Download Department: Science Course Number and Title: 523 (CP) and 518

Department: Science
Course Number and Title: 523 (CP) and 518 (H) Chemistry 1
Course Description
This course covers the most frequent theories of the nature of matter and its interaction. Major
emphasis will be on chemical interactions from both a descriptive and mathematical approach.
The student will derive conclusions from laboratory experiments and solving problems.
MHS Learning Expectations:
• Demonstrate the ability to problem solve effectively.
Essential Questions:
How does chemistry impact society?
How can we use the properties of matter and elements to help us to understand the
interactions of matter?
How do matter and energy cycle in our world?
Students will know:
Students will be able to:
• Physical and chemical properties
• Classify and describe matter using
reflect the nature of the interactions
physical and chemical properties
between molecules or atoms, and
that reflect the nature of the
can be used to classify and describe
interactions between molecules or
matter.
atoms.
• Atomic models are used to explain
• Use atomic models to explain
atoms and help us understand the
atoms and describe the interaction
interaction of elements and
of elements and compounds.
compounds observed on a
• Write the electron configurations
macroscopic scale. Nuclear
for the first twenty elements of the
chemistry deals with radioactivity,
periodic table.
nuclear processes, and nuclear
• Describe the relationship between
properties. Nuclear reactions
nuclear reactions and energy.
produce tremendous amounts of
Relate the law of conservation of
energy and lead to the formation of
mass to nuclear reactions.
elements.
• Identify the three main types of
• Repeating (periodic) patterns of
radioactive decay (alpha, beta, and
physical and chemical properties
gamma) and compare their
occur among elements that define
properties (composition, mass,
families with similar properties. The
charge, and penetrating power).
periodic table displays the repeating
• Describe the process of radioactive
patterns, which are related to the
decay by using nuclear equations,
atoms’ outermost electrons.
and explain the concept of half-life
• Atoms bond with each other by
for an isotope
transferring or sharing valence
• Describe and explain the periodic
electrons to form compounds.
patterns of physical and chemical
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In a chemical reaction, one or more
reactants are transformed into one
or more new products. Chemical
equations represent the reaction
and must be balanced. The
conservation of atoms in a chemical
reaction leads to the ability to
calculate the amount of products
formed and reactants used
(stoichiometry).
Gas particles move independently of
each other and are far apart. The
behavior of gas particles can be
modeled by the kinetic molecular
theory. In liquids and solids, unlike
gases, particles are close to each
other. The driving forces of chemical
reactions are energy and entropy.
The reorganization of atoms in
chemical reactions results in the
release or absorption of heat
energy.
Solids, liquids, and gases dissolve
to form solutions. Rates of reaction
and chemical equilibrium are
dynamic processes that are
significant in many systems (e.g.,
biological, ecological, geological).
Acids and bases are important in
numerous chemical processes that
occur around us, from industrial
procedures to biological ones, from
the laboratory to the environment.
Oxidation-reduction reactions occur
when one substance transfers
electrons to another substance, and
constitute a major class of chemical
reactions.
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properties that occur among
elements.
Describe the process of the
bonding including ionic, polar
covalent, nonpolar covalent, and
hydrogen bonding. Use this
knowledge to construct formulas
and models of the compounds
created.
Understand the process of
chemical reactions and relate the
law of conservation of mass to
balancing equations.
Predict the products of chemical
reactions and perform calculations
that relate to these chemical
reactions.
Determine percent compositions,
empirical formulas, and molecular
formulas.
Calculate the mass-to-mass
stoichiometry for a chemical
reaction.
Calculate percent yield in a
chemical reaction.
Describe the different states of
matter and use the Kinetic
Molecular Theory to explain the
behaviors of gases.
Explain the importance of energy
and entropy in chemical reactions.
Describe the formation and
components of solutions.
Calculate concentration in terms of
molarity. Use molarity to perform
solution dilution and solution
stoichiometry.
Identify and explain the factors that
affect the rate of dissolving (e.g.,
temperature, concentration,
surface area, pressure, mixing).
Compare and contrast qualitatively
the properties of solutions and
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pure solvents (colligative
properties such as boiling point
and freezing point).
Identify the factors that affect the
rate of a chemical reaction
(temperature, mixing,
concentration, particle size,
surface area, catalyst).
Predict the shift in equilibrium
when a system is subjected to a
stress (LeChatelier’s principle) and
identify the factors that can cause
a shift in equilibrium
(concentration, pressure, volume,
temperature).
Relate the rates of reaction and
chemical equilibrium to biological,
ecological, and geological
systems.
Identify and explain acid -base and
oxidation-reduction reactions.
Course Outline
Semester One
Semester Two
Lab Techniques, Lab Safety,
Measurements and Significant Figures
Chemical Reactions continued
Introduction to Matter and the Periodic
Table of Elements
Mole Conversions
Atomic Structure
Percent Composition by Mass and
Empirical/Molecular Formula
Nuclear Chemistry
Stoichiometry
Ionic Compounds
Thermochemistry
Covalent Compounds and VSEPR
Kinetic Molecular Theory and Gas Laws
Metals
Mixtures, Solutions and Molarity
Chemical Reactions
Equilibrium and Acids/Bases
Primary Course Materials
Textbook: Matter and Change (2013) will be provided to each student. In addition, you will
have access to an electronic textbook for your use online. You will be given a username and
password to access the text online.
Additional Materials: laboratory activities, computer simulations, scientific articles, teachercreated projects, and extensions to college level content
Grade Determination:
Quarterly grades will be based on:
Tests
Quizzes
Projects and labs
Homework and class work
50 %
20
20
10
Major Assignments: 4 Formal Lab Reports and 4 Core Assignments, Midyear and final exam,
each containing an Open Response. These assignments are given in common for all students
taking chemistry.
Midyear and Final Exams Midyear and Final Exams will be given. These exams count as 10%
of the respective semester grade. The average of the first and second quarter grades will count
90% in determining the first semester average. Similarly, the second semester average will
include the average of third and fourth quarter grades at 90% and the final exam at 10%. The
average for the entire year will be the average of both semesters.
Q1 = 22.5% Q2 = 22.5% Midterm = 5% Q3 = 22.5% Q4 = 22.5% Final = 5%