1. Ionic Compounds PICK UP AN IONIC COMPOUNDS UNIT PACKET
Copy the Essential Question:
What elements form ionic compounds? How is an ionic bond formed?

2. What’s a chemical bond?
A chemical bond is the force that holds two atoms together
Two types of chemical bonds:
Ionic
Covalent

3. Why do atoms form bonds?
Formation of chemical bonds is due to number of valence electrons
Why do valence electrons play such an important role?
Because elements react to get the stable electron structure of a noble gas
How many electrons do atoms want to have in their outermost energy level? 8

4. The Octet Rule
States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons
Why? This is the stable electron configuration of the noble gases
How do we know if they will gain or lose electrons?
Atoms will do what is easiest to get the most stable electron configuration.
Atoms with 1, 2 or 3 valence electrons will
___________ electrons.
lose
Atoms with 5, 6 or 7 valence electrons will
___________ electrons.
gain

5. How do atoms form bonds? One way is by the formation of ions.
An ion is an atom (or a group of bonded atoms) with a positive or negative charge.
- Proton
- Neutron
- Electron
What would be the easiest way this sodium atom could get the perfect 8?
Sodium Atom
Sodium Ion

6. Positive or Negative Ion?
How can you tell if the ion formed will be positive or negative?
Count the protons and electrons
How many protons? ___
How many electrons? ___
What’s the charge? ___ 11
How many protons? ___
How many electrons? ___
What’s the charge? ___ 11 11 10 +1

7. Ions What type of atoms form positive ions?
Metals
What type of atoms form negative ions?
Nonmetals
Exceptions:
Lets take
a look…

8. Group Charges All alkali metals have a charge of _____.+1
All alkali metals have a charge of _____.
All alkaline earth metals have a charge of _____.
All halogens have a charge of ____.
Group 6A elements have a charge of ____. +2 -1 -2

9. Transition Elements
How many valence electrons do transition elements have?
Two (electron config: ns2)
They will commonly lose those two valence electrons to form ions with a +2 charge
But….they can also lose some of their d electrons to form ions of +3, +4 or greater
Some are consistent:
Ex: Ag+1, Zn+2

10. Roman Numerals System used to indicate numbers
II = 2
III = 3
IV = 4
We use Roman Numerals to indicate charge of transition metals
Copper (II) = Copper +2
Iron (III) = Iron +3

11. Names of Ions A positively charged ion is called a cation.
A cation’s name is the same as the element
A negatively charge ion is called an anion.
An anion’s name has the ending “–ide” added to the root name
Example: Anion of chlorine is the chloride ion.
1. What is the oxygen ion called?
oxide
2. What is the fluorine ion called?
fluoride
3. What is the bromine ion called?
bromide

12. Practice Questions Which type of atoms form cations?
Which type of atoms form anions?
Is Na+ a cation or anion?
Is F- a cation of anion?
Is Ca2+ a cation or anion?
Is Mg2+ a cation or anion?
What is the charge of the iodine ion?
What is the name of the iodine anion?
Would oxygen form a cation or anion?
What is the net charge of zinc (II)?
metals
nonmetals
cation
anion
cation
cation -1
iodide
anion 2+

13. Monatomic vs. Polyatomic
Mono means one
Poly means many
So, a monatomic ion refers to ions with single atoms
A polyatomic ion refers to ions with more than one atom

14. Monatomic Ions
Elements as they are on the periodic table form monatomic ions

15. Common Polyatomic Ions
Formed when more than one atom are grouped together
Charge on polyatomic ions applies to entire group of atoms.
The polyatomic ion acts as an individual ion and is protected with parenthesize in the formula!
Typically end in –ate or -ite
Common Polyatomic Ions
NH4+
Ammonium
NO3-
Nitrate
OH-
Hydroxide
CO32-
Carbonate
SO42-
Sulfate
PO43-
Phosphate
NO2-
Nitrite
Sulfate
Carbonate