1. Sharing is Caring

2.  Make a web that includes the 3 types of bonds we’ve discussed – Ionic, Covalent, and Metallic

3.  Bond between two nonmetals  They SHARE electrons

4.  Electronegativity!  Electronegativity – the tendency of an atom to gain electrons in a chemical bond.  If the difference between the electronegativity's is large, the bond tends to be ionic. is small – it tends to be covalent  Compounds can have both, but usually show one type more than the other chemically, usually tend to be ionic

5.  1. Diatomic Molecules There are 7 diatomic molecules H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2 NEVER found as single atoms if “alone” (That’s why they all have a 2 Naming: Their names are just the name of the element

6.  2. Binary Molecular Compounds Nonmetals without Hydrogens (H)  Formula DOES NOT start with an H Naming  1. First Element – Use the entire name of the element  2. Second Element – Change the ending to –ide  3. USE NUMERIC PREFIXES  Only time you won’t use a prefix is if there is only one atom of a particular element.  DO NOT WORRY OR EVEN THINK ABOUT CHARGES!!

8.  CCl 4  As 2 O 3

9. Always begin with H + Two Types  Binary  Oxyacid *** Remember: The number of hydrogen atoms in the acid equals the charge of the anion

10.  3. Binary Acids Have an H + but no O Naming  1. Use the prefix – hydro  2. Then take the root of the second acid  3. Add –ic to the end  4. Follow with acid

11.  HCl  1. Hydro  2. Chlor  3. –ic  4. Acid  Hydrochloric Acid

12.  4. Oxyacids Must have a polyatomic ion Naming  1. Identify the polyatomic ion  2. Use the root of the anion  3. Depending on the suffix (end)  If it ends in –ate  change to –ic  If it ends in –ite  change to –ous

13.  HNO 3 -  1. Identify the polyatomic ion – Nitrate  2. Use the root of the anion – Nitr  3. Depending on the suffix (end)  If it ends in –ate  change to –ic  If it ends in –ite  change to –ous Nitric Acid Nitrate – ends in –ate So change to –ic

14.  Compound containing carbon and hydrogen  Named using prefixes that correspond to the number of carbons in the compound. 1 – meth 2 – eth 3 – prop 4 – but  After this it used the “normal” prefixes

15.  Ending refers to the type of functional group found in the compound. -ane – alkane - simplest hydrocarbon - only has single bonded carbons with hydrogens -ene – alkene - has a double bonded carbon in the formula -yne – alkyne - has a triple bonded carbon in the formula

16.  Examples 1. 2.

17. FormulaType of Covalent BondName PCl 5 HI N2N2 C2H6C2H6 H 3 PO 4 HClO 2 N2H4N2H4 Dinitrogen tetrahydride Phosphic acid Nitrogen Hydroiodic acid Binary Molecular Diatomic Binary Acid Phosphorous pentachloride Binary Molecular Oxyacid Chlorous acid Hydrocarbonethane