1. Naming and Formula Writing

2. A Quick Review of Ions Cations Anions Transition Metal Ions
Polyatomic Ions (Table E)

3. Cations
Metallic elements tend to LOSE electrons and become positively charged
Group 1A: loses one electron  become +1
Group 2A: lose two electrons  become +2
Group 3A: lose three electrons  become +3

4. Anions Non-metals tend to gain electrons and become negatively charged
RULE: The charge of any ion of a Group A nonmetal is determined by subtracting 8 from the group number.
Example: Group 7A: charge
Group 6A: charge
Group 5A: charge

5. Transition Metal Ions
Many of the transition metals form more than one cation with different ionic charges
Ex. Fe2+ and Fe3+

6. Transition Metal Ions Stock System:
A roman numeral is used to indicate the positive oxidation state ONLY for an element that can have more than one possible state
Example: Fe2+ iron (II)
Fe3+ iron (III)

7. Polyatomic Ions (Table E)
Tightly bound atoms that behave as a unit and carry a charge
Ex: SO42- , HPO42-
The names of most polyatomic ions end in –ite or –ate

8. Types of Compounds Binary Compounds: Any combination of two elements
Ex: NaCl, H2O, SF6
Tertiary Compounds: Any combination of three different elements
Ex: KClO3, H3PO4, (NH4)2S
Quaternary Compounds: Any combination of four different elements
Ex: NaHCO3, (NH4)3PO4

9. Binary Compounds Binary Compounds can be either
Ionic: metal and non-metal
Ex) NaCl, FeO, BaF2
2) Covalent: non-metal and non-metal
Ex) SO2, PCl3

10. Binary Ionic Compounds
To identify an ionic compound, look for
a metal and a nonmetal
Metal = cation
Non-metal = anion
Examples: KCl, MgCl2, CaO, LiBr

11. Naming Binary Ionic Compounds
1) Name the cation first
When naming the cation, do not change the name of the metal
2) Name the anion second
When naming the anion, keep the root of the element name and change the ending to –ide
***No prefixes!!!
Ex) NaCl vs. CaCl2

12. Practice- Binary Ionic Compounds
(ex) BeCl3 beryllium chloride (ex) KF potassium fluoride (ex) MgO magnesium oxide (ex) Na2S sodium sulfide (ex) CaCl2 calcium chloride

13. Ionic Compounds with Polyatomic Ions
For polyatomics, DO NOT change the ending to –ide, keep what is on Table E. (ex) NaOH sodium hydroxide (ex) LiNO3 lithium nitrate (ex) KMnO4 potassium permanganate (ex) NH4Cl ammonium chloride (ex) NH4OH ammonium hydroxide

14. Ionic Compounds with Transition Metals
Use Roman Numerals ONLY if there is a metal with more than one ox # listed on the PT
ex) Cu2O vs. CuO
copper (I) oxide vs. copper (II) oxide
(ex) Fe2O3 vs. FeO
iron (III) oxide vs. iron (II) oxide

15. More Transition Metal Ion Practice
1) Cu2O copper (I) oxide 2) CrCl3 chromium (III) chloride 3) FeCl2 iron (II) chloride 4) CuSO4 copper (II) sulfate 5) MnBr3 manganese (III) bromide

16. Writing Formulas for Ionic Compounds
1) Determine the charges on the cation and anion
If there is a roman numeral in the name, it tells you the charge of the first element
Ex. iron (III) oxide 
Ending of –ate or –ite indicates a polyatomic ion  check charges on RT

17. Writing Formulas for Ionic Compounds
2) Use the cross-over method to determine the subscripts from the charges
Example: Lithium Sulfide Li2S
3) Reduce subscripts to the smallest whole numbers
Example: Magnesium Oxide  MgO
** Do not reduce the subscripts of polyatomic ions!

18. Formulas for Ionic Compounds with PAIs
Use parentheses around polyatomic ions ONLY if there is more than one
Examples:
ammonium chloride  NH4Cl
ammonium phosphate  (NH4)3PO4
magnesium nitrate  Mg(NO3)2
copper (II) phosphate  Cu3(PO4)2

19. Write the formula for:
Magnesium hydroxide  Mg(OH)2
Tin (II) nitrate  Sn(NO3)2
Nickel (II) acetate  Ni(C2H3O2)2
Sodium chromate  Na2CrO4
Aluminum permangate  Al(MnO4)3
Magnesium phosphate  Mg3(PO4)2
Mercury (II) carbonate  HgCO3
Copper (I) sulfate  Cu2SO4

20. How to Identify a Binary Covalent Compound
Non-metal to non-metal
Example: CO2, HF, CH4
The less electronegative element usually comes first

21. Naming a Binary Covalent Compound
Use the prefix system
Mono = one
Di = two
Tri = three
Tetra = four
Penta = five
Hexa = six
Hepta = seven
Octa = eight
Deca = ten

22. Naming Binary Covalent Compounds
Name first element. Only use a prefix if there is more than one.
Always use a prefix to tell how many of the second element there are and change the ending of the second element to –ide.
If the prefix ends in an “o” or an “a”, these letters are dropped for oxygen (ie. 1 oxygen is monoxide, NOT monooxide)

23. Practice
(ex1) NO nitrogen monoxide (ex2) N2O4 dinitrogen tetroxide (ex3) PF5 phosphorus pentafluoride (ex4) XeF4 xenon tetrafluoride (ex5) CCl4 carbon tetrafluoride

24. Writing the Formula of a Covalent Compound
Convert the prefixes from the name into subscripts in the formula
Example: dinitrogen pentoxide  N2O5
Do not write a subscript of “1”
Example: nitrogen monoxide  NO

25. Practice
(ex1) tetraiodine heptoxide I4O7 (ex2) sulfur trioxide SO3 (ex3) phosphorus pentafluoride PF5 (ex4) nitrogen trifluoride NF3 (ex5) disulfur dichloride S2Cl2

26. Naming Acids
Acids are a group of compounds that produce H+ ions (hydronium ions) when dissolved in water
Chemical formula of acids is generally HnX
n = number of hydrogen ions
X = anion

27. Naming Acids
If the acid is binary (contains hydrogen and one other element), start with the prefix hydro- followed by the root of the anion and the suffix –ic, and add the word acid.
hydro_______ic acid
Ex. HCl hydrochloric acid
HI hydroiodic acid
H2S hydrosulfuric acid

28. Naming Acids
2) If the acid contains a polyatomic ion, start with the root of the central atom in the polyatomic ion and add the appropriate suffix followed by the word acid. Suffix: ate  ic ite  ous
Ex. H2SO4
H2SO3
HNO3
HNO2

29. Writing Formulas for Acids
Use the rules for writing the names of acids in reverse to write the formulas for acids.
Be sure that the charges cancel!!!
Ex. hydrobromic acid HBr
Ex. Phosphoric acid H3PO4
Ex. hydroiodic acid HI
Ex. Hypochlorous acid HClO2
Ex. Sulfurous acid H2SO3
Ex. Carbonic acid H2CO3

30. Bases
A base is an ionic compound that produces OH- ions (hydroxide ions) in water
Use the rules for ionic compounds! (nothing new)
Ex) NaOH sodium hydroxide
Ca(OH)2 calcium hydroxide
LiOH lithium hydroxide
magnesium hydroxide Mg(OH)2
potassium hydroxide KOH

31. Summary An –ide ending generally indicates a binary compound
An –ite or –ate means a polyatomic ion that includes oxygen in its formula
Prefixes in a name indicate the compound is molecular
A Roman numeral after the name of a cation shows the ionic charge of the cation