naming ionic compounds. charges group 1a +1 group 2a +2 group 3a +3 group 4a n/a group 5a -3...
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NamingIonic Compounds
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Charges
• Group 1A +1• Group 2A +2• Group 3A +3• Group 4A N/A• Group 5A -3• Group 6A -2• Group 7A -1• Group 8A STABLE
• The charges of monatomic ions, or ions containing only one atom, can be determined by referring to the periodic table
Elements will gain or lose electrons to have 8 valence electrons. (This is the octet rule)
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Ionic Compounds• ion : atom or group of atoms that has a charge • A monatomic ion is one element with a charge• A polyatomic ion is more than one element with a
charge• Example: SO4
2-
• ionic compound: compound formed between a cation ( +) and an anion (-).– usually between a metal and a nonmetal.– also form between a polyatomic ion (like ammonium) and
either a metal or nonmetal.
• TRANSFER valence electrons
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Formation of Ionic Compounds
• objects with opposite charges attract each other.
• ionic bond = the strong attractive force between ions of opposite charge– Strongest type of bond!!
• the overall charge of the compound will be …
• ZERO!
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Examples of Formula Writing• Write the formula for the compound formed between
calcium and nitrogen• Step One: Write the symbols and charges of the
ions formed– Ca2+ N3-
• Step Two: Balance the charges so the total is ZERO– You will need 3 Calcium’s and 2 Nitride’s
• Step Three: Write the Formula– Use subscripts to show the number of each ion needed
–Ca3N2
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More examples
• Write the formula between Mg and Br
• Mg+2 Br -1
• MgBr2
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More examples
• Write the formula for the compound formed between Ca and S
• Ca+2 S-2
• CaS
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Polyatomic Ions• You must use parentheses when using
subscripts with a polyatomic ion
• Ex: Calcium nitrate
• Ca +2 NO3 -1
• Ca(NO3)2
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• Write the formula between ammonium and sulfate
• NH4 +1 SO4 -2
• (NH4)2 SO4
Formula writing with polyatomic Ions
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More examples
• Copper (II) and chlorine• Silver and Nitrate• Magnesium and sulfite• Calcium and sulfur• Potassium and oxygen• Ammonium and phosphate• Ammonium and chlorine
• CuCl2• AgNO3
• MgSO3
• CaS
• K2O
• (NH4)3PO4
• NH4Cl
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• In naming ionic compounds, name the cation first, then the anion.
• Cation name does not change.– If the cation can have more than one charge
(mostly transition metals), use a Roman Numeral after the element name to indicate the charge
• Ex. Iron (II) for Fe2+ or Iron (III) for Fe3+
• Monatomic anions: change the ending to -ide. (ex. Br -, Cl-, O2-)
• Polyatomic Ions: do not change the name (ex. SO4
2-, CO32-, PO4
3-
Naming ionic compounds
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Examples
• NaCl
• MgSO4
• CuSO3
• K3PO4
• Fe(NO3)2
• Ca(ClO3)2
• NH4NO2
• Al(ClO)3
• Sodium chloride• Magnesium sulfate• Copper (II) sulfite• Potassium phosphate• Iron (II) nitrate• Calcium chlorate• Ammonium nitrite• Aluminum hypochlorite
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More examples
• Lead (IV) Oxide• Ammonium Permanganate• Cobalt (II) chloride• Calcium sulfide• Lithium nitrate• Sodium acetate• Tin (II) chloride
• PbO2
• NH4MnO4
• CoCl2• CaS
• LiNO3
• NaCH3COO
• SnCl2