1. The Basics of Ionic Chemical Bonding
Unit 3: Types of Bonding
The Basics of Ionic Chemical Bonding

2. Three types of bonding:
Ionic Bonding:
electrons are transferred
(between a metal and non-metal)
Covalent Bonding:
electrons are shared
(between a non-metal and non-metal)
Metallic Bonding
electrons flow freely
(within a metal)

4. Introduction to Ionic Bonding
An ionic bond forms from the attraction between + and – ions.
An ionic compound is made up of crystals
A crystal consists of a 3D, repeating pattern of alternating + and – ions.

5. Examples: The formation of ionic compounds
Use electron dot structures to predict the compounds that would form between Sodium and Fluorine:
To write the formula write the metal first, then the nonmetal… F Na
NaF
**Naming Ionic compounds: Metal Nonmetal (change the ending on the nonmetal to –ide)
Name: Sodium Fluoride

6. Examples: The formation of ionic compounds
Use electron dot structures to predict the compounds that would form between Magnesium and Chlorine: Cl Mg
MgCl2 Cl
**Naming Ionic compounds: Metal Nonmetal (change the ending on the nonmetal to –ide)
Name: Magnesium Chloride

7. Examples: The formation of ionic compounds
Use electron dot structures to predict the compounds that would form between Aluminum and Sulfur: Al S Al S
Al2S3 S
**Naming Ionic compounds: Metal Nonmetal (change the ending on the nonmetal to –ide)
Name: Aluminum sulfide

8. Chemistry Humor 

9. Ions can be monatomic or polyatomic:
Monatomic: Made up of a single atom
Polyatomic: Made up of multiple atoms
Remember…
Group #:
Charge: X 

10. Polyatomic ions: (See polyatomic ion sheet) are made up of two or more elements covalently bonded together with an overall positive or negative charge.
*The six polyatomic ions that have asterisk with them have to be memorized.

11. Chemical Name to Formula
Aluminum Sulfite Al+3 (SO3)-2 (SO3)-2
Al2(SO3)3

12. You can work backwards to determine the charge on transition metals!
More Examples
Silver Sulfate Ag? (SO4)-2 Ag+1
Ag2(SO4)
Ag+1
You can work backwards to determine the charge on transition metals!

13. More Examples
Calcium Bromide Ca+2 Br-1 Br-1
CaBr2

14. Parentheses () are optional when only one polyatomic ion is needed.
More Examples
Lithium Nitrate Li+1 (NO3)-1
LiNO3
Parentheses () are optional when only one polyatomic ion is needed.

15. But what if the metal is a transition metal?
The Roman Numeral in the name represents the charge on the cation.
Example: Nickel (II) Nitrate

16. More Examples Nickel (II) Nitrate Ni+2 (NO3)-1 (NO3)-1 Ni(NO3)2
The Roman Numeral will always tell you the charge and it will always be positive

17. More Examples
Iron (III) Chloride Fe+3 Cl-1 Cl-1
FeCl3

18. Chemical Formula to Name
Recall the format for chemical formulas… (name of cation – metal) (name of anion – nonmetal) Examples: KBr CaI2 Na2(SO4)
Potassium Bromide
Calcium Iodide
Sodium Sulfate

19. For elements with more than one possible charge (transition metals)… Use the charge on the anion to determine the charge on the cation! Example: Fe2(CrO4)3
+6/2=+3
-2(3)=-6
Iron (III) Chromate

20. Example: Sn(CO3)2 +4
-2(2)=-4
Tin (IV) Carbonate

21. Example: Cu3P
+3/3=+1 -3
Copper (I) Phosphide

22. Example: Co2(CrO4)3
+6/2=+3
-2(3)=-6
Cobalt (III) Chromate

23. Review of Ionic Compounds (Crystals)
Transfer of electrons
Made from a metal and a non-metal
Metals lose electrons, nonmetals gain electrons
Chemical formula is arranged in the smallest whole number ratio
Even though ionic compounds are made up of ions, they ARE ELECTRICALLY NEUTRAL!