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MCSM Chemistry Curriculum Outline – Teacher Version
1. Course Overview: Chemistry is a full-year, two-term course concerning the fundamental
concepts of chemistry. Three themes are emphasized throughout the course.
 The Particulate Nature of Matter
 Changes of Matter
 The Interplay of Matter and Energy
The course will meet six periods each week; with the weekly double period as a dedicated
laboratory time.
2. Standards Connections: The scope and sequence of the curriculum is designed to meet the
requirement of the NYS Physical Setting: Chemistry Core Curriculum and to prepare student for
the NYS Physical Setting: Chemistry Regents Exam.
3. Laboratory: The 1200 minute laboratory seating requirement for the Regents Exam will be
met when a student submits 15 passing laboratory reports. The laboratory portion of the course is
designed to meet the Common Core Standards listed below.
 Follow precisely a complex multistep procedure when carrying out experiments,
taking measurements, or performing technical tasks, attending to special cases or
exceptions defined in the text.
 Determine the meaning of symbols, key terms, and other domain-specific words
and phrases as they are used in a specific scientific or technical context.

Translate quantitative or technical information expressed in words in a text into
visual form (e.g., a table or chart) and translate information expressed visually or
mathematically (e.g., in an equation) into words.
4. Textbook and Reference Tables: Each student will be issued one of the two textbooks listed
below for their use in the course. The textbook will be used primarily at home by the student for
independent study and homework. Each textbook covers all the topics included in the course
curriculum.
 Chemistry: Matter and Change, Glencoe
 Chemistry, Holt
Each student will also be issued a set of Chemistry Reference Tables for use in class, at home,
and on exams.
5. Grading: Throughout the year students produce work that allows the instructor to interpret
their achievement and understanding of the course material. Student grades for the course are
cumulative for each semester and will be calculated by the following rubric.
 60% Exams (6 to 8 per semester)
 20% Laboratory Reports (10 to 13 per semester)
 15% Homework Assignments (multiple times per week)
 5% Class participation
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6. Multiple Points of Entry / Differentiation of Instruction: While everyone in a Chemistry
course is held to the same high standard, there are different paths to understanding depending on
the individual student. Listed below are the ways in which those different paths to understanding
are facilitated.
 Graphic organizers, particle models, graphs, mathematical relationships, and
written descriptions will be used in both teaching of concepts and in student work.
 Daily objectives and activities will range from simple to complex, giving each
student something they can achieve every day, while still challenging all students.
 Heterogeneous ability groups will be employed both in class and in lab to
encourage peer to peer instruction, communication, and unofficial mentoring.
 After school tutoring and make-up labs will be offered to students in need of extra
help/time.
 ELL students will be given subject-specific dictionaries, a Chemistry review
book, extra time on all exams, and be paired with other bilingual students help
them overcome language barriers.
 Students with IEPs will be placed in a classroom with a co-teacher dedicated to
aiding those students in their success. These students will also be given a
Chemistry review book, extra exam time, and/or modified exams. Other
accommodations may be made depending on the specific IEP of the student.
 Advanced student will be offered enrichment projects throughout the year. A
menu of these projects is included in the syllabus.
7. Units of Instruction, Major Topics, and Laboratory: The organizational list below is
indicative of the scope and sequence of the Chemistry course. Each unit will encompass
approximately three weeks of class time and will culminate in a unit exam.
Unit 1: Matter and Energy
Major Topics:
 Atomic Nature of Matter / Conservation of Matter
 Mass, Volume, and Density
 Physical and Chemical Properties
 Physical and Chemical Change
 Elements, Compounds, and Mixtures
 Energy: Forms, Conversions, and Conservation
Laboratory Experiments
 Density of Water and Pennies
 Properties of Oxygen, Hydrogen, and Carbon Dioxide
 Conservation of Mass in Chemical Reactions
 Percent Composition of a Hydrated Compound
Enrichment Topic: History of Chemistry – Chemistry and Alchemy
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Unit 2: Atomic Structure
Major Topics:
 Atomic Theory Development (Dalton / Thomson / Rutherford)
 Sub-Atomic Particles (Masses / Charges / Locations)
 Isotopes and Atomic Mass
 Bohr Atom and Electron Energy Shells
 Spectral Line Production and Element Identification
 Electron Configurations, Ground and Excited States
 Modern Electron Model (Cloud / Quantum-Mechanical)
Laboratory Experiments
 “Pennium” Isotopes and Atomic Mass
 Flame Tests and Spectral Lines
Enrichment Topic: Electron Configurations and s, p, d, and f Orbitals
Unit 3: Periodic Table of Elements
Major Topics:
 Structure and Organization of Table
 Valence Electrons and Valence Energy Levels
 Ions and Ion Formation
 Atomic and Ionic Radii
 Ionization Energy
 Properties of Metals, Nonmetals, and Metalloids
 Properties of Elements by Group
Laboratory Experiments
 Properties and Reactions of Group 2 Metals and Ions
Enrichment Topic: Mendeleev and the History of the Periodic Table
Unit 4: Chemical Bonding
Major Topics:
 Energy of Bond Forming / Breaking
 Ionic Bond Formation
 Covalent Bond Formation
 Molecular Dot Diagrams
 Electronegativity and Bond Polarity
 Molecular Shape and Molecular Polarity
 Bonding, Structure, and Properties
Laboratory Experiments
 Three-Dimensional Molecular Modeling
Enrichment Topic: Molecular Resonance
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Unit 5: Phases of Matter
Major Topics:
 Kinetic Molecular Theory
 Heating and Cooling Curves
 Heat Calculations (q)
 Intermolecular Attractions
 Properties of Metallic, Ionic, and Molecular Solids
 Vapor Pressure and Boiling Point of Liquids
 Ideal Gas Behavior
 Combined Gas Law
Laboratory Experiments
 Heating Curve of Water
 Temperature and Volume of Air
Enrichment Topic: Ideal Gas Law
Unit 6: Chemical Formulas and Equations
Major Topics:
 Ionic Compounds – Formulas and Nomenclature
 Mole Concept
 Molar Mass
 Percent Composition of Compounds
 Empirical and Molecular Formulas
 Chemical Equation Interpretation
 Types of Chemical Equations
 Balancing Chemical Equations
 Mole to Mole Equation Stoichiometry
Laboratory Experiments
 Observing and Classifying Chemical Reactions
 Mass and Mole Relationships in a Chemical Reaction
Enrichment Topic: Mass to Mass Stoichiometry
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Unit 7: Solution Chemistry
Major Topics:
 Solution Composition and Formation
 Concentration – Molarity, Percent, and Parts Per Million
 Ionic and Molecular Solutes / Electrolyte Behavior
 Solubility of Ionic Compounds
 Solubility of Molecular Substances
 Solution Saturation
 Temperature, Pressure, and Solubility
 Solute Effect on Freezing and Boiling Point
 Solution Separation Techniques
Laboratory Experiments
 Solubility and Precipitation of Ionic Compounds
 Solubility and Temperature of Ammonium Chloride
Enrichment Topic: Ion Concentrations and Dilution
Unit 8: Acids and Bases
Major Topics:
 Arrhenius Acids and Bases
 Hydronium and Hydroxide Ion Concentrations
 pH Scale
 Indicators
 Neutralization Reactions
 Titration
 Alternate (H+ Exchange) Acid-Base Theory
Laboratory Experiments
 Acid-Base Indicators
 Acid-Base Titration
Enrichment Topic: Acid-Base Conjugate and Strength Relationships
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Unit 9: Kinetics, Thermodynamics, and Equilibrium
Major Topics:
 Collision Theory
 Conditions Affecting Collisions
 Activation Energy and Catalysts
 Temperature and Kinetic Energy
 Heat Transfer / Exothermic and Endothermic Change
 Heat of Reaction
 Entropy
 Equilibrium Characteristics
 Equilibrium in Physical and Chemical Systems
 Le Chatelier’s Principle – Concentration / Temperature / Pressure Effects
Laboratory Experiments
 Effect of Concentration and Temperature on Mg(s) and HCl(aq) Reaction
 Calorimetry and Heats of Reaction
 Le Chatelier’s Principle Investigation
Enrichment Topic: Industrial Ammonia Synthesis
Unit 10: Electrochemistry
Major Topics:
 Oxidation – Electrons and Charge
 Reduction – Electrons and Charge
 Oxidation States
 Oxidation-Reduction Reactions
 Half-Reactions
 Oxidation-Reduction Activity
 Voltaic Cells
 Electrolytic Cells
Laboratory Experiments
 Oxidation-Reduction Reaction and Activity
 Voltaic Cell Structure and Function
Enrichment Topic: Battery and Fuel Cell Structure
Unit 11: Organic Chemistry
Major Topics:
 Carbon Bonding
 Hydrocarbons
 Functional Groups
 Isomerism
 Organic Reactions
Laboratory Experiments
 Organic Molecular Modeling and Isomerism
Enrichment Topic: Structure and Function of Biologically Significant Molecules
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Unit 12: Nuclear Chemistry
Major Topics:
 Neutron to Proton Ratios in Isotopes
 Radioactive Decay
 Decay Kinetics / Half-Life
 Man-Made Transmutations
 Nuclear Fission
 Nuclear Fusion
 Mass-Energy Conversion
Laboratory Experiments
 Half-Life Simulation with Pennies
Enrichment Topic: Industrial Fission Reactors
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