temperature change a) On heating, solid calcium carbonate yields solid calcium oxide and gaseous carbon dioxide. 4Li(s) + O 2 (g) 2Li 2 O(s)
|
|
- Brandon Parker
- 7 years ago
- Views:
Transcription
1 CHEMISTRY WKST CH. 7 & 8 REVIEW (REACTIONS & EQUATIONS) NAME: JMS 1) What are the 5 evidences that a chemical reaction took place? precipitate forms color change gas released temperature change 2) Consider the equation: 4Al(s) + 3O 2 (g) 2Al 2 O 3 (s) a) Name the reactants. aluminum (Al), oxygen gas (O 2 ) b) Name the product. aluminum oxide c) Is the equation balanced? yes d) What is the physical state of Al 2 O 3? solid e) What does the mean? yields 3) Change these word equations to balanced equations using symbols. energy released a) On heating, solid calcium carbonate yields solid calcium oxide and gaseous carbon dioxide. CaCO 3 (s) CaO(s) + CO 2 (g) b) Solid lithium metal reacts with oxygen gas to form solid lithium oxide. 4Li(s) + O 2 (g) 2Li 2 O(s) c) Solid zinc metal reacts with aqueous hydrochloric acid to form aqueous zinc chloride and hydrogen gas. Zn(s) + 2HCl(aq) ZnCl 2 (aq) + H 2 (g) 4) What law requires us to balance chemical equations? Law of Conservation of Matter 5) When balancing chemical equations, what is the only thing you are allowed to change? The coefficients in front of the formulas of the substances in the equation. 6) Balance the following equations. a) 3Fe + 4H 2 O Fe 3 O 4 + 4H 2 b) 2AlBr 3 + 3Cl 2 2AlCl 3 + 3Br 2 c) 2HNO 3 + Ba(OH) 2 Ba(NO 3 ) 2 + 2H 2 O d) C 8 H O 2 8CO 2 + 8H 2 O e) Na 2 CO 3 + 2HCl 2NaCl + H 2 O + CO 2 f) 3K 2 CO 3 + 2Al(ClO 4 ) 3 Al 2 (CO 3 ) 3 + 6KClO 4 g) 4H 2 O + Cr + Na 2 CrO 4 2Cr(OH) 3 + 2NaOH 7) What are the 4 main driving forces in making a reaction occur? forming a precipitate forming molecular substances like water forming a gas transferring electrons (redox)
2 8) What does the triangle above the arrow mean in a chemical equation? -2- the reactants are being heated 9) Classify each of the following statements as describing a double replacement, single replacement, combustion, synthesis, decomposition or acid-base. There may be more than one answer for a statement give them all. a) O 2 (g) is always a reactant. combustion b) Reaction is always endothermic. decomposition c) 2 compounds reacting to form 2 products, one which is an insoluble solid, gas or water. double replacement d) Reaction is always exothermic. combustion, synthesis e) Forms one product. synthesis f) Forms water and a salt. acid-base g) An element and a compound react to form 2 products, 1 an element and the other a compound. single repl. h) Has only one reactant. decomposition 10) When burning a hydrocarbon, what are the products? CO 2 (g), H 2 O(l) 11) Classify each of the following reactions as double replacement, single replacement, combustion, synthesis, decomposition or acid-base. Include all possibilities. a) Cu + Cl 2 CuCl 2 synthesis b) KBr + AgNO 3 AgBr + KNO 3 double replacement c) 2Ba + O 2 2BaO synthesis, combustion d) Fe + CuSO 4 FeSO 4 + Cu single replacement e) C 3 H 8 + 5O 2 3CO 2 + 4H 2 O combustion f) HCl + KOH KCl + H 2 O acid-base g) 2KClO 3 2KCl + 3O 2 decomposition 12) Tell what physical state the following would be in water. a) K 2 SO 4 (aq) d) MgO (s) b) NH 4 OH (aq) e) Cu(NO 3 ) 2 (aq) c) BaCO 3 (s) f) AlPO 4 (s) 13) List the 7 strong acids. HCl, HBr, HI, HNO 3, HClO 3, HClO 4, H 2 SO 4 14) What is the main difference between strong and weak acids? Strong acids completely dissociate (breaks up into its ions) in water whereas weak acids only partially dissociate in water. 15) List the 7 diatomic elements and their physical state at room temperature. H 2 (g), N 2 (g), O 2 (g), F 2 (g), Cl 2 (g), Br 2 (l), I 2 (s)
3 -3-16) What is the net ionic equation for all strong acids-bases reactions? H + (aq) + OH (aq) H 2 O(l) 17) For each of the following molecular equations, write the ionic equation, circle the spectator ions (if any), and write the net ionic equation. a) Zn(NO 3 ) 2 (aq) + K 2 CO 3 (aq) ZnCO 3 (s) + 2KNO 3 (aq) Zn 2+ (aq) + 2NO 3 (aq) + 2K + (aq) + CO 3 2 (aq) ZnCO 3 (s) + 2K + (aq) + 2NO 3 (aq) Zn 2+ (aq) + CO 3 2 (aq) ZnCO 3 (s) b) Mg(s) + 2AgNO 3 (aq) Mg(NO 3 ) 2 (aq) + 2Ag(s) Mg(s) + 2Ag + (aq) + 2NO 3 (aq) Mg 2+ (aq) + 2NO 3 (aq) + 2Ag(s) Mg(s) + 2Ag + (aq) Mg 2+ (aq) + 2Ag(s) c) HClO 4 (aq) + LiOH(aq) H 2 O(l) + LiClO 4 (aq) H + (aq) + ClO 4 (aq) + Li + (aq) + OH (aq) H 2 O(l) + Li + (aq) + ClO 4 (aq) H + (aq) + OH (aq) H 2 O(l) 18) Tell what acid and base make the following salts. a) Ba(NO 3 ) 2 b) KClO 3 c) NH 4 Br d) Fe 2 (CO 3 ) 3 acid HNO 3 HClO 3 HBr H 2 CO 3 base Ba(OH) 2 KOH NH 4 OH Fe(OH) 3 19) When we did the single replacement lab the only reactions we did with Ca was with an acid and with H 2 O. Why did we not do the other reactions with Ca and the solutions? Calcium reacts with H 2 O. Since the other solutions were in H 2 O, the Ca will react with the H 2 O as well as the solute. In other words, the Ca + H 2 O reaction will interfere with the desired reactions. 20) Why does Zn react more vigorously with an acid than Sn? Zn is much more reactive with an acid than Sn as shown by Zn being farther away from the acid on the activity series than Sn is. 21) Why do we sometimes get a precipitate when mixing 2 solutions? Sometimes there are 2 ions in the resulting mixture that when they come in contact with each other will form an insoluble solid. 22) If a solution of KCl and NaCl is mixed with another solution containing MgCl 2, how many different kinds of ions are present? Would there be a precipitate? Why or why not? There are 4 different ions present. No there will not be a precipitate since the chlorides of the cations (the positive ions) are soluble. Also, since Cl is the anion in all 3 solutions, no new substances would be formed. 23) So far this year we have seen a couple of colored solutions containing transition metals. What color is the solution containing the following ions containing a transition metal? a) Cu 2+ blue b) CrO 4 2 yellow
4 24) Complete and balance the following equations. Include physical states for the products. -4- a) C 6 H 6 (l) + O 2 (g) CO 2 (g) + H 2 O(l) b) Cu(s) + AgNO 3 (aq) Cu(NO 3 ) 2 (aq) + Ag(s) c) Pb(ClO 3 ) 2 (aq) + K 2 SO 4 (aq) PbSO 4 (s) + KClO 3 (aq) d) CuO(s) Cu(s) + O 2 (g) e) MgCO 3 (s) + H 2 SO 4 (aq) MgSO 4 (aq) + CO 2 (g) + H 2 O(l) f) NH 4 OH(aq) + H 3 PO 4 (aq) H 2 O(l) + (NH 4 ) 3 PO(aq) The next one was a mistake it doesn t work. Change it to what is shown on the left and work it out. g) SO 2 (g) + H 2 O(l) H 2 SO 3 (aq) h) Na 2 S(aq) + Ni(NO 3 ) 2 (aq) NaNO 3 (aq) + NiS(s) i) Ba(ClO 3 ) 2 (aq) BaCl 2 (s) + O 2 (g) j) Zn(s) + CuCl 2 (aq) ZnCl 2 (aq) + Cu(s) k) AlCl 3 (aq) + Pb(NO 3 ) 2 (aq) Al(NO 3 ) 3 (aq) + PbCl 2 (s) l) Rb 2 O(s) + H 2 O(l) RbOH(aq) m) CaO(s) + CO 2 (g) CaCO 3 (s) n) Cu(s) + Li 2 CO 3 (aq) NR Cu is less reactive than Li and therefore cannot replace it. o) HgO(l) Hg(l) + O 2 (g) p) K(s) + Cl 2 (g) KCl(s) q) Cl 2 (g) + KBr(aq) KCl(aq) + Br 2 (l) r) H 2 SO 3 (g) H 2 O(l) + SO 2 (g) s) BaCO 3 (s) BaO(s) + CO 2 (g) t) K(s) + H 2 O(l) KOH(aq) + H 2 (g) u) BaCl 2 (s) + O 2 (g) Ba(ClO 3 ) 2 (s) v) RbOH(s) Rb 2 O(aq) + H 2 O(l)
5 VOCAB TO KNOW: electrolyte: Substance that conducts electricity when dissolved or melted endothermic: process that absorbs energy (heat) exothermic: process that gives off energy (heat) hydrocarbon: compound made up of carbon and hydrogen insoluble: won t dissolve oxidation: process that loses electrons precipitate: solid formed by the reaction between two solutions products: substances formed in a reaction they will be on the right side of the arrow in a chemical equation reactants: substances that begin a reaction they will be on the left side of the arrow in a chemical equation reduction: process that gain electrons soluble: will dissolve
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 informationChemical 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 informationChapter 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 informationChapter 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 information2. DECOMPOSITION REACTION ( A couple have a heated argument and break up )
TYPES OF CHEMICAL REACTIONS Most reactions can be classified into one of five categories by examining the types of reactants and products involved in the reaction. Knowing the types of reactions can help
More informationNET 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 informationReactions 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 informationChemical Equations and Chemical Reactions. Chapter 8.1
Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.
More informationBalancing 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 informationExperiment 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 informationChapter 8 - Chemical Equations and Reactions
Chapter 8 - Chemical Equations and Reactions 8-1 Describing Chemical Reactions I. Introduction A. Reactants 1. Original substances entering into a chemical rxn B. Products 1. The resulting substances from
More informationUNIT (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 information6 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 informationChemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
More informationDepartment of Chemical Engineering Review Sheet Chemical Reactions Prepared by Dr. Timothy D. Placek from various sources
Department of Chemical Engineering Review Sheet Chemical Reactions Prepared by Dr. Timothy D. Placek from various sources Introduction This document is intended to help you review the basics of writing
More informationChemistry 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 informationExperiment 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 informationH 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 informationEXPERIMENT 8: Activity Series (Single Displacement Reactions)
EPERIMENT 8: Activity Series (Single Displacement Reactions) PURPOSE a) Reactions of metals with acids and salt solutions b) Determine the activity of metals c) Write a balanced molecular equation, complete
More informationChapter 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 informationWriting, 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 informationstoichiometry = 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 informationChapter 6 Notes Science 10 Name:
6.1 Types of Chemical Reactions a) Synthesis (A + B AB) Synthesis reactions are also known as reactions. When this occurs two or more reactants (usually elements) join to form a. A + B AB, where A and
More information1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)
1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)
More informationSolution. 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 informationCHEMICAL REACTIONS. Chemistry 51 Chapter 6
CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,
More informationChapter 5 Chemical Quantities and Reactions. Collection Terms. 5.1 The Mole. A Mole of a Compound. A Mole of Atoms.
Chapter 5 Chemical Quantities and Reactions 5.1 The Mole Collection Terms A collection term states a specific number of items. 1 dozen donuts = 12 donuts 1 ream of paper = 500 sheets 1 case = 24 cans 1
More informationSolution 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 informationDavid A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College
WRITING CHEMICAL EQUATIONS 2004, 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,
More informationChapter 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 informationTypes of Reactions. CHM 130LL: Chemical Reactions. Introduction. General Information
Introduction CHM 130LL: Chemical Reactions We often study chemistry to understand how and why chemicals (reactants) can be transformed into different chemicals (products) via a chemical reaction: Reactants
More informationNAMING 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 informationExperiment 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 informationWriting 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 informationMoles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:
Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)
More informationChemical Reactions in Water Ron Robertson
Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds
More informationMoles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an
More informationChapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions
Oxidation-Reduction Reactions Chapter 11 Electrochemistry Oxidation and Reduction Reactions An oxidation and reduction reaction occurs in both aqueous solutions and in reactions where substances are burned
More information4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes
Chapter 4 Reactions in Aqueous Solution 4.1 Aqueous Solutions Solution homogeneous mixture of 2 or more substances Solute the substance present in a smaller amount (usually solid in Chap. 4) Solvent the
More informationStoichiometry and Aqueous Reactions (Chapter 4)
Stoichiometry and Aqueous Reactions (Chapter 4) Chemical Equations 1. Balancing Chemical Equations (from Chapter 3) Adjust coefficients to get equal numbers of each kind of element on both sides of arrow.
More informationChemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
More informationUnit 10A Stoichiometry Notes
Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
More informationChemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent.
TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present
More informationI N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS
Chemical reaction = process during which original substances change to new substances, reactants turn to... The bonds of reactants... and new bonds are... The classification of reactions: 1. Classification
More informationName: Class: Date: 2 4 (aq)
Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of
More information2. Write the chemical formula(s) of the product(s) and balance the following spontaneous reactions.
1. Using the Activity Series on the Useful Information pages of the exam write the chemical formula(s) of the product(s) and balance the following reactions. Identify all products phases as either (g)as,
More informationStoichiometry Review
Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen
More information4. Balanced chemical equations tell us in what molar ratios substances combine to form products, not in what mass proportions they combine.
CHAPTER 9 1. The coefficients of the balanced chemical equation for a reaction give the relative numbers of molecules of reactants and products that are involved in the reaction.. The coefficients of the
More informationChapter 6: Writing and Balancing Chemical Equations. AB A + B. CaCO3 CaO + CO2 A + B C. AB + C AC + B (or AB + C CB + A)
78 Chapter 6: Writing and Balancing Chemical Equations. It is convenient to classify chemical reactions into one of several general types. Some of the more common, important, reactions are shown below.
More informationAqueous 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 informationCHM1 Review for Exam 12
Topics Solutions 1. Arrhenius Acids and bases a. An acid increases the H + concentration in b. A base increases the OH - concentration in 2. Strong acids and bases completely dissociate 3. Weak acids and
More informationBalancing Chemical Equations Practice
Science Objectives Students will describe what reactants and products in a chemical equation mean. Students will explain the difference between coefficients and subscripts in chemical equations. Students
More informationPART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)
CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students
More information= 11.0 g (assuming 100 washers is exact).
CHAPTER 8 1. 100 washers 0.110 g 1 washer 100. g 1 washer 0.110 g = 11.0 g (assuming 100 washers is exact). = 909 washers 2. The empirical formula is CFH from the structure given. The empirical formula
More informationRedox and Electrochemistry
Name: Thursday, May 08, 2008 Redox and Electrochemistry 1. A diagram of a chemical cell and an equation are shown below. When the switch is closed, electrons will flow from 1. the Pb(s) to the Cu(s) 2+
More informationThe 5 Types of Chemical Reactions (Chapter 11) By C B 6 th period
The 5 Types of Chemical Reactions (Chapter 11) By C B 6 th period 1) Combination Reactions Is also referred to as a synthesis reaction It is a chemical change in which two or more substances react to form
More informationChemical Reactions 2 The Chemical Equation
Chemical Reactions 2 The Chemical Equation INFORMATION Chemical equations are symbolic devices used to represent actual chemical reactions. The left side of the equation, called the reactants, is separated
More informationSCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample
More informationGeneral Chemistry Lab Experiment 6 Types of Chemical Reaction
General Chemistry Lab Experiment 6 Types of Chemical Reaction Introduction Most ordinary chemical reactions can be classified as one of five basic types. The first type of reaction occurs when two or more
More informationCHEM 110: CHAPTER 3: STOICHIOMETRY: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS
1 CHEM 110: CHAPTER 3: STOICHIOMETRY: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS The Chemical Equation A chemical equation concisely shows the initial (reactants) and final (products) results of
More informationBalancing Chemical Equations Worksheet Intermediate Level
Balancing Chemical Equations Worksheet Intermediate Level Neutralization Reactions Salts are produced by the action of acids. Salts are written metal first, then non-metal. Eg. NaCl not ClNa Acid + Base
More informationCHAPTER 5: MOLECULES AND COMPOUNDS
CHAPTER 5: MOLECULES AND COMPOUNDS Problems: 1-6, 9-13, 16, 20, 31-40, 43-64, 65 (a,b,c,e), 66(a-d,f), 69(a-d,f), 70(a-e), 71-78, 81-82, 87-96 A compound will display the same properties (e.g. melting
More informationAqueous 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 informationAnswers and Solutions to Text Problems
Chapter 7 Answers and Solutions 7 Answers and Solutions to Text Problems 7.1 A mole is the amount of a substance that contains 6.02 x 10 23 items. For example, one mole of water contains 6.02 10 23 molecules
More information1. 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 informationReduction. The gain of electron(s), causing the oxidation number of a species to
Reactions Word Coefficient Decomposition Double replacement Law of conservation of charge Law of conservation of energy Law of conservation of mass Mole ratio Oxidation Precipitate Product Reactant Reaction
More informationneutrons are present?
AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest
More informationMolarity 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 informationChemistry Final Study Guide
Name: Class: Date: Chemistry Final Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The electrons involved in the formation of a covalent bond
More informationGCSE Chemistry. Making Salts Instructions and answers for teachers
GCSE Chemistry Making Salts Instructions and answers for teachers The Activity: Learning Outcomes: To be able to recall the names and chemical formulae for commonly used acids To understand how salts can
More informationAtomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells
Atomic Structure called nucleons Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells The number of protons equals the atomic number This
More informationSanta 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 informationEDULABZ. Na 2 + H 2 CO 3. O + CO 2 (b) CaO + H 2. + NaCl AgCl + NaNO 3 3. Which of the following reactions does not take place?
4 TRANSFORMATION OF SUBSTANCE I. Multiple choice questions: (Tick the correct option). 1. The reaction between magnesium and oxygen is: (a) an endothermic reaction (b) an exothermic reaction (c) a catalysed
More informationFormulae, stoichiometry and the mole concept
3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be
More informationCHEMISTRY COMPUTING FORMULA MASS WORKSHEET
CHEMISTRY COMPUTING FORMULA MASS WORKSHEET Directions: Find the formula mass of the following compounds. Round atomic masses to the tenth of a decimal place. Place your final answer in the FORMULA MASS
More informationCalculations and Chemical Equations. Example: Hydrogen atomic weight = 1.008 amu Carbon atomic weight = 12.001 amu
Calculations and Chemical Equations Atomic mass: Mass of an atom of an element, expressed in atomic mass units Atomic mass unit (amu): 1.661 x 10-24 g Atomic weight: Average mass of all isotopes of a given
More informationAqueous Chemical Reactions
Name: Date: Lab Partners: Lab section: Aqueous Chemical Reactions The purpose of this lab is to introduce you to three major categories of reactions that occur in aqueous solutions: precipitation reactions,
More informationSAMPLE PROBLEM 8.1. Solutions of Electrolytes and Nonelectrolytes SOLUTION STUDY CHECK
Solutions of Electrolytes and Nonelectrolytes SAMPLE PROBLEM 8.1 Indicate whether solutions of each of the following contain only ions, only molecules, or mostly molecules and a few ions: a. Na 2 SO 4,
More informationChem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
More information1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams?
Name: Tuesday, May 20, 2008 1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams? 2 5 1. P2O 5 3. P10O4 2. P5O 2 4. P4O10 2. Which substance
More informationWord Equations and Balancing Equations. Video Notes
Word Equations and Balancing Equations Video Notes In this lesson, you will: Use the law of conservation of mass and provide standard rules for writing and balancing equations. Write and balance equations
More informationSample Exercise 3.1 Interpreting and Balancing Chemical Equations
Sample Exercise 3.1 Interpreting and Balancing Chemical Equations The following diagram represents a chemical reaction in which the red spheres are oxygen atoms and the blue spheres are nitrogen atoms.
More information1332 CHAPTER 18 Sample Questions
1332 CHAPTER 18 Sample Questions Couple E 0 Couple E 0 Br 2 (l) + 2e 2Br (aq) +1.06 V AuCl 4 + 3e Au + 4Cl +1.00 V Ag + + e Ag +0.80 V Hg 2+ 2 + 2e 2 Hg +0.79 V Fe 3+ (aq) + e Fe 2+ (aq) +0.77 V Cu 2+
More informationChapter 3. Chemical Reactions and Reaction Stoichiometry. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT
Lecture Presentation Chapter 3 Chemical Reactions and Reaction James F. Kirby Quinnipiac University Hamden, CT The study of the mass relationships in chemistry Based on the Law of Conservation of Mass
More informationChapter 16: Tests for ions and gases
The position of hydrogen in the reactivity series Hydrogen, although not a metal, is included in the reactivity series because it, like metals, can be displaced from aqueous solution, only this time the
More informationIB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
More informationPhysical Changes and Chemical Reactions
Physical Changes and Chemical Reactions Gezahegn Chaka, Ph.D., and Sudha Madhugiri, Ph.D., Collin College Department of Chemistry Objectives Introduction To observe physical and chemical changes. To identify
More informationWriting Chemical Equations
Writing Chemical Equations Chemical equations for solution reactions can be written in three different forms; molecular l equations, complete ionic i equations, and net ionic equations. In class, so far,
More informationChemistry Ch 15 (Solutions) Study Guide Introduction
Chemistry Ch 15 (Solutions) Study Guide Introduction Name: Note: a word marked (?) is a vocabulary word you should know the meaning of. A homogeneous (?) mixture, or, is a mixture in which the individual
More informationChemical Equations & Stoichiometry
Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term
More informationCLASS TEST GRADE 11. PHYSICAL SCIENCES: CHEMISTRY Test 6: Chemical change
CLASS TEST GRADE PHYSICAL SCIENCES: CHEMISTRY Test 6: Chemical change MARKS: 45 TIME: hour INSTRUCTIONS AND INFORMATION. Answer ALL the questions. 2. You may use non-programmable calculators. 3. You may
More information4.1 Writing and Balancing Chemical Equations
176 Chapter 4 Stoichiometry of Chemical Reactions 4.1 Writing and Balancing Chemical Equations By the end of this section, you will be able to: Derive chemical equations from narrative descriptions of
More informationTopic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole
Topic 4 National Chemistry Summary Notes Formulae, Equations, Balancing Equations and The Mole LI 1 The chemical formula of a covalent molecular compound tells us the number of atoms of each element present
More informationW1 WORKSHOP ON STOICHIOMETRY
INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of
More information20.2 Chemical Equations
All of the chemical changes you observed in the last Investigation were the result of chemical reactions. A chemical reaction involves a rearrangement of atoms in one or more reactants to form one or more
More informationChemical Calculations: Formula Masses, Moles, and Chemical Equations
Chemical Calculations: Formula Masses, Moles, and Chemical Equations Atomic Mass & Formula Mass Recall from Chapter Three that the average mass of an atom of a given element can be found on the periodic
More informationChapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases
Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties
More informationDecomposition. Composition
Decomposition 1. Solid ammonium carbonate is heated. 2. Solid calcium carbonate is heated. 3. Solid calcium sulfite is heated in a vacuum. Composition 1. Barium oxide is added to distilled water. 2. Phosphorus
More informationAPPENDIX B: EXERCISES
BUILDING CHEMISTRY LABORATORY SESSIONS APPENDIX B: EXERCISES Molecular mass, the mole, and mass percent Relative atomic and molecular mass Relative atomic mass (A r ) is a constant that expresses the ratio
More information