1. Going from Neutral to Charged
Atoms and Ions
Going from Neutral to Charged

2. Nuclear Notation: Neutral Atoms

3. Nuclear Notation: Charged Atoms

4. Ion: an atom which has become charged by gaining or losing one or more electrons.
When does an ion form?
When 2 elements (a metal and a non-metal) react together.

5. Trends in Periodic Table: Ability to Lose Electrons
Decreases as you move across a period

6. Trends in Periodic Table: Ability to Gain Electrons
Increases as you move across a period
Stronger nuclear charge as the number of orbits stays the same but number of protons increase.

7. Definitions
Cation:
An atom that loses electrons and becomes positively charged. Ca+2
Anion:
An atom that gains electrons and becomes negatively charged. Br-1

8. Rules for Bohr-Rutherford IONS
1. Calculate p+ and n0 just as you did for neutral atoms.
2. When determining the number of electrons add or subtract according to the charge given.
If the charge is positive subtract, if it is negative add electrons!
Example: O 8

9. Let’s Practice 

10. Summary of Ions:
Electrons lost or gained lie on the valence shell (outer most shell)
If there are less than 4 electrons in an atom’s valence shell it prefers to loose these electrons.
If there are more than 4 electrons in an atom’s valence shell it prefers to gain the remaining electrons to have a full octet.

11. What does Na look like?
What does Na 1+ look like?

12. Fluorine: Bohr-Rutherford and Naming
Draw a Bohr-Rutherford Diagram of Fluorine
Draw its ion
Note: “-” ions get an “ide” ending

13. Isotopes
An Isotope of an element have different mass numbers because they have
different numbers of neutrons, but they have the same atomic number. 13

14. 14

15. Draw the ionic form of first 20 elements ( Bohr Rutherford diagram)+1 +2 +3
+/-4 -3 -2 -1