Atoms+Periodic Table

Atoms+Periodic Table

1. Metallic Character

   • how readily an atom can lose an electron
     • high metallic character=low ionization energy (and vice versa)

2. Ionization Energy

   • First Ionization Energy
     • enough energy to get rid of one electron
   • Second Ionization Energy
     • energy required to remove an electron from a 2+ cation
   • Third Ionization Energy
     • energy required to remove an electron from a 2+ cation

3. Electron Affinity

   • amount of energy associated with adding an electron
     • the more negative the electron affinity, the more willing an atom is to accept an electron
     • caused by a decrease in atomic radius
       • ground state=low energy=more stable

4. Isoelectronic Series

   • a set of atoms and ions that all contain the same number of electrons
   • Radii in an isoelectronic series will increase from most negative to least positive

5. Types of Atoms

   • Ion
     • atoms with a net charge due to the loss or gain of electrons
     • have a smaller radius than a neutral atom. metal atoms are more likely to form cations (which are formed by removing electrons). As more electrons are removed, the remaining electrons are drawn in more closely to the nucleus, making the radius smaller.
   • Anion
     • negatively charged ion
     • has gained electrons
     • non-metals are more likely to form anions
   • Cation
     • positively charged ion
     • has lost electrons
     • metals are more likely to form cations

6. Atoms are most likely to gain or lose a number of electrons that will in having an outer shell of 8

7. Zeff

   • effective nuclear charge that is the net positive charge by valence electrons
   • increases across a period because the number of protons is increasing but the number of shielding electrons is not
   • decreases down a group because the valence electrons' distance from the nucleus increases, so the charge left by electrons is weak.