Why can we make so many aqueous solutions? H2O is known as the “universal solvent” because it can dissolve or be miscible with most ionic and polar substances ***Remember the “Like” dissolves “like” rule

Ionic A compound that contains a cation (+) and anion (-) formed through the transferring of electrons. Water can dissolve many ionic compounds because of its attraction to the charges on the compound (opposites attract) See solubility chart for exceptions:

Examples Water can make an aqueous solution with: NaCl See how water breaks it apart with video link below: https://www.youtube.com/watch?v=xdedxfhcpWo Water cannot make an aqueous solution with: CaCO3 *forces are too strong to break apart (see solubility chart)

Polar Bonding Between 2 nonmetals through the unequal sharing of electrons Check electronegativities (.5> and <1.6) Draw dipoles toward the element with greatest electronegative value to show where electron distribution is the greatest

Examples C --- O S ---Cl

Nonpolar Bonding Between 2 nonmetals through the equal sharing of electrons Check electronegativities (<.5) No dipoles are needed

Examples C --- H I --- I

Polar Molecules A covalently bonded substance where dipoles do not cancel because of the unequal distribution of electrons throughout the substance. Based on geometry/asymmetry of the molecule. Most bent and trigonal pyramid substances are polar

Examples H2O NH3

Nonpolar Molecules A covalently bonded substance where dipoles cancel because of the equal distribution of electrons throughout the substance. Based on geometry/symmetry of the molecule.

Examples O2 CH4

Ionic, Polar or Nonpolar? Ethanol C2H5OH Benzene C6H6 Boron Trichloride BCl3 Lithium Bromide LiBr

Examples Ethanol C2H5OH

Boron Trichloride BCl3

Benzene C6H6

Lithium Bromide LiBr

Soluble In Water? Ethanol C2H5OH Benzene C6H6 Boron Trichloride BCl3 Lithium Bromide LiBr