Chemistry Curriculum Map

Transcription

1 Aug 9-19 SC-HS-1.1.3Students will understand that solids, liquids and gases differ in the distances between molecules or atoms and therefore the energy that binds them together. In solids, the structure is nearly rigid; in liquids, molecules or atoms move around each other but do not move apart; and in gases, molecules or atoms move almost independently of each other and are relatively far apart. The behavior of gases and the relationship of the variables influencing them can be described and predicted. Distinguish between 4 phases of matter C lassify classes of matter Identify classes of matter Distinguish between physical & chemical properties A&H Draw Models of solids, liquids and gases Identify intrinsic & extrinsic properties PLVC careers in chemitry Demonstrate difference between displacement capacity Demo chemical changes Test: MC & OR 1

2 Aug 22-Sept 2 Sept 6-Sept 13 SC-HS-1.1.4Students will understand that in conducting materials, electrons flow easily; whereas, in insulating materials, they can hardly flow at all. Semiconducting materials have intermediate behavior. At low temperatures, some materials become superconductors and offer no resistance to the flow of electrons. SC-HS Students will: explain the relationships and connections between matter, energy, living systems and the physical environment; give examples of conservation of matter and energy. As matter and energy flow through different organizational levels (e.g., cells, organs, organisms, communities) and between living systems and the physical environment, chemical elements are recombined in different ways. Each recombination results in storage and dissipation of energy into the environment as heat. Matter and energy are conserved in each change. DOK 3 SC-HS Students will understand that heat is the manifestation of the random motion and vibrations of atoms. List all types of energy Use SI units for temperature K=273 + C Energy = mc T Demonstrate problem solving techniques A&H Draw enrgy diagrams and heating curves Understand SI prefixes Convert units of measure Define rules for significant figure calculations Use factor labeling Do calculations with correct significant figures Test: MC & ORQ 2

3 Sept SC-HS-1.1.5Students will explain the role of intermolecular or intramolecular interactions on the physical properties (solubility, density, polarity, conductivity, boiling/melting points) of compounds. The physical properties of compounds reflect the nature of the interactions among molecules. These interactions are determined by the structure of the molecule including the constituent atoms. Ways to conduct emperiments Ways to write results of scientific investigations Use SI units and calculations in real situations Density experiment Sept 19-Sept 30 Oct 3-Oct 7 SC-HS-1.1.2Students will understand that the atom s nucleus is composed of protons and neutrons that are much more massive than electrons. When an element has atoms that differ in the number of neutrons, these atoms are called different isotopes of the element. SC-HS-1.2.3Students will understand that the electric force is a universal force that exists between any two charged objects. Opposite charges attract while like charges repel.students will classify or make generalizations about elements from data of observed patterns in atomic structure and/or position on the periodic table. SC-HS-1.1.1The periodic table is a consequence of the repeating pattern of outermost electrons. Aristotle relating to dark ages John Dalton's atomic model JJ Thomson's atomic model Rutherford's Gold foil exp & atomic model Chadwick discovered electrons Atomic Mass units neutron discovery Illustrate Isotopes Electromagnetic radiation Continuous vs bright line spectra Max Planck E=hf Problems with Rutherford's atomic model Bohr model Draw various models of atoms Discussion questions Test Demo BLS/students record differences among elements Students draw Bohr models 1-18 Discussion questions Test 3

4 Oct17-Oct 28 Oct 31- Nov 22 Nov 28-Dec 16 SC-HS-1.1.1Students will classify or make generalizations about elements from data of observed patterns in atomic structure and/or position on the periodic table. The periodic table is a consequence of the repeating pattern of outermost electrons. SC-HS Students will understand that the atom s nucleus is composed of protons and neutrons that are much more massive than electrons. When an element has atoms that differ in the number of neutrons, these atoms are called different isotopes of the element. SC-HS-1.1.1Students will classify or make generalizations about elements from data of observed patterns in atomic structure and/or position on the periodic table. DOK2 SC-HS-1.1.7Students will: construct diagrams to illustrate ionic or covalent bonding; predict compound formation and bond type as either ionic or covalent (polar, nonpolar) and represent the products formed with simple chemical formulas. Bonds between atoms are created when outer electrons are paired by being transferred (ionic) or shared (covalent). A compound is formed when two or more kinds of atoms bind together chemically. Bohr Summerfield Atomic Model Quantum mechanics Quantum numbers Aufbau principle spdf clouds/ orbitals Duality of matter Heisenberg Uncertainty Principle Identify spd blocks on charts Periodic chart terminology Dot formulas Ionic bonding Ionic crystals Covalent bonding Octet rule Hybridization Electronegativity Polar Molecule vs nonpolar molecule Polyatomic ion molcular geometry models A&H Draw wave mechanical models of atoms List electron config for elements Do electron distribution Discover patterns on periodic table List electron cont from chart List electron distribution from chart Test MC/OR Students do dot formulas Students draw geometric models of Ionic crystals and polar or nonpolar molecules Model Molecules with 3D kit 4

5 Jan 4-13 Jan Jan 30-Feb 3 Feb 6-14 Feb Feb Name binary compounds Name traditional method for multivalented metals Name with stock method Name compounds containing polyatomic ions using both methods Write formulas when the name has been given Calculate formula weights of comp Calculate molecular mass Calculate % comp Define mole Illustrate mole problems Use Avogadro's number Determine empirical formula Determine molecular formula Rules for naming binary compounds Rules for traditional and stock method Use PAI along with rules for naming compounds Students write formulas from names Calculate formula and molecular wts Calculate% composition Work mole conversion problems Determine empirical & molecular formula 5

6 Mar1-Mar 9 SC-HS-1.1.6Students will: identify variables that affect reaction rates; predict effects of changes in variables (concentration, temperature, properties of reactants, surface area and catalysts) based on evidence/data from chemical reactions. Rates of chemical reactions vary. Reaction rates depend on concentration, temperature and properties of reactants. Catalysts speed up chemical reactions. DOK 3 SC-HS-1.1.8Students will: explain the importance of chemical reactions in a real-world context; justify conclusions using evidence/data from chemical reactions. Chemical reactions (e.g., acids and bases, oxidation, combustion of fuels, rusting, tarnishing) occur all around us and in every cell in our bodies. These reactions may release or absorb energy. DOK 3 Identify types of reactions Balance reactions Read solubility chart use,,aq in reactins Mar Predict products when given reactants Predict products Use solubility chart Use activity chart April 9-20 Solve stoichiometry problems Solve real world problems 6

7 April 23-May 4 Properties of gases Charles Gas Law Boyles Gas Law Combined Gas Law Ideal Gas Law May 7-11 Enrichment Labs: Chemical and Physical Change Nonreversible Reactions Throughout the Year ACT and Plan Prep: Assessments, OR, and other writings will address ACT \ 7