1. NAMING COMPOUNDS

2. TYPES OF COMPOUNDS Molecular compound (covalent bonds)
Compound made of two nonmetals
NBr5
Ionic compound
Compound made of a metal and a nonmetal
NaCl
Acid (ionic bonds)
Compound that can donate a hydrogen ion
HCl

3. MOLECULAR COMPOUND (TWO NONMETALS)
To name a molecular compound, you have two parts:
The first element in the compound and
The second element in the compound
NBr5
The first element is called by its normal name: N – nitrogen
The second name is called by its name and ends in –ide: Br – bromine  bromide

4. PREFIXES
In addition to naming the elements, you have to name how many they are. To do this you need prefixes.
The prefix goes in the front of the name of the element

5. PREFIXES (CONT) One – mono Two – di Three – tri Four – tetra
Five - penta
Six – hexa
Seven – hepta
Eight – octa
Nine – nona
Ten - deca

6. MOLECULAR COMPOUND (CONT)
Therefore if you start with NBr5:
Mononitrogen pentabromide
BUT wait, if you only have one element in the beginning part of the compound, you don’t have to put the prefix:
Nitrogen pentabromide

7. TRY THESE SCl6 N2O4 P3F5 CCl4 XeO Trinitrogen hexaoxide
Boron pentabromide
Tetrasulfur decafluoride
Phosphorus octaiodide

8. N3O6 BBr5 S4F10 PI8 ANSWERS Sulfur hexachloride Dinitrogen tetraoxide
Triphosphorus pentafluoride
Carbon tetrachloride
Xenon monoxide
N3O6
BBr5
S4F10
PI8

9. SPECIAL CASE
When naming some compounds, it is implied that the compound is a DIATOMIC GAS
There are only 7 diatomic molecules
Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Iodine
Bromine

10. DIATOMIC MOLECULES
If you ever see any of those molecules, you write them as a compound with two of the atoms
Hydrogen – H2
Nitrogen – N2
Oxygen – O2
Fluorine – F2
Chlorine – Cl2
Iodine – I2
Bromine – Br2

11. IONIC COMPOUNDS (METAL AND NONMETAL)
The two parts of naming an ionic compound:
The first element is always the metal
The second element is the nonmetal
CaBr2
The first element is called by its normal name: Ca  Calcium
The second element is named like a molecular compound: Br  bromide
The only difference is that you do not use a prefix ever

12. IONIC COMPOUNDS Therefore if you start with CaBr2: Calcium Bromide
There is no prefix for bromide even though there is a 2

13. IONIC COMPOUNDS
Before we begin practice naming ionic compounds, look at your ion sheet
Remember: To put ionic compounds together, you need to BALANCE THE CHARGE

14. EXAMPLE
How would you show the following ionic compound: Strontium iodide
Strontium  Sr (has a +2 charge: alkali earth metal)
Iodide (has a -1 charge: halogen)
Just like before, cancel swap the charges
Sr+2 + 2I -  SrI2
Your ion sheet gives you the names of several ions with the many possible charges of the transition metals

15. BaCl2 K2O AlF3 CaO TRY THESE Magnesium oxide Potassium sulfide
Sodium chloride
Beryllium iodide

16. ANSWERS MgO K2S NaCl BeI2 Barium chloride Potassium oxide
Aluminum fluoride
Calcium oxide
MgO
K2S
NaCl
BeI2

17. POLYATOMIC IONS An ion that is composed of several atoms
FORMAL DEFINITION
Polyatomic ion: an electrically charged group of two or more chemically bonded atoms that function as a SINGLE ION

18. POLYATOMIC IONS
Since the polyatomic ions are made of more than 1 atom, their names are complicated
Example of some polyatomic ions:
OH -  hydroxide
ClO4 -  perchlorate
CO3-2  carbonate
NH4 +  ammonium

19. POLYATOMIC IONS
IMPORTANT NOTE: When combining polyatomic ions, you still balance out the NET CHARGE:
Example: If you have sodium hydroxide
Sodium: Na+
Hydroxide: OH –
Na+ + OH -  NaOH

20. POLYATOMIC ION
What do you do if you have more than 1 polyatomic ion to balance out a charge?
Example: If you have Magnesium acetate
Magnesium: Mg+2
Acetate: C2H3O2 –
Mg+2 + 2C2H3O2-  Mg(C2H3O2)2
You put the entire polyatomic ion in brackets with the number of ions as a subscript

21. TRY THESE K3BO3 Sr(NO2)2 Mg3(PO4)2 CaSO4 Lithium oxalate
Barium bromate
Sodium Phosphate
Aluminum sulfate
K3BO3
Sr(NO2)2
Mg3(PO4)2
CaSO4

22. ANSWERS Li2C2O4 Ba(BrO3)2 Na3PO4 Al2(SO4)3 Potassium borate
Strontium nitrite
Magnesium phosphate
Calcium sulfate

23. IONIC COMPOUNDS (TRANSITION METALS)
What do you do when you do not know the exact charge of the ion?
In other words, some of the transition metals can have more than 1 ion
Fe+2
Fe+3
You distinguish with Roman numerals

24. IONIC COMPOUNDS (TRANSITION METALS)
Solution: The name of the compound tells you the charge.
If you have a compound of iron and oxygen, an example would be:
Iron (III) oxide
This means that iron has a +3 charge
2Fe+3 + 3O-2  Fe2O3

25. IONIC COMPOUNDS (TRANSITION METALS)
This means that if you’re given the formula, you have to figure out the charge of the metal ion:
Example: MnO2
What you know: O has a -2 charge
Therefore the total negative is -4
This means that you need a +4 to balance
You get Manganese (IV) oxide

26. TRY THESE W(PO4)2 AuBO3 Tl3PO4 Sn(NO3)4 Nickel (III) iodate
Lead (II) chloride
Gold (I) Sulfate
Vanadium (III) chlorate
W(PO4)2
AuBO3
Tl3PO4
Sn(NO3)4

27. Ni(IO3)3 PbCl2 Au2SO4 V(ClO3)3 ANSWERS Tungsten (VI) phosphate
Gold (III) borate
Thallium (I) phosphate
Tin (IV) nitrite

28. ACIDS
What is an acid?
For now: An acid is a compound that will donate a proton (H+)
How do you recognize an acid
Any compound that begins with H+
There are two basic types of acids for naming
Binary acid
Polyatomic acid

29. BINARY ACID A binary acid has a hydrogen ion and a single halide
Examples: HCl, HF, HBr, HI
Naming these acids takes the following format:
Hydro-(root of the name of the halide)-ic acid
Therefore HCl becomes Hydrochloric acid

30. BINARY ACID
What would be the names of the following: HF
HBr HI

31. ANSWERS
Hydrofluoric acid
Hydrobromic acid
Hydroiodic acid

32. POLYATOMIC ACIDS Similar convention to binary acids
(Base name of the polyatomic ion)-ic acid
HC2H3O3
This is an H+ with a C2H3O3-
The name of the polyatomic ion is acetate
The name is Acetic acid

33. POLYATOMIC ACIDS The differences What if you have H2SO4 and H2SO3
What’s the difference in these two names?:
only one can be sulfuric acid

34. POLYATOMIC ACIDS If the ion ends in the name “-ate”
Sulfate, nitrate, chlorate
The name of the acid is (root of ion)-ic acid
Sufuric acid, nitric acid, chloric acid
If the ion ends in the name “-ite”
Sulfite, nitrite, chlorite
The name of the acid is (root of ion)-ous acid
Sulfurous acid, nitrous acid, chlorous acid

35. H2CO3 HNO2 HIO3 H3PO4 TRY THESE Oxalic acid Sulfurous acid
Sulfuric acid
Bromic acid

36. H2C2O4 H2SO3 H2SO4 HBrO3 ANSWERS Carbonic acid Nitrous acid Iodic acid
Phosphoric acid
H2C2O4
H2SO3
H2SO4
HBrO3

37. SUMMARY Before you start naming, determine the type of compound
Molecular, ionic or acid
Naming molecular compounds (nonmetal and nonmetal)
Name of the first element
Base name of the second element + ide
Make sure you use the prefix indicating number of atoms

38. SUMMARY (CONT) Naming ionic compounds (metal and nonmetal)
Name of the first element
Name of the second element + ide or
Name of the second polyatomic ion
Make sure you balance the charges of each ion
If the metal has more than 1 possible charge, indicate the charge with a Roman numeral

39. SUMMARY (CONT) Acids (the compound has a hydrogen ion H+)
Binary acids
Hydro (base name of the halogen)-ic acid
Polyatomic acids
(Base name of the polyatomic ion w/ “-ate”) – ic acid
(Base name of the polyatomic ion w/ “-ite”) – ous acid

40. WRITE THE SYMBOL OR NAME
Calcium chloride
Lead (IV) sulfate
Carbon tetrachloride
Hydroiodic acid
Sulfuric acid
Dinitrogen hexachloride
HBr
NH4NO3
S3Br8 NO
HNO2
Mn(C2H3O2)3
Pb(SO3)2

41. ANWERS CaCl2 Pb(SO4)2 CCl4 HI H2SO4 N2Cl6 Hydrobromic acid
Ammonium nitrate
Trisulfur octabromide
Nitrogen monoxide
Nitrous acid
Manganese (III) acetate
Lead (IV) sulfite

42. PUTTING THIS IN A CHEMICAL REACTION
General Format:
Reactants  Products
Steps
Translate the chemical into its symbol and then put the state of matter AFTER the chemical symbol
Put a “+” between each set of reactants and products

43. STATES OF MATTER Symbols for states of matter: Solid (s) Liquid (l)
Gas (g)
Aqueous (aq)

44. EXAMPLE
Solid sodium is mixed with chlorine gas to form aqueous sodium chloride
Solid sodium = ?
is mixed with = ?
chlorine gas = ?
to form = ?
aqueous sodium chloride = ?

45. Na(s) + Cl2(g)  NaCl(aq)
FINAL ANSWER
Na(s) + Cl2(g)  NaCl(aq)

46. TRY THESE
Solid iron is combined with oxygen gas to produce solid iron(III) oxide.
Aqueous magnesium nitrate is combined with solid zinc to form aqueous zinc nitrate and solid magnesium.

47. Mg(NO3)2(aq) + Zn(s)  Zn(NO3)2(aq) + Mg(s)
ANSWERS
Fe(s) +O2(g)  Fe2O3(s)
Mg(NO3)2(aq) + Zn(s)  Zn(NO3)2(aq) + Mg(s)