Upload
jodie-joseph
View
214
Download
0
Tags:
Embed Size (px)
Citation preview
Periodic TrendsPeriodic Trends
Atomic RadiusAtomic Radius
Atomic RadiusAtomic RadiusDefined as half the distance
between the nuclei of two atomsGoing across the periodic table
◦But why are they smaller towards the right?
Electron ShieldingElectron ShieldingShielding electrons
_____________________________They “shield” the valence electrons
from the _______________from the nucleus
As you add electrons across a period, they are added to the SAME energy level, ______________________________
The increased nuclear charge is able to ______________________________________________________________
Atomic RadiusAtomic RadiusGoing down a group
Ionic RadiusIonic RadiusIon – Atoms lose electrons to become
Atoms gain electrons to become
Ionic RadiusIonic RadiusPositive ions
◦ Always become __________
◦ The lost electron(s) is the valence level ________________________________
Negative ions◦ Always become
______________◦ Addition of
electrons increases repulsion.
Ionic RadiusIonic Radius
Ionic RadiusIonic Radius
Ionization EnergyIonization Energy
Ionization EnergyIonization EnergyThe energy required to remove
an electron from an atom
Ionization EnergyIonization EnergyIncreases across
the periodic table
Decreases as you go down the periodic table
Ionization EnergiesIonization Energies
ElectronegativityElectronegativity
ElectronegativityElectronegativityThe ability of an atom to attract
an electron from another atom.On a scale from .79 to 3.98
Pauling’s
ElectronegativityElectronegativityIncreases across
the periodic table
Decreases as you go down the periodic table