Net Ionic Equations Making Sense of Chemical Reactions

Size: px
Start display at page:

Download "Net Ionic Equations Making Sense of Chemical Reactions"

Transcription

1 14 Making Sense of Chemical Reactions OBJECTIVE Students will be able to write net ionic equations from balanced molecular equations. LEVEL Chemistry NATIONAL STANDARDS UCP.1, UCP.2, B.3 T E A C H E R P A G E S CONNECTIONS TO AP AP Chemistry: III. Reactions A. Reaction Types 1. Acid-base reactions 2. Precipitation reactions 3. Oxidationreduction reactions B. Stoichiometry 1. Ionic and molecular species present in chemical systems: net ionic equations TIME FRAME 45 minutes MATERIALS periodic table solubility rules student white boards (optional) TEACHER NOTES This lesson should follow a study of the five main types of chemical reactions. Having students write net ionic equations will enhance their ability to understand what is really happening in the beaker type questions. The student lecture notes can provide the basis for your lecture over this material. Guide students through the proper steps of writing net ionic equations using several examples until the students feel confident. It often helps to demonstrate the example chemical reactions. This is easily accomplished by mixing the stated solutions in a test tube or beaker and asking students to explain in chemical terms what has taken place. Did the solution change color? Did a gas form? (Your demonstration solutions may need to be fairly concentrated in some cases so that enough gas is formed to actually cause bubbling.) Did a precipitate form? Follow this lesson with The Eight Solution Problem lab to reinforce observing chemical reactions and give students more practice writing net ionic equations. 410 Laying the Foundation in Chemistry

2 14 Train students to write the state symbols for each species. Doing so will reduce the chance of incorrect spectator cancellations. For example, if zinc metal reacts with hydrochloric acid, the following net ionic equation results: Zn(s) + 2 H + (aq) Zn 2+ (aq) + H 2 (g) Students often cancel out the zinc terms even though one is a solid metal while the other is an ion in solution. Requiring students to write the state symbols makes it a bit more evident that the two terms are not identical and therefore do not cancel. Students should memorize the strong acids and the strong bases. An abbreviated table of the most common solubility rules is presented within this lesson. It is strongly recommended that your students begin memorizing the solubility rules during the first year of chemistry. The solubility rules must be memorized for the AP* exam. Continue writing net ionic reactions throughout the year when explaining the chemical reactions associated with demonstrations as well as during pre- and post-lab discussions to continually reinforce this concept. Answers to the examples from the notes: Demonstrate these reactions whenever possible as you guide students through the example reactions. Recognition of state symbols is much easier when students actually see the reaction take place. Example 1 is worked out on the student pages. The answers to examples 2 5 follow. Example 2: Solutions of iron(iii) nitrate and potassium hydroxide are mixed. Balanced formula equation: Fe(NO 3 ) 3 (aq) + 3 KOH(aq) 3 KNO 3 (aq) + Fe(OH) 3 (s) T E A C H E R P A G E S Total ionic equation: Fe 3+ (aq) + 3 NO 3 (aq) + 3 K + (aq) + 3 OH (aq) 3 K + (aq) + 3 NO 3 (aq) + Fe(OH) 3 (s) Balanced net ionic equation: Fe 3+ (aq) + 3 OH (aq) Fe(OH) 3 (s) Example 3: Magnesium ribbon reacts with hydrochloric acid. Balanced formula equation: Mg(s) + 2 HCl(aq) MgCl 2 (aq) + H 2 (g) Total ionic equation: Mg(s) + 2 H + (aq) + 2 Cl (aq) Mg 2+ (aq) + 2 Cl (aq) + H 2 (g) Balanced net ionic equation: Mg(s) + 2 H + (aq) Mg 2+ (aq) + H 2 (g) Laying the Foundation in Chemistry 411

3 14 Example 4: Solutions of acetic acid and lithium bicarbonate are mixed. Balanced formula equation: HC 2 H 3 O 2 (aq) + LiHCO 3 (aq) LiC 2 H 3 O 2 (aq) + H 2 CO 3 (aq) Total ionic equation: HC 2 H 3 O 2 (aq) + Li + (aq) + HCO 3 (aq) Li + (aq) + C 2 H 3 O 2 (aq) + H 2 O(l) + CO 2 (g) Balanced net ionic equation: HC 2 H 3 O 2 (aq) + HCO 3 (aq) H 2 O(l) + CO 2 (g) + C 2 H 3 O 2 (aq) T E A C H E R P A G E S Example 5: Solutions of magnesium chloride and calcium nitrate are mixed. Balanced formula equation: MgCl 2 (aq) + Ca(NO 3 ) 2 (aq) CaCl 2 (aq) + Mg(NO 3 ) 2 (aq) Total ionic equation: Mg 2+ (aq) + 2 Cl (aq) + Ca 2+ (aq) + 2 NO 3 (aq) Ca 2+ (aq) + 2 Cl (aq) + Mg 2+ (aq) + 2 NO 3 (aq) Balanced net ionic equation: No net ionic equation everything cancels so there is no driving force this was just a physical combination of two different solutions with no chemical reaction taking place. ANSWERS TO THE CONCLUSION QUESTIONS 1. Solutions of lead(ii) nitrate and lithium chloride are mixed. Pb(NO 3 ) 2 (aq) + 2 LiCl(aq) 2 LiNO 3 (aq) + PbCl 2 (aq) Pb 2+ (aq) + 2 NO 3 (aq) + 2 Li + (aq) + 2 Cl (aq) 2 Li + (aq) + 2 NO 3 (aq) + PbCl 2 (s) Pb 2+ (aq) + 2 Cl (aq) PbCl 2 (s) 2. Copper metal is placed into a solution of silver nitrate. Cu(s) + 2 AgNO 3 (aq) Cu(NO 3 ) 2 (aq) + 2 Ag(s) Cu(s) + 2 Ag + (aq) + 2 NO 3 (aq) Cu 2+ (aq) + 2 NO 3 (aq) + 2 Ag(s) Cu(s) + 2 Ag + (aq) Cu 2+ (aq) + 2 Ag(s) 3. Solid potassium chlorate decomposes upon heating. 2 KClO 3 (s) 2 KCl(s) + 3 O 2 (g) 2 KClO 3 (s) 2 KCl(s) + 3 O 2 (g) 2 KClO 3 (s) 2 KCl(s) + 3 O 2 (g) NOTE: Solids and gases do not ionize. All three reactions are therefore the same. Students do not need to write three identical equations to receive full credit. 412 Laying the Foundation in Chemistry

4 14 4. Solid sodium metal is placed into distilled water. 2 Na(s) + 2 H 2 O(l) 2 NaOH(aq) + H 2 (g) 2 Na(s) + 2 H 2 O(l) 2 Na + (aq) + 2 OH (aq) + H 2 (g) 2 Na(s) + 2 H 2 O(l) 2 Na + (aq) + 2 OH (aq) + H 2 (g) NOTE: There are no spectator ions in this equation; therefore students need not repeat the second equation in order to receive full credit. 5. Chlorine gas is bubbled into a solution of magnesium bromide. Cl 2 (g) + MgBr 2 (aq) MgCl 2 (aq) + Br 2 (l) Cl 2 (g) + Mg 2+ (aq) + 2 Br (aq) Mg 2+ (aq) + 2 Cl (aq) + Br 2 (l) Cl 2 (g) + 2 Br (aq) 2 Cl (aq) + Br 2 (l) 6. Methane gas is burned in the presence of oxygen gas. CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O(g) NOTE: All reactants and products are either gases or molecular compounds, so this is the net ionic equation. 7. Solutions of silver acetate and barium chloride are mixed. 2 AgC 2 H 3 O 2 (aq) + BaCl 2 (aq) 2 AgCl(s) + Ba(C 2 H 3 O 2 ) 2 (aq) 2 Ag + (aq) + 2 C 2 H 3 O 2 (aq) + Ba 2+ (aq) + 2 Cl (aq) 2 AgCl(s) + Ba 2+ (aq) + 2 C 2 H 3 O 2 (aq) Ag + (aq) + Cl (aq) AgCl(s) 8. Solutions of sodium bicarbonate and hydrochloric acid are mixed. NaHCO 3 (aq) + HCl(aq) NaCl(aq) + H 2 CO 3 (aq) Na + (aq) + HCO 3 (aq) + H + (aq) + Cl (aq) Na + (aq) + Cl (aq) + H 2 O(l) + CO 2 (g) HCO 3 (aq) + H + (aq) H 2 O(l) + CO 2 (g) NOTE: Carbonic acid quickly decomposes into liquid water and carbon dioxide gas. T E A C H E R P A G E S 9. Solutions of ammonium perchlorate and barium hydroxide are mixed. 2 NH 4 ClO 4 (aq) + Ba(OH) 2 (aq) 2 NH 4 OH(aq) + Ba(ClO 4 ) 2 (aq) 2 NH 4 + (aq) + 2 ClO 4 (aq) + Ba 2+ (aq) + 2 OH (aq) 2 NH 3 (g) + 2 H 2 O(l) + Ba 2+ (aq) + 2 ClO 4 (aq) NH 4 + (aq) + OH (aq) NH 3 (g) + H 2 O(l) NOTE: Ammonium hydroxide decomposes into ammonia gas and liquid water. 10. Solutions of tin(ii) fluoride and lithium carbonate are mixed. SnF 2 (aq) + Li 2 CO 3 (aq) SnCO 3 (s) + 2 LiF(aq) Sn 2+ (aq) + 2 F (aq) + 2 Li + (aq) + CO 3 2 (aq) SnCO 3 (s) + 2 Li + (aq) + 2 F (aq) Sn 2+ (aq) + CO 3 2 (aq) SnCO 3 (s) NOTE: Carbonate was not listed directly in the solubility rules so it is considered insoluble. Laying the Foundation in Chemistry 413

5 14 Making Sense of Chemical Reactions Now that you have mastered balancing chemical equations it is time to focus only on the reacting species. Chemical reactions that occur spontaneously do so as a result of several types of driving forces. Writing the net ionic equation for a reaction often makes it evident which driving force caused the reaction. The most common driving forces for chemical reactions are: formation of a precipitate, formation of a molecular compound such as water, and formation of a gas. PURPOSE In this activity you will write balanced formula equations, balanced total ionic equations and balanced net ionic equations to explain chemical reactions. MATERIALS periodic table solubility rules student white boards (optional) CLASS NOTES Net ionic equations represent only the species that are actually reacting in a chemical reaction. The parts of the equation that are not shown in the net ionic equation are known as the spectator ions. Spectator ions do just that; they spectate as opposed to participate in a chemical reaction. Spectator ions must be present initially in order for the reaction to occur since compounds are neutral; however they are not directly involved in the reaction. The type of equations that you have become familiar with thus far are known as balanced formula equations. In balanced formula equations all species are included. Each compound is represented by its correct chemical formula and coefficients are used to balance the equation so that it obeys the law of conservation of matter. In a total ionic equation, substances that ionize extensively in solution are written as separate ions while all others are written as undissociated molecules. How do you know if a substance will extensively ionize in solution? All strong electrolytes will ionize extensively in solution. Electrolytes are comprised of three classes of compounds strong acids, strong bases, and soluble salts. Using the information that follows you should be able to determine whether or not to ionize a particular substance. 1. Strong Acids: HCl, HBr, HI, H 2 SO 4, HNO 3, and HClO 4 Notice HF is missing from this list, so it is classified as a weak acid. Why? The fluoride atom is very small and as a result it is highly attracted to the hydrogen atom. As a result, it does not dissociate completely in aqueous solution. 414 Laying the Foundation in Chemistry

6 14 2. Strong Bases: Hydroxides of group IA and IIA, but Be and Mg are classified as weak since they do not dissociate completely. This is due to the fact that they are small atoms and as a result are highly attracted to the hydroxide ion. Therefore they do not dissociate completely in aqueous solution and are considered weak bases. Ba(OH) 2, Sr(OH) 2, and Ca(OH) 2 are marginally strong bases since they are not as soluble as IA hydroxides. For these IIA hydroxides, to the little extent that they do dissolve, they dissociate 100%. 3. Soluble Salts: Use the solubility rules presented in Table 1 to determine whether or not a compound containing a metal and non-metal will dissolve in aqueous solution and thus behave as a strong electrolyte. Table 1: Solubility Rules Always Soluble if in a Compound Except With NO 3, Group IA, NH 4 +, C 2 H 3 O 2, ClO 4, ClO 3 No Exceptions Cl, Br, I Pb 2+, Ag +, Hg 2 2+ SO 4 2 Pb 2+, Ag +, Hg 2 2+ Ca 2+, Sr 2+, Ba 2+ If a substance is not addressed by one of the three rules listed in Table 1, assume the substance is insoluble or it is a weak electrolyte and does not ionize in solution. (This won t always be correct, but will cover most of the situations you will encounter.) A few other important points: Gases, pure liquids, and solids are non-electrolytes do not ionize H 2 CO 3 (aq) decomposes into H 2 O(l) and CO 2 (g) NH 4 OH(aq) decomposes into H 2 O(l) and NH 3 (g) If a driving force is absent, no gas forms, no precipitate forms nor does any molecular substance such as water form. If you encounter such a situation, write NO REACTION. Example 1 Solutions of sodium chloride and lead(ii) nitrate are mixed. First, write the balanced formula equation. Balanced formula equation: Write the correct chemical formula for each compound and use coefficients to balance the equation. 2 NaCl(aq) + Pb(NO 3 ) 2 (aq) 2 NaNO 3 (aq) + PbCl 2 (s) Laying the Foundation in Chemistry 415

7 14 Total ionic equation: Determine which substances are strong electrolytes and write them in ionic form. 2 Na + (aq) + 2 Cl (aq) + Pb 2+ (aq) + 2 NO 3 (aq) 2 Na + (aq) + 2 NO 3 (aq) + PbCl 2 (s) Cancel ions that are common to both sides of the equation. These are the spectator ions. 2 Na + (aq) + 2 Cl (aq) + Pb 2+ (aq) + 2 NO 3 (aq) 2 Na + (aq) + 2 NO 3 (aq) + PbCl 2 (s) Balanced net ionic equation: Rewrite the equation, focusing on the reacting species. 2 Cl (aq) + Pb 2+ (aq) PbCl 2 (s) Identify the spectator ions in the equation above: Na + and NO 3 Example 2 Solutions of iron(iii) nitrate and potassium hydroxide are mixed. Balanced formula equation: Total ionic equation: Balanced net ionic equation: Example 3 Magnesium ribbon reacts with hydrochloric acid. Balanced formula equation: Total ionic equation: Balanced net ionic equation: 416 Laying the Foundation in Chemistry

8 14 Example 4 Solutions of acetic acid and lithium bicarbonate are mixed. Balanced formula equation: Total ionic equation: Balanced net ionic equation: Example 5 Solutions of magnesium chloride and calcium nitrate are mixed. Balanced formula equation: Total ionic equation: Balanced net ionic equation: Laying the Foundation in Chemistry 417

9 14 Name Period Making Sense of Chemical Reactions CONCLUSION QUESTIONS Using your own paper, write the balanced formula equation, the balanced total ionic equation and finally the balanced net ionic equation for each of the following chemical reactions. You must write all three balanced equations in order to receive full credit. Be sure to include state symbols for each component and correct charges for ions where appropriate. 1. Solutions of lead(ii) nitrate and lithium chloride are mixed. 2. Copper metal is placed into a solution of silver nitrate. 3. Solid potassium chlorate decomposes upon heating. 4. Solid sodium metal is placed into distilled water. 5. Chlorine gas is bubbled into a solution of magnesium bromide. 6. Methane gas is burned in the presence of oxygen gas. 7. Solutions of silver acetate and barium chloride are mixed. 8. Solutions of sodium bicarbonate and hydrochloric acid are mixed. 9. Solutions of ammonium perchlorate and barium hydroxide are mixed. 10. Solutions of tin(ii) fluoride and lithium carbonate are mixed. 418 Laying the Foundation in Chemistry

10 14 Laying the Foundation in Chemistry 419

TYPES OF CHEMICAL REACTION

TYPES OF CHEMICAL REACTION TYPES OF CHEMICAL REACTION I. METATHESIS REACTIONS (or DOUBLE DISPLACEMENT RXNS) In these reactions the ions of the reactants are exchanged: A + B (aq) + C + D (aq) AD (?) + CB (?) Double Displacement

More information

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure

More information

Chapter 9. Answers to Questions

Chapter 9. Answers to Questions Chapter 9 Answers to Questions 1. Word equation: Silicon Tetrachloride + Water Silicon Dioxide + Hydrogen Chloride Formulas: Next, the chemical formulas are needed. As these are all covalent compounds,

More information

Chemical reactions. Classifications Reactions in solution Ionic equations

Chemical reactions. Classifications Reactions in solution Ionic equations Chemical reactions Classifications Reactions in solution Ionic equations Learning objectives Distinguish between chemical and physical change Write and balance chemical equations Describe concepts of oxidation

More information

What is a chemical reaction?

What is a chemical reaction? Chapter 5 Chemical Reactions and Equations What is a chemical reaction? How do we know a chemical reaction occurs? Writing chemical equations Predicting chemical reactions Representing reactions in aqueous

More information

Chemical Reactions Chapter 8 Assignment & Problem Set

Chemical Reactions Chapter 8 Assignment & Problem Set Chemical Reactions Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Chemical Reactions 2 Study Guide: Things You Must Know Vocabulary (know the

More information

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction Introduction Chapter 5 Chemical Reactions and Equations Chemical reactions occur all around us. How do we make sense of these changes? What patterns can we find? 1 2 Copyright The McGraw-Hill Companies,

More information

Chemical Reactions and Equations. Chapter 8

Chemical Reactions and Equations. Chapter 8 Chemical Reactions and Equations Chapter 8 Describing Chemical Reactions A chemical reaction is the process by which one or more substances are changed into different substances Reactants Products When

More information

Solubility Rules for Ionic Compounds in Water

Solubility Rules for Ionic Compounds in Water The Copper Cycle Introduction Many aspects of our lives involve chemical reactions from the batteries that power our cars and cell phones to the thousands of processes occurring within our bodies. We cannot

More information

Molarity of Ions in Solution

Molarity of Ions in Solution APPENDIX A Molarity of Ions in Solution ften it is necessary to calculate not only the concentration (in molarity) of a compound in aqueous solution but also the concentration of each ion in aqueous solution.

More information

Reactions in Aqueous Solutions. Chapter 4

Reactions in Aqueous Solutions. Chapter 4 Reactions in Aqueous Solutions Chapter 4 Practice Write the balanced molecular and net ionic equations for each of the following reactions: 1) Aqueous acetic acid is neutralized by aqueous barium hydroxide

More information

CHEMICAL REACTIONS. When sodium bicarbonate, e.g. baking soda, is combined with an acid, a gas is produced

CHEMICAL REACTIONS. When sodium bicarbonate, e.g. baking soda, is combined with an acid, a gas is produced CHEMICAL REACTIONS OBJECTIVES 1. To study reactions between ions in aqueous solutions 2. To observe exothermic and endothermic reactions 3. To study oxidation-reduction reactions 4. To practice balancing

More information

What physical evidence do we have that sodium hydroxide dissociates into ions when it dissolves in water? NaOH(s) Na + + OH -

What physical evidence do we have that sodium hydroxide dissociates into ions when it dissolves in water? NaOH(s) Na + + OH - Chemistry Date Period Name CW double replacement reactions 030812.doc Double Replacement Reactions Double replacement reactions are some of the most common reactions that are performed in the laboratory.

More information

Experiment 1 Chemical Reactions and Net Ionic Equations

Experiment 1 Chemical Reactions and Net Ionic Equations Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical

More information

Reactions in Aqueous Solutions

Reactions in Aqueous Solutions Chem 101 Reactions in Aqueous Solutions Lectures 15 and 16 Predicting Whether a Reaction Will Occur Forces that drive a reaction Formation of a solid Formation of water Transfer of electrons Formation

More information

Potassium + Chlorine. K(s) + Cl 2 (g) 2 KCl(s)

Potassium + Chlorine. K(s) + Cl 2 (g) 2 KCl(s) Types of Reactions Consider for a moment the number of possible chemical reactions. Because there are millions of chemical compounds, it is logical to expect that there are millions of possible chemical

More information

Experiment 9 - Double Displacement Reactions

Experiment 9 - Double Displacement Reactions Experiment 9 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are

More information

Tutorial 5 NET IONIC EQUATIONS

Tutorial 5 NET IONIC EQUATIONS T-33 Tutorial 5 NET IONIC EQUATIONS The efficiency and extent of a chemical reaction is very much dependent upon the physical state (solid, liquid, gas, or solution) of reactants and products. Not surprisingly,

More information

NET IONIC REACTIONS in AQUEOUS SOLUTIONS AB + CD AD + CB

NET IONIC REACTIONS in AQUEOUS SOLUTIONS AB + CD AD + CB NET IONIC REACTIONS in AQUEOUS SOLUTIONS Double replacements are among the most common of the simple chemical reactions. Consider the hypothetical reaction: AB + CD AD + CB where AB exists as A + and B

More information

Ch. 9 Chemical Reactions

Ch. 9 Chemical Reactions Ch. 9 Chemical Reactions I. Intro to Reactions (p. 282 285) I II III IV V Chemical Reaction Chemical change Atoms of one or more substances (reactants) are rearranged into new substances (products) Signs

More information

AP Review: Predicting Reactions (Question 4) Answers

AP Review: Predicting Reactions (Question 4) Answers AP Review: Predicting Reactions (Question 4) Answers For each of the following three reactions, in part (i) write a balanced equation for the reaction and in part (ii) answer the question about the reaction.

More information

Lecture 6. Classes of Chemical Reactions

Lecture 6. Classes of Chemical Reactions Lecture 6 Classes of Chemical Reactions Lecture 6 Outline 6.1 The Role of Water as a Solvent 6.2 Precipitation Reactions 6.3 Acid-Base Reactions 1 Electron distribution in molecules of H 2 and H 2 O The

More information

NET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is:

NET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NET IONIC EQUATIONS A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NaCl + AgNO 3 AgCl + NaNO 3 In this case, the simple formulas of the various reactants

More information

CHM1 Review for Exam 9

CHM1 Review for Exam 9 Topics 1. Reaction Types a. Combustion b. Synthesis c. Decomposition d. Single replacement i. Metal activity series ii. Nonmetal activity series e. Double replacement i. Precipitates and solubility rules

More information

Identify the letter of the choice that best completes the statement or answers the question.

Identify the letter of the choice that best completes the statement or answers the question. Chemistry Test - Chapter 10 Chemical Equations Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. When balancing a chemical equation, insert

More information

Experiment 8 - Double Displacement Reactions

Experiment 8 - Double Displacement Reactions Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are

More information

stoichiometry = the numerical relationships between chemical amounts in a reaction.

stoichiometry = the numerical relationships between chemical amounts in a reaction. 1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse

More information

EXPERIMENT 5: CHEMICAL REACTIONS AND EQUATIONS

EXPERIMENT 5: CHEMICAL REACTIONS AND EQUATIONS PURPOSE EXPERIMENT 5: CHEMICAL REACTIONS AND EQUATIONS To perform and observe simple chemical reactions. To identify the products of chemical reactions and write balanced equations for those reactions.

More information

6 Reactions in Aqueous Solutions

6 Reactions in Aqueous Solutions 6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface

More information

Laboratory 6: Double Displacement Reactions

Laboratory 6: Double Displacement Reactions Introduction Double displacement reactions are among the most common of the simple chemical reactions to study and understand. We will explore the driving forces behind the chemical reactions, and use

More information

Types of Reactions. CK12 Editor. Say Thanks to the Authors Click (No sign in required)

Types of Reactions. CK12 Editor. Say Thanks to the Authors Click  (No sign in required) Types of Reactions CK12 Editor Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) To access a customizable version of this book, as well as other interactive content, visit

More information

10/21/2013. Chemical REACTIONS you should know. Chemical Reactions. 1 st Write Reaction

10/21/2013. Chemical REACTIONS you should know. Chemical Reactions. 1 st Write Reaction Chapter 3: Chemical Stoichiometry Chemical Equations (Write, Balance, Interpret) Reactions You Should Know Formula Weights (Must know chemical formula Avogadro s number and the Mole Limiting Reactants

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written

More information

6/27/2014. Periodic Table of the ELEMENTS. Chemical REACTIONS you should know. Brief Review for 1311 Honors Exam 2

6/27/2014. Periodic Table of the ELEMENTS. Chemical REACTIONS you should know. Brief Review for 1311 Honors Exam 2 Brief Review for 3 Honors Exam 2 Chapter 2: Periodic Table I. Metals. Representative Metals Alkali Metals Group Alkaline Earth Metals. Group 2 2. Transition Metals II. Metalloids Chapter 3: All Chapter

More information

IONIC REACTIONS in AQUEOUS SOLUTIONS: NET IONIC EQUATIONS AB + CD AD + CB

IONIC REACTIONS in AQUEOUS SOLUTIONS: NET IONIC EQUATIONS AB + CD AD + CB 35 IONIC REACTIONS in AQUEOUS SOLUTIONS: NET IONIC EQUATIONS Double replacements are among the most common of the simple chemical reactions. Consider the hypothetical reaction: AB + CD AD + CB where AB

More information

Balancing Chemical Equations Worksheet

Balancing Chemical Equations Worksheet Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.

More information

Chapter 4: Reactions in Aqueous Solution (Sections )

Chapter 4: Reactions in Aqueous Solution (Sections ) Chapter 4: Reactions in Aqueous Solution (Sections 4.1-4.12) Chapter Goals Be able to: Classify substances as electrolytes or nonelectrolytes. Write molecular, ionic, and net ionic equations for precipitation,

More information

Goals. 1. How are chemical reactions written?

Goals. 1. How are chemical reactions written? Goals 1. How are chemical reactions written? Given the identities of reactants and products, be able to write a balanced chemical equation or net ionic equation. 2. How are chemical reactions of ionic

More information

Classifying Chemical Reactions Chapter 7

Classifying Chemical Reactions Chapter 7 Classifying Chemical Reactions Chapter 7 Classifying Chemical Reactions Chemical reactions can be divided into five categories: I. Combination Reactions II. Decomposition Reactions III. Single-Replacement

More information

EXPERIMENT A5: TYPES OF REACTIONS. Learning Outcomes. Introduction. Upon completion of this lab, the student will be able to:

EXPERIMENT A5: TYPES OF REACTIONS. Learning Outcomes. Introduction. Upon completion of this lab, the student will be able to: 1 Learning Outcomes EXPERIMENT A5: TYPES OF REACTIONS Upon completion of this lab, the student will be able to: 1) Examine different types of chemical reactions. 2) Express chemical equations in molecular,

More information

Chapter 8: Chemical Equations and Reactions

Chapter 8: Chemical Equations and Reactions Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical

More information

Writing and Balancing Chemical Equations

Writing and Balancing Chemical Equations Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often

More information

Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry

Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry AP Chemistry A. Allan Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen's electronegativity is high (3.5) and hydrogen's

More information

Solution. Practice Exercise. Concept Exercise

Solution. Practice Exercise. Concept Exercise Example Exercise 8.1 Evidence for a Reaction Which of the following is experimental evidence for a chemical reaction? (a) Pouring vinegar on baking soda gives foamy bubbles. (b) Mixing two solutions produces

More information

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions. Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration

More information

EXPERIMENT 9: Double Replacement Reactions

EXPERIMENT 9: Double Replacement Reactions EXPERIMENT 9: Double Replacement Reactions PURPOSE a) To identify the ions present in various aqueous solutions. b) To systematically combine solutions and identify the reactions that form precipitates

More information

CHM 130LL: Double Replacement Reactions

CHM 130LL: Double Replacement Reactions CHM 130LL: Double Replacement Reactions One of the main purposes of chemistry is to transform one set of chemicals (the reactants) into another set of chemicals (the products) via a chemical reaction:

More information

Chapter 8 Review and Study Guide

Chapter 8 Review and Study Guide Name: Class: Date: Chapter 8 Review and Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Knowledge about what products are produced in a chemical

More information

Chapter 5 Chemical Reactions and Equations

Chapter 5 Chemical Reactions and Equations Chapter 5 Chemical Reactions and Equations 5.1 (a) single-displacement reaction; (b) anhydrous; (c) molecular equation; (d) decomposition reaction; (e) balanced equation; (f) reactant; (g) spectator ion;

More information

Chapter 7: Chemical Reactions

Chapter 7: Chemical Reactions Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that

More information

USEFUL DEFINITIONS. A substance which cannot be split into anything simpler by chemical means.

USEFUL DEFINITIONS. A substance which cannot be split into anything simpler by chemical means. Formulae and equations 1 USEFUL DEFINITIONS Element Atom A substance which cannot be split into anything simpler by chemical means. The smallest part of an element that can take part in a chemical reaction.

More information

USEFUL DEFINITIONS. A substance which cannot be split into anything simpler by chemical means.

USEFUL DEFINITIONS. A substance which cannot be split into anything simpler by chemical means. 1 USEFUL DEFINITIONS Element Atom Molecule A substance which cannot be split into anything simpler by chemical means. The smallest part of an element that can take part in a chemical reaction. The smallest

More information

Reactions in solution. A subset of chemical reactions

Reactions in solution. A subset of chemical reactions Reactions in solution A subset of chemical reactions Learning objectives Define solution and its components Distinguish among strong, weak and non-electrolyte Identify strong acids and strong bases Apply

More information

Chapter 7 Chemical Reactions

Chapter 7 Chemical Reactions Chemistry 25 Chapter 7 Chemical Reactions Chemical Reactions Reactions involve chemical changes in matter resulting in new substances. Reactions involve rearrangement and exchange of atoms to produce new

More information

Steps for balancing a chemical equation

Steps for balancing a chemical equation The Chemical Equation: A Chemical Recipe Dr. Gergens - SD Mesa College A. Learn the meaning of these arrows. B. The chemical equation is the shorthand notation for a chemical reaction. A chemical equation

More information

Skeleton Equations equations describing a reaction using formulas. HCl(aq) + Zn(s) ZnCl 2 (aq) + H 2 (g)

Skeleton Equations equations describing a reaction using formulas. HCl(aq) + Zn(s) ZnCl 2 (aq) + H 2 (g) 10.1 Reactions and Equations Evidence of Chemical Reactions Chemical Reaction a process in which one or more substances are converted into new substances with different physical and chemical properties.

More information

Name Date Class CHEMICAL REACTIONS. SECTION 8.1 DESCRIBING CHEMICAL CHANGE (pages )

Name Date Class CHEMICAL REACTIONS. SECTION 8.1 DESCRIBING CHEMICAL CHANGE (pages ) 8 CHEMICAL REACTIONS SECTION 8.1 DESCRIBING CHEMICAL CHANGE (pages 203 211) This section explains how to write equations describing chemical reactions using appropriate symbols. It also describes how to

More information

Solubility Rules and Net Ionic Equations

Solubility Rules and Net Ionic Equations Solubility Rules and Net Ionic Equations Why? Solubility of a salt depends upon the type of ions in the salt. Some salts are soluble in water and others are not. When two soluble salts are mixed together

More information

Aqueous Ions and Reactions

Aqueous Ions and Reactions Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for

More information

Dr. Taylor Chapter 8 and 9 Homework Chem 111 Spring 2012

Dr. Taylor Chapter 8 and 9 Homework Chem 111 Spring 2012 Dr. Taylor Chapter 8 and 9 Homework Chem 111 Spring 2012 9.1 (12, 103 and 107) Electrolytes 9.2 (15, 21, 23, 25, 93 and 97) 9.3 (27, 31, 33, 35, 101, 105 and 111) 9.4 (45,47,49 and 51) 8.2 (17, 19, 21

More information

Do Now CHEMICAL REACTIONS. Chemical Reaction. chemical reaction. Chemical Equations. Evidence

Do Now CHEMICAL REACTIONS. Chemical Reaction. chemical reaction. Chemical Equations. Evidence Do Now CHEMICAL REACTIONS What are some signs that a chemical change may have taken place? Where are the reactants and products in a reaction? What do they represent? Describe the law of conservation of

More information

Chapter 04: Reactions in Aqueous Solution. Chemistry, 4 th Edition McMurry/Fay. Types of Chemical Reactions 01. Types of Chemical Reactions 02

Chapter 04: Reactions in Aqueous Solution. Chemistry, 4 th Edition McMurry/Fay. Types of Chemical Reactions 01. Types of Chemical Reactions 02 4 Chapter Reactions in Aqueous Solution Chemistry, 4 th Edition McMurry/Fay Dr. Paul Charlesworth Michigan Technological University Types of Chemical Reactions 01 Precipitation Reactions: A process in

More information

Balancing Equations Notes

Balancing Equations Notes Unit 7 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with

More information

Single and Double Displacement Reactions

Single and Double Displacement Reactions Single and Double Displacement Reactions Objectives To perform and observe a variety of single and double displacement reactions To record observations in detail To identify the products formed in each

More information

Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent

Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Water a polar solvent: dissolves most ionic compounds as well as many molecular compounds Aqueous solution:

More information

Chapter 4: Solution Stoichiometry Cont. Aqueous Solutions

Chapter 4: Solution Stoichiometry Cont. Aqueous Solutions Chapter 4: Solution Stoichiometry Cont. 1 Aqueous Solutions Molarity (dilution calculations, solution stoichiometry); Solubility and Solubility Rules Molecular, Ionic and Net Ionic Equations Precipitation

More information

H 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation.

H 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation. CEMICAL REACTIONS 1 ydrogen + Oxygen Water 2 + O 2 2 O reactants product(s) reactant substance before chemical change product substance after chemical change Conservation of Mass During a chemical reaction,

More information

Inorganic Chemistry Writing (Net Ionic) Equations for Various Reactions

Inorganic Chemistry Writing (Net Ionic) Equations for Various Reactions -1- Inorganic Chemistry Writing (Net Ionic) Equations for Various Reactions On the AP examination you will encounter a question in which you will be required to write net ionic equations for various reactions.

More information

11.2 Types of Chemical Reactions> Chapter 11 Chemical Reactions Types of Chemical Reactions Describing Chemical Reactions

11.2 Types of Chemical Reactions> Chapter 11 Chemical Reactions Types of Chemical Reactions Describing Chemical Reactions Chapter 11 Chemical 11.1 Describing Chemical 11.2 Types of Chemical 11.3 in Aqueous Solution 1 CHEMISTRY & YOU What happens to the wax when you burn a candle? When you burn a candle, a chemical reaction

More information

AP Chem Unit 1 Assignment 3 Chemical Equations

AP Chem Unit 1 Assignment 3 Chemical Equations Symbols used in chemical equations: Symbol Meaning + used to separate one reactant or product from another used to separate the reactants from the products - it is pronounced "yields" or "produces" when

More information

CP Chapter 11 Notes Reactions and Equations

CP Chapter 11 Notes Reactions and Equations CP Chapter 11 Notes Reactions and Equations Evidence of Chemical Reactions How can you tell a reaction has taken place? Temperature change Color change Gas/bubbles Appearance of a (precipitate) Chemical

More information

Chapter 4: Phenomena. Electrolytes. Electrolytes. Molarity & Dilutions. Electrolytes. Chapter 4 Types of Chemical Reactions and Solution Stoichiometry

Chapter 4: Phenomena. Electrolytes. Electrolytes. Molarity & Dilutions. Electrolytes. Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Chapter 4: Phenomena Phenomena: Many different reactions are known to occur. Scientists wondered if these reaction could be separated into groups based on their properties. Look at the reactions below

More information

Part I: Parts and Meaning of a Chemical Equation:

Part I: Parts and Meaning of a Chemical Equation: Chemical Equations Name: Period: Date: Part I: Parts and Meaning of a Chemical Equation: 1) = process by which one or more substances are changed into one or more different substances (atoms are rearranged)

More information

Reactions. Balancing Chemical Equations uses Law of conservation of mass: matter cannot be lost in any chemical reaction

Reactions. Balancing Chemical Equations uses Law of conservation of mass: matter cannot be lost in any chemical reaction Reactions Chapter 8 Combustion Decomposition Combination Chapter 9 Aqueous Reactions Exchange reactions (Metathesis) Formation of a precipitate Formation of a gas Formation of a week or nonelectrolyte

More information

Easy Examples: Hd 10 + Bu 8 HdBu. Introduction. (l) or (aq)? Introduction. Symbols. Yields or Produces. Balancing. (l) or (aq)?

Easy Examples: Hd 10 + Bu 8 HdBu. Introduction. (l) or (aq)? Introduction. Symbols. Yields or Produces. Balancing. (l) or (aq)? Chemical Equations Chemical Equations Like a recipe: Introduction Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) Symbols (s) (l) (aq) (g) Introduction Yields or Produces solid liquid aqueous gas (l) or

More information

Chapter 4 Chemical Reactions

Chapter 4 Chemical Reactions Chapter 4 Chemical Reactions I) Ions in Aqueous Solution many reactions take place in water form ions in solution aq solution = solute + solvent solute: substance being dissolved and present in lesser

More information

Reactions in Aqueous Solution

Reactions in Aqueous Solution CHAPTER 7 1. Water is the most universal of all liquids. Water has a relatively large heat capacity and a relatively large liquid range, which means it can absorb the heat liberated by many reactions while

More information

Bell Task 11/15. Using Table F determine if the following substances are soluble or insoluble.

Bell Task 11/15. Using Table F determine if the following substances are soluble or insoluble. Using Table F determine if the following substances are soluble or insoluble. Silver Iodide Calcium Chromate Barium Hydroxide Sodium Chlorate Strontium Sulfate Lithium Carbonate Bell Task 11/15 Oct 18

More information

Stoichiometry. Stoichiometry Which of the following forms a compound having the formula KXO 4? (A) F (B) S (C) Mg (D) Ar (E) Mn

Stoichiometry. Stoichiometry Which of the following forms a compound having the formula KXO 4? (A) F (B) S (C) Mg (D) Ar (E) Mn The Advanced Placement Examination in Chemistry Part I Multiple Choice Questions Part II - Free Response Questions Selected Questions from 1970 to 2010 Stoichiometry Part I 1984 2. Which of the following

More information

Writing, Balancing and Predicting Products of Chemical Reactions.

Writing, Balancing and Predicting Products of Chemical Reactions. Writing, Balancing and Predicting Products of Chemical Reactions. A chemical equation is a concise shorthand expression which represents the relative amount of reactants and products involved in a chemical

More information

Santa Monica College Chemistry 11

Santa Monica College Chemistry 11 Types of Reactions Objectives The objectives of this laboratory are as follows: To perform and observe the results of a variety of chemical reactions. To become familiar with the observable signs of chemical

More information

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11 SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436

More information

1. Balancing a chemical equation so that it obeys the law of conservation of matter requires:

1. Balancing a chemical equation so that it obeys the law of conservation of matter requires: General Chemistry I Exam 2 Review 1 1. Balancing a chemical equation so that it obeys the law of conservation of matter requires: a. Adjusting the coefficients in front of the d. Changing the formulas

More information

Types of Chemical Reactions

Types of Chemical Reactions Why? Types of Chemical Reactions Do atoms rearrange in predictable patterns during chemical reactions? Recognizing patterns allows us to predict future behavior. Weather experts use patterns to predict

More information

Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ

Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical

More information

AN INVESTIGATION OF CHEMICAL REACTIONS II PART I: RELATIVE REACTIVITIES PRE-LAB QUERIES

AN INVESTIGATION OF CHEMICAL REACTIONS II PART I: RELATIVE REACTIVITIES PRE-LAB QUERIES NAME PARTNER(S) SECTION DATE AN INVESTIGATION OF CHEMICAL REACTIONS II This activity explores the reactivity of a number of metals using single replacement reactions and investigates the role of solubility

More information

Reaction Type & Balancing Review Questions

Reaction Type & Balancing Review Questions Reaction Type & Balancing Review Questions There are 20 questions sets in this review. The corresponding answers can be found in the second half of this document. 1. Match the term with its proper description.

More information

Observing, Writing, and Predicting Chemical Reactions Name:

Observing, Writing, and Predicting Chemical Reactions Name: Chem 110 Lab Clark College Observing, Writing, and Predicting Chemical Reactions Name: Partner s Name: Introduction As someone taking a chemistry class, you will need to understand chemical formulas, chemical

More information

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. 1 7 8 12

More information

NAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide

NAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide NAMING QUIZ 3 - Part A Name: Write the formulas for the following compounds: 1. Zinc (II) Nitrate 2. Manganese (IV) sulfide 3. Barium permanganate 4. Sulfuric acid 5. Silver (I) carbonate 6. Aluminum acetate

More information

EXPERIMENT 10: Electrical Conductivity Chem 111

EXPERIMENT 10: Electrical Conductivity Chem 111 EXPERIMENT 10: Electrical Conductivity Chem 111 INTRODUCTION A. Electrical Conductivity A substance can conduct an electrical current if it is made of positively and negatively charged particles that are

More information

11.3 Reactions in Aqueous Essential Understanding Reactions that occur in aqueous solutions are double-replacement

11.3 Reactions in Aqueous Essential Understanding Reactions that occur in aqueous solutions are double-replacement 11.3 Reactions in Aqueous Solution Essential Understanding Reactions that occur in aqueous solutions are double-replacement reactions. The products are precipitates, water, or gases. Lesson Summary Net

More information

Name Class Date. Chapter: Chemical Equations and Reactions

Name Class Date. Chapter: Chemical Equations and Reactions Assessment Chapter Test B Chapter: Chemical Equations and Reactions PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question

More information

Chemistry. Zumdahl, 7th edition

Chemistry. Zumdahl, 7th edition Chemistry Zumdahl, 7th edition CH4 Types of Chemical Reactions and Solution Stoichiometry Yellow lead(ii) iodide is produced when lead(ii) nitrate is mixed with potassium iodide. P.126 Contents 4.1 Water,

More information

13 Chemical Reactions

13 Chemical Reactions www.ck12.org 275 CHAPTER 13 Chemical Reactions CHAPTER OUTLINE 13.1 CHEMICAL REACTIONS AND EQUATIONS 13.2 BALANCING CHEMICAL EQUATIONS 13.3 TYPES OF REACTIONS CHAPTER 13. CHEMICAL REACTIONS 276 www.ck12.org

More information

Chemical Equations. What is a chemical equation? How do you balance a chemical equation? How do you identify the type of chemical equation?

Chemical Equations. What is a chemical equation? How do you balance a chemical equation? How do you identify the type of chemical equation? Chemical Equations What is a chemical equation? How do you balance a chemical equation? How do you identify the type of chemical equation? Chemical Equations A chemical equation is written as an expression

More information

EXPERIMENT #12 DOUBLE-REPLACEMENT REACTIONS

EXPERIMENT #12 DOUBLE-REPLACEMENT REACTIONS EXPERIMENT #12 DOUBLE-REPLACEMENT REACTIONS Purpose: 1. To study the most common type of double-replacement reactions. Principles: In double-replacement reactions, two compounds are involved in a reaction,

More information

Chemistry AS90171 Describe chemical reactions

Chemistry AS90171 Describe chemical reactions Chemistry AS90171 Describe chemical reactions This achievement standard involves the description of chemical reactions, including the carrying out of calculations. Achievement Merit Excellence Describe

More information

Chemistry Themed. Types of Reactions

Chemistry Themed. Types of Reactions Chemistry Themed Types of Reactions 1 2 Chemistry in the Community-2015-2016 Types of Reactions Date In-Class Assignment Homework T 10/20 TEST on Reactivity of Metals and Redox None W 10/21 Late Start

More information

Outer shell contain few electrons (3or less) Outer shell contains 4 or more electrons

Outer shell contain few electrons (3or less) Outer shell contains 4 or more electrons Chapter 4: Chemical Reactions Elements can be characterized as metals, non-metals and metalloids. The periodic table is arranged according to properties of elements. Mendeleev and Meyer independently arranged

More information