Class Schedule

Song of the Elements: http://privatehand.com/flash/elements.html

Interactive Periodic Table: http://www.chemicool.com

Study guide and laboratory notebooks have been given to all students. Please let me know if you have not received them as yet

Orientation - Class requirements: Fill out forms for ID purposes and Laboratory use at MCC.


Chemistry Course outline

View the alignment of lesson objectives to the state and national standards.

Chemistry

  • Chapter 1: Introduction to Chemistry
      • Units in Chemistry
        The student will learn some of the basic units of measurement used in Chemistry, learn some of the tools and instruments for determining measurements used in the lab, and learn the steps of the scientific method. (Solving Problems Handbook-Chapter 1)
  • Chapter 2: Data Analysis
      • Chemistry Measurements
        Using metric measurements, exact volumes of a liquid and a massed metal solid, the student will calculate common measurements used in chemistry including density, using exponential notation and correct significant figures with regard to lab safety. (Solving Problems Handbook-Chapter 2)
      • Laboratory Safety
        The student will learn how to be safe while working in a laboratory, and examine legal and government policies that concern safety. (Solving Problems Handbook-Chapter 1; pg.4-5)
  • Chapter 3: Matter, Substances and Mixtures
        • Chemical and Physical Changes
          The student will learn to differentiate between physical and chemical changes. (Solving Problems Handbook-Chapter 3)
        • Matter
          The student will learn how atoms of elements bond together to form compounds and learn to identify substances using the proper label. (Solving Problems Handbook-Chapter 3)
  • Chapter 4: Structure of the Atom
        • Atomic Theory Development
          After reading about the history of the atomic theory, the student will research the impact of Democritus, Dalton, J.J. Thomson, Rutherford, Bohr, and Planck on the atomic theory. (Solving Problems Handbook-Chapter 4)
        • Learn about the Nuclear atom and how they differ from each other as well as their stability and decay. (Solving Problems Handbook-Chapter 4)

Exam Chapters 1-4; Oct. 6 - 7

Chapter 5: Electrons in atoms

        • Atomic Particles
          Viewing a periodic table of the elements, the student will identify and describe the number of protons, neutrons, and electrons in an element and answer questions about the fundamental subatomic particles. (Solving Problems Handbook-Chapter 5)
        • Orbital Model of the Atom
          While referencing a periodic table of the elements, the student will write electron configurations, orbital diagrams, and the four quantum numbers for elements. (Solving Problems Handbook-Chapter 5)

Chapter 6: Periodic Table of Elements

· In this lesson the students will describe the periodic trends: radius, ionization energy; and also explain why the periodic table is the most important tool for chemists. (Solving Problems Handbook-Chapter 6-7)

Chapter 8 -9: Ionic Compounds and Covalent Compounds

        • The Atom and Atomic Bonding
          The student will view a list of metals and nonmetals, chart ions as a compound and identify them as either ionic or covalent compounds, and learn more polyatomic ions. (Solving Problems Handbook-Chapter 8-9)
        • VSEPR

The three dimensional structure of covalent molecules.

Chemi Chemistry 2nd. Semester

Chapter 10 – Chemical Reactions

o The student will learn how to write basic equations involving chemical reactions. This will include single and double replacement, oxidation and reduction reactions, combustion, synthesis and acid base neutralizations.

Chapter 11 – Mol Concept

o The concept of the Mol will be explored and the student will learn how to utilize this concept in explaining and describing chemical reactions as well as determining their molecular formulas. Percent Composition and Empirical Formulas
Given empirical data of elements, the student will calculate percent composition and determine its empirical formula.

Chapter 12 – Stoichimetry

o The student will learn to calculate the necessary amount of chemicals needed to completely react with a known mass of others and in so doing be able to determine limiting reactants which will reduce waste and cost overruns.

 

Chapter 19 – Acids and Bases

  • Descriptions of Acids and Bases
    Based on lab descriptions and using Bronsted/Lowry and Arrhenius definitions, the student will calculate pH and pOH of solutions from empirical data. The student will also calculate concentration of acids from pH from empirical data.

Chapter 15 - Solutions

  • The student will learn to distinguish between homogeneous and heterogeneous mixtures. They will also calculate the strengths of solutions based on %, molar and molal concentrations as well as the colligative properties of these solutions.

Chapter 13 – States of Matter

  • The student will use the kinetic molecular theory to explain the physical properties of solids, liquids and gases (phase changes) by comparing the intermolecular forces and how they interact to determine the state of a substance.

Chapter 14 – Gas Laws

  • The student will use these gas laws to calculate how pressure, temperature, volume and the number of moles of gas will change when one or more variables is changed while considering Boyle’s Law, Charles’ Law, the Combined Gas Law, Avogadro’s Law, Graham’s Law of Diffusion and the Ideal Gas Law.

Chapter 22 – 23 Hydrocarbons and substituted hydrocarbons

  • The student will learn some of the basic principles of organic chemistry, learn to identify several types of hydrocarbons, learn some of the conventions for naming hydrocarbons, and learn about the structure and formulas of some common hydrocarbons.