Chemistry is the study of matter and the interactions that matter undergoes. The structure, properties, and changes that matter undergoes are studied from both particulate and bulk (macroscopic) perspectives. The energy transformations that occur during physical, chemical, and nuclear changes are also key and help students make predictions and justifications of the phenomena they observe. Physical and mathematical models are used to enhance learning and aid in the explanation of various physical and chemical concepts/processes.
How can one distinguish and describe various samples of matter?
How can one model the particles that make up matter?
How is chemistry a quantitative science?
Why is it important to safely perform laboratory experiments?
What are the different types of observations that scientists make?
How can particle diagrams be used to represent samples of elements, compounds, homogeneous mixtures and heterogeneous mixtures?
How do scientists represent measurements and know what to round their calculations to?
What changes (chemical, physical, or nuclear) can a sample of matter undergo?
New York Prentice Hall Chemistry 2008 edition for all units: Chapters 1, 2 and 3
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Demonstrate proper lab safety and be knowledgeable of the location and use of safety equipment.
Classify samples of matter and separate various classes of matter.
Use scientific inquiry practices to solve laboratory based problems.
Make quantitative measurements carefully and to the correct level of precision.
Perform metric conversions.
Use scientific notation.
Determine the number of significant figures in a measurement and apply the rules for rounding when appropriate.
Describe the techniques used to separate components of a mixture.
Honors Enrichment:
Students will be expected to:
Solve problems with dimensional analysis.
Perform multi step calculations especially with values that are in exponential format.
MP.2, MP.4, HS-PS1-1
How can one explain the structure, properties, and interactions of matter?
Why does the slightest change in nuclear or electronic structure have such a dramatic effect on the qualities of an atom or ion?
What is our modern understanding of the atom?
How has the model of the atom evolved through time?
How are protons, electrons, and neutrons different from each other?
What information does the nuclide symbol provide regarding the component parts of an atom?
How can there be different atoms for an element?
How is a weighted average different from other types of averages?
New York Prentice Hall Chemistry 2008 edition for all units: Chapters 4 and 5
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Explain the historical development of the modern atom.
Describe Rutheford’s gold foil experiment in detail and indicate his two conclusions.
Use bright line spectra to identify an unknown element in a mixture of elements.
Write and use nuclide symbols as a means to indicate proton, neutron, and electron number for an atom or ion.
Use the periodic table as a resource to determine the organization of subatomic particles.
Compare and contrast the ground state and excited state of an atom or ion.
Define isotopes and be able to calculate average atomic mass given appropriate data.
Calculate the charge of an ion based on the number of protons and electrons.
Write electron configurations for ground state and excited state species using shell notation
Honors Enrichment:
Students will be expected to:
Apply the concepts of the wave-mechanical model to writing various types of electron configuration including orbital notation and noble gas configuration.
Relate the organization of the periodic table to the underlying electronic organization of atoms. For example, s block, p block, d block, and f block.
Describe the four quantum numbers of a given electron.
Use modern electron configurations to lay the foundation for our later unit on chemical bonding. Valence, kernel and lone electrons are highlighted.
Calculate the wavelength, frequency, and energy of a given portion of the electromagnetic spectrum as part of the wave-particle duality discussion of an electron.
Calculate the natural abundances of isotopes provided the necessary data.
HS-PS1.A , HS-PS1-2B, MP.2,MP.4, HS-PS4-4, HS-PS3-5
What forces hold nuclei together and mediate nuclear processes?
Do all radioactive isotopes decay in the same way and at the same rate?
How are nuclear reactions both beneficial and harmful in our lives?
What are the most common types of nuclear decay?
How do we separate the different types of nuclear emanations?
Are there ways to represent nuclear reactions?
How are nuclear reactions different from chemical and physical changes?
What nuclear reactions are used in nuclear power and nuclear weapons?
What are the cons and pros of nuclear energy?
What are some positive uses of radionuclides in our everyday lives?
New York Prentice Hall Chemistry 2008 edition for all units: Chapter 25
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Distinguish between natural transmutation, artificial transmutation, fission, and fusion.
Differentiate between the four types of nuclear reactions.
Distinguish the different nuclear emission particles by mass, charge, penetrating power and ionizing power.
Balance nuclear equations.
Define and solve half life problems.
Outline the risks and benefits of nuclear energy.
Identify the beneficial uses of radioisotopes: C-14, I-131, U-238, and Co-60.
Honors Enrichment:
Students will be expected to:
Calculate mass defect and binding energy of a given nuclide.
Relate binding energy to the stability of a given nucleus.
Label and describe the function of the various parts of a nuclear reactor.
HS-PS1-8, HS-PS1.C, HS-PS3-5, MP.2, MP.4
How does the development of the periodic table relate to periodic law?
How does atomic structure determine the organization of the periodic table?
Who is credited with creating the periodic table of elements?
In what ways can an atom of an element differ from one element to the next?
What evidence can you use to identify an element based on its location on the periodic table?
Is it possible for two different samples of an element to have entirely different properties?
How do periodic properties such as ionization energy help predict chemical properties for an element?
New York Prentice Hall Chemistry 2008 edition for all units: Chapter 6
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Understand the historical development of the periodic table.
List the general properties of metals, nonmetals, and metalloids.
Classify elements as being metals, nonmetals or metalloids based on their position on the periodic table.
Describe general trends regarding: electronegativity,ionization energy,atomic radius,and other physical properties specifically mentioned on table S..
Explain periodic trends in terms of nuclear charge, numbers of principal energy and shielding electrons..
Identify the elements that are solid,liquid and gas elements at STP.
Correlate the placement of elements on the periodic table with their atomic structure.
Identify common allotropes carbon, oxygen, and phosphorus.
Relate the reactivity of metals and nonmetals to their relative positions on the periodic table.
Honors Enrichment:
Students will be expected to:
Describe and explain periodic trends without a Regents reference table.
Understand the periodic table in terms of modern electron configurations.
HS-PS1-1, HS-PS1-2
How do substances combine or change to make new substances?
Are all chemical bonds the same?
How does bond type and electron distribution influence the properties of compounds?
How does the number of valence electrons relate to bond formation?
How does a Lewis structure look different for an ionic compound versus a molecular species?
How is energy involved in bond formation?
How can electronegativity values be used to predict the type of chemical bond?
How are bond polarity and molecular polarity determined?
Can the type of bonding within a substance be determined by the physical properties of the substance?
New York Prentice Hall Chemistry 2008 edition for all units: Chapters 7 and 8
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Draw lewis dot diagrams of ionic and covalent species.
Predict the polarity of a chemical bond based on electronegativity values.
Predict the polarity of a molecule based on its shape and charge distribution.
Explain the relationship between energy and bond formation.
Distinguish properties of ionic vs covalent molecules.
Relate the definition of metallic bonding to a metal’s macroscopic properties.
Differentiate between the different types of intermolecular forces in an effort to explain the macroscopic properties of a sample.
Honors Enrichment:
Students will be expected to:
Describe the electron domain geometry, molecular geometry, and bond angles using the VSEPR model.
Draw Lewis diagrams for complex ions and molecules.
Use the concept of resonance to explain species that can not be described by a single Lewis structure.
Use formal charges to predict which Lewis structure is most probable.
Describe the hybridization that occurs around the central atom in a covalent species.
List the properties of ionic solids, covalent molecules, and metallic substances.
Determine the type and extent of IMF’s in an attempt to account for the VP, BP, MP, Hf, and Hv of given molecules. (This topic can be taught later in the course if necessitated by time considerations)
HS-PS1-1, HS-PS1-3, HS-PS2-6, HS-PS1-2, HS-PS1-4, HS-PS1-5, HS-PS3-5
How do substances combine and change to make new substances?
How does one characterize and explain these reactions and make predictions about them?
How do we demonstrate the quantitative information inherent in a chemical formula?
How do you predict the formulas of ionic compounds using oxidation numbers?
How can the empirical formula of any compound be obtained from experimental mass data?
How do you name ionic and molecular compounds and use their names to determine their chemical formulas?
What is the format for a balanced chemical equation?
What are 4 major types of chemical reactions and their identifying characteristic ?
How do you predict the products of chemical reaction?
How is it possible to make predictions of amounts of reactants needed and products formed using the inherent mathematical relationship of balanced chemical reaction?
New York Prentice Hall Chemistry 2008 edition for all units: Chapters 9-12
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Write chemical formulas and name compounds.
Write and balance chemical equations.
Predict the products of chemical reactions only given the reactants.
Classify the four common types of inorganic reactions and combustion.
Determine formula mass of different compounds.
Calculate the percentage composition of a compound.
Perform mole conversions.
Relate molecular formulas and empirical formulas.
Perform mole to mole stoichiometric conversons.
Demonstrate the Law of Conservation of Mass as it relates to chemical equations.
Honors Enrichment:
Students will be expected to:
Write formulas and name compounds without the help of Regents Reference Tables.
Translate and balance challenging molecular reactions.
Perform mixed mole conversions.
Determine an empirical formula from percent composition and lab data.
Perform limiting reagent calculations.
Compare theoretical yield to actual yield.
Perform mixed mole stoichiometry calculations.
HS-PS1-2, HS-PS1-7, MP.2, MP.4, HS-LS1-5
How can one explain the structure, properties and interactions of matter?
What makes the three common phases matter distinct from one another?
What circumstances determine which phase of matter we observe?
How does energy input and output affect the molecules in a sample?
How can energy be transformed from one form of energy to another?
How do we describe phase changes?
What are the “heat formulas” and how are they used?
What are the five postulates of the Kinetic Theory of Gases?
Does matter follow mathematical laws?
What conditions are optimal for a real gas?
How does evaporation, boiling and vapor pressure relate to each other?
New York Prentice Hall Chemistry 2008 edition for all units: Chapters 13, 14, and 17
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Define potential and kinetic energy.
Give examples of energy and explain how one form can be converted into another.
Compare and contrast the different phases of matter.
Explain heating and cooling curves in terms of changes in kinetic and potential energy.
Relate the Law of Conservation of Energy to a balanced chemical reaction.
Define temperature and relate it to average kinetic energy.
Convert Kelvin to and from degrees Celsius.
Determine the direction of heat flow within a system.
Use the specific heat capacity of a substance with principles of calorimetry.
Determine the heat required for the fusion or vaporization of a substance.
Describe the behavior of solids, liquids and gasses using Kinetic Molecular Theory.
Account for the differences between ideal and real gas behavior.
Use the predictive nature of the combined gas law.
Utilize Avogadros’ Hypothesis.
Define vapor pressure and boiling.
Relate relative vapor pressures to intermolecular force strengths.
Differentiate between boiling point and normal boiling point.
Use vapor pressure curves to determine the boiling point of a liquid at various pressures.
Honors Chemistry:
Students will be expected to:
Label and use the predictive nature of phase diagrams
Calculate the energy required to bring a given mass of solid to a gas given only the temperature change.
Analyze data to derived Boyle’s, Charles and Guy Lussac’s Laws
Use the Ideal Gas Equation to model gas behavior.
Perform calculations with Graham’s and Dalton’s Law of Effusion.
HS-PS1-3, HS-PS1-4, HS-PS1-9, HS-PS2-6, HS-PS1-7, MP.2 and MP.4
How can one explain the structure, properties and interactions of matter?
How can one predict whether one substance will be soluble in another?
What factors affect the rate of dissolution and the degree in which one material dissolves in another?
What does a homogeneous mixture look like at the particulate level?
What attractive forces allow a solute and solvent to interact?
What specific environmental factors determine the solubility of a given solute?
How is solution concentration expressed?
What effect does a solute have on its solute?
How are saturated, unsaturated or supersaturated solutions distinguished from each other?
New York Prentice Hall Chemistry 2008 edition for all units: Chapters 15 and 16
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Compare heterogeneous and homogeneous mixtures.
Distinguish between a solute, solvent and solution.
Identify solutes as an acid, base, salt or nonelectrolyte.
Separate components of mixtures by physical means.
Predict miscibility and solubility using molecular polarity.
Predict which environmental conditions affect the solubility of solids and gasses.
Use solubility rules to predict solubility of a salt.
Determine solubility of a compound at a given temperature using a solubility curve.
Differentiate between saturated, unsaturated, and supersaturated solutions.
Predict temperature at which solution equilibrium will occur.
Calculate molarity and parts per million.
Predict the change in freezing point and boiling point temperatures based on the presence of a specific solute.
Honors Chemistry:
Students will be expected to
Memorize solubility rules and predict whether metathesis reactions occur.
Write net ionic equations for single and double replacement reactions.
Determine the molality and mole fraction of a solution.
Calculate molal freezing point depression, molal boiling point elevation and vapor pressure changes for a solution.
Determine the molecular mass of an unknown solute by its freezing point depression.
Perform solution stoichiometry calculations,
HS-PS1-10,HS-PS1-3, HS-PS2-6, MP.2, and MP.4
How do you recognize a system at equilibrium?
How are reversible reactions affected by changes in concentration, temperature or Pressure?
How do the conditions that exist at the particulate level the rate of a chemical reaction?
What makes a collision effective?
What factors affect the rate of a reaction?
How does the energy of the reactants and products change over the course of a reaction?
What makes equilibrium dynamic?
What are examples of phase, solution and chemical equilibrium?
How does changing the reaction conditions affect a reaction at equilibrium?
How do catalysts affect the rate of chemical reaction?
How is the shape of a potential energy diagram affected by the presence of a catalyst?
New York Prentice Hall Chemistry 2008 edition for all units: Chapter 18
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Use the collision theory to explain how a change in reaction conditions affects the rate of reaction.
List the factors that affect reaction rate.
Distinguish between exothermic and endothermic chemical and physical changes.
Interpret Table I using the heat of reaction values.
Label potential energy diagrams.
Differentiate between different types of equilibria.
Utilize Le Chatelier's principle to predict shifts in reactions.
Define Entropy.
Determine entropy changes given a physical or chemical change.
Predict a spontaneous change given thermodynamic values.
Honors Enrichment:
Students will be able to:
Write mass action expressions.
Solve simple equilibrium calculations.
Understand the usage and magnitude of Kc and Ksp.
Perform Ksp calculations.
Calculate enthalpy change using Hess’s Law, Standard Enthalpies, and Bond Dissociation Energies
Predict spontaneous change using thermodynamic values and Gibbs Free Energy Equation when appropriate.
HS-PS1-4, HS-PS1-5, HS-PS1-6, HS-PS1-2, HS-PS1-10, HS-PS1-7, MP.2, and MP.4
How has the understanding of acids and bases changed through time?
How is the ratio of hydronium and hydroxide fixed in an aqueous solution?
What chemically differentiates an acidic solution from a basic solution?
What quality do acids, bases and salts all share?
What is the net ionic equation for an acid or base neutralization?
How does titration work?
What is the mathematical meaning behind the pH scale?
New York Prentice Hall Chemistry 2008 edition for all units: Chapter 18
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Classify acids and bases by their operational definitions.
Recognize electrolytes and nonelectrolytes using Arrhenius Theory.
Label Bronsted Lowry acids and bases given a reaction.
Differentiate between monoprotic, diprotic and triprotic acids.
Predict reactants or products of neutralization reactions.
Determine pH given solution concentration.
Understand pH as a logarithmic scale.
Determine the unknown concentration of an acid or base given titration data.
Predict indicator results given solutions of different pH values.
Honors Enrichment:
Students will be expected to:
Diagram Bronsted-Lowry reactions including conjugate pairs.
Determine the pH of weak acids and bases.
Compare B-L, Arrhenius and Lewis Acid Base Theories.
Understand the meaning of Ka, Kb and Kw.
Solve problems relating pH, pOH, hydrogen, hydroxide and hydronium concentration.
Predict the pH of a salt solution given the formula of the salts
Name acids and bases using the IUPAC system
HS-PS1-11, MP.2, MP.4, HS-PS1-7
How do electron transfer reactions occur?
Are all chemical reactions reduction-oxidation reactions?
What energy transfers are possible in electrochemical cells?
What is oxidation?
What is reduction?
How does one know if a redox reaction has occurred?
How are redox reactions balanced?
What factors cause a spontaneous reaction?
Which electrochemical cells have reactions that occur spontaneously?
How is electroplating different from electrolysis?
What is the theoretical voltage of a voltaic cell at equilibrium?
New York Prentice Hall Chemistry 2008 edition for all units: Chapters 20 and 21
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Assign oxidation numbers to the elements in a substance.
Define oxidation and reduction.
Read, write and interpret half reactions.
Determine substance(s) oxidized and substances reduced in a chemical reaction.
Verify the Law of Conservation of Charge.
Differentiate between redox and nonredox reactions.
Label and explain the operation of a voltaic cell.
Label and explain the operation of electrolytic cells.
Distinguish between electrochemical and electrolytic cells.
Use table J to predict spontaneous change.
Diagram and outline the process of electroplating.
Honors Enrichment
Students will be able to:
Determine the relative reducing potential and oxidation potential of a species given a table of reduction potentials.
Calculate standard electrode potential for a given redox reaction.
Compare standard to nonstandard conditions for a voltaic cell.
HS-PS1-1, HS-PS1-12, MP.2, MP.4
Why is understanding organic chemistry important in our lives?
How is it possible that there are so many different types of organic compounds?
What is the definition of an organic compound?
What polymers were studied in Biology?
What are saturated and unsaturated fats?
What are the different types of organic compounds?
Why is the goal of nomenclature to have only one name for each organic compound?
What makes one class of organic compounds different from the next?
What are the different types of organic reactions?
What is the usefulness of each type of formula: molecular, condensed, and structural?
New York Prentice Hall Chemistry 2008 edition for all units: Chapters 22-24
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Characterize the properties of organic compounds.
Draw and name hydrocarbons.
Classify hydrocarbons into their appropriate series.
Classify, name, and draw hydrocarbon derivatives.
Distinguish between structural formulas, condensed structural formulas and molecular formulas.
Determine the number of isomers possible of a given formula.
Recognize and complete the seven organic reactions: combustion, fermentation, saponification, esterification, addition, substitution, and polymerization.
Honors Enrichment:
Students will be able to:
Draw and name aromatic hydrocarbons.
Identify hydrocarbon derivatives important in biochemical reactions.
Draw and name all of the isomers of a hydrocarbon or hydrocarbon derivative given only a molecular formula.
Classify alcohols by the number of hydroxyl groups
Classify alcohols as primary, secondary, and tertiary.
Predict the products of etherification, and the oxidation of alcohols, aldehydes and ketones.
HS-PS2-6, HS-PS1-1
How do organisms interact with their environment and what are the effects of these interactions?
How does our daily life impact the world around us?
What can we do to improve the environment?
New York Prentice Hall Chemistry 2008 edition for all units: Chapters 22-24
Honors Text: Chemistry by Chang, 10th edition as needed
Students should be able to:
Research and form opinions on climate change based on scientifically reputable sources.
Research and form opinions on extreme weather events based on scientifically reputable sources.
Research and form opinions on ozone depletion based on scientifically reputable sources.
Research and form opinions on acid rain based on scientifically reputable sources.
Research and form opinions on polar ice depletion based on scientifically reputable sources.
All previous standards are applicable.
LS1, HS-ETS1-1,2,3 and 4