APS Science Curriculum Unit Planner

Transcription

1 Grade Level/Subject APS Science Curriculum Unit Planner Chemistry Stage 1: Desired Results Enduring Understanding Topic 5: Chemical Reactions: Matter exists, interacts, and changes. These changes can be classified by type. These changes can be affected by conditions in which they are performed.. Correlations Unifying Understanding VA SOL The student will investigate and understand how conservation of matter and energy is expressed in balanced equations. CH. 3 The student will investigate and understand how conservation of energy and matter is expressed in chemical formulas and balanced equations. Key concepts include b) balancing chemical equations; c) writing chemical formulas; d) bonding types; e) reaction types; and f) reaction rates, kinetics, and equilibrium. NSES (grade level) AAAS Atlas Essential Questions What causes a reaction? How do we predict reactions before they happen? Can change be predicted? How do the properties of a substance affect change? What factors affect the rate of a chemical reaction and why? How entropy and enthalpy affect the spontaneity of a chemical reaction? What is equilibrium? What is Le Chatlier s Principle? Knowledge and Skills Students should know Conservation of matter is represented in balanced chemical equations. A coefficient is a quantity that precedes a reactant or product formula in a chemical equation and indicates the relative number of particles involved in the reaction. 1

2 o Major types of chemical reactions are synthesis (A+B AB) decomposition (BC B + C single replacement (A+BC B+AC) double replacement (AC+BD AD+BC) neutralization (HX+MOH H2O + MX) combustion (CxHy + O2 CO2 + H2O). Kinetics is the study of reaction rates. Several factors affect reaction rates, including temperature, concentration, surface area, and the presence of a catalyst. Reaction rates/kinetics are affected by activation energy, catalysis, and the degree of randomness (entropy). Catalysts decrease the amount of activation energy needed. Chemical reactions based on the net heat energy are exothermic reactions (heat producing) and endothermic reactions (heat absorbing). Reactions occurring in both forward and reverse directions are reversible. Reversible reactions can reach a state of equilibrium, where reaction rates of the forward and reverse reactions are constant. Le Chatelier s Principle indicates the qualitative prediction of direction of change with temperature, pressure, and concentration. Students should be able to: Recognize the difference between physical and chemical changes. Write a balanced chemical equation of a reaction from the word description of the reaction. Classify types of chemical reactions as synthesis, decomposition, single replacement, double replacement, neutralization, and/or combustion. Balance chemical reactions Predict the products of a reaction Recognize that there is a natural tendency for systems to move in a direction of randomness (entropy). Recognize equations for redox reactions and neutralization reactions. Write the half reactions for oxidation and reduction reactions Distinguish between an endothermic and exothermic process. Interpret reaction rate diagrams. Identify and explain the effect of the following factors that affect the rate and time have on the rate of a chemical reaction: (catalyst, temperature, concentration, size of particles). Distinguish between irreversible reactions and those at equilibrium. Predict the shift in equilibrium when a system is subjected to a stress (Le Chatelier s Principle) and identify the factors that can cause a shift in equilibrium (temperature, pressure, and concentration.) 2

3 Prior Knowledge and Skills Stage 2: Assessment Evidence Matter can be described using both chemical and physical properties. Elements are the simplest form of matter that has a unique set of properties. A compound is a substance that contains two or more elements chemically combined in a fixed proportion. 4. Chemical formulas are used to represent compounds. Subscripts represent the relative number of each type of atom in a molecule or formula unit. The International Union of Pure and Applied Chemistry (IUPAC) system is used for naming compounds. Compounds have different properties than the elements from which they are composed. Bonds form between atoms to achieve stability. Covalent bonds involve the sharing of electrons between atoms. Ionic bonds involve the transfer of electrons between ions. Formative Assessment Summative Assessment Student participation Laboratory Reports Homework (readings, questions, and problems) Tests and Quizzes Laboratory assessment understanding models Stage 3: Learning Plan References to Adopted Materials Prentice Hall Chemistry: Text: Chapter 11: Chemical Reactions Chapter 17: Thermochemistry: Sections 17.1 and 17.2 pp Chapter 18: Rates of Reaction and Equilibrium Chapter 20: Section 20.1 pp Guided Reading and Study Workbook Chapter 11 pp Chapter 17 Sections 17.1 and 17.2 pp Chapter 18 pp Chapter 20 Section 20.1 pp Holt Chemistry: Text: Chapter 8: Chemical Equations and Reactions Chapter 10 Causes of Change Chapter 14: Chemical Equilibrium Chapter 16: Reaction Rates Chapter 17: Oxidation, Reduction and Electrochemistry Section1: Oxidation and Reduction Reactions Suggested Investigations Physical/Chemical Changes Lab - Students perform a series of reactions and determine if a 3

4 physical or chemical change occurred. Reactions to Equations Lab: In this experiment you will use common laboratory techniques to prepare three gases hydrogen, oxygen and carbon dioxide and you will verify the identities of the gases using splint tests. Then you will write and balance the chemical equations for the reactions observed. Activity Series Lab: The purpose of this lab is to perform a series of single replacement reactions, write the equations for the reactions that take place, and empirically determine the activity series for the metals tested. Reaction Kinetics: The Iodine Clock Reaction: One version is Flinn Scientific Catalog No AP4861 Balancing Reaction Cards - Students use cards to help learn balancing reactions. Teacher Demo: Cobalt Chloride Equilibrium Prentice Hall Activities p. 320 Inquiry Activity: Modeling Chemical Reactions p.345: Precipitation Reactions: Formation of Solids LM p.91 Laboratory 14: Types of Chemical Reactions LM p.97 Laboratory 15: Reactivity of Metals Teacher Demo p.325 TE: An Example of a Chemical Change (Sulfuric Acid and Sugar) Teacher Demo p.327 TE: Balance a Chemical Equation (Reaction of CuCl 2 with Aluminum Teacher Demo p.335 TE: Law of Conservation of Mass (Potassium Dichromate with Silver Nitrate.) Teacher Demo p..337 TE: Combustion of Iron Teacher Demo p.506 TE An Endothermic Reaction Teacher Demo p.515 TE: An Exothermic Reaction p. 540 Inquiry Activity: Temperature and Reaction Rates p.544 Quick Lab: Does Steel Burn? P. 550 Interpreting Graphics: Change in Concentration of Reactants and Products LM p Laboratory 36 : Factors Affecting Reaction Rates Holt Activities p.259 Start Up Activity: Observing a Chemical Reaction Teacher Demo p.268 TE Electrolysis of Water p.282 Quick Lab: Balancing Equations by Using Models Outdoor Education Applications None currently noted Resources Web Sites (use for chemical bonding animations and polarity) Fun, interactive, research--based simulations of physical phenomena from the PhET project at the University of Colora. Explorelearning.com Balancing Chemical Equations Collision Theory Chemical Equations 4

5 Videos Prentice Hall Chemistry Alive! Labs Burning Magnesium Methane Bubbles Grain Elevator Explosion Making Sodium Chloride Milk of Mangesia Thermite Reaction Grain Elevator Explosion Discovery Education ( Elements of Chemistry: Compounds and Reactions Clips- Chemical Reactions (3:29) and Ionic Bonding (3:21) Simple Science: Reaction Equations Clip- Naming Compounds and Balancing Equations (5:33) An Introduction to Le Chatelier s Principle Eight Segments (Total 29:05) Chemical Reactions 7 segments (Total 18:09) Dynamic Equilbrium Nine Segments (Total 295) Field Trips None currently noted Other Holt Chapter Resources on CD- ROM pg Concept Review: Ionic Bonding and Salts Holt Chapter Resources on CD- ROM pg Concept Review: Names and Formulas of Ionic Compounds Holt Chapter Resources on CD- ROM pg Concept Review: Covalent Bonds Holt Chapter Resources on CD- ROM pg Concept Review: Drawing and Naming Molecules Holt Chapter Resources on CD- ROM pg Concept Review: Molecular Shapes Holt Chapter Resources on CD- ROM pg Concept Review: Describing Chemical Reactions Holt Chapter Resources on CD- ROM pg Concept Review: Balancing Chemical Equations Holt Chapter Resources on CD- ROM pg Concept Review: Classifying Chemical Reactions Holt Chapter Resources on CD- ROM pg Concept Review : Writing Net Ionic Equations Holt Chapter Resources on CD- ROM pg Concept Review: States and State Changes Holt Chapter Resources on CD- ROM pg Concept Review: Intermolecular Forces Holt Chapter Resources on CD- ROM pg Concept Review: Energy of State Changes Holt Chapter Resources on CD- ROM pg Concept Review: Phase Equilibrium Holt Chapter Resources on CD- ROM pg Concept Review: Solutions Holt Chapter Resources on CD- ROM pg Concept Review: Solubility and the Dissolving Process Holt Chapter Resources on CD- ROM pg Concept Review: Physical Properties of 5

6 Solutions Holt Chapter Resources on CD- ROM pg Concept Review: Oxidation- Reduction Reaction Holt Chapter Resources on CD- ROM pg Concept Review: Introduction to Electrochemistry Holt Chapter Resources on CD- ROM pg Concept Review: Electrolytic Cells Holt Chapter Resources on CD- ROM pg 167 Concept Review: Names and Structures of Organic Compounds 6

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