5 types of chemical reactions
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Transcript of 5 types of chemical reactions
• Synthesis Reaction
• Combination reaction is
the direct union or
combination of two
substances to form a
single compound.
A +B AB
General Formula:
Xander Agnes
A COMBINATION REACTION MAY ALSO INVOLVES AN ELEMENT AND A COMPOUND, OR TWO SIMPLE COMPOUNDS:
2 SO2 + O2 SO3
MgO + H2O Mg(OH)2
2 Ni O+ O22 Ni
1. Nickel reacts with oxygen to form Nickel Oxide
2. Silver reacts with chlorine to form Silver Chloride.
2 Ag + Cl2 2 Ag Cl
3. Oxygen gas reacts to magnesium form magnesium oxide
O2 + 2 Mg 2 MgO
TRY THIS:
1. H2(g) + Cl2(g)
2. Fe2(s) + S(s)
2 HCl(aq)
FeS(s)
• Analysis Reaction
• Decomposition reaction is a
single substance broken into
two or more different
substances.
BAB A +
General Formula:
Xander Agnes
1. THERMAL DECOMPOSITION REACTION- decomposition reaction caused by a rise
in temperature.
2 HgO(S) 2 Hg(g) + O2(g)
CaCO3(s) CaO(s) + CO2(g)
2. ELECTROLYTIC DECOMPOSITION REACTION- decomposition reaction caused by electricity.
Ionic compounds can be decomposed in this manner, either in molten state or in solution.
2 NaCl(l) 2 Na(l) + Cl2(g)
PbBr2(aq) Pb (s) + Br2(aq)
electrolysis
electrolysis
3. PHOTOCHEMICAL DECOMPOSITION REACTION- decomposition reaction caused by light.
2 AgCl2(s) Ag(s) + Cl2(g)
2 AgBr (s) 2 Ag(s) + Br2(g)
light
light
4. Catalysts cannot cause chemicals to decompose, they can speed up the rate of chemical decomposition.
2 H2O2(l) 2 H2O(l) + O2(g)
manganese dioxide
catalyst
2 Au2O3
2 KClO3
TRY THIS:
4 Au + 3 O2
2 KCl + 3 O2
- An atom or a group of atom that replaces part of a compound.
Types of Replacement
Reaction: Single Replacement
Double Replacement
Substitution
Reaction
In this type of chemical
reaction, an element and
a compound react and
form a different element
and a different
compound.
A more reactive element replaces a less active element in its compound.
Two possibilities of
replacement in the
Substitution Reaction:
Cation Replacement
Anion Replacement
Activity Series of the Elements
Metals Non-MetalsLi (most active) F Activity Series of the Element
Metals Non-metals
Li
K
Ba
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Ni
Sn
Pb
H
Cu
Bi
Sb
Hg
Ag
Pt
Au
FClBrOIS
(most active)
(least active)
Fe(s) + CuSO4(aq) FeSO4(aq) + Cu(s)
* Iron is more reactive than Copper
Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g)
* Zinc is more reactive than Hydrogen
CATIONS REPLACEMENT
General Formula: A + BC B + AC
Cu + 2 AgNO3 → 2 Ag + Cu(NO3)2
Fe + Cu(NO3)2 → Fe(NO3)2 + Cu
Ag + Cu(NO3)2 → No reaction
Au + HCl → No reaction
NOTE: IF THE REACTANT IN ELEMENTAL FORM IS NOT THE MORE REACTIVE METAL, THEN NO REACTION WILL OCCUR.
Activity Series of the Elements
Metals Non-MetalsLi (most active) F Activity Series of the Element
Metals Non-metals
Li
K
Ba
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Ni
Sn
Pb
H
Cu
Bi
Sb
Hg
Ag
Pt
Au
FClBrOIS
(most active)
(least active)
TRY THIS:
Zn + 2 HCl
Fe2O3(s) + 2 Al(s)
ZnCl2 + H2
Fe2(l) + Al2O3(s)
ANIONS REPLACEMENT
Cl2 + 2 Na Br → 2 NaCl + Br2
Br2 + 2 KI → 2 KBr + I2
General Formula: A + BC C + AB
I2 + 2 KBr → No reaction
NOTE: LESS REACTIVE HALOGEN CANNOT REPLACE THE MORE REACTIVE HALOGEN.
NO REACTION WILL OCCUR.
Activity Series of the Elements
Metals Non-MetalsLi (most active) F Activity Series of the Element
Metals Non-metals
Li
K
Ba
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Ni
Sn
Pb
H
Cu
Bi
Sb
Hg
Ag
Pt
Au
FClBrOIS
(most active)
(least active)
• Ionic Reaction
• when the negative ions in the two compounds switch places forming two new compounds.
General Formula:
AB+CD AD+CB
SEVERAL TYPES OF DOUBLE REPLACEMENT REACTIONS ARE FREQUENTLY ENCOUNTERED:
1. A reaction between a base such as NaOH, KOH or Ca(OH)2
in aqueous solution and an acid such as HCl, H2SO4 or
CH3COOH. Reactions of this type are called
NEUTRALIZATION and the products are always water
molecules and salt.
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(aq)
2. A reaction between solutions of two soluble salts, a soluble
salt and an acid, or a soluble salt and an alkali which, by
exchanging cations and anions, can produce one insoluble
compound or gas.
NaCl(aq) + AgNO3(aq) NaNO3(aq) + AgCl(s)
1. Sodium Chloride reacts with Potassium Bromide
to form Sodium Bromide and Potassium Chloride.NaCl + KBr NaBr + KCl
2. Iron Sulfide reacts with Hydrochloric Acid to produce
Iron Chloride and Hydrogen Sulfide.
FeS + 2 HCl FeCl2 + H2S
1. Silver Nitrate reacts with Potassium Chloride to produce Silver Chloride and Potassium Nitrate.
AgNO3 + KCl AgCl + KNO3
2. Silver Nitrate reacts with Hydrochloric acid to form Hydrogen Nitrate and Silver Nitrate.
AgNO3 + HCl → HNO3 + AgNO3
TRY THIS:
a chemical reaction in which a substance combines with oxygen and releases energy.
Always produce Carbon Dioxide and Water
General Formula:
CxHy + O2 CO2 + H2O
1. Methane reacts with Oxygen gas to produce Carbon
Dioxide and Water.
CH4 + 2 O2 CO2 + 2 H2O
2. Ethane reacts with Oxygen gas to form Carbon
Dioxide and Water.
2 C2H6 + 7 O2 4 CO2 + 6 H2O
3. Glucose (Sugar) reacts with Oxygen gas forming
Carbon Dioxide and Water.
C6H12O6 + 6 O2 6 CO2 + 6 H2O
EXERCISES
Identify the Types of Chemical Reaction of the following Chemical Equations:
3. N2(g) + 3 H3(g) 2 NH3(g)
1.
2. 2 AgBr(s) 2 Ag(s) + Br2(g)
Cu(s) + 2 AgNO3(s) → 2 Ag(s) + Cu(NO3)2(s)
4. BaCl2(s) + MgSO4(s) BaSO4(s) + MgCl2(s)
5. C3H8(g) + 12 O2(g) → 10 CO2(g) + 4 H2O(g)
ANSWERS:
1. Single Replacement or Substitution Reaction
2. Decomposition Reaction or Analysis Reaction
3. Combination Reaction or Synthesis Reaction
4. Double Replacement
5. Combustion Reaction
1. Silver Nitrate reacts with Copper metal to produce Copper (II) Nitrate and Silver.
2 AgNO3 + Cu Cu(NO3)2 + 2 Ag
2. Magnesium metal reacts with Hydrochloric acid to form Magnesium Chloride and Hydrogen gas.
Mg (s) + 2 HCl (aq) → MgCl2(aq) + H2(g)
TRY THIS:
1. Zinc combines with Hydrochloric Acid producing
Zinc Chloride and Hydrogen gas.
2. Sodium Iodide reacts with Bromine gas to form
Sodium Bromide and Iodine gas.
2 NaI + Br2 → 2 NaBr + I2
3. Aluminum reacts with Hydrochloric Acid to produce
Aluminum Chloride and Hydrogen gas.
2 Al + 6 HCl → 2 AlCl3 + 3 H2
Zn + 2 HCl → ZnCl2 + H2
