1. Chemical Names and Formulas
SC2. Obtain, evaluate, and communicate information about the chemical and physical properties of matter resulting from the ability of atoms to form bonds.
e. Ask questions about chemical names to identify patterns in IUPAC nomenclature in order to predict chemical names for ionic (binary and ternary), acidic, and inorganic covalent compounds.
f. Develop and use bonding models to predict chemical formulas including ionic (binary and ternary), acidic, and inorganic covalent compounds.

2. Metals and Nonmetals Stairway of division on Periodic Table
B, Si, Ge, As, Sb, and Te are metalloids
Bi, Po, and At are disputed
Elements to the RIGHT are nonmetals
Elements to the LEFT are metals

3. Element or Compound? Elements include a single symbol
Compounds include MORE THAN ONE symbol
A formula is a representation of the atoms in a compound
KCr2O7

4. Ionic Compounds Composed of cations and anions
Formed from a metal (+) and non-metal (-), but can be all nonmetals*
the ions are electrostatically attracted (ionically bonded)

5. Molecular Compounds Composed of neutral atoms
the elements are usually nonmetals
the atoms share electrons (covalently bonded)

6. Naming Compounds
Your ability to name compounds and write formulas hinges on your ability to recognize whether a compound is ionic or molecular…
So let’s see if you can do it –

7. IONIC or MOLECULAR? Be and S? P and F? C and N? Cs and Ag? Fe and Cl?
Pb and I?

8. BASIC RULES for BINARY compounds
First element is written/named 1st
uses the full element name
C  carbon K  potassium
Second element is written/named 2nd
uses the root of the name and ends in –ide
chlorine  chloride oxygen  oxide

9. Here are all the prefixes…
1 – mono 6 – hexa
2 – di 7 – hepta
3 – tri 8 – octa
4 – tetra 9 – nona
5 – penta 10 – deca

10. Binary Molecular NAMING COMPOUNDS CCl4 N2O PF3 SiO2 H2O
Use PREFIXES to indicate the number of atoms of each element
Prefix is typically omitted on the first element if it is only one atom
CCl4
N2O
PF3
SiO2
H2O

11. Binary Molecular WRITING FORMULAS
Use the compound name to write the formula with the correct symbols and the appropriate subscripts
sulfur dioxide
silicon tetrafluoride
triphosphorus dioxide
nitrogen trihydride
dicarbon hexahydride

12. Ionic Charges Group 1  Group 2  Group 13  Group 14 
1+ (often just +) 2+ 3+
4+/-

13. Ionic Charges Group 15  Group 16  Group 17  Group 18  3- 2-
1- (often just -)
No ion forms

14. Transition Metal Ion Charges
Ag+ Cu+ and Cu2+ Zn2+ Hg2+ and Hg22+
Fe2+ and Fe3+ Co2+ and Co3+ Cr2+ and Cr3+ Mn2+ and Mn3+ Ni2+ and Ni3+

15. Transition Metal Ion Charges
Pb2+ and Pb4+ Sn2+ and Sn4+

16. Binary Ionic NAMING COMPOUNDS If the first element has only one charge
Use the standard naming rules
KBr
Ag3N
AlCl3
Zn2C
Mg3P2

17. Binary Ionic NAMING COMPOUNDS
If the first element has variable charges
Include a Roman numeral after the cation name to indicate which ion charge it has
FeCl3
CuO
Pb3N2
MnBr3
Sn2C

18. Na+ + Na+ + O2- = Na2O b/c 1+ + 1+ + 2- = 0
IMPORTANT!
When an ionic compound is formed, the sum of the ion charges must equal ZERO
Na+ + O2- ≠ NaO b/c = 1-
Na+ + Na+ + O2- = Na2O b/c = 0

19. Are you ready for the shortcut?
The criss-cross method allows you to easily back-determine ionic charges…
Al O2-
Al O 3 2

20. Let’s see if you’ve got it…
Li and Br 
Mg and Cl 
K and N 
Al and O 

21. Binary Ionic WRITING FORMULAS lithium fluoride strontium sulfide
If the first element has only one charge
lithium fluoride
strontium sulfide
barium nitride
beryllium bromide
aluminum oxide

22. Binary Ionic WRITING FORMULAS iron(III) nitride tin(IV) chloride
If the first element has variable charge
iron(III) nitride
tin(IV) chloride
nickel(III) sulfide
mercury(II) fluoride
copper(I) phosphide

23. Ternary Ionic Consist of more than 2 elements
Include at least one polyatomic ion

24. Polyatomic Ions
Consist of 2 or more nonmetals that, as a unit, have a charge
Most commonly anions
Exception is ammonium
Typically end with –ate or –ite
Exception is hydroxide

25. Polyatomic Ions
NH4+ ammonium OH- hydroxide MnO4- permanganate CO32- carbonate

26. Polyatomic Ions
NO3- nitrate NO2- nitrite SO42- sulfate SO32- sulfite PO43- phosphate PO33- phosphite

27. Polyatomic Ions ClO4- perchlorate ClO- hypochlorite
ClO3- chlorate ClO2- chlorite
ClO4- perchlorate ClO- hypochlorite

28. Polyatomic Ions
CrO42- chromate Cr2O72- dichromate

29. Ternary Ionic NAMING COMPOUNDS KMnO4 Li2CO3 FePO4 NH4OH Pb(NO2)2
Follow the standard rules, naming the cation and anion appropriately
KMnO4
Li2CO3
FePO4
NH4OH
Pb(NO2)2

30. Ternary Ionic WRITING FORMULAS calcium carbonate aluminum phosphite
Follow the standard rules, writing the cation and anion appropriately
calcium carbonate
aluminum phosphite
zinc dichromate
ammonium oxide
tin(II) hypochlorite

31. Acid Nomenclature Acids all have hydrogen as the cation
So they most often start with H
Naming and writing formulas for acids all depend on the anion format

32. Acid Nomenclature
If the anion ends with –ide, the name is hydro-(anion root)-ic acid
HCl  hydrochloric acid
H2S  hydrosulfuric acid
HBr  hydrobromic acid

33. Acid Nomenclature
If the anion ends with –ate, the name is (anion root)-ic acid
HNO3  nitric acid
H2CO3  carbonic acid
H3PO4  phosphoric acid

34. Acid Nomenclature
If the anion ends with –ite, the name is (anion root)-ous acid
HNO2 nitrous acid
H2SO3  sulfurous acid
HClO2  chlorous acid