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Periodic Table Summary
Transcript of Periodic Table Summary
By: Becca Christbaum
Atomic size is the total distance between the center of an atom to the outermost shell of said atom.
Ionization energy tells us how much energy is required to remove an electron from the atom or molecule.
Electronegativity is affected by its atomic number, and the distance that the valence electrons are from the nucleus. This is what describes the tendency of an atom to attract electrons. The higher it's atomic number, the stronger this charge is.
This is when names are given to chemical properties associated with metal. Elements with the metallic property can be reduced, form ionic chlorides, and this is resulted from how fast they are ready to lose their electrons.
Lithium, Sodium, Potassium, Rubidium, Cessium, and Francium occupying group 1 of the periodic table. These elements are very reactive metals
Alkaline Earth Metals
Beryllium, Magnesium, Calcium, Strontium, Barium, Radium, these occupy group two of the periodic table. They are reactive metals that react with water to form insoluable hydroxides.
These elements are in group 17 of the periodic table. It is Flourine, Chlorine, Bromine, Iodine, or Astetine.
These gases are in group 18 of the periodic table. The elements in this group are Helium, Neon, Argon, Krypton, Xenon, and Raidon. They were one thought to be completely unreactive, but now we know Xenon, Krypton and Raidon are known to be reactive.
Atomic size increases from left to right, up to down of the periodic table..
This table shows an approximation
of how much energy is needed to remove
an electron depending on the element that
This table shows how the electronegativity gets higher in some places and lower in others. You can see a trend in electronegativity levels throughout the periodic table.
This table shows the trends of the metallic property.