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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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