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BELL RINGER
• Write the electron configuration for Fr.
• Draw the Lewis dot diagram for Ne, H2O, CO2, and
CH4
• What is the difference between an anion and a
cation?
PERIODIC PROPERTIES
MR. SCHLAMB
ATOMIC RADII
• What is atomic radii?
• It is defined as one half the distance between the
nuclei of identical atoms that are bonded together
 Period trends– the atomic radii across periods (rows)
decreases due to increasing positive charge in the nucleus
 Group trends– the atomic radii down a group (column)
increase due to more energy levels being filled by electrons
causing electrons to be located farther from the nucleus
IONIZATION ENERGY
• What is ionization energy?
• Ionization energy is defined as any process that
results in the formation of an ion
Period trends– in general ionization energies of
the main-group elements increase across each
period
Group trends– among the main-group elements
ionization energies generally decrease
ELECTRON AFFINITY
• What is electron affinity?
• Electron affinity is defined as the energy change
that occurs when an electron is acquired b a
neutral atom.
Period Trends– in general in the p block electron
affinity becomes more negative across the
periods
Group trends– there is almost no trend to follow
IONIC RADII
• What is ionic radii?
• Ionic radii is defined as the radius (see atomic radii)
of two or one ion
Period trends– metals on the left tend to form
cations and nonmetals at the upper right tend to
form anions
Cations are positive anions are negative
ELECTRONEGATIVITY
• Electronegativity is defined as the measure of the
ability of an atom in a chemical compound to
attract electrons from another atom in the
compound
• Period trends– electronegativity tends to increase
across a group
• Group trends– electronegativity tends to decrease
down a group