Accelerated Chemistry 2003-2004 Curriculum Plan
Text: Chemistry: Connections to Our Changing World, LeMay, et al., 2002
Topic / Skills / NJCCS /Scientific Processes / Critical thinking and analysis; Collaboration, peer review; Inquiry and problem solving; observation and data collection, inference / 5.1.A
5.1.B
5.4.A
Mathematical applications / Critical thinking and analysis; Collaboration, peer review; Inquiry and problem solving. Graphing, use of ESA (equation – substitution – answer) methodology, data analysis, statistics. Understand Accuracy, Precision / Uncertainty, Dimensional Analysis, Significant Figures, Exponents, SI (Metric) relationships and conversions / 5.3.A
5.3.B
5.3.D
Safety / Understand and agree to lab safety rules; identify and know how to use safety equipment / 5.1.C.1
Energy & Matter
Chapter 2 / Understand: Definitions, the Laws of Conservation of Energy and of Conservation of Matter, Temperature scales and conversions, Chemical and physical changes, Classifying Matter, Chemical and physical properties / 5.7.A
Atomic Structure
Chapters 3 and 24 / Understand the evolution of atomic models, Components of atomic structure (electrons, protons, and neutrons, including location, relative mass and relative electric charge). Define isotopes and use isotope notation, Write nuclear equations to represent types of nuclear changes, Define half-life and solve related problems including carbon dating, Distinguish between nuclear and chemical reactions using atomic mass units, Understand that the strong nuclear force holds the nucleus together,Recognize biological effects of radiation, Define fission and fusion and write nuclear equations to represent each, Understand the basic components of a nuclear reactor / 5.7.A.1
5.7.A.2
5.7.A.6
Electron Configuration
Chapter 4 / Describe the relationships among wavelength, frequency, velocity and energy, Recognize that the speed of light is a constant and the value of that constant, Describe the regions of the electromagnetic radiation (EMR) spectrum, Relate the line spectrum of hydrogen to the EMR spectrum and to other atoms, Distinguish between quantized and continuous systems, Describe the Bohr atomic model and its limitations, Contrast the quantum mechanic model to other previous atomic models, Write electron configurations using the Aufbau Principle, Hund’s Rule, and the Pauli Exclusion Principle / 5.7.A.3
5.7.A.8
Periodic Table
Chapters 5 and 6 / Identify groups / families and periods, Identify the representative families and the similarities and differences in their electron configurations, Use periodic patterns and trends to organize elements within a period or group / 5.7.A.5
Chemical Formulas and Chemical Bonding
Chapter 7 / Distinguish between ionic and covalent chemical bonding, Identify general properties of ionic compounds and of covalent compounds, Use electron dot diagrams to represent ionic and covalent bonding in formula units and molecules, Recognize types of ions: cation and anion, monatomic and polyatomic, Write formulas for and name ionic compounds, Write formulas for and name covalent compounds, Distinguish between molecular and empirical formulas, Describe and illustrate multiple covalent bonds, Describe the cause of polar and nonpolar covalent bonds and identify molecules containing each, Apply electronegativity concepts to predict the type of chemical bond between two atoms / 5.7.A.4
5.7.A.7
Molecular Shapes
Chapter 8 / Use Ball and Stick models to construct simple molecules, Draw and describe the shape of simple molecules, Apply the VSEPR (valence-shell electron pair repulsion) Theory to explain hybrid orbitals, Identify Intermolecular Attractive Forces (IMAF) (revisited in chapter 14) / 5.7.A.7
Chemical Reactions and Equations
Chapter 9 / Writing unbalanced formula equations when given a word equation, Writing a balanced equation when given and unbalanced formula equation, Writing a balanced equation when given a word equation, Correctly use all four state symbols, Classifying equations as synthesis, decomposition, single replacement, double displacement, and combustion reactions, Classifying reactions as acid/base, redox (oxidation-reduction), precipitation / 5.7.B
The Mole, introduction to Stoichiometry
Chapter 10 / Define a mole in terms of Avogadro’s number, Define a mole in terms of molar mass, Convert between number of moles, mass, and number of particles, Describe molar volume of a gas (that one mole of any ideal gas occupies 22.4 L at Standard temperature and pressure - STP), Use molar volume of a gas at STP to convert between number of particles, mass, and number of moles, Calculate percent composition from a chemical formula, Use percent composition to determine empirical formula, Differentiate molecular and empirical formulas, Find the empirical formula associated with a molecular formula, Find a molecular formula given a molar mass and an empirical formula / 5.7.A
Stoichiometry and Limiting Reactants
Chapter 11 / Define stoichiometry, Use stoichiometry to make conversions using balanced chemical equations: moles A ® moles B, mass A ® moles B, moles A ® mass, mass A ® mass B,
Define the concept of a limiting reactant in terms of chemical reactions and everyday applications, Make any of the above conversions using limiting reactants, Hypothetical situations: calculate how much of the excess reactant was left over, how much more of a product could have been produced, how much more limiting reactant would need to be added, etc. / 5.7.B
Thermochemistry, Thermodynamics and Kinetics
Chapters 12, 22, and 23 / Distinguish exothermic and endothermic reactions, Define enthalpy, change in enthalpy and how they are used in equations, Define standard conditions for standard enthalpy change and its notation, State Hess’s law, Use Hess’s law to find DHo for a reaction, Describe the process of calorimetry, Define rate of reaction, Identify intermediate products of a reaction, Describe a rate law for a chemical reaction, Describe collision theory and relate how it describes the reaction rate, Describe the factors that affect reaction rate in terms of collision theory, Explain the concept of activation energy and activated complex, Define entropy, Describe an increase in the entropy of the universe as a driving force (2nd law of thermodynamics), Create and recognize an energy diagram for an exothermic or endothermic reaction, including EA, DHo, enthalpy of products and enthalpy of reactants, Use the Gibbs free energy equation (DG = DH - TDS) to calculate DG. Decide whether a reaction is spontaneous if only the sign of DHo and DS are given / 5.7.B.1
5.7.B.2
Gases
Chapter 13 / Describe the kinetic molecular theory (KMT) and use the KMT to describe the behavior of gases, Describe changes in pressure, temperature and volume on a molecular level in terms of the KMT, Define gas pressure and describe its measurement, State and use the gas laws to predict properties of ideal gases both quantitatively and qualitatively:
PV = nRT, PV = k, V/T = k, V/n = k. PTOT = Pa + Pb …
Compare ideal and real gas behavior and predict how changing temperature, pressure, and volume can cause a gas to deviate from ideal behavior, Calculate gas density, Use molar volume of a gas to calculate quantities of mass or particles (Review from Ch 10) / 5.7.A
Liquids and Solids
Chapter 14 / Use the kinetic molecular theory (KMT) to describe the behavior of solids, liquids, and gases on a molecular level, Describe three different intermolecular forces (IMF): hydrogen bonds, dipole-dipole interactions, and London dispersion forces, Recognize that intermolecular forces only affect molecular substances, and recognize IMF as one of four types of categories of bonding, which also includes covalent network interactions, metallic bonding, and ionic bonding, Describe the six changes of state (melting, freezing, boiling, condensing, sublimation, deposition), Describe the features of a heating curve, Distinguish heat of fusion and heat of vaporization and use each in calculations, Identify the features of a phase diagram, Use a phase diagram to predict how a change in pressure or temperature will change a given substance / 5.7.A
Solutions
Chapter 15 / Describe properties and different types of solutions, Measure concentration in terms of molarity, molality, mole fraction, and g/mL, Differentiate saturated, supersaturated, unsaturated and be able to predict the state of a solution given a solubility curve, Explain how solutions form and the motion of particles in solution, Define solubility and factors that affect it, Identify factors that affect rate of dissolution, Define colligative property and describe osmotic pressure, boiling point elevation, melting point depression and vapor pressure reduction / 5.7.A
Chemical Equilibrium
Chapter 16 / Explain the concept of reversibility in chemical reactions, Determine K (the equilibrium constant) for a given reaction using the law of mass action, Use the reaction quotient (Q) to determine if a system is at equilibrium, and if not how a system will shift to attain equilibrium, Define and explain Le Chatelier’s principle, Describe how changes in concentration, pressure, and temperature affect a reaction at equilibrium / 5.7.B
Solubility and Precipitation
Chapter 17 / Compare dissolution and precipitation, Apply a list of given solubility rules to write complete and net ionic equations from a given balanced molecular equation, Define solubility product (Ksp) and write the equation relating solubility product to concentration, Evaluate whether or not a precipitate will form using Ksp, Describe how a common ion can shift the solubility equilibrium / 5.7.B
Acids, Bases, and Salts
Chapters18 and 19 / State Arrhenius, Bronsted-Lowry, and Lewis definitions of Acids and Bases, Identify properties of acids and bases, Differentiate strong and weak acids and distinguish acid strength from acid concentration, Identify conjugate acids and conjugate bases, Calculate KA for a given acid and Kb for a given base, Use Kw to relate Ka and Kb, Relate pH to [H+], Describe how titration is used to determine the concentration of an unknown acid or base / 5.7.A
5.7.B
Oxidation and Reduction
Chapter 20 / Define oxidation and reduction, Identify oxidizing agents and reducing agents, Assign oxidation numbers to elements in compounds or ions, Using a given activity series, classify metals in order of reactivity, Describe different types of redox reactions such as corrosion, bleaching, combustion etc., Identify the oxidizing/reducing agents in a chemical equation / 5.7.B
Organic Chemistry
Chapters 25 and 26 / Explain carbon’s unique bonding properties, define organic compounds and organic chemistry, explain how carbon and hydrogen atoms can form numerous hydrocarbon compounds, define isomers, define polymers, differentiate different classes of organic compounds, provide examples of selected classes of organic compounds including their formulas. / 5.7.A
5.7.B
September 2, 2003
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