Chapter 7 Balancing Chemical Equations Chemical Reaction Describes chemical reaction. Describes chemical reaction. Chemical equation: reactants yield.

Slides:



Advertisements
Similar presentations
Chemical Reactions.
Advertisements

Chapter 10 Chemical Reactions.
Chemical Reactions.
Chapter 11 Chemical Reactions.
Unit 5 – Chemical Reactions Chapter 9
The process by which one or more substances are changed into one or more different substances CHEMICAL REACTIONS.
Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products.
Chemical Reactions.
Original slides by Stephen L. Cotton
Chapter 11: Chemical Reacitons
 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.
Chapter 7 “Chemical Reactions”
“Chemical Reactions”.
Chemical Reactions Chapter 8.
Chemical Equations and Reactions
Matter and Change 11.1 Describing Chemical Reactions Chapter 11
Equations & Reactions. 8.1 Describing Chemical Reactions A. Chemical Changes and Reactions produced 1. New substances are produced. breaknew bonds 2.
1 Chapter 7 Chemical Reactions. 2 All chemical reactions l have two parts l Reactants - the substances you start with l Products- the substances you end.
1 Chapter 5 “Chemical Reactions” CP Chemistry. 2 Describing Chemical Reactions l OBJECTIVES: –Describe how to write a word equation.
Chapter 11 Chemical Reactions
Types of Chemical Reactions p
Keefe 1415 CHAPTER 11 PART 1: BALANCING EQUATIONS.
CHEMICAL REACTIONS. Chemical Reactions A process by which the atoms of one or more substances are rearranged to form different substances A process by.
 Balanced Chemical Equation – a representation of a chemical reaction using symbols that show the same number of atoms of each element on both sides.
Chemical Reactions. All chemical reactions involve changes in substances Reactants – starting substances Products – new substances formed Reactants 
Unit 9 Chemical Equations
1 Chemical Reactions Chapter 6. 2 All chemical reactions l Have two parts l Reactants - the substances you start with l Products- the substances you end.
Ch. 5 - Chemical Reactions I. Chemical Changes in Matter Chemical Reactions Law of Conservation of Mass Chemical Equations.
Chemical Reactions Balancing Chemical Equations Types of Reactions.
Chemistry Ch 8 - Chemical Reactions Reactions & Equations When you take substances and rearrange their atoms to form new substances you have created.
2/14/11 – “C” day  Objective: To assess the concepts of ionic and covalent bonding.  Do Now: What property of water is determined by its shape? How.
1 Chemical Reactions. 2 All chemical reactions l have two parts l Reactants - the substances you start with l Products- the substances you end up with.
 Write skeleton equations from the following word equations AND balance them: ◦ In water, iron (III) chloride reacts with sodium hydroxide producing solid.
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.
1 Chemical Reactions. 2 Evidence of Reactions Looking for the clues.
1 Chemical Reactions. 2 All chemical reactions l Have two parts l Reactants - the substances you start with l Products- the substances you end up with.
Chemical Reactions Unit 8. Chemical Reaction vs. Chemical Equation A REACTION is the process where 2 or more atoms or compounds rearrange themselves to.
Chemical Reactions 1. Nature of Chemical Reactions 2. Reaction Types 3. Balancing Chemical Reactions.
1 Chapter 7 Chemical Reactions Killarney High School.
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)
Chemical Reactions. Did a Chemical Reaction Take Place? There are several ways to tell if a chemical reaction has occurred… –Temperature change –Color.
1 Section 8.1 Describing Chemical Change l OBJECTIVES: –Write equations describing chemical reactions, using appropriate symbols.
Chemical Reactions. Describing Chemical Reactions 11.1.
Chapter 9 Balancing Equations. Parts of a Reaction H 2 SO 3 (aq)  H 2 O (l) + SO 2 (g) ReactantsProducts l = liquid g = gas aq = aqueous (water solution)
Chapter 8 Describing Chemical Change Types of Chemical Reactions Reactions in Aqueous Solution.
Chemical Reactions.
Chapter 8 Chemical Reactions.
Unit 6 Chemical Reactions.
 have two parts: 1.Reactants = the substances you start with 2.Products = the substances you end up with  The reactants will turn into the products.
Classifying Chemical Reactions Chapter 9. Chemical Reaction - A process in which the physical and chemical properties of the original substances change.
Chemical Reactions Chemistry Chapter 9. Objectives Recognize evidence of chemical change Represent chemical reactions with equations Classify chemical.
Semester 1 Chemistry Review DAY 2 Formula Weight Find the formula weight of aluminum sulfate. Al 2 (SO 4 ) 3 Al - 2 x = S - 3 x =
Chapter 10: Chemical Reactions. Chemical Reactions Defn – process by which the atoms of one or more substances are rearranged Defn – process by which.
Chapter 11 Chemical Reactions. Word Equations  Reactants  Products  Law of conservation of mass  Iron + oxygen  iron(III) oxide  Hydrogen peroxide.
Chapter 11 Chemical Reactions Chemistry 2. Describing Chemical Reactions 11.1.
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.
Chemical Reactions. Chemical reaction Process by which atoms of one or more substances are rearranged to form different substances General Rule’s to determine.
Chemical Reactions. In a chemical reaction: there is a change in the way atoms are joined together there is a change in the way atoms are joined together.
I. Writing and Balancing Equations II. Identifying Reaction Types Unit 6 Chemical Reactions.
Chemical Reactions.  Chemical Reaction  Reactant  Product  Combustion Reaction  Decomposition Reaction  Single-replacement reaction  Double-replacement.
Chemical Reactions CHAPTER 11. WHAT ARE OUR REPRESENTATIVE, OR BASIC PARTICLES? They are the smallest pieces of a substance. For a molecular compound:
Chapter 10 Chemical Reactions. Reactions and Equations A chemical reaction is the process by which the atoms of one or more substances are rearranged.
Classifying Chemical Reactions Chapter 9. Chemical Reaction - A process in which the physical and chemical properties of the original substances change.
CHAPTER 8 CHEMICAL EQUATIONS The Chemical Equation is a shorthand expression for a chemical change or reaction.
Chemical Equations and Reactions Chapter 8. Key Terms Chemical reaction Chemical equation Coefficient Combustion reaction Synthesis reaction Decomposition.
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 & Equations
Classifying Chemical Reactions
Chemical Reactions.
Presentation transcript:

Chapter 7 Balancing Chemical Equations

Chemical Reaction Describes chemical reaction. Describes chemical reaction. Chemical equation: reactants yield products Chemical equation: reactants yield products Catalyst = substance that speeds up a reaction without being used up.

Symbols Used (s) solid (s) solid (l) liquid (l) liquid (g) gas (g) gas (aq) aqueous (in water solution) (aq) aqueous (in water solution)  gas as a product  gas as a product  ppt. (precipitate)  ppt. (precipitate)  means with heat  means with heat Ptmeans with Platinum catalyst Ptmeans with Platinum catalyst

Balancing Chemical Equations Balanced equations have: the same # of atoms of each element on each side of the equation. Balanced equations have: the same # of atoms of each element on each side of the equation. Law of Conservation of Mass – atoms can neither be created nor destroyed, simply rearranged. Law of Conservation of Mass – atoms can neither be created nor destroyed, simply rearranged.

Rules for Balancing Equations Get the correct formulas for reactants and products. Get the correct formulas for reactants and products. Write reactants on left, products on right and use plus signs and arrows when needed. Write reactants on left, products on right and use plus signs and arrows when needed. Count the # of atoms of each element in reactants and products.(Polyatomic ions on both sides count as one.) Count the # of atoms of each element in reactants and products.(Polyatomic ions on both sides count as one.) Balance # of each element using coefficients. Balance # of each element using coefficients. –Coefficient – whole # in front of a formula.

Rules for Balancing Equations Check each element to make sure equation is balanced. Check each element to make sure equation is balanced. Make sure all coefficients are in the lowest whole number ratio. Make sure all coefficients are in the lowest whole number ratio. Do not change subscripts!!!

Diatomic Molecules Diatomic Molecules- a molecule made up two atoms of the same element. They are only diatomic when they are alone. -There are 7 naturally occurring diatomic molecules. H O N Cl Br I F

5 Types of Reactions - 1 Combination Reaction – elements combine to form a compound. A + B AB

Examples of Combination Reactions 1. 2 Na + Cl 2 2 NaCl 2. Cu + S Cu 2 S 2 3. SO 3 + H 2 O H 2 SO 4 4. CaO + H 2 O Ca(OH) 2 5. Mg + O 2 MgO 2 2

5 Types of Reactions - 2 Decomposition Reaction – elements break down into its element. AB A + B AB A + B

Examples of Decomposition Reactions 1. 2 NaCl 2 Na + Cl 2 2. H 2 O H 2 + O HgOHg +O Challenge: Copper I Chloride Decomposes 2CuCl 2Cu + Cl 2

5 Types of Reactions - 3 Single Replacement Reaction – one element replaces another element in a compound. AB + C A + CB AB + C A + CBor AB + D AD + B AB + D AD + B

Reactivity Series of Metals and Non-Metals The single metallic element will only replace the metal in a compound if it is more reactive. The single metallic element will only replace the metal in a compound if it is more reactive. A chart is used to determine if the lone metal is more reactive. If not, no reaction occurs. A chart is used to determine if the lone metal is more reactive. If not, no reaction occurs. The single non-metallic element will only replace the non-metal in a compound if it is more reactive. The higher up in the group the non-metal is, the more reactive it is. The single non-metallic element will only replace the non-metal in a compound if it is more reactive. The higher up in the group the non-metal is, the more reactive it is.

Examples of Single Replacement Reactions 1. Zn + H 2 SO 4 ZnSO 4 + H 2 2. K + HOH KOH + H 2 3. Cl 2 + NaBr NaCl + Br 2 22

5 Types of Reactions - 4 Double Replacement Reaction – two compounds react and exchange positive ions to form two new compounds. AB + CD AD + CB AB + CD AD + CB

Examples of Double Replacement Reactions 1. NaOH + H 2 SO 4 Na 2 SO 4 + HOH 2. BaCl 2 + K 2 CO 3 BaCO 3 + KCl 3. FeS + HCl H 2 S + FeCl

5 Types of Reactions - 5 Combustion Reaction – oxygen reacts with a compound composed of C and H. C x H y + O 2 CO 2 + H 2 0 C x H y + O 2 CO 2 + H 2 0 Also called Burning (exothermic) The products are always CO 2 and H 2 O.

Examples of Combustion Reactions 1. C 6 H 6 + O 2 CO 2 + H 2 O 2. CH 3 OH + O 2 CO 2 + H 2 O 367½ 21½ CH 3 OH + O 2 CO 2 + H 2 O C 6 H 6 + O 2 CO 2 + H 2 O

Special Decomposition Reactions: 1 Decomposition of a Carbonate: Decomposition of a Carbonate: XCO 3 XO + CO 2 ex. Na 2 CO 3 Na 2 O + CO 2

Special Decomposition Reactions: 2 Decomposition of a Hydroxide: Decomposition of a Hydroxide: XOH XO + H 2 O ex. 2NaOH Na 2 O + H 2 O

Special Decomposition Reactions: 3 Decomposition of a Chlorate: Decomposition of a Chlorate: XClO 3 XCl + O 2 XClO 3 XCl + O 2 ex. NaClO 3 NaCl + O 2

Special Decomposition Reactions: 4 Special single Replacement Reaction: Special single Replacement Reaction: »Group IA or IIA metal and H 2 O X + HOH XOH + H 2 ex. 2Na + 2HOH 2NaOH + H 2

How to ID types of reactions. Combination Reactions – given 2 items that form 1 new compound. Decomposition Reactions – given a single compound that breaks into parts. Single Replacement – given a single element plus a single compound, forms a new compound a a different element. Double Replacement – given two compounds (+’s or –’s change places). Combustion Reaction – given CH compound with Oxygen, always forms water and carbon dioxide.