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What is a chemical reaction? When reactants are converted to products, bonds holding the atoms together are broken and new bonds are formed. Reactants.

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Presentation on theme: "What is a chemical reaction? When reactants are converted to products, bonds holding the atoms together are broken and new bonds are formed. Reactants."— Presentation transcript:


2 What is a chemical reaction? When reactants are converted to products, bonds holding the atoms together are broken and new bonds are formed. Reactants Products Recall that atoms themselves are neither created nor destroyed; they are merely rearranged.

3 What is a word equation? Chemical reactions can be described using words. Either Iron reacts with oxygen to produce iron (III) oxide (rust) Or Iron + Oxygen iron (III) oxide

4 How do we represent chemical equations? Easier to use chemical shorthand to represent chemical relationships Reactants on the left of the arrow and products to the right of the arrow Fe (s) + O2(g) Fe2O3(s) Where (s)= solid (l) = liquid (g) = gas (aq)= aqueous solution (dissolved in water) Heat or catalyst added to a reaction would appear above the arrow. See Table 8.1

5 Balancing Chemical Equations H 2 (g) + O 2 (g) H 2 O(l) Recall that matter is neither created or destroyed, so what is wrong with this picture? Its not balanced, we lost an oxygen, this is not possible so we balance the equation with coefficients, whole numbers that are placed in front representing the relative quantities of each compound. 2 H 2 (g) + O 2 (g) 2 H 2 O(l) Now both sides are equal.

6 Rules for Balancing Equations 1. Determine the correct formulas for all reactants and products in the reaction. Use parentheses when necessary. 2. Count the number of atoms of each element in the reactants and products. For simplicity, a polyatomic ion appearing unchanged on both sides can be counted as a single unit. 3. Balance the elements one at a time using coefficients. if no coefficient is written, it is assumed to be one. You cannot change the subscripts to balance the equation. 4. Check each atom or polyatomic ion to make sure it is balanced. 5. Finally make sure all the coefficients are in lowest possible ratios.

7 Example

8 Flow Chart for Balancing Chemical Equations

9 SECTION 8.2 Types of chemical equations

10 Plan of the Day PODfor extra credit Questions on lab? Homework? Types of Reactions Powerpoint

11 Plan of the day Major Reaction Types Get into a 5 groups Make a quick poster (big, bold, letters) These will be your notes for Reaction Types On your poster: Define your reaction Show an example How can you tell a reaction is your type of reaction Show the skeleton reaction!

12 Plan of the day Finish your notes in the lab while I get set up. Finish demos Work on our learning goal: Be able to identify types of reactions! Finish Worksheet from yesterday Please Bring in your Textbooks--Tomorrow!

13 Plan of the day Business Test corrections, retakes. Lab tomorrowwear appropriate clothing! Thus far in the Reaction Unit? Balancing Equations Identifying the 5 types of reactions What is left? Predicting Products Using solubility rules to predict double replacement reactions Net-Ionic Equations

14 Combination Reactions Two or more substances combine to form a single substance, or… Two or more products combine to form a single product. Example: Mg (s) + O 2 (g) MgO (s)

15 Predicting Combination Reactions 4 Possibilities: Metal + Non-Metal -- Ionic Compound K + Cl2 KCl Non-metal + Non-Metal (more than one product possible) S + O2 SO2 or SO3 Non-metal oxide + H2O acid SO2 + H2O H2SO4 Metallic oxide + H2O metal hydroxide CaO + H2O Ca (OH)2

16 Decomposition Reactions

17 Combustion Reactions Heated hydrogen reacts with oxygen to produce heat and water in a combustion reaction. This is also a combination reaction.

18 Predicting Combustion Element + Oxygen oxides Mg + O2 MgO Hydrocarbons (or alcohols) + Oxygen CO2 + H2O CH4 + O2 CO2 + H2O

19 Single Replacement Reactions

20 Predicting Products if the activity of the metal is higher than the metal cation in solution there will be a reaction, otherwise there is not a reaction. What is happening? The more reactive metal will form a compound with the anion, and the other metal will be pulled out of solution and become a solid metal again. Ex) Mg (s) + Zn(NO3)2 (aq) Mg(NO3)2 (aq)+ Zn(s)

21 Reactivity's A metal will not always replace a metal in a compound dissolved in water because of differing reactivity's. An activity series can be used to predict if reactions will occur.

22 Double Replacement Double replacement reactionsDouble replacement reactions occur when ions exchange between two compounds. A precipitate, gas, or molecule will form. This figure shows a generic double replacement equation.

23 Predicting Double Replacement The solid product produced during a chemical reaction in a solution is called a precipitate. precipitate All double replacement reactions produce either water, a precipitate, or a gas.

24 Double Replacements Continued This table shows the steps to write double replacement reactions.

25 Summary of Reactions This table summarizes different ways to predict the products of a chemical reaction.

26 Pop Quiz 1) Ca(OH) 2 + Al 2 (SO 4 ) 3 CaSO 4 + Al(OH) 3 2)Mg + Fe 2 O 3 Fe + MgO 3)C 2 H 4 + O 2 CO 2 + H 2 O 4)PbSO 4 PbSO 3 + O 2


28 Plan of the day Finals Revisit course expectations Check your grades to make sure they are accurate. Homework for Chapter 8: 33-53 (odd) due Friday!

29 What is a solution? An aqueous solution contains one or more dissolved substances (called solutes) in water.aqueous solutionsolutes The solvent is the most plentiful substance in a solution.solvent

30 Aqueous Solutions Water is always the solvent in an aqueous solution. There are many possible solutessugar and alcohol are molecular compounds that exist as molecules in aqueous solutions. Compounds that produce hydrogen ions in aqueous solutions are acids.

31 Ionic Compounds in Solution Ionic compounds can also be solutes in aqueous solutions. When ionic compounds dissolve in water, their ions separate in a process called dissociation.



34 Aqueous Reactions Continued When two solutions that contain ions as solutes are combined, the ions might react. If they react, it is always a double replacement reaction. Three products can form: precipitates, water, or gases.

35 Complete Ionic Equations Aqueous solutions of sodium hydroxide and copper(II) chloride react to form the precipitate copper(II) hydroxide. 2NaOH(aq) + CuCl 2 (aq) 2NaCl(aq) + Cu(OH) 2 (s) Ionic equations that show all of the particles in a solution as they actually exist are called complete ionic equations.complete ionic equations 2Na + (aq) + 2OH – (aq) + Cu 2+ (aq)+ 2Cl – (aq) 2Na + (aq) + 2Cl – (aq) + Cu(OH) 2 (s)

36 Ions that do not participate in a reaction are called spectator ions and are not usually written in ionic equations. spectator ions Formulas that include only the particles that participate in reactions are called net ionic ionic equations 2OH – (aq) + Cu 2+ (aq) Cu(OH) 2 (s)

37 Predicting Precipitates Using solubility rules for ionic equations we can predict whether a precipitate is formed and thus predicting what the products are. If the solubility rules predict insolubility we have a reaction, a precipitate! Example: Na 2 SO4 (aq) + BaNO 3 (s) ??? Assume double replacement Look at the products Any insoluble?

38 Example NaSO4 + BaNO3 ??? 1. Assume double replacement 2. Look at the products 3. Any insoluble? 4. Na2SO4 + Ba(NO3)2 2NaNO3 + Ba(SO4) 5. Write the complete ionic equation: 6. 2Na + (aq) + SO4 2- (aq) + Ba 2+ (aq) + 2NO3 - (aq) 2Na + (aq) + 2NO3 - (aq) + Ba(SO4) (s) 7. Eliminate all of the ions that did not change from the reactant side to the product side. 8. Ba 2+ (aq) + SO4 2- (aq) Ba(SO4) (s) (net ionic eqn)

39 Plan of the day Problems of the day Questions on homework. Lab Write Up.

40 Plan of the day Lab write up! Examples?

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