1. Before Bell Rings Study for Ionic Naming Quiz

2. ETD#13 Give the formula for the following compounds:
Calcium Phosphate
Lithium Chlorate
Lead (II) Oxide
Name the following compounds:
FeO
Ca(OH)2
CuCl2

3. ETD#14 Give the formula for the following compounds:
Calcium Phosphate – Ca3(PO4)2
Lithium Chlorate – LiClO3
Lead (II) Oxide - PbO
Name the following compounds:
FeO – Iron (II) oxide
Ca(OH)2 – Calcium hydroxide
CuCl2 – Copper (II) Chloride
Remember we only use the roman numerals when the cation (usually a metal) has multiple charges. Ionic compounds are always neutral overall, so we need to have the correct number of each ion to make the total charge equal to zero.

4. Naming Ionic Compounds Quiz
Ion sheet and PT out, everything else away.

5. Learning Targets
I can determine the name/formula for a given molecular compound.

6. Ionic vs. Covalent -Between 2 non-metals - Sharing electrons
Ionic compounds have ionic bonds, meaning electrons have left from one atom and been taken in by another. The bond comes from the opposite charges of the ions. This is why the whole compound needs to be neutral, so that all the ions have the electrons they need.
Covalent bonds happen when two atoms share electrons instead of transferring them from one to the other. When two elements for a compound with a covalent bond, we call this a molecular or covalent compound.
-Between 2 non-metals
- Sharing electrons
Polar Covalent (unequal sharing)
Non-polar Covalent (equal sharing)
- Between metal & non-metal
- Transfer of electrons

7. Molecular/Covalent Bond NOTES
Formed by sharing electrons
Between two Non-Metals
Electronegativity Difference =
small
On the left is molecular, which means that it is sharing electrons and it is a bond between two non-metals

8. Carbon Dioxide How do you name this?
Naming for molecular compounds is all about adding prefixes to the start of the element. When I say “carbon dioxide”, I know there are two oxygen atoms in the compound because I see the prefix “di-” which means two. I also change the ending of the second element in the compound to –ide.
Carbon Dioxide

9. Rules for molecular bonds NOTES
Lower e-negativity atom first
1st Non-Metal normal
2nd Non-Metal ends in –IDE
Prefixes are used to show # of atoms
Mono – 1, Di – 2, Tri – 3, Tetra – 4, Penta - 5
Mono is NEVER used with the 1st Non-Metal,
Here are the rules for molecular naming.
The best way to identify a molecular compound is that it will be a compound formed from two non-metals.
Whichever nonmetal has a lower electronegativity goes first in the name or formula. This is why it is carbon dioxide and not dioxygen carbide, since carbon has a lower electronegativity than oxygen.
The ending of the second nonmetal is always changed to –ide.
The different prefixes (beginning part of the name) tell us how many of that atom there are. If the prefix is mono, it means there is one of that atom, like in carbon monoxide (CO). The prefix di- means there are two of that atom, like in carbon dioxide (CO2). Tri- means three, tetra- means four, and penta- means five.
The prefix mono- is never used as a prefix for the first nonmetal in the compound, but all of the others are.

10. Name or Give Formula: N2O3 Dinitrogen Trioxide PCl3
Phosphorus Trichloride
Sulfur Trioxide
SO3
Dinitrogen Tetrabromide
N2Br4
Al2S3 – Is aluminum sulfide. It is not Dialumnium Trisulfide. You do not use the prefixs because aluminum is a metal. You name just like you did at the beginning of the power point
Question: How do you name Al2S3?

11. Now try these! …Be Careful
Give the names
1)N2O5 2) AlBr3
3) Be3(PO4)2 4) Cl2O
Give the formulas
5) Magnesium Sulfate
6) Calcium Fluoride
7) Diphosphorus Pentafluoride
8) Lithium Nitrite
Dinitrogen Pentoxide
Aluminum Bromide
Beryllium Phosphate
Dichlorine monoxide
MgSO4
CaF2
P2F5
LiNO2

12. Acids: NOTES Always starts with a Hydrogen Two types
1) Does not contain oxygen
Hydro ______ ic Acid (Blank = name of anion)
HBr
Hydrobromic Acid
H2S
Hydrosulfuric Acid
When trying to identify what type of compound we are dealing with, the first element in the name or formula tells us a lot. If the compound starts with a metal or cation (other than H), it will be an ionic compound and follow the ionic naming rules. If the compound starts with a non-metal (right of the staircase on the PT), it will be a molecular compound and will follow the molecular naming rules. If the compound starts with a hydrogen (H), it will be an acid.
The acids we are learning will always be a combination of hydrogen and an anion. If the anion does not have an oxygen, the name is made by putting hydro- as a prefix and –ic as a suffix to the name of the anion. So if I was writing the name of an acid made with bromine, I add hydro– to the front of the bromine and change the ending to –ic, making hydrobromic acid. The same is true if I am making an acid with sulfur. I add hydro- to the front and change the ending to –ic, making hydrosulfuric acid. Remember this is only for acids without oxygen.

13. NOTES Example: H2SO4 ate  ic Sulfuric Acid Example: H2SO3
2) Does Contain Oxygen (has a polyatomic),
Don’t use hydro
Change the ending of the polyatomics
ate becomes ic
ite becomes ous
Example: H2SO4
ate  ic Sulfuric Acid
Example: H2SO3
ite  ous Sulfurous Acid
If the anion does have oxygen in it, we use different rules that depend on the ending of the anion. Acids with oxygen will have polyatomic anions, so we look at the ending of the anion to help us know the acid’s name.
If the anion ends in –ate, the acid it forms will end in –ic. So an acid formed from the sulfate ion (SO4 2-) will have its ending changed from –ate to –ic to make sulfuric acid.
If the anion ends in –ite, the acid it forms will end in –ous. So an acid formed from the sulfite ion (SO3 2-) will have its ending changed from –ite to –ous to make sulfurous acid.

14. I ATE big and got sICk, Take a bITE you little wOUS
H2SO4
ate  ic Sulfuric Acid
H2SO3
ite  ous Sulfurous Acid
Here is a mnemonic device to help you remember. ATE endings have more oxygens than ITE endings, so I ATE big and got sICk reminds us that ATE endings are for the ion with more oxygen atoms (big) and we change the ending to IC (sICk).
Take a bITE you little wOUS reminds us that ITE (bITE) endings are for the anion with less oxygen atoms (little) and we change the ending to ous (wOUS).

15. Writing the formula of an acid
Look at charges and use subscripts to make charges neutral
Hydronitric Acid
H+1 and N-3  H3N
Nitrous Acid
H+1 and NO2-1  HNO2
Nitric Acid
H+1 and NO3-1  HNO3
When writing the formulas for acids, the have to be neutral just like ionic compounds, but all of the positive charge comes from hydrogen. So if the anion has a 2- charge, the formula will start with H2, if the anion has a 3- charge, the formula will start with H3. A good check is to have a number of hydrogen atoms equal to the charge of the anion. + - Ø

16. With Acids Still: -Ic is Big -Ous is a wuss
Nitric Acid vs Nitrous Acid
HNo3
HNO2
Notice the endings for acids work the same as the traditional endings for metals that form ions with different charges. With traditional names for metals, the name that ended in –ic always hade the larger charge, just like the acid that has the larger number of oxygen atoms has the –ic ending. The same pattern is seen with the metals with the smaller charge ending in –ous and the acid with the smaller number of oxygen atoms ending in –ous.

17. Give name HCl Hydrochloric Acid HClO2 Chlorous Acid HClO3 Chloric Acid
Give formula
Phosphoric acid
Hydrophosphoric Acid
Hydrochloric Acid
Chlorous Acid
Chloric Acid
H3PO4
H3P
Make sure that you remember that the hydro has nothing to do with whether or not there is a hydrogen. All acids by definition have hydrogen. The hydro tells you whether or not the acid has an oxygen.

18. Try These: HNO3 H3N HNO2 Sulfurous Acid Sulfuric Acid
Hydrosulfuric Acid
Nitric Acid
Hydronitric Acid
Nitrous Acid
H2SO3
H2SO4
H2S

19. (NH4)3P LiCl Cu2S CaF2 SO3 NaClO3 N2O Ba(OH)2 H2SO3 Ferric Nitride
Diphosphorus tetrafluoride
Sodium Sulfate
Beryllium Phosphate
Magnesium Nitrate
Barium Iodide
Lithium Carbonate
Potassium Acetate
Hydrosulfuric Acid
Here is a mix of compounds to try. The answers are on the next slide.

20. (NH4)3P  Ammonium Phosphide
LiCl  Lithium Chloride
Cu2S  Copper (I) or Cuprous Sulfide
CaF2  Calcium Fluoride
SO3  Sulfur trioxide
NaClO3  Sodium Chlorate
N2O  Dinitrogen Monoxide
Ba(OH)2  Barium Hydroxide
H2SO3 Sulfurous Acid
Ferric Nitride  FeN
Diphosphorus tetrafluoride  P2F4
Sodium Sulfate  Na2SO4
Beryllium Phosphate  Be3(PO4)2
Magnesium Nitrate  Mg(NO3)2
Barium Iodide  BaI2
Lithium Carbonate  Li2CO3
Potassium Acetate  KC2H3O2
Hydrosulfuric Acid  H2S

21. Ide ATE BIG, with little bites
S = sulfIde
SO4-2 = SulfATE
SO3-2 = sulfite

22. Learning Targets
I can determine the name/formula for a given molecular compound.

23. Homework Naming Ionic Compounds WS (from test day)
Due next class
You should be able to do the Binary Molecular Compounds half of the naming WS you got last class.