Ions Continued Unit 3 Topic 2. Charges  Because elements in the same group (column) of the Periodic Table have the same number of valence electrons 

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Presentation transcript:

Ions Continued Unit 3 Topic 2

Charges  Because elements in the same group (column) of the Periodic Table have the same number of valence electrons  They also tend to form ions with the same charge

Charges  Elements in columns 1-13 tend to undergo Oxidation (lose electrons) and form Positive ions. Oxidize (lose electrons) to form Positive Ions

Charges  Elements in columns tend to undergo Reduction (gain electrons) and form Negative ions. Reduces (gains electrons) to form Negative Ions

Oxidation vs Reduction  How am I going to remember these terms? O -Oxidation I -Is L -Loss R -Reduction I -Is G -Gain

Oxidation States  The common oxidation state (ion charge) for elements can be predicted by their position on the Periodic Table

Common Oxidation States (Charges) or ~Charges Vary~ Color Page 2 of your PT Coloring book.

Octet Rule  When elements react by losing or gaining electrons, they will lose or gain the number of electrons needed to become more stable  The most stable electron configuration is a completely filled energy level  Which means you have a filled valence shell of 8 valence electrons known as the octet rule (except Hydrogen and Helium)

8 is Great  Which means you have a filled valence shell of 8 valence electrons known as the octet rule Or in the case of Hydrogen and Helium 2 electrons or zero electrons

Bonding  Positive and negative ions are attracted to each other (because of their opposite charges) and combine to form ionic compounds.  When ions combine to form compounds they must balance out their charges so that the compound ends up with no charge (electrically neutral)

Predicting…  We can predict the formulas for ionic compounds by determining the number of each ion (cation and anion) that is needed to cancel each other’s charges Note: The POSTIVE ion (cation) always goes FIRST!

Valence Electrons? 1 How many does it want to gain or lose? LOSE 1 What’s the charge? +1 Valence Electrons? 7 How many does it want to gain or lose? GAIN 1 What’s the charge? Na Cl IONIC bond is formed

Sodium Chloride  Na +1 + Cl -1  NaCl  (+1) + (-1) = 0

Valence Electrons? 1 How many does it want to gain or lose? LOSE 1 What’s the charge? +1 Valence Electrons? 6 How many does it want to gain or lose? GAIN 2 What’s the charge? -2 Li O IONIC bond is formed NEEDS ONE MORE!

Lithium oxide  Li +1 + O -2  Li 2 O  2(+1) + 1(-2) = 0 CrissCross Method

Barium Iodide  Ba +2 + I -1  BaI 2  (+2) + 2(-1) = 0

Magnesium phosphide  Mg +2 + P -3  Mg 3 P 2  3(+2) + 2(-3) = 0

Magnesium phosphide  Mg +2 + P -3  Mg 3 P 2  3(+2) + 2(-3) = 0

Anion OClP Cation Valence And Charge 2 valance Gain 2 – 2 Na 1Valence Lose 1 +1 Na 2 O Ca Li Al

Naming Ionic Compounds  What is an Ionic Compound?  Positive Metal + Negative Nonmetal  To name compounds:  Positive Metal name + Negative nonmetal name (drop ending and add “ide”  NaCl = sodium chloride

OClPF Na Sodium oxide Ca Li Al Ba Barium phosphide