Mrs. Ginger MartzChemistrySyllabus for the Year 2015-16
Course Description: Chemistry is the study of the composition, structure, and properties of matter and the changes it undergoes. This class should challenge you to think critically, solve problems creatively, and help you understand aspects of the natural world.
Required Classroom Materials:
- 3-ring binder for this class
- Lined Notebook Paper
- Pencils
- One set of 5 dividers
- Calculator (TI-30XA)
- Composition Notebook for laboratory work
Classroom Supplies: Please bring in a roll of paper towels and a box of Kleenex
Class Expectations: Students should come to class fully prepared. In order to be successful mastering the objectives of this course, it will be necessary to take part in classroom discussions, do all assignments and lab work and study for announced tests. All students are expected to follow all rules and work together without disrupting other students or groups. All county policies on BYOD will be enforced. Due to the nature of the subject matter, mature behavior is essential.
Grading: The final grade for each nine-week grading period will be based on various methods of assessment. These methods will include, but are not limited to, tests, homework, journals/logs, projects, portfolios, essays, organized notebooks, computer assignments, quizzes, and class participation. Late assignments will be graded for partial credit (25 points off per day late with a 3 day limit. After 3 days, the assignment will be a zero.). Each nine weeks, classwork will count 25%, labs will count 15%, tests will count 25%, quizzes will count 20% and the nine weeks exam will count 15%. The final average for the class will be computed according to the board policy with the final exam for non-exempt as 20% of the final average. Report cards will be distributed at the end of each nine week grading period. Students’ progress may be monitored using INOW.
Homework: Homework given is designed to reinforce concepts taught in class. Homework will be given regularly, but not every day. It will consist of practice problems and assigned reading. Homework bridges the gap between the classroom and home so that students can reinforce what they have learned and ensure the retention of information.
Labs: The labs completed require following and/or developing processes and procedures, taking observations, and data manipulations. Students communicate and collaborate in lab groups. However, each student will be required to write a laboratory assignment/report in a lab notebook for every lab they perform.
Quizzes: Quizzes are given frequently throughout each unit of study to ensure understanding and retention of information.
Tests: Major tests will be given at the end of each unit. These will be evaluated to ensure mastery of all objectives.
Make-up work: Students with excused absences are allowed to make up missing assignments. Students are responsible for checking the assignment box for missed assignments/handouts. Make-up work or a missed test will be given a grade of zero until it has been completed and graded.Make-up work for excused absences is due within 2 days of returning to class. If multiple days are missed, the teacher and student will determine an appropriate deadline for all work to be completed. Missed labs (with an excused absence) will be marked as ‘E’ meaning excused, and will not count against a student’s average.
Class Updates: If you or your parent would like to receive classroom updates, I have created a Remind text message account. If you would like to join, please text ______to ______.
Conference Information: Parents are strongly encouraged to contact the teacher with any concerns they have about their child’s performance in this class. You may call the school at 342-2670 and leave a message or you may e-mail me at . Please be sure to include your name, your child’s name, phone number and the best time to call.
Alabama Science Course of Study: Chemistry, 2005
1.Differentiate among pure substances, mixtures, elements, and compounds.
•Distinguishing between intensive and extensive properties of matter
•Contrasting properties of metals, nonmetals, and metalloids
•Distinguishing between homogeneous and heterogeneous forms of matter
2.Describe the structure of carbon chains, branched chains, and rings.
3.Use the periodic table to identify periodic trends, including atomic radii, ionization energy, electronegativity,
and energy levels.
•Utilizing electron configurations, Lewis dot structures, and orbital notations to write chemical formulas
•Calculating the number of protons, neutrons, and electrons in an isotope
•Utilizing benchmark discoveries to describe the historical development of atomic structure, including
photoelectric effect, absorption, and emission spectra of elements
Example: Thomson’scathode ray, Rutherford’s gold foil, Millikan’s oil drop,
and Bohr’s bright line spectra experiments
4. Describe solubility in terms of energy changes associated with the solution process.
•Using solubility curves to interpret saturation levels
•Explaining the conductivity of electrolytic solutions
•Describing acids and bases in terms of strength, concentration, pH, and neutralizationreactions
•Describing factors that affect the rate of solution
•Solving problems involving molarity, including solution preparation and dilution
5.Use the kinetic theory to explain states of matter, phase changes, solubility, and chemical reactions.
Example:water at 25 degrees Celsiusremainsin the liquid state becauseofthestrongattraction between water molecules while kinetic energy allowsthesliding of molecules past oneanother
6.Solve stoichiometric problems involving relationships among the number of particles, moles,and masses of
reactants and products in a chemical reaction.
•Predicting ionic and covalentbond types and products given known reactants
•Assigning oxidation numbers for individual atoms of monatomic and polyatomic ions
•Identifying the nomenclature of ionic compounds, binary compounds, and acids
•Classifying chemical reactions as composition, decomposition, single replacement, ordouble
replacement
•Determining the empirical or molecular formula for a compound using percent composition data
7.Explain the behavior of ideal gases in terms of pressure, volume, temperature, and number of particles using
Charles’s law, Boyle’s law, Gay-Lussac’s law, the combined gas law, and the ideal gas law.
8.Distinguish among endothermic and exothermic physical and chemical changes.
Examples:endothermicphysical—phase changefrom ice to water,
endothermic chemical—reaction between citric acid solution andbaking soda,
exothermic physical—phase change from water vapor to water,
exothermic chemical—formation of water from combustion of hydrogenand oxygen
•Calculating temperature change by using specific heat
•Using Le Châtelier’s principle to explain changes in physical and chemical equilibrium
9.Distinguish between chemical and nuclear reactions.
•Identifying atomic and subatomic particles, including mesons, quarks, tachyons, and baryons
•Calculating the half-lifeof selective radioactive isotopes
•Identifying types of radiation and their properties
•Contrasting fission and fusion
•Describing carbon-14 decay as a dating method
Class______Period______
I have read the information for Mrs. Martz’s class and I understand the rules and expectations.
Student’s SignatureDate
Parent/Guardian SignatureDate
Please complete the information below. This will help me contact you if needed and will allow me to send you the weekly science scoop information email.
(Please Print)
Student’s Name:______Grade______
Mother/Guardian’s Name:______
Home #______Work #______Cell #______
Email Address: (Please print or use all capital letters to prevent errors.)
______
Father/Guardian’s Name:______
Home #______Work #______Cell #______
Email Address: (Please print or use all capital letters to prevent errors.)
______
It would help you teach my child more effectively if you knew:
______
______
______
Medical Concerns:
______
______
______