generate testable Students will be able to investigations. Biology 1 2 (can be conclusions. reveal relationships identify sources of error higher.

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1 Honors Chemistry Essential Questions: 1. How can one explain the structure, properties, and interactions of matter? Communication of Scientific Information Anchor Standard 1: Students will be able to design, conduct, evaluate and communicate scientific investigations via a formal lab report. Students will be able to formulate questions, develop a hypothesis, and conduct scientific investigations. scientific method is an that generate testable organized approach to scientific thought is questions. successfully complete the scientific inquiry. substantiated by valid, safely design and freshman science course. curiosity about an reproducible evidence conduct controlled successfully complete observation provides the that leads to logical investigations. Biology 1 2 (can be catalyst to the conclusions. analyze data. concurrently enrolled.) development of a testable analysis of data helps formulate a conclusion. Algebra I with a C or hypothesis. reveal relationships identify sources of error higher. between and among and the effects of those basic understanding of variables. errors on the results. the scientific process of dependent/independent the scientific process. variables. scientific process. hypothesis, model and theory. Board Adopted March 27,

2 Students will be able use statistical, mathematical and graphical methods to analyze data basic units of that measurement. graphical relationships construct a scatter plot graph. rounding rules for significant digits. often lead to mathematical formulas proper format for that can be used to scientific notation. predict properties or behaviors. the tool determines the SI unit (metric system) degree of precision. scientific notation accuracy is dependent significant figures upon skill level. conversion factor dimensional analysis derived unit percent error percent yield precision accuracy utilize % error and/or % yield. use dimensional analysis to convert units of measurement. identify and graph dependent and independent variables. determine a line of best fit. demonstrate the proper use of significant figures and scientific notation. Board Adopted March 27,

3 Students will utilize basic laboratory techniques associated with chemical analysis. Prior Background Knowledge Required have a responsible and safe behavior is crucial in a chemistry classroom. Students will know: names and proper uses of common laboratory equipment. safety data sheet (SDS) guidelines. electronic balance Bunsen burner centrifuge filtration titration decanting that there are proper tools and technology available to collect and analyze data. select and properly use appropriate tools and technology to gather and analyze data. demonstrate basic laboratory techniques. filtering, titrating, and decanting. using an electronic balance. lighting a Bunsen burner. Board Adopted March 27,

4 Matter & Its Interactions Anchor Standard 2: Students will demonstrate knowledge of properties, forms, changes and interactions of physical and chemical systems. Students will explain how atomic structure determines physical and chemical properties of matter and the chemical reactivity of substances. Prior Background Knowledge identify the sub atomic particles. matter consists of building blocks called atoms. Students will know: the properties of matter. distinguishing characteristics of elements, compounds and mixtures. the structure of an atom includes protons and neutrons located in a dense nucleus surrounded by a cloud of electrons. element compound mixture physical & chemical properties physical & chemical change states of matter atomic number mass number ion (cation anion) isotopes that elements can be classified based on their properties. chemical properties are different from physical properties. the atomic number of an element is equal to the number of protons of an atom of that element. the mass number is equal to the total number of protons and neutrons that make up the nucleus of an atom. the average atomic mass is the weighted average of the atomic masses of the naturally occurring isotopes of the element. classify matter as elements, compounds, and mixtures. predict number of protons, neutrons, and electrons from monatomic elements, isotopes and ions. Board Adopted March 27,

5 Students will describe periodicity and how the periodic table can be used to make predictions about behavior periodic patterns exit within the periodic table. that identify the properties of elements based on their know the periodic table is an organized the number of valence electrons determines the location in the periodic table. arrangement of chemical elements. chemistry of the element. predict trends in chemical properties and Vocabulary group vs family metal vs nonmetal malleability ductility metalloid alkali metals alkaline-earth metals transition metals main-group elements halogens noble gas atomic radius valence electrons electronegativity ionization energy the periodic table displays the elements in increasing atomic number resulting in periodicity of the physical and chemical properties. chemical reactivity. predict relative sizes of atoms vs ions. Board Adopted March 27,

6 Students will discuss the contributions that altered the modern model of the atom. the contributions of that Dalton, Thomson, the the atomic theory evolves know atoms have a discovery of as new evidence surfaces. nucleus of protons and neutrons surrounded by orbiting electrons. radioactivity, Rutherford, Bohr. electrons exhibit a dual wave-particle nature. Vocabulary Law of Definite and multiple proportions orbital electron configurations noble-gas configuration quantum numbers Aufbau principle Pauli exclusion principle Hund s rule Heisenberg uncertainty principle trace the development of the emerging models of the atom. write electron configurations. relate periodic trends to electron configurations. Board Adopted March 27,

7 Students will identify different types of chemical bonding and intermolecular forces based on electrostatic forces between particles. the difference between ionic and covalently that distinguish between ionic, covalent bonding know compounds are combinations of elements. bonded compounds. the strengths of intermolecular attractions. (hydrogen bonding, dipole-dipole and London dispersion) covalent, ionic, and metallic bonding polarity dipole sea of electrons Lewis dot/electron-dot diagrams octet rule resonance polyatomic ion formula unit VSEPR (valence shell electron pair repulsion) model hybrid orbitals ionic and covalent bonds are the result of differences in electronegativity. metallic bonding is due to a sea of valence electrons. molecular shapes are the result of maximum separation between electron pairs. and their properties. explain that the sea of electrons gives metals conductivity, malleability, ductility, and luster. draw Lewis dot diagrams to represent elements and compounds. predict the shape and polarity of molecules based on VSPER theory. describe intermolecular attractions. Board Adopted March 27,

8 Students will write chemical formulas and name chemical compounds. rules for naming ionic that identify chemical and covalent compounds. there is a systematic bonding types. rules for naming acids. method for naming rules for assigning compounds. oxidation numbers. subscripts indicate the number of atoms or ions in a formula. binary compound ternary compound oxidation number name and write chemical formulas for ionic and covalent compounds. name and write formulas for acids. assign oxidation numbers to elements in a compound. Board Adopted March 27,

9 Chemical Equations Anchor Standard 3: Students will write chemical combinations and interactions as chemical equations. Students will represent simple chemical changes utilizing words and symbolic equations. equations represent that chemical reactions. matter is conserved in a identify chemical the activity series and chemical reaction. nomenclature. solubility rules. the identity of atoms does not change in a chemical reaction. products and reactants the activity series is used synthesis, decomposition, single & double replacement, and combustion reactions to predict the products of single replacement reactions. solubility tables predict aqueous the formation of precipitate precipitates in double ionic equations replacement reactions. net ionic equations spontaneous redox reactions can be used to spectator ions produce electricity. redox (oxidation reduction) reactions electrochemical cells anode/cathode fission vs fusion reactions alpha, beta and gamma decay a nuclear reaction involves changes within the nucleus which changes the identity of the element. identify the types of reactions. balance chemical equations. predict products formed using the activity series and solubility tables. identify the components of electrochemical cells. balance nuclear equations. Board Adopted March 27,

10 Quantitative Relationships in Chemical Reactions Anchor Standard 4: Students will represent chemical combinations and interactions with definite mathematical proportions. Students will utilize mole ratios to identify, calculate and analyze relationships in a chemical reaction. that. calculate the molar mass of a compound. balance chemical equations. that the number of chemical particles in a given mass can determined knowing that 1 mole equals x10 23 particles. a mole is a unit representing x particles and is the basis for all mathematical calculations in chemistry. convert among units of grams, moles, and particles. Avogadro s number molar mass Students will use mathematical proportions expressed as empirical and molecular formulas. difference between that empirical and molecular percent composition is mole conversions. formulas. used to determine the empirical formula of a compound. percent composition an empirical formula empirical formula shows the simplest molecular formula whole-number ratio of atoms in a given compound. the molecular formula is a whole number multiple of the empirical formula. calculate percent composition. determine empirical and molecular formulas from experimental data. Board Adopted March 27,

11 Students will use stoichiometric relationships to support the claim that atoms and mass are conserved during chemical reactions Prior Background Knowledge Students will know: that mole conversions. balance chemical equations. that quantitative relationships exist between reactants and products in a chemical reaction. stoichiometry limiting reactants mass-mass mass-volume volume-volume percent yield stoichiometry calculations rely on the fixed quantitative proportions of substances in a chemical reaction. percent yield shows the relationship between the theoretical yield and actual (experimental) yield. calculate stoichiometric relationships in chemical reactions. mass mass solution stoichiometry mass volume volume volume determine limiting reactants. calculate % yield. Board Adopted March 27,

12 The States of Matter Anchor Standard 5: Students will describe the states of matter using the Kinetic Molecular Theory. Students will explain that the states of matter are determined by the Kinetic Molecular Theory. the Kinetic Molecular that Theory. the strength of attractions states of matter. between particles phase changes. determines the state of ideal vs real gases matter. surface tension capillary action boiling vapor pressure heating and cooling curve phase diagram identify solid, liquid and gas properties based on Kinetic Molecular Theory. Board Adopted March 27,

13 Students will explain the behavior of gases using the Kinetic Molecular Theory. Prior Background Knowledge Students will know: that the behavior of gasses is that related to the motions of its gas pressure is due to the uses ratio and proportions. atoms and molecules. motion of gas molecules and their collisions with explain the difference the container walls. between direct and Kelvin temperature there is a direct inverse proportions. Boyles law relationship between the isolate variables. Charles law temperatures of a gas and Gay-Lussac s kinetic energy. (Amonton s) law Kelvin temperature must combined gas law be used with gas ideal gas law properties. Dalton s law of partial pressure Graham s law diffusion effusion describe the behavior of gases using the kinetic molecular theory. solve gas law problems. Board Adopted March 27,

14 Students will predict changes to solutions based on their colligative properties. that there are a variety of that ways to express the solutes raise the boiling calculate the moles of a solute. concentrations of solutions. point and lower the freezing point of a solvent. colligative properties of solvent solutions depend only on solute the total number of solute solution particles present. molarity colligative properties freezing point depression boiling point elevation osmotic pressure vapor pressure lowering calculate solution concentrations. molarity molality percent (m/v, v/v) ppm, ppb etc predict qualitative changes in freezing and boiling point of a solvent upon addition of a solute. calculate change in fp and bp of a solvent upon addition of a solute. Board Adopted March 27,

15 Acids & Bases Anchor Standard 6: Students will observe and describe acids and bases in a chemical system. Students will list the general properties of aqueous acids, bases and salts and demonstrate effective titration techniques. properties of acids and that describe solutions as bases. a concentration of an acidic, basic or neutral calculate the molarity of a unknown solution can be based on their properties. solution. determined by titrating identify conjugate acid stoichiometry Arrhenius with a solution of known base pairs. calculations. Bronsted-Lowry concentration. calculate the molarity of a Lewis ph and poh are related solution from titration conjugate acid-base pairs to the concentration of data. hydronium or hydroxide titration calculate ph and poh ions. acid base indicator given the concentration endpoint of hydronium or hydroxide ions. equivalence point standard solution ph poh Board Adopted March 27,

16 Reaction Rates and Chemical Equilibrium Anchor Standard 7: Students will use collision theory to describe reaction rates and the state of equilibrium. Students will identify the factors in a chemical system that affect the frequency of molecular collisions, reaction rates and the state of equilibrium. equilibrium. that write balanced chemical equations. calculate molarity. collision theory activation energy catalyst rate determining step reaction mechanisms LeChetelier s principle Equilibrium constants: Kw, Keq, Ksp, Ka, Kb chemical reactions rates depend on factors that influence the frequency of collision of reactant molecules. many reactions are reversible and reach a state of dynamic equilibrium, where the forward and reverse reactions rates are equal. adjust the rate of a chemical reactions by changing concentration, temperature, surface area or adding a catalyst. identify exothermic and endothermic reactions. perform equilibrium calculations involving Kw, Keq, Ksp, Ka, Kb. Board Adopted March 27,

17 Reaction Energy Anchor Standard 8: Students will explore the energy changes within chemical and physical processes. Student will state that the change of energy in a chemical reaction is the net result of breaking bonds and forming new bonds. thermochemistry is the that determine whether a study of the changes in energy is stored in reaction is endothermic differentiate between energy that accompany chemical bonds. or exothermic. physical and chemical changes. chemical and physical changes. energy involved in a chemical reaction is the investigate and calculate the energy relationships identify phase changes. net result of breaking in physical and chemical balance chemical bonds and forming new changes. equations. thermochemistry bonds. specific heat calorimeter molar heat of fusion heat & temperature molar heat of endothermic/exothermic vaporization heats of fusion and enthalpy and Hess s vaporization law thermodynamic specific heat relationships Hess s law enthalpy entropy Board Adopted March 27,