1. Chemical Nomenclature
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2. Compounds
2 or more elements forming a chemical bond
Bond can be formed by combining positive metal ions and negative nonmetal ions (Ionic compound)
Bonds can form by combining 2 nonmetals sharing electrons (Covalent compound)
Helps all elements involved reach the octet
Subscript = tells how many elements are present in the chemical bond. Subscripts go behind and slightly below the element they describe C6H12O6 (6 Carbon, 12 Hydrogen 6 Oxygen)

3. Ionic Compound: Type I Binary
1 Metal + 1 nonmetal (Binary = 2) Two elements only = Binary
OVERALL NET CHARGE = 0
Metal from Family 1, 2, or Al, Zn, Cd, Ag, Ga, In
These metals always have the same charge (fixed charge)
Total + charge must equal and cancel total - charge. All charges cancel
Balanced formula NEVER shows the ion charges
Subscript tells how many of each ion are in the compound
To name: name of metal first, name of nonmetal ending in “ide”

4. Ionic Compound Type I Examples
Magnesium + bromide Silver + oxide
Mg Br Ag O-2
MgBr Ag2O
Magnesium Bromide Silver Oxide
Notice how all Type 1 Binary compounds have only 2 elements in them (2 capital letters) - one from the left (metal) and 1 from the right (nonmetal).
Notice the subscript is behind and below.
Notice how the compound no longer shows the charges because they have cancelled out.

5. Code for Type I Compounds Yellow + Red

6. Ionic Compound: Type II Binary
1 Metal + 1 nonmetal (Binary = 2)
Transition metals or members from Families 3, 4, or 5 that can be positive (never Al, Ga, or In)
These metals always change their charge (variable charge)
Roman numeral in the name tells the + (positive) charge (metal’s charge)
Remember: Total + charge must equal and cancel total - charge. All charges cancel
Subscript tells how many of each ion are in the compound
Name always ends in “ide”
TOTAL NET CHARGE = 0

7. Roman Numerals
I = 1 IV = 4 VII = 7 X = 10 II = 2 V = 5 VIII = 8 III = 3 VI = 6 IX = 9

8. Ionic Compound Type II Examples
Iron (III) fluoride Iron (II) fluoride Gold (III) sulfide
Fe F Fe F Au S-2
FeF FeF Au2S3
REMEMBER THE ROMAN NUMERAL TELLS THE CHARGE OF THE METAL!!!!
Follow criss cross rule
When trying to determine the compound name begin with nonmetal because its charge doesn’t change and uncross the subscripts
Look at only the metals that are shaded blue (have multiple charges) and the nonmetals (shaded red)

9. Practice – Write names and formulas
Fe2O3
CuCl
CuCl2
PbS
PbS2
Chromium (VI) oxide
Cobalt (III) sulfide
Nickel (II) bromide
Mercury (II) phosphide
Tin (II) iodide

10. Code for type II compounds Blue + Red

11. A dangerous solvent
DHMO

12. Dihydrogen monoxide - The Invisible Killer
Dihydrogen monoxide is colorless, odorless, tasteless, and kills uncounted thousands of people every year.

13. DHMO deaths
Most of these deaths are caused by accidental inhalation of DHMO, but the dangers of dihydrogen monoxide do not end there.
Prolonged exposure to its solid form causes severe tissue damage.
Symptoms of DHMO ingestion can include excessive sweating and urination, and possibly a bloated feeling, nausea, vomiting and body electrolyte imbalance.
For those who have become dependent, DHMO withdrawal means certain death.
May cause severe burns.

14. Dihydrogen monoxide
Also known as hydroxyl acid, and is the major component of acid rain.
Contributes to the "greenhouse effect."
Contributes to the erosion of our natural landscape.
Accelerates corrosion and rusting of many metals.
May cause electrical failures and decreased effectiveness of automobile brakes.
Has been found in excised tumors of terminal cancer patients.

15. Contamination
Quantities of dihydrogen monoxide have been found in almost every stream, lake, and reservoir in America today.
The pollution is global, and the contaminant has even been found in Antarctic ice.
DHMO has caused millions of dollars of property damage in the midwest, and recently in New Orleans.

16. No Government Cooperation
The American government has refused to ban the production, distribution, or use of this damaging chemical due to its "importance to the economic health of this nation."
In fact, the navy and other military organizations are conducting experiments with DHMO, and designing multi-billion dollar devices to control and utilize it during warfare situations. Hundreds of military research facilities receive tons of it through a highly sophisticated underground distribution network. Many store large quantities for later use.

17. Recognizing DHMO
Often chemicals go by different names, learn to identify the chemical components of each term in a chemical name.

18. Hydrogen is commonly known by it’s elemental name H
Di - Hydrogen
Di means two
Hydrogen is commonly known by it’s elemental name H

19. Mono – means one or single Oxide is commonly known as O or oxygen
Monoxide
Mono – means one or single
Oxide is commonly known as O or oxygen

20. Di-Hydrogen Mon-oxide
Two hydrogens and one oxygen together in one compound would have the chemical formula

21. H 2 O

22. Covalent Compounds: Type III Binary
Charges do not matter – NO IONS INVOLVED
The valence electrons are shared
Contain only 2 NONMETALS (right of the stair step) RED + RED
Hydrogen would be considered a nonmetal in these compounds
The name of the compound contains prefixes
Name ends in “IDE”
The compounds form COVALENT bonds (share electrons)

23. Prefixes
Mono = 1 (use this on the 2nd element only)
Di = 2
Tri = 3
Tetra = 4
Penta = 5
Hexa = 6
Hepta = 7
Octa = 8
Nona = 9
Deca = 10
Only type 3 compounds contain prefixes
Prefix is equal to the subscript of the element

24. Diphosphorus Pentoxide = P2O5 Sulfur Trioxide = SO3
Examples
Diphosphorus Pentoxide = P2O5
Sulfur Trioxide = SO3
Dichlorine tribromide = Cl2Br3
Tetraoxygen pentanitride = O4N5

25. Naming Conventions
Write the first elements subscript as a prefix (unless it is mono) then name the first elements
Write the second elements subscript as a prefix then change the ending to “IDE

26. AsBr4 = Arsenic tetrabromide P4S10 = Tetraphosphorus decasulfide
Examples
AsBr4 = Arsenic tetrabromide
P4S10 = Tetraphosphorus decasulfide
Cl2O = Dichlorine monoxide
H2O = Dihydrogen monoxide

27. Ionic Compounds: Type IV Ternary
Still must cancel total + charge with total – charge
Still must use subscripts to tell number of ions needed to balance
All contain a POLYATOMIC ion. All polyatomic ions have their own name, symbol, and charge
All polyatomic ions are found inside parentheses ( )
Cannot change what’s inside the ( )
Write a polyatomic ion’s subscript (if it needs one) outside its ( )
Shaded green on color coded periodic table
ZERO NET CHARGE

28. Examples of Polyatomic Ions
Hydroxide (OH)-1 - found in Drano
Bicarbonate (HCO3)-1 - makes the fizz in soda
Sulfate (SO4)-2 - found in car battery acid
Phosphate (PO4)-3 - found in soda as a preservative
Ammonium (NH4)+1 - found in household cleaners and fertilizers

29. Ionic Compounds: Type IV Ternary
Type IV compounds are half + ions and half – ions (just like types 1 and 2)
Type IV compound’s + half may be:
From family 1, 2, Zn, Al, Cd, Ag (you already know their charges)
One that uses a roman numeral (which is the + charge)
Ammonium (NH4)+, which is a polyatomic ion
Type IV compound’s – half may be from Families 7, 6, or 5 (you know their charges) or could be a negatively charged polyatomic ion

30. Polyatomic Ion Alternate Names/Formulae
Hydrogen Carbonate = Bicarbonate
Hydrogen Sulfate = Bisulfate
Hydrogen Sulfite = Bisulfite
Acetate: CH3COO- = C2H3O2-

31. Can be any color on the periodic table + green. Yellow + Green
Can be any color on the periodic table + green Yellow + Green Blue + Green Green + Red Green + Green

32. Name the positive ion as normal (1st)
Name the negative ion if polyatomic according to name in box (2nd)
Change the ending to “ide” if negative ion is from families 5, 6 or 7 (2nd)