1. How Can I Make Sense Out Of This? It’s Like Another Language!!
CuCl2
N2O5
Naming Compounds
How Can I Make Sense Out Of This?
It’s Like Another Language!!
This slideshow is intended for a high school chemistry class. The class would be comprised of mostly juniors, but would also include some sophomores and seniors.
Chromium (III) sulfate
Carbon tetrachloride

2. Background Octet Rule Ionic Compounds Covalent Compounds
Cation and Anion held together by electrostatic force
Cation (+)
Anion (-)
Also Called Salts
Covalent Compounds
Nonmetals sharing electrons

3. Charges of Commonly Formed Monatomic Ions+1 +2 +3 -3 -2 -1

4. Naming Ionic Compounds
Name the cation first and the anion second.
Typically left to right
Monatomic cations
Simply use the element name.
Group 1a & 2a metals have only one oxidation #.
Ex.
Na+  Sodium
Mg2+  Magnesium

5. Ionic Compounds Cont.
Transition metals and metals on the right side of the periodic table often have more than one oxidation #.
Use roman numerals after the element name to indicate the oxidation #
Ex.
Fe2+  iron (II)
Fe3+  iron (III)

6. Ionic Compounds Cont. Monatomic anions
Take their name from the root of the element name plus the suffix –ide.
Ex.
O2-  oxide
N3-  nitride
F-  fluoride
If the compound contains a polyatomic ion, simply name the ion.

7. You must know names and formulas for polyatomic ions!!!

8. Dealing With Polyatomic Ions
Most polyatomic anions, consist of a nonmetallic element combined with different numbers of oxygen atoms
These polyatomic anions are called oxyanions
The following suffixes are used with the root of element bound to the oxygens name
-ate
-ite
One less oxygen

9. Polyatomic Ions Cont.
When more than two oxyanions are formed by an element the following prefixes are used
Hypo-
One less oxygen than –ite
Per-
One more oxygen than -ate

10. Examples ClO3- ClO2- ClO- ClO4- Chlorate Chlorite Hypochlorite
perchlorate

11. Let’s Put it All Together
Na2S
Sodium sulfide
Pb(NO3)2
lead (II) nitrate
NH4F
Ammonium fluoride
Fe3(PO3)2
Iron (II) phosphite

12. Naming Binary Molecular Compounds
Prefixes are used to indicate the number of atoms of each type present in the compound.
Mono- is not used on the first element.
The first name in the formula is always named first
Use the element name from the periodic table.
The second element in the formula is named next
use the root of the element and add the suffix –ide.

13. Prefixes 1  mono- 2  di- 3  tri- 4  tetra- 5  penta- 6  hexa-
7  hepta-
8  octa-
9  nona-
10  deca-

14. Let’s Try It CCl4 N2O5 H2O Carbon tetrachloride Dinitrogen pentoxide
Dihydrogen monoxide
Aka  water
DHMO

15. Naming Acids Acids contain H 2 Types of Acids
H typically written 1st in formula
2 Types of Acids
Binary Acids
Oxyacids
Contain oxyanions

16. Naming Acids Cont. Binary Acids oxyacids Use the prefix hydro-
Use the root of the second part of the acid and add the ending –ic
End by adding the word acid
Do not write hydro-
Use the root of the oxyanion
If the oxyanion ends in –ate replace it with –ic.
If it ends in –ite replace it with –ous.
End by adding the word acid

17. Let’s See What We Can Do HCl H2CO3 H2SO4 HI HC2H3O2 HF HClO H3PO3
Hydrochloric acid
H2CO3
Carbonic acid
H2SO4
Sulfuric acid HI
Hydroiodic acid
HC2H3O2
Acetic acid HF
Hydrofluoric acid
HClO
Hypochlorous acid
H3PO3
Phosphorous acid