1. Warm Up1 : Write from memory the definitions of: Valence e- Cation
Anion
Octet Rule
Isotope

2. THOSE LOOK FAMILIAR… Law of Definite Proportions
Ratio of atoms in a cmpd equates to the ratio of masses of each element (masses of elements are always in same proportions)
Law of Multiple Proportions = Dalton!
Multiple proportions are possible of the same 2 elements (water 2:1 and peroxide 2:2)

3. Nomenclature (naming compounds and writing formulas)
In Chemistry there are:
Symbols (for elements ; we call them atoms)
ex. Na or Cl
Formulas (for compounds; we call them molecules or formula units)
Ex. NaCl or CO2
Equations (for reactions)
Ex. 2Na(l) + Cl2(g) → 2NaCl(s)

4. There are two types of compounds:
Ionic (start with a metal or a positive polyatomic ion); M&NM
Called formula units
Have high melting points (why? Ions)
Are electrolytic in their molten or aqueous state
Are solid at room temperature
Have a crystalline structure (think salt…)
Usually soluble in water
Covalent (start with a nonmetal); NM & NM
Called molecules
Low melting points (think butter…)
Volatile
Non-electrolytic

5. Tells us if a molecular or ionic cmpd… definitions?
Compound Formulas
Ex. SO3
Tells us:
types of element in the compound
How many atoms of each
The way the compound is bonded and therefore its properties
Tells us if a molecular or ionic cmpd… definitions?

6. Which of the following compounds are:
electrolytic?
Which are volatile?
Probably soluble?
Na2S SCl Al2O3 KF F OF2

7. Pull out Polyatomic Ions Sheet
Start to memorize these!
Always use parentheses, please!

8. Writing compound formulas:
Ionic:
Covalent:
get the symbol and the charge of the ions
Make subscripts out of prefixes from the name
From periodic table
Mono-1
Monatomic ions table
Di-2
(pg 192)
Tri-3
Or polyatomic ion sheet
Tetra-4
Criss-cross charges (making the atom electrically neutral)
Penta – 5
Hexa-6
Hepta-7
Octa - 8

9. How to get charges from the periodic table:
All atoms want to have 8 valence e- = very stable!
Count to the nearest noble gas (skip T-metals)
Does the atom have to gain or lose e- to get to that noble gas?

10. Tin = Sn 2+ or 4+
Cobalt = Co 2+ or 3+

11. Transition Metals – variability in charges (Cu, Fe, Hg, Pb, Sn, Cr, Mn, Co)
Stock System
Roman numerals after name (tells you charge!)
Classical System
Root word, “ous” (cation smaller of the two possible ionic charges) or “ic” (cation larger of the two possible)… unsure of charge though

12. Practice just ionic cmpd names

13. Practice just with molecular cmpds

14. Flow Chart
Contains prefixes … molecular cmpd… use prefixes to write formula!
No prefixes … ionic cmpd… use criss cross to write formula!

15. sulfur trioxide Iron (III) carbonate barium bromide tin (II) fluoride
BI/ BM/ T
Formula
sulfur trioxide
Iron (III) carbonate
barium bromide
tin (II) fluoride
magnesium oxide

16. sulfur hexafluoride Aluminum acetate diphosphorus sulfide
BI/ BM/ T
Formula
sulfur hexafluoride
Aluminum acetate
diphosphorus sulfide
potassium nitrite
ammonium chloride

17. silicon tetrachloride
BI/ BM/ T
Formula
chlorine monoxide
silicon tetrachloride
chlorine trifluoride
beryllium oxide
magnesium fluoride

18. Diatomic molecules - Halogens

19. Make polyatomic ion flash cards
“-ate” = 1 more O… ate another O
“-ite” = 1 less O
“hypo-” = 2 less O
“-ium” = ammonium, hydronium
“-ide ion” = hydroxide ion, cyanide ion

20. Practice on your own!

21. WU 2:
Study for Ionic vs Covalent Quiz

22. Quiz

23. Enrichment /Intervention:
Pick up a test and review the questions that you missed. Also, put your vocab on your desk!
Especially:
AR, EN, IE, EA
Calculate the atomic mass of the isotopes listed in the free response problem (NOT A BASIC AVERAGE!)
If you performed highly on this test, the complete the puzzle in the back of the room 

24. Naming Compounds Ionic: Name the ions Polyatomic ions
do not change name
Monatomic cations
Do not change name
Ex. Mg = magnesium
Mg 2+ = magnesium
Of transition metals
Include the charge of the ion in parentheses (you will have to calculate the charge
Ex. SnCl2 tin(II)

25. Ionic cont… Monatomic anions
Drop the last syllable (or two) and add the suffix ide
Ex. Cl = chlorine Cl- = chloride
F = fluorine F- = fluoride

26. Covalent:
Add prefixes to names of elements to indicate the number of atoms present. End the second element in – ide.
If there is only 1 atom of the first element, do not put a prefix
Mono-1
Di-2
Tri-3
Tetra-4
Penta – 5
Hexa-6
Hepta- 7
Octa – 8
Ex. ClO N3F2

27. Who am I? Ca(NO3)2 ALWAYS PUT PARENTHESES ON POLYATOMIC IONS!
H+ + CO32-  H2CO3

28. Acid Nomenclature Rules pg 272

29. Acid Nomenclature
Acids are compound that have an “acidic hydrogen” ion (H in front)
Naming acids:
Binary Acids (HNm)
To name use form:
Hydro__________ic acid
Ternary acids (HXO)
No hydro
If polyatomic ion ends in ate, drop –ate and add –ic acid
If poyatomic ion ends in –ite, drop –ite and add -ous acid

30. Examples: HCl H2S HClO2 HNO3 HCN H2CO3 You Try: HF H3N HNO2 H2Cr2O7 H2C2O4

31. Writing formulas for acids-
Treat like it is ionic
If it starts with hydro it is bonded to a NM from the PToE
If no hydro- bonded to a polyatomic ion
Ex.
Chromic acid
Acetic acid
Perchloric acid

32. You try: Hydrophosphoric acid Phosporic acid Hypochlorous acid Sulfurous acid Sulfuric acid Hydrosulfuric acid