1. II. Ionic Bonds Part 2

2. Recall - Formation of Cations

3. Recall - Formation of Anions

4. Recall - Charges of Ions
Chlorine atom:
17 electrons 17-
17 protons 17 +
Neutral 0
Chlorine ion:
18 electrons 18-
17 protons 17 +
Net charge 1-
Magnesium atom:
12 electrons 12-
12 protons 12 +
Neutral 0
Magnesium ion:
10 electrons 10-
12 protons 12 +
Net charge 2+

5. A. Octet Rule
Atoms wants to achieve the electron configuration of the closest noble gas.
Atoms will gain or lose electrons to ensure 8 valence electrons
By gaining or losing electrons, atoms become electrically charged
the charge is called THE oxidation number
Atoms gain or lose electrons by accepting or donating to other atoms
ELECTRONS DO NOT JUST “FLOAT” AWAY

8. B. Ionic Bonding Analogy
Write down an analogy in your notes that describes ionic bonding. Be prepared to share with the class.
For example: “Ionic bonding can be compared to dogs and bones. Imagine two separate dogs, one big one small, each with their own bone. The big dog steals the bone from the small dog (because he wants it more), leaving the small dog with no bone. Because the big dog now has two bones (one of which belongs to the small dog), the small dog is attracted to the big dog.”

9. C. Predicting Ionic Charges
Oxidation numbers for representative elements (groups IA, IIA, IIIA, IVA, VA, VIA, VIIA, VIIIA) depend upon the group each element is in
Oxidation states vary for most transitional metals, except zinc (Zn2+), cadmium (Cd2+), and silver (Ag+)

10. Group 1A:
Lose 1 electron to form 1+ ions H+
Li+
Na+ K+
Rb+

11. Group 2A:
Loses 2 electrons to form 2+ ions
Be2+
Mg2+
Ca2+
Sr2+
Ba2+

12. Loses 3
electrons to form
3+ ions
Group 3A:
B3+
Al3+
Ga3+

13. Neither! Group 4A elements rarely form ions
EXCEPTION: Sn and Pb!! Treat like transition metals
Do they lose 4 electrons or gain 4 electrons?
Group 4A:

14. N3-
Nitride
Gains 3
electrons to form
3- ions
Group 5A:
P3-
Phosphide
As3-
Arsenide

15. O2-
Oxide
S2-
Sulfide
Group 6A:
Gains 2
electrons to form
2- ions
Se2-
Selenide
Te2-
Telluride

16. Group 7A:
Gains 1 electron to form
1- ions F–
Fluoride
Br–
Bromide
Cl–
Chloride I–
Iodide

17. Stable noble gases do not form ions!
Group 8A:

19. Check
How many valence electrons do the following atoms/ions have? H
Cl– H+
Li+ O
O2-

20. D. Transition Metals
Due to transition metals having varying oxidation numbers, roman numerals are used to denote charges.
Example:
Iron can have an oxidation number of +2 or +3
Iron (II) = Fe2+
Iron (III) = Fe3+

21. Check Write the following ions using ion notation (symbol and charge)
Magnesium ion
Copper (II)
Sulfur ion (sulfide)
Chromium (VI)
Bromine ion (bromide)
Nickel (III)
Potassium ion

22. Ionic Bonds Homework #1 Put the following into ion notation
Iodine ion (iodide)
Vanadium (V)
Aluminum ion
Manganese (III)
Barium ion
Rubidium ion
Palladium (II)
Nitrogen ion (nitride)
Oxygen ion (oxide)
Copper (I)
Write the following transition metals from their ion notation
V4+
Au+
Au3+
Co2+
Mn7+