Larger atomic radius?
 Li or F?
 Whay?
Li has fewer protons=less
attraction between valence e- and
nucleus=bigger
-Name this ionic compound:
LiF

What’s the ionic charge on these ions?
◦Br -1
◦Se -2
◦N -3
+2
◦Ca
+1
◦K
“Oxidation #”= Charge!!!

What’s the oxidation # on these ions?
◦Br
-2
◦Se
-3
◦N
+2
◦Ca
+1
◦K
-1
1. Color in the valence e- for your element
(RED for METAL and BLUE for NON-METAL)
2. Find 5 other atoms (people) to bond with to
form a full octet
3. Write down the name and formula of your
compound
Cation Anion Formula Name
1
2
3
4
5
On the back of your handout…
Write the formula for these ionic compounds
 Potassium chloride KCl
 Calcium iodide CaI
2
 Magnesium nitride
Mg3N2
 Beryllium oxide BeO
 Aluminum sulfide Al2S3
 Potassium nitride K3N
 Aluminum chloride AlCl
3
Let’s check out Fe ….
What happens to Transition Metals?
Read p.208
4s2
3d6
Usually lose 2s valence, but can
also lose e- in d orbitals….so
Fe can be Fe2+ or Fe3+
Let’s check out V….
What happens to Transition Metals?
Read p.208
4s2
3d6
Usually lose 2s valence, but can
also lose e- in d orbitals….so
V2+, V3+, V4+, V5+ http://www.youtube.com/watch?v=sFAGQLok
ym4
Transition Metals
Fe can be Fe2+ or Fe3+ (write with
Roman numerals)
 Fe2+ is Iron (II)
 Fe3+ is Iron (III)
Why?!
Chemistry 11-10 Bellwork
Write the formula for the following ionic
compounds
 A) Sodium Chloride
 B) Magnesium Flouride
 C) Aluminum Nitride
 D) Beryllium Phosphide




Name the following Compounds
1) K2O
2) MgS
Let’s check out Fe ….
What happens to Transition Metals?
Read p.208
4s2
3d6
Usually lose 4s valence, but can
also lose e- in d orbitals….so
Fe can be Fe2+ or Fe3+
Transition Metals
What is the oxidation number for
 Zinc (III)
 Cu (II)
 V (IV)
 Ni (II)


Criss-Cross Iron (III) sulfide
Fe3+
S2-
=Fe2S3
Criss-cross it up! Write formulas…
(III) chloride FeCl3
 Zinc (II) oxide ZnO
 Silver (I) Nitride Ag3N
 Copper (II) chloride CuCl2
 Copper (I) chloride CuCl
 Nickel (II) bromide NiBr2
 Iron
‘Round the Room
Find an ionic compound in a
container around the lab
stations
2. Write out the formula for the
compound based on the name
1.
Physical Properties of Ionic Bondsp.214-215
•
•
•
•
Read this section
Fill out the Concept Map
“Concept” box = Ionic Bonds
Properties may include:
• conductivity, melting point,
hardness, strength of bond…
Ionic Bond Properties
High melting points which shows that the
______
Strong
ionic bonding is _______
Dissolves in water to separate the ions –
 _________
_________conductors
of electricity since ions
Good
move freely.
 ____
Very ______
Poor conductors of electricity in solid
form
 Demo…

Ionic Bonds

Monatomic - ______
______
One
Atom ______
Ion
◦ End in –ide (on front of your chart)

Polyatomic - _______
______
Many ______
Atom Ion
◦ On the back of your chart
2> elements, but acts like ONE ion!
 Write these on the BACK of your PT

-1
-2
-3
+1
Formula
(OH)(C2H3O2)(HCO3)(NO3)(SO4)2(CO3)2(PO4)3(NH4)+
Name
Hydroxide
Acetate
Bicarbonate
Nitrate
Sulfate
Carbonate
Phosphate
Ammonium
Give the Formulas for the following:
 Magnesium
 Iron
nitrate
(III) hydroxide
 Sodium
Carbonate
Find the formula using the criss-cross
method
Ammonium oxide
 Lithium phosphate
 Copper (II) carbonate
 Sodium bicarbonate (Sodium hydrogen
carbonate)
 Magnesium acetate
 Iron (III) sulfate
 Iron (III) sulfide
