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Atomic Structure and Atomic Structure and PeriodicityPeriodicity
Periodic TrendsPeriodic Trends
Ionization EnergyIonization Energy
An electron can be removed from an An electron can be removed from an atom if enough energy is absorbed (+)atom if enough energy is absorbed (+)
Ionization energyIonization energy – the energy – the energy required to remove one electron from required to remove one electron from a gaseous neutral atoma gaseous neutral atom
A (g) + energy A (g) + energy A A+ + (g) + e(g) + e--
measurements of this are made on measurements of this are made on individual atoms in gas phase to avoid individual atoms in gas phase to avoid interactions with nearby atoms interactions with nearby atoms
Ionization Energy Ionization Energy
Ionization EnergyIonization Energy
if one electron is removed, the if one electron is removed, the positive charge binds the electrons positive charge binds the electrons more tightly so 2more tightly so 2ndnd ionization energy ionization energy must be highermust be higher
the largest jump in energy is when the largest jump in energy is when you remove a core electron instead you remove a core electron instead of valenceof valence
Ionization EnergyIonization Energy
Ionization EnergyIonization Energy
Across Period:Across Period: requires more requires more
energy to remove energy to remove an electron so an electron so increasesincreases
because electrons because electrons added in the same added in the same energy level do energy level do not shield not shield electrons from electrons from nuclear chargenuclear charge
Down Group:Down Group: requires less requires less
energy to remove energy to remove electron so electron so decreasesdecreases
because the because the valence electrons valence electrons are farther away are farther away from protons from protons attracting themattracting them
Ionization EnergyIonization Energy
Ionization EnergyIonization Energy
Electron AffinityElectron Affinity
Electron AffinityElectron Affinity – the energy change – the energy change when an electron is added to a when an electron is added to a gaseous neutral atomgaseous neutral atom exothermic (-)exothermic (-)
A + eA + e- - A A-- + energy + energy
Electron AffinityElectron Affinity Across Period:Across Period:
releases more releases more energy so number energy so number increases (gets increases (gets more negative)more negative)
because electrons because electrons added in the same added in the same energy level do energy level do not shield not shield electrons from electrons from nuclear chargenuclear charge
Down Group:Down Group: releases less releases less
energy so number energy so number decreases (gets decreases (gets less negative)less negative)
because the because the electrons being electrons being added are farther added are farther away from the away from the attracting protonsattracting protons
Electron AffinityElectron Affinity
Atomic RadiiAtomic Radii
Defined by the edge of Defined by the edge of its orbital but since the its orbital but since the edges are fuzzy, edges are fuzzy, difficult to determinedifficult to determine
Atomic RadiiAtomic Radii – half the – half the distance between the distance between the nuclei of identical nuclei of identical atoms that are bonded atoms that are bonded togethertogether
Atomic RadiiAtomic Radii Across Period:Across Period:
atoms get smalleratoms get smaller because of the because of the
increased number of increased number of protons attracting protons attracting the electronsthe electrons
the electrons added the electrons added in the same energy in the same energy level do not shield level do not shield electrons from electrons from nuclear chargenuclear charge
Down Group:Down Group: atoms get largeratoms get larger increasesincreases because the because the
energy levels energy levels being added to being added to the atomthe atom
Atomic/Ionic RadiiAtomic/Ionic Radii