Periodic Table S2
The Periodic Table
Warmup:
Overview of the Periodic Table
Metals
Metalloids
Nonmetals
Noble Gases
Trends of the Periodic Table
“periodic” = repeating pattern
Overall theme = electrons’ positions relative to each other and the nucleus determine the
following properties:
4. Electron configuration
5. Ionic radius
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Periodic Table S2
4. Electron configuration
1A
2A
1
2
H 1s1
He 1s2
Li 2s1
Be 2s2
Na 3s1
Mg 3s2
K 4s1
Ca 4s2
Rb 5s1
B
3-12
3A
4A
5A
6A
7A
8A
13
14
15
16
17
18
F 2s22p5
Ne 2s22p6
B 2s22p1 C 2s22p2
N 2s22p3 O 2s22p4
3s23p1
3s23p2
3s23p3
3s23p4
3s23p5
3s23p6
Sc-Zn 3d
4s24p1
4s24p2
4s24p3
4s24p4
4s24p5
4s24p6
Sr 5s2
Y-Cd
4d
5s25p1
5s25p2
5s25p3
5s25p4
5s25p5
5s25p6
Cs 6s1
Ba 6s2
La-Hg 5d
6s26p1
6s26p2
6s26p3
6s26p4
6s26p5
6s26p6
Fr 7s1
Ra 7s2
Ac-Une 6d
(followed
1+
2+
2+
by s)
3+
4+
1+ or 2+
3-
2-
1-
4-
(generally)
B
Lanthanide/
Actinide
series
Begin in
period 6
Noble gas configuration = [core] electrons
“outer” electrons = “valence” electrons
Elements of “A” groups have valence
electrons in s and p orbitals.
Ce-Lu 4f
Th-Lr 5f
(followed by s)
(Note: USA uses A and B.
Rest of world uses 1-18)
1+ or 2+
(generally)
The position of a valence electron and the ability to remove it from an atom are related to
•
the number of protons in the nucleus
•
the extent to which the valence electron is shielded from the positively-charged
nucleus by the negatively-charged core electrons
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0
Periodic Table S2
Isoelectronic Series
= same number of electrons
(iso = equal)
1. Draw the complete electron configuration of each of the following elements.
2. What ions will they form?
3. When ions, how many electrons does each have? How many protons?
4. Predict the relative diameters of the members of this isoelectronic series.
Element
Electron config
Ion
O
F
Ne
Na
Mg
Prediction (smallest to largest):
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Ion # e-
Ion # p+
Periodic Table S2
6. Ionic Radius
a)
Cations (+) are always SMALLER than the original atom
( # e-’s   repulsion and greater pull on the valence e-’s by the nucleus
 remaining e-’s shrink to nucleus)
b)
Anions (-) are always LARGER than the original atom
( # e-’s   repulsion  shell swells)
Ionic Radius
1. In this table of ionic radii, how is the charge of the ions of elements in groups 1A-4A
related to the group number? _____________________________________________
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