iiiiii 6.3 periodic trends (p. 187-194) ch. 6 - the periodic table
TRANSCRIPT
![Page 1: IIIIII 6.3 Periodic Trends (p. 187-194) Ch. 6 - The Periodic Table](https://reader038.vdocuments.us/reader038/viewer/2022102517/5697bfc11a28abf838ca4195/html5/thumbnails/1.jpg)
I II III
6.3 Periodic Trends
(p. 187-194)
Ch. 6 - The Periodic Table
0
50
100
150
200
250
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.
0
50
100
150
200
250
0 5 10 15 20
Ato
mic
Ra
diu
s (p
m)
Atomic Number
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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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B. Chemical Reactivity
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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
0
50
100
150
200
250
0 5 10 15 20Atomic Number
Ato
mic
Ra
diu
s (
pm
)
D. Atomic Radius
Li
ArNe
KNa
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1
2
3
4 5
6
7
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 (inner shell) electrons block the attraction between the nucleus and the valence electrons.
Why smaller to the right?
Increased nuclear charge without additional shielding pulls e- in tighter
D. Atomic Radius
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Which atom has the larger radius?
Be or Ba
Ca or Br
Ba
Ca
Examples
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First Ionization Energy
0
500
1000
1500
2000
2500
0 5 10 15 20Atomic Number
1s
t Io
niz
ati
on
En
erg
y (k
J)
E. Ionization Energy
KNaLi
Ar
NeHe
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1
2
3
4 5
6
7
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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Which atom has the higher 1st I.E.?
N or Bi
Ba or Ne
N
Ne
Examples
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1
2
3
4 5
6
7
Melting/Boiling Point Highest in the middle of a period.
F. Melting/Boiling Point
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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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Ionic Radius Cations (+)
lose e-
smaller
© 2002 Prentice-Hall, Inc.
Anions (–)
gain e-
larger
G. Ionic Radius
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Which particle has the larger radius?
S or S2-
Al or Al3+
S2-
Al
Examples
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H. Electronegativity
Ability of an atom to attract an electron
Fluorine attracts the electron more than Hydrogen
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Electronegativity Trends
In groups, electronegativity decreases when atomic number increases
In periods, electronegativity increases with atomic number
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Example
Compare the Ionization Energies of metals and nonmetals.
Metals have low IE and Nonmetals have high IE.
Compare the Electronegativies of metals and nonmetals.
Metals have low EN and Nonmetals have high EN.
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Summary of Periodic Table Trends
Moving Left --> Right Atomic Radius Decreases Ionization Energy Increases Electronegativity Increases
Moving Top --> Bottom Atomic Radius Increases Ionization Energy Decreases Electronegativity Decreases