1. 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

2. 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:

3. Examples Water can make an aqueous solution with: NaCl
See how water breaks it apart with video link below:
Water cannot make an aqueous solution with:
CaCO3
*forces are too strong to break apart (see solubility chart)

5. 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

6. Examples
C --- O
S ---Cl

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

8. Examples
C --- H
I --- I

9. 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

10. Examples
H2O
NH3

11. 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.

12. Examples O2
CH4

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

14. Examples
Ethanol C2H5OH

15. Boron Trichloride BCl3

16. Benzene C6H6

17. Lithium Bromide LiBr

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