1 CHEMISTRY The Nature of Chemistry Topic(s) Concepts Competencies (Eligible Anchor Descriptions Vocabulary Textbook Duration (with Standards) Content) Pages (in days) The Scientific 3.2.10.A6: CHEM.A.1.1.1: CHEM.A.1.1: The Nature of Chemistry L1: Ch 1 (p3-27) 2-5 Method • Compare and contrast • Classify physical or • Identify and describe how Analytical chemistry scientific theories. chemical changes within a observable and measurable Biochemistry Laboratory • Know that both direct system in terms of matter properties can be used to Chemistry Procedure(s) and indirect observations and/or energy. classify and describe matter Inorganic chemistry and Safety are used by scientists to and energy. Organic chemistry study the natural world CHEM.A.1.1.2: Physical chemistry The Metric and universe. • Classify observations as Science System, • Identify questions and qualitative and/or Technology Significant concepts that guide quantitative. Figures, and scientific investigations. Scientific Methods and L1 and L2: 2-5 Measurement • Formulate and revise CHEM.A.1.1.3: Laboratory Safety & Teacher and explanations and models • Utilize significant figures to Procedures department using logic and evidence. communicate the Control generated • Recognize and analyze uncertainty in a quantitative Control experiment materials; Flinn alternative explanations observation. Dependent variable Scientific Safetly and models. Erlenmeyer flask (E-flask) Contract • Explain the importance of Graduated cylinder accuracy and precision in Hypothesis making valid Independent variable measurements. Laboratory balance Laboratory burner 3.2.C.A6: Law • Examine the status of Observation existing theories. Science Scientific method • Evaluate experimental Theory information for relevance Variable and adherence to Laboratory equipment science processes. Beaker • Judge that conclusions Beaker tongs are consistent and logical Buret with experimental Buret clamp conditions. Chemical splash googles • Interpret results of Control experimental research to Control experiment predict new information, Crucible and cover propose additional Crucible tongs investigable questions, or Dropper bottles 1 CHEMISTRY advance a solution. Evaporating dish • Communicate and Funnel defend a scientific Hot plate argument. Laboratory apron Micropipettes Pasteur pipettes Petri dish Ring stand Rubber policeman Rubber stoppers Scoopula Spatula Test tube Test tube brush Test tube holder/ test tube clamp Test tube tongs Thermometer Utility clamp Watch glass Well plate/ spot plate Wire gauze Math- Metric system, L1: C1 (p11-16) 5-10 Significant Figures, Measurement Absolute zero Accepted value Accuracy Celcius temperature scale Dimensional analysis Error Experimental value Heat Human error Hydrometer Kelvin temperature scale Mass Matter Metric system Percent error Precision Qualitative Quantitative 1 CHEMISTRY Random error Rounding Scientific notation Significant digits (significant figures) Specific gravity System Internacional (SI) Systemic error Temperature Unit Weight Metric prefixes Giga- (G, 109) Mega- (M, 106) Kilo- (K, 103) deci- (d, 10-1) centi- (c, 10-2) milli- (m, 10-3) micro- (µ, 10-6) nano- (n, 10-9) pico- (p, 10-12) Metric Units Atmosphere (atm) Cubic meter (m3) Degrees Celcius (°C) Density (d) Gram (g) Joule (J) Kelvins (K) Liter (L) Mole (mol) Volume (V) Newton (N) Pascal (Pa) Hertz (Hz or 1/sec or sec-1) 1 CHEMISTRY Matter & Energy Topic(s) Concepts Competencies Anchor Descriptions Vocabulary Textbook Duration (with Standards) (Eligible Content) Pages (in days) Matter & Energy 3.2.10.A1: CHEM.A.1.1.1: CHEM.A.1.1: Matter and Energy L1: Ch 2 (p20-41); 8-15 • Identify properties of • Classify physical or chemical • Identify and describe how Allotrope Ch 5 (p135-141), matter that depend on changes within a system in observable and measurable Alloy and Ch 10 (p288- sample size. terms of matter and/or properties can be used to Amorphous solid 293) • Explain the unique energy. classify and describe matter Atom properties of water and energy. Boiling (polarity, high boiling CHEM.A.1.1.2: Boiling point point, forms hydrogen • Classify observations as Chemical change bonds, high specific heat) qualitative and/or Chemical property that support life on Earth. quantitative. Chromatography Colloid 3.2.10.B2: CHEM.A.1.1.3: Compound • Explain how the overall • Utilize significant figures to Condensation energy flowing through a communicate the uncertainty Crystal system remains constant. in a quantitative observation. Distillation Electrolysis 3.2.12.A1: CHEM.A.1.1.4: Element • Compare and contrast • Relate the physical Energy colligative properties of properties of matter to its Evaporation mixtures. atomic or molecular Freezing • Compare and contrast the structure. Freezing point unique properties of water Fusion to other liquids. CHEM.A.1.1.5: Gas • Apply a systematic set of Glass 3.2.C.A1: rules (IUPAC) for naming Heterogeneous mixture • Differentiate between compounds and writing Homogeneous mixture physical properties and chemical formulas (e.g., CHEM.A.1.2: Kinetic energy chemical properties. binary covalent, binary ionic, • Compare the properties of Liquid Matter • Differentiate between pure ionic compounds containing mixtures. substances and mixtures; polyatomic ions). Melting differentiate between Melting point Mixture heterogeneous and CHEM.A.1.2.1: Phase homogeneous mixtures. • Compare properties of Phase change solutions containing ionic or Phase diagram 3.2.C.B2: molecular solutes (e.g., Physical change • Explore the natural dissolving, dissociating). Physical property tendency for systems to Plasma move in a direction of Potential energy 1 CHEMISTRY disorder or randomness CHEM.A.1.2.2: Pure substance (entropy). • Differentiate between Radiant energy homogeneous and Solid 3.2.10.B3: heterogeneous mixtures Solution • Explain how heat energy (e.g., how such mixtures can Sublimation will move from a higher be separated). Suspension temperature to a lower Symbol temperature until CHEM.A.1.2.3: Triple point equilibrium is reached. • Describe how factors (e.g., Unit cell temperature, concentration, Vapor surface area) can affect Vapor pressure solubility. Vaporization CHEM.A.1.2.4: • Describe various ways that concentration can be expressed and calculated (e.g., molarity, percent by mass, percent by volume). CHEM.A.1.2.5: • Describe how chemical bonding can affect whether a substance dissolves in a given liquid. 1 CHEMISTRY Atomic Theory and Structure Topic(s) Concepts Competencies Anchor Descriptions Vocabulary Textbook Duration (with Standards) (Eligible Content) Pages (in days) EMR 3.2.10.A5: CHEM.A.2.1.1: CHEM.A.2.1: EMR L1: Ch 11 10 • Describe the historical • Describe the evolution of • Explain how atomic theory Absorption spectrum (p324-327) Atomic Structure development of models atomic theory leading to serves as the basis for the Amplitude and History of the atom and how the current model of the study of matter. Color they contributed to atom based on the works Electromagnetic radiation Nuclear Chemistry modern atomic theory. of Dalton, Thomson, Electromagnetic spectrum and Radioactivity Rutherford, and Bohr. Emission spectrum 3.2.12.A2: Energy level Electron • Distinguish among the CHEM.A.2.1.2: Excited state Configurations isotopic forms of • Differentiate between the Frequency (ν or or ν) elements. mass number of an Ground state • Explain the probabilistic isotope and the average Heisenberg uncertainty principle nature of radioactive atomic mass of an Matter-wave decay based on element. CHEM.A.2.2: Photoelectric effect subatomic • Describe the behavior of Photon rearrangement in the CHEM.A.2.2.1: electrons in atoms. Plank’s constant (h) atomic nucleus. • Predict the ground state Principle quantum number (n) • Explain how light is electronic configuration Quantized absorbed or emitted by and/or orbital diagram for Quantum electron orbital a given atom or ion. Spectrum transitions. Speed of light (c) CHEM.A.2.2.2: Wavelength (λ) 3.2.12.A3: • Predict characteristics of • Explain how matter is an atom or an ion based People transformed into energy on its location on the Bohr, Neils in nuclear reactions periodic table (e.g., DeBroglie, Louis according to the number of valence Einstein, Albert equation E=mc2. electrons, potential types Heisenberg, Werner of bonds, reactivity). Planck, Max 3.2.C.A2: • Compare the electron CHEM.A.2.2.3: Atomic Structure & History L1: Ch 3 6-7 configurations for the • Explain the relationship Atom (p46-78); first twenty elements of between the electron Atomic mass number (atomic Ch 11 the periodic table. configuration and the mass, or mass number: A) (p322-323) atomic structure of a given Atomic mass unit (amu) 3.2.C.A3: atom or ion (e.g., energy Atomic number (Z) • Identify the three main levels and/or orbitals with Average atomic mass types of radioactive electrons, distribution of Cathode ray Compound 1 CHEMISTRY decay and compare electrons in orbitals, Electron (e-) their properties. shapes of orbitals). Electrostatic Attraction • Describe the process of Element radioactive decay by CHEM.A.2.2.4: Ion using nuclear equations • Relate the existence of Isotope and explain the concept quantized energy levels to Molecule of half-life for an atomic emission spectra. Neutron (n0) isotope. Nucleus • Compare and contrast Nuclide nuclear fission and Proton (p+) nuclear fusion. Strong (Nuclear) Force 3.2.C.A5: People • Recognize discoveries Ancient Greeks: Aristotle, from Dalton (atomic Democritus, Leuccipus theory), Thomson (the Bequerel, Henri electron),