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Copy of Periodic Trends

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by

David Maxin

on 19 December 2015

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Transcript of Copy of Periodic Trends

Atomic Radius
Decreases in atomic radi as you move from left to right across a period
Used to describe the size of the atom
Because of the increasing positive charge in the nucleus and the fact that principle energy level remains the same
Increases in atomic radi as you move down groups
Ionic Radius
Ionizaton Energy
Electron Affinity
Decreases in ionic radii as you move from left to right across a period
Increases in ionic radii as you move down a group
Because an ion's outer electrons are in orbitals corresponding to high principle energy levels
Because the loss of valence electrons causes the ionic radius to be smaller
Measure of the size of an atoms ion in a crystal lattice
http://www.rsc.org/chemsoc/visualelements/pages/data/graphic/patterns_graph.gif
Because the nuclear charge increases, and electrons are added to orbitals corresponding to successivley higher principal energy levels
Generally increases as you move from left to right on a period
Because the increased nuclear charge of each successive element produces an increased hold on the valence electrons
Defined as the energy required to remove an electron from a gaseous atom
Decreases in energy as you move down a group
This decrease in energy occurs because atomic size increases as you move down the group
Decreases as you move down a group
Work's Cited
Increases as you move from left to right across a period
the energy change that occurs when an electron is added to a neutral atom
Because the valence electrons are closer to the nucleus
Because the electrons are farther away from the nucleus
http://www.docbrown.info/page07/sblock.htm
http://www.creative-chemistry.org.uk/alevel/module1/trends1.htm
http://tannerm.com/size.htm
http://staff.norman.k12.ok.us/~cyohn/index_files/ionizationenergynotes.htm
http://www.creative-chemistry.org.uk/alevel/module1/trends7.htm
Glencoe Science: Chemistry, Matter, and Change; pages 187-194
Effective nuclear charge
Z eff
the net force experienced by an electron in an atom due to the positively charged nucleus
shielding effect
PERIODIC TRENDS in ATOMIC PROPERTIES
1.7
Full transcript