4.coordinate covalent bond

• true metals
• Cu, Ag, etc.

• b/w molecules (weak)
• 1.van der waal's forces
• -London Dispersion forces
• -dipole-dipole
• 2.hydrogen bond (H-FON)

• 1.solid ionic crystles don't conduct electricity
• 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

absorbs energy

releases 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

the energy released when an atom in its vapor states gains an electron

Name cation+stem of anion+ide

• ex.MgI₂= magnesium iodide
• KBr= potassium bromide

• 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

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

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

• 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

there maybe 2 or more lewis structures of a single compound

• 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

1. excellent conductors of heat and electricity- to be a conductor you must have charged particles and must be free to move

• found b/w all molecules
• if it werent for LDF you could push molecules together but they wouldnt stay that way
• such as in cooling

• must have polar molecules
• its an additional force of attraction

• 1.H-FON
• usually have high boiling points