Making Stable Atoms… Ions!
SCH 4C
REVIEW
 The atoms we have studied so far are __________________ (they have _____ overall charge).

Atoms are neutral when: _________________________________________________________
To become more _______________, an atom attempts to ______________ _____ _____________
____________________ until its outer shell is full.
RECALL that for all the atoms studied in this class:
OCTET RULE
-
1st shell holds a maximum of __________ electrons
-
2nd shell holds a maximum of __________ electrons
-
3rd shell holds a maximum of ___________ electrons
-_________________________________________________________________
_________________________________________________________________
 An element's outer shell (called _____________ shell) is full and most
____________ when it contains eight electrons (this stability is the reason that
the noble gases are so unreactive).
 Atoms tend to combine in such a way that they each have _____ electrons in
their valence shells. Molecules or ions tend to be most stable like this.
 Exception: The _______ shell which follows the _________ RULE since it
only holds ______ electrons.
IONS
- When an atom gains or loses _________________ it is no longer neutral. It is now a
charged particle called an ________.
 If an atom loses electrons, it has more protons (____) than electrons (____) and will
have an overall ______________charge.
 If an atom gains electrons, it has more electrons ( ____) than protons (____) and will
have an overall ________________ charge.
Reminder – ONLY electrons can move, protons are NOT gained or lost
2 ways we can determine how many electrons an atom will lose of gain:
1) Drawing Lewis diagrams and using the OCTET RULE
2) Using the Periodic Table (IA, IIA, IIIA, IVA, VA, VIA, VIIA, VIIIA)
1)
a.
b.
c.
d.
Drawing Lewis diagrams
Draw the Lewis diagram for the element.
Determine if the element will gain or lose the electrons to satisfy the OCTET RULE.
Draw in extra electrons or remove electrons, as appropriate.
Write the correct charge in the top right corner of the diagram.
Example: Oxygen
Using Lewis Structures, draw the appropriate ion for the following elements.
Fluorine
Magnesium
Sodium
Phosphorus
Chlorine
Argon
Potassium
Beryllium
Lithium
Nitrogen
Sulfur
Iodine
Rubidium
Silicon
2. Using the location on the periodic table only, provide the ion (symbols and charges) for the following
elements or the element for the ion.
Element
Lithium
Ion
Boron
Element
Ion
Al3+
Neon
F1-
Chlorine
S2-
Calcium
Na1+
Nitrogen