unit vi: chemical reactions i.5. types of chemical reactions
TRANSCRIPT
Unit VI: CHEMICAL REACTIONS
I.5. Types Of Chemical Reactions
Types of Reactions
1. Synthesis2. Decomposition3. Single Replacement4. Double Replacement
Neutralization (Water Forming)
5. Combustion1. Combustion of hydrocarbons2. Combustion of metals
Synthesis
Two or more substances combine to form a compound
A + B → AB
Synthesis
Synthesis
Often: elements a compound
2Al + 3F2 2AlF3
Synthesis
Examples 2H2 + O2 → 2H2O
2Mg + O2 → 2MgO
CaO + CO2 → CaCO3
Synthesis
potassium + oxygen
calcium + phosphorous
Synthesis
A special type of synthesis
CoCl2 + 6H2O CoCl2● 6H2O
Synthesis
A compound + an element a “bigger” compound
2SO2 + O2 2SO3
Synthesis - Overview
Always more more than 1 reactantthan 1 reactant
Usually forms only 1 productonly 1 product
Decomposition
One substance breaks down into more than one substance
AB → A + B
Decomposition
Decomposition
EXAMPLES: 2HgO → 2Hg + O2
2H2O → 2H2 + O2
MgCl2→ Mg + Cl2
Decomposition
Note: Unless otherwise told, break all compounds COMPLETELY down to its elements. (Even break up PAIs)
Decomposition
Note: Unless otherwise told, break all compounds COMPLETELY down to its elements. (Even break up PAIs)
Decomposition
Note: Unless otherwise told, break all compounds COMPLETELY down to its elements. (Even break up PAIs)
Decomposition
A special type of decomposition
CuSO4● 5H2O CuSO4 + 6H2O
Decomposition
AlsoA Bigger Compound Smaller Compound + An Element
2KClO3 2KCl + 3O2
Single Replacement
One substance replaces another in a compound Metals replace metals Non-metals replace non-metals
AB + C → A + BC
Single Replacement
Single Replacement
Two Types1. Metal Single Replacement
2. Non-metal Single Replacement
Single Replacement
Examples of Metal SR
Zn + CuSO4 → Cu + ZnSO4
Fe + 3AgNO3 → 3Ag + Fe(NO3)3
Single Replacement
Metal SRs
Single Replacement
Metal SRs
Single Replacement
Some Non-Metal SRs
Single Replacement
Some Non-Metal SRs
Single Replacement
The catch some elements are not strong enough to replace others
Plan:1. Predict Products2. Fix Formulas3. Balance Equation4. Determine from Activity Series if
Reaction will Proceed
Double Replacement
Both compounds change partners
Again refer to the activity series to see if reaction will proceed
AB + CD → AD + BC
Double Replacement
Double Replacement
Refer to the activity series to determine the relative reactivity of elements. For example, calcium is more reactive than hydrogen; therefore, calcium can replace hydrogen in a reaction.
Ca(s) + 2 HOH(l) Ca(OH)2(s) + H2(g)
Double Replacement
Examples: 2KI(aq) + Pb(NO3)2(aq) → 2KNO3(aq) + PbI(s)
AgNO3 + KCl → AgCl(s) + KNO3
Double Replacement
Double Replacement
Double Replacement
Neutralization
Sub-type of Double Replacement Reaction
Sometimes called water forming
ACID + BASE → WATER + SALT
Neutralization
Neutralization
Combustion (aka Burning Stuff)
Substance reacts with oxygen (fast enough to produce heat and light)
Two Types of Combustion1. Combustion of hydrocarbons
2. Combustion of metals
Combustion
Hydrocarbons NOTE: O2 is ALWAYS A REACTANTALWAYS A REACTANT! When burning hydrocarbons ASSUMEASSUME
the products are
CO2 + H2O
Combustion
CxHy + O2 → CO2 + H2O
Combustion
Combustion
Combustion
Combustion of Metals = Synthesis
Combustion
Combustion of Metals = Synthesis
Combustion
Combustion of Metals = Synthesis
Assignments
Do Problem Set #3 and #4 on page in your Student Workbook
Do Exercises 65 (a, c, e), 66 (b, d, f, h, j, l, n, p, r, t, v, x), 67 (a, c, e, h, j, l, n, p, r) on page 118 [Hebden]
Do Hand-In Assignment # 8
Lab
Do Experiment 5C – page 71-73[Heath] This experiment will take most of the
class your pre-lab must be complete beforebefore the lab begins
Fill in the Blank Lab Format you are only responsible for the questions asked in the lab handout