Chemistry Standards of Learning Curriculum Guide

Transcription

1 Scientific Investigation Introduction to Chemistry CH.1 a, b, c, d, e, i understand that experiments in which variables are measured, analyzed, and evaluated, produce observations and verifiable data. Key concepts include a) designated laboratory techniques; b) safe use of chemical and equipment; c) proper response to emergency situations; d) manipulation of multiple variables with repeated trials; e) accurate recording organizing, and analysis of data through repeated trials; i) construction and defense of a scientific viewpoint (the nature of science). Review experimental design used in scientific investigation. Identify the following basic lab equipment: breaker, flask, graduated cylinder, test tube, test tube rack, test tube holder, ring stand, wire gauze, clay triangle, crucible with lid, evaporation dish, watch glass, wash bottle, and dropping pipette. Identify, locate, and know how to use laboratory safety equipment including aprons, goggles, gloves, fire extinguishers, fire blanket, safety shower, eye wash, broken glass container, and fume hood. Understand and demonstrate: MSDS warnings: handling, lethal dosage, hazards, disposal, clean-up Safety rules for science Laboratory safety cautions Safe techniques and procedures CH.1 a, b, c, d, e, i ChemA 1 st /4 th (4 Days) Demonstration experiments Video Lab equipment samples Equipment Identification Sheets Safety Test Have Students sign Safety Pledge Safety Video: - Accident At Jefferson High Demonstrations Chromatography Lab Lab practical Laser Discs Safety in Science Teaching manual New Pathways To Chemistry Modules #3, #5, #9, #15 Teaching Science Web Page Demonstrate the following basic lab techniques: filtering, decanting, using chromatography, lighting gas burners. Danville Public Schools, 2003 (Revised 10/21/2003) 1 Chemistry

2 Structures and Periodic Properties of Matter Introduction to Chemistry Electron Configuration and the Periodic Table CH.2 d, h understand that the placement of elements on the periodic table is a function of their atomic structure. The periodic table is a tool used for the investigations of d) families or groups; and h) chemical and physical properties. CH.1 a, b, c, h understand that experiments in which variables are measured, analyzed, and evaluated, produce observations and verifiable data. Key concepts include a) designated laboratory techniques; b) safe use of chemicals and equipment; c) proper response to emergency situations. d) manipulation of multiple variables with repeated trials; h) the use of appropriate technology including computers, graphing calculators, and probeware for gathering data and communicating results; Review definitions and identification of physical and chemical properties. Differentiate between elements, compounds, heterogeneous mixtures, and homogeneous mixtures (solutions). Recognize the following physical properties: density, conductivity, melting point, boiling point, malleability, ductility, and specific heat capacity. Recognize that reactivity is the tendency of an element to enter into a chemical reaction. Use probes, graphing calculators, and balances using graduated scale plus the estimated digit to gather data. Make the following measurements using appropriate equipment: volume, mass, temperature, and pressure. Review location and use of safety equipment. CH.2 d, h CH.1 a, b, c, h ChemA 1 st /4 th (3 days) Video A Matter Of States Demonstration Phillip Morrison Video Lab (Probes From Math Dept., MCL Equipment Demonstration Video Lab practical Reference materials such as Handbooks Probes with calculators or computers Safety in Science Teaching manual Danville Public Schools, 2003 (Revised 10/21/2003) 2 Chemistry

3 Structure and Periodic Introduction to Chemistry Properties of Matter Electron Configuration and the Periodic Table Applications CH.1 a, d, e, f, g understand that experiments in which variables are measured, analyzed, and evaluated, produce observations and verifiable data. Key concepts include a) designated laboratory techniques; d) manipulation of multiple variables with repeated trials; and e) accurate recording, organizing, and analysis of data through repeated trials. f) mathematical and procedural error analysis; and g) mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis). Understand: SI and Metric Units SI and Metric Conversions using factor-label method (dimensional analysis) Calculation of the mean of a set of measurements Know: Most frequently used SI prefixes (m, c, d, k) Identification of variables Procedural errors and their elimination Be able to: Design and perform experiments to test predictions Identify variables Predict outcome(s) when a variable is changed Record data using significant digits CH.1 a, d, e, f, g Ch.2 a, b ChemA 1 st /4 th (20 days) Problem sets Lab practical Graphing calculators Electronic balances Periodic Table Utilize graphing data: Dependent and independent variables Danville Public Schools, 2003 (Revised 10/21/2003) 3 Chemistry

4 Structure and Periodic Introduction to Chemistry Properties of Matter Electron Configuration and the Periodic Table CH.2 a, b understand that the placement of elements on the periodic table is a function of their atomic structure. The periodic table is a tool used for the investigations of a) average atomic mass, mass number, and atomic number; b) isotopes, half lives, and radioactive decay; Scale and units Line of best fit (regression line) Illustrate that: Scientific notation is used to write very small and very large numbers. The last digit of any valid measurement must be estimated and is therefore uncertain. Significant digits and scientific rules for calculations. Make the following measurements using the specified equipment: Volume: graduated cylinder, pipette, volumetric flask, buret Mass: electronic or dial-a-gram balances Demonstration Significant Figures Lab Applications Demonstrate precision in measurement. Understand accuracy in terms of closeness to the true value of a measure. Danville Public Schools, 2003 (Revised 10/21/2003) 4 Chemistry

5 Structure and Periodic Introduction to Chemistry Properties of Matter Electron Configuration and the Periodic Table Applications Review location, charge, and relative size of subatomic particles electron, proton, and neutron. Explain the following relationships: The atomic number of an element is the same as the number of protons In a neutral atom, the number of electrons is the same as the number of protons. The average mass for each element is the weighted average of that element s naturally occurring isotopes. Calculate relative atomic mass. Explain the following: An isotope is an atom that has a different number of neutrons than other atoms of the same element. Some isotopes are radioactive; many are not. Half-life is the length of time required for half of a given sample of a radioactive isotope to decay. Demonstration Practice s Lab practical Reference materials such as Handbooks Demonstratio n-size periodic table Student notebook-size periodic table Laser discs Danville Public Schools, 2003 (Revised 10/21/2003) 5 Chemistry

6 Structure and Periodic Structure CH. 2 b, i understand that the placement of elements on the periodic table is a function of their atomic structure. The periodic table is a tool used for the investigations of b) isotopes, half lives, and radioactive decay; i) historical and quantum models. Determine the half-life of a radioactive substance. Describe alpha, beta, and gamma radiation with respect to penetrating power and composition. Identify the modern atomic theory as the Quantum Mechanical Model. CH.2 b, i ChemA 2 nd /5 th (3 days) Electron Configuration and the Periodic Table Applications Danville Public Schools, 2003 (Revised 10/21/2003) 6 Chemistry

7 Structure and Periodic Structure Electron Configuration and the Periodic Table Applications CH.2 a, b, c, d, e, f understand that the placement of elements on the periodic table is a function of their atomic structure. The periodic table is a tool used for the investigations of a) average atomic mass, mass number, and atomic number; b) isotopes, half lives, and radioactive decay; c) characteristics of subatomic particles as to mass and charge; d) families or groups; e) series and periods; f) trends including atomic radii, electronegativity, shielding effect, and ionization energy; For any neutral atom of a particular element, use the periodic table to determine atomic number, atomic mass, the number of protons, the number of electrons, and the number of neutrons. State and identify the location of the following on the periodic table: alkali metals, alkaline earth metals, transition metals, halogens, inert gases, and metalloids. Determine that: Vertical columns called groups have similar properties because of similar valence electron configurations. Horizontal rows called periods have predictable properties based on an increasing number of outer orbital electrons. Periods and groups are named by numbering columns and rows Some elements are diatomic list CH.2 a, b, c, d, e, f ChemA 2 nd /5 th (8 days) Periodic Table Practice Worksheets Trends On The Periodic Table World of Chemistry Video Periodic Table Student lab reports Periodic table Orbital models Danville Public Schools, 2003 (Revised 10/21/2003) 7 Chemistry

8 Scientific Investigation Structure and Periodic Structure Electron Configuration and the Periodic Table Applications CH.2 i understand that the placement of elements on the periodic table is a function of their atomic structure. The periodic table is a tool used for the investigations of historical and quantum models. CH.1 e, g, i understand that experiments in which variables are measured, analyzed, and evaluated, produce observations and verifiable data. Key concepts include e) accurate recording, organizing, and analysis of data through repeated trials. g) mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis). i) construction and defense of a scientific viewpoint (the nature of science). Graph data to determine relationships and trends electronegativity, shielding effect, atomic radius, ionization energy Recognize that discoveries and insights have changed the model of the atom over time. Relate the following major insights regarding the atomic model to the principal scientists listed below: Particles Democritus First atomic theory of matter John Dalton Discovery of the electron J. J. Thomson Discovery of the nucleus Rutherford Discovery of charge of electron Millikan Planetary model of atom Neils Bohr Periodic table Mendeleev Periodic table by atomic number Mosely Quantum of energy Planck Uncertainty principle CH.2 i CH.1 e, g, i ChemA 2 nd /5 th (3 days) Boiling Curve Lab World of Chemistry Video The Atom Lab practical Reference materials such as Handbooks Demonstratio n-size periodic table Student notebook-size periodic table Laser discs Danville Public Schools, 2003 (Revised 10/21/2003) 8 Chemistry

9 Formulas, and Reactions Reactions and Equations CH.3 a, c, d understand how conservation of energy and matter is expressed in chemical formulas and balanced equations. Key concepts include a) nomenclature; c) writing chemical formulas (molecular, structural, empirical, and Lewis diagrams); d) bonding types (ionic, covalent); Recognize that bonds form to achieve stability. Explain the Law of Multiple Proportions. Identify and use: empirical, molecular, and structural formulas Subscripts Name binary compounds using the Stock system (Roman numerals). Recognize and use polyatomic ions such as carbonate, sulfate, nitrate, hydroxide, phosphate, and ammonia. Know chemical formulas for certain common substances (water, carbon monoxide, carbon dioxide, sulfur dioxide, and carbon tetrafluoride). CH.3 a, d, c ChemA 2 nd /5 th (9 days) Periodic Table Formula Graphing Trends Student lab reports size periodic table Student notebook-size periodic table Models of molecular shapes Danville Public Schools, 2003 (Revised 10/21/2003) 9 Chemistry

10 Structure and Periodic Structure Electron Configuration and the Periodic Table Applications CH.2 a, b, c, g understand that the placement of elements on the periodic table is a function of their atomic structure. The periodic table is a tool used for the investigations of a) average atomic mass, mass number, and atomic number; b) isotopes, half lives, and radioactive decay; c) characteristics of subatomic particles as to mass and charge; g) mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis). Illustrate how negative and positive ions are formed and how to represent them. Recognize that transition metals can have multiple oxidation states. Name and write formulas for certain elements that naturally occur as diatomic molecules (oxygen, hydrogen, nitrogen). CH.2 a, b, c, g ChemA 2 nd /5 th (2 Day) Danville Public Schools, 2003 (Revised 10/21/2003) 10 Chemistry

11 Molar Scientific Investigation Stoichiometry Reactions and Equations CH.4 a, b understand that quantities in a chemical reaction are based on molar relationships. Key concepts include a) Avogadro's principle and molar volume; b) stoichiometric relationships; CH.1g understand that experiments in which variables are measured, analyzed, and evaluated, produce observations and verifiable data. Key concepts include mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis). Summarize the basic concepts of stoichiometry: Atoms and molecules are too small to count by usual means. A mole is a way of counting any type of particle (atoms, molecules, formula units). Stoichiometry involves quantitative relationships. Stoichiometric relationships are based on mole quantities in a balanced equation. Know and use: Avogadro s number Molar volume of a gas at STP Total grams of reactant(s) = total grams of product(s). Calculate percent composition. Calculate empirical and molecular formulas CH.4 a, b CH.1g ChemA 2 nd /5 th (8 days) Dimensional Analysts Lab Problem sets Lab practical Graphing calculators Electronic balances Periodic Table Danville Public Schools, 2003 (Revised 10/21/2003) 11 Chemistry

12 Formulas, and Reactions Reactions and Equations CH.3 b, e understand how conservation of energy and matter is expressed in chemical formulas and balanced equations. Key concepts include b) balancing chemical equations; e) reaction types (synthesis, decomposition, single and double replacement, oxidationreduction, neutralization, exothermic and endothermic); CH.1g understand that experiments in which variables are measured, analyzed, and evaluated, produce observations and verifiable data. Key concepts include mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis). Infer that the conservation of matter is represented by balanced equations. Recognize and write equations for the major types of chemical reactions synthesis, decomposition, single replacement, double replacement, and redox reactions. Evaluate a chemical reaction and write equations, determine formulas, and balance chemical equations using coefficients. CH.3 b, e ChemA 3 rd /6 th (4 days) Lab Student lab reports Probe ware Simulation software Graphing calculators Periodic table New Pathways to Chemistry Module #14 Experiment with Enzymes Danville Public Schools, 2003 (Revised 10/21/2003) 12 Chemistry

13 Molar Scientific Investigations Stoichiometry Reactions and Equations CH.4 a, b understand that quantities in a chemical reaction are based on molar relationships. Key concepts include a) Avogadro s principle and molar volume; and b) stoichiometric relationships. CH.1g understand that experiments in which variables are measured, analyzed, and evaluated, produce observations and verifiable data. Key concepts include mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis). Make calculations involving the following relationships: Mole-mole Mass-mass Mole-mass Mass-volume Mole-volume Volume-volume Particle-particle Illustrate that: Ratios and proportions are used in calculations. Identify the limiting reactant in a chemical reaction. Calculate percent yield of a reaction. CH.4 a, b CH.1 g ChemA 3 rd /6 th (10 days) World of Chemistry Video Mole Lab Problem sets Lab practical Graphing calculators Electronic balances Periodic table Danville Public Schools, 2003 (Revised 10/21/2003) 13 Chemistry

14 and Formulas and Reactions Structure and Periodic Electron Configuration and the Periodic Table Reactions and Equations CH.3 d understand how conservation of energy and matter is expressed in chemical formulas and balanced equations. Key concepts include d) bonding types (ionic, covalent). CH.2f understand that the placement of elements on the periodic table is a function of their atomic structure. The periodic table is a tool used for the investigations of f) trends including atomic radii, electronegativity, shielding effect, and ionization energy. Summarize the following concepts about ionic bonding: Ionic bonds involve the transfer of electrons. Ionization energy is the energy required to remove the most easily held electron. Elements with low ionization energy form ions easily. CH.3 d CH.2 f ChemA 3 rd /6 th (2 days) World of Chemistry Video Bond Unit Student Lab Reports size periodic table Student notebook-size periodic table Models of molecular shapes Danville Public Schools, 2003 (Revised 10/21/2003) 14 Chemistry

15 and Formulas and Reactions Structure and Periodic Electron Configuration and the Periodic Table Structure CH.2 d, e, g, i understand that the placement of elements on the periodic table is a function of their atomic structure. The periodic table is a tool used for the investigations of d) families or groups; e) series and periods; g) mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis). i) historical and quantum models. CH.3 c understand how conservation of energy and matter is expressed in chemical formulas and balanced equations. Key concepts include c) writing chemical formulas (molecular, structural, empirical, and Lewis diagrams); Understand that: Electron configuration is the arrangement of electrons around the nucleus of an atom based on their energy level. Atoms can gain or lose electrons within the outer energy level. Determine the electron configuration for elements up to Z = 17. Know the following scientists & contributions. Quantum of energy Planck Uncertainty principle Heisenberg Wave theory de Broglie Apply the following principles: Aufbau Principle Pauli Exclusion Principle Hund s Rule Energy levels are designated 1-7. Orbitals are designated s, p, d, and f according to their shapes. These orbitals relate to regions of the Periodic Table. CH.2 d, e, g, i CH.3 c ChemA 3 rd /6 th (8 days) Practice Worksheets Practice Electron Configurations Complete Orbital Diagrams Short-hand Diagrams Unit Student lab reports Periodic table Orbital models Danville Public Schools, 2003 (Revised 10/21/2003) 15 Chemistry

16 and Formulas and Reactions Structure and Periodic Electron Configuration and the Periodic Table Loss of electrons from neutral atoms results in the formation of an ion with a positive charge (cation). Gain of electrons by a neutral atom results in the formation of an ion with a negative charge (anion). Valence electrons and possible oxidation number based on electron configuration. Draw Lewis Dot Diagrams to show both covalent and ionic bonding. Structure Danville Public Schools, 2003 (Revised 10/21/2003) 16 Chemistry

17 Scientific Investigation Phases of Matter and Kinetic Molecular Theory Properties of Matter Kinetic Theory CH.5 c, d, e understand that the phases of matter are explained by kinetic theory and forces of attraction between particles. Key concepts include c) phase changes; d) molar heats of fusion and vaporization; e) specific heat capacity; and CH.1 g Interpret a heating curve graph Calculate energy change and using specific heat Understand that the solid, liquid, and gas phases of a substance have different energy content. CH.5 c, d, e CH.1 g ChemB 1 st /4 th (4 days) Boiling Water Lab World of Chemistry Video A Matter of States Lab practical Unit Test See Earlier Sections understand that experiments in which variables are measured, analyzed, and evaluated, produce observations and verifiable data. Key concepts include mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis). Danville Public Schools, 2003 (Revised 10/21/2003) 17 Chemistry

18 and Formulas and Reactions Phases of Matter and Kinetic Molecular Theory Kinetic Theory Bonding Reactions and Equations CH.3 a, b, c, d understand how conservation of energy and matter is expressed in chemical formulas and balanced equations. Key concepts include a) nomenclature; b) balancing chemical equations; c) writing chemical formulas (molecular, structural, empirical, and Lewis diagrams); and d) bonding types (ionic, covalent). CH.5 c understand that the phases of matter are explained by kinetic theory and forces of attraction between particles. Key concepts include phase changes; Summarize the following concepts about covalent bonding: Covalent bonds involve sharing of electrons. Polar molecules result when a molecule behaves as if one end were positive and the other negative. Predict, draw, and name molecular shapes (linear, bent, trigonal planar, tetrahedral). Recognize polar and non-polar molecules. CH.3 a, b, c, d CH.5 c ChemB 1 st /4 th (5 days) Video Water Molecular Model Kit Student lab reports size periodic table Student notebook-size periodic table Models of molecular shapes Danville Public Schools, 2003 (Revised 10/21/2003) 18 Chemistry

19 and Formulas and Reactions Molar Reactions and Equations CH.3 e, f understand how conservation of energy and matter is expressed in chemical formulas and balanced equations. Key concepts include e) reaction types (synthesis, decomposition, single and double replacement, oxidationreduction, neutralization, exothermic and endothermic); and f) reaction rates and kinetics (activation energy, catalysis, degree of randomness). CH.4 f understand that quantities in a chemical reaction are based on molar relationships. Key concepts include f) chemical equilibrium. Identify the following relative to chemical reactions: Spontaneous reactions may be fast or slow. Randomness (entropy), heat content (enthalpy), and temperature affect spontaneity. reactions based on the net heat energy are exothermic (heat producing) and endothermic (heat absorbing). Reaction rates/kinetics are affected by activation energy, catalysis, and the degree of randomness (entropy). Interpret reaction rate diagrams CH.3 e, f CH.4 f ChemB 1 st /4 th (3 days) Labs Energy Curves World of Chemistry Video Driving Forces Student lab reports Probeware Simulation software Graphing calculators Periodic table New Pathways to Chemistry Module #14 Experiment with Enzymes Danville Public Schools, 2003 (Revised 10/21/2003) 19 Chemistry

20 Structure and Periodic Electron Configuration and the Periodic Table Reactions and Equations CH.2 d, e, f understand that the placement of elements on the periodic table is a function of their atomic structure. The periodic table is a tool used for the investigations of d) families or groups; e) series and periods; and f) trends including atomic radii, electronegativity, shielding effect, and ionization energy. CH.3 d understand how conservation of energy and matter is expressed in chemical formulas and balanced equations. Key concepts include d) bonding types (ionic, covalent). Point out that: The Periodic Law states that when elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern. The periodic table is arranged by increasing atomic numbers. Identify the following trends in the periodic table: Shielding effect is constant across the period and increases within given groups from top to bottom. radius decreases from left to right and increases from top to bottom within given groups. Ionization energies generally increase from left to right and decrease from top to bottom of a given group. Electronegativity increases from left to right, and decreases from top to bottom. CH.2 d, e, f CH.3 d ChemB 1 st /4 th (3 days) Trends on the Periodic Table Video Student lab reports Periodic table Orbital models Danville Public Schools, 2003 (Revised 10/21/2003) 20 Chemistry

21 Scientific Investigation Phases of Matter and Kinetic Molecular Theory Kinetic Theory Properties of Matter CH.5 a-f understand that the phases of matter are explained by kinetic theory and forces of attraction between particles. Key concepts include a) pressure, temperature, and volume; b) vapor pressure. c) phase changes; d) molar heats of fusion and vaporization; e) specific heat capacity; and f) colligative properties. CH.4 c-e Recognize the following relative to the Kinetic Molecular Theory: Atoms and molecules are in constant motion. The theory is a model for predicting and explaining gas behavior. Forces of attraction between molecules determine the physical changes in physical state. Pressure, temperature, and volume changes can cause a change in physical state. Solid, liquid, and gas phases of a substance have different energy content. CH.5 a-f CH.4 c-e CH.1 g ChemB 1 st /4 th (13 days) World of Chemistry Video Modeling the Unseen Diver Lab practical Unit test Graphing calculators Laser discs Test understand that quantities in a chemical reaction are based on molar relationships. Key concepts include c) partial pressure; d) gas laws; e) solution concentrations; Danville Public Schools, 2003 (Revised 10/21/2003) 21 Chemistry

22 Scientific Investigation Phases of Matter and Kinetic Molecular Theory Kinetic Theory Properties of Matter CH.1 g understand that experiments in which variables are measured, analyzed, and evaluated, produce observations and verifiable data. Key concepts include mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis). Recognize the following properties of gases: Gases have mass and occupy space. Gas particles are in constant, rapid, random motion and exert pressure as they collide with the walls of their containers. An Ideal Gas does not exist, but this concept is used to model gas behavior. A Real Gas exists, has intermolecular forces and particle volume, and can change states. State the following: Boyle s Law Dalton s Law of Partial Pressures Charles Law The Ideal Gas Law (PV=nRT) Solve problems and interpret graphs involving all gas laws. Use pressure units such as KPa and mm of Hg. Use molarity units/mole/dm 3 or moles/l Danville Public Schools, 2003 (Revised 10/21/2003) 22 Chemistry

23 Scientific Investigation Phases of Matter and Kinetic Molecular Theory Molar Kinetic Theory Properties of Matter CH.5 a-f understand that the phases of matter are explained by kinetic theory and forces of attraction between particles. Key concepts include a) pressure, temperature, and volume; b) vapor pressure. c) phase changes; d) molar heats of fusion and vaporization; e) specific heat capacity; and f) colligative properties. CH.4 c-e understand that quantities in a chemical reaction are based on molar relationships. Key concepts include c) partial pressure; d) gas laws; e) solution concentrations; Identify the forces of attraction as hydrogen bonding, dipole-dipole attraction, and London dispersion (van der Waals forces). Define vapor pressure as a property of a substance determined by intermolecular forces. Understand that: Specific amounts of energy are absorbed or released during phase changes. Boiling point of liquids is affected by changes in atmospheric pressure. Define specific heat capacity. CH.5 a-f CH.4 c-e CH.1 g ChemB 2 nd /5 th (8 days) Heat of Fusion Lab Benzene Lab Heating Curve Melting Point Danville Public Schools, 2003 (Revised 10/21/2003) 23 Chemistry

24 Scientific Investigation Phases of Matter and Kinetic Molecular Theory Molar Kinetic Theory CH.1 g understand that experiments in which variables are measured, analyzed, and evaluated, produce observations and verifiable data. Key concepts include mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis). Properties of Matter Danville Public Schools, 2003 (Revised 10/21/2003) 24 Chemistry

25 Formulas and Reactions Molar Reactions and Equations CH.3 e, f understand how conservation of energy and matter is expressed in chemical formulas and balanced equations. Key concepts include e) reaction types (synthesis, decomposition, single and double replacement, oxidationreduction, neutralization, exothermic and endothermic); and f) reaction rates and kinetics (activation energy, catalysis, degree of randomness). CH.4 f understand that quantities in a chemical reaction are based on molar relationships. Key concepts include f) chemical equilibrium. Calculate energy changes using molar heat of fusion and molar heat of vaporization. Perform calorimetry calculation Calculate energy changes using specific heat capacity. Interpret a phase diagram of water. Graph and interpret a heating curve Review solute, solvent, and solution types and calculate solution concentration. Recognize that: The number of solute particles changes the freezing point and boiling point of a pure substance. Freezing point of liquids is affected by the presence of certain solids. Polar substances dissolve ionic or polar substances; non-polar substances dissolve non-polar substances. CH.3 e, f CH.4 f ChemB 2 nd /5 th (3 days) Phase Diagrams Specific Heat Lab Endothermic and Exothermic Labs Video Catalysis Worlds of Chemistry Video Molecules In Action Student lab reports Probe ware Simulation software Graphing calculators Periodic table New Pathways to Chemistry Module #14 Experiment with Enzymes Danville Public Schools, 2003 (Revised 10/21/2003) 25 Chemistry

26 Formulas and Reactions Molar Reactions and Equations Recognize that: Catalysts decrease the amount of activation energy needed. Reactions can occur in two directions simultaneously. LeChatelier s Principle indicates the qualitative prediction of direction of change with temperature, pressure, and concentration. A reaction is said to reach equilibrium when the forward reaction rate equals the reverse reaction rate. Danville Public Schools, 2003 (Revised 10/21/2003) 26 Chemistry

27 Molar Acids/Bases and Electrolytes CH.4 g understand that quantities in a chemical reaction are based on molar relationships. Key concepts include g) acid/base theory: strong electrolytes, weak electrolytes, and nonelectrolytes; dissociation and ionization; (ph, poh), and the titration process. Recognize that acids and bases are defined by several theories. State the characteristics of acids and bases based on: Arrhenius Theory Bronsted-Lowry Theory Define ph and poh. Understand the relationship between ph and poh. Explain that strong electrolytes dissociate completely and weak electrolytes dissociate partially. Utilize acid-base titration and ph indicators in the laboratory. CH.4 g ChemB 2 nd /5 th (4 days) Video Proton in Chemistry Demonstration Lab Lab practical Safety in Science Teaching manual New Pathways in Chemistry Module #11 Know: [ ] refers to molar concentration. 2H 2 O (e) H 3 O + + OH - Indicators show color changes at certain phs Danville Public Schools, 2003 (Revised 10/21/2003) 27 Chemistry

28 Molar Applications Organic Chemistry Define organic chemistry and biochemistry. Differentiate between alkanes, alkenes, and alkynes in terms of the type of carbon bonds. ChemB 3 rd /6 th after completion of SOL test Demonstration Video: Carbon Danville Public Schools, 2003 (Revised 10/21/2003) 28 Chemistry