1. BinaryCompounds “The most mind blowing concept one could ever learn.” - N.S. By AK, NS, And JK 2007

2. “-ide” Binary compounds are distinguishable due to the “ide” at the end of the second element in the name.

3. Binary Compounds: A compound with two elements Type 1: “Ionic” (metal + non metal) Charged! “Covalent” (non metal + non metal) Type 2:

4. Ionic Compounds Metal + Non Metal

5. 0 The total charge of all the atoms in an Ionic compound must equal… (zero)

6. With Water (H2O) the Hydrogen has a charge of 1 the Oxygen has a charge of -2 1+1+-2=O It takes two hydrogen atoms to cancel out the charge of the oxygen atom For Example

7. Transition Metals • Transition Metals can be found in the center of the periodic table. • These elements can change their charges depending upon what they are paired with. • These charges are noted in compounds with roman numerals.

8. For Example The transition metal, lead, can have a charge of +4 or +2 With a charge of 2 when paired with oxygen the compound is written as lead(II) oxide. Pb+2 and O-2 = PbO

9. Covalent Compounds Nonmetal+Nonmetal

10. Covalent Compounds • Elements do not develop charges within covalent compounds. • You know how much of each element is in the compound based on the prefixes on the elements in the scientific name.

11. The Prefixes • Mono - 1 (only on second element) • Di - 2 • Tri - 3 • Tetra - 4 • Penta - 5 • Hexa - 6 • Hepta - 7 • Octa - 8 • Nona - 9 • Deca - 10

12. CO2 CO C2O3 Carbon Dioxide Carbon Monoxide Dicarbon Trioxide For Example

13. The End