AR, IR, IE
Atomic Radius, Ionic Radius, Ionization Energy
Atomic Radius
SInce we cannot pinpoint the positions of electrons, we cannot have a boundary as there will always be a probability of an electron being there
Instead distance from adjacent Nuclei ( Internuclear Distance )
Down a group --> AR increases the # of E-levels increase
More Mathematically: ( where N is the Principle Energy Level )
Across a period --> AR decreases stays the same & increases --> More charge --> Atoms are more grouped together.
More Mathematically: --> They are inversely Proportional
Ionic Radius
Where as Atomic Radius notes the distance between adjacent nucleus of Neutral atoms, Ionic Radius look at Cations & Anions
Note Cations are smaller ( greater charge ) than a stable atom
Note Anions are larger ( greater repulsion ) than a stable atom
One can easily see that for Isoelectrionic Cations , the one with the greater sum charge has a smaller ( more charge attracting )
One can easily see that for Isoelectrionic Anions, the one with the least sum charge has a bigger ( More charge repelling )
Ionization Energy
Mole ( mol ) is an SL unit used to measure the amount of any substance: Typically used to measure large quantities of tiny entities like Atoms, Molecules, and particles. here for true definition ( IMPORTANT ).
or Avogadro's number
First Ionization Energies ( ) are a way to measure the attraction between the nucleus & the outer electron.
More precisely its the amount of Energy to completely remove an electron from an neutral atom
From this we can find some trends
Down a group --> Increased distance from Nucleus to Valence
IE becomes smaller
More Mathematically:
Across a period --> increases charge increases
IE becomes bigger
More Mathematically:
Looking at the graph of Ionization Energies amongst the Elements, we can find evidence of why the First Energy Level has maximum of , evidence why s-orbitals contain only 2 electrons, etc..
Screening Effect and Effective Nuclear Charge
--> Approximate the attractive force Valence Electrons "Feel" from nucleus
With being the Effective Nuclear Charge.
With being the Nuclear Charge ( # of protons )
They are tightly packed --> so act as one large charge
With being the # of Core Electrons , that block/shield the valence electrons
Electrons in Atoms
Lyman's Series --> From ( UV )
The elements and have ground states at ( why ? )
Balmar Series --> From ( Visible )
Paschen's Series --> From
Brackett Series --> From
Since the Energy Levels get closer and closer as N converges to , eventually being so insignificantly close that it forms a continuum . Once reached there, the atom becomes an ion.
Calculating IE from Spectral Frequency
Goal: Relate Frequency & Energy
we use the following equations
where c = m/s
We can now relate to result in the equation:
However note that IE is the amount of energy needed to remove 1 mole of from 1 mole of a gas we must multiply by , Avogadro's Number. For convention, one must turn into for
IE can be calculated from wavelength or frequency that corresponds to the energy of the electron transition.
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