Download Organic Chemistry Curriculum Map - Belle Vernon Area School District

Curriculum Map for Organic Chemistry
Course Understandings
Students will understand:
 Chemistry is the
study of matter
and the changes it
undergoes.



Atomic theory is
the foundation for
the study of
chemistry.
The nature of
science depends
on the ability to
conduct scientific
experiments with
reproducible
results.
Chemical bonding
occurs as a result
of attractive
forces between
particles.
Essential Questions

In what ways has
the theory of the
atom changed over
time due to
technological
improvements?
 What are the
differences between
pure substances and
mixtures?
 What factors
determine the types
of chemical bonds
that form between
particles?
Assessments


Formative Assessments –
 Students will be assessed using a
weekly quiz to check
understanding.
 Students will be informally
assessed using in class
assignments, homework, and
class activities.
 A posttest will be given at the
conclusion of each chapter to
assess comprehension and
analysis of concepts.


How does the
distribution of
electrons in atoms
affect the formation
of a compound?
First Quarter
Diagnostic –
Students’ prior knowledge will be
assessed through teacher
questioning.
Students’ prior knowledge will be
tested through homework
problems.
Summative Assessments –
Quarterly Exam #1 will be given
to assess student comprehension
and analysis.
Course Knowledge/Skills
Standard: 3.2.C.A1 – Differentiate between physical
properties and chemical properties
Anchor: CHEM.A.1.1 – Identify and describe how
observable and measureable properties can be used to
classify and describe matter and energy.
Eligible Content
 CHEM.A.1.1.2 – Classify observations as qualitative
and/or quantitative.
Standard: 3.2.C.A1 – Differentiate between pure substances
and mixtures; differentiate between heterogeneous and
homogeneous mixtures
Anchor: CHEM. A.1.2 – Compare the properties of mixtures
Eligible Content
 CHEM.A.1.2.1 – Compare properties of solutions
containing ionic or molecular solutes (e.g.,
dissolving, dissociating).
 CHEM.A.1.2.2 – Differentiate between
homogeneous and heterogeneous mixtures (e.g.,
how such mixtures can be separated).
 CHEM.A.1.2.3 – Describe how factors (e.g.,
temperature, concentration, surface area) can affect
solubility.
Anchor: CHEM. A.2.1 – Explain how atomic theory serves
as the basis for the study of matter
Eligible Content
 CHEM.A.2.1.1 – Describe the evolution of the 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.
Anchor: CHEM.B.1.2 – Apply the mole concept to the
composition of matter
Eligible Content
 CHEM.B.1.2.2 – Apply the law of definite
proportions to the classification of elements and
compounds as pure substances
Standard: 3.2.C.A4 – Predict how combinations of
substances can result in physical and/or chemical changes.
Anchor: CHEM.B.1.1 – Explain how the mole is a
fundamental unit of chemistry.
Eligible Content
 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).
Standard: 3.2.C.A5 – Models – Recognize discoveries from
Dalton (atomic theory), Thomson (the electron), Rutherford
(the nucleus), and Bohr (planetary model of the atom) and
understand how each discovery leads to modern theory.
Anchor: CHEM.A.1.1 Identify and describe how observable
and measurable properties can be used to classify and
describe matter and energy.
Eligible Content
 CHEM.A.1.1.1 – Classify physical or chemical
changes within a system in terms of matter and/or
energy.
Standard 3.2.C.A5 – Describe Rutherford’s “gold foil”
experiment that lead to the discovery of the nuclear atom.
Identify the major components (protons, neutrons, and
electrons) of the nuclear atom and explain how they
interact.
Anchor: CHEM.A.2.1 – Explain how atomic theory serves s
the basis for the study of matter.
Eligible Content
 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.
Standard: 3.2.C.A1 – Explain the relationship of an elements
position on the periodic table to its atomic number,
ionization energy, electro-negativity, atomic size, and
classification of elements.
Anchor: CHEM.A.2.1 – Explain how atomic theory serves as
the basis for the study of matter.
Eligible Content
 CHEM.A.2.1.2 – Differentiate between the mass
number of an isotope and the average atomic mass
of an element.
Anchor: CHEM.A.2.3 – Explain how periodic trends in the
properties of atoms allow for the prediction of physical and
chemical properties.
Eligible Content
 CHEM.A.2.3.2 – Explain how the periodicity of
chemical properties led to the arrangement of
elements on the periodic table.
Standard: 3.2.C.A1 – Use electro-negativity to explain the
difference between polar and non-polar covalent bonds.
Anchor: CHEM.B.2.3 – Explain how atoms form chemical
bonds.
Eligible Content
 CHEM.B.1.3.2 – Classify a bond as being polar
covalent, non-polar covalent, or ionic.
Standard: 3.2.C.A2 – Compare the electron configurations
for the first twenty elements of the periodic table.
Anchor: CHEM.A.2.2 – Describe the behavior of electrons
in atoms.
Eligible Content
 CHEM.A.2.2.1 – Predict the ground state electronic
configurations and/or orbital diagram for a given
atom or ion.
Standard: 3.2.C.A2 – Relate the position of an element on
the periodic table to its electron configuration and compare
its reactivity to the reactivity of other elements in the table.
Anchor: CHEM.A.2.2 – Describe the behavior of electrons
in atoms.
Eligible Content
 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.
Anchor: CHEM.A.2.2 – Describe the behavior of electrons
in atoms.
Eligible Content
 CHEM.A.2.2.4 – Relate the existence of quantized
energy levels to atomic emission spectra.
Standard: 3.2.C.A2 – Explain how atoms combine to form
compounds through both ionic and covalent bonding.
Anchor: CHEM.A.1.1 – Identify and describe how
observable and measureable properties can be used to
classify and describe matter and energy.
Eligible Content
 CHEM.A.1.1.4 – Relate the physical properties of
matter to its atomic or molecular structure.
Anchor: CHEM.B.1.3 – Explain how atoms for chemical
bonds.
Eligible Content
 CHEM.B.1.3.1 – Explain how atoms combine to form
compounds through ionic and covalent bonding.
Standard: 3.2.C.A2 – Predict chemical formulas based on the
number of valence electrons.
Anchor: CHEM.A.1.1 – Identify and describe how
observable and measureable properties can be used to
classify and describe matter and energy.
Eligible Content
 CHEM.A.1.1.5 – Apply systematic set of rules (IUPAC)
for naming compounds and writing chemical
formulas (e.g., binary covalent binary ionic, ionic
compounds containing polyatomic ions).
Standard: 3.2.C.A2 – Draw Lewis dot structures for simple
molecules and ionic compounds.
Anchor: CHEM.A.2.2 – Describe the behavior of electrons
in atoms.
Eligible Content
 CHEM.A.2.2.3 – Explain the relationship between
the electron configurations 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).
Anchor: CHEM.B.1.3 – Explain how atoms form chemical
bonds.
Eligible Content
 CHEM.B.1.3.3 – Use illustrations to predict the
polarity of a molecule.
Anchor: CHEM.B.1.4 – Explain how models can be used to
represent bonding.
Eligible Content
 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).
Eligible Content
 CHEM.B.1.4.2 – Utilize Lewis dot structures to
predict the structure and bonding in simple
compounds.
Students will understand:
 Periodic trends in
the properties of
atoms allow for
the prediction of
physical and
chemical
properties.

 What factors
identify the types of
chemical reactions?

How can materials
with the same
chemical
composition be so
different?
Chemical
reactions are
predictable.


Formative Assessments –


What is the role of
carbon in the
molecular diversity
of life?
Second Quarter
Diagnostic –
Students’ prior knowledge
will be assessed through
teacher questioning.
Students’ will be assessed
through homework
problems.

Students will be assessed
using a weekly quiz to check
understanding.
Students will be informally
assessed using in class
assignments, homework, and
class activities.
Standard: 3.2.C.A1 – Differentiate between pure substances
and mixtures; differentiate between heterogeneous and
homogeneous mixtures
Anchor: CHEM. A.1.2 – Compare the properties of mixtures
Eligible Content
 CHEM.A.1.2.1 – Compare properties of solutions
containing ionic or molecular solutes (e.g.,
dissolving, dissociating).
 CHEM.A.1.2.2 – Differentiate between
homogeneous and heterogeneous mixtures (e.g.,
how such mixtures can be separated).
 CHEM.A.1.2.3 – Describe how factors (e.g.,
temperature, concentration, surface area) can affect
solubility.
Anchor: CHEM. A.2.1 – Explain how atomic theory serves
as the basis for the study of matter
Eligible Content

A posttest will be given at
the conclusion of each
chapter
to
assess
comprehension and analysis
of concepts.
Summative Assessments –
 Quarterly Exam #2
will be given to assess
student
comprehension and
analysis.


CHEM.A.2.1.1 – Describe the evolution of the 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.
Standard: 3.2.C.A5 – Models – Recognize discoveries from
Dalton (atomic theory), Thomson (the electron), Rutherford
(the nucleus), and Bohr (planetary model of the atom) and
understand how each discovery leads to modern theory.
Anchor: CHEM.A.1.1 Identify and describe how observable
and measurable properties can be used to classify and
describe matter and energy.
Eligible Content
 CHEM.A.1.1.1 – Classify physical or chemical
changes within a system in terms of matter and/or
energy.
Standard: 3.2.C.A2 – Explain how atoms combine to form
compounds through both ionic and covalent bonding.
Anchor: CHEM.A.1.1 – Identify and describe how
observable and measureable properties can be used to
classify and describe matter and energy.
Eligible Content
 CHEM.A.1.1.4 – Relate the physical properties of
matter to its atomic or molecular structure.
Anchor: CHEM.B.1.3 – Explain how atoms for chemical
bonds.
Eligible Content
 CHEM.B.1.3.1 – Explain how atoms combine to form
compounds through ionic and covalent bonding.
Standard: 3.2.C.A2 – Draw Lewis dot structures for simple
molecules and ionic compounds.
Anchor: CHEM.A.2.2 – Describe the behavior of electrons
in atoms.
Eligible Content
 CHEM.A.2.2.3 – Explain the relationship between
the electron configurations 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).
Anchor: CHEM.B.1.3 – Explain how atoms form chemical
bonds.
Eligible Content
 CHEM.B.1.3.3 – Use illustrations to predict the
polarity of a molecule.
Anchor: CHEM.B.1.4 – Explain how models can be used to
represent bonding.
Eligible Content
 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).
Eligible Content
 CHEM.B.1.4.2 – Utilize Lewis dot structures to
predict the structure and bonding in simple
compounds.
Standard: 3.2.C.A4 – Interpret and apply the Laws of
Conservation of Mass, Constant Composition (Definite
Proportions), and Multiple Proportions.
Anchor: CHEM.B.1.2 – Apply the mole concept to the
composition of matter
Eligible Content
 CHEM.B.1.2.2 – Apply the law of definite
proportions to the classification of elements and
compounds as pure substances
Standard: 3.2.C.A4 – Classify chemical reactions as synthesis
(combination), decomposition, single displacement
(replacement), double displacement, and combustion.
Anchor: CHEM.B.2.1 – Predict what happens during a
chemical reaction.
Eligible Content:


 What factors
identify the types of
chemical reactions?
Students will understand:
 Chemical
reactions are
predictable.


Periodic trends in
the properties of
atoms allow for
the prediction of
physical and
chemical
properties.

How can materials
with the same
chemical
composition be so
different?
What is the role of
carbon in the
molecular diversity
of life?


Third Quarter
Diagnostic –
Students’ prior knowledge
will be assessed through
teacher questioning.
Students’ prior knowledge
will be tested through
homework problems.
Formative Assessments –
 Students will be assessed
using a weekly quiz to check
understanding.
 Students will be informally
assessed using in class
assignments, homework, and
class activities.
 A posttest will be given at
the conclusion of each
chapter to assess
comprehension and analysis
of concepts.
Summative Assessments –
 Quarterly Exam #3
will be given to assess
student
comprehension and
analysis.
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.
Standard: 3.2.C.A1 – Differentiate between pure substances
and mixtures; differentiate between heterogeneous and
homogeneous mixtures
Anchor: CHEM. A.1.2 – Compare the properties of mixtures
Eligible Content
 CHEM.A.1.2.1 – Compare properties of solutions
containing ionic or molecular solutes (e.g.,
dissolving, dissociating).
 CHEM.A.1.2.2 – Differentiate between
homogeneous and heterogeneous mixtures (e.g.,
how such mixtures can be separated).
 CHEM.A.1.2.3 – Describe how factors (e.g.,
temperature, concentration, surface area) can affect
solubility.
Anchor: CHEM. A.2.1 – Explain how atomic theory serves
as the basis for the study of matter
Eligible Content
 CHEM.A.2.1.1 – Describe the evolution of the 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.
Standard: 3.2.C.A5 – Models – Recognize discoveries from
Dalton (atomic theory), Thomson (the electron), Rutherford
(the nucleus), and Bohr (planetary model of the atom) and
understand how each discovery leads to modern theory.
Anchor: CHEM.A.1.1 Identify and describe how observable
and measurable properties can be used to classify and
describe matter and energy.
Eligible Content
 CHEM.A.1.1.1 – Classify physical or chemical
changes within a system in terms of matter and/or
energy.
Standard: 3.2.C.A2 – Explain how atoms combine to form
compounds through both ionic and covalent bonding.
Anchor: CHEM.A.1.1 – Identify and describe how
observable and measureable properties can be used to
classify and describe matter and energy.
Eligible Content
 CHEM.A.1.1.4 – Relate the physical properties of
matter to its atomic or molecular structure.
Anchor: CHEM.B.1.3 – Explain how atoms for chemical
bonds.
Eligible Content
 CHEM.B.1.3.1 – Explain how atoms combine to form
compounds through ionic and covalent bonding.
Standard: 3.2.C.A2 – Draw Lewis dot structures for simple
molecules and ionic compounds.
Anchor: CHEM.A.2.2 – Describe the behavior of electrons
in atoms.
Eligible Content
 CHEM.A.2.2.3 – Explain the relationship between
the electron configurations 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).
Anchor: CHEM.B.1.3 – Explain how atoms form chemical
bonds.
Eligible Content
 CHEM.B.1.3.3 – Use illustrations to predict the
polarity of a molecule.
Anchor: CHEM.B.1.4 – Explain how models can be used to
represent bonding.
Eligible Content
 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).
Eligible Content
 CHEM.B.1.4.2 – Utilize Lewis dot structures to
predict the structure and bonding in simple
compounds.
Standard: 3.2.C.A4 – Interpret and apply the Laws of
Conservation of Mass, Constant Composition (Definite
Proportions), and Multiple Proportions.
Anchor: CHEM.B.1.2 – Apply the mole concept to the
composition of matter
Eligible Content
 CHEM.B.1.2.2 – Apply the law of definite
proportions to the classification of elements and
compounds as pure substances
Standard: 3.2.C.A4 – Classify chemical reactions as synthesis
(combination), decomposition, single displacement
(replacement), double displacement, and combustion.
Anchor: CHEM.B.2.1 – Predict what happens during a
chemical reaction.
Eligible Content:
 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.
Students will understand:
 Chemical
reactions are

How are changes in
matter
accompanied by

Fourth Quarter
Diagnostic –
Lab concepts will be assessed
while applying content skills.
Standard: 3.2.C.A1 – Differentiate between pure substances
and mixtures; differentiate between heterogeneous and
homogeneous mixtures
predictable.
changes in energy?


What is the role of
carbon in the
molecular diversity
of life?
How do structures
of biologically
important
molecules (e.g.,
carbohydrates,
lipids, proteins,
nucleic acids)
account for their
functions?
 How might
advances in science
and technology
affect society?


Students’ prior knowledge will be
assessed through teacher
questioning.
Students’ prior knowledge will be
tested through homework
problems.
Formative Assessments –
Students will be assessed using a
weekly quiz to check
understanding.
•
Students will be informally
assessed using in class assignments,
homework, and class activities.
•
A posttest will be given at the
conclusion of each chapter to assess
comprehension and analysis of concepts.


Summative Assessments –
Quarterly Exam #4 will be given
to assess student comprehension
and analysis.
Anchor: CHEM. A.1.2 – Compare the properties of mixtures
Eligible Content
 CHEM.A.1.2.1 – Compare properties of solutions
containing ionic or molecular solutes (e.g.,
dissolving, dissociating).
 CHEM.A.1.2.2 – Differentiate between
homogeneous and heterogeneous mixtures (e.g.,
how such mixtures can be separated).
 CHEM.A.1.2.3 – Describe how factors (e.g.,
temperature, concentration, surface area) can affect
solubility.
Anchor: CHEM. A.2.1 – Explain how atomic theory serves
as the basis for the study of matter
Eligible Content
 CHEM.A.2.1.1 – Describe the evolution of the 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.
Standard: 3.2.C.A5 – Models – Recognize discoveries from
Dalton (atomic theory), Thomson (the electron), Rutherford
(the nucleus), and Bohr (planetary model of the atom) and
understand how each discovery leads to modern theory.
Anchor: CHEM.A.1.1 Identify and describe how observable
and measurable properties can be used to classify and
describe matter and energy.
Eligible Content
 CHEM.A.1.1.1 – Classify physical or chemical
changes within a system in terms of matter and/or
energy.
Standard: 3.2.C.A2 – Explain how atoms combine to form
compounds through both ionic and covalent bonding.
Anchor: CHEM.A.1.1 – Identify and describe how
observable and measureable properties can be used to
classify and describe matter and energy.
Eligible Content
 CHEM.A.1.1.4 – Relate the physical properties of
matter to its atomic or molecular structure.
Anchor: CHEM.B.1.3 – Explain how atoms for chemical
bonds.
Eligible Content
 CHEM.B.1.3.1 – Explain how atoms combine to form
compounds through ionic and covalent bonding.
Standard: 3.2.C.A2 – Draw Lewis dot structures for simple
molecules and ionic compounds.
Anchor: CHEM.A.2.2 – Describe the behavior of electrons
in atoms.
Eligible Content
 CHEM.A.2.2.3 – Explain the relationship between
the electron configurations 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).
Anchor: CHEM.B.1.3 – Explain how atoms form chemical
bonds.
Eligible Content
 CHEM.B.1.3.3 – Use illustrations to predict the
polarity of a molecule.
Anchor: CHEM.B.1.4 – Explain how models can be used to
represent bonding.
Eligible Content
 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).
Eligible Content
 CHEM.B.1.4.2 – Utilize Lewis dot structures to
predict the structure and bonding in simple
compounds.
Standard: 3.2.C.A4 – Interpret and apply the Laws of
Conservation of Mass, Constant Composition (Definite
Proportions), and Multiple Proportions.
Anchor: CHEM.B.1.2 – Apply the mole concept to the
composition of matter
Eligible Content
 CHEM.B.1.2.2 – Apply the law of definite
proportions to the classification of elements and
compounds as pure substances
Standard: 3.2.C.A4 – Classify chemical reactions as synthesis
(combination), decomposition, single displacement
(replacement), double displacement, and combustion.
Anchor: CHEM.B.2.1 – Predict what happens during a
chemical reaction.
Eligible Content:
 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.