Ch. 8.4 to 8.5
Transcript of Ch. 8.4 to 8.5
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Types of reactions and reactivity
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1. Describe the trends found in the periodic table with respect to:
a) atom size
b) ionization energy
c) Electronegativity
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•In a composition reaction, also known as a synthesis reaction, two or more reactants combine to form a single product.
•This type of reaction is represented by the following general equation. A + X --> AX
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•Formation of binary compound from its elements2 Mg(s) + O2(g) --> 2 MgO(s)S8 (s) + 8 O2(g) --> 8 SO2(g)2 Na(s) + Cl2(g) --> 2 NaCl(s)
•Reactants can also be compounds.
CaO(s) + H2O(l) --> Ca(OH)2(s)
SO2(g) + H2O(l) --> H2SO3(aq)
CaO(s) + SO2(g) --> CaSO3(s)
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In a decomposition reaction, a single reactant undergoes a reaction that produces two or more simpler substances.
Decomposition reactions are the opposite of composition reactions.
They are represented by the following general equation.
AX --> A + XDecomposition reactions take place only when energy is added.
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a)Decomposition of Binary Compounds* compound breaks up into its elements
2 H2O (l) --> 2 H2 (g) + O2 (g)2 HgO (s) --> 2 Hg (l) + O2 (g)
b)Decomposition of Metal Carbonates* when heated, metal carbonates decompose into a
metal oxide and carbon dioxide
CuCO3 (s) --> CuO (s) + CO2 (g)
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c) Decomposition of Metal Chlorates* when heated, metal chlorates
decompose into a metal chloride and oxygen
2 KClO3 (s) --> 2 KCl (s) + 3O2 (g)
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*The equation represents an incomplete chemical reaction.
Al + Cl2 --> What is the product of the chemical reaction?
A.Al2Cl3
B.AlClC.AlCl2
D.AlCl3
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*The chemical equation represents the reaction between sodium (Na) and oxygen (O2).
4 Na + O2 --> What is the product of this reaction?
A.2 Na2OB.2 NaOC.2 NaO2
D.2 Na2O2
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•In a single replacement reaction, one element replaces a “similar” element in a compound.•Single replacement reactions can be represented by the following general equation: Element + Compound --> Element + CompoundA + BC --> B + AC •“Similar” = metals replace metals = nonmetals replace nonmetalsException: Hydrogen replaces metals and
metals can replace hydrogen
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•Activity series is a list of elements organized according to the ease with which the elements undergo certain chemical reactions. •For metals, greater activity means a greater ease of lose of electrons (forming cations).•For nonmetals, it means a greater ease of gaining electrons (making anions).•Use the provided list to determine if any given SDR will occur.
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Metals Name Symbol Lithium Li+ Sodium Na+
Potassium K+ Rubidium Rb+ Barium Ba+2 Strontium Sr+2
Calcium Ca+2
Decreasing activity
↓
reacts with water and acids
Magnesium Mg+2
Aluminum Al+3
Manganese Mn Zinc Zn+2
Chromium Cr+3 Iron Fe Cadmium Cd+2 Cobalt Co+2 Nickel Ni+2
Tin Sn Lead Pb
reacts with acids replacing hydrogen
Hydrogen H2
Antimony Sb Bismuth Bi Copper Cu Mercury Hg Silver Ag+1
Platinum Pt Gold Au
fairly unreactive
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•Examples:1. Cu(s) + AgNO3(aq) -->
2. Cl2(g) + NaBr(aq) -->
3. Mg(s) + HCl(aq) -->
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•In double-replacement reactions, the positive ions of two compounds exchange places to form two new compounds.•Double replacement reactions can be represented by the following general equation:
AX + BY --> AY + BX
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•Examples:1. KI (aq) + Pb(NO3)2 (aq) -->
2. Mg(C2H3O2)2 (aq) + Na3PO4 (aq) -->
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• In a combustion reaction, a substance combines with oxygen (O2), releasing a large amount of energy in the form of light and heat.
•Most combustion reactions involve the reaction of a carbon-based compound with oxygen. The products are carbon dioxide and water.
•They are represented by the following general equation.X + O2 --> CO2 + H2O
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•Examples:1. CH4 + O2 -->
2. C8H18 + O2 -->
3. C6H12O6 + O2 -->
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*You have one minute to answer these two questions concerning today’s lesson.
*What was the most important thing you learned?
*What is one question you would still like answered?