1. Ionic and Covalent Compounds
Mrs. Taylor

2. Millions of compounds form from the elements of the periodic table
Naming is essential in chemistry

3. Two Types of Compounds
Ionic
Covalent

4. Ionic Compounds
Are formed between metals and nonmetals

5. CO2 NH3 H2O O2 N2 H2 Covalent Compounds
Are formed between 2 or more nonmetals
Compound may be formed between two different nonmetals
Compound may be formed between two of the same nonmetals.
CO NH H2O
O N H2

6. Exit Ticket 1. Where are metals located? Right or left?
2. Which element is the exception?
3. Ionic Compounds are formed between __________ and ___________.
4. Covalent Compounds are formed between ___________________.
5. Give an example of an ionic bond.
6. Give an example of a covalent bond.

7. COMPOUND FORMATION
Elements want to form bonds so that they can achieve eight electrons in their outer most energy level. THIS IS AN OCTET!
The electrons in the outermost level are called valence electrons

8. Valence Electrons
We can determine the number of valence electrons an element has by the group of the periodic table that the element is in.

9. HELIUM is the only exception
HELIUM is the only exception! Helium is has 2 electrons even though it is in the last group!

10. IONIC COMPOUND FORMATION
When an atom of a nonmetal takes one or more electron from an atom of a metal so both atoms end up with eight valence electrons
In other words, a nonmetal is gaining an electrons (anion) and a metal is losing electrons (cation).
We can think of ionic bonds as an attraction between positive and negative particles.

12. Determining Charges of the Periodic Table (WRITE THEM ON YOUR PT)

13. Writing Formulas for Ionic Compounds: (No transition metals)
Made of metals and nonmetals
Metal always goes first, nonmetal goes second
Name ends in –ide if no polyatomic ion present
Net ionic charge must = zero
If ionic charges are equal in magnitude but opposite in sign, they cancel
If there is a polyatomic ion, put parenthesis around it

14. Polyatomic Ion
Covalently bonded group of nonmetal elements with a charge.
Ex: CO NH4+

15. Practice Calcium nitride Sodium oxide Lithium Chloride
Magnesium sulfide
 Lithium carbonate
Magnesium sulfate
Calcium phosphate
Aluminum acetate

16. C. Naming Ionic Compounds: Those that do NOT contain a transition metal  
Name ends in –ide unless there is a polyatomic ion present
Just write the name of the ions you see

17. Practice
NaBr
CaCl2
Mg3(PO4)2
Li2SO4

18. A. Writing Formulas for Molecular Compounds
Prefixes tell you the number of each type of atom
Do NOT criss cross any numbers!

19. Practice Dichlorine tetrafluoride Nitrogen triodide
Trisulfur hexafluoride
 Carbon monoxide
Tetrabromine hexanitride

20. B. Naming Molecular Compounds
If there is a single atom of the first element, omit ­mono-
Name ends in –ide

21. Practice
P2O5
S2Cl6
CO2
Cl2O
CCl4

22. S U P E R 7 Diatomic Molecules Elements that do not exist alone.
There are seven. (N2, O2, F2, Cl2, Br2, I2 and H2)

23. Exceptions to the Rules
H2O  Water
NH3  Ammonia