2. Chemical Bond  Chemical bond  force of attraction between atoms in a compound

3.  Chemical Formula  shows the elements that make up a compound & its subscript tells how many of each element

4. Types of Compounds  Ionic compounds  metal + nonmetal  Covalent Compounds  nonmetal + nonmetal

5. Rules for naming Ionic Compounds  Ionic compounds are formed when a metal and nonmetal bond

6. Ionic Compounds Cont.  1. The first element says its name  2. The second element starts to say its name, but changes its ending to ide

7. Examples of Ionic Compounds  Sodium + Chlorine = Sodium Chloride Formula: Na 1 Cl 1  Potassium + Fluorine = Potassium Fluoride Formula: K 1 F 1

8. Rules for Subscripts in Formulas  To determine subscripts, use the element’s oxidation number

9. Oxidation Numbers  Group 1 alkali metals is +1  Group 2 alkali earth metals is +2  Group 13 boron group is +3  Group 14 carbon group is +4 or -4  Group 15 nitrogen group is -3  Group 16 oxygen group is -2  Group 17 halogen group is -1

10. Oxidation cont.  The oxidation numbers cross over to the opposite element and become subscripts  Example : (+2) (-1) Beryllium + Bromine = Beryllium Bromide Formula: Be 1 Br 2

11. More examples of naming  +3 -2 Aluminum + Oxygen = Aluminum Oxide Formula: Al 2 O 3

12. Common nonmetals name  Oxygen → oxide  Sulfur → sulfide  Fluorine → fluoride  Chlorine →chloride  Carbon → carbide  Nitrogen → nitride  Hydrogen → hydride  Bromine → bromide

13. Rules for Covalent Compounds  Covalent Compounds form when a nonmetal and nonmetal bond

14. Covalent Compounds cont.  The first element says its name plus has a prefix which tells the subscript  The second element has a prefix, then starts to say its name, but changes its ending to ide

15. Examples of Covalent Compounds  diBoron + diPhosphorous = B 2 P 2  (mono)Carbon Tetrahydride = C 1 H 4

16. Prefix names  1mono  2di  3tri  4tetra  5penta  6hexa  7hepta  8octa  9nona  10 deca

17. Polyatomic ions  If a compound has more than 2 elements, then it has a polyatomic ion.  Polyatomic ions have special names and charges  See page 173

18. Some Polyatomic Ions (p173)  Ammonia NH 4 Acetate C 2 H 3 O 2  Hydroxide OH Peroxide O 2  Nitrate NO 3 Permanganate MnO 4 Sulfate SO 4 Hydrogen sulfate HSO 4  Carbonate CO 3 Hydrogen carbonate HCO 3  Phosphate PO 4 Hydrogen Phosphate HPO 4  Chromate CrO 4 Dichromate Cr 2 O 7  Silicate SiO 3 Hypochlorite OCl

19. Properties of Acids  Taste sour  Contain Hydrogen (H)  React w/ metals to produce Hydrogen  Litmus from blue to red

20. Name of AcidFormulaWhere Found Acetic acidHC 2 H 3 O 2 Vinegar Boric acidH 3 BO 3 Eyewash Carbonic acid H 2 CO 3 Rain water, soft drinks Hydrochloric acid HClGastric juice Citric acidH3C6H5O7H3C6H5O7 Citrus fruit Sulfuric acidH 2 SO 4 Batteries, acid rain

21. Properties of Bases  Taste bitter  Contain OH polyatomic  Feels slippery  Litmus from red to blue

22. Name of BaseFormulaWhere Found Aluminum hydroxide Al(OH) 3 Deodorants, antacids Magnesium hydroxide Mg(OH) 2 Laxatives, antacids Potassium hydroxide KOHSoap, glass Sodium hydroxide NaOHDrain cleaner, soap making Calcium hydroxide Ca(OH) 2 mortar