Unit 3 – Chemical Reactions.  In many ionic reactions, not all of the chemical species undergo a change.  Those that do not change are called spectator.

Slides:

Advertisements

Similar presentations

Balancing Chemical Equations

Advertisements

Reactions in Aqueous Solutions

Chemical Reactions.

Dissolving an Ionic Electrolyte

Chapter 8 Chemical reactions

Chemical Reactions One or more substances are converted into new substances with different physical and chemical properties. [

Compounds in Aqueous Solutions. I. Dissociation Separation of ions that occurs when an ionic compound dissolves in water Balance chemical equation for.

Net Ionic Equations Precipitates ► A precipitate is the solid substance that separates from solution ► Precipitates can also form from reactions ► Reactions.

Net Ionic Equations.

Notes on Total and Net Ionic Equations. Ionic Compounds (Metal and Nonmetal) (Cation and Anion) If soluble these compounds will DISSOLVE and DISSOCIATE.

Net Ionic Equations mixing ionic compounds. Ionic interactions When you dissolve 2 or more ionic compounds in water some parts of it may react together.

Net Ionic Equations.

Solubility Rules and Precipitation Reactions. Not all ionic compounds dissolve! Instead of doing experiments all the time to see which ones will dissolve,

Unit 1 – reactions in aqueous solutions Lesson 2

Objectives To learn more about some of the results of chemical reactions To learn to predict the solid that forms in a precipitation reaction To learn.

 The ability to dissolve or break down into its component ions in a liquid  Example:  NaCl is soluble  Completely dissolves in water  AgCl is insoluble.

NCEA AS S1.8 Chemical Reactions NCEA L1 Science 2012.

Net Ionic Equations Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Net Ionic Equations.

Topic: Reactions in Aqueous Solution Do Now: Pick up 2 tests. Add correct answers to your test.

Types of Equations.

Journal Quiz #38 1.Calcium phosphate reacts with sodium hydroxide 2.Write the complete balanced equation 3.If you start with 50 grams of calcium phosphate,

Unit 2 - Chemical Reactions. Double displacement occurs between ions in aqueous solution. A reaction will occur when a pair of ions come together to produce.

Precipitates and Solubility

WRITING CHEMICAL EQUATIONS - Review Reactants (starting materials)  Products (ending materials) 2 Na(s) + Cl 2 (g)  2 NaCl(s) should be read as: 2 moles.

NCEA L1 Science Science NCEA L1 1.8 Chemical reactions.

Objective:  write a formula equation, complete ionic equation, and net ionic equation that represent a reaction.

Reactions in Aqueous Solution

WRITING CHEMICAL EQUATIONS

Reactions in Aqueous Solutions 1. Solutions (textbook p ) Aqueous Solution – A solution in which the solvent is water. Water is the solvent (does.

Chapter 6: Chemical Reactions.  Predict and write equations for precipitation reactions.  Write molecular, complete ionic, and net ionic equations.

Reactions in Aqueous Solution. Reactions in aqueous solution Many reactions, esp. many double replacement reactions, occur in water. What happens when.

Aqueous Reactions and Solution Stoichiometry. Electrolyte- a substance whose aqueous solutions contain ions. Nonelectrolyte- a substance that does not.

Aqueous Solutions Some solutes exist as molecules when dissolved in water (sugar, ethanol) Many solutes dissociate or form ions in water Acids form H +

Chemistry 20. Aqueous Up until this point we have said that when a chemical is dissolved in water it is aqueous. In reality, something else is happening.

Reactions of Ions in Solutions. Net Ionic Equations NaOHCuCl 2 Na + Cl - Cu +2 Cl - Dissolved in a solution the ionic compound breaks down into it’s ions.

CCBAB Compound ABCompound CD AD Compound ADCompound CB D ++ Magnesium Chloride MgCl 2 Calcium Hydroxide Ca(OH) 2 Magnesium Hydroxide Mg(OH) 2 Calcium Chloride.

Chapter 4; Reactions in Aqueous Solutions I.Electrolytes vs. NonElectrolytes II.Precipitation Reaction a)Solubility Rules.

Reactions. Ionic solutions can be identified by their ability to conduct electricity. If a large number of ions are present in a solution, the solution.

Reactions in Aqueous Solution Objectives: 1. Write and balance net ionic equations 2. Use solubility rules to predict the precipitate formed in double.

2 Word Equations. Phase Symbols Are subscripts that indicate the phase of the chemical.

Compounds in Aqueous Solutions When dissolved in water, ionic and molecular compounds behave differently.

4.5 Precipitation Reactions

1.15 Using Solubility Rules to Predict Precipitate Formation pp

Chapter 4-3 Chemical Quantities and

Water: removing dissolved solutes Chapter 12. Precipitation Reactions When two solutions are mixed, an insoluble compound sometimes forms. When two solutions.

Precipitation Reactions

Precipitation Reactions

Ionic Equations Most ionic compound dissociate (or break apart) when dissolved in water to form its component ions For example: NaCl (aq) really looks.

Ch (Net Ionic Equations)

Net ionic equations Na + Al 3+ S 2– 2Ca 2+ PO 4 3– 3Cl –

Double Displacement Reactions

Net Ionic Equations.

Ionic Equations. Net Ionic Equations AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) What happens when you put AgNO 3 and NaCl in water?

Chemical Equations Molecular, Total Ionic & Net Ionic Equations.

Reaction Prediction. You should already know... ionic, molecular, and acid nomenclature. how to balance chemical equations. the five common types of chemical.

Chapter 11 Chemical Reactions. Word Equations  Reactants  Products  Law of conservation of mass  Iron + oxygen  iron(III) oxide  Hydrogen peroxide.

Ions in Aqueous Solution Pb(NO 3 ) 2 (s) Pb(NO 3 ) 2 (aq) Pb 2+ (aq) + 2 NO 3 1– (aq) add water dissociation: Pb 2+ NO 3 1– Pb 2+ NO 3 1– “splitting into.

11.3 Reactions in Aqueous Solution 1 > Chapter 11 Chemical Reactions 11.1 Describing Chemical Reactions 11.2 Types of Chemical Reactions 11.3 Reactions.

Pick up a Packet and write down the following Essential Question: How are precipitation reactions written and how is a compound determined to be soluble.

Precipitation Reactions (Reactions that form a precipitate)

Precipitation Reactions & Solubility Rules Thursday, February 18 th, 2016.

MOLECULAR, (TOTAL) IONIC AND NET IONIC EQUATIONS 1.Sodium chloride and silver nitrate → sodium nitrate and silver chloride NaCl + AgNO 3 → NaNO 3 + AgCl(s)

Review of Science 10 Dissociation and Word Equations.

Reactions in Aqueous Solution. Aqueous Solutions Most chemical reactions involve substances dissolved in water –Solvent – Most plentiful substance in.

Net Ionic Equations The formation of an insoluble solid (a precipitate) drives a chemical reaction. Chemists use 3 types of equations to represent aqueous.

Ions in Aqueous Solutions

IONIC EQUATIONS.

11.3 Net Ionic Equations A complete ionic equation is an equation that shows dissolved ionic compounds as dissociated free ions. A precipitate of silver.

Ionic Equations.

Ch (Net Ionic Equations)

Presentation transcript:

Unit 3 – Chemical Reactions

 In many ionic reactions, not all of the chemical species undergo a change.  Those that do not change are called spectator ions.  When we remove these spectator ions from a chemical equation, they produce what is called a net ionic equation.  These indicate only the substances that undergo a change.

 Use the following 3 steps when writing net ionic equations:  1. Balance the equation for atoms.  2. Write out the dissolved chemical species as they exist in solution. Precipitates, liquids and gases are not written as ions. This is called a total ionic equation.  3. Remove common aqueous ions (ions that are in both the reactant and product). The resulting equation is then the net ionic equation.

 A solution of barium chloride combines with a solution of sodium carbonate to form a precipitate of barium carbonate and a solution of sodium chloride.  So… barium chloride + sodium carbonate  barium carbonate + sodium chloride BaCl 2(aq) + Na 2 CO 3(aq)  BaCO 3(s) + NaCl (aq)

 Now, we have something we can work with.  Step 1: Balance the equation for atoms. BaCl 2(aq) + Na 2 CO 3(aq)  BaCO 3(s) + 2NaCl (aq)

 Step 2: Write out the dissolved chemical species as they exist in solution. BaCl 2(aq) + Na 2 CO 3(aq)  BaCO 3(s) + NaCl (aq) becomes… Ba 2+ (aq) + 2Cl - (aq) + 2Na + (aq) + CO 3 2- (aq)  BaCO 3 (s) + 2Na + (aq) + 2Cl - (aq)

 Step 3: Remove common aqueous ions. Ba 2+ (aq) + 2Cl - (aq) + 2Na + (aq) + CO 3 2- (aq)  BaCO 3 (s) + 2Na + (aq) + 2Cl - (aq) becomes… Ba 2+ (aq) + CO 3 2- (aq)  BaCO 3(s) (net ionic equation)

 You will notice that in your net ionic equations, the number of atoms should be balanced, as well as the charge.  In our example, we had 1 Ba, 1 C, and 3 O on both sides of the net ionic equation, and the charges (-2 and +2) also balanced.  Number of atoms should remain constant as well. For example, if you were doing step 2 for something involving 2CaCl 2, the dissociation would look like this: 2Ca + (aq) + 4Cl - (aq)