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Periodic TrendsPeriodic Trends
Shielding EffectShielding Effect Inner electrons: electrons between the Inner electrons: electrons between the
nucleus and the outermost energy level.nucleus and the outermost energy level.
The inner electrons shield the valence The inner electrons shield the valence electronselectrons (outermost electrons) from the (outermost electrons) from the positive charge of the nucleus.positive charge of the nucleus.
This causes a reduction in attraction This causes a reduction in attraction between the nucleus and the valence between the nucleus and the valence electronselectrons so that the valence electrons so that the valence electrons are held more loosely.are held more loosely.
Incr
ease
s
Stays the same
Shielding EffectShielding Effect
Atomic RadiusAtomic RadiusThe atomic radius is the distance from
the atomic nucleus to the atom’s outer “surface”.
The atomic radius gets gradually smaller with increasing atomic number.
The atomic radius is the distance from the atomic nucleus to the atom’s outer “surface”.
The atomic radius gets gradually smaller with increasing atomic number.
Trends in Atomic SizeTrends in Atomic Size6.3
Ionic RadiusIonic RadiusWhen metals lose
electrons they become smaller due to the nuclear charge being larger than the number of electrons. Electrons are held tighter.
When nonmetals gain electrons they become larger due to the nuclear charge being less than the number of electrons. Electrons are held looser.
When metals lose electrons they become smaller due to the nuclear charge being larger than the number of electrons. Electrons are held tighter.
When nonmetals gain electrons they become larger due to the nuclear charge being less than the number of electrons. Electrons are held looser.
Trends in Ionic SizeTrends in Ionic Size
Trends in Ionic SizeTrends in Ionic Size
6.3S
ize
ge
ner
ally
incr
ease
s
Ionization EnergyIonization Energy
the amount of energy required to pull an electron away from an atom to form a positively charged ion.
the amount of energy required to pull an electron away from an atom to form a positively charged ion.
Trends in Ionization EnergyTrends in Ionization Energy6.3
ElectronegativityElectronegativity
Electronegativity is thought of as an atom’s “electron pulling power.”
Electronegativity is thought of as an atom’s “electron pulling power.”
ElectronegativityElectronegativity
The greater an atom’s electronegativity, the greater its ability to pull electrons towards itself when bonded.
.Fluorine has the highest electronegativity.
The greater an atom’s electronegativity, the greater its ability to pull electrons towards itself when bonded.
.Fluorine has the highest electronegativity.
Trends in ElectronegativityTrends in Electronegativity
INCREASES Decre
ase
s