Chemical Reactions 1. Chapter 7 Vocabulary Words Reactant Product Chemical Energy Exothermic Reaction Endothermic Reaction Chemical Equation Mole Ratio.

Slides:



Advertisements
Similar presentations
Unit 5 – Chemical Reactions Chapter 9
Advertisements

Chemical Reactions (aka Chemical Changes).
Chapter 11: Chemical Reacitons
Chemical Equations Test Review.
1 Chemical Reactions.
Types of Reactions 1.Synthesis reactions 2.Decomposition reactions 3.Single displacement reactions 4.Double displacement reactions 5.Combustion reactions.
IIIIIIIVV Intro to Reactions Ch. 8 – Chemical Reactions.
There are five types of chemical reactions you need to know: 1.Synthesis reactions 2.Decomposition reactions 3.Single displacement reactions 4.Double.
 Mass is never created or destroyed-ALL must be conserved and accounted for during a chemical reaction  The same number of atoms of reactant elements.
5 Types of Chemical Reactions
Unit 10: Chemical Equations
Chapter 6: Chemical Reactions. Chemical Equation represents a chemical change or reaction Reactants  Products Reactants – chemicals before the reaction.
Chemical Reactions.
Chemical Reactions Chapter 8.
Matter and Change 11.1 Describing Chemical Reactions Chapter 11
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.
Balancing Chemical Equations
Chapter 8: Chemical Equations and Reactions. 8.1 Describing Chemical Reactions a process in which 1 or more substances are converted into a NEW substance.
IIIIIIIVV I.Intro to Reactions Chemical Reactions.
Warm Up 12/18 Write the formula of the following ionic compound: magnesium phosphide. Hint: A magnesium cation has a charge of +2, and a phosphorus anion.
Chemical Reactions and Equations Chapter 8. What does a chemical formula represent?  The elements contained in a chemical substance  Indicates the number.
Aim: Stoichiometry and Chemical Reactions Review.
Chapter 10 Notes, Part I Parts of an equation Types of reactions.
S-133 Write the formula for Palladium (IV) Oxide Calcium Fluoride
Chemical Reactions and Equations Chapter 8. What does a chemical formula represent?  The elements contained in a chemical substance  Indicates the number.
Ch. 5 - Chemical Reactions I. Chemical Changes in Matter Chemical Reactions Law of Conservation of Mass Chemical Equations.
Ch – Chemical Reactions II. Balancing Equations read: (p. 278 – 283)
Chapter 11: Chemical Reacitons 11.1 Describing Chemical Reactions.
Unit 8 Chemical Reactions. What is a Chemical Reaction? When a substance is changed into another substance by chemical means When a substance is changed.
Chemical Reactions. PARTS OF A CHEMICAL EQUATION 2Mg + O 2  2MgO ReactantsProducts Coefficient “Produces Yields Forms” Subscript.
TYPES OF CHEMICAL REACTIONS
1 Chapter 6 Chemical Reactions. 2 Indications of a Chemical Reaction? l Color change l Odor change l Precipitate formed l Energy change (temperature/light)
Unit 7 Chemical Reactions Types of Reactions. Type of Reactions Chemical reactions are classified into five general types.
Unit 6 Chemical Reactions and Equations
Chapter 11 – Chemical Reactions There are many types of chemical reactions. We will study 5 of these. By being able to identify the type of chemical reaction.
Chemical Reactions. Writing Formulas: Review carbon tetrafluorideCF 4 Na 3 PO 4 sodium phosphate Cu 2 SO 4 cuprous sulfate AnalysisIf “Yes” The compound.
Chemical Equations and Reactions Chapter 8
Chemical Reactions Chapter 11 Steps to Writing Reactions 1. Transcribe words into formulas 2. Predict the product(s) using the type of reaction as a.
CH 8 Chemical Equations and Reactions Section 3 Classifying Chemical Reactions.
IIIIIIIVV I.Intro to Reactions Unit 7 – Chemical Reactions.
Chapter 10: Chemical Reactions. Chemical Reactions Defn – process by which the atoms of one or more substances are rearranged Defn – process by which.
Unit 4: Chemical Reactions. Warm Up Use the following Activity series to predict the products and balancing the equations Least ReactiveMost Reactive.
Chemical Reactions Quantitative Chem. Indicators of a Chemical Reaction.
Chemical Reactions Predicting Products. Combination (Synthesis) n the combination of 2 or more substances to form a single compound n only one product.
 1.What is the difference between a chemical and physical change? 2.Give an example of a chemical change and a physical change. 3.How can you tell a.
Symbolic Language of Chemistry
Chapter 8-Chemical Equations & Reactions 8.1-Describing Chemical Reactions 8.1-Describing Chemical Reactions 8.2-Types of Chemical Reactions 8.2-Types.
Chapter 6 Words to Know Key WordMeaning  catalyst catalytic converter combustion decomposition double replacement neutralization (acid-base) precipitate.
CHEMICAL REACTIONS! Chapter 11. Chemical reactions are occurring around us all the time: 1. Food cooking 2. Fuel being burned in a cars engine 3. Digesting.
Describing a Chemical Reaction Indications of a Chemical Reaction –Evolution of heat, light, and/or sound –Production of a gas –Formation of a precipitate.
Chemical Equations and Reactions Chemical Reactions A chemical rxn involves a chemical change in the identity of one or more chemical species. A chemical.
Types of Reactions. Synthesis Decomposition Single-replacement Double-replacement Combustion.
Unit 5: Stoichiometry and Chemical Reactions
Ch. 8 – Chemical Reactions
I. Chemical Changes in Matter Chemical Reaction
Equations.
Balancing, States of Matter, and Writing
I. Chemical Changes in Matter
Chemical Reactions and Stoichiometry
Chemical Reactions.
I. Chemical Changes in Matter
TYPES OF CHEMICAL REACTIONS
Chapter 11 Chemical Reactions 11.2 Types of Chemical Reactions
Chemical Reactions 1. H2 + I2 HI S 2. Na + H2O NaOH + H2 SR 3. CO + O2
Chemical Equations Test Review.
I. Chemical Changes in Matter
I. Chemical Changes in Matter
I. Chemical Changes in Matter
I. Chemical Changes in Matter
Presentation transcript:

Chemical Reactions 1

Chapter 7 Vocabulary Words Reactant Product Chemical Energy Exothermic Reaction Endothermic Reaction Chemical Equation Mole Ratio Synthesis Reaction Decomposition Reaction Combustion Reaction Single-Replacement Reaction Double Replacement Reaction Free Radical Oxidation-Reduction Reaction Catalyst Enzyme Substrate Chemical Equilibrium 2

What are elements made of? atoms What are chemical compounds made of? Two or more atoms of different elements What are the different types of compounds? Ionic  Metal + Nonmetal Covalent  Nonmetal + Nonmetal 3

3CuCl 2 + 2Al  2AlCl 3 + 3Cu reactantsproducts “yields” coefficient subscript 4

Types of Chemical Reactions 1.Synthesis 2.Decomposition 3.Single displacement 4.Double displacement 5

1. Synthesis reactions Occur when two substances combine and form 1 new compound A + B  AB Reactant + Reactant  1 Product Ex: 2H 2 + O 2  2H 2 O Ex: C + O 2  CO 2 6

2. DecompositionRxns Compound breaks up into elements or into smaller, simpler compounds AB  A + B 1 Reactant  Product + Product Ex: 2 H 2 O  2H 2 + O 2 7

Practice Identify the type of reaction for each of the following synthesis or decomposition reactions N 2 + O 2  BaCO 3  Co + S  NH 3 + H 2 CO 3  NI 3  8 2 NO (NH 4 ) 2 CO 3 N 2 + I 2 Co 2 S 3 BaO + CO 2 Synthesis Decomposition Synthesis Decomposition

Types of Reactions 1.Synthesis 2.Decomposition 3.Single displacement 4.Double displacement 9

3. Single Replacement Reactions Occur when one element replaces another in a compound. AB + C  CB + A Ex: CuCl 2 + 2Al  2AlCl 3 + 3Cu 10

Double Replacement Rxns Occurs when two elements swap places with one another *AB + CD  AD + CB Ex: Pb(NO 3 ) 2 + K 2 CrO 4  PbCrO 4 + 2KNO 3 11

Practice Identify the type of reaction. Pb(NO 3 ) 2 + 2KI  PbI 2 + 2KNO 3 Zn + 2HCl → ZnCl 2 + H 2 Fe + Cu(NO 3 ) 2 → Fe(NO 3 ) 2 + Cu FeS + HCl  FeCl 2 + H 2 S 12 SR DR SR DR

13

Counting Atoms CaCO 3 Ca= C= O= C 2 H 4 O 2 C= H= O= 2Li 3 AsO 4 Li= As= O= 2Ca(AlO 2 ) 2 Ca= Al= O= 14

BR: What is a chemical reaction? Describe it in your own words. EQ: In a chemical equation, where are the: Products? Reactants? 15 SPS2. Apply the Law of Conservation of Matter by balancing the following types of reactions: Synthesis Decomposition, Single replacement, and Double replacement. Left/Beginning Right/End

Mg + 2HCl  MgCl 2 + H 2 What are the reactants in this reaction? What are the products in this reaction? Mg and HCl MgCl 2 + H 2

Balancing Chemical Equations According to the Law of Conservation of Matter, atoms are not ____created______ or __destroyed___ during a chemical reaction. Scientists know that there must be the __same________ number of atoms on each ____side_________ of the ______equation______. To balance the chemical equation, you must place _______coefficients_____________ in front of the chemical formulas in the equation. You cannot __add______ or ____change______ subscripts!

How to balance an equation... 1) Count the number of atoms for each type of element on the reactants and products sides of the equation. 2) Pick an element that is not equal on both sides of the equation. 3) Place a coefficient in front of the formula with that element 4) Adjust your counts. 5) Continue placing coefficients to get the same number of atoms of each element on each side. Reduce your coefficients if possible.

Practice ___Mg + ___O 2  ___MgO

___N 2 + ___H 2  ___NH 3

___Cu 2 O + ___C  ___Cu + ___CO 2

___H 2 O 2  ___H 2 O + ___O 2

Balancing Chemical Equations BR: What do you use to balance chemical equations? Coefficients EQ: What law requires us to balance our chemical equations? Law of Conservation of Matter

Identify each type of reaction by their general equation: a. AB  A + B b. AB + C  CB + A c. A + B  AB d. AB + CD  AD + CB 25 Decomposition Single Replacement Double Replacement Synthesis

___Ca + ___O 2  ___CaO

Endothermic vs. Exothermic Reactions

Balancing Chemical Equations Iron(III) hydroxide breaks down to form iron(III) oxide and water. 28

Balancing Chemical Equations Aluminum fluoride combines with magnesium nitrate to form aluminum nitrate and magnesium fluoride. 29

Balancing Chemical Equations Calcium chloride combines with hydrogen sulfate to form calcium sulfate and hydrogen chloride. 30

Balancing Chemical Equations Aluminum fluoride combines with magnesium nitrate to form aluminum nitrate and magnesium fluoride.

Balancing Chemical Equations Iron(III) hydroxide breaks down to form iron(III) oxide and water.

Balancing Chemical Equations Calcium chloride combines with hydrogen sulfate to form calcium sulfate and hydrogen chloride.

34

35

36

Classifying and Balancing Chemical Reactions Part 3 6. AgNO 3 + KCl  AgCl + KNO 3 already balanced 7. 2H 2 O 2  2H 2 O + O 2 8. (NH 4 ) 2 SO 4 + Ba(NO 3 ) 2  BaSO 4 + 2NH 4 NO 3 9. MgI 2 + Br 2  MgBr 2 + I 2 already balanced 10. SO 3 + H 2 O  H 2 SO 4 already balanced

Write the chemical equations and balance them... 2AlF 3 + 3Mg(NO 3 ) 2  2Al(NO 3 ) 3 + 3MgF 2 CaCl 2 + H 2 SO 4  CaSO 4 + 2HCl 2Fe(OH) 3  Fe 2 O 3 + 3H 2 O

Write the following chemical equations in words and balance them... 2Al + 3CuSO 4  Al 2 (SO 4 ) 3 + 3Cu Aluminum and copper (II) sulfate yield aluminum sulfate and copper. SiO 2 + 2C  Si + 2CO Silicon dioxide plus carbon form silicon plus carbon monoxide. 2CaCO 3  2Ca + 2C + 3O 2 Calcium carbonate produces calcium, carbon, and oxygen.

Write the reaction in words and balance the equation. 1.K + H 2 O  KOH + H 2 potassium + dihydrogen oxide (water)  potassium hydroxide + hydrogen 2.CuCl 2 + Al  AlCl 3 + Cu copper (II) chloride + aluminum  aluminum chloride + copper 40

Write the chemical equation and balance. 1.Aluminum and oxygen gas (O 2 ) combine to form aluminum oxide. Al + O 2  Al 2 O 3 2. Carbon and iron(III)oxide react to form iron and carbon dioxide. C + Fe 2 O 3  Fe + CO 2 41