17 Elements of Chemistry
Learning Objectives
After studying Chapter 17, students will be able to:
1.
Understand the nature of chemistry.
2.
Distinguish between atoms and molecules.
3.
Describe and explain properties of elements.
4.
Analyze and explain atomic and molecular changes in a chemical reaction.
5.
Compare and contrast physical and chemical properties.
6.
Name simple chemical compounds.
Possible Misconceptions to Correct
1.
Not so! Chemistry is more complex than biology.
2.
Not so! Ice and liquid water are two different materials.
3.
Not so! Water molecules are not moving in frozen water.
4.
Not so! It is important to memorize the periodic table.
5.
Not so! Chemical and physical changes are easy to distinguish
6.
Not so! Compounds retain properties of the elements from which they are made.
In the Explorations Practice Book :
1.
Submicroscopic Thinking
2.
Physical and Chemical Changes
3.
Melting Points of Elements
4.
Densities of Elements
18 How Atoms Bond and Molecules Attract
Learning Objectives
After studying Chapter 18, students will be able to:
1.
Apply the shell model of the atom to chemical bonding.
2.
Distinguish between an atom and an ion.
3.
Predict the formula of an ionic compound using the periodic table.
4.
Distinguish between ionic and covalent bonds.
5.
Understand how some molecules are polar.
6.
Understand how the polarity of molecules affects macroscopic properties.
Possible Misconceptions to Correct
1.
Not so! Atoms are held together by some sort of glue.
2.
Not so! The periodic table is not much more than a listing of known elements.
3.
Not so! Covalently bonded atoms are held together because they share electrons.
4.
Not so! Ionic and covalent bonds have nothing in common.
5.
Not so!
Oil and water don’t mix because their molecules are not attracted to each other.
In the Explorations Practice Book :
1.
Types of Chemical Bonds
2.
Metallic Bonding

3.
Shells and the Covalent Bond
4.
Atoms to Molecules to Molecular Attractions
5.
Types of Molecular Attractions
In the Lab Manual :
1.
Molecules by Acme (molecular models)
19 How Chemicals Mix
Learning Objectives
1.
After studying Chapter 19, students will be able to:
2.
Recognize that most materials around them are mixtures.
3.
Understand how mixtures can be separated by physical means.
4.
Recognize that macroscopic samples cannot be classified as 100% pure.
5.
Distinguish solutions and suspensions from heterogeneous mixtures.
6.
Understand the concept of the mole.
7.
Use various terms associated with solutions.
Possible Misconceptions to Correct
1.
Not so! Fish breathe water.
2.
Not so! All impurities found in drinking water are bad for our health.
3.
Not so! Sugar no long occupies space upon dissolving in water.
4.
Not so! Solutes in boiling water evaporate along with the water.
5.
Not so! Natural orange juice is 100% pure.
6.
Not so! A solution must be in the liquid phase.
In the Practice Book :
1.
Solution Terms and Supersaturation
2.
Find the Solution
In the Lab Manual :
1.
Salt and Sand (separation of a mixture)
2.
Pure Sweetness (purification of brown sugar)
3.
Sugar Soft (percent sugar determination)
4.
you suppose might be the last? Why?
20 How Chemicals React
Learning Objectives
After studying Chapter 20, students will be able to:
1.
Balance simple chemical equations.
2.
Understand how concentration and temperature affect reaction rates.
3.
Explain how catalysts lower the activation energy of a reaction.
4.
Relate chlorofluorocarbons to depletion of atmospheric ozone.
5.
Calculate whether a reaction is endo- or exothermic using bond energies.
6.
Understand entropy as the tendency of energy to disperse.

Possible Misconceptions to Correct
1.
Not so! Balancing chemical equations is an important skill.
2.
Not so! All chemical reactions are instantaneous.
3.
Not so! Catalysts don’t participate in a chemical reaction.
4.
Not so! Bond energies are the same for all atoms.
5.
Not so! Exothermic reactions don’t need the input of energy.
6.
Not so! Entropy is a measure of disorder.
In the Practice Book :
1.
Balancing Chemical Equations
2.
Exothermic and Endothermic Reactions
In the Lab Manual :
1.
Bubble Round-up (collection of a gas)
21 Two Types of Chemical Reactions
Learning Objectives
After studying Chapter 21, students will be able to:
 Identify acids and bases found in their daily living.
 Understand acid/base as a behavior of chemicals.
 Recognize a salt as the product of the reaction of an acid and a base.
 Understand what is meant by acidic, neutral, and basic solutions.
 Describe and explain the concept of pH.
 Apply the concepts of acids and bases to our environment.
 Identify oxidation/reduction as the loss/gain of electrons.
 Understand how a battery works.
 Understand how fuel cells work and their significance for the future.
 Explain what happens as iron rusts.
 Compare and contrast combustion with respiration.
Possible Misconceptions to Correct
 Not so! It would be lethal to ingest an acid or a base.


Not so! All salt is made of sodium chloride.
Not so! pH’s cannot be less than zero.
 Not so! Atmospheric carbon dioxide is necessarily bad news.
 Not so! A half-reaction can occur on its own.
 Not so! Silver tarnish can only be cleaned by polishing.
 Not so! Batteries run out because they lose charge.
 Not so! Playing the car radio has no effect on fuel efficiency.
In the Practice Book :
1.
Exchanging Protons
2.
Exchanging Electrons
In the Lab Manual :
3.
Sensing pH (red cabbage juice pH indicator)

4.
Upset Stomach (titration)
5.
Tubular Rust (percent oxygen in air)
22 Organic Compounds
Learning Objectives
After studying Chapter 22, students will be able to:
1.
Recognize why carbon is such a unique element.
2.
Identify how fossil fuels are a valuable source for material goods.
3.
Explain how petroleum is refined into various products.
4.
Appreciate the diversity of carbon compounds.
5.
Describe the formation of synthetic polymers.
6.
Distinguish between addition and condensation polymers.
Possible Misconceptions to Correct
1.
Not so! Organic chemistry is not related to organic farming.
2.
Not so! Organic structures should be memorized.
3.
Not so! Higher octane fuels burn faster.
4.
Not so! Double covalent bonds can rotate.
5.
Not so! All organic compounds smell terrible.
6.
Not so! Polymers are not found in nature.
7.
Not so! There is an unlimited supply of plastics.
In the Explorations Practice Book :
1.
Carbon Questions
2.
Structures of Organic Compounds
3.
Polymers
In the Lab Manual :
1.
Smells Great! (preparation of fragrant esters)
2.
Name That Recyclable (densities of organic polymers)
23 Biological Chemistry
Learning Objectives
After studying Chapter 23, students will be able to:
1.
Recognize the four basic classes of biomolecules.
2.
Understand that carbohydrates provide structure and energy.
3.
Distinguish between saturated and unsaturated fats.
4.
Identify amino acids as the monomers of proteins.
5.
Understand the role of nucleic acids.
6.
Classify vitamins as water or lipid soluble.
7.
Recognize the biochemical make-up of the food we eat.
Possible Misconceptions to Correct
1.
Not so! Cows digest grass.
2.
Not so! Zero cholesterol in your body is a good thing.
3.
Not so! Saturated fats are always bad for you.
4.
Not so! Muscle mass is increased by eating lots of protein.
5.
Not so! It’s not possible to overdose on vitamins.

6.
Not so!
A vegetarian diet cannot provide adequate protein.
Explorations Practice Book :
1.
Polysaccharides
2.
Fatty Molecules