CK-12 Foundation is a nonprofit organization on a mission to reduce the cost of K-12 textbook materials in the US. The CK-12 Chemistry - Intermediate Quizzes and Tests is a companion to CK-12's Chemistry - Intermediate FlexBook® and includes one quiz per lesson, one chapter test, and one unit test.
Reinforcement Activity
Check Your Understanding
Points to Consider
Making the FlexBook ® Textbook Flexible
Chapter Overview
Online Resources
Pacing the Lessons
What is Chemistry?
Key Concept
Standards
Lesson Objectives
Lesson Vocabulary
Teaching Strategies
Have each group create a PowerPoint presentation on one of the five frontiers of chemistry described in the lesson: energy, medicine, materials, environment, and agriculture.
Reinforce and Review
The Scientific Method
The majority of students in a high school chemistry course will be familiar with the scientific method. Begin the topic by asking students about key terms related to the scientific method.
C HAPTER
2 Matter and Change
Chapter Outline
Properties of Matter
Have students brainstorm all the physical properties of matter they can think of. Lower ability students can benefit from making particle models of the three states of matter.
Classification of Matter
The main focus of this lesson is for students to understand the difference between a pure substance and a mixture. Have students answer the lesson review questions at the end of lesson 2.2 in the CK-12 Chemistry – Intermediate FlexBook® resource.
Changes in Matter
Assign students a different element and ask them to investigate the physical and chemical properties of their element. All samples of matter have both physical and chemical properties and can thus undergo physical and chemical changes.
The International System of Units
Start a lesson by asking the class if they can name all seven units of the SI. For example, the meter was originally defined (by the French) as one ten-millionth of the distance from the equator to the North Pole along the meridian passing through Paris.
Unit Conversions
Converting area and volume units is often very difficult because the conversion unit must be expressed squared or cubed. Both when reporting measured values and when performing calculations, the uncertainty in a measurement must be taken into account.
Uncertainty in Measurements
Students often think that an electronic balance (or pH meter) gives an exact reading because they don't have to read it visually like a graduated cylinder. As an example, give them a series of measurements and let them calculate the average deviation and explain the purpose of the calculation.
A TOMS
Chemistry Concepts
Atoms
Explain the law of conservation of mass, the law of definite proportions and the law of multiple proportions. Some students may be under the mistaken impression that the law of multiple proportions contradicts the law of definite proportions.
Lesson Review Questions
The Nuclear Model of the Atom
They should include brief descriptions of each scientist's contributions on the timeline. Have a group of students investigate James Chadwick's experiments that led to the discovery of the neutron.
Isotopes and Atomic Mass
Even for elements that have only one naturally occurring isotope, the atomic mass in the periodic table is still not a whole number. Finally, have them use their list to calculate the average atomic mass of their element and compare it to the periodic table.
5 Electrons in Atoms
- L IGHT
- Light
- The Quantum Mechanical Model
- Electron Arrangement in Atoms
The energies of all the electrons in any atom can be described using four quantum numbers. His work in quantum mechanics is most responsible for the modern model of the atom.
6 The Periodic Table
History of the Periodic Table
Dmitri Mendeleev proposed a periodic table arranged in order of increasing atomic mass of the elements, resulting in columns of elements with similar chemical behavior. Finally, open a discussion of the history of the periodic table by noting that early attempts to organize the table were made in the early 1800s, long before the discovery of subatomic particles.
Electron Configuration and the Periodic Table
A number of online activities are available to begin a study of the periodic table and its organizational principles. Once students have become comfortable with the periodic table and the electron configurations, give them an empty periodic table – only empty boxes.
Periodic Trends
The concept of effective nuclear charge (Ze f f) can be used in conjunction with electron shielding. The period trend for the effective nuclear charge is that it increases by one over a period.
7 Chemical Nomenclature
- I ONS
- Ions
- Ionic Compounds
- Acids and Bases
Ionic Compounds www.ck12.org Lattice energy is what leads to the stability of a crystal lattice. The basic nomenclature is similar to other ionic compounds: the name of the cation followed by "hydroxide".
8 Ionic and Metallic Bonding
I ONS
Ions
Students can begin this lesson by practicing the common ionic skills they learned in chemical nomenclature when writing formulas for ionic compounds. Ionic compounds adopt the structure of an extended, three-dimensional network of alternating positive and negative ions held together by electrostatic attractive forces.
Ionic Bonds and Ionic Compounds
Show the students how all the fragments have smooth surfaces and compare this to the sodium chloride model. Some students may benefit from making drawings or models of the ionic crystal lattice for various compounds.
Metallic Bonds
Seeing the coordination numbers of different metals from unit cell diagrams (Figure 8.14) can be difficult. Certain atomic orbitals must undergo hybridization to create the necessary types of orbitals formed in certain molecules.
Lewis Electron Dot Structures
For a polyatomic ion, the sum of the formal charges is equal to the charge of the ion. This eliminates the first structure due to the formal charge on the singly bonded nitrogen.
Molecular Geometry
Be sure to have molecular models handy when discussing all the different shapes described in the lesson. This activity also requires students to recognize the hybridization of central atoms, which is covered in Lesson 9.4.
Polarity and Intermolecular Forces
The current will be "pulled" towards the balloon due to the charge separation in the water molecule. This is due to the small size of the hydrogen ion and its inability to obtain a crystalline structure.
Hybridization of Atomic Orbitals
Remind them of the earliest examples (H2, F2) where overlap was able to occur of unhybridized atomic orbitals. Ask them to draw the hybrid orbitals and draw the models of the example molecules.
The counting unit of the mole is the unit used by chemists to account for the number of representative particles that participate in reactions. The molar mass of a substance is the mass in grams of one mole of particles of that substance.
The Mole Concept
Introduce Avogadro's number and the mole unit and give students plenty of practice doing conversion problems. If some students have more difficulty with the math, pair them with more advanced students to work on these conversion problems and then on conversion problems using Avogadro's number.
Mass, Volume, and the Mole
Some students might learn the mole's roadmap and how to use it by making a type of flashcard set. Have students write each of the three pairs of conversion factors from the mole's roadmap on the two sides of a 3×5 card.
Chemical Formulas
Another laboratory activity appropriate for this lesson is determining the formula of a hydrate. By converting to moles, students can calculate the mole ratio of water to anhydrous salt and thus determine the formula of the hydrate.
11 Chemical Reactions
Chemical Equations
A balanced chemical equation has the same number of atoms of each element on both the reactant and product sides of the equation. Chemical reactions Hold up models of the three molecules and ask if anything seems wrong about this equation regarding the law of conservation of mass and Dalton's theory.
Common Misconceptions
- Types of Chemical Reactions
- Mole Ratios
- Stoichiometric Calculations
- Limiting Reactant and Percent Yield
The limiting reactant is the one that will run out first in the course of the reaction. Emphasize that the theoretical yield of a product must be based on the initial amount of the limiting reactant.
13 States of Matter
- S OLIDS
- Kinetic-Molecular Theory and Gases
- Liquids
- Solids
- Changes of State
The boiling point of a liquid is reached when the temperature of the liquid is equal to the surrounding atmospheric pressure. Define vapor pressure and understand its relationship to intermolecular forces and liquid temperature.
14 The Behavior of Gases
- G AS L AWS
- Gas Properties
- Gas Laws
- Ideal Gases
Charles' law: A gas law which states that the volume of a given mass of gas varies directly with the absolute temperature of the gas when the pressure is kept constant. The ideal gas law is an extension of the combined gas law and Avogadro's law that concluded the Gas Laws lesson.
Enrichment
Gas Mixtures and Molecular Speeds
Dalton's law states that the total pressure of a gas mixture is equal to the sum of all the partial pressures. Use Dalton's law and mole fractions to calculate the partial pressure of a gas in a mixture.
Properties of Water
The map should contain information about the physical properties of the water molecule as well as macroscopic properties of water such as surface tension and low vapor pressure. Cohesion and adhesion are two additional properties of water related to its strong hydrogen bonding.
Aqueous Solutions
Try to lead students to the definition that a solution is any homogeneous mixture, regardless of the phases involved. Have students answer the lesson review questions at the end of Lesson 15.2 in the CK-12 Chemistry – Intermediate FlexBook® resource.
Colloids and Suspensions
Discuss or show the Brownian motion of a colloid and how this random motion of the colloidal particles prevents them from settling to the bottom of the container as in a suspension. The rate of dissolution is affected by temperature, solute particle size, and mixing agitation.
Electrochemical Cells
Continue to a discussion of the types of solutions and either show examples or do the activity below (in Science Inquiry) about degrees of saturation. A supersaturated solution can only be prepared in the laboratory by "tricking" the solution into having more dissolved solute than would be possible by heating and cooling.
Cell Potentials
Since the density of the solution is greater than 1 g/ml, the molality is greater than the molarity. Add the mass of the solute to 1 kg to obtain the mass of the solution.
Electrolysis
Both the freezing point depression and the boiling point elevation depend on the reduction in vapor pressure. Discuss how the effect on the boiling point is extremely minimal when a few teaspoons of salt are added to a pot of water.
Science Inquiry
- Net Ionic Equations
- H EAT F LOW
- H ESS ’ S L AW
- Heat Flow
- Thermochemical Equations
When activated, a chemical reaction causes the temperature of the cold pack to drop by absorbing heat energy from the surroundings. A complete understanding of a chemical reaction requires knowledge of the amount of heat absorbed or released during the reaction.
