Mr. Matthew Totaro Legacy High School Honors Chemistry Chemical Bonding.
Mr. Matthew Totaro Legacy High School Honors Chemistry Chemical Reactions.
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Transcript of Mr. Matthew Totaro Legacy High School Honors Chemistry Chemical Reactions.
Mr. Matthew TotaroLegacy High SchoolHonors Chemistry
ChemicalReactions
2
Chemical Reactions• Reactions involve
chemical changes in matter resulting in new substances.
• Reactions involve rearrangement and exchange of atoms to produce new molecules.Elements are not
changed into new elements during a reaction.
Thermite Reaction
3
Example of a Chemical Reaction
Reactants Products
4
Evidence for a Chemical Reaction• Look for evidence of a new substance.
• Visual clues (permanent).Color change. Precipitate formation.
Solid that forms when liquid solutions are mixed.
Gas bubbles. Large energy changes.
Container becomes very hot or cold (transfer of heat).
Emission of light.• Other clues.
New odor. Whooshing sound from a tube. Permanent new state.
5
Evidence of a Chemical Change
Color Change
Formation of Solid PrecipitateFormation of a Gas
Emission of LightRelease or Absorption of Heat
6
Evidence of Chemical Change, Continued
• In order to be ABSOLUTELY SURE that a chemical reaction has taken place, you need to go down to the molecular level and analyze the structures of the molecules at the beginning and at the end.
Is boiling watera chemical change?
7
Practice—Decide Whether Each of the Following Involve a Chemical
Reaction.• Photosynthesis• Heating sugar until it turns black• Heating ice until it turns liquid• Digestion of food• Dissolving sugar in water• Burning of alcohol in a flambé dessert
Yes, CO2 and H2O combine into carbohydrates
Yes, sugar decomposing
No, molecules still same Yes, food decomposing and combining
with stomach acid
No, molecules still same
Yes, alcohol combining with O2 to make CO2 and H2O
Chemical Equations
Concise representation of a chemical reaction
9
The Combustion of Methane
• Methane gas burns to produce carbon dioxide gas and gaseous water.Whenever something burns it combines
with O2(g).
Anatomy of a Chemical Equation
CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)
Anatomy of a Chemical Equation
Reactants appear on the left side of
the equation.
CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)
Anatomy of a Chemical Equation
Products appear on the right side of the
equation.
CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)
Anatomy of a Chemical Equation
The states of the reactants and products are written in
parentheses to the right of each compound.
CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)
Anatomy of a Chemical Equation
Coefficients are inserted to balance
the equation.
CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)
Subscripts and Coefficients Give Different Information
• Subscripts tell the number of atoms of each element in a molecule
Subscripts and Coefficients Give Different Information
• Coefficients tell the number of molecules
17
Symbols Used in Equations
• Symbols used to indicate state after chemical.(g) = gas; (l) = liquid; (s) = solid.(aq) = aqueous = dissolved in
water.• Energy symbols used above the
arrow for decomposition reactions. ∆ = heat. hv = light.shock = mechanical.elec = electrical.
18
The Law of Conservation of Mass
Law of Conservation of Mass“We may lay it down as an
incontestable axiom that, in all the operations of art and
nature, nothing is created; an equal amount of matter
exists both before and after the experiment. Upon this principle, the whole art of
performing chemical experiments depends.”--Antoine Lavoisier, 1789
20
Conservation of Mass in a Reaction
• In a chemical reaction, matter cannot be created or destroyed.Therefore, the total mass cannot
change.And the total mass of the reactants
will be the same as the total mass of the products.
• In a chemical reaction, all the atoms present at the beginning are still present at the end.If all the atoms are still there, then
the mass will not change.
21
Balancing Example• When magnesium metal burns in air,
it produces a white, powdery compound magnesium oxide.
Mg(s) + O2(g) → MgO(s)
22
Another Balancing Example
• Under appropriate conditions at 1000°C, methane gas reacts with oxygen gas to produce gaseous carbon dioxide and steam
CH4(g) + O2(g) → CO2(g) + H2O(g)
Reaction Types
Synthesis (Combination) Reactions
• the combination of 2 or more substances to form a compound
• only one product
A + B AB
Synthesis (Combination) Reactions
• Examples:N2 (g) + 3 H2 (g) 2 NH3 (g)
C3H6 (g) + Br2 (l) C3H6Br2 (l)
2 Mg (s) + O2 (g) 2 MgO (s)
• Two or more substances react to form one product
2H2 (g) + O2 (g) 2H2O (g)
Decomposition Reactions
• a compound breaks down into 2 or more simpler substances
• only one reactant
AB A + B
Decomposition Reactions
• Examples:CaCO3 (s) CaO (s) + CO2 (g)
2 KClO3 (s) 2 KCl (s) + O2 (g)
2 NaN3 (s) 2 Na (s) + 3 N2 (g)
• One substance breaks down into two or
more substances
Combustion Reactions
CH4(g) + 2O2(g) CO2(g) + 2H2O(g)
• the burning of any substance in O2 to produce heat
A + O2 B
Combustion Reactions
• Examples:CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)
C3H8 (g) + 5 O2 (g) 3 CO2 (g) + 4 H2O (g)
• Rapid reactions that produce a
flame• Most often
involve hydrocarbons reacting with oxygen in the
air
31
Whoosh Bottle Demo is a Combustion
Reaction
C. Johannesson
Single Replacement• one element replaces another in a
compoundmetal replaces metal (+)
nonmetal replaces nonmetal (-)
A + BC B + AC
33
Single Replacement Example
C. Johannesson
Single ReplacementCu(s) + 2AgNO3(aq) Cu(NO3)2(aq) + 2Ag(s)
C. Johannesson
AB + CD AD + CB
Double Replacement
• ions in two compounds “change partners”
• cation of one compound combines with anion of the other
36
Double Replacement Example
C. Johannesson
Double Replacement
Pb(NO3)2(aq) + K2CrO4(aq) PbCrO4(s) + 2KNO3(aq)
38
Practice—Classify the Following Reactions as Synthesis, Decomposition, Single
Displacement, or Double Displacement.
3 Mg(s) + 2 FeCl3(aq) 3 MgCl2(aq) + 2 Fe(s)
CO2(g) + H2O(l) H2CO3(aq)
3 KOH(aq) + H3PO4(aq) K3PO4(aq) + 3 H2O(l)
)(CO )CaO( )(CaCO 23 gss
39
Practice—Classify the Following Reactions as Synthesis, Decomposition, Single
Displacement, or Double Displacement, Continued.
3 Mg(s) + 2 FeCl3(aq) 3 MgCl2(aq) + 2 Fe(s)
CO2(g) + H2O(l) H2CO3(aq)
3 KOH(aq) + H3PO4(aq) K3PO4(aq) + 3 H2O(l)
)(CO )CaO( )(CaCO 23 gss
Single replacement.
Double replacement.
Decomposition.
Synthesis.
Reaction Prediction
Synthesis Reactions
A + B AB
Al (s) + O2 (g)
Two substances combine to form a single compound.
Aluminum reacts with oxygen to produce aluminum oxide
Decomposition Reactions
K2CO3 (s) ∆
One compound breaks down into multiple substances (usually because of the
presence of heat).
AB A + B
Metal carbonate + heat → metal oxide + carbon dioxide gas
Combustion Reactions
CH4 (s) + O2 (g)
One substance reacts with Oxygen to form Carbon Dioxide and Water
A + O2 CO2 + H2O
Single Replacement Reactions
Cu (s) + AgNO3 (aq)
A + BC B + AC
A more active metal replaces a metal in a compound to form a new compound and an element
Double Replacement Reactions
AgNO3 (aq) + KCl (aq)
AB + CD AD + CB
Two compounds exchange partners to form two new compounds