Types of Chemical Reactions. Reactants: Zn + I 2 Product: Zn I 2.

Types of Chemical Reactions

Reactants: Zn + I 2 Product: Zn I 2

Types of Chemical Reactions: At the conclusion of our time together, you should be able to: 1.List the 5 basic types of chemical reactions 2.Use this list to describe a reaction

Decomposition Simple Reactions Synthesis (Combination) Single Replacement Double Replacement

Decomposition Synthesis Single Replacement Double Replacement ABAB + AB AB + ABAB + C + C ABAB + C + CDD

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Types of Reactions There are five types of chemical reactions we will talk about: There are five types of chemical reactions we will talk about: 1. Synthesis reactions 2. Decomposition reactions 3. Single displacement reactions 4. Double displacement reactions 5. Combustion reactions You need to be able to identify the type of reaction and predict the product(s) You need to be able to identify the type of reaction and predict the product(s)

Steps to Writing Reactions Some steps for doing reactions Some steps for doing reactions 1. Identify the type of reaction 2. Predict the product(s) using the type of reaction as a model 3. Balance it Don’t forget about the diatomic elements! (BrINClHOF) or (7 + 1) For example, Oxygen is O 2 as an element. In a compound, it can’t be a diatomic element because it’s not an element anymore, it’s a compound!

Synthesis Reactions

Synthesis Reactions: At the conclusion of our time together, you should be able to: 1.Recognize a synthesis chemical reaction 2.Balance this reaction type

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Synthesis reactions Synthesis reactions occur when two substances (generally elements) combine and form a compound. (Sometimes these are called combination or addition reactions.) Synthesis reactions occur when two substances (generally elements) combine and form a compound. (Sometimes these are called combination or addition reactions.) reactant + reactant  1 product Basically: A + B  AB Basically: A + B  AB Example: 2H 2 + O 2  2H 2 O Example: 2H 2 + O 2  2H 2 O Example:C + O 2  Example:C + O 2  CO 2

Synthesis Reactions Here is another example of a synthesis reaction Here is another example of a synthesis reaction

Synthesis Reaction Predict the products and balance the following reaction: Predict the products and balance the following reaction: Na + Cl 2  NaCl NaCl 2 Na + Cl 2  2 NaCl

Synthesis Reactions = One main purpose: One main purpose: To make a more complex compound!! To make a more complex compound!!

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Synthesis Reactions: Let’s see if you can: 1.Recognize a synthesis chemical reaction 2.Balance this reaction type

Practice Predict the products. Write and balance the following synthesis reaction equations. Predict the products. Write and balance the following synthesis reaction equations. Sodium metal reacts with chlorine gas Sodium metal reacts with chlorine gas Na (s) + Cl 2(g)  Na (s) + Cl 2(g)  Solid Magnesium reacts with fluorine gas Solid Magnesium reacts with fluorine gas Mg (s) + F 2(g)  Mg (s) + F 2(g)  Aluminum metal reacts with fluorine gas Aluminum metal reacts with fluorine gas Al (s) + F 2(g)  Al (s) + F 2(g)  NaCl MgF 2 AlF 3

Practice State the type, predict the products and balance the following reactions: State the type, predict the products and balance the following reactions: Cesium reacts with bromine gas  Cs + Br 2  CsBr CsBr 2 Cs + Br 2  2 CsBr

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Decomposition Reactions

Decomposition Reactions: At the conclusion of our time together, you should be able to: 1.Identify decomposition chemical reactions 2.Balance this type of reaction

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Decomposition Reactions Decomposition reactions occur when a compound breaks up into the elements or in a few to simpler compounds Decomposition reactions occur when a compound breaks up into the elements or in a few to simpler compounds 1 Reactant  Product + Product 1 Reactant  Product + Product In general: AB  A + B In general: AB  A + B Example: 2 H 2 O  2H 2 + O 2 Example: 2 H 2 O  2H 2 + O 2 Example: 2 HgO  Example: 2 HgO  2Hg + O 2

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Decomposition Reactions For Decomposition reactions to occur we need energy as a catalyst in the form of: For Decomposition reactions to occur we need energy as a catalyst in the form of: Heat Heat Light Light Electricity Electricity Mechanical shock Mechanical shock Or a chemical catalyst Or a chemical catalyst

Decomposition Reactions Another view of a decomposition reaction: Another view of a decomposition reaction:

Decomposition Exceptions Carbonates and chlorates are special case decomposition reactions that do not go to the elements. You should be able to recognize these as decomposition only. Carbonates and chlorates are special case decomposition reactions that do not go to the elements. You should be able to recognize these as decomposition only. Carbonates (CO 3 2- ) decompose to carbon dioxide and a metal oxide Carbonates (CO 3 2- ) decompose to carbon dioxide and a metal oxide Example: CaCO 3  CO 2 + CaO Example: CaCO 3  CO 2 + CaO Chlorates (ClO 3 - ) decompose to oxygen gas and a metal chloride Chlorates (ClO 3 - ) decompose to oxygen gas and a metal chloride Example: 2 Al(ClO 3 ) 3  2 AlCl 3 + 9 O 2 Example: 2 Al(ClO 3 ) 3  2 AlCl 3 + 9 O 2

Decomposition Exceptions Ternary acids will tend to decompose to water and the nonmetal oxide. Ternary acids will tend to decompose to water and the nonmetal oxide. Example: H 2 SO 3  H 2 O + SO 2 Example: H 2 SO 3  H 2 O + SO 2 There are other special cases, but we will not explore those in this class There are other special cases, but we will not explore those in this class

Practice of Decomposition Predict the products and balance the following reactions: Predict the products and balance the following reactions: H2OH2OH2OH2O H 2 + O 2 2 H 2 O  2 H 2 + O 2

Practice Predict the products. Then, write and balance the following decomposition reaction equations: Predict the products. Then, write and balance the following decomposition reaction equations: Solid Lead (IV) oxide decomposes PbO 2(s)  Solid Lead (IV) oxide decomposes PbO 2(s)  Aluminum nitride decomposes Aluminum nitride decomposes AlN (s)  AlN (s)  Pb + O 2 Al + N 2

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Decomposition: Let’s see if you can: 1.Identify decomposition chemical reactions 2.Balance this type of reaction

Practice Identify the type of reaction for each of the following decomposition reactions, and write the balanced equation: BaCO 3(s)  NI 3(s)  BaO + CO 2 N 2 + I 2 2, 1, 3

Practice of Decomposition Predict the products and balance the following reactions: Predict the products and balance the following reactions: Iron (II) oxide decomposes  Iron (II) oxide decomposes  FeO  Fe + O 2 2 FeO  2 Fe + O 2

Practice Identify the type of reaction for each of the following synthesis or decomposition reactions, and write the balanced equation: N 2(g) + O 2(g)  BaCO 3(s)  Co (s) + S (s)  NI 3(s)  (Co = +3) Nitrogen monoxide 2 NO BaO + CO 2 Co 2 S 3 2, 3, 1 N 2 + I 2 2, 1, 3

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Single Displacement

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Single Displacement: At the conclusion of our time together, you should be able to: 1.Identify a basic single displacement reaction 2.Use the reactivity series table to determine if the reaction will take place 3.Balance a single displacement reaction

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Single Replacement Reactions Single Replacement Reactions occur when one element replaces another in a compound. Single Replacement Reactions occur when one element replaces another in a compound. A metal can replace a metal (+) OR a halogen can replace a halogen (-). A metal can replace a metal (+) OR a halogen can replace a halogen (-). element + compound  element + compound element + compound  element + compound A + BC  AC + B (if A is a metal) OR A + BC  BA + C (if A is a ) A + BC  BA + C (if A is a halogen ) (remember the cation always goes first!)

Single Replacement Reactions For these reactions, you must remember: For these reactions, you must remember: When H 2 O splits into ions, it splits into H + and OH - (not H+ and O -2 !!) A single replacement reaction will only occur if the replacement ion has a higher activity than the original ion in the compound To determine this, refer to a relative activity table

Relative Activities Metals Decreasing ActivityHalogens Lithium, LiFluorine, F Potassium, KChlorine, Cl Calcium, CaBromine, Br Sodium, NaIodine, I Magnesium, Mg Aluminum, Al Zinc, ZnHydrogen, H Chromium, CrCopper, Cu Iron, FeMercury, Hg Nickel, NiSilver, Ag Tin, SnPlatinum, Pt Lead, PbGold, Au

Single Replacement Reactions (note: Li is higher relative activity than H): (note: Li is higher relative activity than H):

A Displacement Reaction: metallic copper with silver nitrate Cu + Ag NO 3 Ag + Cu(NO 3 ) 2 Note: Cu is higher relative activity

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Single Replacement Reactions Write and balance the following single replacement reaction equation: Write and balance the following single replacement reaction equation: Zinc metal reacts with aqueous hydrochloric acid Zinc metal reacts with aqueous hydrochloric acid Zn (s) + HCl (aq)  Zn (s) + HCl (aq)  ZnCl 2 + H 2(g) Note: Zinc replaces the hydrogen ion in the reaction because of higher relative activity 2

Single Replacement Aluminum metal reacts with aqueous copper (II) nitrate Aluminum metal reacts with aqueous copper (II) nitrate Al (s) + Cu(NO 3 ) 2(aq)  Al (s) + Cu(NO 3 ) 2(aq)  Al(NO 3 ) 3(aq) + Cu 2 Al (s) + 3 Cu(NO 3 ) 2(aq)  2 Al(NO 3 ) 3(aq) + 3 Cu

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Single Displacement: Let’s see if you can: 1.Identify a basic single displacement reaction 2.Use the reactivity series table to determine if the reaction will take place 3.Balance a single displacement reaction

Try This… Predict the products and balance the following reactions: Predict the products and balance the following reactions: Zinc reacts with aqueous copper (II) sulfate Zinc reacts with aqueous copper (II) sulfate Zinc is higher relative activity so… Zn + CuSO 4  Zinc is higher relative activity so… Zn + CuSO 4  Cu + Z n SO 4

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Try This… Predict the products and balance the following reactions: Predict the products and balance the following reactions: Copper (II) reacts with aqueous calcium sulfate Copper (II) reacts with aqueous calcium sulfate Cu + CaSO 4  Cu + CaSO 4  Copper is lower relative activity so… Copper is lower relative activity so… Cu + CaSO 4  NR Cu + CaSO 4  NR

Try These Last Two: Sodium chloride solid reacts with fluorine gas Sodium chloride solid reacts with fluorine gas NaCl (s) + F 2(g)  NaF (s) + Cl 2(g) NaCl (s) + F 2(g)  NaF (s) + Cl 2(g) Note that fluorine replaces chlorine in the compound Aluminum metal reacts with aqueous copper (II) nitrate Aluminum metal reacts with aqueous copper (II) nitrate Al (s) + Cu(NO 3 ) 2(aq)  Al (s) + Cu(NO 3 ) 2(aq)  Al(NO 3 ) 3(aq) + Cu 2, 3, 2, 3 Demo Time!! 22

Double Displacement

Double Displacement: At the conclusion of our time together, you should be able to: 1.List the types of chemical reactions that we’ve covered so far 2.Identify a double displacement reaction 3.Determine the products of a double displacement reaction by the foil method 4.Balance a double displacement reaction

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Double Replacement Reactions Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound Compound + compound  compound+ compound Compound + compound  compound+ compound AB + CD  AD + CB AB + CD  AD + CB

Double Replacement Reactions Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together Example: Example: AgNO 3(aq) + NaCl (s)  AgNO 3(aq) + NaCl (s)  AgCl (s) + NaNO 3(aq) Another example: Another example: K 2 SO 4(aq) + Ba(NO 3 ) 2(aq)  KNO 3(aq) + BaSO 4(s) KNO 3(aq) + BaSO 4(s) 2

3 Driving Forces for Double Replacement Reactions Water Forms Gas Forms Solid Forms If one of the above is not a product, there will be no reaction.

Double Displacement Reactions K 2 CrO 4(aq) + Ba(NO 3 ) 2(aq)  BaCrO 4(s) + 2 KNO 3(aq) Soluble Soluble Soluble Soluble Insoluble Soluble Insoluble Soluble Driving Force? Solid Forms (Precipitate)

Neutralization Reaction Acid + Base  Salt + Water HCl + NaOH  NaCl + H 2 O SolubleSoluble SolubleSoluble Soluble Molecular Soluble Molecular Driving Force? Water Forms

Practice Predict the products. Balance the equation Predict the products. Balance the equation 1. FeCl 3 (aq) + NaOH (aq)  2. H 2 SO 4 (aq) + NaOH (aq)  3. KOH (aq) + CuSO 4 (aq)  4. Ba(NO 3 ) 2(aq) + K 2 CrO 4 (aq)  5. Demo Time!! NaCl + Fe(OH) 3 Na 2 SO 4 + H 2 O Cu(OH) 2 + K 2 SO 4 BaCrO 4 + KNO 3

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Double Displacement: Let’s see if you can: 1.List the types of chemical reactions that we’ve covered so far 2.Identify a double displacement reaction 3.Determine the products of a double displacement reaction by the foil method 4.Balance a double displacement reaction

Practice Quiz Write the double displacement reaction and give the driving force: Write the double displacement reaction and give the driving force: Silver nitrate reacts with calcium chloride Silver nitrate reacts with calcium chloride AgNO 3 + CaCl 2  AgCl + Ca(NO 3 ) 2 2AgNO 3 + CaCl 2  2AgCl + Ca(NO 3 ) 2 Every compound above is soluble except for silver chloride. What is the driving force? Solid Forms

Practice Predict the products. Don’t balance the equation. Predict the products. Don’t balance the equation. 1. HCl (aq) + AgNO 3 (aq)  2. CaCl 2 (aq) + Na 3 PO 4 (aq)  3. Pb(NO 3 ) 2(aq) + BaCl 2 (aq)  4. Demo Time!! AgCl + HNO 3 NaCl + Ca 3 (PO 4 ) 2 Ba(NO 3 ) 2 + PbCl 2

The Final Reaction Type Combustion

Combustion: At the conclusion of our time together, you should be able to: 1.Identify a basic combustion reaction 2.Predict the products of combustion reactions 3.Balance this reaction type

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Combustion Reactions Combustion reactions occur when a hydrocarbon reacts with oxygen gas. Combustion reactions occur when a hydrocarbon reacts with oxygen gas. This is also called burning!!! In order to burn something you need the 3 things in the “fire triangle”: This is also called burning!!! In order to burn something you need the 3 things in the “fire triangle”: 1) A Fuel (hydrocarbon) 2) Oxygen to burn it with 3) Something to ignite the reaction (spark) 1) A Fuel (hydrocarbon) 2) Oxygen to burn it with 3) Something to ignite the reaction (spark)

Combustion Reactions In general: C x H y + O 2  CO 2 + H 2 O In general: C x H y + O 2  CO 2 + H 2 O Products in combustion are ALWAYS carbon dioxide and water. (although incomplete burning does cause some by- products like carbon monoxide) Products in combustion are ALWAYS carbon dioxide and water. (although incomplete burning does cause some by- products like carbon monoxide) Combustion is used to heat homes and run automobiles (octane, as in gasoline, is C 8 H 18 ) Combustion is used to heat homes and run automobiles (octane, as in gasoline, is C 8 H 18 )

Combustion Reactions In general: C x H y + O 2  CO 2 + H 2 O In general: C x H y + O 2  CO 2 + H 2 O They are always exothermic They are always exothermic (they give off heat) (they give off heat)

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Combustion of Methane CH 4 + O 2  CH 4 + O 2  CO 2 + H 2 O 1 2 2

Combustion of Pentane: Predict the products and balance the reaction: Predict the products and balance the reaction: C 5 H 12 + O 2  CO 2 + H 2 O CO 2 + H 2 O 56 8

Predict the products and balance the reaction: Predict the products and balance the reaction: C 3 H 7 OH + O 2  CO 2 + H 2 O CO 2 + H 2 O Combustion of Propanol 2 68 9

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Combustion: Let’s see if you can: 1.Identify a basic combustion reaction 2.Predict the products of combustion reactions 3.Balance this reaction type

Practice Predict the products and balance the reaction of hexene burning in air: C 6 H 12 + O 2  C 6 H 12 + O 2  CO 2 + H 2 O 669

Combustion Example Example C 5 H 12 + O 2  CO 2 + H 2 O C 5 H 12 + O 2  CO 2 + H 2 O Write the products and balance the following combustion reaction: Write the products and balance the following combustion reaction: C 10 H 22 + O 2  C 10 H 22 + O 2  CO 2 + H 2 O 568 20 31 22 2

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Mixed Practice State the type, predict the products, and balance the following reactions: State the type, predict the products, and balance the following reactions: 1. BaCl 2 + H 2 SO 4  2. C 6 H 12 + O 2  3. Zn + CuSO 4  4. Cs + Br 2  5. FeCO 3  Double Displacement Combustion Single Displacement Synthesis Decomposition

Types of Chemical Reactions. Reactants: Zn + I 2 Product: Zn I 2.

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Types of Chemical Reactions. Reactants: Zn + I 2 Product: Zn I 2.

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