Course title

Chem

Pre-requisite

Algebra I or teacher approval

Course description

19. Brief Course Description

Chemistry explores the fundamental concepts required to understand conceptually matter on the atomic and macroscopic level. The course emphasizes data analysis; investigations; class discussions; and research. The course requires students to focus on questioning; experimentation; data analysis; research; and investigation skills. Students apply the knowledge learned in the classroom to laboratory experiments. Chemistry topics include the physical and chemical properties of matter; chemical reaction; atomic theory; molarity; gases; thermochemistry; and the electronic structure and the periodic table.

B. COURSE CONTENT

20. Course Goals and/or Major Student Outcomes
Students in Chemistry will demonstrate the required knowledge and skills outlined in the California State Chemistry Standards .as they work toward the school-wide goals of becoming:

Critical readers who explore a wide range of texts in diverse genres and styles as they interrogate; decode; and interpret the world they live in and the human condition.

Effective communicators who speak; listen and write with clarity and purpose.

Skilled problem solvers who employ systematic reasoning; construct logical arguments; and use abstract symbols to describe; order; explain and communicate about the world.

Discriminating thinkers who investigate the world through scientific inquiry utilizing appropriate tools; technologies; processes; and ethical rigor.

21. Course Objectives
Course Themes Standards
Students will understand:
1. The periodic table displays the elements in increasing atomic number and shows how periodicity of the physical and chemical
properties of the elements relates to atomic structure. As a basis for understanding this concept.

2. Biological; chemical and physical properties of matter result form the ability of atoms to form bonds from electrostatic forces between
electrons and protons and between atoms and molecules.

3. The conservation of atoms in chemical reactions leads to the principle of conservation of matter and the ability to calculate the mass of products and reactants.

4. The kinetic molecular theory describes the motion of atoms and molecules and explains the properties of gases.

5. Acids; bases; and salts are three classes of compounds that form ions in water solutions.

6. Solutions are homogenous mixtures of two or more substances.

7. Energy is exchanged or transformed in all chemical reactions and physical changes of matter

8. Chemical reaction rates depend on factors that influence the frequency of collision of reactant molecules.

9. Chemical equilibrium is a dynamic process at the molecular level.

10. The bonding of characteristics of carbon allow the formation of many different organic molecules of varied sizes; shapes; and chemical basis of life.

11. Nuclear processes are those which an atom nucleus changes; including radioactive decay of naturally occurring and human-made
isotopes; nuclear fission; and nuclear fusion.

Chemistry Standard 1:a-e

Chemistry Standard 2:a-e

Chemistry Standard 3:a-e

Chemistry Standard 4:a-f

Chemistry Standard 5:a-d

Chemistry Standard 6:a-d

Chemistry Standard 7:a-d

Chemistry Standard 8:a-c

Chemistry Standard 9:a & b

Chemistry Standard 10:a-c

Chemistry Standard 11:a-e

Core Concepts:
This course covers the fundamental concepts of chemistry through lecture; labs; group investigation and discussion. The course makes a connection between the macroscopic world of chemistry that students observe in their every day lives and the microscopic world of ions and molecules. Students examine the concepts through daily readings; labs; practice examples and solutions; and teacher led discussions. The course pays careful attention to nomenclature and helps students build facility with the ?language? of chemistry.

22. Course Outline

Unit Mehtods/Activities
Nomenclature
? Naming compounds
? Compounds that contain a metal and a nonmetal
? Binary compounds that contain only nonmetals
? Compounds that contain polyatomic ions
? Acids
? Writing formulas from names

Structure of Matter
? Atomic theory and atomic structure
? Evidence for the atomic theory
? Atomic masses; determination by chemical and physical means
? Atomic number and mass number; isotopes
? Electron energy levels: atomic spectra; quantum numbers; atomic orbitals
? Periodic relationships; atomic radii; ionization energies; electron affinities; oxidation states
? Physical and chemical changes
? Elements and compounds
? Mixtures and pure substances
? Separation of mixtures
? Energy changes
? Elements; Atoms and Ions
? The Elements
? Symbols for the Elements
? Dalton?s Atomic Theory
? Formulas of Compounds
? Isotopes
? The Periodic Table
? Organizing principles for the Elements
? Natural States of the Elements
? Ions
? Compounds That Contain Ions

Reactions
? Reaction types
Acid-base reactions; concepts of Arrhenius; Br╦ćnsted-Lowry and Lewis; coordination complexes; amphoterism
? Precipitation reactions
? Oxidation-reduction reactions
? Faraday's laws; standard half-cell potentials; Nernst
equation; prediction of the direction of redox reactions
? Balancing Chemical Equations
? Evidence for a Chemical Reaction
? Reactions in Aqueous Solutions
? Predicting whether a reaction
will occur
? Reactions in which a solid
forms
? Describing reactions in
aqueous solutions
? Reactions that form water
? Acids and bases
? Reactions of metals with Nonmetals (Oxidation-Reduction)
? Oxidation number
? The role of the electron in oxidation-reduction
? Electrochemistry: electrolytic and galvanic cells

Chemical Composition and Quantities
? Weight calculations
? Atomic mass?counting atoms by weight
? The mole and molar mass
? Formulas of compounds
? Empirical formulas
? Molecular formulas
? Reading chemical equations
? Moles and mole relationships
? Mass calculations
? Calculations involving limiting reactants

Modern Atomic Theory
? Electromagnetic radiation and energy
? Hydrogen energy levels and hydrogen orbitals
? Bohr model of the atom
? Wave mechanical model of the atom
? Atomic properties of the Periodic Table
? Electron configuration
? Electron arrangements
? Binding force
? Types: ionic; covalent; metallic; hydrogen bonding; Van der Waals (including London dispersion forces)
? Relationships to states; structure; and properties of matter
? Polarity of bonds; electro negativities
? Molecular models
? Lewis structures
? Valence bond: hybridization of orbitals; resonance; sigma and pi bonds
? VSEPR (Valence Shell Electron Pair Repulsion)
? Geometry of molecules and ions; structural isomerism of simple organic molecules and coordination complexes; dipole moments of molecules; relation of properties to structure

States of Matter
? Gases
? Pressure; volume; temperature
? Laws of ideal gases
? Charles?s law; Avogadro?s Law; Boyle?s Law; The Ideal Gas Law
? Equation of state for an ideal gas
? Partial pressures
? Kinetic-molecular theory
Interpretation of ideal gas laws on the basis of this theory
? Avogadro's hypothesis and the mole concept
? Dependence of kinetic energy of molecules on temperature
? Deviations from ideal gas laws
? Gas stoichemistry
? Liquids and solids
? Liquids and solids from the kinetic-molecular viewpoint
? Phase diagrams of one-component systems
? Evaporation and vapor pressure
? The solid state?types of solids
? Bonding in solids
? Changes of state; including critical points and triple points
? Structure of solids; lattice energies

Solutions
? Types of solutions and factors affecting solubility
? Mass percent
? Molarity
? Dilution
? Intermolecular forces
? Methods of expressing concentration
? Raoult's law and colligative properties; osmosis
? Solution reaction
? Neutralization
? Normality
? Stoichiometry
? Ionic and molecular species present in chemical systems:
net ionic equations
? Balancing of equations including those for redox reactions
? Mass and volume relations with emphasis on the mole concept; including empirical formulas and limiting reactants
? Acids and Bases
? Acid strength
? Water as an acid and base
? pH Scale
? Determining the pH of strong acid solutions
? Buffered Solutions

Equilibrium
? Concept of dynamic equilibrium; physical and chemical; Le
? Le Chatelier's principle; equilibrium constants
? Quantitative treatment
? Equilibrium constants for gaseous reactions: Kp; Kc
? Equilibrium constants for reactions in solution
? Chemical equilibrium
? Heterogeneous equilibria
? Solubility equilibria
? Oxidation-Reduction Reactions and Electrochemistry
? Oxidation-reduction reactions
? Reactions between nonmetals
? Balancing oxidation using Half-Reaction Method
? Electrochemistry
? Corrosion
? Electrolysis

Nuclear Energy
? Radioactive decay
? Nuclear transformations
? Detection of radioactivity ---Half-life
? Using radioactivity to date objects
? Nuclear fission
? Nuclear reactors
? Nuclear fusion
? Repercussions of nuclear energy

? Vocabulary Sort?Structural analysis of terms.
? Modeling compounds
? Naming compounds---the rules
? Reading names
? (Lab) Temperature Conversion Students learn how to convert measurements from one scale to another Celsius to kelvins; Celsius to Fahrenheit and Fahrenheit to Celsius
? (Lab) Writing equations in Algebra and Chemistry a comparison

(Lab) Distinguishing between physical and chemical changes. Students observe:
Milk sour
Breaking up rocks
Water vaporizing
? Atoms?conventional model study
? Distinguishing between physical and chemical properties
? Distinguishing between physical and chemical changes
? Modeling physical changes on the atomic level?journal diagrams
? Distinguishing between mixtures and pure substance?commercial product examination
? (Lab) Molar Mass and Avogadro?s Number
? (Lab) Molecular Mass
? Calculating percent composition
? (Lab) amounts of reactants and products
? Determination of empirical formulas
? Reading the Periodic Table
? (Lab) Limiting reagents and yield of reaction
? Rutherford?s logic

? Describing chemical reactions
(Lab) Secret Message?lemon juice messages
? Writing chemical equations
? Reading chemical equations
? Categorizing types of reactions
? (Lab) Precipitation and acid-base reactions
? (Lab) Activity series of metals
? (Lab) Redox reactions
? Balancing equations
? (Lab) CaO Experiment - Exothermic Reactions
? Predicting reactions
? (Lab) Oxidation states
? (Lab) Electrical conductivity of aqueous solutions
? Predicting precipitates in solutions when two ionic compounds are mixed
? Describing reactions in aqueous solutions
? Reactions between strong acids and strong bases
? Oxidation and Reduction
? (Lab) Rust

? ? (Lab) Jelly Bean Experiment - Mass Measurement
? The mole
? Calculating mass using amu
? Review of Avogadro?s number
? Calculating the number of atoms
? Calculating molecular formulas
? Molar mass?converting given a chemical compound
? (Lab) Verifying molecular formulae
? Determining empirical formulas

? The Bohr model
?
? (Lab) Wave/Particle modeling
? Diagramming/describing orbitals and energy levels
? The Periodic Table from the perspective of atomic structure
? Examining electron configuration and arrangement
? (Lab) Electronegativity
? Diagramming/describing bonding
? Bonding and states of matter
? (Lab) Molecular geometry
? Classifying types of bonds
? Bond polarity and molecular polarity
? Lewis structures and valence electrons
? Stability and noble gas electron configuration
? Predicting molecular structure using the VSEPR model

? Boyle?s Law
? (Lab) atmospheric pressure
? Pressure unit conversion
? (Lab) Analysis of Boyle?s data
? Calculating volume using Boyle?s Law
? Calculating pressure using Boyle?s Law
? Charles?s Law?absolute zero
? Calculating volume using Charles?s Law
? Calculating temperature using Charles?s Law
? Avogadro?s Law
? The Ideal Gas Law?changing conditions
?(Lab) Popcorn and Charles?s Law
?Dalton?s Law of Partial Pressure
?(Demonstration Lab) Potassium chlorate and the production of oxygen by thermal decomposition
? Using the Kinetic Molecular Theory to explain gas law observations
? Phase changes
? Energy requirements for changes of state
? Water and phase changes
? Calculating energy changes?solid to liquid
? Diagramming crystalline solids

? (Lab) Solubility
? Concentration of a solution
? Calculating mass percent
? Determining the mass of a solute
? Calculating molarity
? Calculating ion concentration
? Calculating the number of moles
? (Lab) Dilution
? Calculating concentrations of diluted solutions
? Stoichiometry of solution reaction
? (Lab) Salt - Solutions and Solubility
? (Lab) pH Indicator? Neutralization
? Calculating equivalent weight
? Calculating the pH of strong acid solutions
? Writing conjugate bases
? pH scale?identifying the pOH and pH for solutions

? Collision model of chemical reactions
? Reaction rates?catalysts
?Equilibrium conditions
? Calculating values for the equilibrium constant
? Le Chatelier?s Principle?predicting changes when equilibrium is disturbed
? (Lab) Dynamic equilibria
? Qualitative analysis
?(Lab) Reaction quotient
? Writing solubility product expressions
? Assigning oxidation states
? Identifying oxidation and reduction in a reaction
? Identifying oxidizing and reducing agents
? Electrochemical cells
? (Demonstration Lab) Copper and nitric acid

? Equations that describe radioactive decay
? Electron capture
? Particle bombardment
? (Lab) Half-life simulation
? Effects of radiation

23. Texts & Supplemental Instructional Materials

Chemistry; 5th Edition; Zumdahl; Houghton-Mifflin Co.; 2000
Prentice Hall Chemistry; 6th Edition; Wilbraham; Antony C.; Dennis D. Staley; Michael S. Matta; and Edward L. Waterman
24. Key Assignments

Labs
? (Lab) Dynamic equilibria
? (Lab) Temperature Conversion Students learn how to convert measurements from one scale to another Celsius to kelvins; Celsius to Fahrenheit and Fahrenheit to Celsius
? (Lab) Writing equations in Algebra and Chemistry a comparison
? (Lab) Distinguishing between physical and chemical changes. Students observe:
Milk sour
Breaking up rocks
Water vaporizing
? (Lab) Molar Mass and Avogadro?s Number
? (Lab) Molecular Mass
? (Lab) amounts of reactants and products ? Vocabulary Sort?Structural analysis of terms.
? (Lab) Limiting reagents and yield of reaction
? (Lab) Secret Message?lemon juice messages
? (Lab) Precipitation and acid-base reactions
? (Lab) Activity series of metals
? (Lab) Redox reactions
? (Lab) Oxidation states
? (Lab) Electrical conductivity of aqueous solutions
? (Lab) CaO Experiment - Exothermic Reactions
? (Lab) Rust
? (Lab) Jelly Bean Experiment - Mass Measurement
? (Lab) Verifying molecular formulae
? (Lab) Wave/Particle modeling
? (Lab) Electronegativity
? (Lab) Molecular geometry
? (Lab) atmospheric pressure
? (Lab) Analysis of Boyle?s data
? (Lab) Popcorn and Charles?s Law
? (Demonstration Lab) Potassium chlorate and the production of oxygen by thermal decomposition
? (Lab) Dilution
? (Lab) Salt - Solutions and Solubility
? (Lab) pH Indicator? Neutralization
? (Lab) Solubility
? (Lab) Reaction quotient
? (Lab) Half-life simulation
? (Demonstration Lab) Copper and nitric acid

Other Sample Assignments
? Reading names
? Atoms?conventional model study
? Distinguishing between physical and chemical properties
? Distinguishing between physical and chemical changes
? Modeling physical changes on the atomic level?journal diagrams
? Distinguishing between mixtures and pure substance?commercial product examination
? Calculating percent composition
? Determination of empirical formulas
? Reading the Periodic Table
? Describing chemical reactions
? Writing chemical equations
? Reading chemical equations
? Balancing equations
? Predicting precipitates in solutions when two ionic compounds are mixed
? Describing reactions in aqueous solutions
? Oxidation and Reduction
? Calculating mass using amu
? Calculating the number of atoms
? Calculating molecular formulas
? Determining empirical formulas
? Diagramming/describing orbitals and energy levels
? Diagramming/describing bonding
? Bonding and states of matter
? Classifying types of bonds
? Stability and noble gas electron configuration
? Predicting molecular structure using the VSEPR model
? Pressure unit conversion
? Calculating volume using Boyle?s Law
? Calculating pressure using Boyle?s Law
? Calculating volume using Charles?s Law
? Calculating temperature using Charles?s Law
? The Ideal Gas Law?changing conditions
? Using the Kinetic Molecular Theory to explain gas law observations
? Calculating energy changes?solid to liquid
? Diagramming crystalline solids
? Calculating mass percent
? Determining the mass of a solute
? Calculating molarity
? Calculating ion concentration
? Calculating the number of moles
? Calculating concentrations of diluted solutions
? Calculating equivalent weight
? Calculating the pH of strong acid solutions
? Writing conjugate bases
? pH scale?identifying the pOH and pH for solutions
? Reaction rates?catalysts
? Calculating values for the equilibrium constant
? Writing solubility product expressions
? Assigning oxidation states
? Identifying oxidation and reduction in a reaction
? Identifying oxidizing and reducing agents

25. Instructional Methods and/or Strategies:
? Socratic seminar
? Group Investigation
? Example study and analysis
? Practice solutions
? Reciprocal Reading
? Labs
? Simulations

26. Assessment Methods and/or Tools
? Student work will be graded by teacher
? Student portfolios will be kept by teacher and assessed at semesters and at year?s end.
? Students will perform laboratory experiments where they can apply their knowledge to real world situations.
? Tests will be used as appropriate.
? Final exams will be given once per trimester and must be passed with 60% accuracy to receive credit.
? A five point writing rubric will be used to assess essays.
? In-class writings; quizzes; class activities; unit tests
? Self- and Peer-assessment
? Informal and on-going assessment
? Teacher conferencing
? Major papers; performances; and projects
? Labs are measured by attached rubric
? Grading:
20% Labs
20% Study Sheets
20% Test/Quiz
15% Final/Midterm
15% Participation
10% Portfolio

Level Scientific Procedures and Reasoning Strategies Interpretation and Communication of data Scientific Concepts
Novice Beginning use of tools and procedures.

Application of tools and procedures may not relate to the investigation. Beginning use of strategies.

Strategy use may be incomplete and may not bring about a successful completion of the investigation. Beginning level explanation.

There is a beginning use of notation; scientific repre-sentation; and termin-ology that may not relate to the task.

The explanation may be missing a conclusion or recorded data. Beginning level of understanding of underlying concepts; principles or theories.

Beginning level of understanding of observable characteristics and properties of objects; organisms or patterns.
Apprentice Used some appropriate tools and procedures.

Parts of the investigation demonstrate effective use of tools and procedures.
Used a strategy that was somewhat useful; leading to partial completion of the task/investigation.

Some evidence of scientific reasoning used.

Testing; questioning; recording and interpreting data is partially complete. The explanation is partially complete.

There is some use of appropriate notation; scientific representation; and terminology

Conclusions are partially supported by data and explanation. Some reference to relevant scientific concepts; principles; or theories.

Demonstrates partial understanding of observable characteristics and properties of objects; organisms or patterns.
Practitioner Used appropriate tools and technologies to gather and analyze data; with only minor errors. Used a strategy that led to completion of the investigation/task.

Used effective scientific reasoning.

Used testable questions; conducted experiment; and supported results with data. A clear explanation was presented.

Used scientific representations; notation and terminology.

Used data to support conclusions Made reference to relevant scientific concepts; principles or theories.

Demonstrates understanding of observable character-ristics and properties of objects; organisms; or patterns.
Expert Accurately and proficiently used all appropriate tools and technologies to gather and analyze data. Used a sophisticated strategy and revised strategy where appropriate to complete the task.

Employed refined and complex reasoning

Framed testable questions; designed experiment; gathered and recorded data; analyzed data; and verified results Provided clear; effective explanation detailing how the task was carried out.

Precisely used multiple scientific representations; notations and terminology.

Interpretation of data supported conclusions; and raised new questions or was applied to new contexts. Provided evidence of in-depth; sophisticated understanding of relevant scientific concepts; principles or theories.

Demonstrates understanding of observable characteristics and properties of objects; organisms; or patterns.

Went beyond the task/investigation to make other connections or extend thinking.

D. OPTIONAL BACKGROUND INFORMATION

28. Context for Course (optional)
29. History of Course Development

The RenArts curriculum team revised this course adhering more closely to the A-G course outline template. One of A-G?s cadre of experts met with our team at length and helped us better structure and format our course outlines.

School country

United States

School state

California

School city

Los Angeles

High school

Renaissance Arts Academy

School / district Address

1800 Colorado Blvd.

School zip code

90065

Requested competency code

Lab Science

Date submitted

Approved

Yes

Approved competency code

  • LCHM
  • Chemistry

Approved date

Online / Virtual

No