Naming Ionic Compounds. Charges Group 1A +1 Group 2A +2 Group 3A +3 Group 4A N/A Group 5A -3...

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Naming Ionic Compounds

Transcript of 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