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Naming and Writing Formulas for Compounds

Naming and Writing Formulas for Compounds. Two Systems for naming: Stock (Roman numerals) Old System . Ionic Compounds. Binary Compounds Write the name of the positive ion 1 st

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Naming and Writing Formulas for Compounds

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  1. Naming and WritingFormulasfor Compounds

  2. Two Systems for naming: Stock (Roman numerals) Old System Ionic Compounds

  3. Binary Compounds Write the name of the positive ion 1st Check to see if it has more than one oxidation #. If it does determine the charge and use a Roman numeral to designate the charge Write the root name of the negative ion. Change the ending to an –ide ending. Compounds with Polyatomic ions Same steps as binary for positive ion For negative ion, just write the name of the polyatomic *** DO NOT ADD THE ENDING –IDE Stock System

  4. --Ions w/ more than one oxidation # (transition metals, groups 3-12) Hg Cu Pb Sn Cr Fe ***Note: Zn is +2 Ag is +1 Assign an oxidation # to the negative ion Ex. Hg Cl-1 Multiply the oxidation # by the subscript Ex. Hg Cl-1 1 Since the compound is neutral the overall charge must = 0 Ex. Hg+1 Cl-1 = 0 1 1 +1-1 = 0 Determining Charge for Ions with Variable Oxidation #’s

  5. Sodium Chloride Strontium chloride Sodium hydroxide Copper (II) chloride Lead (IV) oxide Copper (I) hydroxide Mercury (II) bromide Aluminum oxide Strontium oxide Mercury (II) oxide Remember…. Roman numerals are only used for those ions with more than one charge!!!!!!!! Practice • NaCl • SrCl2 • NaOH • CuCl2 • PbO2 • CuOH • HgBr2 • Al2O3 • SrO • HgO

  6. 1. Write the name of the positive ion 1st. Check to see if the ion has more than one oxidation #. If it does, determine the charge and add one of the following endings –ous for lower -ic for higher Remember… -ous is less -ic is more Write the root of the negative ion Add –ide if it is an element Write the name of the ion if it is a polyatomic Old System

  7. Cu +1 cuprous Hg+1 mercurous Fe+2 ferrous Pb+2 plumbous Sn+2 stannous Cu+2 cupric Hg+2 mercuric Fe+3 ferric Pb+4 plumbic Sn+4 stannic Old System Names

  8. Hg(OH)2 SnCl2 PbO CuCl FeO Fe2O3 7. HgOH Mercuric hydroxide Stannous chloride Plumbous oxide Cuprous chloride Ferrous oxide Ferric oxide 7. Mercurous hydroxide Examples

  9. Writing Formulas for Ionic Compounds

  10. Write the symbols for the ions side by side, with the positive ion 1st • Cross over charges diagonally to give subscripts (Subscripts tell how many of each element are in the compound). • Check the subscripts to make sure the compound is neutral. • Do not write subscripts that are 1 (they are understood) • Do not write subscripts that are the same # • If the subscripts are divisible by the same #, reduce them to give the simplest ratio • If the compound contains a polyatomic ion that will have a subscript from crossing over, you must PUT PARENTHESIS AROUND IT!!!!

  11. Write the formula for: Strontium Chloride Sr+2 Cl -1 SrCl2 **subscripts that are 1 are not written Write the formula for: Magnesium Oxide Mg +2 O-2 MgO ** subscripts that are the same # are not written Examples

  12. Write the formula for: Lead (IV) oxide ** remember, the Roman numeral tells you the oxidation # Pb+4 O-2 Pb2O4 (these can be reduced) PbO2 Write the formula for: Stannic sulfate Sn +4 SO4-2 (the –ic ending tells you that it is tin’s higher charge) Sn(SO4)2 ** the subscripts can be reduced and sulfate must have parenthesis because it is a polyatomic ion and it has a subscript that will be written More Examples

  13. Lithium bromide Strontium sulfide Aluminum oxide Mercury (II) hydroxide Plumbic carbonate Ferrous oxide Ferric oxide Ammonium sulfate Write the formulas for: • LiBr • SrS • Al2O3 • Hg(OH)2 • Pb (CO3)2 • FeO • Fe2O3 • (NH4)2(SO4)

  14. ONLY USED FOR NAMING COVALENTLY BONDED COMPOUNDS (Remember… this will be two nonmetals bonded together) Write the name of the least electronegative element 1st. A prefix is used w/the name of the 1st element only if more than one atom is present The second element always get a prefix Then write the root and add -ide Naming Binary Molecular Formulas

  15. Number Prefix 1 Mono 2 Di 3 Tri 4 Tetra 5 Penta 6 Hexa 7 Hepta 8 Octa 9 Nona 10 Deca Numerical Prefixes for Binary Molecular

  16. Examples • Name: • N2O Dinitrogen monoxide • NO Nitrogen monoxide • N2O3 Dinitrogen trioxide

  17. Use the prefixes to tell you how many of each element is in the compound. Examples: Disulfur trioxide S2O3 Carbon monoxide CO Carbon tetrachloride CCl4 Writing Formulas for Binary Molecular

  18. Naming Acids

  19. Recognizing Acids • At this very beginning level, you will recognize an acid by the fact that its formula starts with H, as in these examples: • HClHNO3H2SO4HClO3H3BO3

  20. For acids in which the anion is an element, the name of the acid begins with the prefix hydro- - The acid’s name also includes the root name of the anion and the word acid In addition, you must change the suffix of the anion to –ic Ex: HCl Hydrochloric Acid For acids in which the anion is a polyatomic, the prefix hydro- IS NOT USED!!! Write the name of the polyatomic and: -Change –ate to –ic (or to –oric/-uric for a few cases) -And -ite to -ous Then write the word acid. The name of an acid is derived from its anion:

  21. Phosphoric Acid • Carbonic Acid • Sulfuric Acid • Iodic Acid • Hydrofluoric Acid • Nitrous Acid • Name the following acids: • 1) H3PO4 • 2) H2CO3 • 3) H2SO4 • 4) HIO3 • 5) HF • 6) HNO2

  22. ***Remember… the prefix “hydro-”means its an element bonded with hydrogen***if “hydro-” is not present, then a polyatomic is bonded with hydrogen Write the formula for these acids: • hydrobromic acid • nitric acid • sulfurous acid • phosphorous acid • acetic acid • HBr • HNO3 • H2SO4 • H3PO3 • HC2H3O2

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