Chemistry

Chemistry

Chemistry Curriculum Map

1st 9 Weeks

Week

Concept

Benchmarks

Activities

Assessments

1

Chapter 1: Introduction to Chemistry

Section 1.1: A Story of Two Substances

Standard/s:

Section 1.2: Chemistry and Matter

Define substance

Explain the formation and importance of ozone

Describe the development of chlorofluorocarbons

Compare and contrast mass and weight

Explain why chemists are interested in a submicroscopic description of matter

Identify the area of emphasis for various branches of chemistry

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2

Chapter 1: Introduction to Chemistry

Section 1.3: Scientific Methods

Section 1.4: Scientific Research

Identify the common steps of scientific methods

Compare and contrast types of data

Identify types of variables

Describe the difference between a theory and scientific law

Compare and contrast pure research, applied research, and technology

Apply knowledge of laboratory safety

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3

Chapter 2: Analyzing Data

Section 2.1: Units and Measurement

Section 2.2: Scientific Notation and Dimensional Analysis

Section 2.3: Uncertainty in Data

Define SI base units for time, length, mass, and temperature

Explain how adding a prefix changes a unit

Compare the derived units for volume and density

Express numbers in scientific notation

Convert between units using dimensional analysis

Define and compare accuracy and precision

Describe the accuracy of experimental data using error and percent error

Apply rules for significant figures to express uncertainty in measured and calculated values

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4

Chapter 2: Analyzing Data

Chapter 3: Matter-Properties and Changes

Section 2.4: Representing Data

Section 3.1: Properties of Matter

Standard/s: C.1.2

Section 3.2: Changes in Matter

Standard/s: C.1.3, C.1.4, C.1.6

Create graphs to reveal patterns in data

Interpret graphs

Identify the characteristics of a substance

Distinguish between physical and chemical properties

Differentiate among the physical states of matter

Define physical change and list several common physical changes

Define chemical change and list several indications that a chemical change has taken place

Apply the law of conservation of mass to chemical reactions

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5

Chapter 3: Matter-Properties and Changes

Section 3.3: Mixtures of Matter

Standard/s: C.1.1

Section 3.4: Elements and Compounds

Standard/s: C.2.5

Contrast mixtures and substances

Classify mixtures as homogeneous or heterogeneous

List and describe several techniques used to separate mixtures

Distinguish between elements and compounds

Describe the organization of elements in the periodic table

Explain how all compounds obey the laws of definite and multiple proportions

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6

Chapter 4: The Structure of the Atom

Section 4.1: Early Ideas About Matter

Standard/s: C.1.6, C.2.1, C.2.2

Section 4.2: Defining the Atom

Standard/s: C.2.2

Compare and contrast the atomic models of Democritus, Aristotle, and Dalton

Understand how Dalton's theory explains the conservation of mass

Define atom

Distinguish between the subatomic particles in terms of relative charge and mass

Describe the structure of the atom, including the locations of the subatomic particles

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7

Chapter 4: The Structure of the Atom

Section 4.3: How Atoms Differ

Standard/s: C.2.3, C.2.4

Section 4.4: Unstable Nuclei and Radioactive Decay

Standard/s: C.2.9

Explain the role of atomic number in determining the identity of an atom

Define an isotope

Explain why atomic masses are not whole numbers

Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number

Explain the relationship between unstable nuclei and radioactive decay

Characterize alpha, beta, and gamma radiation in terms of mass and charge

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8

Chapter 5: Electrons in Atoms

Section 5.1: Light and Quantized Energy

Section 5.2: Quantum Theory and the Atom

Compare the wave and particle natures of light

Define a quantum of energy, and explain how it is related to an energy change of matter

Contrast continuous electromagnetic spectra and atomic emission spectra

Compare the Bohr and quantum mechanical models of the atom

Explain the impact of de Broglie's wave-particle duality and the Heisenberg uncertainty principle on the current view of electrons in atoms

Identify the relationships among a hydrogen atom's energy levels, sublevels, and atomic orbitals

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9

Chapter 5: Electrons in Atoms

Section 5.3: Electron Configuration

Standard/s: C.2.5, C.2.6

Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron configurations using orbital diagrams and electron configuration notation

Define valence electrons, and draw electron-dot structures representing an atom's valence electrons

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2nd Nine Weeks

Daniel

Week

Concept

Benchmarks

Activities

Assessments

1

Chapter 6: The Periodic Table and Periodic Law

6.1: Development of the Modern Periodic Table

6.2: Classification of the Elements

Standard/s: C.2.5, C.2.6

Trace the development of the periodic table

Identify key features of the periodic table

Explain why elements in the same group have similar properties

Identify the four blocks of the periodic table based on their electron configuration

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Project

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2

Chapter 6: The Periodic Table and Periodic Law

Chapter 7: Ionic Compounds and Metals

6.3: Periodic Trends

Standard/s: C.2.5

7.1: Ion Formation

Standard/s: C.3.1, C.3.2

Compare period and group trends of several properties

Relate period and group trends in atomic radii to electron configuration

Define a chemical bond

Describe the formation of positive and negative ions

Relate ion formation to electron configuration

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3

Chapter 7: Ionic Compounds and Metals

7.2: Ionic Bonds and Ionic Compounds

Standard/s: C.3.1, C.3.2

7.3: Names and Formulas for Ionic Compounds

Standard/s: C.3.3, C.3.4

Describe the formation of ionic bonds and the structure of ionic compounds

Generalize about the strength of ionic bonds based on the physical properties of ionic compounds

Categorize ionic bond formation as exothermic or endothermic

Relate a formula unit of an ionic compound to its composition

Write formulas for ionic compounds and oxyanions

Apply naming conventions to ionic compounds and oxyanions

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Chemical Nomenclature

4

Chapter 7: Ionic Compounds and Metals

7.4: Metallic bonds and the Properties of Metals

Standard/s: C.3.5

Describe a metallic bond

Relate the electron sea model to the physical properties of metals

Define alloys, and categorize them into two basic types

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5

Chapter 8: Covalent Bonding

8.1: The Covalent Bond

Standard/s: C.2.6, C.3.1, C.3.2, C.3.5

8.2: Naming Molecules

Standard/s: C.3.3, C.3.4

Apply the octet rule to atoms that form covalent bonds

Describe the formation of single, double, and triple covalent bonds

Contrast sigma and pi bonds

Relate the strength of a covalent bond to its bond length and bond dissociation energy

Translate molecular formulas into binary molecuar compound names

Name acidic solutions

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6

Chapter 8: Covalent Bonding

8.3: Molecular Structures

Standard/s: C.3.3

8.4: Electronegativity and Polarity

Standard/s: C.3.5

List the basic steps used to draw Lewis structures

Explain why resonance occurs, and identify resonance structures

Identify three exceptions to the octet rule, and name molecules in which these exceptions occur

Describe how elecronegativity is used to determine bond type

Compare and contrast polar and nonpolar covalent bonds and polar and nonpolar molecules

Generalize about the characteristics of covalently bonded compounds

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7

Chapter 9: Chemical Reactions

9.1: Reactions and Equations

Standard/s: C.1.3, C.4.1, C.4.2

9.2: Classifying Chemical Reactions

Standard/s: C.4.1, C.4.5

Recognize evidence of chemical change

Represent chemical reactions with equations

Balance chemical equations

Classify chemical reactions

Identify the characteristics of different classes of chemical reactions

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8

Chapter 9: Chemical Reactions

9.3: Reactions in Aqueous Solutions

Standard/s: C.4.1, C.4.2

Describe aqueous solutions

Write complete ionic and net ionic equations for chemical reactions in aqueous solutions

Predict whether reactions in aqueous solutions will produce a precipitate, water, or a gas

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9

Finals

Includes all previous standards

Includes all previous benchmarks

Questions/Discussion

Review

Semester 1 final exam

3rd 9 Weeks

Week

Concept

Benchmarks

Activities

Assessments

1

Chapter 10: The Mole

10.1: Measuring Matter

Standard/s: C.4.3

10.2: Mass and the Mole

Standard/s: C.4.3

Explain how a mole is used to indirectly count the number of particles of matter

Relate the mole to a common everyday counting unit

Convert between moles and number of representative particles

Relate the mass of an atom to the mass of a mole of atoms

Convert between number of moles and the mass of an element

Convert between number of moles and number of atoms of an element

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2

Chapter 10: The Mole

10.3: Moles of Compounds

Standard/s: C.4.3

Recognize the mole relationships shown by a chemical formula

Calculate the molar mass of a compound

Convert between the number of moles and mass of a compound

Apply conversion factors to determine the number of atoms or ions in a known mass of a compound

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3

Chapter 10: The Mole

10.4: Empirical and Molecular Formulas

Standard/s: C.4.7

10.5: Formulas of Hydrates

Standard/s: C.4.7

Explain what is meant by the percent composition of a compound

Determine the empirical and molecular formulas for a compound from mass percent and actual mass data

Explain what a hydrate is and relate the name of the hydrate to its composition

Determine the formula of a hydrate from laboratory data

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4

Chapter 11: Stoichiometry

11.1: Defining Stoichiometry

Standard/s: C.4.2, C.4.3

11.2: Stoichiometric Calculations

Standard/s: C.4.2, C.4.3

Describe the types of relationships indicated by a balanced chemical equation

State the mole ratios from a balanced chemical equation

List the sequence of steps used in solving stoichiometric problems

Solve stoichiometric problems

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5

Chapter 11: Stoichiometry

11.3: Limiting Reactants

Standard/s: C.4.2, C.4.3

11.4: Percent Yield

Standard/s: C.4.2, C.4.3

Identify the limiting reactant in a chemical equation

Identify the excess reactant, and calculate the amount remaining after the reaction is complete

Calculate the mass of a product when the amounts of more than one reactant are given

Calculate the theoretical yield of a chemical reaction from data

Determine the percent yield for a chemical reaction

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6

Chapter 12: States of Matter

12.1: Gases

Standard/s: C.1.5, C.5.1

12.2: Forces of Attraction

Standard/s: C.3.1

Use the kinetic-molecular theory to explain the behavior of gases

Describe how mass affects the rates of diffusion and effusion

Explain how gas pressure is measured and calculate the partial pressure of gas

Describe intramolecular forces

Compare and contrast intramolecular forces

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7

Chapter 12: States of Matter

12.3: Liquids and Solids

12.4: Phase Changes

Standard/s: C.6.1, C.6.2, C.6.3

Contrast the arrangement of particles in liquids and solids

Describe the factors that affect viscosity

Explain how the unit cell and crystal lattice are related

Explain how the addition and removal of energy can cause a phase change

Interpret a phase diagram

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8

Chapter 13: Gases

13.1: The Gas Laws

Standard/s: C.5.3

13.2: The Ideal Gas Law

Standard/s: C.5.2, C.5.3

State the relationship among pressure, temperature, and volume of a constant amount of gas

Apply the gas laws to problems involving the pressure, temperature, and volume of a constant amount of gas

Relate number of particles and volume using Avogadro's principle

Relate the amount of gas present to its pressure, temperature, and volume using the ideal gas law

Compare the properties of real and ideal gases

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9

Chapter 13: Gases

13.3: Gas Stoichiometry

Standard/s: C.5.2, C.5.3

Determine volume ratios for gaseous reactants and products by using coefficients from chemical equations

Apply gas laws to calculate amounts of gaseous reactants and products in a chemical reaction

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4th Nine Weeks

Daniel

Week

Concept

Benchmarks

Activities

Assessments

1

Chapter 14: Mixtures and Solutions

14.1: Types of Mixtures

Standard/s: C.7.1,

Compare the properties of suspensions, colloids, and solutions

Identify types of colloids and types of solutions

Describe electrostatic forces in colloids

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2

Chapter 14: Mixtures and Solutions

 14.2 Solution Concentration

Standard/s: C.7.2, C.7.3

14.3: Factors Affecting Solvation

Standard/s: C.7.2

14.4: Colligative Properties of Solutions

Standard/s: C.7.1, C.7.5

 Descibe concentration using different units
 
Determine the concentrations of solutions
 
Calculate the molarity of a solution
 
Describe how intermolecular forces affect solvation

Define solubility

Understand what factors affect solubility

Describe colligative properties

Identify four colligative properties of solutions

Determine the boiling point 

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3

       

4

       

5

       

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7

   

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