B - Naming conventions of compounds and ions

Define a binary ionic bond

• Ionic bond formed from only two elements

Describe the procedure for naming Binary ionic compounds

• Name of cation first

  Anion second

• -ide suffix is added to anion’s root name

Describe the procedure for naming binary ionic compounds where the metal can have multiple oxidation states in the compound

• Name of cation first

• Roman numerals are added to cation’s name

• Anion second

• -ide suffix is added to anion’s root name

Name the ion formulas, systematic and common names of Chromium

Name the ion formulas, systematic and common names of Cobalt

Name the ion formulas, systematic and common names of Copper

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Name the ion formulas, systematic and common names of Iron

Name the ion formulas, systematic and common names of Lead

Name the ion formulas, systematic and common names of Mercury

Name the ion formulas, systematic and common names of Tin

Describe the procedure for naming ionic compounds with polyatomic ions

• Cation first

• Polyatomic second with full name

  e.g. Cr₂(CO₃)₃ = Chromium(II) Carbonate

Describe the procedure for naming ionic compounds which are hydrates

• The full name of the ionic compound first

• Greek numerical prefix + ‘-hydrate’ is added to the end

• e.g. CuSO₄ • 5H₂O = Copper(II) Sulphate pentahydrate

Define a binary acid

• Acid only containing two elements

• e.g. HCl

Describe the procedure for naming binary acids

• hydro + anion root + -ic + acid

• e.g. HCl = Hydrochloric acid

Define an oxoacid

• An acid which contains a polyatomic ion with oxygen in it

• e.g. HClO₄

Describe the procedure for naming oxoacids

• oxoacid name + -ous/-ic suffix + acid

• -ous is used if the anion contains the -ite suffix

• -ic is used if the anion contains the -ate

• e.g. Nitrate (NO₃^-) becomes Nitric acid and Nitrite (NO₂^-) becomes nitrous acid

Describe the procedure for covalent compounds

• Greek prefix + Element with lower group number/higher row +++ Greek prefix + second element + -ide

• -a is dropped when naming oxides

• e.g. N₂F₄ = Dinitrogen tetrafluoride