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Unit 12 Notes: Chemical Reactions
Part 1: Balancing Equations
Chemical Reactions occur when ____________ between atoms are __________________ or _________________.
Indications that a chemical reaction has occurred:
Chemical Symbols:
Chemical Formulas:
Chemical Equations:
Chemical reactions begin with _____________________ and end with ________________________.
Symbols used in Equations:
Law of Conservation of Matter:
When a chemical reaction occurs, the amount of ____________________ must equal the amount of ________________________. If an equation does not have equal numbers of atoms on each side, it is not ________________.
To balance an equation, use __________________________ which are numbers in front of a symbol or formula. NEVER change the __________________!
Al (s) + O2 (g) ------( Al2O3 (s)
What is wrong with this equation?
Fix it with coefficients!
The final equation has 2 meanings:
Practice Balancing Equations:
1. H2(g) + O2(g) -( H2O(l)
2. C3H8(g) + O2 ( CO2(g) + H2O
3. B4H10(g) + O2(g) ( B2O3(g) + H2O(l)
4. sodium phosphate + iron (III) oxide ( sodium oxide + iron (III) phosphate
5. sodium chloride + silver nitrate ( sodium nitrate + silver chloride
6. Iron (III) hydroxide ( iron (III) oxide + water
7. radium phosphide + sodium ( sodium phosphide + radium
8. cesium + sulfur ( cesium sulfide
9. potassium metal + chlorine gas ( potassium chloride
_____________________________________are atoms that always occur in pairs and should be written as pairs in equations:
Unit 12 Part 2: Types of Reactions
5 types of Chemical Reactions:
1. Synthesis:
Practice predicting the products:
a. sodium metal reacts with chlorine gas
b. solid magnesium reacts with fluorine gas
2. Decomposition:
Practice predicting the products:
a. solid lead (IV) oxide decomposes:
b. aluminum nitride decomposes:
Decomposition exceptions:
________________________ and _________________________ do not decompose into single elements.
Carbonates decompose to _________________________ and a ________________ ________________.
Chlorates decompose to __________________________ and a _______________________ ________________.
3. Single Replacement Reactions:
Practice:
a. Zinc metal reacts with aqueous hydrochloric acid
b. Sodium chloride solid reacts with fluorine gas
4. Double Replacement Reactions:
Practice:
a. HCl(aq) + AgNO3(aq) (
b. CaCl2(aq) + Na3PO4(aq) (
c. Pb(NO3)2(aq) + BaCl2(aq) (
d. FeCl3(aq) + NaOH(aq) (
e. H2SO4(aq) + NaOH(aq) (
f. KOH(aq) + CuSO4(aq) (
5. Combustion Reactions:
Practice:
a. C5H12 + O2 (
b. C10H22 + O2 (
Mixed Practice: ID the type of reaction, predict the products, balance
a. BaCl2 + H2SO4 (
b. C6H12 + O2 (
c. Zn + CuSO4 (
d. Cs + Br2 (
e. FeCO3 (
Activity Series:
In single replacement reactions you have to use an _________________ ________________________ to determine if an element can replace another:
Li (More reactive)
Mg
Al
Zn
Cr
Fe
Pb
H
Cu
Hg (Less reactive)
Au
Elements can replace other elements that are __________ _________________. (top can replace bottom)
Example: Pb2O3 + Cu (
These substance won’t react with each other. The copper is not strong enough or “active” enough to replace the lead.
In addition to more active metals replacing less active metals, __________________ can also replace other __________________. (Most reactive at top…fluorine)
Practice:
a. FeO2 + Cr (
b. FeS + Hg (
c. ZnCl2 + H2 (
Energy Involved in Chemical Reactions:
Endothermic Reactions:
Exothermic Reactions:
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