Course title
SCI7090Pre-requisite
Algebra I, Biology/Honors Biology or Principles of Science/Honors Principles of ScienceCourse description
Chemistry places emphasis on mathematical formulas; atomic history and structure; problem-solving; dimensional analysis and laboratory procedures. In the laboratory; students learn basic laboratory procedures and techniques; the laboratory provides an opportunity to illustrate the concepts discussed in class and in literature. A scientific calculator is strongly recommended. Prerequisite: Algebra I; Biology and/or Principles of Science.
This course is designed to expose the student to principles and applications of chemistry. The topics covered include: measurement; matter; the atom; the periodic table; nomenclature; formulas; equations; energy; bonding; reactions; the mole; acids and bases; biochemistry; gases and solution chemistry.
Course ExpectationsWhen the student has completed the course fulfilling all requirements; he/she will be able:To make and record observations.To develop a hypothesis based on their observations.To design and conduct an experiment to test a hypothesis.To distinguish between accuracy and precision.To make qualitative and quantitative measurements.To identify the number of significant figures in a measurement.To measure mass and volume.To calculate density of an object from experimental data.To distinguish different Metric prefixes.To convert from American / British standards units to Metric units and viceversa.To compare and contrast types of waves in terms of wavelength; frequency;and energy.To analyze line spectra to determine the identity of an unknown element.To analyze covalent compounds in terms of melting point and conductivity.To compare and contrast properties of covalent and ionic compounds.To construct Lewis structures for covalent compounds.To determine the average weights of each isotope of a fictitious element.To determine the relative abundance of isotopes of a fictitious element.To calculate from experimental data the atomic mass of a fictitious element.
Laboratory ActivitiesLaboratory skills are essential in any science course. The laboratory activities included this course provides students with visual and hands-on activities to help with the understanding of the concepts being learned. A total of 80% of the labs are Hands-On and account for 48 hours of the 60 hours of lab work to be completed.
Resources: Students use content powered by Florida Virtual School for the online component of the course. The Agua Fria Union High School District?s adopted materials for textbooks and other resources will be made available to students. A variety of other online websites and references will also be used as notes in the activities and labs.Students submit the results of all labs; homework; quizzes and tests electronically to the instructor. All final exams are taken in a supervised classroom at the end of the course. Students must pass their final exam in order to get credit for the course. Students must complete all labs prior to taking the final exam to receive lab credit for course.Safety: As with any laboratory science; in some investigations safety issues will arise. Prior to starting any laboratory work; the student and a parent or guardian must read; sign; and submit the attached safety contract. Safety rules must be strictly adhered to and safety goggles must be worn for ANY ACTIVITY INVOLVING CHEMICALS; GLASSWARE; or A HEAT SOURCE.
Student Evaluation
Grading: A = 90%+B = 80-89%C = 70-79%D = 60-69%F = below 60% or failed the final exam
Required Materials:High-speed internet connection (provided)Computer (provided)Headphones (provided if necessary)Various lab materials which will be listed for each lab. (provided)
Labs:Copies of all lab reports; pictures; graphs or other materials made will be compiled in a digital or print notebook. There will be at least three appropriate/relevant pictures for each lab. Six sample labs from the complete labs list below are included.
?CHEMISTRY ? Semester 1†SAMPLE LAB SEQUENCETable of Contents:1. The Cat?s Meow (Hands-on) ? 0.5 hour2. Raisin? It Up (Hands-on) ? 1.5 hours3. Density of Solids; Liquids; & Gases (Hands-on) ? 2 hours4. Quantitative and Qualitative Measurements (Hands-on) ? 2 hours5. Hit the Bulls eye (Hands-on) ? 0.5 hour6. Accuracy and Precision: Balance Lab (Virtual) ? 1 hour7. Isotopes & Atomic Mass (Hands-on) ? 1.5 hours8. Calculating Molar Mass (Hands-on) ? 1 hour9. Line Spectra (Virtual) ? 1 hour10. Electron Probability (Hands-on) ? 1.5 hours11. Graphing Periodic Trends (Virtual) ? 2 hours12. Properties of Metals and Non-metals (Hands-on) ? 1 hour13. Formula Writing: Ionic Compounds (Hands-on) ? 2 hours14. Covalent Bonding (Virtual) ? 1 hour15. Chemical Names & Formulas (Virtual) ? 1.5 hours16. Determining Empirical Formulas (Virtual) ? 1 hours17. Chemical and Physical Properties (Hands-on) ? 2 hours18. Conservation of Mass (Hands-on) ? 1.5 hours19. Decomposition of Baking Soda (Hands-on) ? 1.5 hours20. Chemical Reactions (Virtual) ? 1 hour21. S?Mores Stoichiometry (Hands-on) ? 2 hours22. Percent Yield (Virtual) ? 1 hourTOTAL: 30 hours (Hands-on = 21 hours; Virtual = 9 hours)CHEMISTRY ? Semester 2SAMPLE LAB SEQUENCE1. Properties of Water (Hands-on) ? 2.5 hours2. Phase Changes (Hands-on) ? 2 hours3. Gas Laws (Virtual) ? 1 hour4. Paper Chromatography (Hands-on) ? 2 hours5. Solubility of a Salt (Hands-on) ? 2 hours6. Molarity of a Solution (Hands-on) ? 2 hours7. Molar Mass Determination: Freezing Point Depression Method (Hands-on) ? 1 hour8. Calculating Calories (Hands-on) ? 1 hour9. Heat of Fusion (Hands-on) ? 2 hours10. Calorimetry (Virtual) ? 1 hour11. Entropy and Enthalpy (Hands-on) ? 1.5 hours12. Acids and Bases (Hands-on) ? 3 hours13. Neutralization of Antacids (Hands-on) ? 1 hour14. Acid ? Base Titration (Virtual) ? 1 hour15. Equilibrium (Hands-on) ? 1 hour16. Oxidation-Reduction (Hands-on) ? 1 hour17. Radioactive Decay (Hands-on) ? 1 hour18. Constructing a Solar Still (Hands-on) ? 2 hours19. Polymers (Hands-on) ? 2 hours20. The Egg: A Biochemical Storehouse (Hands-on) ? 1 hourTOTAL: 30 hours (Hands-on = 27 hours; Virtual = 3 hours)
CHEMISTRY ? Semester 1†LAB DETAILSModule 1 ? Chemistry and You3. Lesson 1.04 Matter and MeasurementsLab: Density of Solids; Liquids; and GasesType: Hands-on.Materials: scale; Metric ruler; graduated cylinder; wood cube; wood block; 10 pennies; iron nail; small piece of copper; water; 20-30 mL vegetable oil; 5 g salt; red; blue & green food coloring; zip-lock baggie.Time needed: 2 hours.Summary: Density is an important physical property of matter. The relationship between an object?s mass and its volume is called density. Density is calculated using the equation:density = mass/volume. The common unit of density is g/cm3; but since 1 cm3 = 1 mL; we can also use g/mL. In this laboratory activity; students will take measurements of mass and volume for different objects and use their measurements to calculate the object?s density.
Objectives: 1. to measure mass and volume.2. to define density.3. to calculate density of an object from experimental data.
AZ State Standards: Strand 1; Concept 2; #1 & 5; Strand 5; Concept 1 #1.Source: adapted from S. Panzilius: Maine West High School.
4. Lesson 1.06 Unit ConversionsLab: Qualitative and Quantitative MeasurementsType: Hands-on.Materials: scale; Metric ruler; graduated cylinder; wood block; cardboard box; small metal pieces; 10 pennies; water.Time needed: 2 hours.Summary: Everyone makes and uses measurements. Measurements are fundamental to science as well. It is important to be able to make measurements and to be able to convert between American / British Standard units of measurement and Metric units of measurement.Qualitative measurements are results given in a descriptive form without using numbers or measuring devices. They are based on observation. Quantitative measurements are results given in a numerical form usually using some type of measuring device. In this investigation; students will make both qualitative measurements and quantitative measurements. They will also practice converting from American / British Standard units of measurement to Metric units of measurement and vice versa.Objectives: 1. To make qualitative and quantitative measurements.2. To describe Metric units of length; mass; and volume.3. To distinguish different Metric prefixes.4. To convert from American / British standards units to Metric units and vice versa.AZ State Standards: Strand 1; Concept 2; #1 & 5; Strand 5; Concept 1 #1.Source: adapted from S. Panzilius: Maine West High School.
Module 417. Lesson 4.01 Chemical vs. PhysicalLab: Chemical and Physical ChangesType: Hands-on.Materials: apple; beaker; graduated cylinder; test tubes; sodium chloride; sodium bicarbonate; acetic acid; piece of paper; matches; candle; cabbage juice; calcium chloride; ice; watch glass; stove burner; beaker; food coloring; safety goggles.Time needed: 2 hours.Summary: Matter has both physical properties and chemical properties. Likewise; changes that occur to matter can be either physical or chemical. Physical changes are changes that do not alter the chemical composition of the substance. In chemical changes; also called chemical reactions; one or more substances change into different substances. A chemical change always results in a change in chemical composition of the substances involved. In this laboratory; students will conduct a series of mini-experiments in order to examine physical changes and chemical changes.Objectives: 1. To differentiate between physical and chemical changes in matter.2. To observe evidence for chemical changes (reactions).AZ State Standards: Strand 5; Concept 1; #1 & 2; Strand 5; Concept 4; #2.Source: adapted from S. Panzilius: Maine West High School.
CHEMISTRY ? Semester 2†LAB SEQUENCE
5. Lesson 5.06 ? Solubility and ConcentrationLab: Solubility Curve of a SaltType: Hands-on.Materials: ammonium chloride crystals; large test tube; 400 mL beaker; thermometer; scale;scoop; graduated cylinder; safety goggles; oven mitt; stove top burner.Time needed: 2 hours.Summary: The solubility of a solute is the amount of solute dissolved in a given amount of a certain solvent at equilibrium; under specified conditions (the ability to dissolve). Increasing the temperature usually increases the solubility of solids in liquids (endothermic changes only); and decreasing the temperature has the reverse effect (exception; gaseous solutions). In this activity; students will construct a solubility curve representing data collected experimentally. Masses of salt will be varied and temperatures required to dissolve it will be recorded.Objective: 1. To produce a solubility curve.2. To apply knowledge of solubility curves to predict solubility at differenttemperatures.AZ State Standards: Strand 5; Concept 1; #1.Source: unknown.
12. Lesson 7.01 ? Acids & BasesLab: Acids & BasesType: Hands-on.Materials: red cabbage; paring knife; large pot; stove top burner; small Dixie cups or 10 test tubes & test tube rack; vinegar; lime or lemon juice; orange juice; soda water; pickle juice; windex; tomato juice; shampoo; liquid soap; coke; milk; vitamin C; apple slice; baking soda; borax; aspirin; washing soap; table salt; coffee; sugar; mortar and pestle; spoon or small scoop; dropper; pH paper.Time needed: 3 hours.Summary: Acids and bases are present in many household products. Acid compounds give foods a sour taste. In solution; acids are electrolytes and they conduct electricity. Bases are compounds that react with acids to form water and a salt. Bases taste bitter and will have a slippery feel. Both acids and bases will cause indicators to change color. In this investigation; students will observe the properties of acids and bases and will determine which household substances are acids and which are basesObjectives: 1. To describe properties of acids and bases.2. To produce an acid-base indicator.3. To identify common products as acids or bases..AZ State Standards: Strand 5; Concept 1 #3; Strand 5; Concept 4; #11.Source: unknown.
16. Lesson 7.06 ? Oxidation and ReductionLab ? Oxidation-ReductionType: Hands-on.Materials: 20 dull pennies; º cup vinegar (acetic acid); 1 tsp sodium chloride; shallow glass or clear plastic dish; plastic spoon or fork; 2 clean steel screws or nails (not galvanized) or paper clips; water; measuring spoons; paper towels.Time needed: 1 hour.Summary: Oxidation and reduction always occur simultaneously. The substance gaining oxygen is oxidized and the substance losing oxygen is reduced. No oxidation occurs without reduction; and no reduction occurs without oxidation. Reactions that involve these processes are thus called oxidation-reduction reactions or redox reactions for short. In this laboratory; students will explore oxidation-reduction reactions.Objectives: 1. To define oxidation and reduction.2. To assign oxidation numbers to elements in a reaction.3. To describe and explain what occurs during a oxidation-reduction reaction.AZ State Standards: Strand 5; Concept 4; #12.Source: Florida Virtual Labs.
School country
United StatesSchool state
ArizonaSchool city
AvondaleSchool / district Address
1481 N. Eliseo Felix Jr. WaySchool zip code
85323Requested competency code
Lab ScienceDate submitted
Approved
YesApproved competency code
- LCHM
- Chemistry