Course: CP Chemistry Year: Teacher: L. Page. Unit 2: Matter and Energy Approximate Time Frame: # of Weeks 4

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1 Course: CP Chemistry Year: Teacher: L. Page Unit 1: Matter and Change Approximate Time Frame: # of Weeks 4 Biological, chemical and physical properties of matter result from the ability of atoms to form bonds from electrostatic forces between electrons and protons and between atoms and molecules. What is matter and how can it be classified and identified? What do all bits of the same substance have in common? Classification of matter as pure substance, or mixture with subtypes of element, compound, homogenous and heterogeneous mixtures. (CT Science Enrichment (pub for HS How do I know that something has changed from one substance to another? How do I measure & describe the amount of matter in a sample? Matter exists as particles elements and compounds. Mixtures contain elements and/or compounds. Chemical reactions result in elements rearranging themselves into new substances with different properties. The amount of matter in a sample can be described by count, mass, or volume. create a matter chart and classify a substance using a matter chart. design a sequence of steps to perform a separation of mixtures using physical means. Work on analyzing data with mathematics and making insightful conclusions based on scientific knowledge Begin to be able to identify hazards in lab. Know & be able to apply the matter chart. Know & be able to apply the states of matter. Know & be able to apply the laboratory safety equipment location and use and laboratory safety procedures Know & be able to apply the concept of density and the density formula. D = m/v Element Compound Mixture Pure substance Homogeneous mixture Heterogeneous mixture Solid Liquid Gas Plasma Mass Volume Density Unit 2: Matter and Energy Approximate Time Frame: # of Weeks 4

2 Using Physical & Be able to Mathematics Chemical distinguish and changes in exothermic and Computational matter require endothermic Thinking energy transfer. reactions and Mathematical Measurements identify the and vary in their direction of heat computational precision and transfer thinking at the accuracy. This qualitatively level needs to be builds on K 8 reflected in how Counting and and progresses we record and using significant to using report digits to round algebraic measurements answers to thinking and and all correctly reflect analysis, a calculated the precision of a range of linear values that measured or and nonlinear come from calculated value. functions those Problem solving including measurements. skills of trigonometric We can use dimensional functions, graphs and analysis and exponentials mathematical divide an and logarithms, analysis to conquer. and make deeper computational insights into a tools for set of lab data. statistical analysis to analyze, represent, and model data. Simple computational simulations are created and used based on mathematical models of basic assumptions. reflect the precision of a measurement by reading and recording the significant digits in any measured value. apply the calculation rules for significant digits to your calculations and round the results based on the significant digits rules. calculate the percent error in a measurement and to describe the level of precision and accuracy of that measurement. Know and be able to use the SI units and prefix values in a unit conversion. transcribe to scientific notation from standard format and back. Be able Know and be able to apply the rules for counting the number of significant digits in a measured value and any exceptions. Know & be able to apply the calculation rules for significant digits. Know & be able to apply rounding to any given number of significant digits in decimal or scientific notation. Know and be able to apply the percent error formula for a measurement and be able to describe the level of precision and accuracy of that measurement. Know and be able to use the SI units and prefix values in a unit conversion. transcribe to scientific notation from standard decimal format and back. use numbers in scientific notation in a calculation. use problem solving and Endothermic Exothermic System Surroundings Heat transfer Significant digits Percent error Scientific notation a. Coefficient b. Exponent Decimal notation SI prefixes a. Giga b. Mega c. Kilo d. Hecta e. Deka f. Deci g. Centi h. Milli i. Micro j. Nano k. pico Dimensional analysis

3 Use mathematical representations of phenomena to describe explanations. (NGSS Practices: HS- PS2-2,HS-PS2-4) to use numbers scientific notation in a calculation. use problem solving and dimensional analysis to solve conversion problems. dimensional analysis to solve conversion problems. Unit 3: Atomic Structure & Electrons Approximate Time Frame: # of Weeks 4 The periodic table displays the elements in increasing atomic number and relates to atomic structure. (CT Science Enrichment (pub for HS Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the 1. What is an atom? 2. What particles make up an atom? 3. Where are subatomic particles located? 4. How is the arrangement of elements on the periodic table related to the structure of the atom? identity of an element from the number of protons. give the number of protons, neutrons and electrons for any atom, isotope or ion. use Aufbau s order, Hund s Rule and Pauli Exclusion Principle to electron Know that the nucleus of the atom is much smaller than the atom yet contains most of its mass. The quantum model of the atom is based on experiments and analyses by many scientists, including Dalton, Thomson, Bohr, Rutherford and many others. describe the quantum model of the atom, and the evidence and experimental basis for the historical theorists models (for scientists, including Proton Neutron Electron Nucleus Atom Isotope Atomic mass unit Electron configuration Orbital Notation Quantum Number Principle Quantum Number Emission Spectrum Ground State Excited State

4 outermost energy level of atoms. (NGSS HS PS1 1) Develop a model based on evidence to illustrate the relationships between systems or between components of a system. Scientists construct and use models to generate knowledge and to advance understanding. There are universal methods, protocols, tools, habits of mind and technologies that should be used when conducting a scientific experiment to learn about nature. (NGSS Practices: HS- PS1-4, HS-PS1-8) configuration of any element. write the orbital filling notation for any element. Dalton, Thomson, Bohr, Rutherford) and the Modern Atomic Theory. (SC) describe the quantum model of the atom, and the evidence and experimental basis for the historical theorists models (for scientists, including Dalton, Thomson, Bohr, Rutherford) and the Modern Atomic Theory. (SC) use Aufbau s order, Hund s Rule and Pauli Exclusion Principle to electron configuration of any element. write the orbital filling notation for any element.

5 Unit 5: Periodic Table of Elements Approximate Time Frame: # of Weeks 4 The periodic table Define the mass displays the elements in increasing atomic number (A) and be able to determine it for any isotope or ion number and shows Define and be able to how periodicity of the physical and chemical explain how atomic mass is determined for an element. properties of the elements relates to atomic structure. (CT Science Enrichment (pub for HS Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms. (NGSS HS PS1 1) How does the organization of information about the elements allow us to make connections, identify trends and most importantly predict the properties both physical and chemical of unknown elements? How is the arrangement of elements on the periodic table related to the structure of the atom? The Periodic Table is a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms. Trends of Electronegativity and Atomic Radius of the Periodic Table. Properties of Families in the Periodic Table including Metals, nonmetals, semimetals (metalloids), Noble gases, Halogens and Alkali Metals. Be able to describe and apply the following concepts: The periodic table can be used to identify metals, semimetals, nonmetals and halogens. The periodic table can be used to identify trends in ionization energy, Electronegativity, the relative sizes of ions and atoms, and the number of electrons available for bonding. The electronic configuration of elements and their reactivity can be identified based on their position in the periodic table. Group Period Atomic radius Electronegativity Metals Nonmetals Metalloids Transition metals Main group elements Valence electrons Unit 6: Ionic Bonding & Nomenclature Approximate Time Frame: # of Weeks 4

6 Biological, chemical and physical properties of matter result from the ability of atoms to form bonds from electrostatic forces between electrons and protons and between atoms and molecules. (CT Science Enrichment (pub for HS Communicate scientific and technical information about why the molecular-level structure is important in the functioning of designed materials. (NGSS HS-PS2-6) Structure and Properties of Matter The structure and interactions of matter at the bulk scale are determined by How does form drive function of ionic compounds? What are the forms of ionic and metallic compound crystal lattices? How are these crystal lattice structures formed and held together? What are some of the properties related to the crystal lattice structure of these substances? Ionic compound crystals, such as NaCl, are repeating patterns of positive and negative ions. Ionic compounds are held together by the electrostatic attraction of oppositely charged ions. Ionic compound formulas are the lowest whole number ratio of cation to anion that is neutral in overall charge. Predict the chemical formula of ionic compounds using the periodic table to find the charges of monovalent metals. predict the charge of monovalent metal ions and nonmetal ions using the periodic table. write ionic compound formulas have the lowest whole number ratio of cation to anion that is neutral in overall charge. name any cation, anion and ionic compound. Know and be able to apply the following concepts: Metallic substances freely share electrons. Ions are formed when atoms transfer electrons. Ionic compounds form when ions are attracted to each other due to their opposite charges (ionic bonds). Salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction. Electronegativity and ionization energy are related to bond formation and type of bond. Structure of ionic compounds is directly related to their physical properties such as hardness, high melting and boiling points, and brittleness. Atom Compound Ion Cation Anion Molecule Element Crystal lattice Monovalent metal Multivalent metal Stock nomenclature Polyatomic ion

7 electrical forces within and between atoms. (NGSS PS1.A) Unit 7: Chemical Bonds Covalent Bonding & Nomenclature Approximate Time Frame: # of Weeks 5 Biological, chemical How does form and physical drive function of properties of covalent matter result from compounds? the ability of atoms What are the to form bonds from forms of covalent electrostatic forces compound between electrons molecules? and protons and How are these between atoms molecules formed and molecules. and held (CT Science Enrichment (pub for HS Communicate scientific and technical information about why the molecular-level structure is together? What are some of the properties related to the structure of these molecular compounds? Atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds. Covalent compound molecules, such as H 2 O, are held together by the attraction of both atoms to the shared electrons in the bond. Lewis dot structures can provide models of atoms and molecules. Draw the Lewis dot structures for a simple molecule that has up to eight valence electrons on the central atom. Predict the molecular geometry (shape) of simple molecules from the Lewis dot structures using Valence Shell Electron Pair Repulsion Theory. Determine the polarity of bonds based on electronegativity difference. Be able to describe and apply the following concepts: Atoms combine to form molecules by sharing electrons to form covalent bonds. Chemical bonds between atoms in molecules such as H 2, CH 4, NH 3, H 2 CCH 2, N 2, Cl 2, and many large biological molecules are covalent. Lewis dot structures can provide models of atoms and molecules. Molecular geometry (shape) of simple molecules can be predicted from Lewis dot structures using Valence Shell Electron Pair Repulsion Theory. Atom Compound Molecule Element Lewis Structure Valence Electron Electronegativity difference Polarity VSEPR Molecular Geometry a. Linear b. Angular c. Trigonal planar d. Tetrahedral e. Trigonal pyramidal

8 important in the functioning of designed materials. (NGSS HS-PS2-6) Structure and Properties of Matter The structure and interactions of matter at the bulk scale are determined by electrical forces within and between atoms. The shape of simple molecules and their polarity can be predicted from Lewis dot structures. Determine the type of bond based on the types of atoms in the compound. name or write formula from name for any inorganic covalent compound. name or write formula from name for any binary acid or oxoacid. Polarity of molecules is related to molecular geometry and electronegativity of bonds. Electronegativity and ionization energy are related to bond formation and type of bond. (NGSS PS1.A) Unit 8: Reactions Approximate Time Frame: # of Weeks 4 Reaction Rates Chemistry is by Chemical Know the format and Reactant count! Equations are describe symbols used in a Product Chemical reaction A balanced based on the law chemical chemical equation and Yields rates depend on chemical of Conservation reactions by be able to describe Catalyst factors that equation allows of Matter. writing balanced chemical reaction from Aqueous influence the us to convert A complete equations. the balanced complete Solid frequency of from amount of chemical chemical equation. Liquid collision of reactant one reactant to equation shows balance a Know and be able to Gas molecules. the amount of that state of all complete define and categorize Combustion any other reactants and chemical reactions as: Synthesis

9 (CT Science Enrichment (pub for HS Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties. (NGSS: HS-PS1-2) reactant or product using the mole ratio. Chemicals have to come into contact with each other to react and chemical reactions fall into a few categories. products and the reaction conditions and ratio by count (or in moles) of all reactants and products. chemical equation. write a complete chemical equation from a description. classify the type of chemical reaction based on the pattern of reactants & products. a. Combustion b. Synthesis c. Decomposition d. Single Replacement e. Double Displacement Know and be able to apply Le Chatlier s Princliple qualitatively when there are changes in concentration, temperature or pressure, the equilibrium shifts. Decomposition Single replacement Double replacement Coefficient Subscript Law of Conservations of Matter Le Chatlier s Principle Equilibrium Reversible reaction Unit 9: Stoichiometry Approximate Time Frame: 4 Weeks Conservation of Matter and Stoichiometry Be able to describe and apply the following concepts: The conservation of atoms in chemical reactions leads to the principle of conservation of Chemistry is by count! We must know how many of any chemical we have. What is the mole and why is it used in chemistry? The mole (6.02 x representative particles) is central in chemistry and allows us to convert from Know and be able to use Avogadro s number, molar mass and molar volume if a gas at STP in calculations involving the mole. Know and be able to use Avogadro s number and molar mass in Mole Avogadro s Number Molar mass Atomic mass Mole ratio Stoichiometry

10 matter and the ability to calculate the mass of products and reactants. (CT Science Enrichment (pub for HS Use mathematical representations to support the claim that atoms, and therefore mass, are conserved during a chemical reaction. (NGSS Standard HS-PS1-7). How is the periodic table related to the mole? How is a balanced equation used in Stoichiometry?. mass to number of representative particles (via moles) and volume of a gas at STP. The Periodic table gives us the mass of 1 mole of any element known as the molar mass (atomic mass in grams). A balanced chemical equation allows us to convert from amount of one reactant to the amount of any other reactant or product using the mole ratio. convert between mass, mole, volume of a gas at STP and number of particles using the correct mathematical algorithms. molar mass of any element from the periodic table and any compound given the chemical formula or name. mole ratio from any substance to any other substance from the balanced equation. use stoichiometry to theoretical yield (mass, moles or volume of a gas at STP) of any other substance in a chemical equation from the given calculations involving the mole. Know and be able to apply the process to calculate the molar mass of any element from the periodic table and any simple compound given the chemical formula or name. Chemical reactions can be described by writing balanced equations. The quantity one mole is set by defining one mole of carbon; 12 atoms to have a mass of exactly 12 grams. One mole equals 6.02.x particles (atoms or molecules). The molar mass of a molecule can be determined from its chemical formula and a table of atomic masses. The mass of a molecular substance can be converted to moles, number of particles, or volume of gas at standard temperature and pressure. Standard Temperature and Pressure (STP) Molar Volume at STP Percent Composition Actual Yield Theoretical Yield Percent Yield

11 amount of any other substance in the chemical equation. Percent Composition of any compound Percent Yield of a reaction if given actual yield. Unit 10: Enrichment Topic Solutions and Intermolecular Forces (not always covered) Approximate Time Frame: 2 Weeks Chemical Bonds What are some of Polarity and use The atoms and Intermolecular Forces the properties intermolecular the molecules in liquids Hydrogen Bonding Biological, dependent on forces in a electronegativity move in a random Dipole dipole chemical and intermolecular molecule difference and pattern relative to one interactions physical properties and determine its identity of the another because the London Dispersion of matter result intramolecular properties and atoms to intermolecular forces Forces from the ability of bonds? function. are too weak to hold Van Der Waals Forces atoms to form How does the Solutions consist type of the atoms or Polar covalent bonds & bonds from structure of a of a solute intermolecular molecules in a solid molecules electrostatic forces molecule and its between electrons polarity facilitate dissolved in a forces present in form. Nonpolar Covalent and protons and intermolecular solvent. a molecule. Molarity and percent Bonds & molecules between atoms and attractions? Concentration of by mass calculations. Ionic Bonds molecules. How does this a solution can be determine if a Intermolecular Forces Solution explain the qualitatively small molecule is and their relative Solute (CT Science properties of described as polar or not strengths and how to Solvent water and other unsaturated, based on use electronegativity Concentration Enrichment (pub important saturated and electronegativity difference to find the Saturated for HS substances? supersaturated. difference and type if intermolecular Unsaturated Concentration of VSEPR shape. force present. Supersaturated a solution can be Molarity quantitatively calculate the Percent by mass

12 Types of Interactions : Attraction and repulsion between electric charges at the atomic scale explain the structure, properties, and transformations of matter, as well as the contact forces between material objects. (NGSS - PS2.B. HS-PS2-6, secondary to HS- PS1-1,secondary to HS-PS1-3.) described using molarity and percent by mass. Molarity of a solution. Or use molarity to volume of a solution or amount of solute to add to a solution. molarity in a dilution. Percent by mass of a solution. How to polarity of bonds and molecules. Unit 11: Enrichment Topic Acids & Bases (not always covered) Approximate Time Frame: 1 Week Enrichment Topic Acids and Bases react An acid causes Be able to describe Be able to describe and Acid with each other to the amount of H + and apply the apply the following Base form water and a in a solution to following concepts: concepts: ph salt. The strength of increase. Acids, Bases, and Acids, Bases, and Salts poh an acid or base Acids taste sour & Salts Students will be able Hydronium ion depends on its react with metal. Students will be to differentiate Hydroxide ion solubility and its A base causes the able to between acids, bases, Lewis Acids & Bases ability to form ions in amount of OH in differentiate and salts. Brønsted Lowry Acids & solution a solution to between acids, Students will be able bases (dissociation). increase. bases, and salts. to determine and Monoprotic acid

13 Bases taste bitter & feel slippery. ph 0 to 6 is acidic ph 8 to 12 is basic ph 7 is neutral. Students will be able to determine and explain concentration and relative ionization of acids and relate that to strength of acids and bases. Students will be able to explain the purpose and use of an indicator. Students will be able to describe and identify neutralization reactions. Students will be able to perform acid base reactions. Students will be able to describe solutions, calculate concentrations of solutions and describe factors that affect solubility. Students will be able to calculate hydrogen ion concentrations and ph for both explain concentration and relative ionization of acids and relate that to strength of acids and bases. Students will be able to explain the purpose and use of an indicator. Students will be able to describe and identify neutralization reactions. Students will be able to perform acid base reactions. Students will be able to describe solutions, calculate concentrations of solutions and describe factors that affect solubility. Students will be able to calculate hydrogen ion concentrations and ph for both strong and weak acids. Diprotic acid Triprotic acid

14 strong and weak acids. Unit 12: Enrichment Topic Gas Laws (rarely covered) Approximate Time Frame: 2 Weeks Enrichment Topic What are the properties of gases? How do molecules of a gas interact with each other? How do ideal gases interact with each other? What calculations can be done with gases based on Avogadro s Law? Properties of an ideal gas PV=nRT Kinetic Molecular Theory Gases and Gas Laws Students will be able to describe kinetic molecular theory to explain behavior. Students will be able to use the ideal gas equation, Boyle s Law, Charles Law, Combined Gas Law and Avogadro s Law to solve problems to solve problems. Gases and Gas Laws Know and be able to explain and apply the gas laws. Know and be able to apply kinetic molecular theory to explain behavior. Know and be able to apply the ideal gas law, Boyle s Law, Charles Law, Combined Gas Law and Avogadro s Law to solve problems. Know and be able to describe an ideal gas. Ideal gas Volume Pressure Moles