Kendall/Hunt Chemistry
This text:
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Student Responses (from anonymous end of trial surveys)
Color, Wrap-Around Teacher's Edition contains the following:
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Section 3.5—gas behavior
Section 4.2—Atomic Structure
Section 4.5—Periodicity
Section 4.6—Light
Section 4.7—Light & Matter
Section 8.5—Environmental Concerns
Section 10.3—Batteries
Chapter 11—Polymers
Chapter 12
Resources from University of Colorado Physics Education Technology (PhET)
What effects have the text had on students using it?
Students (regular HS general chemistry) were given pre/post surveys with 15 questions. The effect of using Chemistry You Need to Know compared to traditional chemistry texts was analyzed. Effect size is the difference of the averages divided by the average of the standard deviation. It's a way that behavioral scientists judge what a "practical" or important effect is.
An effect size smaller than 0.2 is considered minimal
0.5 is considered moderate
0.8 is considered a large effect.
As you can see 9 out of the 15 questions showed a large positive effect of the use of Chemistry You Need to Know and another 4 questions showed a moderate effect. There were NO questions for which the traditional effect had any positive effect at all!
Effect size—the larger the number, the greater the positive benefit of using Chemistry You Need to Know.
| 1.26 | I’m interested in chemistry |
| 1.24 | I was able to read and understand this book |
| 1.22 | I like science classes |
| 1.175 | This chemistry book applied chemistry to my life |
| 1.16 | I can see how different science concepts relate to each other (it’s not just random facts/information) |
| 1.11 | I feel comfortable “doing science” |
| 1.04 | I feel chemistry is relevant to my life |
| 0.96 | I’m comfortable learning/talking about chemistry |
| 0.88 | I enjoy labs |
| 0.78 | I feel science is relevant to my life |
| 0.74 | In this classes, I feel like I have “done science” |
| 0.69 | I understand what “chemistry” is about |
| 0.597 | I feel comfortable using math in science class |
| 0.23 | I enjoy writing my own procedures for labs (designing them myself) |
| 0.17 | I learn better if concepts are applied to my life |
Chapter
1—Scientists’ Tools
Scientific
processes
Variables
and constants
Predictions
and hypothesis
Writing
procedures
Gathering
data
Drawing
conclusions
Section
1.2—Observations and Measurements
Taking
Observations
Gathering
data
Uncertainty
in measurement
Lab
1.2--Measurements
Section
1.3—Designing your own labs
Lab 1.3 (student designed)--The most absorbent paper towel
Section
1.4—Converting units
Dimensional
analysis
Metric
conversions
Converting
with multiple steps
Section
1.5—Significant digits
Performing
calculations with significant digits
Section
1.6—Scientific Notation
Chapter
1 Summary
Chapter
1 Review
Chapter
2—Antacids
Section
2.1—Types of matter
Classifying
Pure substances
Classifying
Mixtures
Section
2.2—Naming chemicals
Writing
Ionic Compounds names
Writing
Molecular compound names
Writing
element names
Section
2.3—Writing chemical formulas
Writing
ionic compound formulas
Writing
Diatomic element formulas
Section
2.4—Defining, naming and writing acids and bases
Naming
acids
Writing
acid formulas
Writing
and naming bases
Section
2.5: Characteristics of acids and bases, and the pH scale
Strength
versus concentration of acids and bases
PH
scale
Measuring
pH
Lab
2.5--Acids and bases
Section
2.6—Chemical Equations
Parts
of a chemical equation
Double
replacement and neutralization reactions
Section
2.7—Balancing chemical reactions
Lab 2.7--Mass during a chemical reaction
Law
of conservation of mass/matter
Balancing
chemical equations
Section
2.8—Speeding up a reaction
Lab 2.8 (student designed)--Speeding up a reaction
Collision
theory
Catalysts
speed up reactions
Final
Chapter 2 Project (Student designed)—Finding the most effective
antacid
Chapter
2 Summary
Chapter
2 Review
Chapter
3—Airbags
Section
3.1—States of Matter
Properties
of three states of matter
Changes
in state
Section
3.2—Properties of matter
Physical
and chemical properties
Intensive
and Extensive Properties
Section
3.3—Density
Lab 3.3 (student designed)--Density
Section
3.4—Changes in matter
Physical
changes
Chemical
changes
Common
misconceptions concerning changes
Lab
3.4--Chemical changes
Section
3.5—Gas behavior
Gases
exert Pressure
Changes
in the gases result in changes in the pressure
Kinetic
Molecular Theory
Real
versus Ideal gases
Section
3.6—Counting atoms and molecules
The
mole
Atomic
and molecular masses
Molecular
mass is used to convert between moles and grams
Section
3.7—Gas Laws
Lab 3.7--Gas Laws
Converting
units of pressure
Avogadro’s
gas law
Charles’
Gas Law
Boyles’
Gas Law
Combined
gas Law
Ideal
gas law
Choosing
the appropriate law
Standard
Temperature and Pressure
Final
Chapter 3 Project—Evaluating methods of
producing a gas
Chapter
3 Summary
Chapter
3 Review
Chapter
4—Light and color
Section
4.1—Development of atomic theory
Discovering
the fundamental particles of the atom
Refining
the atomic theory further
Modern
atomic theory
Section
4.2—Atomic structure
Protons
in the atom
Mass
number and Neutrons in the atom
Charges
on atoms and electrons
Isotopes—atoms
of the same element can be different
Lab
4.2--Average atomic mass
Section
4.3—Electron structure
Electron
levels, subshells and orbitals
Showing
electron configurations
Section
4.4—Periodic table
Lab 4.4 (student designed)--Table of elements
The
modern periodic table
Electron
configurations and the periodic table
Periodic
table as a map for electron configurations
Section
4.5—Periodicity
Lab 4.5--Graphing periodic trends
Periodicity—Atomic
radius
Periodicity—Ionization
energy
Periodicity—Electron
affinity
Ion
radius
Section
4.6—Light
Wave
Properties
Energies
and colors of visible light
Section
4.7—Light and matter
Light
interaction with matter
Quantization
of photons and absorption by electrons
Measuring
light’s interaction with matter
Ways
of producing light
Lab
4.7 (student designed)--Glow sticks and temperature
Final
Chapter 4 Project—Writing project on
“Glowing” things
Chapter
4 Summary
Chapter
4 Review
Chapter
5—Soap
Section
5.1—Types of bonding
Bonding
between metals and non-metals
Bonding
between non-metals
Bonding
between metals
Characteristics
of different types of bonds
Melting
and boiling points.
Solubility
in water.
Conductivity
of electricity
Lab
5.1 (student designed)--types of bonds
Section
5.2—Drawing molecules
Determining
valence electrons
Placing
the electrons around the symbol
Lewis
Dot structures for ionic compounds
Balancing
ion charges
Lewis
Structures for Covalent compounds
Single
bonds
Arranging
atoms and forming bonds
Lone
pairs
Double
bonds
Triple
bonds
Lewis
structures that can be written more than one way
Lewis
Dot structures for polyatomic ions
Exceptions
to the octet rule
Section
5.3—How compounds arrange themselves in 3D
Lab 5.3--Covalent Molecules in 3D
Geometry
of Covalent bonding
Distortion
of angles with lone pairs
Ionic
compound structures
Section
5.4—Polarity of molecules
Electronegativity
and the periodic table
Electronegativity
and polarity of bonds
Polarity
of bonds and polarity of molecules
Section
5.5—Intermolecular forces
Intramolecular
versus Intermolecular forces
Dipole-dipole
interactions
Hydrogen
bonding
Section
5.6—Effects of intermolecular forces on properties of compounds
Melting,
Evaporating and boiling
Importance
of water’s intermolecular forces to life
Viscosity
Solubility
Oil
and water
Surface
tension
How
Soap’s affects solubility
Affect
of soap on surface tension
Lab
5.6--Intermolecular forces
Final
Chapter 5 Project—Making and evaluating soap
Chapter
5 Summary
Chapter
5 Review
Chapter
6—Sports Drinks
Section
6.1—Solutions and electrolytes
How
ionic compounds dissolve in water
Misconception
about dissolving
Forming
electrolytes in water
Clarification
of terms
Lab
6.1 (student designed)--Solution saturation and temperature
Making
a solution
Section
6.2—Concentrations of solutions
Percent
concentration
Molarity
concentration
Converting
between %(W/V) and molarity
Concentration
of electrolytes
Lab
6.2 (student designed)--Concentrations of solutions
Section
6.3—Acidity of solutions, pH
Calculating
pH from concentration of hydronium
Strength
of acids and pH
Solving
for concentration of hydronium
Bases
Acids
and bases are electrolytes
Autonization
of water
Section
6.4—Solubility and precipitations
Precipitation
reactions
Solubility
of ionic compounds
Lab
6.4--Solubility and precipitations
Solubility
rules
Section
6.5—Stoichiometry
Mole
ratio in a balanced chemical reaction
Molecular
mass and finding moles for stoichiometry
Molarity
and finding moles for stoichiometry.
Combining
molecular mass and molarity in stoichimetry
problems
Stoichiometry
with gases
Titrations
Lab
6.5A--Stoichiometry--titration
Lab
6.5B--Stoichiometry--gravimetric
Section
6.6—Limiting reactants
Limiting
and excess reactants
Lab
6.6--Limiting reactants
Section
6.7—Properties of solutions
Lab 6.7--Properties of solutions
Vapor
pressure
Vapor
pressure of a solution
Effects
of electrolyte versus a non-electrolyte
solutes
Boiling
point of a solution
Freezing
point of a solution
Final
Chapter 6 Project—Creating a carbonated
beverage with stoichiometry
Chapter
6 Summary
Chapter
6 Review
Chapter
7—Hot and Cold Packs
Section
7.1—Endothermic and Exothermic
System
versus surroundings
Endothermic
processes
Exothermic
processes
Section
7.2—Calorimetry and heat capacity
Heat,
energy and enthalpy
Units
for measuring energy
Heat
capacity
Using
heat capacity in calculations
Calorimetry
Lab
7.2--Calorimetry and heat capacity
Section
7.3—Changes in state
Temperature
doesn’t change during change in state
Enthalpy
changes during change in state
Melting
and freezing
Boiling
and condensation
Heating
curves—adding energy to a substance
Heating
curves—removing energy from a substance
Lab
7.3 (students designed)--Enthalpy changes during changes in state
Section
7.4—Enthalpy of chemical reaction
Enthalpy
of formation
Enthalpy
of reaction
Taking
into account the number of moles of the compound in the reaction
Enthalpy
and stoichiometry
Lab
7.4--Enthalpy of a chemical reaction
Section
7.5—Hess’s Law
Steps
for completing a Hess’s Law problem
Final
Chapter 7 Project—Making a hot or cold pack
Chapter
7 Summary
Chapter
7 Review
Chapter
8—Chemistry in Industry
Section
8.1—Equilibrium
Reversible
reactions
Establishing
equilibrium
Dynamic
Equilibrium
Determining
if a system is at equilibrium
Section
8.2—Equilibrium constants
Writing
equilibrium constant expressions
Not
all reactants and products are included in the Equilibrium constant
expression
Aqueous
solutions and gases
Pure
solids
Pure
liquids
Using
equilibrium constant expressions in calculations
Meaning
of an equilibrium constant
Equilibrium
constants and temperature
Lab
8.2--Equilibrium constants
Section
8.3—Reaction quotients
Reaction
quotient
Which
way to go to get to equilibrium
Section
8.4—Le Chatelier’s Principle
Le
Chatelier’s Principle
Effect
of changing concentrations
Adding
more reactant or products (increasing concentration)
Removing
reactants or products (decreasing concentration)
Effect
of changing in volume (changes in pressure)
Increasing
the volume
Decreasing
the volume
When
changes in volume have no effect
Effect
of changing temperature
In
an endothermic reaction
In
an exothermic reaction
When
changes don’t disturb the equilibrium
Speeding
up the time it takes to reach equilibrium
Lab
8.4--Le Chatelier's Principle
Section
8.5—Environmental concerns
Earth
Waste
Renewable
and non-renewable resources
Water
Air
Ozone
Greenhouse
gases and global warming
Your
job
Final
Chapter 8 Project (Student designed)—Determining if a reaction is endo
or exothermic
Chapter
8 Summary
Chapter
8 Review
Chapter
9—Forensic chemistry
Section
9.1—Analysis with solubility
What
things will dissolve in water?
Dissolving
a substance and equilibrium
Writing
equations and equilibrium constant expression for dissolving a substance
Lab
9.1A--Finding Ksp for a compound
Determining
if a substance will precipitate out
Precipitation
reactions
Using
solubility information for analysis of a sample
Qualitative
and quantitative analysis
Lab
9.1B--Analysis with solubility
Section
9.2—Analysis with chromatography
Paper
chromatography
Thin
Layer Chromatography
Liquid
Chromatography
Gas
chromatography
Lab
9.2--Analysis of marker ink with chromatography
Section
9.3—Analysis of a chemical formula
Percent
composition
Empirical
formulas
Molecular
formulas
Lab
9.3A--Empirical formula
Hydrates
Hydrate
formulas
Lab
9.3B (student designed)--hydrate formulas
Final
Chapter 9 Project—Writing project on
forensic science
Chapter
9 Summary
Chapter
9 Review
Chapter
10—Batteries
Section
10.1—Oxidation and reduction
Defining
reduction and oxidation
Reduction
and Oxidation happen simultaneously
Determining
Oxidation number
Identifying
what’s being reduced or oxidized in a reaction
Oxidizing
agent and reducing agent
Section
10.2—Redox reactions
Single
replacement reactions
Lab
10.2--Developing an activity series
Activity
series
Balance
redox reactions
Writing
half reactions
Balancing
redox reactions in an acidic solution
Balancing
redox reactions in a basic solution
Section
10.3—Electricity and redox reactions
Voltaic
cells
Line
notation
Lab
10.3 (student designed)--Making a battery
Calculating
cell potential
Standard
Reduction potentials
Cell
potential
Standard
reduction potential is an intensive property
Non-standard
cells
Concentration
cells
Electrolytic
cells
Final
Chapter 10 Project—Writing project on
batteries
Chapter
10 Summary
Chapter
10 Review
Chapter
11—Polymers
Section
11.1—Hydrocarbons
Alkanes
Alkenes
Alkynes
Alkene/Alkyne
isomers
Section
11.2—Organic functional groups
Hydrocarbon
side-branches
Haloalkanes
Alcohols
Ethers
Amines
Carbonyl
containing compounds
Carboxylic
acids
Aldehyde
Ketones
Anhydride
Aromatic
compounds
Lab
11.5--Synthesis of an Organic Molecules
Section
11.3—Polymers
Thermoplastics
versus thermoset plastics
Reactions
forming polymers
Addition
polymerization
Condensation
Polymerization
Properties
of polymers
Polymers
in the body
Lab
11.3--Observing a polymer
Final
Chapter 11 Project (Student designed)—Making the bounciest bouncy ball
Chapter
11 Summary
Chapter
11 Review
Chapter
12—Nuclear radiation
Section
12.1—Nuclear radiation
Discovery
of nuclear radioactivity
What
is nuclear radioactivity?
Types
of radioactive decay
Nuclear
reactions and equations
Half-lives
Lab
12.1--Determining the half-life of an isotope
Section
12.2—Nuclear radiation—harmful and helpful
Effects
of radiation on the body
Radiation
causing cancer
Radioactive
elements replacing other elements in the body
Radiation
used for Healing
Nuclear
Dating
Energy—fission
versus fusion
Final Chapter 12 Project—Writing