Types of Chemical Reactions (rxns.)
|
|
- Myles Nelson
- 5 years ago
- Views:
Transcription
1 Types of Chemical Reactions (rxns.) Introduction Chemical reactions occur when bonds (between the electrons of atoms) are formed or broken Chemical reactions involve changes in the chemical composition of matter (the making of new materials with new properties) energy changes Bond breaking absorbs Energy (endothermic process) Bond making releases Energy (exothermic process) Symbols represent elements Formulas describe compounds Chemical equations describe a chemical reaction 1
2 Types of Reactions Reactions are classified by their products. There are five main types of chemical reactions we will talk about: 1. Synthesis reactions 2. Decomposition reactions 3. Single replacement reactions 4. Double replacement reactions 5. Combustion reactions You need to be able to identify the type of reaction and predict the product(s) Steps to Writing Reactions Some steps for doing reactions: 1. Identify the type of reaction 2. Predict the product(s) using the type of reaction as a model 3. Balance it Don t forget about the diatomic elements! (BrINClHOF) For example, Oxygen is O 2 as an element. In a compound, it can t be a diatomic element because it s not an element anymore, it s a compound! 2
3 Synthesis Reactions Synthesis (meaning to make) are Also called Direct combination or combination reactions Addition reactions typified by their single product. If you have a reaction in which at least 2 elements or compounds are reacted and produce a single product, the reaction is a synthesis reaction. Synthesis Reactions reactant + reactant à 1 product Basically: A + B à AB Example: 2H 2 + O 2 à 2H 2 O Example: C + O 2 à CO 2 Note: Single Product! This is your clue that this is a synthesis or combination reaction. 3
4 Synthesis Reactions Here is another example of a synthesis reaction Examples of Synthesis Reactions 2Na + S Na 2 S This one is an example of two elements in atomic form (Na and S) combining to form a compound (sodium sulfide). 2H 2 + O 2 2H 2 O In this example, A and B are two elements in molecular form (hydrogen and oxygen molecules), and the product is water, which is simply the chemical combination of hydrogen and oxygen. 4
5 Examples of Synthesis Reactions 4Fe + 3O 2 2Fe 2 O 3 In this example, substance A is an element in atomic form (Fe), and substance B is an element in molecular form (O 2 ). The result is a direct chemical combination of the two elements (FeO, iron oxide, which is rust ). CuO + H 2 O Cu(OH) 2 This is an example where both substances going into the reaction are molecules. The result is what you get when you add all of the atoms in the reaction together. Practice Predict the products. Write and balance the following synthesis reaction equations. Sodium metal reacts with chlorine gas Na (s) + Cl 2(g) à Solid Magnesium reacts with fluorine gas Mg (s) + F 2(g) à Aluminum metal reacts with fluorine gas Al (s) + F 2(g) à 5
6 Decomposition Reactions Decomposition reactions are really just the opposite of a synthesis reaction. Remember, if you can make a substance, you should be able to break it back apart into its components. A good way to remember decomposition reactions to to remember what happens when something decomposes. It falls apart! Decomposition Reactions Decomposition reactions occur when a compound breaks up into the elements or in a few to simpler compounds 1 Reactant à Product + Product Basically: AB à A + B Example: 2 H 2 O à 2H 2 + O 2 Example: 2 HgO à 2Hg + O 2 Note: Single Reactant! The single reactant is your clue that this is a decomposition reaction. 6
7 Decomposition Reactions Another view of a decomposition reaction: Decomposition Exceptions Carbonates and chlorates are special case decomposition reactions that do not go to the elements. Carbonates (CO 3 2- ) decompose to carbon dioxide and a metal oxide Example: CaCO 3 à CO 2 + CaO Chlorates (ClO 3- ) decompose to oxygen gas and a metal chloride Example: 2 Al(ClO 3 ) 3 à 2 AlCl O 2 There are other special cases, but we will not explore those in this class 7
8 Practice Predict the products. Then, write and balance the following decomposition reaction equations: Solid Lead (IV) oxide decomposes PbO 2(s) à Aluminum nitride decomposes AlN (s) à Practice Identify the type of reaction for each of the following synthesis or decomposition reactions, and write the balanced equation: N 2 (s) + O 2(g) à BaCO 3(s) à Co (s) + S (s) à NH 3(g) + H 2 CO 3(aq) à NI 3(s) à 8
9 Single Replacement Reactions Single replacement reactions occur when one chemical takes the place of another in a reaction. In the typical single replacement reaction, an element trades places with one of the ions in a compound. Single Replacement Reactions Single Replacement Reactions: A metal can replace a metal (+) OR a nonmetal can replace a nonmetal (-). element + compoundà product + product A + BC à AC + B (if A is a metal) OR A + BC à BA + C (if A is a nonmetal) (remember the cation always goes first!) When H 2 O splits into ions, it splits into H + and OH - (not H+ and O -2!!) 9
10 Single Replacement Reactions Another view: The Activity Series Not all single replacement reactions will occur. This depends upon the location of the elements present in the activity series Elements above MAY replace elements below; elements below MAY NOT replace elements above them on the series 10
11 You will be given a copy of this!!!! Single Replacement Reactions Write and balance the following single replacement reaction equation: Zinc metal reacts with aqueous hydrochloric acid Zn (s) + 2 HCl (aq) à ZnCl 2 + H 2(g) Note: Zinc replaces the hydrogen ion in the reaction [If ZnCl 2 + H 2(g) à Zn (s) + HCl (aq) the reaction WOULD NOT OCCUR because Hydrogen is below zinc on the activity series] 11
12 Single Replacement Reactions Sodium chloride solid reacts with fluorine gas 2 NaCl (s) + F 2(g) à 2 NaF (s) + Cl 2(g) Note that fluorine replaces chlorine in the compound Aluminum metal reacts with aqueous copper (II) nitrate Al (s) + Cu(NO 3 ) 2(aq) à Double Replacement Reac/ons Double replacement reac/ons are iden/fied by two ions trading places and forming new compounds. 12
13 Double Replacement Reactions Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound two ions trade places and forming new compounds. Compound + compound à product + product AB + CD à AD + CB Notice that one ion from compound AB replaces one ion from compound CD. Double Replacement Reactions Think about it like foil ing in algebra, first and last ions go together + inside ions go together Example: AgNO 3(aq) + NaCl (aq) à AgCl (s) + NaNO 3(aq) Another example: K 2 SO 4(aq) + Ba(NO 3 ) 2(aq) à 2KNO 3(aq) + BaSO 4(s) 13
14 Solubility For a double replacement reaction to have occurred, a solid (precipitate) MUST be formed There are rules to determine which of the materials formed is the solid If no solid is formed, there is said to be no reaction. Figure 8.4: The forming of solid AgCl. 14
15 Solubility Tables Solubility tables help determine which materials are soluble in water and which are not In general, Solubility Rules can be summarized as follows 1. All compounds containing alkali metal cations and the ammonium ion are soluble. 2. All compounds containing NO 3-, ClO 4-, ClO 3-, and C 2 H 3 O 2 - anions are soluble. 3. All chlorides, bromides, and iodides are soluble except those containing Ag +, Pb 2+, or Hg All sulfates are soluble except those containing Hg 2 2+, Pb 2+, Sr 2+, Ca 2+, or Ba All hydroxides are insoluble except compounds of the alkali metals, Ca 2+, Sr 2+, and Ba All compounds containing PO 4 3-, S 2-, CO 3 2-, and SO 3 2- ions are insoluble except those that also contain alkali metals or NH 4+. You will be given a copy of this!!!! Practice Predict the products. Balance the equation 1. HCl (aq) + AgNO 3(aq) à 2. Pb(NO 3 ) 2(aq) + BaCl 2(aq) à 3. FeCl 3(aq) + 3NaOH (aq) à 4. H 2 SO 4(aq) + 2NaOH (aq) à 15
16 Combustion Reactions Combustion reactions are the ones that burn (or explode!). There are two types of combustion reactions complete or incomplete reactions. These reactions are identified by their products. They either produce carbon monoxide and water or carbon dioxide and water. Complete Combustion Reactions These reactions burn efficiently which means they produce carbon dioxide and water. These reactions typically burn cleanly and leave very little residue behind. 16
17 Combustion Reactions Combustion reactions occur when a hydrocarbon reacts with oxygen gas. This is also called burning!!! In order to burn something you need the 3 things in the fire triangle : 1) A Fuel (hydrocarbon) 2) Oxygen to burn it with 3) Something to ignite the reaction (spark) Combustion Reactions In general: C x H y + O 2 à CO 2 + H 2 O Products in combustion are ALWAYS carbon dioxide and water. (although incomplete burning does cause some byproducts like carbon monoxide) Combustion is used to heat homes and run automobiles (octane, as in gasoline, is C 8 H 18 ) 17
18 Complete Combustion Reactions CH 4 + O 2 CO 2 + H 2 O They may also be written: O 2 CH 4 CO 2 + H 2 O With O 2 written above the arrow Clues: CO 2 (carbon dioxide) in the product along with water Combustion Example C 5 H O 2 à 5 CO H 2 O Write the products and balance the following combustion reaction: C 10 H 22 + O 2 à 18
19 Incomplete Combustion Reactions Incomplete combustion reactions occur when something does not burn efficiently. This can cause a lot of harm if the gases produced cannot escape. Carbon monoxide,an odorless and colorless gas, is dangerous. People poisoned by this gas usually become sleepy and can die due to exposure. Incomplete Combustion Reactions CH 4 + O 2 CO + H 2 O + CO 2 These reactions may also be written by: O 2 CH 4 CO + H 2 O + CO 2 Again, the O 2 is usually written over the arrow. Clue: CO (Carbon monoxide as a product.) 19
20 Combustion Reactions Edgar Allen Poe s drooping eyes and mouth are potential signs of CO poisoning. Mixed Practice State the type, predict the products, and balance the following reactions: 1. BaCl 2 + H 2 SO 4 à 2. C 6 H 12 + O 2 à 3. Zn + CuSO 4 à 4. Cs + Br 2 à 5. FeCO 3 à 20
21 Predicting Products of Reactions Completing reactions requires knowledge of the different reaction types (sometimes called mechanisms). You must first identify the reaction type by the reactants. The only type of reaction that cannot be predicted this way is the combustion reaction since the products are very similar. First Step: Identify reaction type Example: Al + O 2 Clue: 2 elements Synthesis or combination reaction 21
22 Second Step: Write the net ionic equation for the reactants Al + O 2 becomes Al 3+ + O 2- Step 3 Using clues, complete reaction taking care to write each formula correctly by checking charges and criss-crossing if necessary. Al + O 2 Al 3+ O 2- Al + O 2 Al 2 O 3 22
23 Predicting Products of Reactions (cont.) For Single Replacement reactions, check activity series to make sure the reaction goes. Once you write the molecular equation, you should check for reactants and products that are soluble or insoluble. (Double Replacement only) Reactions in Aqueous Solutions a.k.a. Net Ionic Equations Molecular Equations: shows complete formulas for reactants and products Does not show what happens on the molecular level Total (or Complete) Ionic Equations: All substances that are strong electrolytes (are soluble and dissociate) are written as their ions. Some ions participate in the reaction Some ions do NOT participate in the reaction-called spectator ions. Net Ionic Equations: show only the ions that participate in the reaction 23
24 Writing Total Ionic Equations Once you write the molecular equation (synthesis, decomposition, etc.), you should check for reactants and products that are soluble or insoluble. We usually assume the reaction is in water We can use a solubility table to tell us what compounds dissolve in water. If the compound is soluble (does dissolve in water), then splits the compound into its component ions If the compound is insoluble (does NOT dissolve in water), then it remains as a compound Writing Total Ionic Equations Molecular Equation: K 2 CrO 4 + Pb(NO 3 ) 2 à PbCrO KNO 3 Soluble Soluble Insoluble Soluble Total Ionic Equation: 2 K + + CrO Pb NO 3 - à PbCrO 4 (s) + 2 K NO 3-24
25 Net Ionic Equations These are the same as total ionic equations, but you should cancel out ions that appear on BOTH sides of the equation Total Ionic Equation: 2 K + + CrO Pb NO 3 - à PbCrO 4 (s) + 2 K NO 3 - (Spectator ions) Net Ionic Equation: CrO Pb +2 à PbCrO 4 (s) Net Ionic Equations Try this one! Write the molecular, total ionic, and net ionic equations for this reaction: Silver nitrate reacts with Lead (II) Chloride in hot water. AgNO 3 + PbCl 2 à Molecular: 2 AgNO 3 + PbCl 2 à 2 AgCl + Pb(NO 3 ) 2 Total Ionic: 2 Ag NO Pb Cl - à 2 AgCl (s) + Pb NO 3 - Net Ionic: 2Ag + + 2Cl - à 2AgCl (s) 25
26 Acid-Base Reactions Acid: produces hydrogen ions (H + ) in solution (Arrhenius) proton donor (Lewis) Base: produces hydroxide ions (OH - ) in solution (Arrhenius) proton acceptor (Lewis) The reaction ALWAYS forms water and an ionic compound (mostly aqueous, known as a salt). The actual definition of a salt is the ionic product of an acid-base neutralization reaction) Acid-Base Neutralization Chemically the reaction looks like this: Acid + Base Salt + Water A classic example: HCl + NaOH NaCl + H 2 O Hydrochloric Acid Water Sodium Hydroxide (Lye) Sodium Chloride (Table Salt) 26
27 Acid-Base Reactions Example HNO 3 (aq) + KOH (aq) à Molecular: HNO 3 (aq) + KOH (aq) à H 2 O (l) + KNO 3 (aq) Total Ionic: H + (aq) + NO - 3 (aq) + K + (aq) + OH - (aq) à H 2 O (l) + K + (aq) + NO 3 - (aq) Net Ionic: H + (aq) + OH - (aq) à H 2 O (l) Acid-Base Neutralization Here s the equation again: HCl + NaOH NaCl + H 2 O Chemically, this is a double replacement reaction: The H traded its Cl for an OH The Na traded its OH for a Cl. 27
28 Oxidation-Reduction Reactions a.k.a. Redox Equations Between a metal and a nonmetal forming an ionic compound Electron transfer occurs Oxidation numbers: assigning an excess or deficiency in electrons for each element (the charge based on the compound). Rules for Oxidation Number (ox. #) Determination 1. The sum of the oxidation numbers add up to the charge a. all elements have an ox. # of 0 b. ions of elements, ox. # is the charge (Cl - ) c. the sum of the ox. # of a complex ion equals the charge (CO 3-2 ) 2. H is 1+ when combined with a nonmetal and 1- with a metal H 3 PO 4 CaH 2 H= 1+ PO 4 = 3- Ca = 2+ H= 1-28
29 Rules for Oxidation Numbers (cont.) 1. F is always 1-; Cl, Br, I are 1- except when combined with each other or O 2. O is 2- except when combined with F (F 2 O) 3. Group I is 1+ and Group II is 2+ in their compounds Recognizing Redox Rxns. oxidation 2 HCl (aq) + Mg (s) à MgCl 2 (aq) + H 2 (g) (-1) 0 reduction Net: 2 H + (aq) + Mg 0 (s) à Mg 2+ (aq) + H 0 2 (g) Loss of electron = oxidation Gain of electron = reduction LEO the lion goes GER" 29
30 Half Reactions Separate the individual oxidation and reduction reactions. Look at electron movement Half rxn.: Mg 0 (aq) à Mg e- 2e- + 2 H + à H 2 0 Net: 2 H + (aq) + Mg 0 (aq) à Mg 2+ (aq) + H 2 0 (q) Oxidizing agent: the one reduced (H+) Reducing agent: the one oxidized (Mg 0 ) Recognition of Redox rxns. Ø Oxidation # changes Ø Reactions with oxygen Ø Reaction of any element (forms a new compound) Balancing Ø Balance by mass Ø Balance by charge Ø Balance net ionic equation 30
31 Example Problem: Fe (s) + Cl 2 (aq) à FeCl 3 (aq) 1. Balance by mass 2 Fe (s) + 3Cl 2 (aq) à 2 FeCl 3 (aq) 2. Write the ionic equation 2 Fe (s) + 3 Cl 2 (aq) à 2 Fe3+ (aq) + 6 Cl - (aq) 3. Write half reaction 2 Fe 0 (s) à 2 Fe e- 6e- + Cl 2 à 2 Cl - 3. Balance by charge (want # of e- to cancel) 2 Fe 0 (s) à 2 Fe e-) 6e- + 3Cl 20 à 6 Cl - ) + 2 Fe 0 (s) + 6e- + 3Cl 2 à 2 Fe e- + 6 Cl - Final eqn.: 2 Fe (s) + 3Cl 2 à 2 Fe Cl - 31
Types of Reactions. There are five main types of chemical reactions we will talk about:
Chemical Reactions Types of Reactions There are five main types of chemical reactions we will talk about: 1. Synthesis reactions 2. Decomposition reactions 3. Single displacement reactions 4. Double displacement
More informationTypes of Reactions. There are five types of chemical reactions we observed in the lab:
Chemical Reactions Acids and Bases Acids: Form hydrogen ions (H + ) when dissolved in water. HCl (aq) H + (aq) + Cl - (aq) Examples: HCl (hydrochloric acid), HNO 3 (nitric acid), H 2 SO 4 (sulfuric acid),
More informationCHEMICAL REACTIONS. Introduction. Chemical Equations
CHEMICAL REACTIONS Chemistry I Chapter 7 1 Chemical Equations Their Job: Depict the kind of reactants and products and their relative amounts in a reaction. 4 Al (s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) The
More informationCHEMICAL REACTIONS. Types of Reactions. Steps to Writing Reactions
Types of Reactions CHEMICAL REACTIONS There are five types of chemical reactions we will talk about: 1. Synthesis reactions 2. reactions 3. Single displacement reactions 4. reactions 5. Combustion reactions
More informationCHEMICAL REACTION. Engr. Yvonne Ligaya F. Musico 1
CHEMICAL REACTION Engr. Yvonne Ligaya F. Musico 1 Chemical Reaction Engr. Yvonne Ligaya F. Musico 2 Introduction Chemical reactions occur when bonds between the outermost parts of atoms are formed or broken
More informationChapter 9. Vocabulary Ch Kick Off Activity. Objectives. Interpreting Formulas. Interpreting Formulas
Chapter 9 Chemical Vocabulary Ch. 9.1 Chemical reaction Reactant Product Word Equation Skeleton Equation Chemical equation Coefficient 1 2 Objectives Write chemical equations to describe chemical reactions
More informationChemical Reactions. All chemical reactions can be written as chemical equations.
Chemical Reactions All chemical reactions can be written as chemical equations. What is a Chemical Reaction? Chemical reactions represent chemical changes A chemical change occurs when a substance has
More informationChemical Equations and Chemical Reactions
Chemical Equations Chemical Equations and Chemical Reactions Chemical equations are concise representations of chemical reactions. Chemical Equations Symbols Used in Chemical Equations The formulas of
More informationChemical Reactions and Equations
Chemical Reactions and Equations 5-1 5.1 What is a Chemical Reaction? A chemical reaction is a chemical change. A chemical reaction occurs when one or more substances is converted into one or more new
More informationChemical Equations. Chemical Reactions. The Hindenburg Reaction 5/25/11
Chemical Reactions CHM 1032C Chemical Equations Chemical change involves a reorganization of the atoms in one or more substances. The Hindenburg Reaction Reactants are on left, products to the right. Arrow
More informationCHEMICAL REACTIONS WORDS, SYMBOLS AND ABBREVIATIONS
CHEMICAL REACTIONS All chemical reactions have two parts: (1) A substance that undergoes a reaction is called a. In other words, reactants are the substances you start with. (2) When reactants undergo
More informationBIG IDEA TWO. October 13, 2016
BIG IDEA TWO October 13, 2016 Topics to Cover in Big Idea 2 1. Ionic, metallic, and covalent bonds 2. Polarity and dipole moment 3. Intermolecular forces (IMF): 4. Lewis dot structures 5. Resonance forms
More informationBALANCING EQUATIONS NOTES
BALANCING EQUATIONS NOTES WHY DO WE NEED TO BALANCE CHEMICAL EQUATIONS? The LAW OF CONSERVATION OF MASS says that matter cannot be created or destroyed. In other words, you cannot end up with any more
More informationelemental state. There are two different possibilities: DESCRIPTION 1. One cation (+ ion) replaces another. 2. One anion (- ion) replaces another.
CHEMICAL TYPES HANDOUT In these reactions, a free element reacts with a compound to form another compound and release one of the elements of the original compound in the elemental state. There are two
More informationCHAPTER Describing Chemical Reactions Reactants Products. New substances produced The arrow means yields TYPES OF EQUATIONS.
CHAPTER 11 Chemical Reactions 11.1 Describing Chemical Reactions Reactants Products New substances produced The arrow means yields Where do Chemical Reactions occur? Everywhere!!! In living organisms In
More informationCHEMICAL REACTIONS 3/1/2012 PARTS OF A CHEMICAL EQUATION. Reactants: Zn + I 2 Product: ZnI 2. Indicators of chemical reactions
CHEMICAL REACTIONS Reactants: Zn + I 2 Product: ZnI 2 Indicators of chemical reactions Emission of light or heat Production of a gas Formation of a precipitate Color change Emission of odor PARTS OF A
More informationA reaction in which a solid forms is called a precipitation reaction. Solid = precipitate
Chapter 7 Reactions in Aqueous Solutions 1 Section 7.1 Predicting Whether a Reaction Will Occur Four Driving Forces Favor Chemical Change 1. Formation of a solid 2. Formation of water 3. Transfer of electrons
More informationIndicators of chemical reactions
Indicators of chemical reactions Emission of light or heat Formation of a gas Formation of a precipitate Color change Emission of odor All chemical reactions: have two parts Reactants - the substances
More informationSolubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
More informationCHAPTER 11: CHEMICAL REACTIONS. Mrs. Brayfield
CHAPTER 11: CHEMICAL REACTIONS Mrs. Brayfield WRITING EQUATIONS Write the chemical equation for the following: Magnesium metal reacts with hydrochloric acid to form aqueous magnesium chloride and hydrogen
More informationCh. 8 Chemical Reactions
Ch. 8 Chemical Reactions Intro to Reactions I II III IV V Signs of a Chemical Reaction Evolution of heat and light Formation of a gas Formation of a precipitate Color change Law of Conservation of Mass
More informationChapter 7: Chemical Reactions
C h a p t e r 7, C h a p t e r 1 6 ( 2-5 ) : C h e m i c a l R e a c t i o n s P a g e 1 Chapter 7: Chemical Reactions Read Chapter 7 and Check MasteringChemistry due dates. Evidence of Chemical Reactions:
More information8 Chemical Equations. Flames and sparks result when aluminum foil is dropped into liquid bromine.
8 Chemical Equations Flames and sparks result when aluminum foil is dropped into liquid bromine. Chapter Outline 8.1 The Chemical Equation 8.2 Writing and Balancing Chemical Equations 8.3 Types of Chemical
More informationChemistry I-H Types of Reactions / Reaction Prediction / Reaction Theory
Chemistry I-H Types of Reactions / Reaction Prediction / Reaction Theory I. Synthesis (combination) A + B ---------> AB Substances that are chemically combined may be two elements or two compounds. If
More informationChapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
More informationBalancing Equations Notes
. Unit 6 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 informationBalancing CHEMICAL EQUATIONS
Balancing CHEMICAL EQUATIONS CHEMICAL REACTIONS involves a chemical change in the identity of one or more chemical species Ex. Rusting of iron (Fe): chemical rxn btwn water and iron involve the breaking
More informationPart 01 - Notes: Reactions & Classification
Objectives: Identify, define, and explain: combination reaction, synthesis reaction, decomposition reaction, single replacement reaction, double replacement reaction, combustion reaction, rapid oxidation,
More informationChapter 8. Chemical Equations. Flames and sparks result when aluminum foil is dropped Into liquid bromine.
Chapter 8 Chemical Equations Flames and sparks result when aluminum foil is dropped Into liquid bromine. Introduction to General, Organic, and Biochemistry 10e John Wiley & Sons, Inc Morris Hein, Scott
More information11-1 Notes. Chemical Reactions
11-1 Notes Chemical Reactions Chemical Reactions In a chemical reaction 1 or more substances (the reactants) change into 1 or more new substances (the products). Reactants are always written on the left
More informationDefinition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change.
Chemical Reactions I. What is a chemical reaction? Definition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change. A. How can you
More informationBalancing 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 informationTYPES OF CHEMICAL REACTIONS SYNTHESIS (COMPOSITION), DECOMPOSITION AND REPLACEMENT (SINGLE AND DOUBLE), AND COMBUSTION
TYPES OF CHEMICAL REACTIONS SYNTHESIS (COMPOSITION), DECOMPOSITION AND REPLACEMENT (SINGLE AND DOUBLE), AND COMBUSTION YOU CAN THINK OF ATOMS AS PEOPLE GETTING TOGETHER AS COUPLES... Analogy One person
More informationChapter 4. Properties of Aqueous Solutions. Electrolytes in Aqueous Solutions. Strong, weak, or nonelectrolyte. Electrolytic Properties
Chapter 4 Reactions in Aqueous Solution Observing and Predicting Reactions How do we know whether a reaction occurs? What observations indicate a reaction has occurred? In your groups, make a list of changes
More informationCHEMICAL REACTIONS. The process by which one or more substances are changed into one or more different substances
CHEMICAL REACTIONS The process by which one or more substances are changed into one or more different substances Equations Reactions are represented by a chemical equation Reactants Products Must have
More informationChemical Reactions and Equations Types of Reactions Predicting Products Activity Series Identifying Oxidation-Reduction Reactions
Chemical Reactions and Equations Types of Reactions Predicting Products Activity Series Identifying Oxidation-Reduction Reactions A preview of things we will do Chemical Reactions are AWESOME! Characteristics
More informationCHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS
CHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS CHEMICAL REACTIONS Occurs when matter combines or breaks apart to produce new kinds of matter with different properties with a change in energy. EVIDENCE FOR
More informationUnit 6.3 Types of Chemical reactions
Unit 6.3 Types of Chemical reactions Most chemical reactions can be classified into one of five types of reactions. It depends on both the reactants used and the products formed. The possible chemical
More informationChemical Reaction Types
Chemical Reactions Chemical Reaction Types There are 5 types of chemical reactions that you need to know Combination reaction Decomposition reaction Combustion reaction Single replacement (redox) reaction
More informationAqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).
Aqueous Reactions Defining Aqueous Reactions Aqueous reactions are reactions that take place in water. To understand them, it is important to understand how compounds behave in water. Some compounds are
More informationChemical Reactions. Ch. 11 Chemical Reactions. Chemical Reactions. Chemical Reactions
Chemical Reactions Ch. 11 Chemical Reactions when a substance changes identity Reactants - original Products - resulting law of conservation of mass total mass of reactants = total mass of products In
More informationChapter 4; Reactions in Aqueous Solutions. Chapter 4; Reactions in Aqueous Solutions. V. Molarity VI. Acid-Base Titrations VII. Dilution of Solutions
Chapter 4; Reactions in Aqueous Solutions I. Electrolytes vs. NonElectrolytes II. Precipitation Reaction a) Solubility Rules III. Reactions of Acids a) Neutralization b) Acid and Carbonate c) Acid and
More informationCh 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON
Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the
More informationChemical Reactions
http://www.youtube.com/watch?v=hgn7ase8e6w&sns=em Chemical Reactions Agenda Day 39- Types of Chemical Reactions- Synthesis and Decomposition Lesson: PPT- Synthesis and decomposition Assign OBS. Table
More informationCHEMICAL REACTIONS. Discuss breaking/forming bonds 10/29/2012. Products Reactants
CHEMICAL REACTIONS - Page 321 Products Reactants Reactants: Zn + I 2 Product: Zn I 2 Discuss breaking/forming bonds Chemical Reaction or Change process in which one or more substances are converted into
More informationBalancing Equations Notes
. Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with the (starting
More informationMoles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Micro World atoms & molecules Macro World grams Atomic mass is the mass of an atom in
More informationChapter 5 Classification and Balancing of Chemical Reactions
Chapter 5 Classification and Balancing of Chemical Reactions 5.1 Chemical Equations Chemical equations describe chemical reactions. - As words: hydrogen plus oxygen combine to form water - As a chemical
More informationChapter 4 Chemical Formulas, Reactions, Redox and Solutions
Terms to Know: Solubility Solute Solvent Solution Chapter 4 the amount of substance that dissolves in a given volume of solvent at a given temperature. a substance dissolved in a liquid to form a solution
More informationHonors text: Ch 10 & 12 Unit 06 Notes: Balancing Chemical Equations
Notes: Balancing Chemical Equations Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products are completely
More informationUnit 4: Reactions and Stoichiometry
Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)
More information2) Solve for protons neutrons and electrons for the bromide ION.
1) Write the formulas for the following a) Calcium nitride c)lithium hydroxide b) Iron (III) sulfide d) sulfuric acid 2) Solve for protons neutrons and electrons for the bromide ION. 3) Write the electron
More informationWhat Do You Think? Investigate GOALS
Cool Chemistry Show Activity 4 Chemical Equations GOALS In this activity you will: Represent chemical changes using word equations and chemical equations. Distinguish between different classes of chemical
More informationTypes of Chemical Reactions
Types of Chemical Reactions There are five types of chemical reactions: 1. Formation (combination) 2. Decomposition 3. Single Displacement 4. Double Displacement 5. Combustion 1 Formation (Combination)
More informationUnit 5: Chemical Equations and Reactions & Stoichiometry
pg. 10 Unit 5: Chemical Equations and Reactions & Stoichiometry Chapter 8: Chemical Equations and Reactions 8.1: Describing Chemical Reactions Selected Chemistry Assignment Answers (Section Review on pg.
More informationUnit 1 - Foundations of Chemistry
Unit 1 - Foundations of Chemistry Chapter 2 - Chemical Reactions Unit 1 - Foundations of Chemistry 1 / 42 2.1 - Chemical Equations Physical and Chemical Changes Physical change: A substance changes its
More informationUnit IV: Chemical Equations & Stoichiometry
Unit IV: Chemical Equations & Stoichiometry A. The chemical equation B. Types of chemical reactions A. Activity series of metals B. Solubility rules C. Rules for writing and balancing equations D. Calculations
More informationIntroduction to Chemical Reactions. Making new substances
Introduction to Chemical Reactions Making new substances Main Ideas Chemical Reactions are represented by Chemical Equations. Chemical Equations are balanced to show the same number of atoms of each element
More informationUnit Learning Targets (L.T.):
Unit 9: Chemical Equations and Reactions Chapters 8 and 19 Name Block Unit Learning Targets (L.T.): By the end of the unit, students will be able to: Chapter 8: 1. Correctly write and balance chemical
More informationChapter 5. Chemical reactions
Chapter 5 Chemical reactions Chemical equations CaO(s) + CO 2 (g) CaCO 3 (s) + CO(g) Chemical equation - representation of a chemical reaction; uses the symbols of the elements and formulae of the compounds
More informationIntro to Reactions/ Balancing Equations
Intro to Reactions/ Balancing Equations Chemical Reactions Chemical reactions involve change. Evidence of a chemical reaction could include the following Evolution of heat, light, and/or sound Production
More informationThe solvent is the dissolving agent -- i.e., the most abundant component of the solution
SOLUTIONS Definitions A solution is a system in which one or more substances are homogeneously mixed or dissolved in another substance homogeneous mixture -- uniform appearance -- similar properties throughout
More informationReaction Writing Sheet #1 Key
Reaction Writing Sheet #1 Key Write and balance each of the following reactions and indicate the reaction type(s) present: 1. zinc + sulfur zinc sulfide 8 Zn (s) + S 8 (s) 8 ZnS (s) synthesis 2. potassium
More informationCh. 8 Notes ~ CHEMICAL REACTIONS NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 8 Notes ~ CHEMICAL REACTIONS NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Chemical Reactions (rxns.) A. chemical reaction an expression showing the conversion
More informationThe Copper Cycle. HCl(aq) H + (aq) + Cl (aq) HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl (aq)
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 informationChapter 11. Symbols used in equations indicates a reversible reaction (More later) heat. Chemical Reactions
Chapter 11 Chemical Reactions All chemical reactions have two parts Reactants - the substances you start with Products- the substances you end up with The reactants turn into the products. Reactants Products
More informationNihal İKİZOĞLU 1. TYPE of CHEMICAL REACTIONS. Balance the following chemical equations. 1. Fe + H 2 SO 4 Fe 2 (SO 4 ) 3 + H 2
TYPE of CHEMICAL REACTIONS Balance the following chemical equations. 1. Fe + H 2 SO 4 Fe 2 (SO 4 ) 3 + H 2 2. C 2 H 6 + O 2 H 2 O + CO 2 3. KOH + H 3 PO 4 K 3 PO 4 + H 2 O 4. SnO 2 + H 2 Sn + H 2 O 5.
More informationWord Equations. Symbols used in equations. Unit 7: Chemical Reactions. hydrogen peroxide water + oxygen
Unit 7: Chemical Reactions Chemical reactions involve a reorganization of the atoms in one or more substances. Can be represented in different ways 1 Word Equations hydrogen peroxide reacts to produce
More informationChapter 4 Electrolytes and Aqueous Reactions. Dr. Sapna Gupta
Chapter 4 Electrolytes and Aqueous Reactions Dr. Sapna Gupta Aqueous Solutions Solution - a homogeneous mixture of solute + solvent Solute: the component that is dissolved Solvent: the component that does
More informationReactions in Aqueous Solutions
Copyright 2004 by houghton Mifflin Company. Reactions in Aqueous Solutions Chapter 7 All rights reserved. 1 7.1 Predicting if a Rxn Will Occur When chemicals are mixed and one of these driving forces can
More informationChemical Reactions. Burlingame High School Chemistry 1
Chemical Reactions 1 Chemical Equations Chemical equations are use to describe: the substances that react, the reactants the substances that are formed, the products the relative amounts of all substances
More informationChapter 4: Stoichiometry of Chemical Reactions. 4.1 Writing and Balancing Chemical Equations
Chapter 4: Stoichiometry of Chemical Reactions 4.1 Writing and Balancing Chemical Equations A chemical equation represents or symbolizes a chemical reaction. o Substances are represents by their chemical
More informationed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13
ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)
More information7.01 Chemical Reactions
7.01 Chemical Reactions The Law of Conservation of Mass Dr. Fred Omega Garces Chemistry 100 Miramar College 1 Chemical Reactions Making Substances Chemical Reactions; the heart of chemistry is the chemical
More informationChapter 7 Chemical Reactions
Chapter 7 Chemical Reactions Evidence of Chemical Change Release or Absorption of Heat Color Change Emission of Light Formation of a Gas Formation of Solid Precipitate Tro's "Introductory 2 How Do We Represent
More informationinsoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water
Aqueous Solutions Solubility is a relative term since all solutes will have some solubility in water. Insoluble substances simply have extremely low solubility. The solubility rules are a general set of
More informationChapter 4 - Types of Chemical Reactions and Solution Chemistry
Chapter 4 - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent - the water molecule is bent with and H-O-H angles of approx. 105 º - O-H bonds are covalent - O is slightly
More information7.01 Chemical Reactions
7.01 Chemical Reactions The Law of Conservation of Mass Dr. Fred Omega Garces Chemistry 152 Miramar College 1 Chemical Reactions Making Substances Chemical Reactions; the heart of chemistry is the chemical
More informationVarious Types of Reactions
Various Types of Reactions Matthew Park Outline: 1. Synthesis / Replacement / Decomposition Reactions 2. Precipitation Reactions 3. Acid-Base Reactions 4. Summary: Metathesis Reactions NOTE: Not all of
More informationChemical Reactions. Chemical changes are occurring around us all the time
Chemical changes are occurring around us all the time Food cooking Fuel being burned in a car s engine Oxygen being used in the human body The starting materials are called reactants The ending materials
More informationSCH 3UI Unit 5 Outline Chemical Reactions Homework Questions and Assignments complete handouts: Balancing Equations #1, #2, #3, #4
Lesson Topics Covered 1 Note: Chemical Reactions and Chemical Equations definition of chemical reaction four signs of chemical change the Law of Conservation of Mass balancing chemical equations SCH 3UI
More informationChem 1A Dr. White Fall Handout 4
Chem 1A Dr. White Fall 2014 1 Handout 4 4.4 Types of Chemical Reactions (Overview) A. Non-Redox Rxns B. Oxidation-Reduction (Redox) reactions 4.6. Describing Chemical Reactions in Solution A. Molecular
More informationChapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill
Chapter 4 Reactions in Aqueous Solutions Copyright McGraw-Hill 2009 1 4.1 General Properties of Aqueous Solutions Solution - a homogeneous mixture Solute: the component that is dissolved Solvent: the component
More informationNotes: Chemical Reactions. Diatomic elements: H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2 I Bring Clay For Our New Hut OR HOBrFINCl
Name Chemistry-PreAP Notes: Chemical Reactions Period Review: Some elements do not occur as single atoms when uncombined with other elements. They will bond with themselves, forming a molecule. In any
More informationAP Chemistry Unit #4. Types of Chemical Reactions & Solution Stoichiometry
AP Chemistry Unit #4 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to: Predict to some extent whether a substance will be a strong electrolyte,
More informationNet Ionic Equations. Making Sense of Chemical Reactions
Making Sense of Chemical Reactions Now that you have mastered writing balanced chemical equations it is time to take a deeper look at what is really taking place chemically in each reaction. There are
More informationChapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions. Dr. Sapna Gupta
Chapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions Dr. Sapna Gupta Types of Reactions Two classifications: one how atoms are rearrangement and the other is chemical
More informationChemical Reactions. Indicators of a Chemical Reaction. Indicators of a Chemical Reaction 1. Formation of a solid (called a precipitate)
Chemical Reactions Quantitative Chem Indicators of a Chemical Reaction Indicators of a Chemical Reaction 1. Formation of a solid (called a precipitate) 1 Indicators of a Chemical Reaction 1. Formation
More informationSolution Chemistry. Chapter 4
Solution Chemistry Chapter 4 Covalent Molecule Dissolving in Water Ionic Compound Dissolving in Water Electrolytes and Nonelectrolytes Electrolytes/Nonelectrolytes Type Dissociation Electrical Conductivity
More informationReactions in Aqueous Solutions
Chapter 4 Reactions in Aqueous Solutions Some typical kinds of chemical reactions: 1. Precipitation reactions: the formation of a salt of lower solubility causes the precipitation to occur. precipr 2.
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Topics General properties of aqueous solutions Precipitation reactions Acid base reactions Oxidation reduction reactions Concentration of solutions Aqueous reactions
More informationTypes of Chemical Reactions
Types of Chemical Reactions 1) Combination (Synthesis) Reaction 2) Decomposition 3) Single Replacement 4) Double Replacement 5) Combustion 6) Oxidation-Reduction (Redox) Combination (Synthesis) Reactions
More informationUnit 5 Chemical Reactions Notes. Introduction: Chemical substances have physical and chemical properties
Unit 5 Chemical Reactions Notes Introduction: Chemical substances have physical and chemical properties Physical Properties 2 Types of Physical Properties Extensive Physical Properties Intensive Physical
More informationNotes: Chemical Reactions (text Ch. 8)
U Name Per. Notes: Chemical Reactions (text Ch. 8) NOTE: This set of class notes is not complete. We will be filling in information in class. If you are absent, it is your responsibility to get missing
More information9-1 The Nature of Chemical Reactions
9-1 The Nature of Chemical Reactions What are chemical reactions and why do they occur? A chemical reaction is a process in which one or more substances are converted into new substances with different
More informationCH 4 AP. Reactions in Aqueous Solutions
CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,
More informationHW 7 KEY!! Chap. 7, #'s 11, 12, odd, 31, 33, 35, 39, 40, 53, 59, 67, 70, all, 77, 82, 84, 88, 89 (plus a couple of unassigned ones)
HW 7 KEY!! Chap. 7, #'s 11, 12, 15-21 odd, 31, 33, 35, 39, 40, 53, 59, 67, 70, 72-75 all, 77, 82, 84, 88, 89 (plus a couple of unassigned ones) 11) NOTE: I used the solubility rules that I have provided
More informationChapter 9. Chemical Reaction
Chapter 9 Chemical Reaction Everyday Chemical Reaction O Can you name some? O Cooking Pizza O Changes the ingredients O Combustion O Driving to school burns gasoline O Wheelbarrow rusting (especially in
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationScience 1206 Chemistry Unit #11
Science 1206 Chemistry Unit #11 Types of Chemical Reactions Types of Chemical Reactions Five types of chemical reactions: Formation (synthesis) Decomposition Single Displacement Double Displacement Combustion
More information