Synthesis Decomposition Single Replacement Combustion

Slides:



Advertisements
Similar presentations
Unit 7 Chemical Reactions
Advertisements

IIIIIIIVV Ch. 21 – Chemical Reactions II. Types of Chemical Reactions.
Types of Chemical Reactions 5 Main Categories + Acid/Base Reactions.
Chemical Reactions.
The five general types of reaction are combination, decomposition, single- replacement, double-replacement, and combustion.
 REACTANTS  PRODUCTS 1. Starting substances (reactants) becomes new substances (products).  2. Bonds are broken and new bonds are formed, but atoms.
IIIIIIIVV Intro to Reactions Ch. 8 – Chemical Reactions.
The five general types of reaction are combination, decomposition, single- replacement, double-replacement, and combustion.
Chemical Equations. What are they? Equations showing chemical change(s). Example: CH 4 + 2O 2 CO 2 + 2H 2 O **Law of Conservation of Mass: reactantsproducts.
5 Types of Chemical Reactions
Chemical Equations & Reactions Chapter 8. Objectives List observations that suggest that a chemical reaction has taken place. List three requirements.
Classifying Chemical Reactions. Decomposition Description: Compounds break down Form: AB  A + B Example: MgO  Mg + O.
Chapter 11 Chemical Reactions 11.2 Types of Chemical Reactions
Chemical Reactions Chapter 8.
Types of Chemical Reactions
Chemical Reactions: Reactants change chemical and physical properties …. to become new substances made from the same elements; these are called products.
IIIIIIIVV I.Intro to Reactions Ch.7– Chemical Reactions.
Chapter 5 Chemical Reactions The Nature of Reactions Types of Reactions Oxidation-Reduction Reactions Balancing Chemical Equations Rates of change.
IIIIIIIVV I.Intro to Reactions Chemical Reactions.
Chapter 10 Notes, Part I Parts of an equation Types of reactions.
IIIIIIIVV Chemical Reactions Types of Chemical Reactions.
IIIIIIIVV Chemical Reactions Types of Chemical Reactions.
Rules for Balancing Equations Determine the correct formula for all reactants and products. Write the formulas for the reactants on the left side of arrow.
Types of Chemical Reactions Writing Chemical Reactions.
By: Seamus O’Brien.  In a chemical reaction the elements bond to each other through the taking or sharing of valence electrons.  During chemical reactions.
Chemical Equations and Reactions. Some Definitions Chemical reaction = The process by which one or more substances are changed into one or more different.
Chapter 24 Lesson 3 Classifying Chemical Reactions.
Chemical Reactions Types of Chemical Reactions. Chemical Reactions  Objectives  Define and give general equations for synthesis, decomposition, single-displacement,
Aim: What are the five general types of reactions? Do Now: Write and balance the Chemical Equation 1.Zinc and lead (II) nitrate react to form zinc nitrate.
How can we tell if a reaction takes place?. There are four clues: 1. _______________ 2. _______________ 3. _______________ 4. _______________.
 In a chemical reaction, one or more substances change into new/different substances  According to the Law of Conservation of Mass a skeleton chemical.
Types of Reactions Including reaction prediction.
Unit 7 Chemical Reactions Types of Reactions. Type of Reactions Chemical reactions are classified into five general types.
Chapter 6: Chemical Reactions.  Identify redox reactions.  Identify and write equations for combustion reactions.
Types of Chemical Reactions
IIIIIIIVV Chemical Reactions Types of Chemical Reactions.
Type of Reactions Chemical reactions are classified into several general types Combination (Synthesis) Decomposition Single Replacement Double Replacement.
Classifying Chemical Reactions. Types of Reactions There are literally millions of chemical reactions that occur every day. Chemists have defined five.
Types of Reactions. The Six Different Types of Reactions Synthesis Reaction Decomposition Reaction Single Replacement Reaction Double Replacement Reaction.
Chapter 8 Notes, Part I Parts of an equation Types of reactions.
Types of Reactions.
Chemical Reactions Ch. 8.
Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products.
IIIIIIIVV I.Intro to Reactions Unit 7 – Chemical Reactions.
Types of Chemical Reactions I. Single replacement reaction II. Double replacement reaction III. Combination (synthesis) reaction IV. Decomposition reaction.
Chapter 11 Chemical Reactions 11.2 Types of Chemical Reactions
What are the Types of Chemical Reactions? 1. Synthesis Reaction 2. Decomposition Reaction 3. Single Replacement Reaction 4. Double Replacement Reaction.
Chapter 5 Chemical Reactions
 In a chemical reaction, one or more substances change into new/different substances  According to the Law of Conservation of Mass a skeleton chemical.
We know the signs that a chemical reaction has occurred, but how do we know what is going on the molecular/atomic level (i.e., how do we know what compounds.
IIIIIIIVV Chemical Reactions Types of Chemical Reactions.
Chemical Reactions Types of Chemical Reactions. Chemical Reactions 5 Types of Chemical Reactions » synthesis » decomposition » single-displacement » double-displacement.
Movie: types of chemical reactions:
Chapter 8 Chemical Equations and Reactions. Types of Chemical Reactions  Direct Combination: (Synthesis) A + B  AB  Decomposition: AB  A + B  Single.
Chemical Reactions. In a chemical reaction, atoms are rearranged to form new compounds. The starting substances = reactants Ending substances = products.
IIIIIIIVV C. Johannesson Ch. 8 – Chemical Reactions II. Types of Chemical Reactions (p )
Redox Reactions Synthesis Decomposition Single Replacement Combustion.
Chapter 8-Chemical Equations & Reactions 8.1-Describing Chemical Reactions 8.1-Describing Chemical Reactions 8.2-Types of Chemical Reactions 8.2-Types.
Chemical Reactions CHAPTER 11. WHAT ARE OUR REPRESENTATIVE, OR BASIC PARTICLES? They are the smallest pieces of a substance. For a molecular compound:
Types of Reactions.
Chapter 19: Chemical Reactions
CHEMISTRY Jacqueline P. Hancock, B.S.,M.Ed
Classifying Reactions
Chemical Reactions A + B AB Reaction Type:
Types of Chemical Reactions
Chapter 11 Chemical Reactions 11.2 Types of Chemical Reactions
Types of Reactions.
Classifying Reactions
Classifying Reactions
Presentation transcript:

Synthesis Decomposition Single Replacement Combustion Redox Reactions Synthesis Decomposition Single Replacement Combustion

objective I can classify redox reactions so I can recognize patterns of chemical behavior and predict the products of reactions.

Redox Reaction Review In an oxidation – reduction reaction (or Redox reaction), electrons are lost by one element and gained by another element. Reactions that involve elements as reactants or products are always redox. EX. Mg (s) + O2 (g)  MgO(s)

Which of the following is a redox reaction? 2K(s) + Cl2(g) → 2KCl(s) H2O2(aq) → H2O(l) + O2(g) 2Al(s) + 3Cu(SO4)(aq) → 3Cu(s) + Al2(SO4)3(aq) CH4(g) + O2(g) → CO2(g) + 2H2O(l) all of the above are redox reactions [Default] [MC Any] [MC All]

Redox Reactions We classify chemical reactions so that we can recognize patterns of chemical behavior, and predict the products that will form. The following four types of reactions are all considered Redox Reactions. Synthesis A + B  AB Decomposition AB  A + B Single Replacement A + BC  B + AC Combustion CxHy + O2  CO2 + H2O

Synthesis Redox Reaction A + B  AB two or more substances combine to form a single substance. The two reactants are frequently a Metal and a non-Metal. The product that they form is then a(n) ionic compound. To write the correct formulas for ionic compounds, we use the criss-cross method.

Synthesis Redox Reaction A. Group A metals and a nonmetal react with each other to produce a compound made up of a metal cation and a nonmetal anion. __K + __Cl2  ________ __K + __Cl2  __KCl 2K + Cl2  2KCl

Synthesis Redox Reaction A. Group A metals and a nonmetal react with each other to produce a compound made up of a metal cation and a nonmetal anion. __K + __Cl2  ________ __K + __Cl2  __KCl 2K + Cl2  2KCl

Synthesis Redox Reaction B. More than one product is also possible when a transition metal and a nonmetal react. Fe + S  FeS iron(II) sulfide 2Fe + 3S  Fe2S3 iron(III) sulfide

Synthesis Redox Reaction C. When two nonmetals react by synthesis, more than one product is often possible. S + O2  SO2 sulfur dioxide 2S + 3O2  2SO3 sulfur trioxide

Which of the following represents a synthesis reaction? AB  A + B A + BC  B + AC A + B  AB AB + CD  CB + AD [Default] [MC Any] [MC All]

Which of these is a synthesis redox reaction? CH4(g) + O2(g) → CO2(g) + 2 H2O(l) 2H2O2(aq) → 2H2O(l) + O2(g) 2K(s) + Cl2(g) → 2KCl(s) [Default] [MC Any] [MC All]

Decomposition Redox Reaction AB  A + B In a decomposition reaction, a single compound is broken down into two or more products. The reactant: a single compound The products: more than one element or compound. Most decomposition reactions require a catalyst in the form of a chemical, heat, light, or electricity.

TNT C7H5N3O6 TNT is one of the most commonly used explosives for military and industrial applications. 2 C7H5N3O6(s) → 3 N2(g) + 5 H2(g) + 12 CO(g) + 2 C(s)

Which of these is a decomposition reaction? CH4(g) + O2(g) → CO2(g) + 2 H2O(l) 2H2O2(aq) → 2H2O(l) + O2(g) 2K(s) + Cl2(g) → 2KCl(s) [Default] [MC Any] [MC All]

Lab Demonstrations Synthesis Reaction: Decomposition Reactions: “Iron reacts with oxygen to produce iron (III) oxide (rust)” Iron + oxygen  iron(III) oxide ____Fe(s) + ____O2(g)  ____Fe2O3 (s) Decomposition Reactions: “Hydrogen peroxide decomposes to form water and oxygen gas.” Hydrogen Peroxide  water + oxygen ____H2O2 (aq)  ____H2O(l) + ____O2(g) “In the presence of electricity, water decomposes to form oxygen and hydrogen” ____H2O(l)  ___H2(g) + ___ O2 (g)

REdox Reactions part II Single Replacement Combustion REdox Reactions part II

Single-Replacement Reactions A + BC  B + AC A metal element replaces a second metal element in the compound. “A replaces B” AC and BC are ionic compounds Example: 3 Mg (s) + 2 AlCl3 (aq)  2 Al (s) + 3 MgCl2 (aq)

Which of the following represents a single replacement reaction? AB  A + B A + BC  B + AC A + B  AB AB + CD  CB + AD [Default] [MC Any] [MC All]

Which of the following is a single replacement redox reaction? 2 K(s) + Cl2(g) → 2 KCl(s) H2O2(aq) → H2O(l) + O2(g) 2 Al(s) + 3 Cu(SO4)(aq) → 3 Cu(s) + Al2(SO4)3(aq) CH4(g) + O2(g) → CO2(g) + 2 H2O(l) none of the above [Default] [MC Any] [MC All]

Single Replacement Reactions A + BC  B + AC Not all single replacement reactions can occur. Whether one metal will replace another metal from a compound can be determined by the relative reactivities of the two metals.

Single Replacement Reactions A + BC  B + AC A reactive metal will only replace a metal listed below it in the Activity Series. Mg(s) + Zn(NO3)2(aq)  Mg(s) + Li(NO3)(aq) 

Single Replacement Reactions A + BC  B + AC A reactive metal will only replace a metal listed below it in the Activity Series. Mg(s) + Zn(NO3)2(aq)  Mg(NO3)2(aq) + Zn(s) Mg(s) + Li(NO3)(aq)  no reaction

Which of these is higher on the activity series? calcium magnesium [Default] [MC Any] [MC All]

Which of these is higher on the activity series? hydrogen magnesium [Default] [MC Any] [MC All]

Mg(s) + 2HCl(aq)  H2(g) + MgCl2(aq) A reactive metal will only replace a metal listed below it in the Activity Series. Which of these reactions will NOT occur? Mg(s) + 2HCl(aq)  H2(g) + MgCl2(aq) H2(g) + MgCl2(aq)  Mg(s) + 2HCl(aq) [Default] [MC Any] [MC All]

Can this single replacement reaction occur Can this single replacement reaction occur? “aluminum reacts with rust to produce iron and aluminum oxide” 2Al(s) + Fe2O3(s)  2Fe(s) + Al2O3(s) Yes No

Combustion Reactions

Combustion Reactions CxHy + O2  CO2 + H2O + energy A. In a combustion reaction, a compound reacts with oxygen to produce energy as heat, light or electricity. B. Reactants: hydrocarbons (compounds of hydrogen and carbon) and oxygen Products: carbon dioxide and water

Which of these is always the products of a combustion reaction? oxygen and heat hydrogen and oxygen water and carbon dioxide carbon dioxide and oxygen [Default] [MC Any] [MC All]

You observe the combustion of butane C4H10…… You observe the combustion of butane C4H10……. Which of these reactants must also be present? C4H10 water carbon dioxide gas oxygen gas hydrogen gas [Default] [MC Any] [MC All]

Combustion reaction Example: CH4 (g) + 2O2 (g)  CO2 (g) + 2H2O

Hydrocarbon molecule examples - CxHy propane C3H8 methane CH4 octane C8H18

Which of the following represents a combustion redox reaction? AB  A + B A + BC  B + AC HxCy + O2  CO2 + H2O A + B  AB AB + CD  CB + AD none of the above [Default] [MC Any] [MC All]

Which of these is a combustion reaction? C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) 2H2O2(aq) → 2H2O(l) + O2(g) 2K(s) + Cl2(g) → 2KCl(s) [Default] [MC Any] [MC All]

Redox Lab Demos Single Replacement: aluminum reacts with iron(III)oxide to replace the iron and forms aluminum oxide __Al(s) + __Fe2O3(s)  __Fe(s) + __Al2O3(s) Combustion: Propane (C3H8) reacts with oxygen to produce carbon dioxide gas, water and heat. __ C3H8 + __O2  __ CO2 + __H2O + heat Ethyl alcohol reacts with oxygen to produce carbon dioxide gas and water