Chemistry Curriculum Paterson School District 2005 Unit 1: Introduction to Chemistry and Matter Matter and Change, Measurements and Calculations Objectives: Introducing Chemistry as a Physical Science Explaining Matter and Its Properties Learning the Elements Reviewing the Scientific Method Understanding Units of Measurement Using Scientific Measurements Content: Defines the field of chemistry and distinguishes between different branches of chemistry Defines matter and contrasts major physical and chemical changes that matter can undergo Outlines the basic form of a chemical equation and describes how matter is classified Introduces the periodic table as a classification scheme for the elements with descriptions of metals, nonmetals, and Metalloids Covers the scientific method and its component activities, such as Observing, collecting data, formulating and testing hypotheses, and theorizing Presents Sl units of measurement, the concepts of mass and density, and the use of conversion factors Describes accuracy and precision, percent error, the use of significant figures and scientific notation, and steps to use in solving problems Skills: TSWBAT [The items with *** in front of them are for non-honors classes] *** Define chemistry • List examples of the branches of chemistry • Compare and contrast basic research, applied research, and technological development *** Distinguish between the physical or chemical properties of matter *** Classify changes of matter as physical or chemical *** Explain the gas, liquid, and solid states in terms of particles
Transcript
Chemistry Curriculum Paterson School District
2005 Unit 1: Introduction to Chemistry and Matter Matter and Change, Measurements and Calculations Objectives:
Introducing Chemistry as a Physical Science Explaining Matter and Its Properties Learning the Elements Reviewing the Scientific Method Understanding Units of Measurement Using Scientific Measurements
Content: Defines the field of chemistry and distinguishes between different branches of chemistry
Defines matter and contrasts major physical and chemical changes that matter can undergo
Outlines the basic form of a chemical equation and describes how matter is classified
Introduces the periodic table as a classification scheme for the elements with descriptions of metals, nonmetals, and Metalloids
Covers the scientific method and its component activities, such as Observing, collecting data, formulating and testing hypotheses, and theorizing
Presents Sl units of measurement, the concepts of mass and density, and the use of conversion factors
Describes accuracy and precision, percent error, the use of significant figures and scientific notation, and steps to use in solving problems
Skills: TSWBAT [The items with *** in front of them are for non-honors classes]
*** Define chemistry • List examples of the branches of chemistry • Compare and contrast basic research, applied research, and
technological development *** Distinguish between the physical or chemical properties of matter *** Classify changes of matter as physical or chemical *** Explain the gas, liquid, and solid states in terms of particles
*** Distinguish between a mixture and a pure substance, elements and symbols *** Use a periodic table to name elements, given their symbols *** Use a periodic table to write the symbols of elements, given their names *** Describe the arrangement of the periodic table ***List the characteristics that distinguish metals, nonmetals, and metalloids *** Describe the scientific method *** Distinguish between qualitative and quantitative observations *** Describe the differences between hypotheses, theories, laws, and models *** Distinguish between a quantity, a unit, and a measurement standard *** Name SI units for length, mass, time, volume, and density *** Distinguish between mass and weight *** Perform density calculations • Transform a statement of equality to a conversion *** Distinguish between accuracy and precision • Determine the number of significant figures in measurements • Perform mathematical operations involving significant figures *** Convert measurements into scientific notation • Distinguish between inversely and directly proportional relationships
Assessment:
Class Participation Objective Evaluation [Quizzes, Tests, Worksheets] Laboratory Homework Attitude
Projects and Products:
Density of Pennies, p. 39 Internet: www.scilinks.org
Alchemy, p. 8 (HC2011) Physical/chemical changes, p. 12 (HC2012) Periodic table, p. 20 (HC2013) Element names, p. 22 (HC2014) Scientific methods, p. 29 (HC2021) Sl units, p. 34 (HC2022) Detecting air pollution, p. 43 (HC2023) Significant figures, p. 46 (HC2024)
2005 Unit 2: Organization of Matter Atoms: The Building Blocks of
Matter, Arrangement of Electrons in Atoms, The Periodic Law, Chemical Bonding
Objectives:
Explain the Atom from Philosophical Idea to Scientific Theory Elucidate the Structure of the Atom Show the Counting Atoms Give the Chronology of the Development of a New Atomic Model Develop the Quantum Model of the Atom Demonstrate Electron Configurations Give the History of the Periodic Table Compare Electron Configuration and the Periodic Table Correlate Electron Configuration and Periodic Properties Introduce Chemical Bonding Identify Covalent Bonding and Molecular Compounds Explain Ionic Bonding and Ionic Compounds Consider Metallic Bonding Show and Explain Molecular Geometry
Content:
The history and development of atomic theory, from Democritus to Dalton to the modern era
The experiments that led to the discovery of the electron and the nucleus as well as the principal properties of these subatomic particles
The manner in which the number of atoms of an element and the number of subatomic particles inside atoms can be expressed and measured
The principles of electromagnetic radiation and the development of the Bohr model of the atom
The location of electrons around the nucleus from a wave -mechanical, or quantum, perspective using quantum numbers
The rules used to determine the electron configurations of the elements and introduces electron configuration notations
Mendeleev and other chemists in developing the periodic table and how the periodic law is used to predict elements' physical and chemical properties
The relationship between electron configuration and the arrangement of elements in groups, blocks, and periods of the periodic table, as well as the elements' general properties
Explores the relationship between the periodic law and electron
configuration, including trends in the properties of electron affinity, electronegativity, ionization energy, atomic radii, and ionic radii
Chemical bonding and uses electronegativity values to contrast polar-covalent, nonpolar-covalent, and ionic bonding
The characteristics of covalent bonding, including the relationship between bond length and bond strength and the use of Lewis structures
The characteristics of ionic bonding The characteristics of metallic bonding and the resulting properties
of metals Theories of molecular geometry, including VSEPR theory and
hybridization theory It also covers how intermolecular attraction is affected by molecular geometry
Skills: TSWBAT [The items marked with *** in front of them are for non-honors classes]
*** Explain the law of conservation of mass and the law of definite proportions • Explain the law of multiple proportions *** Summarize Dalton's atomic theory • Explain the relationship between Dalton's atomic theory and the
law of conservation of mass, the law of definite proportions, and the law of multiple proportions
• Summarize the observed properties of cathode rays that led to the discovery of the electron
• Summarize the experiment carried out by Rutherford and his coworkers that led to the discovery of the nucleus
*** List the properties of protons, neutrons, and electrons *** Define atom *** Explain what isotopes are *** Define atomic number and mass number, and describe how they apply to isotopes *** Given the identity of a nuclide, determine its number of protons, neutrons, and electrons *** Define mole in terms of Avogadro's number, and define molar mass *** Solve problems involving mass in grams, amount in moles, and number of atoms of an element • Explain the mathematical relationship among the speed,
wavelength, and frequency of electromagnetic radiation • Discuss the dual wave-particle nature of light • Discuss the significance of the photoelectric effect and the
line-emission spectrum of hydrogen to the development of the atomic model
*** Describe the Bohr model of the hydrogen atom • Discuss Louis de Broglie's role in the development of the
quantum model of the atom • Compare and contrast the Bohr model and the quantum model
of the atom • Explain how the Heisenberg uncertainty principle and the
Schroedinger wave equation led to the idea of atomic orbitals • List the four quantum numbers, and describe their significance *** Relate the number of sublevels corresponding to each of an atom's main energy levels, the number of orbitals per sublevel, and the number of orbitals per main energy level *** List the total number of electrons needed to fully occupy each main energy level • State the Aufbau principle, the Pauli exclusion principle, and
Hund's rule • Describe the electron configurations for the atoms of any
element using orbital notation, electron configuration notation, and, when appropriate, noble-gas notation
• Explain the roles of Mendeleev and Moseley in the development of the periodic table
*** Describe the modern periodic table *** Explain how the periodic law can be used to predict the physical and chemical properties of elements *** Describe how the elements belonging to a group of the periodic table are interrelated in terms of valence electrons • Describe the relationship between electrons in sublevels and
the length of each period of the periodic table *** Locate and name the four blocks of the periodic table and explain the reasons for these names • Discuss the relationship between group configurations and
group numbers *** Describe the locations in the periodic table and the general properties of the alkali metals, the alkaline earth metals, the halogens, and the noble gases *** Define electronegativity • Define atomic and ionic radii, ionization energy, and electron
affinity *** Compare the periodic trends of electronegativity and state the reasons for these variations • Compare the periodic trends of atomic radii, ionization energy
and state the reasons for these variations *** Define valence electrons, and state how many are present in atoms of each main-group element
• Compare the atomic radii, ionization energies, and electronegativities of the d-block elements with those of the main-group elements
*** Define chemical bond *** Explain why most atoms form chemical bonds *** Describe ionic and covalent bonding • Explain why most chemical bonding is neither purely ionic nor
purely covalent *** Classify bonding type according to electronegativity differences *** Define molecule and molecular formula • Explain the relationships between potential energy, distance
between approaching atoms, bond length, and bond energy *** State the octet rule • List the six basic steps used in writing Lewis structures • Explain how to determine Lewis structures for molecules
containing single bonds, multiple bonds, or both *** Draw single Lewis dot structures for atoms and simple molecules • Explain why scientists use resonance structures to represent
some molecules • Compare and contrast a chemical formula for a molecular
compound with one for an ionic compound • Discuss the arrangements: of ions in crystals • Define lattice energy and explain its significance *** Compare the distinctive properties of ionic and molecular compounds • Write the Lewis structure for a polyatomic ion given the identity
of the atoms combined and other appropriate information • Describe the electron-sea model of metallic bonding, and
explain why metals are good electrical conductors • Explain why metal surfaces are shiny • Explain why metals are malleable and ductile but ionic-crystal
line compounds are not • Explain VSEPR theory • Predict the shapes of molecules or polyatomic ions using
VSEPR theory • Explain how the shapes of molecules are accounted for by
hybridization theory *** Describe dipole-dipole forces and hydrogen bonding • Describe induced dipoles and London dispersion forces • Explain what determines molecular polarity
Assessment:
Class Participation Objective Evaluation [Quizzes, Tests, Worksheets]
Laboratory Homework Attitude
Projects and Products:
Constructing a Model, p. 69 The Wave Nature of Light: Interference, p. 100 Designing Your Own Periodic Table, p. 127 Internet: www.scilinks.org
Atomic theory, p. 66 (HC2031) Carbon, p. 67 (HC2032) Subatomic particles, p. 71 (HC2033) Isotopes, p. 77 (HC2034) Electromagnetic spectrum, p. 91 (HC2041) Photoelectric effect, p. 93 (HC2042) William Ramsay, p. 108 (HC2043) Periodic table, p. 123 (HC2051) Noble gases, p. 125 (HC2052) Alkali metals, p. 133 (HC2053) Alkaline earth metals, p. 133 (HC2054) Halogens, p. 137 (HC2055) Covalent bonding, p. 162 (HC2061) Ultrasound, p. 166 (HC2062) Ionic bonding, p. 177 (HC2063) Metallic bonding, p. 181 (HC2064) VSEPR theory, p. 185 (HC2065) Hydrogen bonding, p. 192 (HC2066)
Laboratory: 3-1 Conservation of Mass 798 4-1 Flame Tests 801 Resources:
Text: Modern Chemistry; Holt, Rinehart and Winston, 2000 Handouts Internet Articles Virtual Activities
2005 Unit 3: Language of Chemistry Chemical Formulas and
Chemical Compounds, Chemical Equations and Reactions, Stoichiometry, Chemical Equations and Reactions
Objectives:
Understanding Chemical Names and Formulas Introduction to Oxidation Numbers Practice in Using Chemical Formulas Determining Chemical Formulas How to Describe Chemical Reactions Recognize the Different Types of Chemical Reactions Learn the Theory and Use of the Activity Series of the Elements Introduction to Stoichiometry Stoichiometric Calculations Determination of Limiting Reactants and Percent Yield
Content:
The naming of binary ionic and molecular compounds How oxidation numbers are assigned and the Stock system of naming
compounds How to calculate formula masses, molar masses, and percentage
compositions How to determine chemical formulas from percentage compositions
and empirical data Description of Chemical Reactions Types of Chemical Reactions Activity Series of the Elements Definition of mole ratio and introduction to molar mass as a conversion
factor in solving stoichiometry problems. Demonstration of solutions to problems involving conversions from
moles of given to moles of unknown, from moles to mass, from mass to moles, and from mass to mass
Explains the concepts of limiting reactant and percent yield and provides strategies for solving problems based on these concepts
Skills: TSWBAT [The items with *** in front of them are for non-honors classes]
*** Explain the significance of a chemical formula
*** Determine the formula of an ionic compound formed between two given ions *** Name an ionic compound given its formula *** Using prefixes, name a binary molecular compound from its formula *** Write the formula of a binary molecular compound given its name *** Assign oxidation numbers *** Give the oxidation number for each element in the formula of a chemical compound *** Name binary molecular compounds *** Calculate the formula mass or molar mass of any given compound *** Use molar mass to convert between mass in grams and amount in moles of a chemical compound • Calculate the number of molecules, formula units, or ions in a
given molar amount of a chemical compound *** Calculate the percentage composition of a given chemical compound • Define empirical formula, and explain how the term applies to
ionic and molecular compounds • Determine an empirical formula from either a percentage or a
mass composition *** Explain the relationship between the empirical formula and the molecular formula of a given compound • Determine a molecular formula from an empirical formula *** Give observations that suggest that a chemical reaction has taken place *** Know the requirements for a correctly written chemical equation *** Write a word equation and a formula equation for a given chemical reaction
*** Balance a formula equation by inspection *** Define and give general equations for synthesis, decomposition, single-replacement, and double replacement reactions
*** Classify a reaction as synthesis, decomposition, single replacement, double replacement, or combustion • List three types of synthesis reactions and six types of
decomposition reactions • List four types of single replacement reactions and three types
of double replacement reactions *** Predict the products of simple reactions given the reactants
• Explain the significance of an activity series • Use an activity series to predict whether a given reaction will
occur and what the products will be *** Define stoichiometry • Describe the importance of the mole ratio in stoichiometric
calculations *** Write a mole ratio relating two substances in a chemical equation *** Calculate the amount in moles of a reactant or product from the amount in moles of a different reactant or product *** Calculate the mass of a reactant or product from the amount in moles of a different reactant or product *** Calculate the amount in moles of a reactant or product from the mass of a different reactant or product *** Calculate the mass of a reactant or product from the mass of a different reactant or product • Describe a method for determining which of two reactants is a
limiting reactant • Calculate the amount in moles or mass in grams of a product,
given the amounts in moles or masses in grams of two reactants, one of which is in excess
*** Distinguish between theoretical yield, actual yield, and percent yield *** Calculate percent yield, given the actual yield and quantity of a reactant
Assessment:
Class Participation Objective Evaluation [Quizzes, Tests, Worksheets] Laboratory Homework Attitude
Projects and Products:
Balancing Equations Using Models, p. 264 Limiting Reactants in a Recipe, p. 292 Internet: www.scilinks.org
Chemical Formulas, p.203 (HC2071) Acids, p. 214 (HC2072) Photochemical Reaction, p. 221 (HC2073) Chemical Reactions, p. 242 (HC2081) Chloroform, p. 255 (HC2082) Precipitate, p. 262 (HC2083 Activity Series, p. 265 (HC2084 Acid Water, p. 268 (HC2085)
Lavoisier, p. 279 (HC2091) Laboratory: Pre-Lab Gravimetric Analysis p. 804 7-1 Separation of Salts by Fractional Crystallization p. 806 7-2 Naming Ionic Compounds p. 810 7-3 Determining the Empirical Formula of Magnesium Oxide p. 813 9-1 Mass and Mole Relationships in a Chemical Reaction p. 816 9-2 Stoichiometry and Gravimetric Analysis p. 819 Resources:
Text: Modern Chemistry; Holt, Rinehart and Winston, 2000 Handouts Internet Articles Virtual Activities
Unit 4: Phases of Matter Physical Characteristics of Gases Molecular Composition of Gases Liquids and Solids
Objectives: Explaining The Kinetic Molecular Theory of Matter Defining and Measuring Pressure Stating and Applying the Gas Laws Relating Volume and Mass of Gases Describing the Ideal Gas Law Calculating the Stoichiometry of Reactions involving Gases Defining Effusion and Diffusion and Explaining the Factors Affecting
the Rate of Them Describing the Properties and the Changes of Liquids Describing the Properties and the Changes of Solids Explaining the Changing Process of States of Matter Describing the Structure and the Properties of Water
Contents:
How pressure is measured Conversion units of pressure Introduction of the kinetic molecular theory of matter How the theory accounts for certain physical properties of ideal
gases, which differ from real gases Definition of pressure and standard pressure in terms of force Gas laws that express simple mathematical relationships between
the pressure, temperature, volume, and quantity of gases The relationships between the volume, mass, and number of
particles of a gas Avogadro’s law that leads to the concept of molar volume of a gas Derivation of the ideal gas law, which is put to practical use in
calculations How to use the relationship between the volume and moles of a
gas to carry out stoichiometric calculations from chemical reactions The relationship between the mass of gas particles and their rate of
effusion Using the kinetic-molecular theory to describe properties of liquids
and explain changes of state involving liquids Describes the properties of solids, contrasts them with liquid
properties, and explains them of the basis of the kinetic-molecular theory
Changes of state and the factors that determine them
The concept of equilibrium in terms of changes of state The structure, physical properties, and changes of state of water
Skills: TSWBAT [The items with *** in front of them are for non-honors classes]
*** State the kinetic-molecular theory of matter, and describe how it explains certain properties of matter *** Define the terms ideal gas and real gas *** Describe each of the following characteristic properties of gases: expansion, density, fluidity, compressibility, diffusion, and effusion *** Describe the conditions under which a real gas deviates from “ ideal” behavior *** Define pressure and relate it to force *** Know how pressure is measured • Convert units of pressure *** State the standard conditions of temperature and pressure • Use the kinetic-molecular theory to explain the relationships
between gas volume, temperature, and pressure • Use Boyle’s law to calculate volume-pressure changes at
constant temperature • Use Charles’s law to calculate volume-temperature changes
at constant pressure • Use Gay-Lussac’s law to calculate pressure-temperature
changes at constant volume *** Use the combined gas law to calculate volume-temperature-pressure changes *** Use Dalton’s law of partial pressures to calculate partial pressures and total pressures • State the law of combining volumes *** State Avogadro’s law and explain its significance *** Define standard molar volume of a gas • Use standard molar volume to calculate the molar mass of a
gas *** State the ideal gas law • Derive the ideal gas constant and discuss its units *** Using the ideal gas law, calculate pressure, volume, temperature, or amount of gas when the other three quantities are known • Using the ideal gas law, calculate the molar mass or density
of a gas • Reduce the ideal gas law to Boyle’s law, Charles’s law, and
Avogadro’s law.
• Describe the conditions under which each applies • Explain how Gay-Lussac’s law and Avogadro’s law apply to
the volumes of gases in chemical reactions *** Use a chemical equation to specify volume ratios for gaseous reactants or products, or both *** Use volume ratios and the gas laws to calculate volumes, masses, or molar amounts of gaseous reactants or products • State Graham’s law of effusion • Determine the relative rates of effusion of two gases of
known molar masses • State the relationship between the molecular velocities of
two gases and their molar masses *** Describe the motion of particles in liquids and the properties of liquids according to the kinetic-molecular theory *** Discuss the process by which liquids can change into a gas. *** Define vaporization • Discuss the process by which liquids can change into a
solid. Define freezing *** Describe the motion of particles in solids and the properties of solids according to the kinetic-molecular theory • Distinguish between the two types of solids • Describe the different types of crystal symmetry. Define
crystal structure and unit cell *** Explain the relationship between equilibrium and changes of state • Predict changes in equilibrium using Le Chatelier’s principle *** Explain what is mean by equilibrium vapor pressure *** Describe the processes of boiling, condensation, freezing, melting, deposition and sublimation • Interpret phase diagrams *** Describe the structure of a water molecule *** Discuss the physical properties of water. Explain how they are determined by the structure of water • Calculate the amount of heat energy absorbed or released
when a quantity of water changes state Assessment:
Class Participation Objective Evaluation [Quizzes, Tests, Worksheets] Laboratory Homework Attitude
Projects and Products: Diffusion. p.353 Internet: www.scilinks.org
Gases, p.303 (HC2101) Diffusion/effusion, p.305 (HC2102) Carbon monoxide, p.307 (HC2103) Gas laws, p.314 (HC2104) Avogadro’s law, p.333 (HC2111) Torricelli, p. 338 (HC2112) Robert Boyle, p.338 (HC2113) Thomas Graham, p.352 (HC2114) Properties of liquids, p.363 (HC2121) Crystalline solids, p.370 (HC2122) Factors affecting equilibrium, p.372 (HC2123) Volatile/nonvolatile liquids, p.377 (HC2124)
Laboratory: 12-1 "Wet" Dry ice p. 822 12-2 Measuring the Triple Point Pressure Of C02 p. 824 Resources:
Text: Modern Chemistry: Holt, Rinehart and Winston, 2002 Handouts Internet Articles Virtual Activities
2005 Unit 5: Solutions and Their Behavior Solutions, Ions in
Aqueous Solutions and Colligative Properties, Acids and Bases, Acid-Base Titration and pH
Objectives:
Relating Types of Mixtures Understanding the Solution Process Determining the Concentration of Solutions Evaluating Compounds in Aqueous Solutions Recognizing Colligative Properties of Solutions Understanding the Properties of Acids and Bases Learning Acid-Base Theories Relating Acid-Base Reactions Understanding Aqueous Solutions and the Concept of pH How to Determine pH and Titrations
Content:
Characteristics that distinguish solutions from suspensions and colloids
The physical and chemical factors that affect solubility Concentration expressed as molarity and molality with calculations The dissociation of ionic compounds and the ionization of some
molecular compounds when they dissolve in water Strong and weak electrolytes How precipitation reactions occur Methods of writing ionic equations for precipitation reactions Description and mathematics of boiling-point elevation and
freezing-point depression The mechanism of osmosis and the cause of osmotic pressure Description of acids and bases Arrhenius acids and bases Acid-base nomenclature and strong and weak acids and bases The Bronsted-Lowry and Lewis theories Acid-base reactions in aqueous solutions The ionization of water and the equilibrium concentrations of H30+
and OH- in water and in aqueous solutions of acids and bases The mathematical concept of pH How acid-base indicators work and how indicators, pH meters, and
titrations are used to determine the pH of a solution
Skills: TSWBAT [The items with *** in front of them are for non-honors classes]
*** Distinguish between heterogeneous and homogeneous mixtures • List three different solute solvent combinations *** Compare the properties of suspensions, colloids, and solutions *** Distinguish between electrolytes and nonelectrolytes *** List and explain three factors that affect the rate at which a solid solute dissolves in a liquid solvent *** Explain solution equilibrium, and distinguish among saturated, unsaturated, and supersaturated solutions *** Explain the meaning of "like dissolves like" in terms of polar and nonpolar substances • List the three interactions that contribute to the heat of solution,
and explain what causes dissolution to be exothermic or endothermic
*** Compare the effects of temperature and pressure on solubility • Given the mass of solute and volume of solvent, calculate the
concentration of a solution *** Given the moles of solute and volume of solution, calculate the molarity of a solution *** Given the concentration of a solution, determine the amount of solute in a given amount of solution *** Given the concentration of a solution, determine the amount of solution that contains a given amount of solute *** Write equations for the dissolution of soluble ionic compounds in water *** Predict whether a precipitate will form when solutions of soluble ionic compounds are combined, and write net ionic equations for precipitation reactions • Compare dissociation of ionic compounds with ionization of
molecular compounds • Draw the structure of the hydronium ion, and explain why it is
used to represent the hydrogen ion in solution *** Distinguish between strong electrolytes and weak electrolytes *** Identify four colligative properties, and explain why they are classified as colligative properties • Calculate freezing-point depression, boiling-point elevation, and
solution molality of nonelectrolytic solutions • Calculate the expected changes in freezing point and boiling
point of an electrolytic solution
• Discuss causes of the differences between expected and experimentally observed colligative properties of electrolytic solutions
*** List general properties of aqueous acids and bases *** Name common binary acids and oxyacids, given their chemical formulas • List five acids commonly used in industry and the laboratory,
and give two properties of each *** Define acid and base according to Arrhenius's theory of ionization *** Explain the differences between strong and weak acids and bases • Define and recognize Bronsted-Lowry acids and bases • Define a Lewis acid and a Lewis base • Name compounds that are acids under the Lewis definition but
are not acids under the Bronsted-Lowry definition • Describe a conjugate acid, a conjugate base, and an
amphoteric compound *** Explain the process of neutralization • Explain how acid rain damages marble structures *** Describe the ionization of water *** Define pH, and give the pH of a neutral solution at 25'C *** Explain and use the pH scale *** Given [H30+] or [OH-], find pH [in whole numbers] *** Given pH, find [H30+] or [OH-] [in whole numbers]
Assessment:
Class Participation Objective Evaluation [Quizzes, Tests, Worksheets] Laboratory Homework Attitude
Projects and Products:
Observing Solutions, Suspensions, and Colloids, p. 399 Household Acids and Bases, p.458 Testing the pH of Rainwater, p. 496 Internet: www.scilinks.org
Solutions, p. 397 (HC2131) Colloids, p. 397 (HC2132) Electrolytes/nonelectrolytes, p. 399 (HC2133) Perfluorcarbons, p. 411 (HC2134) Precipitation reactions, p. 427 (HC2141) Hydronium ion, p. 431 (HC2142) Electrolysis, p. 435 (HC2143)
Osmosis, P. 442 (HC2144) Acids, p. 456 (HC2151) Bases, p. 457 (HC2152) Household acids and bases, p. 458 (HC 2153) Salt, p. 474 (HC2154) pH, p. 481 (HC2161) Acid rain, p. 492 (HC2162) Titration/indicators, p. 499 (HC2163)
Laboratory: Pre-Lab Paper Chromatography p. 828 13-1 Separation of Pen Inks by Paper Chromatography p. 830 13-2 Colorimetry and Molarity p. 834 14-1 Testing Water, p. 838 Pre-Lab Volumetric Analysis p. 842 16-1 How Much Calcium Carbonate Is in an Eggshell? p. 844 16-2 Investigating Overwrite Marking Pens p.848 16-3 Is It an Acid or a Base? p. 851 16-4 Percentage of Acetic Acid in Vinegar p. 854 Resources:
Text: Modern Chemistry; Holt, Rinehart and Winston, 2000 Handouts Internet Articles Virtual Activities
2005 Unit 6: Chemical Reactions: Reaction Energy and Reaction
Kinetics Chemical Equilibrium, Oxidation-Reduction Reactions
Objectives:
Explaining, and Calculating the Heat Transfers in Reactions- Thermochemistry
Discussing the Driving Force of Reactions Explaining the Process of a Reaction Defining, and Calculating the Reaction Rate
and Discussing the factors influencing the rate Explaining The Nature of Chemical Equilibrium Discussing the ways of Shifting Equilibrium Describing the Equilibria of Acids, Bases, and
Salts Applying the Principles of Equilibrium to
saturated solutions of sparingly soluble salts Assigning Oxidation Numbers to substances
and Explaining Oxidation and Reduction Balancing Redox Equations Recognizing Oxidizing and Reducing Agents Describing how to use redox reactions to
produce Electrochemical cells
Contents: Heat; temperature; heats of reaction,
formation, and combustion; and enthalpy change
How to use enthalpy, entropy, and free energy to predict whether a reaction will occur
Collision theory and activation energy to describe the mechanisms by which chemical reactions take place
The factors that influence the rate of a chemical reaction and shows how to calculate the reaction rate from experimental data
Reversible reactions, the state of equilibrium, and K, the equilibrium constant
The shift of equilibria in response to changes in concentration, pressure and temperature and discusses the common-ion effect
The equilibria of acids, bases, and salts; explains the acid-ionization constant, Ka; and discusses buffering and hydrolysis
Solubility equilibria and explains calculations involving the solubility-product constant, Ksp, and precipitate formation
Oxidation and reduction reactions and provides rules for determining oxidation numbers
Guidelines for balancing redox equations by using the half-reaction method
The roles of the oxidizing agent and the reducing agent in a redox reaction
The operation of electrochemical cells and distinguishes between voltaic cells and electrolytic cells
Skills: TSWBAT [The items with *** in front of them are for non-honors classes]
*** Define temperature and state the units in which it is measured *** Define heat and state its units *** Perform specific-heat calculations ***Explain heat of reaction, heat of formation, heat of combustion, and enthalpy change • Solve problems involving heats of reaction,
heats of formation, and heats of combustion • Explain the relationship between enthalpy
change and the tendency of a reaction to occur
• Explain the relationship between entropy change and the tendency of a reaction to occur
• Discuss the concept of free energy, and explain how the value of this quantity is calculated and interpreted
• Describe the use of free energy change to determine the tendency of a reaction to occur
*** Explain the concept of reaction mechanism *** Use the collision theory to interpret chemical reactions • Define activated complex *** Define activation energy *** Define chemical kinetics
• Relate activation energy to heat of reaction • Define chemical kinetics, and explain the
two conditions necessary for chemical reactions to occur
*** Discuss the factors that influence reaction rate *** Define catalyst, and discuss two different types • Explain and write rate laws for chemical
reactions *** Define chemical equilibrium *** Explain the equilibrium constant • Write chemical equilibrium expressions and
carry out calculations involving them *** Discuss the factors that disturb equilibrium • Discuss conditions under which reactions
go to completion *** Describe the common-ion effect • Explain the concept of acid-ionization
constants, and write acid-ionization equilibrium expressions
*** Review the ionization constant of water *** Explain buffering • Compare cation and anion hydrolysis • Explain what is meant by solubility-product
constants, and calculate their values • Calculate solubilities using solubility-
product constants • Carry out calculations to predict whether
precipitates will form when solutions are combined
• Assign oxidation numbers to reactant and product species
*** Define oxidation and reduction *** Explain what an oxidation-reduction reaction (redox reaction) is • Explain what must be conserved in redox
equations • Balance redox equations by using the half-
reaction method • Relate chemical activity to oxidizing and
reducing strength • Explain the concept of auto-oxidation • Explain what is required for an
electrochemical cell
*** Describe the nature of voltaic cells *** Describe the nature of electrolytic cells *** Explain the process of electroplating • Describe the chemistry of a rechargeable
cell • Calculate cell potentials from a table of
standard electrode potentials Assessment
Class Participation Objective Evaluation [Quizzes, Tests, Worksheets] Laboratory Homework Attitude
Laboratory: Pre-LabCalorimetry p. 858 17-1 Measuring the Specific Heats of Metals p. 860 17-2 Calorimetry and Hess's Law p. 864 17-3 Rate of a Chemical Reaction p. 868 18-1 Equilibrium Expressions p. 871 18-2 Measuring Ka for Acetic Acid p. 875 19-1 Blueprint Paper p.878 19-2 Reduction of Manganese in Permanganate Ion p.881 Resources:
Text: Modern Chemistry; Holt, Rinehart and Winston, 2000 Handouts Internet Articles
Explaining the Structure and the Stability of The Nucleus Recognizing the Different Types of Radioactive Decay Describing the Applications of Nuclear Radiation Defining and Comparing Nuclear Fission and Nuclear Fusion
Content:
Identifies the forces that affect the stability of the nucleus How to write balanced nuclear equations Outlines the different types of radioactive decay and
demonstrates calculations involving the half-life of an isotope Surveys the penetrating ability of nuclear radiation and methods
for detecting radiation Describes some common applications of nuclear radiation Explains the difference between fission and fusion and
discusses their uses and potential uses as energy sources
Skills: TSWBAT
• Explain what a nuclide is, and describe the different ways nuclides can be represented
• Define and relate the terms mass defect and nuclear binding energy
• Explain the relationship between nucleon number and stability of nuclei
• Explain why nuclear reactions occur, and know how to balance a nuclear equation
• Define and relate the terms radioactive decay and nuclear radiation
• Describe the different types of radioactive decay and their effects on the nucleus
• Define the term half-life, and explain how it relates to the stability of a nucleus
• Define and relate the terms decay series, parent nuclide, and daughter nuclide
• Explain how artificial radioactive nuclides are made, and discuss their significance
• Compare the penetrating ability and shielding requirements of alpha particles, beta particles, and gamma rays
• Define the terms roentgen and rem, and distinguish between them
• Describe the devices used in radiation detection • Discuss applications of radioactive nuclides • Define nuclear fission, chain reaction, and nuclear fusion,
and distinguish between them • Explain how a fission reaction is used to generate power • Discuss the possible benefits and the current difficulty of
