1. Chapter 2: Inorganic Chemistry
Atomic structure and the periodic table
Bonds – ionic, covalent (and hydrogen)
Solubility and polarity, electrolytic properties
Properties of water, hydrogen bonding
Acids, bases and buffers

2. Atomic structure Number of protons Atomic number
Number of protons + number of neutrons
(isotopes vary in # neutrons)
Equal to # of protons
Row on periodic table
Group # (1-8)
(active bonding electrons)
Atomic number
Atomic mass
Number of electrons
Electron energy levels
# valence electrons

4. Bonds involve valence electrons
Metals tend to transfer electrons
Nonmetals tend to take electrons when bonding with metals
Nonmetals tend to share electrons when bonding to other non-metals
Ions: charged atoms due to the gain or loss of electrons
Ionic bonds: cations and anions
Covalent bonds: shared electrons

5. Covalent and Ionic bonds

6. Ionic bonds Metals form cations when they lose valence electrons
Nonmetals form anions when they gain valence electrons
Generally are hydrophilic, dissolve in water, form electrolytes
Ionic equations show the ions into which they separate

7. Covalent bonds Shared electrons Non-metals to non-metals
Do not form ions in solution
May be polar or non-polar covalent
Covalent bonds are stronger than ionic bonds
CHNOPS compounds of living things (“organic”) are covalently bonded

8. H2O is a polar molecule, covalently bonded but with an unequal distribution of shared electrons

9. Water is the “versatile solvent”
The hydrogen bonds
between
hydrogen and
oxygen
cause unique
properties of
water

10. Polar solvents dissolve polar solutes
Sugar dissolves in water
Salt dissolves in water
Only ionic compounds form electrolytes in water

11. Nonpolar solutes do not dissolve in polar solvents (water)
Salad oil
Oil
Gasoline
Vegetable shortening
butter

12. Acids, Bases, Buffers pHyrion paper Acids release H+ in solution
Bases release OH- in solution
Buffers resist changes in pH

13. pH scale

14. Biological systems depend on buffers
Narrow tolerances to changes in pH
Acid rain alters pH of soils and aquatic ecosystems
Limestone is used as a buffer in acidified lakes