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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. 7.21)
and for atoms with more than one electron (Fig. 8.7)
-
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;
-
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 electron configuration using a complete box orbital diagram (p. 297)
-
an electron configuration using short form
- an abbreviated or condensed electron configuration (core notation)
-
identify
on the periodic table:
-
s,p,d, and f block elements
-
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
|
| Read: |
Text
Chapter 8, pp. 302-335 |
| Video
Programs: |
- Aufbau Principle
- Electron Configuration
and Periodic Table
|
| Textbook
Assignments: |
Read
and Understand all "Sample Problems," "Follow
Up Problems" and select any 5 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 Appredix E. |
| Mandatory ChemSkill Builder Assignments to be submitted for grade (Scores of 80% or higher on each assigned HW section will receive full credit. ) |
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)
|
| TAKE
EXAM 4: |
Exam
4 covers Units 7 and 8. |
| Note:
Complete Solutions, including all units of measurement,
must be shown for all problems. |
[Top]
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