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What do these have in common? CO 2 H 2 O C 3 H 8 HCl C 6 H 12 O 6 MgCl K 2 O
They are all compounds – 2 or more elements chemically bound together
Ionic Compounds Ionic compounds are compounds that consist of a positive ion and a negative ion that are attracted to one another because of their opposite electrical charges.
What are ions? An atom or group of atoms that has gained or lost electrons and has a negative or positive charge as a result.
Positively charged ions (cations) Ca 2+ Na + K + Mg 2+ Al 3+ Sr 2+ The first one is a calcium ion. What are the other ones called?
Sodium Potassium Magnesium Aluminum Strontium
Negatively charged ions (anions) Cl - F - O 2- P 3- S 2- N 3- The first one is a chloride ion. What are the other ones called?
Fluoride Oxide Phosphide Sulfide Nitride
What happens when two oppositely charged ions come together? Na + + Cl - ?
They form an ionic compound that has a neutral charge! NaCl
Quick Task Take all 6 positively charged ions from this presentation and combine them with the 6 negatively charged ions from the this presentation and write their names and formulas
Names are easy – positive ions first and negative ions last Sodium chloride
A bunch of names Calcium chloride Calcium fluoride Calcium oxide Calcium phosphide Calcium sulfide Calcium nitride Sodium chloride Sodium fluoride Sodium oxide Sodium phosphide Sodium sulfide Sodium nitride Potassium chloride Potassium fluoride Potassium oxide Potassium phosphide Potassium sulfide Potassium nitride Magnesium chloride Magnesium fluoride Magnesium oxide Magnesium phosphide Magnesium sulfide Magnesium nitride Aluminum chloride Aluminum fluoride Aluminum oxide Aluminum phosphide Aluminum sulfide Aluminum nitride Strontium chloride Strontium fluoride Strontium oxide Strontium phosphide Strontium sulfide Strontium nitride
Formulas? Remember they have to be neutral after they combine Ca 2+ + Cl - ?
Ca 2+ combines with 2 Cl - to give: CaCl 2 The 2 chlorides add up to -2, cancelling out the +2 charge of the calcium
A bunch of formulas CaCl2 CaF2 CaO Ca3P2 CaS Ca3N2 NaCl NaF Na2O Na3P Na2S Na3N KCl KF K2O K3P K2S K3N MgCl2 MgF2 MgO Mg3P2 MgS Mg3N2 AlCl3 AlF3 Al2O3 AlP Al2S3 AlN SrCl2 SrF2 SrO Sr3P2 SrS Sr3N2
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Unit 4 Notes Chemistry Mr. Nelson Why do atoms bond? Why DONT some atoms bond? The noble gases – why? They have a full s and p subshell of electrons.
Naming Chemical Compounds. Binary Ionic Compounds Binary = 2 types of elements Ionic = made of ions Compound = atoms bonded together.
Nomenclature Chapter 4. Nomenclature = Naming Common names were created before there was a system in place Common names were created before there was.
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AP Notes Chapter 2 Molecules, Ions and Their Compounds.
Chapter 7 Ionic Bonding Keeping Track of Electrons The electrons responsible for the chemical properties of atoms are those in the outer energy level.
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