The document discusses ionization energy and atomic and ionic radii. It defines an ion as a charged atom or molecule resulting from an imbalance of protons and electrons. The first ionization energy is the amount of energy required to remove an electron from the outermost shell of an atom. Each subsequent ionization energy is greater than the preceding one. Atomic radius decreases left to right on the periodic table as nuclear charge increases, while it increases down a group as electron shells expand. Positive ions have smaller radii than their parent atoms due to their increased nuclear charge.

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