AH Curriculum Example

AH Curriculum Example

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  • The goal of this course is to teach basic chemistry skills to students with little or no knowledge of chemistry. Students will be expected to learn words from a variety of vocabulary lists. This course is preparatory to more advanced study of chemistry. You will need to know basic algebra to be successful in this course. You will also have to have a calculator that has a log function. There is a tool available at the very bottom of the list of content called "Interactive Tools." You will find a Virtual Journal there in which you can make entries on topics where notes will be handy for continued reference. One good way to use the Interactive Tools is to use a split computer screen with notes on one side and the lesson you are working on on the other side.  Or you can even use two computers or a computer and an Ipad to achieve the objective of being able to look and your notes and the lesson at the sam time. Or, another way is just to keep a physical (paper) notebook for this course.  Each student has a particular way of learning--some learn best by writing something down with a pencil and paper; others need to say the formulas out loud; others learn best just with the computer.  As a student, it is important for you to figure out what type of learning is most effective for you.  In your course journal, include a clear space for formulas, definitions of variables, and definitions of laws and theories.  You will need to reference these frequently, so it is most effective to keep these together. Unit 1: Atoms and the Periodic Table Why is Chemistry important? All things are made up of atoms, and atoms behave in predictable ways. If you know the name of an element from the Periodic table, you can predict the characteristics of that element: the mass, what state the atoms are in, and how they will react with other atoms. Why did the Hindenburg explode, while the Goodyear blimp never does? How do Forensic Chemists determine that someone was poisoned? How does Ozone form, and why is it important? All these are covered in Chemistry. It is going to be extremely important when going through the course material that you take notes. You will venture to many sites outside of our school for further explanation and detail for the lessons you are covering. When you click on a link and it takes you to another website, you will be responsible for the information that is on the link, so be sure you using reliable sources. Just because something is on the internet doesn't mean it is true! Sometimes books and articles give unreliable inforrmation, too.  So use your critical thinking skills!
  • Unit 1 Unit 1 Main Ideas: Three basic laws describe how matter behaves in chemical reactions. Compounds contain atoms in whole-number ratios. Atoms can be subdivided into smaller particles. Atoms contain positive and negative particles. Atoms have small, dense, positively-charged nuclei. A nucleus contains protons and neutrons. The radii of atoms are expressed in picometers. Light has characteristics of both particles and waves. When certain frequencies of light strike a metal, electrons are emitted. Electrons exist only in very specific energy states for atoms of each element. Bohr’s model of the hydrogen atom explained electron transition states. Mendeleev’s periodic table grouped elements by their properties. Moseley arranged elements by their atomic numbers. Modern periodic tables arrange the elements by both atomic number and properties. Electrons have wave-like properties. The speed and position of an electron cannot be measured simultaneously. Orbitals indicate probable electron locations. Quantum numbers describe atomic orbitals. Electrons fill in the lowest-energy orbitals first. There are three ways to indicate electron configuration. No electrons can occupy a higher-energy sublevel until the sublevel below it is filled. The period of an element is determined by its electron configuration. Atomic radii are related to electron configuration. Removing electrons from atoms to form ions requires energy. Adding electrons to atoms to form ions also requires energy. When atoms become ions, their radii change. Only the outer electrons are involved in forming compounds. Atoms have different abilities to capture electrons. The properties of d-block metals do not vary much.
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