Chemistry A Course Syllabus
Huntington ParkHigh School
Instructor: Mr. Adolfo
Overview
Chemistry A is a course in high school chemistry with emphasis on the experimental development of basic concepts through laboratory investigations, and the mathematical expression of laboratory findings.
Mastery
Students are allowed to repeat any homework assignment for full credit. Assignments are re-evaluated w/ original criteria.
Late Assignments
Late assignments can be turned in until two weeks prior to the end of the semester. The instructor will periodically make updated summaries of all course assignments available to those who wish to make up missed assignments.
Absences and Tardiness
Absences equate to gaps in one's course work. Since legitimate absences do occur, it is expected that the student will complete missed and/or make-up work. Excessive absences may lead to academic failure.
Tardiness disrupts the whole class and will count directly against your class participation grade. If you are late, slip in quietly. Excessive tardiness will lead to a parent conference.
How Grades are Computed
Final Letter Grades will be based on a percentage of total points available at the end of the Semester.
A:90% and above
B:80% and above
C:70% and above
D: 60% and above
F:below 60%
Points for Individual Assignments
Daily Classwork:10 Points
Weekly Homework: 25 Points
Weekly Extra Credit:25 Points
Laboratories:50 Points
Quizzes50 Points
Projects:100 Points
Final Examinations200 Points
Required Materials
Spiral Bound Notebook
Scientific Calculator
All assignments (except projects, quizzes, and exams) will be completed in a bound spiral notebook. Notebooks will be collected for grading approximately every two weeks.
Topics Covered:
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.
a. Atomic number and atomic mass.
b. Identify metals, semimetals, nonmetals, halogens, alkali metals, alkaline earth metals and transition metals,
c. Trends in ionization energy, electronegativity, and sizes of ions and atoms.
d. The number of electrons available for bonding.
e. The nucleus of the atom contains most of its mass.
f.* The lanthanide, actinide, and transactinide elements and that the transuranium elements were synthesized and identified in laboratory experiments.
g.* The position of an element in the periodic table relates to its quantum electron configuration and to its reactivity with other elements in the table.
h.* The experimental basis for Thomson’s discovery of the electron, Rutherford’s nuclear atom, Millikan’s oil drop experiment, and Einstein’s explanation of the photoelectric effect.
i.* The development of the quantum theory of atomic structure and the historical importance of theBohr model of the atom.
j.* Spectral lines are the result of transitions of electrons between energy levels and that these lines correspond to photonswith a frequency related to the energy spacing between levels by using Planck’s relationship (E = hv).
2. Biological, chemical, and physical properties of matter result from the ability of atoms to form bonds from electrostatic forces betweenelectrons and protons and between atoms and molecules.
a. Atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons toform ionic bonds.
b. Chemical bonds between atoms in molecules such as H2, CH4, NH3, H2CCH2, N2, Cl2, and many large biological moleculesare covalent.
c. Salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction.
d. Atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular forces aretoo weak to hold the atoms or molecules in a solid form.
e. Draw Lewis dot structures.
f.* Predict the shape and polarity of simple molecules from Lewis dot structures.
g.* Electronegativity and ionization energy relate to bond formation.
h.* Identify solids and liquids held together by Van der Waals forces or hydrogen bonding and relate these forces tovolatility and boiling/ melting point temperatures.
3. The conservation of atoms in chemical reactions leads to the principle of conservation of matter and the ability to calculate the mass ofproducts and reactants.
a. Describe chemical reactions by writing balanced equations.
b. The quantity one mole is set by defining one mole of carbon 12 atoms to have a mass of exactly 12 grams.
c. One mole equals 6.02 10 23 particles (atoms or molecules).
d. Determine the molar mass of a molecule from its chemical formula and a table of atomic masses and how to convert the mass of a molecular substance to moles, number of particles, or volume of gas at standard temperature and pressure.
e. Calculate the masses of reactants and products in a chemical reaction
f.*Calculate percent yield in a chemical reaction.
g.* Identify oxidation and reduction reactions and balance oxidation-reduction reactions.
4. The kinetic molecular theory describes the motion of atoms and molecules and explains the properties of gases.
a. The random motion of molecules and their collisions with a surface create the observable pressure on that surface.
b. Random motion of molecules explains the diffusion of gases.
c. Apply the gas laws to relations between the pressure, temperature, and volume of any amount of an ideal gas or anymixture of ideal gases.
d. The values and meanings of standard temperature and pressure (STP).
e. Convert between the Celsius and Kelvin temperature scales.
f. There is no temperature lower than 0o Kelvin (Absolute Zero).
g.* The kinetic theory of gases relates the absolute temperature of a gas to the average kinetic energy of its molecules or atoms.
h.* Students know how to solve problems by using the ideal gas law in the form PV = nRT.
i.* Students know how to apply Dalton’s law of partial pressures to describe the composition of gases and Graham’s law to predict diffusionof gases.
*Will be covered if time permits.