1. Types of Chemical Bonds

2. Compound
Substance made by combing two or more elements together (they have no charge)

3. Why do atoms form compounds?
To become chemically stable.
An atom is chemically stable when the outer energy level is complete or full. (Usually 8 Ve-)

4. Atoms or groups of atoms that have a charge
Ions
Atoms or groups of atoms that have a charge
They gain or lose electrons to get 8 Ve-

5. Cation – Positively charged ions. (Metals)
Anions Negatively charged ions (non metals)

6. 2 H2O Coefficient – Represents the # of units of each substance
Subscript – Represents the # of atoms in a molecule of a particular element

7. Superscript – Represents the oxidation # or charge of the ion
Superscript – Represents the oxidation # or charge of the ion. (e- gained or lost)
SO42-
Subscript – Represents the # of atoms in a molecule of a particular element

8. Between Metals and Non Metals ions
Ionic Bonding
Between Metals and Non Metals ions
Electrons are transferred and the opposite charges attract.

9. Can form Multiple Bonds
Covalent Bonding
Between two Non Metals
Electrons are Shared.
Can form Multiple Bonds

10. Ionic Compounds

11. Ionic Compounds
Ion:
Any atom that has a charge
Cation:
An ion with a + charge
anion:
An ion with a - charge

12. A bond that forms between (+) metals and (-) non metals.
Ionic Bonds
A bond that forms between (+) metals and (-) non metals.
Electrons are transferred and then the opposite charges attract.

13. Elements want 8 valence electrons
Octet Rule
Element always move to become more stable. Most elements change their electron configuration to match the configuration of noble gasses.
Elements want 8 valence electrons

14. 1+ 2+ 3+ 3- 2- 1-

15. Rules for Writing Ionic Compounds
1.Charge must always cancel out
+ and – charges add up to zero.
2. Find the charges from the periodic table or the chart.

16. Rules for Writing Ionic Compounds
3.If the charges are the same they cancel out and it is a one to one ratio.
Ca1O1
Ca2+ , O2-

17. 4.If they are not find the least common mutiple
Ca Cl1- = 2
The number that goes in the formula is what you would multiple the charge by to equal the L. C. M.
Ca1Cl2

18. Rules for Writing Ionic Compounds
Or… reduce the charges and use the cross rule
Sn O2-
Ca Cl1-
Sn O1-
Sn O1-
Ca1Cl2
Sn1O2

19. Rules for Naming Ionic Compounds
1. The first element (metal) name does not change.
2. The second elements name ending changes to -ide
NaO
MgCl2
Al2S3

20. Rules for Naming Ionic Compounds
(except for polyatomic ions, use the name on the chart)
SO42-
= sulfate
Na2SO4
= sodium sulfate

21. Rules for Naming Ionic Compounds
3. If it is a transition metal Roman Numerals must be used.
FeCl2
FeCl
FeCl3
The Roman numeral tells you the charge of the transition metal

22. Rules for Naming Ionic Compounds
4. There are no prefixes in ionic compounds