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| Goal
I. Predict the electron configuration of atoms and ions by reference to
the periodic table of the elements. |
Objectives: To meet the requirements of Goal
I, you must be able to:
- describe the
major differences between orbital energies for the hydrogen
atom (Fig. 7.20) and for atoms with more than one electron
(Fig. 8.4)
-
use the concepts
of shielding and effective nuclear charge to explain the
observations:
-
in an atom with more than one electron, electrons in
different subshells within the same shell have different energies;
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in atoms of different elements,
electrons in the same subshell have different energies;
-
describe
the Aufbau approach to determining electron configuration;
-
define the
term degenerate as it applies to orbitals within an atom;
-
state and apply
Hund's Rule; recognize paramagnetic and diamagnetic electron
configurations;
-
write, for
an atom in its ground state or in a specified excited state, the following:
-
an abbreviated electron configuration
using core notation,
-
an orbital diagram; (p. 299)
-
identify
on the periodic table:
-
s,p,d, and f block elements
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main group elements, first, second,
and third transition series; lanthanide and actinide series;
-
use
the periodic table to predict the valence shell electron configurations
in atoms of main group elements and first row transition elements;
-
predict
charges on ions formed by main group elements; write ground state electron
configurations for ions with specified charges;
-
distinguish the
ground state electronic configuration of an atom or ion from an excited
state configuration;
-
identify isoelectronic
atoms and ions.[Top]
| Goal II. Relate periodic
trends in electron configuration to properties of elements. |
Objectives: To meet the requirements of Goal
II, you must be able to:
-
relate
trends in atomic radii within groups and across periods to electron configurations;
compare relative sizes of atoms and their ions;
-
relate
trends in the first ionization energies of elements within groups and across
periods to electron configurations;
-
relate
the relative magnitudes of successive ionization energies for an element
to the electronic configuration of its atoms;
-
relate
trends of electron affinities of elements within groups and across periods
to electron configurations;
-
explain the
significance of a negative value for electron affinity;
-
discuss the
major distinguishing chemical characteristics of hydrogen, the alkali metals,
the alkaline-earth metals, halogens, transition metals, actinides and lanthanides,
and noble gases and relate these characteristics to electron configurations.[Top]
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Unit 8 Assignments
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| Read: |
Text
Chapter 8, pp. 292-325 |
| Video
Programs: |
- Aufbau Principle
- Electron Configuration
and Periodic Table
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| Textbook
Assignments: |
Read
and Understand all "Sample Problems," "Follow
Up Problems" and the blue-colored problems at the
end of the chapters.
The
answers for the Follow Up Problems are at the end
of the chapter; the answers for the blue-colored
problems are in Appendix C.The answers for each
of these are in Appendix C.
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| ChemSkill
Builder Assignments: |
Mandatory
assignments to be submitted for grade
Chapter 9, Sections
9.3, 9.4, 9.5 (box orbital diagrams, electron
configuration I & II)
Chapter 11, Sections
11.1, 11.2 (size of atoms and ions, ionization
energy, electron affinity)
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| TAKE
EXAM 4: |
Exam
4 covers Units 7 and 8. You will be given a copy of
the Periodic Table.
You may use a 3" x 5" hand-written study card for Exams 1, 2, 3, 4, and 5. (NOT TO BE USED FOR THE NOMENCLATURE TEST.) You must hand-write the information you would like to have on your card yourself -- no technology miracles allowed. Formulas, constants, definitions, concepts, solubility tables, etc., may be on the study card. NO SAMPLE PROBLEMS are allowed to be on the card. You may write on both sides of the study card. The card must be submitted with your exam. Any abuse of this privilege will result in a failing grade for the course. |
| Note:
Complete Solutions, including all units of measurement,
must be shown for all problems. |
[Top]
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