1. Unit 2: Chemistry 4.2 Beautiful Bonding and Naming Compounds
Science 10
Unit 2: Chemistry
4.2 Beautiful Bonding and Naming Compounds

2. Objectives By the end of the lesson you should be able to:
Describe simple and complex ions
Describe the differences between covalent and ionic bonds
Name and make all types of ionic and covalent compounds

3. WARM UP! Counting Atoms Practice
Formula
# of Atoms
NaCl
Mg(OH)2
HNO3
(NH4)2O
H2SO4
NH4NO3 2 5 5 11 7 9

4. Complex and Simple Ions
Simple Ions: one atom with a charge
H S-2 Cu Cu+2
Complex Ions: more than one atom with an overall charge
Called polyatomic ions
SO4-2 NO NH4+1

5. Remember… ALL ELEMENTS WANT TO HAVE FULL OUTER SHELLS!
The combining capacity (ion charge) tells you how many electrons have to be lost/gained to get a full outer shell

6. Ionic Compounds Always involve a metal and a non-metal
Electrons are always transferred from the metal to the non-metal
Create ions because losing and gaining electrons (charges result)

7. Covalent Compounds Always involves 2 or more non-metals
Electrons are shared between the non-metals
Occurs in all diatomic molecules
DO NOT form ions!

8. Naming Ionic Compounds
Only 2 elements:
Metal always first; name never changes
Non-metal second; ending becomes “ide” (see page 186 and data booklet)
EX:
NaCl = sodium chloride
MgF2 = magnesium fluoride
Al2O3 = aluminum oxide

9. Making Ionic Compounds
Get symbol and charge
Charges are the same skip to step 2
If charges are different “swap and drop”
Combine
Examples On Whiteboard
Ex. Sodium chloride
Magnesium oxide
Aluminum fluoride
Magnesium nitride

10. Naming Multivalent Ionic Compounds
Multivalent = more than one combining capacity (ion charge)
Same naming as Ionic Compounds
BUT use a roman numeral to show which combining capacity is used
Mostly found in the Transition Metals section
I II III IV V VI VII VIII

11. Making Multivalent Ionic Compounds (Roman Numeral given)
Get appropriate ion (from Roman Numeral)
Charges are the same skip to step 2
If charges are different “swap and drop”
Combine
Reduce to lowest common ratio if needed.
Examples on whiteboard
Eg. Manganese (IV) sulfide
Cobalt (III) oxide
Cobalt (II) oxide

12. Naming Multivalent Ionic Compounds (no Roman Numeral given)
Write the options
Determine which pairing will give the correct formula
Write the name same as you did with Binary Ionic Compounds
Add the appropriate Roman Numeral between the metal and non-metal
Examples on whiteboard
Eg. Au3N FeO Fe2O3

13. Naming Polyatomic Ionic Compounds
Found in Data Booklet and page 192
Usually seen in more complicated compounds
Look up both names
Check for Roman Numerals
Combine
Endings NEVER change!
Examples on whiteboard
Eg. NH4CH3COO
(NH4)2SO4
FeSO3

14. Making Polyatomic Ionic Compounds
Get symbol and charge
If same skip to step 2
If different “swap and drop”
Combine – use brackets if need be for polyatomic ions ONLY
Eg. Manganese (III) chlorate Ammonium sulfate

15. Naming Covalent Compounds
Name first element
Name second element with “ide” ending
Add any needed prefixes

16. Prefixes IF first atom is 1 DO NOT add “mono” Change any “oo” to “o”
Prefix # Atoms
Mono Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca
Change any “oo” to “o”
I.E. monooxide = monoxide

17. Naming Covalent Compounds
Examples on whiteboard
Eg. CO
N2O3
CS2
CCl4
P4O10

18. Making Covalent Compounds
Write each symbol
Add any subscripts using prefixes
Examples on whiteboard
Eg. Nitrogen tribromide
dichlorine monoxide

19. Naming Covalent Compounds With Hydrogen
Memorize:
CH4 = methane
NH3 = ammonia
H2O = water

24. Naming Covalent Compounds With Hydrogen
HF = hydrogen fluoride
HCl = hydrogen chloride
HBr = hydrogen bromide
HI = hydrogen iodide
But when dissolved in water they become acids:
HF(aq) = hydrofluoric acid
HCl(aq) = hydrochloric acid
HBr(aq) = hydrobromic acid
HI(aq) = hydroiodic acid

25. Summary IONIC “ide” endings Multivalent = Roman numerals
Swap electrons
Metal + non metal
“ide” endings
Multivalent = Roman numerals
Polyatomics = brackets
COVALENT
Share electrons
Two non metals
“ide” endings
prefixes