Writing Net Ionic Equations. Review UCEHB Double Replacement (UCEHB pg. 47; 55) Double Replacement (UCEHB pg. 47; 55) Redox / Single Replacement (UCEHB.

Slides:



Advertisements
Similar presentations
Reactions in Aqueous Solutions Chapter 7
Advertisements

Reactions in Aqueous Solutions
Reactions in Aqueous Solutions
WRITING AP EQUATIONS AP equation sets are found in the free-response section of the AP test. You are given three sets of reactants and you must write.
Net Ionic Equations Double Replacement Redox / Single Replacement
CHEMICAL REACTIONS.
Chemical Reactions Honor’s
Non-redox Reactions/ Double Replacement Reactions
Ionic Equations & Reactions
Chapter 11 Chemical Reactions
The main tasks of Chap 8 Sect 1 - Writing reactions from word problems – challenging Sect 2 - Balance Equations—easiest Sect 3 - Classify Equations, Complete.
Writing Chemical Reactions
Stoichiometry and Reactions
Chemical Reactions Chapter 11.
Chemical Equations and Reactions
Chemical Equations Preparation for College Chemistry Columbia University Department of Chemistry.
Reactions in Aqueous Solutions
Reactions in Aqueous Solutions
Types Of Chemical Reactions
Chapter 11 Chemical Reactions
Equations Double Replacement Redox Single Replacement (another redox) CompositionDecomposition Complex Ions Combustion.
1 Reactions in Aqueous Solutions Chapter 7. 2 Sodium Reacting with Water.
CH.3 Balancing Reactions Reaction Types
Chapter #7 Chemical Reactions. CHAPTER #7 CONTENTS 7-1 Grade School Volcanoes, Cars, & Detergents 7-2 Evidence of Chemical Reactions 7-3 The Chemical.
 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.
1 Reactions in Aqueous Solutions Chapter 7. 2 Predicting Whether a Reaction Will Occur “forces” that drive a reaction formation of a solid formation of.
Reactions in Aqueous Solutions
Predicting Products of Chemical Reactions Honors Chemistry Ch 10 (Still)
Chapter 9 Review 1.AgNO 3 + H 2 SO 4  Ag 2 SO 4 +HNO 3 What is the ratio of coefficients: 2 : 1 : 1 : 2 Is there a precipitate formed? yes. Ag 2 SO 4,
Reactions in Aqueous Solutions, Predicting Products and Classifying Types of Chemical Reactions.
Hall © 2005 Prentice Hall © 2005 General Chemistry 4 th edition, Hill, Petrucci, McCreary, Perry Chapter Four 1 Synthesis Reactions Type 1: A metal combines.
Net Ionic equations §A solution of Barium Chloride reacts with a solution of sodium sulfate §BaCl 2 + Na 2 SO 4 → §BaCl 2 + Na 2 SO 4 → BaSO 4 + 2NaCl.
Ch. 4 REACTIONS,SOLUTIONS Concentration [ ] dilution, molarity (moles/L) Replacement Rxns activity series, solubility Electrolytes Reduction – Oxidation.
College Chemistry Chapter 3 Stoichiometry. Law of Conservation of Mass All chemical and physical reactions must follow the LCM. Lavoisier was the first.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Reactions Chapter 4.
Section 4.1 Water Soluble Compounds Strong Electrolytes Weak Electrolytes Non Electrolytes Strong acids And Strong Bases Example: HNO 3 H.
Predicting Products to Reactions. Create this chart ReactantsPossible Rxn Type Possible Products.
Combustion Metal Oxide and Water  Nonmetal Oxide + Water Synthesis Salt containing polyatomic ion  Reactant + Reactant  Ammonia + Water  Dissociation.
Section 4.1 and 4.2 Types of Chemical Reactions and Aqueous Solutions.
Chapter 11 Chemical Reactions 11.1 Describing Chemical Reactions 11.2 Types of Chemical Reactions 11.3 Reactions in Aqueous Solutions The objective of.
Types Of Chemical Reactions
How do chemists know what to mix together to make the products they want??? Substances react with one another in similar ways depending on their chemical.
Oxidation Numbers, Reactions in Aqueous Solutions, & Predicting Products.
Chemical Reactions. What a chemical equation looks like: yields 2 Na (s) + Cl 2 (g)  2 NaCl (s) coefficients symbols state of matter.
Chapter 8 Types of Reactions. I. Introduction A.There are 5 basic reaction types: 1) Combination 2) Decomposition 3) Single Replacement 4) Double Replacement.
Chapter 8 Reactions in Aqueous Solution. Will a reaction Occur? Driving Forces in a Chemical Reaction  Formation of a solid  Formation of water  Formation.
Chapter 11, Chemical Reactions Day 1 is slides 1-30.
Reactions in Aqueous Solutions. 7.1 Predicting Whether a Reaction Will Occur? Driving Forces Formation of solid Formation of water Transfer of electrons.
1.To learn about some of the factors that cause reactions to occur 2.To learn to identify the solid that forms in a precipitation reaction 3.To learn to.
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.
Unit 7 Reactions in Solution Chem II Objectives  Describe the driving force for a chemical reaction.  Use generalizations to predict the products of.
Chemical Reactions. Writing Formulas: Review carbon tetrafluorideCF 4 Na 3 PO 4 sodium phosphate Cu 2 SO 4 cuprous sulfate AnalysisIf “Yes” The compound.
Sect.11.1 “Chemical Reactions” Chemical Rn: process by which one or more substances are changed into one or more different substances. Reminder: Substances.
8 - 1 Acid-Base Reactions If an acid reacts with a metal, a salt of that acid and hydrogen is produced.  aluminum + sulfuric acid → aluminum sulfate +
Preparation for AP Exam Free Response Question #4 Writing Reactions.
CH 8 Chemical Equations and Reactions Section 3 Classifying Chemical Reactions.
Types of Chemical Reactions I. Single replacement reaction II. Double replacement reaction III. Combination (synthesis) reaction IV. Decomposition reaction.
Write and balance the equation and identify the reaction type for each of the following reactions: Potassium metal reacts with chlorine gas Zn metal reacts.
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 =
What are the Types of Chemical Reactions? 1. Synthesis Reaction 2. Decomposition Reaction 3. Single Replacement Reaction 4. Double Replacement Reaction.
Chapter 11 Chemical Reactions. Word Equations  Reactants  Products  Law of conservation of mass  Iron + oxygen  iron(III) oxide  Hydrogen peroxide.
 Synthesis – 1 product  Decomposition – 1 reactant  Single displacement – 1 element & 1 compound react to produce a different element & a different.
Chapter 8 CHEMICAL REACTIONS. COMPONENTS OF A CHEMICAL REACTION ReactantsCatalystProduct(s) MnO 2 Fe(s) +O 2 (g)Fe 2 O 3 (s) State designations (s=solid,
Chemical Reactions Unit 11 (Chapter 11). Chemical Reactions A chemical reaction is a chemical change – Changes the way atoms are bonded to each other.
Reactions Online lecture. Metathesis Double Replacement Reactions.
Chemical Equation A representation of a chemical reaction: C 2 H 5 OH + 3O 2  2CO 2 + 3H 2 O reactants products.
Net Ionic Equations Double Replacement Redox / Single Replacement
DO NOW Pick up handout. Get out Concept Review handout.
Predicting the Products of Chemical Reactions
Predicting Products of Reactions
Presentation transcript:

Writing Net Ionic Equations

Review UCEHB Double Replacement (UCEHB pg. 47; 55) Double Replacement (UCEHB pg. 47; 55) Redox / Single Replacement (UCEHB pg. 45;63) Redox / Single Replacement (UCEHB pg. 45;63) Composition/Decomposition (UCEHB pg. 75) Composition/Decomposition (UCEHB pg. 75) Complex Ions (UCEHB pg. 23;79) Complex Ions (UCEHB pg. 23;79) Combustion (UCEHB pg. 29) Combustion (UCEHB pg. 29)

Double Replacement Reactions Identify the type: Identify the type: –Acid / Base: look for terms like excess;equal number of moles; equal volumes of __M. Think about the types of acids/bases; conjugate acid/base pairs. NH 3 + HF NH F – NH 3 + HF NH F – –Precipitation: memorize the solubility rules. Ba 2+ + SO 4 2- BaSO 4 Ba 2+ + SO 4 2- BaSO 4 –Both 2 H + + SO Ca(OH) 2 CaSO HOH 2 H + + SO Ca(OH) 2 CaSO HOH

Double Replacement Reactions –Reactants frequently in aqueous solutions. –Produce molecular compound such as water; gas; or precipitate. –Know how these gases CO 2 ; SO 2 ; NH 3 ; and H 2 S are formed. –Solubility rules help tell: »Which are ions in solution. »Identify the precipitate.

Redox / Single Replacement Redox Redox Know: Know: –Common oxidizing and reducing agents and the products formed. (UCEHB pg.68) –Use of key terms: acidified MnO 4 - ; H 2 O 2 ; Cr 2 O 7 2- ; HNO 3 MnO 4 - ; H 2 O 2 ; Cr 2 O 7 2- ; HNO 3 –Elements with multiple oxidation states Sn 2+ ; Sn 4+ ; Cr 2+ ; Cr 3+ ; Cr 6+ ; I - ; IO - ; IO 2 - ; Sn 2+ ; Sn 4+ ; Cr 2+ ; Cr 3+ ; Cr 6+ ; I - ; IO - ; IO 2 - ; O(-1 or -2) O(-1 or -2) –Acidic and Basic conditions 4 MnO H H 2 O 2 4 Mn O H 2 O 4 MnO H H 2 O 2 4 Mn O H 2 O

Redox / Single Replacement Single Replacement Single Replacement Like replaces like Like replaces like –Metals replace metals. 2Na (s) + 2H 2 O (l) 2 NaOH (aq) + H 2(g) 2Na + 2HOH 2 NaOH + H 2 2 Na (s) + 2H 2 O (l) 2Na + (aq) + 2OH - (aq) + H 2(g) 2 Na (s) + 2H 2 O (l) 2Na + (aq) + 2OH - (aq) + H 2(g) –Nonmetals replace nonmetals. Cl 2 (g) + 2 KI (aq) 2 K + (aq) + 2 Cl - (aq) + I 2(s) Cl 2 (g) + 2 KI (aq) 2 K + (aq) + 2 Cl - (aq) + I 2(s) Cl 2 (g) + 2 KI (aq) 2 K + (aq) + 2 Cl - (aq) + I 2 (s) Must be in aqueous solution to dissociate. Strong bases in aqueous solution 100% dissociation.

Combustion Reaction of a hydrocarbon/alcohol or other organic molecule with oxygen gas to produce carbon dioxide and water. Reaction of a hydrocarbon/alcohol or other organic molecule with oxygen gas to produce carbon dioxide and water. –Oxygen is a reactant. C 3 H 8 + 5O 2 3CO 2 + 4H 2 O C 3 H 8 + 5O 2 3CO 2 + 4H 2 O CH 3 CH 2 OH + 3O 2 2CO 2 + 3H 2 O CH 3 CH 2 OH + 3O 2 2CO 2 + 3H 2 O

Decomposition/Composition Decomposition: Decomposition: –has only one reactant and it breaks up into elements and /or compounds MgCO 3 MgO + CO 2 MgCO 3 MgO + CO 2 Ba(OH) 2 BaO + H 2 O Ba(OH) 2 BaO + H 2 O 2Al 2 O 3 4Al + 3O 2 2Al 2 O 3 4Al + 3O 2

Decomposition/Composition Composition: Composition: – has two reactants that combine into one product: S O 2 8 SO 2 S O 2 8 SO 2 –Nonmetal oxides plus water makes acid: acid: SO 3 + H 2 O 2 H + + SO 4 2- SO 3 + H 2 O 2 H + + SO 4 2- –Metal oxides plus water makes base: CaO + H 2 O Ca(OH) 2 CaO + H 2 O Ca(OH) 2

Complex Ions Particles that generally combine with excess ammonia or hydroxides to form complex ions with a charge Particles that generally combine with excess ammonia or hydroxides to form complex ions with a charge Cu NH 3 Cu(NH 3 ) 4 2+ Cu NH 3 Cu(NH 3 ) 4 2+ Al OH - Al(OH) 4 - Al OH - Al(OH) 4 - AgCl + 2 NH 3 Ag(NH 3 ) Cl - AgCl + 2 NH 3 Ag(NH 3 ) Cl - having the correct ligand number is not required but being consistent with number and charge is important having the correct ligand number is not required but being consistent with number and charge is important

Review Identify type of reaction. Identify type of reaction. –Remember: »What drives each type of reaction. »Conditions that must be met for each reaction type. Write a balanced equation. Write a balanced equation. –Include phase notations. Write the ionic equation. Write the ionic equation. –Check for appropriate charges. Write the net ionic equation. (This is your answer, but the other steps may provide you with information you need to answer the questions!) Write the net ionic equation. (This is your answer, but the other steps may provide you with information you need to answer the questions!) –Eliminate spectator ions.