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Periodic Trends
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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 (
pm
)
Atomic Number
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Trends
Atomic Radius Ionization Energy Electronegativity Valence Electrons Energy LevelsReactivity of MetalsReactivity of Nonmetals Melting and Boiling Points
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Atomic Radius – Size of an atom
0 5 10 15 200
50
100
150
200
250 Atomic Number vs. Atomic Radius
Atomic Number
Ato
mic
Rad
ius
(pm
)
Atomic Radius
Li
ArNe
KNa
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Periodic Trend: Atomic RadiusAt
omic
Rad
ius:
Incr
ease
sAtomic Radius: Decreases
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Period Trend:Atomic Radius
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Smaller (Decreases) to the right
Increased nuclear charge without additional shielding pulls e- in tighter
Larger (increases) going down
Jump in size of nucleus and new energy level
Shielding - core e- block the attraction between the nucleus and the valence e-
Atomic Radius
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Ionization Energy – Energy required to remove the outermost electrons
0 5 10 15 200
500
1000
1500
2000
2500 Atomic Number vs. Ionization Energy
Atomic Number
Io
niz
atio
n E
ner
gy
(kJ)
Ionization Energy
KNaLi
Ar
NeHe
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Periodic Trend:Ionization Energy
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Increases to the right
In small atoms, e- are close to the nucleus where the attraction is stronger and nuclear charge increases so attraction between nucleus and electrons increases.
Decreases going down
More energy levels have electrons further from the nucleus so attraction less and the shielding affect.
Ionization Energy
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Electronegativity
Electronegativity – An atom’s desire to grab another atom’s electrons.
Ne ArHe
FCl
Li Na K
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Periodic Trend:Electronegativity
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Electronegativity
Increases to the Right
Electrons are closer to the nucleus and nuclear charge is greater so attraction between nucleus and valence electrons greater.
Decreases going down
Shielding affect where electrons in lower energy levels shield the positive charge of the nucleus to the electrons so attraction is less between nucleus and valence electrons
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Summary of Periodic Trends
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1
2
3
4
5
6
7
Chemical Reactivity
Families Similar valence e- within a group result in
similar chemical properties
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Reactivity of Metals
Reactivity of Metals: Decreases
Reac
tivity
of M
etal
s: In
crea
ses Francium is the
most reactive metal
Francium m
ost reacti
ve Metal
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Reactivity of Metals
Decreases to the right Nuclear charge increases and electrons
are closer so stronger attraction for electrons and higher ionization energy.
Increases going down More energy levels so electrons are
farther away and shielding electrons cause attraction to be less between nucleus and electrons.
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Reactivity of Nonmetals
Reactivity of Nonmetals: Increases
Reac
tivity
of N
onm
etal
s: D
ecre
ases
Fluorine is the most reactive Nonmetal
Fluorine is most reactive Nonmetal
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Reactivity of Nonmetals
Increases to the right Nuclear charge increases so stronger
attraction for electrons and higher electronegativity.
Decreases going down Nuclear charge decreases due to
shielding electrons and the electrons are further away. This causes lower electronegativities.
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1
2
3
4
5
6
7
Melting/Boiling Point Highest in the middle of a period.
Melting/Boiling Point
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