iiiiii ch. 5 - the periodic table i. history (p. 123 - 127)
TRANSCRIPT
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I II III
Ch. 5 - The Periodic Table
I. History(p. 123 - 127)
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A. Mendeleev
Dmitri Mendeleev (1869, Russian) Organized elements
by increasing atomic mass.
Elements with similar properties were grouped together.
There were some discrepancies.
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A. Mendeleev
Dmitri Mendeleev (1869, Russian) Predicted properties of undiscovered
elements.
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B. Moseley - 1913
Henry Mosely (1913, British)
Organized elements by increasing atomic number.
Resolved discrepancies in Mendeleev’s arrangement.
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I II III
II. Organization of theElements
Ch. 5 - The Periodic Table
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MetalsNonmetalsMetalloids
A. Metallic Character
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Main Group ElementsTransition MetalsInner Transition Metals
B. Blocks
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I II III
III. Periodic Trends
(p. 140 - 154)
Ch. 5 - The Periodic Table
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0 5 10 15 20Atomic Number
Ato
mic
Ra
diu
s (
pm
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A. Periodic Law
When elements are arranged in order of
increasing atomic #, elements with similar
properties appear at regular intervals.
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B. Chemical Reactivity
Families Similar valence e- within a group result in
similar chemical properties
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B. Chemical Reactivity
Alkali MetalsAlkaline Earth MetalsTransition MetalsHalogensNoble Gases
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Atomic Radius size of atom
© 1998 LOGALFirst Ionization Energy Energy required to remove one e- from a
neutral atom.
© 1998 LOGAL
Melting/Boiling Point
C. Other Properties
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Atomic Radius
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Ato
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Ra
diu
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D. Atomic Radius
Li
ArNe
KNa
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Atomic Radius Increases to the LEFT and DOWN
D. Atomic Radius
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Why larger going down?
Higher energy levels have larger orbitals
Shielding - core e- block the attraction between the nucleus and the valence e-
Why smaller to the right?
Increased nuclear charge without additional shielding pulls e- in tighter
D. Atomic Radius
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First Ionization Energy
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E. Ionization Energy
KNaLi
Ar
NeHe
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First Ionization Energy Increases UP and to the RIGHT
E. Ionization Energy
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Why opposite of atomic radius?
In small atoms, e- are close to the nucleus where the attraction is stronger
Why small jumps within each group?
Stable e- configurations don’t want to lose e-
E. Ionization Energy
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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.
E. Ionization Energy
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Al 1st I.E. 577 kJ
2nd I.E. 1,815 kJ
3rd I.E. 2,740 kJ
Core e- 4th I.E. 11,600 kJ
Successive Ionization Energies
Large jump in I.E. occurs when a CORE e- is removed.
E. Ionization Energy
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Melting/Boiling Point Highest in the middle of a period.
F. Melting/Boiling Point
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Ionic Radius
Cations (+)
lose e-
smaller
© 2002 Prentice-Hall, Inc.
Anions (–)
gain e-
larger
G. Ionic Radius
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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 atom has the higher melting/boiling point?
Li or C
Cr or Kr
C
Cr
Examples
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Which particle has the larger radius?
S or S2-
Al or Al3+
S2-
Al
Examples