1. Matter Elements Compounds
A single pure substance that can not be broken down (decomposed)
Ie: Periodic table of elements
***
Diatomic Elements
Br2I2N2Cl2H2O2F2
Compounds
2 or more elements combined in a fixed definite ratio.
Can be decomposed
H2O CO2

2. Mixtures: Varied Ratio
Matter
Mixtures: Varied Ratio
HOMOGENEOUS
True Solutions (aq)
See only 1 part
NaCl (aq)
Separated by evaporation and Distillation
Boiling points
HETEROGENEOUS
See multiple parts
Sand and water
Chocolate chip ice cream
Separated by filtration

3. 3 C6H12O6 3 – coefficient, how many glucose
Formula Writing
Formulas show both:
Quantitative – how much, how many atoms
Qualitative – what types of elements present
3 C6H12O – coefficient, how many glucose
(3 moles)
This tells you:
Quantitative(subscripts) – 6 Carbon, 12 Hydrogen
and 6 Oxygen are present
Qualitative – Made up of Carbon, Hydrogen and Oxygen

4. . Types of Formulas Empirical – simplest whole number ratio CH2O
Molecular (true formula)
C6H12O6
Condensed CH3CH2CH3
Structural
Hydrates
CuSO H2O .

5. Formula Writing
1. Sum of all oxidation numbers of any formula must = 0
2. work only with the metals, non-metals and
polyatomic ions (table E)
CrissCross Method
K+ Cl- Mg+2 S-2 Al+3 Cl Mg Br -
KCl MgS AlCl3 MgBr2

6. Formula Writing
1. Sum of all oxidation numbers of any formula must = 0
2. work only with the metals, non-metals and
polyatomic ions (table E)
CrissCross Method
K+ ClO4- Mg+2 PO4-3 Al+3 NO Mg Mn04-
KClO4 Mg3(PO4) Al(NO2)3 Mg(MnO4)2
*****Note the parenthesis around the polyatomic ions

7. Zone 1
Zone 3
Zone 2
M-NM = Ionic Nm-Nm = covalent (molecular compounds)

8. Binary Compounds - ide
Zone 1-3
Zone 3-3
Zone 2-3
Grp 1,2 M – NM Trans M – NM Molecular compounds (Covalent NM – NM)
“Call it like you see it” “Call it like you see it” Use Prefix on 2nd NM
Roman Numerals to indicate Use on first if more than NM
NaCl FeCl FeCl mono, 2- di, 3-tri,
Name Metal – Sodium Name Metal with ox # – Tetra, 5- penta, 6 hexa
Name the Non Metal Iron II Chloride Iron III Chloride
(Chlorine) drop end
add - ide CO Carbon Monoxide
Sodium Chloride CO2 Carbon Dioxide
N2O5 Dinitrogen Pentoxide
KF MgCl CaO CuCl CuCl2

9. Zone 1
Zone 4
Zone 2
Zone 3

10. Ternary Compounds Zone 1-3 Zone 2-3 Zone 3-4 Zone 3-3 Group 1,2 M–PI-nm
Na2SO4
Sodium Sulfate
Al2(SO4)3
Aluminum Sulfate
PI + - PI -
m nm
(call it like you say it)
(NH4)2SO4
Ammonium Sulfate
NH4NO3
Ammonium Nitrate
Transition M –PI- nm
(Roman Numerals)
Cu2SO4
Copper (I) Sulfate
CuSO4
Copper (II) sulfate
PI+ - NM m
(name it like a binary
–ide)
NH4Cl
Ammonium chloride

11. Naming Acids Binary vs Ternary
(formula always begin with H)
H – polyatomic ion
(end in ate or ite)
H – ate H- ite
Remember, you ate it and it was icky!
(ate-ic) (ite-ous)
H2SO4 HNO2
Sulfuric Acid Nitrous Acid
HCl
Always start with “Hydro”
Name the non-metal
Chlorine
Change ending to
- ic acid
Name = Hydrochloric Acid

12. HNO3
HCl
H2SO4
HC2H3O2
HBr
HNO2
H2PO4
Sulfuric Acid
Nitric Acid
Hydrochloric Acid

14. Types of Equations Synthesis ( 2 to 1) A + B AB Decomposition
Fermentation (Organic)
Always produces Alcohol and CO2
(C2H5OH + CO2)
C6H12O6  C2H5OH + CO2
Combustion (Organic)
(Always produces CO2 and H2O
Burn reaction – need O2
C3H8 + O2  CO2 + H2O

15. Types of Equations
Single Replacement ( element-compound element compound) Red is the Metal A + BC  AC + B ***Remember Table J Activity Series Who is the Bully? Ca + HCl  CaCl2 + H2 (g) works. Cu + HCl  N.R. Why? AG + MgCl2  Reaction….yes or no?

16. Types of Equations
Double Replacement ( compound-compound compound - compound) Red is the Metal A B + C D  AD + CB HCl + NaOH  NaCl + HOH NaCl + HOH  NaOH + HCl MgCl2 + (NH4)2SO4 

17. A Reaction will go to completion when:
A gas (g) is produced
Water is a product
One of the products is insoluble (does not dissolve)
Table F solubility Guidelines

18. Solubility Guidelines for Aqueous solutions
Table F
Solubility Guidelines for Aqueous solutions

19. Try these out! Zn + HCl  ZnCl2 + H2 NaClO3  NaCl + O2
What type of reactions do we see?
Zn + HCl  ZnCl2 + H2
NaClO3  NaCl + O2
P4 + Cl2  PCl3
HCl + Mg(OH)2  MgCl2 + H(OH)
BaO + SO3  BaSO4
Pb + AgNO3  Ag + Pb(NO3)2
AgNO3 + Na2CrO4  Ag2CrO4 + NaNO3

20. 2Ca0 + O20  2Ca+2O-2 Balancing Equations
**An equation must show conservation of both Mass and Charge and Energy!!!!!!
2Ca0 + O20  2Ca+2O-2
Steps to follow:
1. Write the correct formula first, if needed
2. Pick a start point and let it take you to the next……
3. If you see water, change the formula from H2O to H(OH)
4. Always work the polyatomic ions (SO4, NO3etc.) as a whole
5. Try not to deal with any odd # coefficients.
a. if present, double their value to make it even

21. PRACTICE
___HgO  ___Hg + ___O2
___ Li + ___Br2  ___ LiBr
___Al + ___Cl3  ___AlCl3
___Al2O3  ___Al + ___O2
___Ca3(PO4)2 + ___H2SO4  ___Ca(SO4) + ___ H3PO4
(Combustion Reactions: Always do in this order- C,H,O)
____C3H8 + ___O2  ___CO2 + ____H2O

22. NaCl + F2  NaF + Cl2
AgNO3 + MgCl2  AgCl + Mg(NO3)2
FeCl3 + NaOH  Fe(OH)3 + NaCl
AlBr3 + K2SO4  KBr + Al2SO4
CH4 + O2  CO2 + H2O
Na + H2O  NaOH + H2
C3H6 + O2  CO2 + H2O