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Transcript of IIIIII I. Periodic Trends The Periodic Table. A. Chemical Reactivity zFamilies ySimilar valence e -...
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I II III
I. Periodic Trends
The Periodic Table
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0 5 10 15 20Atomic Number
Ato
mic
Ra
diu
s (
pm
)
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A. Chemical Reactivity
Families Similar valence e- within a group result in
similar chemical properties
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A. Chemical Reactivity
Alkali MetalsAlkaline Earth MetalsTransition MetalsHalogensNoble Gases
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Atomic Radius size of atom
© 1998 LOGAL
© 1998 LOGAL
B. Other Properties
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Atomic Radius
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0 5 10 15 20Atomic Number
Ato
mic
Ra
diu
s (
pm
)
C. Atomic Radius
Li
ArNe
KNa
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Atomic Radius Increases going DOWN a group Why? Increased number of energy levels
C. Atomic Radius
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C. Atomic Radius
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Decreases moving from left to right across a period.
Why? Increased effective nuclear charge Greater attraction between valence
electrons and protons in the nucleus
As you move across a period,
the number of valence
electrons and the number of
protons increases
Therefore, there is a stronger
attraction!
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D. Ionization Energy
First Ionization Energy Energy required to remove one e- from
an atom.
H(g) → H+(g) + e- ∆Ho = -1312.0 kJ/mol
He(g) → He+(g) + e- ∆Ho = 2372.3 kJ/mol
Li(g) → Li+(g) + e- ∆Ho = 572.3 kJ/mol
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First Ionization Energy
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t Io
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ati
on
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erg
y (k
J)
D. Ionization Energy
KNaLi
Ar
NeHe
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First Ionization Energy Increases UP and to the RIGHT
E. Ionization Energy
Why? Moving up a column there is a stronger attraction between the electrons and the nucleus
Moving across a period, there is also increased attraction between the electrons and the nucleus because decreased atomic size
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Successive Ionization Energies
Mg 1st I.E. 736 kJ
2nd I.E. 1,445 kJ
Core e- 3rd I.E. 7,730 kJ
Large jump in I.E. occurs when a CORE e- is removed.
D. Ionization Energy
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Ionic Radius
Cations (+)
lose e-
smaller
© 2002 Prentice-Hall, Inc.
Anions (–)
gain e-
larger
E. Ionic Radius
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F. Electronegativity
*The measure of how strongly an atom attracts another atom’s electrons
• Increases from left to right (except for noble gases)
• Increases as you move up a group
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Which atom has the larger radius?
Be or Ba
Ca or Br
Ba
Ca
Examples
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Which atom has the higher 1st I.E.?
N or Bi
Ba or Ne
N
Ne
Examples
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Which particle has the larger radius?
S or S2-
Al or Al3+
S2-
Al
Examples