II. Ionic Bonds Part 2

Recall - Formation of Cations

Recall - Formation of Anions

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+

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

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.”

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+)

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

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

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

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:

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

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

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

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

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

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+

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

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+