This is my first upload to Slideshare.

1. Ionization Energy
&
Ionic Radii vs Atomic Radii
By: Santiago Velásquez

2. What is an ion?!
 An ion is a charged atom or molecule. It is charged
because the number of electrons do not equal the
number of protons in the atom or molecule.

3. What is an ion?!
 An ion is a charged atom or molecule. It is charged
because the number of electrons do not equal the
number of protons in the atom or molecule.

4. What is first ionization
energy?
 Ionization is a process in which atoms lose or gain
electrons and become ions.

5. What is first ionization
energy?
 Ionization is a process in which atoms lose or gain
electrons and become ions.
 The first ionization energy is therefore a measure of the
strength of the attraction between the outermost
electrons and the nucleus.

6. What is first ionization
energy?
 Ionization is a process in which atoms lose or gain
electrons and become ions.
 The first ionization energy is therefore a measure of the
strength of the attraction between the outermost
electrons and the nucleus.

7. 1st, 2nd, and 3rd ionization
energies
 The symbol I1 stands for the first ionization energy
and the symbol I2 stands for the second ionization
energy
 Each succeeding ionization energy is larger than the
preceding energy. This means that I1<I2<I3<...<In will
always be true.

8. Ionic Radii Atomic Radii

9. Atomic Radius (Radii)
 The boundaries of an atom are fuzzy, and an atom’s
radius can vary under different conditions.
 To compare different atomic radii, they must be
measured under specified conditions.
 Atomic radius - one-half the distance between the
nuclei of identical atoms that are bonded together.

10. Atomic Radii

11. Atomic Radii
• Atoms tend to be smaller as you go from left to right on
the periodic table.
• This is due to increasing positive charge in the nucleus,
pulling the electrons closer to the center.
• Atoms tend to be larger down a group.
• This trend is due to the increasing size of the electron
cloud as electrons fill up larger energy levels.

12. Atomic Radii

13. Ion Radius (Radii)
 Positive ions tend to be smaller than neutral atoms.
 The larger the positive charge, the smaller the ion.
 Again, this is due to increasing positive charge in the
nucleus, pulling the electrons closer to the center.

14. Ion Radii

15. Ion Radii
 Positive ions tend to be smaller than neutral atoms.
 The larger the positive charge, the smaller the ion.
 Again, this is due to increasing positive charge in the
nucleus, pulling the electrons closer to the center.

16. Thanks for watching! :D