AP Chemistry
Unit 1 Syllabus - Atomic Structure & the Periodic Table
DATE
8/24
TOPIC
Chromatography Lab
ASSIGNMENT
Complete lab write-up
8/27
Polyatomic Ion Quiz
Lab Due
Pg. 71 #35, 37, 43-49 odd
Complete practice wkst
Notes – atomic structure & history
(2.1-2.5)
8/28
Homework Quiz
Drill & Practice Wkst (bottom ½)
Notes – electron configurations,
quantum mechanical model
(7.1-7.8)
Study!
8/29
Notes – Electronic Spectrum
Pg. 323 #59 (ignore “in the hydrogen
atom”), 65(a,d,e), 67, 71, 75, 79
8/30
Homework Quiz
Pg. 71 #51, 53
Pg. 324 #85-89 odd, 93
8/31
Notes – Periodic Trends
(2.7, 7.11-7.13)
Complete drill & practice wkst (top ½)
Homework Quiz
Complete Learning Log
Extra Practice & Learning Log
9/4
Learning Log Due
Complete lab write-up
Chemical Reactivity Lab
9/5
Lab Due
Review
9/6
TEST 1
Study for test
Learning Log
1. Thoroughly explain and give examples of the following:
-quantum numbers
-effective nuclear charge
-electron shielding
-electron configurations
-historical development of current model of the atom
2. Thoroughly explain and give examples of the following periodic trends:
-size of atoms
-size of ions
-electronegativity
3. List the following elements in order of increasing first ionization energy.
Explain your reasoning for listing them in that order.
Al
Cl
F
Mg
P
S
4. The values of the first three ionization energies for magnesium and argon are
as follows:
I1
I2
I3
Mg
735
1443
7730
Ar
1525
2665
3945
a. Give the electronic configuration of Mg and Ar.
b. In terms of these configurations, explain why the values of the first
and second ionization energies of Mg are significantly lower than the
values for Ar, whereas the third ionization energy of Mg is much larger
than the third ionization energy of Ar.
c. If a sample of Ar in one container and a sample of Mg in another
container are each heated and chlorine is passed into each chamber
what compounds, if any, will be formed? Explain in terms of the
electronic configurations given in part (a).
d. Element Q has the following first three ionization energies:
I1 = 496
I2 = 4568
I3 = 6920
What is the formula for the most likely compound of element Q with
chlorine? Explain the choice of formula on the basis of ionization
energies.
5. Explain each of the following observations using principles of atomic
structure.
a. Potassium has a lower first ionization energy than lithium.
b. The ionic radius of N3- is larger than that of O2-.
c. A calcium atom is larger than a zinc atom.
d. Boron has a lower first ionization energy than beryllium.