WAYNESBORO AREA SCHOOL DISTRICT CURRICULUM …€¦ · · 2015-07-07WAYNESBORO AREA SCHOOL DISTRICT CURRICULUM - CHEMISTRY COURSE NAME: Chemistry ... M11.A1.2.3, M11.A.2.2.1, M11.A.2.2.2

WAYNESBORO AREA SCHOOL DISTRICT CURRICULUM - CHEMISTRY

COURSE NAME: Chemistry

UNIT: Introduction NO. OF DAYS: 6 days

KEY LEARNING(S):

UNIT ESSENTIAL QUESTIONS: How is Chemistry important in your life?

STANDARD CONCEPTS Eligible Content & Skills

# OF DAYS

ESSENTIAL QUESTIONS A = Acquisition

ET = Extended Thinking

RESOURCES/ MATERIALS

TIER 2 VOCABULARY

TIER 3 VOCABULARY

Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A1.2.3, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.2.2.1, S11.A.3.1.1, S11.A.3.2.1, S11.C.1.1.1

How is Chemistry important in your life? Why do we study Chemistry? What are areas of research in Chemistry? What steps do scientists use to solve problems?

Matter Chemistry Technology Macroscopic Microscopic Scientific Method Observation Hypothesis Experiment Manipulated Variable Responding Variable Theory Scientific Law Quantitative Qualitative Traditional Application Conservation Production Pollutant Communication Collaboration Analyze Evaluate Calculate

Organic Chemistry Inorganic Chemistry Biochemistry Analytical Chemistry Physical Chemistry Pure Chemistry Applied Chemistry


UNIT: Matter and Change (chapter 1) NO. OF DAYS: 12 days

KEY LEARNING(S): matter, mixtures, changes, law of conservation of matter

UNIT ESSENTIAL QUESTIONS: How does matter undergo physical and chemical changes?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. CHEM.A.1.2 Compare the properties of mixtures. Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A.1.2.3, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.2.2.1, S11.A.3.1.1, S11.A.3.2.1, S11.C.1.1.1

CHEM.A.1.1.1 Classify physical or chemical changes within a system in terms of matter and/or energy. CHEM.A.1.1.2 Classify observations as qualitative and/or quantitative. CHEM.A.1.2.2 Differentiate between homogeneous and heterogeneous mixtures (e.g., how such mixtures can be separated).

SAS EQ: what are the

difference between pure

substances and mixtures?

How are changes in matter

accompanied by changes in

energy?

Local EQ: How are physical

properties and physical

changes of matter related?

How can the different types of

mixtures be separated? How

do elements, compounds,

and mixtures differ? How can

you identify that a chemical

change has occurred?

Matter Mixture Pure Substance Molecule Compound Element Atom Subscript Reactants Solution Alloy Heterogeneous Homogeneous Volume Mass Filtration Physical properties Physical change Chemical properties Chemical change Reaction Vapor Chemical symbol Reversible Irreversible Classify Formula Chemical symbol

Law of Conservation of Mass Distillation Extensive Properties Intensive Properties Precipitate


UNIT: Matter and Change NO. OF DAYS: 12

KEY LEARNING(S): matter, mixtures, changes, law of conservation of matter

UNIT ESSENTIAL QUESTIONS: How does matter undergo physical and chemical changes?

CONCEPT

FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES

Exit Pass Google Form Padlet

Chemistry in a Bag Lab Matter Map Chapter 1 Assessment

Chemistry in a Bag Lab Matter Concept Map


UNIT: Scientific Measurement NO. OF DAYS: 16 days

KEY LEARNING(S): conversions, metrics, significant figures, density, SI measurement

UNIT ESSENTIAL QUESTIONS: How is measurement applied to science?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.2, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.2.2.1, S11.A.3.1.2, S11.A.3.2.1, S11.C.1.1.1

CHEM.A.1.1.3 Utilize significant figures to communicate the uncertainty

in a quantitative observation.

SAS EQ: What are the

differences between pure

substances and mixtures?

Local EQ: How are accuracy

and precision different? How

does measurement error

affect a calculation? How do

significant figure rules affect

calculations? What are basic

units of the SI system? What

are the prefixes and their

values? How is dimensional

analysis used to make unit

conversions? How is density

determined? How can

graphs, equations, and

models be used to analyze

systems?

Measurement Scientific notation Accuracy Precision Accepted Value Experimental Value Percent error SI system Weight Celsius Conversion Factor Dimensional Analysis Density Error International System of units Length Volume Mass Scale Temperature Energy Converting

Significant Figures Kelvin Absolute Zero


UNIT: Scientific Measurement NO. OF DAYS: 16

KEY LEARNING(S): conversions, metrics, significant figures, density, SI measurement

UNIT ESSENTIAL QUESTIONS: How is measurement applied to science?

CONCEPT


Exit Slips Google Forms Padlet Conversions Graphics Worksheet (with conversion factor pictures)

Sugar Content of Beverages Lab Report Chapter 2 Assessment(s)

Sugar Content of Beverages (Density) lab Conversion Quest Sig. Fig/Scientific Notation Quiz Test – concentrating on dimensional analysis


UNIT: Atomic Structure NO. OF DAYS: 12 days

KEY LEARNING(S): atomic structure: parts, number, and location, atomic models, average atomic mass

UNIT ESSENTIAL QUESTIONS: How has the model of the atom changed over time?

STANDARD CONCEPTS Eligible Content &

Skills

# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. CHEM.A.2.1 Explain how atomic theory serves as the basis for the study of matter. Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.2.2.1, S11.A.3.1.1, S11.A.3.2.1, S11.C.1.1.1, S11.C.1.1.2

CHEM.A.1.1.4 Relate the physical properties of matter to its atomic or molecular structure. CHEM.A.2.1.1 Describe the evolution of atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford, and Bohr. CHEM.A.2.1.2 Differentiate between the mass number of an isotope and the average atomic mass of an element.

SAS EQ: In what ways has the theory of

the atom changed over time due to

technological improvements? What are the

difference between pure substances and

mixtures? How are changes in matter

accompanied by changes in energy?

LOCAL EQ: What were the contributions

of Democritus and Dalton to the atomic

theory? What were the contributions of

Thompson and Rutherford to the atomic

theory? How are the three types of

subatomic particles different from one

another? How is the identity of an atom

affected by each subatomic particle? How

is atomic mass different from mass

number?

Atom Electrons Protons Neutrons Nucleus Atomic Number Mass Number Isotopes Period Group Model Indivisible Indestructible Theory Particles Average Weighted

Dalton’s Atomic Theory Cathode Ray Atomic Mass Unit Average Atomic Mass Periodic Table


UNIT: Atomic Structure NO. OF DAYS: 12

KEY LEARNING(S): atomic structure: parts, number, and location, atomic models, average atomic mass

UNIT ESSENTIAL QUESTIONS: How has the model of the atom changed over time?

CONCEPT


Exit Slips Google Forms Padlet

Atom/Ion/Isotope Model Atomic Structure Illustration – visually display location of protons, neutrons, and electrons in a diagram Chapter 3 Assessment

Element Builder Gizmo (simulation lab) Atomic Timeline Atomic Mass of Candium Lab Atom/Ion/Isotope Model


UNIT: Electrons NO. OF DAYS: 12 days

KEY LEARNING(S): Quantum numbers, electron configuration, orbital diagram, light properties

UNIT ESSENTIAL QUESTIONS: How are electrons arranged in an atom?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.A.2.1 Explain how atomic theory serves as the basis for the study of matter. CHEM.A.2.2 Describe the behavior of electrons in atoms. Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.2, M11.A.2.2.1, M11.A.3.1.1 Science S11.A.1.1.4, S11.A.1.1.5, S11.A.3.2.3, S11.C.1.1.2, S11.C.1.1.4

CHEM.A.2.1.1 Describe the evolution of atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford, and Bohr. CHEM.A.2.2.1 Predict the ground state electronic configuration and/or orbital diagram for a given atom or ion. CHEM.A.2.2.2 Predict characteristics of an atom or an ion based on its location on the periodic table(e.g., number of valence electrons, potential types of bonds, reactivity). CHEM.A.2.2.3 Explain the relationship between the electron configuration and the atomic structure of a given atom or ion (e.g., energy levels and/or orbitals with electrons, distribution of electrons in orbitals, shapes of orbitals). CHEM.A.2.2.4 Relate the existence of quantized energy levels to atomic emission spectra.

SAS EQ: How are changes in matter

accompanied by changes in energy?

How does the distribution of electrons

in atoms affect the formation of a

compound? In what ways has the

theory of the atom changed over time

due to technological improvements?

LOCAL SAS: How did the Bohr Model

and Quantum Mechanical Model

change the atomic theory? How does

the periodic table reflect quantum

numbers? How do the Aufbau

principle, Pauli exclusion principle, and

Hund’s rule determine an element’s

electron configuration? Why do we

see light?

Amplitude Electromagnetic Radiation Frequency Hertz Photons Quantum Spectrum Wavelength Orbital Shell Sublelvel Stable Inversely proportional Ground state (or level) Excited State (or level)

Atomic Emission Spectrum (spectra) Aufbau Principle Electron Configuration Energy Levels Hund’s Rule Pauli Exclusion Principle Quantum Mechanical Model


UNIT: Electrons NO. OF DAYS: 12

KEY LEARNING(S): Quantum numbers, electron configuration, orbital diagram, light properties

UNIT ESSENTIAL QUESTIONS: How are electrons arranged in an atom?

CONCEPT



Electron Configuration of atom and its common ion Poster Chapter 4 Assessment

Spectrum Activity Flame Test lab Electron Configuration Gizmo (lab Simulation) Atomic Timeline


UNIT: Periodic Table of the Elements NO. OF DAYS: 12 days

KEY LEARNING(S): predicting properties of the periodic table, periodic law

UNIT ESSENTIAL QUESTIONS: How is the periodic table organized?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.A.2.3 Explain how periodic trends in the properties of atoms allow for the prediction of physical and chemical properties. Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.2.2.1, S11.A.3.2.3, S11.A.3.3.1, S11.C.1.1.4

CHEM.A.2.3.1 Explain how the periodicity of chemical properties led to the arrangement of elements on the periodic table. CHEM.A.2.3.2 Compare and/or predict the properties (e.g., electron affinity, ionization energy, chemical reactivity, electronegativity, atomic radius) of selected elements by using their locations on the periodic table and known trends.

SAS EQ: How does the distribution of

electrons in atoms affect the formation

of a compound?

LOCAL EQ: How has the Periodic

Table been modified since its

development? Where are the different

groups on the periodic table located?

How can the periodic table be used to

predict physical and chemical properties

of elements? How are trends in atomic

size, ionic size, ionization energy, and

electronegativity reflected on the

periodic table?

Ion Metalloids Metals Nonmetals Semimetals Trend Organizing Groups Families

Alkali metal Alkaline Earth Metal Anion Cation Atomic Radius Electronegativity Halogen Inner Transition metal Ionization Energy Noble Gases Periodic Law Representative Elements Transition Metal Periodicity Nuclear Charge Shielding effect


UNIT: Periodic Table of the Elements NO. OF DAYS: 12

KEY LEARNING(S): predicting properties of the periodic table, periodic law

UNIT ESSENTIAL QUESTIONS: How is the periodic table organized?

CONCEPT



Predicting the Density Based on Group Properties Lab Ch. 5 Assessment

Graphing of trends activity 3D Trends Model Predicting the Density Lab


UNIT: Bonding NO. OF DAYS: 12 days

KEY LEARNING(S): Draw Lewis Structures, build 3-D VSPER theory models, predict polarity

UNIT ESSENTIAL QUESTIONS: How are compounds formed? Why do molecules have different shapes?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.B.1.3 Explain how atoms form chemical bonds. CHEM.B.1.4 Explain how models can be used to represent bonding. CHEM.A.1.2 Compare the properties of mixtures. R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.1.1.5, S11.A.3.2.3, S11.C.1.1.3

CHEM.B.1.3.1 Explain how atoms combine to form compounds through ionic and covalent bonding. CHEM.B.1.3.2 Classify a bond as

being polar covalent, non‐polar

covalent, or ionic. CHEM.B.1.3.3 Use illustrations to predict the polarity of a molecule. CHEM.B.1.4.1 Recognize and describe different types of models that can be used to illustrate the bonds that hold atoms together in a compound (e.g., computer models,

ball‐and‐stick models, graphical

models, solid‐sphere models,

structural formulas, skeletal formulas, Lewis dot structures). CHEM.B.1.4.2 Utilize Lewis dot structures to predict the structure and bonding in simple compounds. CHEM.A.1.2.5 Describe how chemical bonding can affect whether a substance dissolves in a given liquid.

SAS EQ: What factors determine the types of chemical bonds that form between particles? How does the distribution of electrons in atoms affect the formation of a compound? LOCAL EQ: How is the octet rule applied to all elements? How do the different types of ions form? How do you draw Lewis dot structures for elements and compounds? How are ionic compounds formed? How are metallic compounds formed? How are alloy different from the elements they are made from? How do the properties of ionic compounds differ from molecular compounds? How are molecular compounds formed? How is VSEPR theory used to determine molecular shape? How does molecular shape affect polarity?

Chemical Formula Ionic Bond Ionic Compound Metallic Bond Octet Rule Covalent Bond Hydrogen Bonds Molecular Compound Molecular Formula Molecule Van der Waal Forces Salt Brittle Ductile Malleable Dissolved Conduct Alloy Diatomic Single bond Double bond Triple bond

Electron Dot Structure Formula Unit Halide Ion Valence Electron Diatomic Molecule Dipole Polar Covalent Bond Nonpolar Covalent Bond Polar molecule Polyatomic ion Unshared pairs VSEPR Theory Shared pair Structural formula


UNIT: Bonding NO. OF DAYS: 12

KEY LEARNING(S): Draw Lewis Structures, build 3-D VSPER theory models, predict polarity

UNIT ESSENTIAL QUESTIONS: How are compounds formed? Why do molecules have different shapes?

CONCEPT



Chapter 6 Assessment VSPER Theory Model Building activity (with pretzels, marshmallows, and m&m’s) Polarity Comic Book – polar bears & penguins Visible Representation of the 3 Types of Bonds (Venn Diagram, etc.)


UNIT: Nomenclature NO. OF DAYS: 10 days

KEY LEARNING(S): naming binary and molecular compounds using the stock naming system

UNIT ESSENTIAL QUESTIONS: How are the names of compounds determined?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. CHEM.B.1.2 Apply the mole concept to the composition of matter. Reading – R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math – M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2.2 Science – S11.A.3.1.1, S11.C.1.1.4, S11.C.1.1.3

CHEM.A.1.1.5 Apply a systematic set of rules (IUPAC) for naming compounds and writing chemical formulas (e.g., binary covalent, binary ionic, ionic compounds containing polyatomic ions). CHEM.B.1.2.2 Apply the law of definite proportions to the classification of elements and compounds as pure substances.

SAS EQ: What are the difference between

pure substances and mixtures?

LOCAL EQ: How are the different types of

ions named? How do you translate between

an ionic compound’s name and formula?

When do ionic compounds need roman

numerals in their name? How do you translate

between a molecular compound’s name and

formula? What are the prefixes used in

naming molecular compounds?

How are acids and bases named differently?

How do the laws of definite and multiple

proportions describe chemical compounds?

Acid Base Monatomic ion Binary Polyatomic ion Formulas Subscripts Balance Charges Oxidation state Molecular compound Prefix Roman numeral Suffix

Law of Definite Proportions Law of Multiple Proportions Nomenclature


UNIT: Nomenclature NO. OF DAYS: 10

KEY LEARNING(S): naming binary and molecular compounds using the stock naming system

UNIT ESSENTIAL QUESTIONS: How are the names of compounds determined?

CONCEPT



Chapter 7 Assessment Compounds Scavenger Hunt – ex. Household items to give formula and name (that we have learned about in class)


UNIT: Moles NO. OF DAYS: 14 days

KEY LEARNING(S): converting moles, empirical and molecular formulas, percent composition

UNIT ESSENTIAL QUESTIONS: How is matter measured?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.B.1.1 Explain how the mole is a fundamental unit of chemistry. CHEM.B.1.2 Apply the mole concept to the composition of matter. Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.2.2.1, S11.A.3.1.3, S11.C.1.1.2

CHEM.B.1.1.1 Apply the mole concept to representative particles (e.g., counting, determining mass of atoms, ions, molecules, and/or formula units). CHEM.B.1.2.1 Determine the empirical and molecular formulas of compounds. CHEM.B.1.2.3 Relate the percent composition and mass of each element present in a compound.

SAS EQ: How do stoichiometric ratios relate reactants to products in a chemical reaction?

LOCAL EQ: Why are moles so important? How is the molar mass determined for elements and compounds? How can a mole be converted into mass, volume, and representative particles? How is percent composition calculated? How is empirical formula determined from percent composition? How is a molecular formula determined from an empirical formula?

Molecules Atoms Ions Convert (ing) Mass Atomic mass Relationship

Avogadro’s Hypothesis Avogadro’s Number Empirical Formula Molar Mass Molar Volume Mole Molecular formula Percent Composition Representative Particle Standard Temperature & Pressure Formula Units Avogadro’s number


UNIT: Moles NO. OF DAYS: 14

KEY LEARNING(S): converting moles, empirical and molecular formulas, percent composition

UNIT ESSENTIAL QUESTIONS: How is matter measured?

CONCEPT



Mole Worksheet #2 Mole Project Chapter 9 Assessment

Mole Lab: measuring varying units with accuracy Mole Project – compare everyday materials to a mole Mole Worksheet #2 (new name TBD) Mole Roadmap – picture representation, etc.


UNIT: Equations NO. OF DAYS: 8 days

KEY LEARNING(S): writing and balancing equations, identifying the type, predicting the products of SR and DR reactions

UNIT ESSENTIAL QUESTIONS: Why is it important to balance and classify chemical reactions?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.B.2.1 Predict what happens during a chemical reaction. Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2 Science S11.A.1.3.2, S11.A.2.1.3, S11.A.3.1.2, S11.C.2.1.2

CHEM.B.2.1.3 Classify reactions as synthesis, decomposition, single replacement, double replacement, or combustion. CHEM.B.2.1.4 Predict products of simple chemical reactions (e.g., synthesis, decomposition, single replacement, double replacement, combustion). CHEM.B.2.1.5 Balance chemical equations by applying the Law of Conservation of Matter.

SAS EQ: What factors identify the types of chemical reactions? How do stoichiometric ratios relate reactants to products in a chemical reactions? LOCAL EQ: What are the steps in writing a balanced chemical equation? How do the 5 classifications of chemical reactions differ from each other? How are the products of a chemical reaction predicted?

Chemical Equation Coefficients Subscripts Yield Reactants Products Reaction Skeleton equation Catalyst Classify Compound Substance Element Heat Energy Hydrocarbon

Balanced Equations Combustion RXN Synthesis RXN Combustion RXN Decomposition RXN Double Replacement RXN Single Replacement RXN Activity series


UNIT: Equations NO. OF DAYS: 8

KEY LEARNING(S): writing and balancing equations, identifying the type, predicting the products of SR and DR reactions

UNIT ESSENTIAL QUESTIONS: Why is it important to balance and classify chemical reactions?

CONCEPT


Exit Slips Google Forms Padlets

Chapter 8 Assessment Balancing Blocks Predicting Products Lab – students will predict single/double replacement products (some may not react)


UNIT: Stoichiometry NO. OF DAYS: 16 days

KEY LEARNING(S): using stoichiometry to solve for reactants & products, limiting reactant, percent yield

UNIT ESSENTIAL QUESTIONS: Why is stoichiometry essential to chemistry?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.B.2.1 Predict what happens during a chemical reaction. Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.2.2.1, S11.A.3.1.2, S11.C.2.1.2

CHEM.B.2.1.1 Describe the roles of limiting and excess reactants in chemical reactions. CHEM.B.2.1.2 Use stoichiometric relationships to calculate the amounts of reactants and products involved in a chemical reaction.

SAS EQ: How do stoichiometric ratios relate reactants to products in a chemical reaction? LOCAL EQ: How does the mole ratio relate the reactants and products of a chemical equation? How are mole ratios used to predict the amounts of reactants and/or products What is the limiting reactant and how is it determined?

Quantitative Calculate Conservation Mass Mole Volume Predicting Conversion factor Formed Ratio Efficiency

Actual Yield Excess Reagent Limiting Reagent Mole Ratio Percent Yield Stoichiometry Theoretical Yield


UNIT: Stoichiometry NO. OF DAYS: 16

KEY LEARNING(S): using stoichiometry to solve for reactants & products, limiting reactant, percent yield

UNIT ESSENTIAL QUESTIONS: Why is stoichiometry essential to chemistry?

CONCEPT



Chapter 9 Assessment(s) Baking Soda Decomposition Lab – with accuracy component Recipe to Grocery List Activity – apply stoichiometric principles to it

COURSE NAME: Chemistry (NOT DIRECTLY INCLUDED IN “KEYSTONE CONTENT DOCUMENT”)

UNIT: States of Matter NO. OF DAYS: 2 days

KEY LEARNING(S):

UNIT ESSENTIAL QUESTIONS: How does the kinetic theory apply to solids, liquids, and gases?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

Why do gases behave the

way they do?

How do gases behave

differently than liquids?

How do gases behave

differently than solids?

How does a phase diagram

represent the changes in

states of matter?

Gas Pressure Pressure Atmospheric Pressure Barometer Pascal Model Collisions Elastic Constant Random Motion Insignificant Particles Kinetic energy Kelvin temperature Evaporation Condensation Melting Freezing Boiling Sublimation Deposition Crystal Solid Liquid Gas

Kinetic Theory Standard Atmosphere Vapor Pressure Allotropes Amorphous Phase diagram Triple point Critical point


UNIT: States of Matter NO. OF DAYS: 8

KEY LEARNING(S):

UNIT ESSENTIAL QUESTIONS: How does the kinetic theory apply to solids, liquids, and gases?

CONCEPT



UNIT: Gas Laws NO. OF DAYS: 16 days

KEY LEARNING(S):

UNIT ESSENTIAL QUESTIONS: What are the relationships between volume, temperature, pressure, and moles of a gas?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.B.2.2 Explain how the kinetic molecular theory relates to the behavior of gases. Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.1.1.4, S11.A.2.1.3, S11.A.3.1.2, S11.C.1.1.5

CHEM.B.2.2.1 Utilize mathematical relationships to predict changes in the number of particles, the temperature, the pressure, and the volume in a gaseous system (i.e., Boyle’s law, Charles’s law, Dalton’s law of partial pressures, the combined gas law, and the ideal gas law). CHEM.B.2.2.2 Predict the amounts of reactants and products involved in a chemical reaction using molar volume of a gas at STP.

SAS EQ: In what ways has the theory of the atom changed over time due to technological improvements? LOCAL EQ: How is gas pressure affected? How did Boyle, Charles, and Gay-Lussac describe the relationships among, the temperature, pressure, and volume of a gas? What is the difference between a real and an ideal gas? How can the Ideal Gas Law be applied to stoichiometry? How can partial pressure be used to calculate total pressure?

Evaporation Boiling Point Compressible Inverse Direct Indirect Constant Sum Total

Boyle’s Law Charles’ Law Gay-Lussac Law Combined Law Dalton’s Law of Partial Pressure Ideal Gas Constant Ideal Gas Law Partial pressure


UNIT: Gas Laws NO. OF DAYS: 16

KEY LEARNING(S): solve problems using the appropriate gas law equation

UNIT ESSENTIAL QUESTIONS: What are the relationships between volume, temperature, pressure, and moles of a gas?

CONCEPT



Chapter 11 Assessment(s) Pressure – Temperature Lab Pressure – Volume Lab Molar Mass of Butane Lab


UNIT: Solubility NO. OF DAYS: 10 days

KEY LEARNING(S):

UNIT ESSENTIAL QUESTIONS: How are solutions formed?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

CHEM.A.1.2 Compare the properties of mixtures. Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.1.1.4, S11.A.2.1.3, S11.A.3.1.2, S11.C.1.1.5

CHEM.A.1.2.1 Compare properties of solutions containing ionic or molecular solutes (e.g., dissolving, dissociating). CHEM.A.1.2.3 Describe how factors (e.g., temperature, concentration, surface area) can affect solubility.

SAS EQ: LOCA EQ: How is solubility affected? How do you read a solubility curve? How are the concentrations of a solution described?

Saturated Solution Solubility Unsaturated Solution Supersaturated Solution Concentration Dilute Solution Concentrated Solution Dissolve Agitate Surface area Particle size Units

Miscible Immiscible Molarity Percent Mass Percent Volume


UNIT: Solubility NO. OF DAYS: 10

KEY LEARNING(S): converting among solution units: molarity, % mass, % volume, predicting solubility

UNIT ESSENTIAL QUESTIONS: How are solutions formed?

CONCEPT



Chapter 12 Assessments Making a Solubility Curve Activity Solubility Lab Beer’s Law Lab – copper composition Unsaturated/Saturated/Supersaturated Solutions Lab – hand warmers (sodium acetate)

COURSE NAME: Chemistry (OPTIONAL – NOT REQUIRED BY “KEYSTONE CONTENT DOCUMENT”)

UNIT: Acids and Bases NO. OF DAYS:

KEY LEARNING(S):

UNIT ESSENTIAL QUESTIONS: Why are acid and base reactions important for life?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.1.1.4, S11.A.2.1.3, S11.A.3.1.2, S11.C.1.1.5

How do the properties of

acids and bases differ?

How can pH be measured?

How are strong acids and

bases differentiated from

weak acids and bases?

Why is an acid/base reaction

called a neutralization

reaction?

Strong acid Strong base Weak acid Weak base Neutralization Salt

Binary acid Oxyacid Arhenius acid Arhenius base BronstedLlowry Acid Bronsted-Lowry Base Bronssted-Lowry Acid-Base Reaction Monoprotic Acid Polyprotic Acid Diprotic Acid Triprotic Acid Lewis Acid Lewis Base Lewis Acid-Base Reaction Conjugate Acid Conjugate Base Amphoteric


UNIT: Acids and Bases NO. OF DAYS:

KEY LEARNING(S):

UNIT ESSENTIAL QUESTIONS: Why are acid and base reactions important for life?

CONCEPT



Chapter 14 Assessment Test pH of Household Items Cabbage Juice pH Indicator

COURSE NAME: General Chemistry (OPTIONAL – NOT REQUIRED BY “KEYSTONE CONTENT DOCUMENT”)

UNIT: Nuclear Chemistry NO. OF DAYS:

KEY LEARNING(S):

UNIT ESSENTIAL QUESTIONS: How is nuclear chemistry used in everyday life?


# OF DAYS




TIER 2 VOCABULARY

TIER 3 VOCABULARY

Reading R11.A.2.1, R11.A.2.2.2, R11.A.2.4.1 Math M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2.2 Science S11.A.1.1.4, S11.A.2.1.3, S11.A.3.1.2, S11.C.1.1.5

Why are certain elements

radioactive?

How are the 3 types of

radiation different from each

other?

How is nuclear energy

generated?

What are the pros and cons of

nuclear fission and fusion?

How is radiation detected and

used in your life?

Nuclear Reaction Radioactive Decay Nuclear Radiation Film Badge Geiger-Muller Counter Radioactive Dating Nuclear Waste Nuclear Fission Chain Reaction Nuclear Reactor Nuclear Power Plant Nuclear Fusion

Nucleon Nuclide Mass Defect Nuclear Binding Energy Nculear Shell Model Magic Number Transmutation Radioactive Nuclide Alpha Particle Beta Particle Positron Electron Capture Gamma Ray Half-life Decay Series Parent Nuclide Daughter Nuclide Artificial Transmutation Transuranium Element Roetgen Rem Scintillation Counter Radioactive Tracer Critical Mass Shielding Control Rod Moderator


UNIT: Nuclear Chemistry NO. OF DAYS:

KEY LEARNING(S):

UNIT ESSENTIAL QUESTIONS: How is nuclear chemistry used in everyday life?

CONCEPT



Chapter 21 Assessment Student Research & Presentation – Areas of Nuclear Chemistry Gizmo – Half-life & Radioactive Decay

Documents

WAYNESBORO AREA SCHOOL DISTRICT CURRICULUM …€¦ · · 2015-07-07WAYNESBORO AREA SCHOOL DISTRICT CURRICULUM - CHEMISTRY COURSE NAME: Chemistry ... M11.A1.2.3, M11.A.2.2.1, M11.A.2.2.2