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I
II
III
Periodic Trends
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Valence Electrons
Electrons available to be lost, gained, or shared in the
formation of chemical compounds
Outer energy level
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Atomic Radius
Distance from the center of atom’s nucleus to outermost electron.
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1
2
3
4 5
6
7
Decreases UP and to the RIGHT Or Increases DOWN and to the LEFT
Atomic Radius
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0
50
100
150
200
250
0 5 10 15 20Atomic Number
Ato
mic
Ra
diu
s (
pm
)Atomic Radius
Li
ArNe
KNa
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Describe in terms of atomic structure:
Going down a group from top to bottom, adding energy levels.
Higher energy levels have larger orbital's
Describe in terms of atomic forces:
Shielding Effect ~ inner core e- block the attraction between the nucleus and the valence e-
Atomic Radius
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Describe in terms of atomic structure: Electrons remain in the same energy level (not
farther away)
Describe in terms of atomic forces:
Increased nuclear charge (+) without additional shielding pulls e- in tighter
Atomic Radius
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An atom or group of bonded atoms that has a positive or negative charge.
Ion
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Cations (+)
lose e-
smaller
© 2002 Prentice-Hall, Inc.
Anions (–)
gain e-
larger
Ionic Radius
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Larger – down a group.
Smaller – across a period.
Cations: Smaller than neutral atom
Anions: Larger than neutral atom
Ionic Radius
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Trends in Ionic Size
Trends in Ionic Size
6.3S
ize
ge
ner
ally
incr
ease
s
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1
2
3
4 5
6
7
The amount of energy required to remove an electron from a neutral atom.
Increases UP and to the RIGHT
Ionization Energy
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Ionization Energy
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Opposite trend from atomic radius. Larger atoms ~electrons held less
strongly ~ takes less energy to remove one.
Smaller atoms ~ electrons held more strongly ~ takes more energy to remove one.
Ionization Energy
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Why small jumps within each group?
Ionization Energy
0
500
1000
1500
2000
2500
0 5 10 15 20Atomic Number
1st
Ion
izat
ion
En
erg
y (k
J)
Stable electron configurationsdo not easily give up electrons
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Amount of energy to remove 1st electron, 2nd electron, 3rd electron.
Each higher ionization requires more energy.
Na Na+ + e- 496 KJ/mol
Na+ Na+2 + e- 4565 KJ/mol
Na+2 Na+3 + e- 6912 KJ/mol
*1st, 2nd, and 3rd Ionization Energies
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Electron Affinity
The energy change that occurs when an electron is added to an atom.
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Negative Electron Affinities
Energy is given off when an electron is added to an atom.
Non-Metals tend to gain electrons.
Non-Metals have NEGATIVE affinities.
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Positive Electron Affinities
Energy is required to add an electron to an atom.
Metals tend to lose electrons
Metals have POSITIVE affinities.
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Noble Gas Electron Affinities
Noble Gases have high positive electron affinities.
Octet Rule!
8 valence electrons
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Electronegativity
The ability of an atom to attract electrons
Predict using octet rule and atomic radius.
F is most electronegative, Cs and Fr are least
electronegative.
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Electronegativity