Teacher: Gilson Week Of: September 1-5 Class: C.P. Chemistry Hr: 2. BenchMarks
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- Gladys Bryan
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1 Teacher: Gilson Week Of: September 1-5 Introduction: Benchmarks: C1.1 Scientific Inquiry C1.1A Generate new questions that can be investigated in the lab or field C1.1E Describe a reason for a given conclusion using evidence from an investigation C1.1f Predict what would happen if the variables, methods, or timing on an investigation were changed C1.1h Design and conduct a systematic scientific investigation that tests a hypothesis. Draw conclusions from data presented in charts or tables C1.2 Scientific Reflection and Social Implications C1.2f Critique solutions to problems, given criteria and scientific constraints No School: Labor Day *Describe beginning of class expectations *Describe end of class expectations *List required materials for class Wednesday : * Describe ipad Expectations *Demonstrate how to set up and write in their interactive notebook *Describe the class rules and consequences *Demonstrate how to complete an absent slip * Demonstrate how to log into the TI-nSpire calculator *Demonstrate how to open a document on their calculator and answer the questions *Describe the procedures for a High & Low Level Lockdown, Fire Drill and Tornado Drill *Describe the grading policy * Demonstrate how to use a QR scanner *Describe the contents of the syllabus *Name and describe the type of learning style you prefer: auditory, tactile, visual
2 Teacher: Gilson Week Of: September 8-12 Chapter 1: Benchmarks C1.1C Conduct scientific investigations using appropriate tools and techniques C1.1E Describe a reason for a given conclusion using evidence from an investigation C1.1f Predict what would happen if the variables, methods, or timing of an investigation were changed C2.2B Describe and draw the various states of matter in terms of the motion, arrangement, and relative spacing of the molecules (atoms) making up the substance. Present a drawing that shows the number of particles in the system does not change as a result of a phase change. P4.p2A Distinguish between an element, compound, or mixture based on drawings or formula C5.2B Distinguish between chemical and physical changes in terms of the properties of the reactants and products C1.1h Draw conclusions from data presented in charts or tables. *Use scientific notation accurately with positive and negative exponents *Convert between Celsius, Fahrenheit, and Kelvin temperatures *Describe participation and learning readiness expectations *Distinguish between an element, compound, or mixture based on drawings or formula *Describe and draw the various states of matter Wednesday : *Distinguish between an element, compound, or mixture based on drawings or formula *Describe and draw the various states of matter * Distinguish between chemical and physical changes in terms of the properties of the reactants and products *Draw pictures to distinguish between physical and chemical changes *Name and give the function of several types of lab equipment *Accurately read a meniscus on a graduated cylinder *Accurately read a digital scale *Describe lab expectations
3 Teacher: Gilson Week Of: September Chapter 1: Benchmarks C1.1C Conduct scientific investigations using appropriate tools and techniques C1.1E Describe a reason for a given conclusion using evidence from an investigation C1.1f Predict what would happen if the variables, methods, or timing of an investigation were changed C2.2B Describe and draw the various states of matter in terms of the motion, arrangement, and relative spacing of the molecules (atoms) making up the substance. Present a drawing that shows the number of particles in the system does not change as a result of a phase change. P4.p2A Distinguish between an element, compound, or mixture based on drawings or formula C5.2B Distinguish between chemical and physical changes in terms of the properties of the reactants and products C1.1h Draw conclusions from data presented in charts or tables. *calculate and compare the densities of various substances *Identify the dependent and independent variables in an experiment *Identify control and experimental groups in an experiment *experimentally determine the density of solids, liquids, and gases Wednesday : *Draw and describe reasons for conclusions from data presented in charts or tables *perform unit conversions using dimensional analysis *perform unit conversions using dimensional analysis *determine the number of significant figures in a measurement *round solutions to math problems correctly based on sig figs. *Determine the number of significant figures in a measurement *Round solutions to math problems correctly based on sig. figs
4 Teacher: Gilson Week Of: September Chapter 1: Benchmarks C1.1C Conduct scientific investigations using appropriate tools and techniques C1.1E Describe a reason for a given conclusion using evidence from an investigation C1.1f Predict what would happen if the variables, methods, or timing of an investigation were changed C2.2B Describe and draw the various states of matter in terms of the motion, arrangement, and relative spacing of the molecules (atoms) making up the substance. Present a drawing that shows the number of particles in the system does not change as a result of a phase change. P4.p2A Distinguish between an element, compound, or mixture based on drawings or formula C5.2B Distinguish between chemical and physical changes in terms of the properties of the reactants and products C1.1h Draw conclusions from data presented in charts or tables. *Perform unit conversions using dimensional analysis *Determine the number of significant figures in a measurement *Round solutions to problems correctly based on sig. figs *Differentiate between accuracy and precision *Round solutions to problems correctly based on sig figs Wednesday : *Give examples of questions on the Chapter 1 Test *Substitute *Chemistry Year Long Pre-test *Define and give examples for Chemistry vocabulary terms *No School: Fall Festival
5 Teacher: Gilson Week Of: September 28-October 3 Chapter 2: Benchmarks C4.2A-Name simple binary compounds using their formulae C4.2B-Given the name, write the formula of simple binary compounds C4.2c-Given a formula, name the compound C4.2d-Given the name, write the formula of ionic and molecular compounds C4.8A-Identify the location, relative mass, and charge for electrons, protons, and neutrons C4.8B-Describe the atom as mostly empty space with an extremely small, dense nucleus consisting of the protons and neutrons and an electron cloud surrounding the nucleus C4.8D-Give the number of electrons and protons present if the fluoride ion has a -1 charge C4.9A-Identify elements with similar chemical and physical properties using the periodic table C4.10A-List the number of protons, neutrons, and electrons for any given ion or isotope C4.10B-Recognize that an element always contains the same number of protons C4.10e-Write the symbol for an isotope, XZA, where Z is the atomic number, A is the mass number, and X is the symbol for the element C1.2i-Explain the progression of ideas and explanations that lead to science theories that are part of the current scientific consensus or core knowledge *demonstrate mastery of Chapter 1 concepts on a written test *Name the two parts of an atom *Draw a representative atom Wednesday : *Name scientists associated with the advancement of atomic structure and describe their contributions *Locate metals, nonmetals, and metalloids on the periodic table *Name elements with similar physical and chemical properties on the periodic table * List the number of protons, neutrons, and electrons for any given ion or isotope * Recognize that an element always contains the same number of protons * Write the symbol for an isotope, XZA, where Z is the atomic number, A is the mass number, and X is the symbol for the element *Name laboratory equipment (Bunsen Burner, stirring rod, glass tubing) *Light and adjust a Bunsen Burner *Cut, bend, and fire polish glass
6 Teacher: Gilson Week Of: October 6-10 Chapter 2: Benchmarks C4.2A-Name simple binary compounds using their formulae C4.2B-Given the name, write the formula of simple binary compounds C4.2c-Given a formula, name the compound C4.2d-Given the name, write the formula of ionic and molecular compounds C4.8A-Identify the location, relative mass, and charge for electrons, protons, and neutrons C4.8B-Describe the atom as mostly empty space with an extremely small, dense nucleus consisting of the protons and neutrons and an electron cloud surrounding the nucleus C4.8D-Give the number of electrons and protons present if the fluoride ion has a -1 charge C4.9A-Identify elements with similar chemical and physical properties using the periodic table C4.10A-List the number of protons, neutrons, and electrons for any given ion or isotope C4.10B-Recognize that an element always contains the same number of protons C4.10e-Write the symbol for an isotope, XZA, where Z is the atomic number, A is the mass number, and X is the symbol for the element C1.2i-Explain the progression of ideas and explanations that lead to science theories that are part of the current scientific consensus or core knowledge *compare and contrast metals, nonmetals, and metalloids *give examples of metals, nonmetals, and metalloids *for any neutral element, ion, or isotope list their: atomic number, mass number, atomic mass, # protons, # neutrons, and # electrons *Substitute: Work Day Wednesday : *describe tests to differentiate between metals and nonmetals *differentiate between an ion, isotope, and neutral atom *name binary ionic compounds (metals with one oxidation state) *write formulas for binary ionic compounds (metals with one oxidation state) * name binary ionic compounds (metals with > oxidation state) *write formulas for binary ionic compounds (metals with > oxidation state)
7 Teacher: Gilson Week Of: October Chapter 2: Benchmarks C4.2A-Name simple binary compounds using their formulae C4.2B-Given the name, write the formula of simple binary compounds C4.2c-Given a formula, name the compound C4.2d-Given the name, write the formula of ionic and molecular compounds C4.8A-Identify the location, relative mass, and charge for electrons, protons, and neutrons C4.8B-Describe the atom as mostly empty space with an extremely small, dense nucleus consisting of the protons and neutrons and an electron cloud surrounding the nucleus C4.8D-Give the number of electrons and protons present if the fluoride ion has a -1 charge C4.9A-Identify elements with similar chemical and physical properties using the periodic table C4.10A-List the number of protons, neutrons, and electrons for any given ion or isotope C4.10B-Recognize that an element always contains the same number of protons C4.10e-Write the symbol for an isotope, XZA, where Z is the atomic number, A is the mass number, and X is the symbol for the element C1.2i-Explain the progression of ideas and explanations that lead to science theories that are part of the current scientific consensus or core knowledge *name binary compounds between 2 nonmetals *write formulas for binary compounds between 2 nonmetals *identify whether a binary compound is Type I, Type II or Type III *experimentally determine if a change in matter is physical or chemical Wednesday : *name and write formulas for several polyatomic ions *name polyatomic compounds * write formulas for polyatomic compounds *write formulas and names for Type I, Type 2, and Type 3 binary compounds *write formulas and names of polyatomic compounds
8 Teacher: Gilson Week Of: October Chapter 2: Benchmarks C4.2A-Name simple binary compounds using their formulae C4.2B-Given the name, write the formula of simple binary compounds C4.2c-Given a formula, name the compound C4.2d-Given the name, write the formula of ionic and molecular compounds C4.8A-Identify the location, relative mass, and charge for electrons, protons, and neutrons C4.8B-Describe the atom as mostly empty space with an extremely small, dense nucleus consisting of the protons and neutrons and an electron cloud surrounding the nucleus C4.8D-Give the number of electrons and protons present if the fluoride ion has a -1 charge C4.9A-Identify elements with similar chemical and physical properties using the periodic table C4.10A-List the number of protons, neutrons, and electrons for any given ion or isotope C4.10B-Recognize that an element always contains the same number of protons C4.10e-Write the symbol for an isotope, XZA, where Z is the atomic number, A is the mass number, and X is the symbol for the element C1.2i-Explain the progression of ideas and explanations that lead to science theories that are part of the current scientific consensus or core knowledge *write the names and formulas for inorganic acids *differentiate between empirical, molecular, and structural formulas *give examples of empirical, molecular, and structural formulas *identify elements on the periodic table with very similar properties *list properties of groups of elements *name and write formulas for hydrates *Substitute: Work Day -Work on Chapter 2 Vocabulary/Practice Exercises -Chapter 2 Practice Test! *describe the meaning of the mole unit *celebrate MOLE DAY *give examples of questions on the Chapter 2 Test
9 Teacher: Gilson Week Of: October Chapter 3: Benchmarks C4.6a-Calculate the number of moles of any compound or element given the mass of the substance C4.6b-Calculate the number of particles of any compound or element given the mass of the substance C4.10c-Calculate the average atomic mass of an element given the percent abundance and mass of the individual isotope C4.10d-Predict which isotope will have the greatest abundance given the possible isotopes for an element and the average atomic mass in the periodic table C4.1a-Calculate the percent by weight of each element in a compound based on the compound formula C4.1b-Calculate the empirical formula of a compound based on the percent by weight of each element in the compound C4.1c-Use the empirical formula and molecular weight of a compound to determine the molecular formula C5.2g-Calculate the number of atoms present in a given mass of element C5.2A Balance simple chemical equations applying the conservation of matter C5.2d Calculate the mass of a particular compound formed from the masses of starting materials C5.2e Identify the limiting reagent when given the masses of more than one reactant *demonstrate mastery of Chapter 2 Concepts on a written test *correct mistakes on the Chapter 2 Test *take Chapter 3 Pretest *calculate the average atomic mass of a mixture of isotopes *calculate the molar mass of an element and compound *convert between moles and grams *convert between moles and atoms/molecules *perform Halloween demonstrations and activities
10 Teacher: Gilson Week Of: November 3-7 Chapter 3: Benchmarks C4.6a-Calculate the number of moles of any compound or element given the mass of the substance C4.6b-Calculate the number of particles of any compound or element given the mass of the substance C4.10c-Calculate the average atomic mass of an element given the percent abundance and mass of the individual isotope C4.10d-Predict which isotope will have the greatest abundance given the possible isotopes for an element and the average atomic mass in the periodic table C4.1a-Calculate the percent by weight of each element in a compound based on the compound formula C4.1b-Calculate the empirical formula of a compound based on the percent by weight of each element in the compound C4.1c-Use the empirical formula and molecular weight of a compound to determine the molecular formula C5.2g-Calculate the number of atoms present in a given mass of element C5.2A Balance simple chemical equations applying the conservation of matter C5.2d Calculate the mass of a particular compound formed from the masses of starting materials C5.2e Identify the limiting reagent when given the masses of more than one reactant *interpret a mass spectrometer graph *calculate the % composition by mass of each element in a compound *Work Day -Juniors & Seniors at Career Day *calculate the empirical formula of a compound based on the percent by weight of each element in the cmpd *use the empirical formula and the molar mass to determine the molecular formula *identify the reactants and products in a chemical equation *state the law of conservation of mass *balance chemical equations *balance chemical equations
11 Teacher: Gilson Week Of: November Chapter 3: Benchmarks C4.6a-Calculate the number of moles of any compound or element given the mass of the substance C4.6b-Calculate the number of particles of any compound or element given the mass of the substance C4.10c-Calculate the average atomic mass of an element given the percent abundance and mass of the individual isotope C4.10d-Predict which isotope will have the greatest abundance given the possible isotopes for an element and the average atomic mass in the periodic table C4.1a-Calculate the percent by weight of each element in a compound based on the compound formula C4.1b-Calculate the empirical formula of a compound based on the percent by weight of each element in the compound C4.1c-Use the empirical formula and molecular weight of a compound to determine the molecular formula C5.2g-Calculate the number of atoms present in a given mass of element C5.2A Balance simple chemical equations applying the conservation of matter C5.2d Calculate the mass of a particular compound formed from the masses of starting materials C5.2e Identify the limiting reagent when given the masses of more than one reactant *solve stoichiometry problems for their theoretical yield *calculate the % yield of a reaction *solve limiting and excess reagent stoichiometry problems *identify the limiting and excess reagent in a stoichiometry problem *calculate the amount of excess reagent left in a stoichiometry problem *solve stoichiometry problems *draw pictures to represent the reactants and products in a chemical reaction *ChemThink: Online chemistry problems *collect gases by water displacement *determine the optimal ratio of reactants in a chemical reaction
12 Teacher: Gilson Week Of: November Chapter 3: Benchmarks C4.6a-Calculate the number of moles of any compound or element given the mass of the substance C4.6b-Calculate the number of particles of any compound or element given the mass of the substance C4.10c-Calculate the average atomic mass of an element given the percent abundance and mass of the individual isotope C4.10d-Predict which isotope will have the greatest abundance given the possible isotopes for an element and the average atomic mass in the periodic table C4.1a-Calculate the percent by weight of each element in a compound based on the compound formula C4.1b-Calculate the empirical formula of a compound based on the percent by weight of each element in the compound C4.1c-Use the empirical formula and molecular weight of a compound to determine the molecular formula C5.2g-Calculate the number of atoms present in a given mass of element C5.2A Balance simple chemical equations applying the conservation of matter C5.2d Calculate the mass of a particular compound formed from the masses of starting materials C5.2e Identify the limiting reagent when given the masses of more than one reactant *collect gases by water displacement *determine the optimal ratio of reactants in a chemical reaction *solve stoichiometry problems *define theoretical yield, actual yield, % yield, limiting reagent, excess reagent *give examples of questions on the Chapter 3-Stoichimetry test *demonstrate mastery of Chapter 3-Stoichiometry on a written test *correct errors on the Chapter 3 Test *take Chapter 4 Pretest
13 Teacher: Gilson Week Of: November Chapter 4: Benchmarks: C5.7A- Recognize formulas for common inorganic acids, carboxylic acids, and bases formed from families I and II C5.7B-Predict products of an acid-base neutralization C5.7C-Describe tests that can be used to distinguish an acid from a base C5.6a-Balance half-reactions and describe them as oxidations or reductions *Present Periodic Tables *Sophomore VoTech Visit 1 st 4 th Hours *Present Periodic Tables *West Point Cadet Presentation 9-10AM *No School *No School
14 Teacher: Gilson Week Of: December 1-5 Chapter 4: Benchmarks: C5.7A- Recognize formulas for common inorganic acids, carboxylic acids, and bases formed from families I and II C5.7B-Predict products of an acid-base neutralization C5.7C-Describe tests that can be used to distinguish an acid from a base C5.6a-Balance half-reactions and describe them as oxidations or reductions *Differentiate between electrolytes and nonelectrolyte *Predict whether a compound will be an electrolyte or nonelectrolyte *Determine whether an ionic compound is soluble or insoluble *Interpret a solubility curve *Predict the products of a double replacement reaction *Write complete and net ionic equations *Identify spectator ions in a precipitation reaction *Write molecular, complete, and net ionic equations *Draw pictures to represent the reactants and products in a precipitation reaction *List properties of acids and bases *Describe tests used to determine whether a substance is acidic, basic, or neutral *Identify and predict the products of an acid-base neutralization reaction *Perform precipitation reactions
15 Teacher: Gilson Week Of: December 8-12 Chapter 4: Benchmarks: C5.7A- Recognize formulas for common inorganic acids, carboxylic acids, and bases formed from families I and II C5.7B-Predict products of an acid-base neutralization C5.7C-Describe tests that can be used to distinguish an acid from a base C5.6a-Balance half-reactions and describe them as oxidations or reductions *differentiate between a precipitation reaction and acid-base reactions *classify substances as a Bronsted acid, Bronsted base or both *determine the oxidation number for any element in a compound *predict the products of a single replacement reaction *Substitute: Work Day * identify the reduced and oxidized element in a single replacement reaction *identify the reducing agent and oxidizing agent in a redox reaction *list the main types of chemical reactions *identify the type of chemical reaction
16 Teacher: Gilson Week Of: December Chapter 4: Benchmarks: C5.7A- Recognize formulas for common inorganic acids, carboxylic acids, and bases formed from families I and II C5.7B-Predict products of an acid-base neutralization C5.7C-Describe tests that can be used to distinguish an acid from a base C5.6a-Balance half-reactions and describe them as oxidations or reductions *define concentration *solve Molarity problems *rank concentrations of solutions from weakest to strongest *solve dilution problems *describe how to make solutions by diluting a stronger solution *describe how to make solutions by dissolving a solid in water *identify the 6 types of reactions *predict the products of SR, DR, and AB reactions *give examples of questions on the Chapter 4 Test *demonstrate mastery of Chapter 4 on a written test
17 Teacher: Gilson Week Of: January 5-9 Chapter 5: Benchmarks: P4.p1A-For a substance that can exist in all three phases, describe the relative motion of the particles in each of the phases P4.p1B-For a substance that can exist in all three phases, make a drawing that shows the arrangement and relative spacing of the particles in each of the phases P4.p1C-For a single compound, present a drawing that shows the number of particles in the system does not change as a result of the phase change C4.5a-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-volume relationship of gases C4.5b-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-temperature relationship of gases C4.5c-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the temperature-volume relationship of gases *define pressure *list units of pressure *convert between units of pressure *solve gas law problems involving changes in pressure, volume, or temperature (Boyles, Charles, Gay Lussac) *predict changes in pressure, volume, or temperature of gases *list several properties of hydrogen *solve gas law problems involving changes in pressure, volume, or temperature (Boyles, Charles, Gay Lussac) *list practical examples of Boyles Law *Snow Day *Snow Day
18 Teacher: Gilson Week Of: January Chapter 5: Benchmarks: P4.p1A-For a substance that can exist in all three phases, describe the relative motion of the particles in each of the phases P4.p1B-For a substance that can exist in all three phases, make a drawing that shows the arrangement and relative spacing of the particles in each of the phases P4.p1C-For a single compound, present a drawing that shows the number of particles in the system does not change as a result of the phase change C4.5a-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-volume relationship of gases C4.5b-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-temperature relationship of gases C4.5c-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the temperature-volume relationship of gases *solve ideal gas law problems *Exam Review *Exam Review *2 nd Hour Exam *No Class
19 Teacher: Gilson Week Of: January Chapter 5: Benchmarks: P4.p1A-For a substance that can exist in all three phases, describe the relative motion of the particles in each of the phases P4.p1B-For a substance that can exist in all three phases, make a drawing that shows the arrangement and relative spacing of the particles in each of the phases P4.p1C-For a single compound, present a drawing that shows the number of particles in the system does not change as a result of the phase change C4.5a-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-volume relationship of gases C4.5b-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-temperature relationship of gases C4.5c-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the temperature-volume relationship of gases *No School *solve combined gas law and ideal gas law problems *list several properties of helium gas * use the ideal gas law to solve for molar mass & density *list several properties of nitrogen gas *solve gas stoichiometry problems STP and STP *list several properties of fluorine gas *solve gas stoichiometry problems STP and STP
20 Teacher: Gilson Week Of: January Chapter 5: Benchmarks: P4.p1A-For a substance that can exist in all three phases, describe the relative motion of the particles in each of the phases P4.p1B-For a substance that can exist in all three phases, make a drawing that shows the arrangement and relative spacing of the particles in each of the phases P4.p1C-For a single compound, present a drawing that shows the number of particles in the system does not change as a result of the phase change C4.5a-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-volume relationship of gases C4.5b-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-temperature relationship of gases C4.5c-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the temperature-volume relationship of gases *state Dalton s Law of Partial Pressure *explain how to collect a gas using water displacement *list properties of chlorine gas *list properties of neon *solve Dalton s Law of Partial Pressure Problems *demonstrate how to collect gases by water displacement *perform splint tests on gases to determine the type of gas produced *solve gas law problems *calculate the amount of gas needed to fill up an airbag
21 Teacher: Gilson Week Of: February 2-6 Chapter 5: Benchmarks: P4.p1A-For a substance that can exist in all three phases, describe the relative motion of the particles in each of the phases P4.p1B-For a substance that can exist in all three phases, make a drawing that shows the arrangement and relative spacing of the particles in each of the phases P4.p1C-For a single compound, present a drawing that shows the number of particles in the system does not change as a result of the phase change C4.5a-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-volume relationship of gases C4.5b-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-temperature relationship of gases C4.5c-Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the temperature-volume relationship of gases Chapter 6: Benchmarks: C3.1a-Calculate the H for a given reaction using Hess s Law C3.1b/C3.4d-Draw enthalpy diagrams for exothermic and endothermic reactions. C3.1c-Calculate the H for a chemical reaction using simple coffee cup calorimetry C3.1d-Calculate the amount of heat produced for a given mass of reactant from a balanced chemical equation C3.4A-use the terms endothermic and exothermic correctly to describe chemical reactions in the lab. C3.4B-Explain why chemical reactions will either release or absorb energy C3.4c-Write chemical equations including the heat term as part of equation or using H notation C5.4B Measure, plot, and interpret the graph of the temperature vs. time of an ice-water mixture, under slow heating, through melting and boiling.
22 *give examples of questions on the Chapter 5 Test *list properties of Xenon and Radon *demonstrate mastery of Chapter 5 on a written test *correct errors on the Chapter 5 test *take Chapter 6 Pretest *list and describe several types of energy *SUBSTITUTE *ACT Practice *give examples of several energy transformations *experimentally determine the difference in evaporation rates of alcohol and water
23 Teacher: Gilson Week Of: February 9-13 BenchMarks Chapter 6: Benchmarks: C3.1a-Calculate the H for a given reaction using Hess s Law C3.1b/C3.4d-Draw enthalpy diagrams for exothermic and endothermic reactions. C3.1c-Calculate the H for a chemical reaction using simple coffee cup calorimetry C3.1d-Calculate the amount of heat produced for a given mass of reactant from a balanced chemical equation C3.4A-use the terms endothermic and exothermic correctly to describe chemical reactions in the lab. C3.4B-Explain why chemical reactions will either release or absorb energy C3.4c-Write chemical equations including the heat term as part of equation or using H notation C5.4B Measure, plot, and interpret the graph of the temperature vs. time of an ice-water mixture, under slow heating, through melting and boiling. *give examples of energy transformations *differentiate between endothermic and exothermic reactions *analyze a heating and cooling curve *experimentally determine the difference in evaporation rates of alcohol and water *analyze heating and cooling curves *define enthalpy *use stoichiometry to determine the amount of heat lost or gained in a chemical reaction *SUBSTITUTE *ACT Practice *No School
24 Teacher: Gilson Week Of: February BenchMarks Chapter 6: Benchmarks: C3.1a-Calculate the H for a given reaction using Hess s Law C3.1b/C3.4d-Draw enthalpy diagrams for exothermic and endothermic reactions. C3.1c-Calculate the H for a chemical reaction using simple coffee cup calorimetry C3.1d-Calculate the amount of heat produced for a given mass of reactant from a balanced chemical equation C3.4A-use the terms endothermic and exothermic correctly to describe chemical reactions in the lab. C3.4B-Explain why chemical reactions will either release or absorb energy C3.4c-Write chemical equations including the heat term as part of equation or using H notation C5.4B Measure, plot, and interpret the graph of the temperature vs. time of an ice-water mixture, under slow heating, through melting and boiling. *2 Hour Delay-No Class * use stoichiometry to determine the amount of heat lost or gained in a chemical reaction *graph the enthalpy change in a reaction *define specific heat *define heat of vaporization and heat of fusion *compare the specific heat of various substances *calculate the amount of heat gained or lost during a temperature change *Snow Day *Snow Day
25 Teacher: Gilson Week Of: February Chapter 6: Benchmarks: C3.1a-Calculate the H for a given reaction using Hess s Law C3.1b/C3.4d-Draw enthalpy diagrams for exothermic and endothermic reactions. C3.1c-Calculate the H for a chemical reaction using simple coffee cup calorimetry C3.1d-Calculate the amount of heat produced for a given mass of reactant from a balanced chemical equation C3.4A-use the terms endothermic and exothermic correctly to describe chemical reactions in the lab. C3.4B-Explain why chemical reactions will either release or absorb energy C3.4c-Write chemical equations including the heat term as part of equation or using H notation C5.4B Measure, plot, and interpret the graph of the temperature vs. time of an ice-water mixture, under slow heating, through melting and boiling. *calculate the amount of heat energy transferred between objects in contact *explain the process of calorimetry *list and convert between several units used to measure energy *calculate the heat of a reaction using Hess s Law *calculate the heat of a reaction using the heat of formation of the reactants and products *calculate the heat of reaction using either Hess s law of heats of formation *give examples of questions on the Chapter 6-Thermochemistry Test *demonstrate a MRE
26 Teacher: Gilson Week Of: March 2-6 Chapter 7: Benchmarks: Quantum Theory C4.8e-Write the complete electron configuration of elements in the first four rows of the periodic table C4.8f-Write kernel structure for main group elements C4.8g-Predict oxidation states and bonding capacity for main group elements using their electron structure C4.8h-Describe the shape and orientation of s and p orbitals C4.8i-Describe the fact that the electron location cannot be exactly determined at any given time. C2.4a-Describe energy changes in flame tests of common elements in terms of the characteristic electron transitions C2.4c-Explain why an atom can absorb only certain wavelengths of light C2.4d-Compare various wavelengths of light in terms of frequency and relative energy P4.4A-Describe specific mechanical waves in terms of wavelength, amplitude, frequency, and speed. P4.6A-Identify the different regions on the electromagnetic spectrum and compare them in terms of wavelength, frequency and energy P4.6h-Explain the relationship between the frequency of an electromagnetic wave and its technological uses P4.r7a-Calculate and compare the energy in various electromagnetic quanta *demonstrate mastery of the Chapter 6 Test-Thermochemistry *No Class *Juniors Testing-Work Day *correct errors on the Chapter 6 Test *take Chapter 7 Pretest *label and define the parts of a wave *experimentally determine the specific heat of an unknown metal
27 Teacher: Gilson Week Of: March 9-13 Chapter 7: Benchmarks: Quantum Theory C4.8e-Write the complete electron configuration of elements in the first four rows of the periodic table C4.8f-Write kernel structure for main group elements C4.8g-Predict oxidation states and bonding capacity for main group elements using their electron structure C4.8h-Describe the shape and orientation of s and p orbitals C4.8i-Describe the fact that the electron location cannot be exactly determined at any given time. C2.4a-Describe energy changes in flame tests of common elements in terms of the characteristic electron transitions C2.4c-Explain why an atom can absorb only certain wavelengths of light C2.4d-Compare various wavelengths of light in terms of frequency and relative energy P4.4A-Describe specific mechanical waves in terms of wavelength, amplitude, frequency, and speed. P4.6A-Identify the different regions on the electromagnetic spectrum and compare them in terms of wavelength, frequency and energy P4.6h-Explain the relationship between the frequency of an electromagnetic wave and its technological uses P4.r7a-Calculate and compare the energy in various electromagnetic quanta
28 *list the parts of the electromagnetic spectrum *give examples of applications to the parts of the electromagnetic spectrum *calculate the speed, wavelength, frequency, and period of waves *describe Bohr s model of the atom *differentiate between excited state and ground state electrons *calculate the energy absorbed or released by electrons changing energy levels *Substitute: AP Biology Field Trip *calculate the wavelength, frequency and energy of electromagnetic radiation *describe an atom s electron cloud *draw the shapes of s and p orbitals *explain why elements emit different colors when heated *write complete and noble gas electron configurations for atoms *draw Bohr models of atoms
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