M. Elizabeth 2011 - 2012
Chemistry
Grant Union High School
Chemistry
Grant Union High School
Major Course Topics
Unit 1 Introduction to Chemistry and Data Analysis Resources (August 12 - August 26)
Learning Rules and Tools of the Class and Laboratory
Textbook Exploration word Periodic Table pdf
SI Measurement pdf NIST Conversions pdf
Chapter 1 of your book includes the following topics:
What is Chemistry in the first place?
The Stories of Two Chemicals
Chemistry and Matter
Scientific Methods
Scientific Research
Georgia
Chapter 2 of your book includes the following topics:
Units of measurement
Scientific Notation and Dimensional Analysis
How reliable are measurements?
Representing Data.
Unit 1 Introduction to Chemistry and Data Analysis Resources (August 12 - August 26)
Learning Rules and Tools of the Class and Laboratory
Textbook Exploration word Periodic Table pdf
SI Measurement pdf NIST Conversions pdf
Chapter 1 of your book includes the following topics:
What is Chemistry in the first place?
The Stories of Two Chemicals
Chemistry and Matter
Scientific Methods
Scientific Research
Georgia
- Physical and Chemical Properties Movie Notes Worksheet Lab Data Sheet
Classification of Matter Movie Notes Practice
Separation of Mixtures Movie Notes Density Problems word Lab 1 2
Review pdf
Chapter 2 of your book includes the following topics:
Units of measurement
Scientific Notation and Dimensional Analysis
How reliable are measurements?
Representing Data.
- We will be discussing metric conversions using dimensional analysis. We will convert large and small numbers into and out of scientific
accuracy. We will learn when we can round numbers and when we cannot -- a concept called SIGNIFICANT FIGURES!!!
Unit 3: Electrons in Atoms and Period Table (September 21 - October 2)
Where exactly are these electrons? You will become a master of the elements of our Earth if you learn the Periodic Table trends and
what makes an atom reactive.
Although the Periodic Table is primarily organized by number of protons contained in an atom of an element. It is further organized
into groups and periods. There are several other relationships that can be drawn from the organization of the elements. This is known
as Periodic Law.
Chapter 5 - Electrons in Atoms - contains the following topics:
Light and Quantized Energy
Quantum Theory and the Atom
Electron Configurations
Chapter 6 - The Periodic Table and Periodic Law -is divided into the following topics:
Development of the Modern Periodic Table
Classification of the Elements
October 5 - October 9 2010 - Quarter EXAM
Practice Exam pdf Practice Exam 2 word District Review ppt word
Twin Rivers District Assessment December 16 - December 17 - Semester Final
Practice Exam pdf Practice Exam 2 word District Review 1 ppt word
Practice Questions Review word ppt with answers key District Review 2 ppt word
r
Chemistry CST Practice Test pdf
Chemistry CA Framework pdf
Laboratory Report Evaluation pdf
TRUSD Chemistry Pacing Guide pdf
Periodic Table
Math Handbook pdf
Chemistry CA Framework pdf
Laboratory Report Evaluation pdf
TRUSD Chemistry Pacing Guide pdf
Periodic Table
Math Handbook pdf
Spring Semester
Unit 6 - Gases, Acids and Bases, and Solutions
Chapter 13 (1/4/11 - 1/19/11) Gas Pressure and Phase Diagrams
Students know the random motion of molecules and their collisions with a surface create the observable pressure on that surface.
Students know the random motion of molecules explains the diffusion of gases.
Chapter 14 (1/20/11 - 2/14/11)
Students know how to apply the gas laws to relations between the pressure, temperature, and volume of any amount of an ideal gas or
any mixture of ideal gases.
Boyle's Law, Charles Law, Guy Lussac's Law, Combined Gas Law and Ideal Gas Law
Chapter 19 Acids and Bases (2/15/10 - 2/21/10)
Acids and bases are present in the soil of Earth, the foods you eat and the products you buy.
Remember amino acids that make up proteins crucial for your existence.
Compare aids and bases, define and calculate pH and pOH of aqueous solutions.
Explain how buffers work to resist changes in pH
Chapter 15 Solution (2/22 - 3/5)
Solutions are homogeneous mixtures of two or more substances. As a basis for understanding this concept:
Students know the definitions of solute and solvent.
Students know how to describe the dissolving process at the molecular level by using the concept of random molecular motion
Students know temperature, pressure, and surface area affect the dissolving process.
Students know how to calculate the concentration of a solute in terms of grams per
liter, molarity, parts per million, and percent composition.
Twin Rivers District Assessment March 8-12, 2011 - Midterm
North Carolina Practice Problems word New York Regents Practice Problems word
California Practice Problems pdf Standards Review Practice Problems word
Twin Rivers Midterm Review ppt You Gotta Know review word
Unit 6 - Gases, Acids and Bases, and Solutions
Chapter 13 (1/4/11 - 1/19/11) Gas Pressure and Phase Diagrams
Students know the random motion of molecules and their collisions with a surface create the observable pressure on that surface.
Students know the random motion of molecules explains the diffusion of gases.
Chapter 14 (1/20/11 - 2/14/11)
Students know how to apply the gas laws to relations between the pressure, temperature, and volume of any amount of an ideal gas or
any mixture of ideal gases.
Boyle's Law, Charles Law, Guy Lussac's Law, Combined Gas Law and Ideal Gas Law
Chapter 19 Acids and Bases (2/15/10 - 2/21/10)
Acids and bases are present in the soil of Earth, the foods you eat and the products you buy.
Remember amino acids that make up proteins crucial for your existence.
Compare aids and bases, define and calculate pH and pOH of aqueous solutions.
Explain how buffers work to resist changes in pH
Chapter 15 Solution (2/22 - 3/5)
Solutions are homogeneous mixtures of two or more substances. As a basis for understanding this concept:
Students know the definitions of solute and solvent.
Students know how to describe the dissolving process at the molecular level by using the concept of random molecular motion
Students know temperature, pressure, and surface area affect the dissolving process.
Students know how to calculate the concentration of a solute in terms of grams per
liter, molarity, parts per million, and percent composition.
Twin Rivers District Assessment March 8-12, 2011 - Midterm
North Carolina Practice Problems word New York Regents Practice Problems word
California Practice Problems pdf Standards Review Practice Problems word
Twin Rivers Midterm Review ppt You Gotta Know review word
Chapter 19 ppt
Movie Clip Anhydride
Movie Clip Ion Conductivity
Movie Clip Strong/Weak Acids
Movie Clip Salt Formation
Movie Clip Neutralization
Movie Clip Buffer
Movie Clip Titration
Movie Clip Anhydride
Movie Clip Ion Conductivity
Movie Clip Strong/Weak Acids
Movie Clip Salt Formation
Movie Clip Neutralization
Movie Clip Buffer
Movie Clip Titration
Handouts Unit 1
Scientific
Simpson Variable 1
Spongebob Controls
Density Lab
Plastics Calculation
Rounding Song mov
Unit Conversion Song mov
Sig Figs and Rounding 1
Sig Figs
Sig Figs and Algebra
Percent Composition word
Chemistry Math
Georgia Videos and Aids
Scientific Notation video
Metric Conversions video
Scientific
Simpson Variable 1
Spongebob Controls
Density Lab
Plastics Calculation
Rounding Song mov
Unit Conversion Song mov
Sig Figs and Rounding 1
Sig Figs
Sig Figs and Algebra
Percent Composition word
Chemistry Math
Georgia Videos and Aids
Scientific Notation video
Metric Conversions video
Mr Gulch Explains
NDT Technical
Tutorials
NDT Technical
Tutorials
Kinetic Theory & Gases SG word
Chapter 13 Kinetic Theory ppt
Chapter 13/14 States of Matter
ppt
Chapter 14 Gases ppt
Gases ppt
Ideal Gases ppt
Combined Laws ppt
Gases KMVPT ppt
Solid Liquid Gas pdf
Gas Law notes pdf
Phase Diagram pdf
Temperature Conversion
Practice word
Temp. Conversions Practice 2
pdf
Pressure Conversion Practice
word
Kinetic energy and Gas Law
notes word
Kinetic Energy Questions word
Boyle's Law Practice word
Charles' Law Practice word
Gas Temp Volume Graphing word
Combined Gas Law Practice word
Ideal Gas Law Practice word
Gases and Stoichometry word
Mixed Gas Laws word
States of Matter ppt
Kinetic Energy/Combined Gas
Laws ppt
Molarity Practice Problems word
Chapter 13 Kinetic Theory ppt
Chapter 13/14 States of Matter
ppt
Chapter 14 Gases ppt
Gases ppt
Ideal Gases ppt
Combined Laws ppt
Gases KMVPT ppt
Solid Liquid Gas pdf
Gas Law notes pdf
Phase Diagram pdf
Temperature Conversion
Practice word
Temp. Conversions Practice 2
Pressure Conversion Practice
word
Kinetic energy and Gas Law
notes word
Kinetic Energy Questions word
Boyle's Law Practice word
Charles' Law Practice word
Gas Temp Volume Graphing word
Combined Gas Law Practice word
Ideal Gas Law Practice word
Gases and Stoichometry word
Mixed Gas Laws word
States of Matter ppt
Kinetic Energy/Combined Gas
Laws ppt
Molarity Practice Problems word
Unit 7 - Thermodynamics, Equilibrium, and Reaction Rates
Thermodynamics (3/15-3/19)
Energy is exchanged or transformed in all chemical reactions and physical changes of matter.
CA Standards for mastery
7a. Temperature and heat flow are described in terms of the motion of molecules (or atoms).
Temperature is a measure of the average kinetic energy of molecular motion in a sample. Heat is energy
transferred from a sample at higher temperature to one at lower temperature. Often, heat is described as
flowing from the system to the surroundings or from the surroundings to the system. The system is defined
by its boundaries, and the surroundings are outside the boundaries, with “the universe” frequently
considered as the surroundings.
7. b. Chemical processes can either release (exothermic) or absorb (endothermic) thermal energy.
Endothermic processes absorb heat, and their equations can be written with heat as a reactant.
Exothermic processes release heat, and their equations can be written with heat as a product.
The net heat released to or absorbed from the surroundings comes from the making and breaking of
chemical bonds during a reaction: breaking a bond always requires energy and making a bond almost always
releases energy. The amount of energy per bond depends on the strength of the bond.
The potential energy of the reaction system may be plotted for the different reaction stages: reactants,
transition states, and products. This plot will show reactants at lower potential energy than products for an
endothermic reaction and reactants at higher potential energy than products for an exothermic reaction. A
higher energy transition state usually exists between the reactant and product energy states that affect
the reaction rate.
7. c. Energy is released when a material condenses or freezes and is absorbed when a material evaporates
or melts. Physical changes are accompanied by changes in internal energy. Changes of physical state either
absorb or release heat. Evaporation and melting require energy to overcome the bonds of attractions in the
corresponding liquid or solid state. Condensation and freezing release heat to the surroundings as internal
energy is reduced and bonds of attraction are formed
Reaction Rates (3/22-3/24)
8. Chemical reaction rates depend on factors that influence the frequency of collision of reactant molecules.
As a basis for understanding this concept:
a. the rate of reaction is the decrease in concentration of reactants or the increase in concentration of
products with time.
b. reaction rates depend on such factors as concentration, temperature, and pressure.
c. catalysts increases the reaction rate. A catalyst increases the rate of a chemical reaction without taking
part in the net reaction. A catalyst lowers the energy barrier between reactants and products by promoting
a more favorable pathway for the reaction. Surfaces often play important roles as catalysts for many
reactions. One reactant might be temporarily held on the surface of a catalyst. There the bonds of the
reactant may be weakened, allowing another substance to react with it more quickly. Living systems speed
up life-dependent reactions with biological catalysts called enzymes.
Chemical Equilibrium ( 3/25 - 3/26, 4/6-4/9)
Chemical equilibrium is a dynamic process that occurs when there is not changes in a product or reactant
concentration that undergo reversible reactions with several factors affecting equilibrium that must be
considered when writing expressions used to quantify a state of equilibrium. Changes in heat accompanying
chemical reactions and spontaneity of chemical reactions are key topics, along with physical states of
substances undergoing chemical reactions, for example gases respond to changes in pressure and volume.
Calculation of concentration and molarity for solutions, particularly for aqueous solutions and use of
exponents are needed to solve quantitative problems.
When a stress is applied to a chemical reaction in equilibrium, a shift will occur to partly relieve the stress.
Organic Chemistry
The bonding characteristics of carbon allow the formation of many different organic molecules of varied
sizes, shapes, and chemical properties and provide the biochemical basis of life.
As a basis for understanding this concept:
10a. Students know large molecules (polymers), such as proteins, nucleic acids, and starch, are formed by
repetitive combinations of simple subunits. Polymers as consisting of repetitive and systematic combinations
of smaller, simpler groups of atoms, including carbon. All polymeric molecules, including biological molecules,
such as proteins, nucleic acids, and starch, are made up of various unique combinations of a relatively small
number of chemically simple subunits. For example, starch is a polymer made from a large number of simple
sugar molecules joined together.
10. b. Carbon bonding results given carbon’s four bonding electrons and four vacancies available to form
bonds, allowing the formation of a large variety of structures ranging from simple hydrocarbons to complex
polymers and biological molecules. covalent bonds—single or multiple—with other carbon atoms and with
atoms of other elements. The compounds range from simple hydrocarbon molecules (e.g., methane and
ethane) to complex organic polymers and biological molecules (e.g., proteins) and include many manufactured
polymers used in daily life (e.g., polyester, nylon, and polyethylene).
10. c. Amino acids are the building blocks of proteins. Proteins are large single-stranded polymers often
made up of thousands of relatively small subunits called amino acids. The bond attaching two amino acids,
known as the peptide bond, is identical for any pair of amino acids. The chemical composition of the amino
acid itself varies. Variation in composition and ordering of amino acids gives protein molecules their unique
properties and shapes. These properties and shapes define the protein’s functions, many of which are
essential to the life of an organism. The blueprint for building the protein molecules is deoxyribonucleic
acid (DNA). Biotechnology is advancing rapidly as more is learned about DNA, amino acid sequences, and the
shapes and functions of proteins.
Thermodynamics (3/15-3/19)
Energy is exchanged or transformed in all chemical reactions and physical changes of matter.
CA Standards for mastery
7a. Temperature and heat flow are described in terms of the motion of molecules (or atoms).
Temperature is a measure of the average kinetic energy of molecular motion in a sample. Heat is energy
transferred from a sample at higher temperature to one at lower temperature. Often, heat is described as
flowing from the system to the surroundings or from the surroundings to the system. The system is defined
by its boundaries, and the surroundings are outside the boundaries, with “the universe” frequently
considered as the surroundings.
7. b. Chemical processes can either release (exothermic) or absorb (endothermic) thermal energy.
Endothermic processes absorb heat, and their equations can be written with heat as a reactant.
Exothermic processes release heat, and their equations can be written with heat as a product.
The net heat released to or absorbed from the surroundings comes from the making and breaking of
chemical bonds during a reaction: breaking a bond always requires energy and making a bond almost always
releases energy. The amount of energy per bond depends on the strength of the bond.
The potential energy of the reaction system may be plotted for the different reaction stages: reactants,
transition states, and products. This plot will show reactants at lower potential energy than products for an
endothermic reaction and reactants at higher potential energy than products for an exothermic reaction. A
higher energy transition state usually exists between the reactant and product energy states that affect
the reaction rate.
7. c. Energy is released when a material condenses or freezes and is absorbed when a material evaporates
or melts. Physical changes are accompanied by changes in internal energy. Changes of physical state either
absorb or release heat. Evaporation and melting require energy to overcome the bonds of attractions in the
corresponding liquid or solid state. Condensation and freezing release heat to the surroundings as internal
energy is reduced and bonds of attraction are formed
Reaction Rates (3/22-3/24)
8. Chemical reaction rates depend on factors that influence the frequency of collision of reactant molecules.
As a basis for understanding this concept:
a. the rate of reaction is the decrease in concentration of reactants or the increase in concentration of
products with time.
b. reaction rates depend on such factors as concentration, temperature, and pressure.
c. catalysts increases the reaction rate. A catalyst increases the rate of a chemical reaction without taking
part in the net reaction. A catalyst lowers the energy barrier between reactants and products by promoting
a more favorable pathway for the reaction. Surfaces often play important roles as catalysts for many
reactions. One reactant might be temporarily held on the surface of a catalyst. There the bonds of the
reactant may be weakened, allowing another substance to react with it more quickly. Living systems speed
up life-dependent reactions with biological catalysts called enzymes.
Chemical Equilibrium ( 3/25 - 3/26, 4/6-4/9)
Chemical equilibrium is a dynamic process that occurs when there is not changes in a product or reactant
concentration that undergo reversible reactions with several factors affecting equilibrium that must be
considered when writing expressions used to quantify a state of equilibrium. Changes in heat accompanying
chemical reactions and spontaneity of chemical reactions are key topics, along with physical states of
substances undergoing chemical reactions, for example gases respond to changes in pressure and volume.
Calculation of concentration and molarity for solutions, particularly for aqueous solutions and use of
exponents are needed to solve quantitative problems.
When a stress is applied to a chemical reaction in equilibrium, a shift will occur to partly relieve the stress.
Organic Chemistry
The bonding characteristics of carbon allow the formation of many different organic molecules of varied
sizes, shapes, and chemical properties and provide the biochemical basis of life.
As a basis for understanding this concept:
10a. Students know large molecules (polymers), such as proteins, nucleic acids, and starch, are formed by
repetitive combinations of simple subunits. Polymers as consisting of repetitive and systematic combinations
of smaller, simpler groups of atoms, including carbon. All polymeric molecules, including biological molecules,
such as proteins, nucleic acids, and starch, are made up of various unique combinations of a relatively small
number of chemically simple subunits. For example, starch is a polymer made from a large number of simple
sugar molecules joined together.
10. b. Carbon bonding results given carbon’s four bonding electrons and four vacancies available to form
bonds, allowing the formation of a large variety of structures ranging from simple hydrocarbons to complex
polymers and biological molecules. covalent bonds—single or multiple—with other carbon atoms and with
atoms of other elements. The compounds range from simple hydrocarbon molecules (e.g., methane and
ethane) to complex organic polymers and biological molecules (e.g., proteins) and include many manufactured
polymers used in daily life (e.g., polyester, nylon, and polyethylene).
10. c. Amino acids are the building blocks of proteins. Proteins are large single-stranded polymers often
made up of thousands of relatively small subunits called amino acids. The bond attaching two amino acids,
known as the peptide bond, is identical for any pair of amino acids. The chemical composition of the amino
acid itself varies. Variation in composition and ordering of amino acids gives protein molecules their unique
properties and shapes. These properties and shapes define the protein’s functions, many of which are
essential to the life of an organism. The blueprint for building the protein molecules is deoxyribonucleic
acid (DNA). Biotechnology is advancing rapidly as more is learned about DNA, amino acid sequences, and the
shapes and functions of proteins.
Reaction Rate Standard Notes word
Reaction Rate Video - Thank you
Georgia
Notes word
Reaction Rate Crossword word
Glencoe Ch 17 ppt
Reaction Rate ppt
Reaction Rate Video - Thank you
Georgia
Notes word
Reaction Rate Crossword word
Glencoe Ch 17 ppt
Reaction Rate ppt
An analogy can be made with
a pair of escalators operating
between two floors. If the
same number of people go up
as go down in a ten-minute
interval, the rate of people
moving up equals the rate of
people moving down. Overall,
any extra people arriving on
one floor are canceled out by
others leaving the floor.
Therefore, the number of
people on each floor will be
constant over time, and the
population of the two floors
is in dynamic equilibrium. This
analogy can be extended to a
chemical reaction by
considering that if the
number of moles produced in
one direction of the reaction
is the same as the number
consumed in the opposite
direction, then the reaction
has reached a state of
dynamic equilibrium.
a pair of escalators operating
between two floors. If the
same number of people go up
as go down in a ten-minute
interval, the rate of people
moving up equals the rate of
people moving down. Overall,
any extra people arriving on
one floor are canceled out by
others leaving the floor.
Therefore, the number of
people on each floor will be
constant over time, and the
population of the two floors
is in dynamic equilibrium. This
analogy can be extended to a
chemical reaction by
considering that if the
number of moles produced in
one direction of the reaction
is the same as the number
consumed in the opposite
direction, then the reaction
has reached a state of
dynamic equilibrium.
Equilibrium Notes word
Equilibrium Video -
Thank you Georgia
Notes Taking Guide pdf
Lab: Equilibrium Datasheet pdf
Lab: Le Chatelier’s Principle pdf
Calculating Keq pdf
Le Chatelier’s Principle pdf
Equilibrium Glencoe ppt
Equilibrium Video -
Thank you Georgia
Notes Taking Guide pdf
Lab: Equilibrium Datasheet pdf
Lab: Le Chatelier’s Principle pdf
Calculating Keq pdf
Le Chatelier’s Principle pdf
Equilibrium Glencoe ppt
Organic Chemistry Notes (word)
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