| KEY: | |
| delivery method (text selections are given in a separate column) | evaluation method |
| l = lecture | T = lecture test |
| n = notes | Lx = lab number x (labs are also delivery methods)1 |
| F = final exam | |
| v = video tape or internet streaming video available | CI = critical item question or lecture test |
| old item |
Performance/Task: The student will: | text sections |
delivery method |
eval. method |
| Theory of Atomic Structure | ||||
| 1 |
Know what is meant by "Quantum"
and be able to describe the fundamental differences between classical
and quantum physics |
7.1 |
||
| 2 |
Be able to describe the dual nature of
matter, giving some examples of this dual nature |
7.4 |
||
| 3 |
Be able describe and to give reasons for quantum numbers | 7.5 |
||
| 4 |
Know what is meant by energy levels and the meaning of the four quantum numbers for an electron in an atom | 7.6 | l/n/v | T/L7 |
| 5 |
Know the selection rules for the quantum numbers of electrons in an atom. | 7.6 | l/n/v | T/L7 |
| 6 |
Know how to designate the quantum numbers by the letter designation, i. e. the electron configurations. | 7.6, 7.7 | l/n/v | T/L7 |
| 7 |
Be able to use the aufbau principle based on the hydrogen atom to give the electron configuration for any atom in its ground state.. | 7.8, 7.9 | l/n/v | T/L7 |
| 8 |
Know the order of the high stability configurations and Hund's rule. | 7.8 | l/n/v | T/L7 |
| Periodic Trends | ||||
| 9 |
Know the periodic trends, the exceptions to the trends, and the logic behind both for inozation energy, electron affinity, atomic and ionic radius. | 8.3-8.5 | l/n/v | T |
| 10 |
Know the definition of electronegativity and the periodic trends for it. | 9.5 | l/n/v | T |
| 11 |
Be able to describe the peroxides and superoxides in terms of oxidation number and ions formed | 8.6 | l/n/v | T |
| Bond Structure | ||||
| 12 |
Know the definition of valence electrons and how to tell how many there are for a particular atom | 8.2 | l/n/w/v | T/L7 |
| 13 |
Be able to use the Lewis dot structures
of ionic and covalent molecules and ions using valence electrons. Know and be able to apply the rules for Lewis dot formulas give in the lab manual |
9.2-9.9 |
l/n/w/v |
T/L8 |
| 14 |
Know the definitions of an ionic and covalent compounds and how each is formed.. | 9.2, 9.4 | l/n/v | T/L8 |
| 15 |
Be able to explain the reason for the formation
of ionic or covalent compounds based on the tendency to obtain highly
stable electron configuations |
9.3 |
||
| 16 |
Be able to describe the bonding
involved in a covalent compound including the possibility of double
and triple bonding. |
9.4, 10.5 |
||
| 17 |
Know the definition of lone or unshare electron pair and how to show this in the Lewis dot structure | 9.4 | l/n/v | T/L8 |
| 18 |
Be able to predict whether a compound is ionic or covalent based upon electronegativity and periodic table position. | 9.5 | l/n/v | T/L8 |
| 19 |
Be able to distinguish between hydrogen
compounds with H having an oxidation number -1 and those with +1 |
9.5 |
||
| 20 |
Be able to recognize the presence of resonance
and symbolize it. |
9.8 |
||
|
|
||||
| 21 |
Know the rules for creating hybrid orbials and be able to apply them to determine electron geometry | 10.1 | l/n/v | T/L8 |
| 22 |
From the molecular structure, be able to
determine if a molecule is polar and, if so, what the orientation of the
dipole is |
9.5, 10.2 |
l/n/v |
T/L8 |
| 23 |
From the hybrid orbitals and the lone electron pairs, be able to predict the electronic and molecular geometry | 10.3,10.4 | l/n/v | T/L8 |
| 24 |
Know the definition of sigma and pi bonds and the physical appearance and how these might affect geometry (including hindered rotation) | 10.5 | l/n/v | T/L8 |
| Ionic Bonding | ||||
| 25 |
Know the definition of ionic compound formation and be able to describe what an ionic compound is | 5.1-5.5 | l/n/w/v | T |
| 26 |
Be able to explain the reason for the formation of ionic or covalent compounds based on the tendency to obtain highly stable configurations. | ? | l/n/v | T |
| 27 |
Be able to decide whether a compound is ionic or covalent; that is, know how to tell by electronegativity difference or Periodic Table positions. | 5.10 | l/n/v | T |
| 28 |
Be able to distinguish between the hydrogen compounds with -1 oxidation number, the hydrides, and +1, the nonmetal hydrogen compounds. | 5.3, 4.3 | l/n/v | T |
| 29 |
Be able to write combination reactions of non-metals (including H) with metals to give principal oxidation number. | 5.2-5.5 | l/n/v | T |
| 30 |
Be able to give the formula for the normal oxides for groups 1, 2, 3 and 13 metals. | 5.6 | l/n/v | T |
| 31 |
Be able to describe the peroxides and superoxides in terms of oxidation number and the ions formed. | 5.6 | l/n/v | T |