the differences between that Students will be able to describe the states of matter.

Transcription

1 Advanced Chemistry Essential Questions: 1. What is the best design, process to conduct, means to evaluate and form of communication for scientific investigations? 2. How can one use scientific knowledge of properties, forms, changes and interactions to describe physical and chemical systems? 3. How are chemical combinations and interactions defined by mathematical proportions? 4. How can energy exchanges, molecular kinetics and manipulation of conditions at equilibrium describe the behavior of matter? I. Structure and Properties Anchor Standard 1.1: matter and energy from an atomic perspective. the differences between energy forms such as the classes of matter are describe the states of matter. potential, kinetic, law of conservation of energy, different and how they differ at the particle level. describe the scientific work, energy and heat. results should be method. expressed by measuring use dimensional analysis to convert basic units of measurement. and expressing data with precision and accuracy. distinguish between physical processes and chemical reactions and between physical and chemical properties. the classifications of matter including mixtures, pure substances, immiscible, distillation, filtration and chromatography. Vocabulary: intensive property extensive properties states of matter atomic theory law scientific method theory dimensional analysis precision accuracy temperature scales Board Adopted March 27, distinguish between the classes of matter and how they differ at the particle level. distinguish between potential and kinetic energy. distinguish between exact and uncertain values and express uncertain values with the appropriate number of significant figures. accurately convert nonstandard SI values from one set of units to another.

2 Anchor Standard 1.2: atoms, ions and molecules as the building blocks of matter. the contributions of write symbols to describe differentiate among models of atoms, molecules, elements, Dalton, Thomson, the discovery of radioactivity, Rutherford, Millikan and Bohr. mass, number of particles and number of moles can be interconverted. the three types of subatomic particles of atoms and the monoatomic ions they compounds, and mixtures. patterns of the periodic form. predict the number of protons, neutrons, electrons and mass table. Vocabulary: use the period table to explain and predict the properties of elements. numbers for monatomic nuclides use natural abundance elements, isotopes and Avogadro and isotopic masses to ions. moles calculate average atomic write balanced equations molar mass mass values. to describe reactions. use chemical formulas and average atomic masses to calculate molecular masses and molar masses. Board Adopted March 27,

3 Anchor Standard 1.3: Students will explain the properties of elements using atomic structure. wave properties of light. sizes and shape of trends of radius, ionic identify the properties of orbitals. radius, ionization energy, elements. the rules for writing affinity and predict relative sizes of electron configurations electronegativity are atoms & ions. (Hund, Aufau, and Pauli) related to atomic determine the valence trends of radius, ionic structure. number of electrons based radius, ionization energy, on position of an element in the periodic table. affinity and electronegativity. draw orbital diagrams. write electron configurations. relate electron configurations to periodicity. Vocabulary: Atomic spectra Quantum theory (photoelectric effect) quantum numbers Hydrogen spectra and Bohr model de Broglie wave Heisenberg uncertainty principle the concept of effective nuclear charge can be used to explain differences in the energies of atomic orbitals and to predict the relative sizes of atoms and monatomic ions. the ionization energies and electron affinities of the elements is related to their positions in the periodic table. interconvert the energies, wavelengths, and frequencies of electromagnetic radiation. explain the photoelectric effect using quantum theory. relate the energies and wavelengths of photons absorbed and emitted by atoms to electron transitions between atomic energy levels. apply the Heisenberg uncertainty principle to particles in motion and calculate their de Broglie wavelengths. assign quantum numbers to orbitals and use their values to describe the sizes, energies, and orientations of orbitals. use the Aufbau principle and Hund s rule to write electron configurations and draw orbital diagrams of atoms and monatomic ions. Board Adopted March 27,

4 II. Bonding & Forces Anchor Standard 2.1: Students will distinguish between chemical bonding types. ionic, covalent and metallic bonds the relative strengths of distinguish between ionic characteristics. ion ion interactions can and covalent bonding. naming and writing be calculated. draw Lewis dot diagrams to represent elements and compounds based on valence electrons. formulas (binary ionic, transition & main group, polyatomic, binary molecular, binary acids and oxoacids). bond order, bond energy, and bond length are related. the octet rules exceptions. length and strength of bonds. Vocabulary: electronegativity polarity resonance structures formal charge free radical describe ways in which covalent, ionic, and metallic bonds are alike and ways in which they differ. name molecular and ionic compounds and write their formulas. draw complex Lewis structures of ionic and molecular compounds and polyatomic ions. predict the polarity of covalent bonds based on differences in the electronegativities of the bonded elements. draw resonance structures and use formal charges to evaluate their relative importance. Board Adopted March 27,

5 Anchor Standard 2.2: Students will use bond theory to explain molecular geometry. VESPR theory with our without lone pairs molecular geometry is predict the shape and polarity of molecules based on VSEPR (Valence geometries of molecules with multiple central atoms determined by valance bond theory, and hybrid and expanded orbitals. Shell Electron Pair chirality and molecular Repulsion) theory. recognition use VSEPR theory to describe intermolecular forces. molecular orbital theory Vocabulary: polar bonding steric number bond order electron group geometries (linear, triagnol planer, tetrahedral, trigonal bipyramidal, octahedral) molecular geometries (angular or bent, triagonal pyramidal, seesaw, T- shaped, squarepyramidal, square planer) dipole moment valence bond theory hybrid orbitals sigma bond pi bond chirality molecular orbital theory (MO theory) bonding and antibonding theory Cont. valence bond theory can be used to explain bond angles and molecular shape. atomic orbital hybridization can be used to visualize molecular shape. use VSEPR and the concept of steric number to predict the bond angles in molecules and the shapes of molecules with one central atom. predict whether a substance is polar or nonpolar based on its molecular structure. recognize chiral molecules. draw molecular orbital diagrams of small molecules. use MO theory to predict bond order. explain magnetic properties and spectra. Board Adopted March 27,

6 diamagnetic paramagnetic Anchor Standard 2.3: intermolecular forces and the attraction between particles. the information provided in a phase diagram. identify solids, liquids and gases properties based on kinetic theory. interpret a phase diagram. distinguish between the different phases of matter. properties of water result from hydrogen bonding including surface tension, capillary action and density. Vocabulary: London ion dipole dipole-dipole hydrogen bonding solubility viscosity functional groups hydrophilic hydrophobic supercritical fluid triple point critical point trends in boiling point, viscosity, and other physical properties of molecular compounds are based on the nature and the strengths of interactions between their molecules. ionic compounds and polar molecular compounds dissolve in polar solvents and nonpolar molecular compounds dissolve in nonpolar solvents. the unusual properties of water and how they related to the hydrogen bonds formed by water molecules. identify the solute(s) and solvent in a solution. identify the regions of a phase diagram and explain the effect of temperature and pressure on phase changes. Board Adopted March 27,

7 III. Chemical Reactions Anchor Standard 3.1: mass relationships and chemical reactions through stoichiometry. how to balance complex chemical equations. a balanced chemical identify the 5 types of equation can be used to chemical reactions. Vocabulary: relate the masses of balance chemical equations. conservation of mass % Composition reactants and products. predict products of a chemical reaction. empirical formula molecular formula determine if a product limiting reactants will form based on % yield solubility. strong electrolytes write molecular, ionic and weak electrolytes net ionic equations. nonelectrolytes determine the formula of net ionic equation a compound given chemical name. spectator ions determine the chemical name from a chemical formula. identify number of moles of each element from its formula. assign oxidation numbers to elements in a compound. use the chemical formula for a compound to calculate formula mass, molar mass, and percentage composition. write complex balanced chemical equations to describe chemical reactions. interconvert the chemical formula and percent composition of a substance. determine the molecular formula of a substance from its percent composition and molar mass. use analysis data to determine the empirical formula of a substance. determine the limiting reactant in a reaction mixture. calculate the theoretical and percent yields in a chemical reaction. Board Adopted March 27,

8 Anchor Standard 3.2: the chemistry of aqueous solutions in chemical reactions. acid, base and neutral express the concentrations reactions oxidation numbers can be of solutions in different convert between units of precipitant reactions used to identify redox units, including molarity. moles, grams, particles redox reactions reactions, oxidizing calculate the mass of a and liters of a substance. agents and reducing solute or the volume of a calculate molarity. Vocabulary: agents. solution required to make molarity precipitations can be a solution of specified molality predicted using solubility volume and concentration. rules. dilutions distinguish between strong electrolytes, weak titration electrolytes, and analytes nonelectrolytes. ion exchange write complex molecular, oxidation numbers total ionic, and net ionic saturated solution equations for reactions in supersaturated solution solution. calculate the concentration of a solute of the quantity of a precipitate from stoichiometry data. use changes in oxidation numbers to write balanced equations describing redox reactions. determine the concentration of a solute from titration data. Board Adopted March 27,

9 Anchor Standard 3.3: energy changes in chemical reactions through thermochemistry. energy can exist as a reactant or product. the internal energies identify enthalpy changes as exothermic or enthalpy changes changes of thermodynamic systems can be related to endothermic. Vocabulary: heat flows and work done. calculate enthalpies of reactions. Calorimetry Hess s Law enthalpy enthalpy of vaporization heat capcity specific heat molar heat capacity calorimeter enthalpies of reaction thermochemical equation standard conditions stand enthalpy of formation thermochemistry system surroundings first law of thermodynamics state function distinguish between endothermic and exothermic processes. calculate the heat gained or lost during changes in temperature and physical state. use calorimetry data to calculate enthalpies of reaction. calculate enthalpies of reaction using Hess s law and enthalpies of formation. Board Adopted March 27,

10 IV. Properties of States of Matter Anchor Standard 4.1: the properties of gases. Prior Background Knowledge Students will know: the gas Laws including Boyles, Charles, the root- mean- square describe the behavior of gases using the kinetic molecular theory. Avogadro, and the Combined Gas Law speed of a gas can be calculated from its mass and absolute temperature. solve gas law problems. Vocabulary: effusion standard temperature and pressure (STP) ideal gases mixture of gases Henry s Law diffusion real gases ideal gas van der Waals behaviors kinetic molecular theory Graham s law of effusion barometer manometer universal gas constant the van der Waals equation can be used to correct for nonideal behavior of gases. Board Adopted March 27, use kinetic molecular theory to explain the properties of gases. relate Graham s law to the relative rates of effusion of gases. calculate changes in the volume, temperature, pressure, and number of moles of an ideal gas using gas laws including the ideal gas law. use the ideal gas law to calculate the density and molar mass of an ideal gas. use balanced chemical equations to relate the volumes of gas- phase reactants and products using the stoichiometry of reaction and the ideal gas law. relate the mole fraction, partial pressure, and quantity of a gas in a mixture. relate solubility of a gas to Henry s law. use the van der Waals equation to correct for nonideal behavior of gases.

11 Anchor Standard 4.2: concentration and colligative properties of solutions. the effects of concentrations based on the Born- Haber cycle can predict changes in freezing and boiling point of a substance upon molality. Vocabulary: be used to calculate enthalpy. changes as substances dissolve addition of a solute. Colligative properties molality boiling point freezing point osmotic pressure vapor pressure Born-Haber cycle enthalpy of solution vapor pressure volatile Clausius-Clapeyron equation Raoult s law can t Hoff factor (i) osmotic pressure reverse osmosis the Clausius-Clapeyron equation is useful for calculating vapor pressure. Raoult s law can be used to calculate vapor pressures of solutions. express concentrations in molality. calculate the freezing points and boiling points of solutions. predict the direction of solvent flow in osmosis. use colligative properties to determine molar masses. Board Adopted March 27,

12 V. Chemical Kinetics and Equilibrium Anchor Standard 5.1: the driving force of thermodynamics. Prior Background Knowledge Students will know: Vocabulary: thermodynamics is the thermodynamics why reactions occur. entropy spontaneous reactions nonspontaneous reactions second law of thermodynamics microstates third law of thermodynamics standard molar entropies reversible process Gibbs free energy stand free energy of formation predict the signs of entropy changes for chemical reactions and physical processes. predict the relative entropies of substances based on their molecular structures. calculate entropy changes in chemical reactions using standard molar entropies. calculate free-energy changes in chemical reactions from the changes in enthalpy and entropy for the reactions. calculate standard freeenergy changes in chemical reactions using the appropriate standard free energy of formation values. predict the spontaneity of a chemical reaction as a function of temperature. calculate the net change in free energy of coupled spontaneous reactions. Board Adopted March 27,

13 Anchor Standard 5.2: chemical kinetics. the effect of concentration. rate laws can assess the recognize the effect that the effect of temperature. validity of a reaction different factors have on the effect of catalysts. mechanism. molecular collisions. identify change in Vocabulary: enthalpy and activation reaction rates energy from a potential rate orders energy diagram. rate law reaction order rate constant overall reaction order activation energy transition state activated complex Arrhenius equation reaction mechanism elementary steps rate-determining steps catalysts use the stoichiometry of a reaction to relate the rates at which the concentrations of its reactants and products change as the reaction proceeds. determine the rate law and overall order for a chemical reaction using initial rate data. use integrated rate laws to identify the orders of reactions and determine their rate constants. explain the effect of temperature on the rates of reactions. identify catalysts and describe their impact on reaction rates and mechanisms. Board Adopted March 27,

14 Anchor Standard 5.3: chemical equilibrium. relationships between Kc and Kp. nature has a dynamic predict the result of chemical equilibria. increasing or decreasing Vocabulary: the value of a reaction concentration, chemical equilibrium quotient can be used to temperature, surface area equilibrium constant predict the direction of a or presence of a catalyst. reaction quotient reversible chemical anticipate the change in a heterogenous equilibria reaction. chemical system Le Chatelier s principle equilibrium predictions predicted by LeChatelier s can be made based on principle. changing concentration of reactants/products, pressure, volume, temperature or addition a catalyst. use equilibrium concentration or partial pressure data to calculate the value of Kc or Kp. interconvert Kc and Kp values of gas- phase reactions. calculate K values of related reactions. predict how a reaction at equilibrium responds to changes in reaction conditions. calculate the concentrations or partial pressures of reactants and products in a reaction mixture at equilibrium from their starting values and the value of K. relate the standard freeenergy change of a reversible reaction to its equilibrium constant. predict the value of K at any temperature from thermodynamic data. Board Adopted March 27,

15 Anchor Standard 5.4: aqueous equilibria. Vocabulary: explain and use the ph scale. calculate ph and poh given the concentration of hydronium or hydroxide ion. calculate the molarity of a solution from titration data. Acids & bases including Lewis, Bronsted-Lowry, and Arrhenius conjugate base conjugate acid ph degree of ionization polyprotic acids ph buffer ph indicator solubility Ksp Ka & Kb Mono, di and polyprotic acids ph of salts titrations dilutions salt the strengths of acids and bases is related to their Ka, Kb, pka, and pkb values and to their percent ionization or dissociation in water. identify the Bronsted Lowry acids and bases and their conjugate bases and acids in chemical reactions. interconvert [H+], [OH ], ph, and poh values. calculate the ph values of solutions of weak acids and bases and the salts of their conjugate bases and acids. predict whether a salt is acidic, basic, or neutral. explain how ph buffers control ph, and calculate the ph of a conjugate acid base pair. interpret the results of an acid base titration. relate the solubility of an ionic compound to its solubility product and solution ph. Board Adopted March 27,

16 Anchor Standard 5.5: the interconversion of chemical to electrical energy in electrochemistry. Prior Background Knowledge Students will know: combine the appropriate Vocabulary: cell potentials can be half- reactions to write net describe the components electrochemistry calculated from standard ionic equations describing of an electrochemical cell. redox reduction potentials. redox reactions. identify the direction of electrochemical cells Nernst s equation can be draw cell diagrams and the movement of anode used to calculate describe the components of electrons resulting in cathode nonstandard cell electrochemical cells and voltage. potentials. cell diagram their roles in masses of reactants can be interconverting chemical standard reduction interconverted with and electrical energy. potential quantities of electrical standard cell potential charge. electromotive force (emf) voltaic cell cell potential Faraday constant Nernst equation fuel cell batteries Board Adopted March 27,

17 VI. Application and Organic Extensions Anchor Standard 6.1: Time Permitting: Students will consider the particulate view to common life applications. Prior Background Knowledge Students will know: explain the conductivity of Vocabulary: density of a solid is metals and N/A semiconductors related to the masses of semiconductors. metallic structures the particles. distinguish between alloys substitutional and crystalline nonmetals interstitial alloys. ceramics -ray diffraction Anchor Standard 6.2: Time Permitting: a basic overview of organic chemistry. Prior Background Knowledge Students will know: distinguish between the Vocabulary: organic compounds can molecular structures and N/A carbon s properties be named and drawn. properties of the different alkanes, alkenes, and alkynes organic compounds have constitutional and classes of hydrocarbons. explain the differences aromatic compounds stereoisomers. between alcohols, ethers, (cyclic) the properties of amines, ketones, and amines, alcohols, ethers, aldehydes, ketones, carboxylic acids, esters an amides polymers if related to their molecular structures. aldehydes. explain the difference between carboxylic acids, esters, and amides. Board Adopted March 27,

18 Anchor Standard 6.3: Time Permitting: simple biochemical compounds of life. describe the molecular Vocabulary: the four levels of protein structures and chemical N/A proteins structures are stabilized properties of amino acids carbohydrates by intermolecular forces and the nature of the lipids and covalent bonds. bonds that link them nucleic acids together in peptides and proteins. describe the molecular structures of simple sugars and polysaccharides and how the compounds are used as energy sources and for energy storage. describe the molecular structure and the physical and chemical properties of saturated and unsaturated glycerides. describe the structures of DNA and RNA and how they function together to translate gen tic information. Board Adopted March 27,

19 Anchor Standard 6.4: Time Permitting: Students will expand their understanding of nuclear chemistry established in prior benchmarks. Prior Background Knowledge Students will know: N/A Vocabulary: fission fusion decay medicinal, radiometric dating, dosage and risk the energy released in a nuclear reaction can be calculated from the masses of the products and reactants. calculate the quantity of a radionuclide remaining after a defined decay time. compare and contrast nuclear fission and nuclear fusion. describe the dangers of exposure to nuclear radiation. describe the process of determining the age of a sample by radiometric dating. Board Adopted March 27,