Periodic Trends. Shielding Effect Inner electrons: electrons between the nucleus and the outermost...

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.

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

Ionization EnergyIonization Energy

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.”

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

Periodic Trends. Shielding Effect Inner electrons: electrons between the nucleus and the outermost...

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