1. How Elements Form Compounds

2. This is how elements combine to form compounds.
In order for atoms to have a stable valence shell, they will link up with other atoms by stealing, giving up or sharing electrons.
This is how elements combine to form compounds.
Top: limestone. Bottom left: calcium chloride (road salt) Bottom right: copper II sulfate: ALL EXAMPLES OF IONIC COMPOUNDS

3. There are two major types of compounds that can form between atoms:
1. Ionic compounds: where metals (+) bonds with non-metals (-) *stealing
2. Molecular (Covalent) compounds: where non-metals bond with other non-metals *sharing
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4. Ionic Compounds – made up of positive and negative ions that results in the transfer of electrons from metal to non-metal.
Ex: Sodium + Chlorine
Sodium will “share” it’s one extra electron with chlorine (who is missing one)
The positive and negative charge are attracted to each other because they have opposite charges.

5. Here we see that Na (metal) will give it’s valence electron to Cl (non-metal) so that they both have stable shells!
Once this happens, the ionic charge of Na will be 1+ and the ionic charge of Cl will be 1-.
These two opposing charges will attract each other and a chemical bond will be formed creating the ionic compound  sodium chloride (NaCl)

6. Sometimes, more than one electron can be transferred!
Ex: Calcium + oxygen
Calcium has two extra electrons that it will share with oxygen. Ca+2 O-2
This compound’s name is

7. Sometimes, more than one atom of each element will have to be involved.
Ex: calcium + chlorine
This compound’s name is

8. Naming Compounds Ionic Compounds
Write the name of the first element as it appears on the periodic table
Change the ending of the second element to “-ide”
Example: NaCl
Sodium Chloride

9. Naming Ionic Compounds
Name the following Ionic Compounds:
LiF
Be3N2
MgCl CaO
AlF K2S
ZnBr CaBr2

10. Naming Ionic Compounds
Name the following Ionic Compounds:
Lithium flouride beryllium nitride
Magnesium chloride calcium oxide
Aluminum floride potassium sulfide
Zinc bromide calcium bromide
LiF
Be3N2
MgCl CaO
AlF K2S
ZnBr CaBr2

11. Naming when you have metals with more than one Charge
Some metals make more than one ionic charge. Most of these are found in the transition metals on the PT
If you use a metal that can make more than one ionic charge, you must use a roman numeral following the metal’s name to indicate which ion charge was used.
The name of the non-metal still ends in “-ide”.
NOTE: The little number in the formulas is NOT it’s charge! It represents HOW MANY of the ions are used in the formula.

12. Build the following molecules with your ion fit kit and then give them a name in your notes.
CuBr
FeO
CuBr2
Fe2O3
NiI3
Sn3N2
NiI2
Sn3N4

13. Build the following molecules with your ion fit kit and then give them a name in your notes.
CuBr
Copper (I) bromide Iron (II) oxide
Copper (II) bromide Iron (III)oxide
Nickel (III) iodide Tin (II) nitride
Nickel (II) iodide tin (IV) nitride
FeO
CuBr2
Fe2O3
NiI3
Sn3N2
NiI2
Sn3N4

14. What pattern appears between the charges of the ions and how many of each ion there are in the formula?
The charge of the metal is how many non-metals you need in the formaula and vice versa… most of the time.
This is called the criss cross method

15. Naming with Polyatomic Ions:
A polyatomic ion is a group of atoms that together hold an overall ionic charge
If a polyatomic ion is in a formula, just state its name as written. You do NOT change it’s ending.

16. Build the following molecules with your ion fit kit and then give them a name in your notes.
Na2SO4
NH4Cl
Al(OH)3
Fe(NO3)3
Zn(BrO3)2
(NH4)3PO4

17. Build the following molecules with your ion fit kit and then give them a name in your notes.
Na2SO4
NH4Cl
Sodium sulphate aluminum chloride
Aluminum hydroxide iron (III) nitrate
Zinc bromate ‘ ammonium phosphate
Al(OH)3
Fe(NO3)3
Zn(BrO3)2
(NH4)3PO4