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Chemistry R
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Note: Standards are based on NYSSLS which will not be implemented until 2025-26, but content is based on current Physical Setting: Chemistry Regents standards.
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PacingUnit TitleStandardsContentVocabularyLearning Targets/Focus QuestionsResourcesAssessment
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NumberDescription
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2-3 daysElement SymbolsKnow the names and symbols of 40 elements most commonly used in this course Students will identify 40 common elements by their names and symbolsFlash cards, Quizizz practiceQuiz
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Approximately 7 days interspersed with first two unitsLab BasicsLab Safety - Conduct yourself safely in a lab setting, know what to do in case of lab accident or emergency.Eyewash, safety shower, fire blanket, first aid kit, fire extinguisher, lab aprons, safety goggles/goggle cabinet, apparatus, neutralize, volatile, fume hood, insoluble, dilute, distilled water, bunsen burnerStudents will know the proper procedures for dealing with:
injuries
fires
chemical handling
chemical cleanup
lab attire
lab behavior
glassware		Flinn lab safety contract, Flinn lab safety test, POGIL Safety FirstLab safety test
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Writing a lab report - Set up lab folder, sign lab contracts etcPurpose, materials, procedure, data/observations, calculations, conclusion Students will be able to write a proper lab reportLab NotebookEvaluating student lab reports through year
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Lab Equipment - Learn lab stations, know equiment in lab kits, restock missing itemsWatch glass/evaporating dish, crucible, crucible tongs, iron ring, clay triangle, striker, ring clamp/s-clamp, thermometer clamp, test tube, test tube clamp, test tube holder, microspatula/scoopula, beaker, flask, graduated cylinder, beaker tongs, wire gauze, bunsen burner, grease pencilStudents will be able to identify basic lab equipmentLab Kits and included lab equipmentLab report
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Using Bunsen Burner - Learn how to use Bunsen burner, set appropriate flame, set up ring stand for heating crucibles, beakers, and test tubes.Bunsen Burner, striker, collar, barrel, air intake, gas flow valve, gas intake, base, blue triangle, ring standStudents will be able to set up and use a Bunsen burner in chemistry labBunsen Burner, beaker, ring stand, crucible, crucible tongs, iron ring, clay triangle, striker/lighter, test tube, test tube clamp, utility clamp, thermometer clamp, stampLab Report
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2 weeksStudy of MatterHS-PS1-10.
Use evidence to support claims regarding the formation, properties and behaviors of solutions at bulk scales.
Particulate Nature of MatterAtom, Chemical Change, Chemical Equation, Chemical Reaction, Chemical Property, Chemistry, Chromatography, Composition, Compound, Diatomic, Distillation, Element, Empirical Formula, Filtration, Gas, Homogeneous, Heterogeneous, Ion, Liquid, Mass, Matter, Mixture, Mole, Molecule, Molecular Formula, Particle Diagram, Physical Change, Physical Property, Polyatomic Ion, Solid, Solution, Standard Temperature and Pressure (STP), State/Phase, Structural Formula, Substance, Vapor1. Recognize, understand, and use all vocabulary terms.
2. Use the density formula to calculate density, mass, or volume.
3. Use density to identify a substance.
4. Explain the particle nature of matter.
5. Identify the 4 types of particles that make up matter.
6. Classify matter as a substance or mixture.
7. Describe the properties of elements, compounds, and mixtures.
8. Identify the 7 diatomic elements.
9. Identify the states of matter and their properties.
10. Draw a particle diagram of each state.
11. Identify STP.
12. Identify and compare homogeneous and heterogeneous mixtures.
13. Explain how to separate parts of a mixture and identify specific separation techniques.
14. State or identify the three basic types of chemical formulas.
15. Reduce an empirical formula to its simplest form.
16. Identify a mixture and describe its properties.
17. Identify and contrast physical and chemical changes.
18. Determine when a chemical reaction has occurred.
19. Read a chemical equation.
20. State and apply the law of conservation.
Investigating Matter 1 Lab (properties and mixtures), Investigating Matter 2 Lab (chemical changes), worksheets, unit review, unit test
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HS-PS1-2
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
States of Matter
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Properties of Matter
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Classifying Matter
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Elements
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Compounds
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Chemical Formulas
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Mixtures
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Changing Matter
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Chemical Equations
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Law of Conservation
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3 WeeksMath of ChemistryHS-PS1-7
. Use mathematical representations to support the claim that atoms, and therefore mass, are conserved during a chemical reaction
S.I. SystemAtomic Mass, Atomic Symbol, Chemical Formula, Formula Mass, Gram Formula Mass, Joule, Kelvin, Micro-, Molar, Mass, Mole, Nano-, Pascal, Percent, Composition, Percent, Error, Pico-, Scientific Notation, Significant Figures (Sig Figs), Standard Number or Standard NotationRecognize, understand, and use all vocabulary terms.
2. Identify and use the basic units of measurement.
3. Use Table C to convert between units of measurement.
4. Use Table T to convert between Celsius and Kelvin temperatures.
5. Use the percent error formula.
6. Define significant figures.
7. Make measurements to the correct number of significant figures.
8. Identify the number of significant figures in a measurement.
9. Round numbers and calculations to the correct number of significant figures.
10. Interpret a number written in scientific notation.
11. Read a chemical formula.
12. Count the number of each type of atom in a chemical formula.
13. Calculate formula mass.
14. Calculate gram formula mass.
15. Use the mole formula to find moles, mass, or gram formula mass.
16. Calculate percent composition of a substance or mixture.
17. Use the Law of Conservation to find the missing mass of a substance.		Density Lab, Mole Calculation Lab, various worksheets, review packet, unit test
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Accuracy, Precision and Percent error
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Significant Figures
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Calculations with Signifcant Figures
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Scientific Notation
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Chemical Formulas
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Law of Conservation of Mass
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3 weeksStates of MatterHS-PS1-9.
Analyze data to support the claim that the combined gas law describes the relationships among volume, pressure, and temperature for a sample of an ideal gas.
States and Intermolecular ForcesAvogardo’s Law, Boiling, Boiling point, Boyle’s Law, Charles’ Law, Combined Gas Law, Condensation, Condensation point, Cooling curve, Crystallization, Deposition, Endothermic, Exothermic, Evaporation, Freezing, Freezing point, Heating curve, Gas, Guy-Lussac’s Law, Ideal Gas, Kinetic Molecular Theory, Liquid, Melting point, Phase, Real Gas, Solid , Solidification, State, Sublimation, Vapor, Vapor pressure1. Know and use all vocabulary terms.
2. Identify the three states of matter and their properties.
3. Identify a crystal as a solid with a regular geometric pattern.
4. Draw a particle diagram representing each state.
5. Use state to compare the strengths of intermolecular forces.
6. Identify phase changes, and whether they are exothermic or endothermic .
7. Identify the properties of substance that allow it to sublime.
8. Identify CO2(s) and I2(s) as substances that can sublime.
9. Define melting and boiling point in terms of vapor pressure and/or equilibrium.
10. Label state, changes of state, and temperature changes on a heating or cooling curve.
11. Identify the effects of pressure on a substance’s melting and boiling point.
12. Use Table S to identify the state of a given element at any temperature.
13. Use Table H to determine vapor pressure and boiling point, and to compare the
strengths of intermolecular forces.
14. Explain the relationship between intermolecular forces and vapor pressure.
15. Identify the four properties of an ideal gas.
16. List 3 differences between an ideal gas and a real gas.
17. Identify the conditions in which a real gas will behave most like an ideal g
18. Identify the two real gases which most closely resemble an ideal gas.
19.State and apply Avogadro’s Law.
20. Explain the relationships between temperature, volume and pressure as described by
Boyle’s Law, Charles’ Law, and Gay Lussac’s Law.
21. Use the Combined Gas Law formula to calculate temperature, volume, and pressure.		vacuum pump, gallium, peep demo, two balloon demo, phetGas Law lab, worksheets, unit review, unit test
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Changing State
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Vapor Pressure
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KMT/Ideal Gases
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Avagadro's Law
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Combined Gas Law
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3 weeksAtomic TheoryProtons, neutrons, electronsAtom, Atomic Mass, Atomic Mass Unit (u), Atomic Number, Atomic Symbol, Bright Line Spectrum, Electron, Electron Configuration, Excited State, Ground State, Ion, Isotope, Kernel, Lewis Structure, Mass Number, Neutron, Notation, Nucleon, Nucleus, Plum Pudding Model, Proton, Octet Rule, Orbital, Principal Energy Level, Quantum Mechanical Model, Spectroscope, Subatomic Particle, Valence Level, Wave Mechanical ModelKnow and use all vocabulary terms
2. Identify the three subatomic particles, as well as their charges, masses, and location in the atom.
a. Be able to describe, compare and contrast the atomic models (Dalton model, plum pudding model,
nuclear model, Bohr model, wave-mechanical model).
3. Describe the gold foil experiment, and what it revealed about the atom.
4. Identify and write the atomic symbol of an element in the correct format.
5. Identify the relationship between atomic number and
a. subatomic particles
b. nuclear charge
c. an element’s identity
6. Define and calculate mass number.
7. Identify isotopes of the same element, and explain their similarities and differences.
8. Be able to write, read and interpret the proper notation for an isotope.
9. Calculate number of protons and neutrons present in any isotope.
10. Identify what the atomic mass unit is based on.
11. Use % abundance of isotopes to calculate atomic mass.
12. Define and calculate atomic mass.
13. Use the periodic table to identify an element’s
a. atomic symbol and atomic number
b. atomic mass
c. most common isotope
d. electron configuration
14. Explain how positive and negative ions are formed.
15. Calculate the charge of an ion and/or use charge to determine the number of electrons of an ion.
16. Describe how electrons move between principal energy levels.
17. Determine the maximum number of electrons that may be held by an energy level and orbital.
18. Correctly read electron configurations.
19. Identify an atom’s valence level.
20. Explain the importance of valence electrons.
21. Identify the number of electrons in the valence level.
22. Draw a correct Lewis structure/electron-dot diagram of an atom or ion.
23. Explain how a bright line spectrum is created and what it is used for.		Atomic ModelsDigital Lab - atomic structure, Size of Atom Lab, Flame Test Lab, worksheets, unit review, test
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History of Atomic Theory
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Characteristics
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Ions
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Electrons and Electron Configuration
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Bright line Spectrum
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2 weeksPeriodic TableHS-PS1-1
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
HistoryAlkali Metal, Alkaline Earth Metal, Atomic Radius, Electronegativity, Energy levels, Family, First Ionization Energy, Group, Halogen, Metal, Metallic Bond, Metallic character, Metalloid, Noble gas, Nonmetal, Period, Periodic Table, Periodic Law, Reactivity, Semi-metal, Transition element/transition metal
Know and use all vocabulary terms.
2. Define the Periodic Law.
3. Explain how the periodic table is arranged.
4. Explain what characteristics are shared by elements in the same period.
5. Explain what characteristics are shared by elements in the same group.
6. Identify metals, nonmetals metalloids and on the periodic table.
7. List the properties of metals and non-metals.
8. Explain how metallic bonds are formed.
9. Compare the metallic character of different elements.
10. Explain the trends of atomic radius seen on the periodic table.
11. Compare the size of two different atoms using the periodic table.
12. Explain how atomic radius changes when an atom becomes an ion.
13. Explain how electronegativity and first ionization energy indicate reactivity.
14. Explain what happens to metals and nonmetals in most chemical reactions.
15. Explain the trend of reactivity seen on the periodic table.
16. Compare the reactivities of two metals or nonmetals
17. Name the various groups of elements.
18. Identify the properties of each group of elements.		Property Cards, element samples, periodic tablePeriodic Properties Lab, Patterns, Lab, Worksheets, Unit Review, unit test
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HS-PS1-2
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
Organization - Periods and Groups
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Metals, Nonmetals, Metalloids
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Metallic Bonding
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Trends: Atomic and Ionic Radius
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Trends: Reactivity - Electronegativity and First Ionization Energy
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Characteristics of Element Groups
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3 weeksIonic BondingHS-PS1-1
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
Bonding BasicsBase, Binary Compound, Covalent Bond, Ionic Bond, Network, Noble Gas Configuration, Polyatomic Ion, Salt Know all vocabulary terms.
2. Identify the electrons used in bonding.
3. Explain why atoms bond in terms of their electron configuration.
4. Identify the electron configuration of an atom after it has bonded.
5. Explain how bonding affects atomic stability.
6. Explain how bonding affects the energy of atoms.
7. Identify the three types of bonds, how they are formed, and the elements that form them.
8. Draw Lewis dot diagrams for positive and negative ions.
9. Name positive ions using the correct roman numeral (when needed).
10. Name negative ions using the correct suffix.
11. Identify ionic compounds by their properties.
12. In terms of ions, explain why ionic solutions conduct electricity.
13. Given the name, write the formula of an ionic compound.
14. Given the formula, write the name of the ionic compound.
15. Draw the Lewis dot structure for an ionic compound.
16. Identify polyatomic ions in a chemical name or formula.
17. Identify compounds that contain both ionic and covalent bonds.		Salt ModelWorksheets,Unit Review, Unit Test
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HS-PS1-3.
Plan and conduct an investigation to gather evidence to compare the structure of substances at the bulk scale to infer the strength of electrical forces between particles.
Bonds and Energy
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HS-PS2-6
Communicate scientific and technical information about why the particulate-level structure is important in the functioning of designed materials.*
Types of Bonds
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HS-PS1-4.
. Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy.
Ions
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HS-PS3-5
Develop and use a model of two objects interacting through electric or magnetic fields to illustrate the forces between objects and the changes in energy of the objects due to the interaction. [
Naming Ions
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Drawing Lewis Ions
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Ionic Bonds
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Properties of Ionic Compounds
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Ionic Compound Names and Formulas
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Drawing Lewis Ionic Compounds
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Polyatomic Ions
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Names & Formulas with Polyatomic Ions
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2 weeksCovalent Bonds, Polarity, and Intermolecular ForcesHS-PS1-1Use 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 atomsForming covalent bondsasymmetrical
covalent bond
dipole
dipole-dipole attraction
double bond
electronegativity difference
hydrogen bond
intermolecular force (IMF)
molecular substance
molecule
molecule-ion attraction
polar
polarity
shared electron
single bond
SNAP rule
soluble
symmetrical
triple bond
unpaired electron
weak force
1. Recognize, understand, and use all vocabulary terms. 2. Use the density formula to calculate density, mass, or volume. 3. Use density to identify a substance. 4. Explain the particle nature of matter. 5. Identify the 4 types of particles that make up matter. 6. Classify matter as a substance or mixture. 7. Describe the properties of elements, compounds, and mixtures. 8. Identify the 7 diatomic elements. 9. Identify the states of matter and their properties. 10. Draw a particle diagram of each state. 11. Identify STP. 12. Identify and compare homogeneous and heterogeneous mixtures. 13. Explain how to separate parts of a mixture and identify specific separation techniques. 14. State or identify the three basic types of chemical formulas. 15. Reduce an empirical formula to its simplest form. 16. Identify a mixture and describe its properties. 17. Identify and contrast physical and chemical changes. 18. Determine when a chemical reaction has occurred. 19. Read a chemical equation. 20. State and apply the law of conservation.
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HS-PS1-3.Plan and conduct an investigation to gather evidence to compare the structure of substances at the bulk scale to infer the strength of electrical forces between particles.Properties of molecular substances
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HS-PS2-6Communicate scientific and technical information about why the particulate-level structure is important in the functioning of designed materials.*Naming molecular substances
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HS-PS3-5Develop and use a model of two objects interacting through electric or magnetic fields to illustrate the forces between objects and the changes in energy of the objects due to the interaction. [Drawing Lewis structures
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Bond Polarity
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Molecule polarity
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Intermolecular forces
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2 weeksSolutionsHS-PS1-10.UUse evidence to support claims regarding the formation, properties and behaviors of solutions at bulk scales.Defining/characterizing solutionsAlloy
Colligative property
Concentrated
Concentration
Dilute
Dissociation/dissociate
Insoluble
Miscible
Molarity
Parts per million (ppm)
Percent composition
Saturated
Soluble
Solubility Curve
Solute
Solution
Solvent
Supersaturated
Unsaturated		Know and use all vocabulary terms.
2. Identify the properties of a solution.
3. Identify the solute and solvent in a solution.
4. Explain how solubility is affected by chemical bonds, temperature, and pressure.
5. From a description, determine if a solution is saturated, unsaturated, or supersaturated.
6. Use the reference tables to determine if a solution is saturated, unsaturated, or
supersaturated.
7. Use the reference table to determine if a substance is soluble in water.
8. Calculate the concentration of a solution in molarity and ppm.
9. Describe the proper procedure for mixing a solution of a specific concentration.
10. Describe the effect of a solute on the freezing and boiling points of a liquid.
11. Determine which solute will have the greatest effect on the freezing and boiling points of
a liquid.
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HS-PS3-5Develop and use a model of two objects interacting through electric or magnetic fields to illustrate the forces between objects and the changes in energy of the objects due to the interaction. [Solubility
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Bonding and Solubility
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Factors affecting solubility
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Solubility Rules/Table F
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Saturation - defining
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Saturatation - Table G
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Concentration molariity
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concentration ppm
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colligative properties
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2 weeksChemical ReactionsHS-PS1-2Construct 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 propertiesDecribing chemical reactionsBalanced Equation Chemical Equation Chemical Reaction Decomposition Double Replacement Reaction Law of Conservation Product Reactant Single Replacement Reaction Synthesis Unbalanced EquationKnow and use all vocabulary terms. 2. Identify the reactants and products of a chemical reaction. 3. Identify what changes during a chemical reaction, and what is conserved. 4. Use coefficients in a chemical equation to determine the amounts (moles) of material involved in a given reaction. 5. Identify the ratio of substances involved in chemical reactions. 6. Use the ratios in a chemical equation to determine the quantities of any substance in that equation. 7. Be able to identify the four basic types of chemical reactions (synthesis, decomposition, single replacement, double replacement). 8. Identify whether an equation is balanced or unbalanced. 9. Balance an unbalanced equation. 10. Predict the products of a chemical reaction.Types of chemical reactions Lab, Unit test
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HS-PS1-4.. Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy.Chemical Equations
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HS-PS1-7. Use mathematical representations to support the claim that atoms, and therefore mass, are conserved during a chemical reactionBalancing Equations
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Types of Chemical Reactions
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Predicting Products (optional)
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1 WeekEnergyHS-PS1-4.
Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy.
Defining energyCelsius
Cooling Curve
Energy
Endothermic
Exothermic
Heat
Heat of Fusion
Heat of Reaction
Heat of Vaporization
Heating Curve
Joule
Kelvin
Specific Heat Capacity
Temperature		Know and use all vocabulary terms.
2. Identify different forms of energy.
3. State and apply the law of conservation of energy.
4. Describe the flow of energy in a system.
5. Describe the relationship between energy and temperature.
6. Distinguish the difference between heat and temperature.
7. Convert between Kelvin and Celsius temperature.
8. Correctly describe the nature of “cold”.
9. Use Table I to determine Heat of Reaction of an equation.
10. Identify endothermic and exothermic reactions.
11. Calculate the change in energy as a substance changes temperature.
12. Calculate the change in energy as a substance changes phase.
13. Use heating and cooling curves to identify and compare heat of fusion and heat of
vaporization.		hot packs/cold packs, mechanical toysHot packs/cold packs lab, Unit test
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HS-PS3-1.Create a computational model to calculate the change in the energy of one component in a system when
the change in energy of the other component(s) and energy flows in and out of the system are known		Types of energy
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HS-PS3-4Plan and conduct an investigation to provide evidence that the transfer of thermal energy when two components of different temperature are combined within a closed system results in a more uniform energy distribution among the components in the system (second law of thermodynamics). [Converting energy
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Measuring energy
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Temperature
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Energy and Chemical Changes
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q=mCAT
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Heat of Reaction/Table I
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Energy and Phase Change