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Chemistry 11: Naming Binary Inorganic Compounds Naming Binary ionic compounds with one oxidation state (group 1, II, aluminum, zinc, cadmium, silver) Recall that ionic compounds consist of a metal and a nonmetal. When writing the name of an ionic compound: The name of the __________ is written first The stem of the non-metal follows, followed by ________ What are the stems for: o Oxygen o Hydrogen o Nitrogen o Chlorine o Sulfur o Fluorine Ex. MgCl2 __________________________ Li3N _________________________ Al2S3 __________________________ Writing Formulas of Binary ionic compounds 1. Write the symbols of the elements with the metal first, then the non-metal. Write the ionic charge of each element, above and to the right, for each element. Ca2+ P32. Criss-cross the numbers down to become subscripts on the opposite element. Drop the charges Ca2+ P3Ca P 3. Cancel to the lowest ratio by dividing by the largest common factor. Example 1: beryllium oxide Metals with multiple oxidation states Many transition metals have more than one possible oxidation state. Element Symbol Copper Iron Lead Mercury Tin Antimony Cobalt Gold Cu Fe Pb Hg Sn Sb Co Au Lower Oxidation State +1 +2 +2 +1 +2 +3 +2 +1 Classical Stock Cuprous Ferrous Plumbous Mercurous Stannous Stibnous Cobaltous Aurous (I) (II) (II) (I) (II) (III) (II) (I) Higher Oxidation State +2 +3 +4 +2 +4 +5 +3 +3 Classical Stock Cupric Ferric Plumbic Mercuric Stannic Stibnic Cobaltic Auric (II) (III) (IV) (II) (IV) (V) (III) (III) 1 Balancing Charges Method to give names from Formulas AuN Fe2O3 To write formulas from names Iron (III) chloride Naming of Compounds that contain Polyatomic Ions Polyatomic ions are ___________ molecules. The atoms within a polyatomic ion are usually very tightly bound together, so the ion retains its identity within ionic compounds and over the course of many chemical reactions. o o o o Compounds formed with polyatomic ions must have _________________________, just like those formed from monatomic ions This means that in many compounds there will be more than one unit of a given polyatomic ion This is reflected in the formulas of these compounds by the use of ______________. The subscript after the parentheses tells you how many units of that ion you have Chart of Polyatomic Ions Valence = +1 Name Ammonium Ion NH4+ Ion CNC2H3O2ClOClO2ClO3ClO4HCO3- Ion CO32CrO42Cr2O72- Name cyanide acetate (also CH3COO-) hypochlorite chlorite chlorate perchlorate bicarbonate Valence = -1 Ion MnO4NO2NO3OH- Valence = -2 Ion O22SO32SO42- Name carbonate chromate dichromate Ion PO43- Name permanganate nitrite nitrate hydroxide Name peroxide sulfite sulfate Valence = -3 Name phosphate 2 For those ions that contain oxygen, there is a pattern for their naming: ClO- hypochlorite ClO2- chlorite ClO3- chlorate ClO4- perchlorate It is easiest to remember those formulae that end in “ate” and derive the others from it. The compound that contains __________________ will have an “ite” suffix. One fewer oxygen than the “ite” compound will have a _________ prefix. The compound that contains one more oxygen than the “ate” compound will have a _________ prefix. Common names of some ionic compounds and their uses IUPAC Name Chemical Formula Mg(OH)2 Common name Milk of magnesia Use of property Antacid N2O Laughing gas Na2CO3 Washing soda Used in dentistry as an anaesthetic General cleaner NaCl Table salt Enhancing flavour NaHCO3 Baking soda NaOH Lye Making baked goods rise Neutralizing acids CaCl2 Road Salt K2CO3 Potash Lowers the melting point of water Animal feed, fertilizer Practice I. Give names for the following compounds. These are all group I, and II metals. They only ever have one charge. Find it from your periodic tables. Metal name first then nonmetal with –ide ending. a. Li2O _____________________________ b. MgS _____________________________ c. CaF2 _____________________________ d. BeF2 _____________________________ e. K3P ______________________________ f. Mg3P2 ____________________________ g. CaO ______________________________ h. Na3P _______________________________ 3 i. Ba3N2 ______________________________ II. Give names for the following compounds. These are all group I, and II metals. They only ever have one charge. Find it from your periodic tables. Metal name first then the polyatomic ion name. LiNO3 _____________________________ MgSO4 ____________________________ Ca3(PO4)2 __________________________ Be(OH)2 ___________________________ KClO3 ______________________________ MgCN ____________________________ Li2CO3_____________________________ NaCl04 _____________________________ BaCrO4 ____________________________ K2Cr2O7____________________________ LiCl03 _____________________________ Mg(MnO4)2 ________________________ III. Write formulas for the following compounds. Find the charges and use the criss-cross method. a. magnesium oxide _________________ k. strontium sulfide b. barium nitride l. __________________ c. potassium sulfide __________________ d. calcium bromide _________ calcium phosphide _________ m. magnesium chloride __________ __________________ e. aluminum sulfide __________________ f. beryllium oxide __________________ g. sodium fluoride __________________ h. lithium nitride ____________________ IV. Give names for the the following compounds. These metals can have more than one oxidation state (charge). You must use the balancing charges method to find the charge (Roman numeral). Polyatomic ions are also in this section. Naming with group 3-12 metals (Roman numeral) and polyatomic ions. Pb3(PO4)2 _______________________________________________ CuCl Fe2O3 ______________________________________________ ______________________________________________ Pb(CO3)2 ______________________________________________ Sn(OH)2 ______________________________________________ 4 SnSO3 ______________________________________________ HgCl2 ______________________________________________ Co(CN)2 ______________________________________________ CuO ______________________________________________ Pb(ClO3)4 ______________________________________________ Mixed Names and Formulas (All types) Iron (III) hydroxide __________________ Silver chloride _____________________ sodium hydroxide ____________________ lithium oxide _________________________ cobalt (III) bicarbonate __________________ aluminum sulfide _______________________ ammonium cyanide ______________________ iron (III) phosphide _______________________ vanadium (V) phosphate __________________ sodium permanganate ____________________ manganese (III) fluoride __________________ Ba(OH)2 _________________________________________ Mg3(PO4)2 ________________________________________ Sn(CO3)2 _________________________________________ Sr(NO2)2 _________________________________________ Sn(OH)2 __________________________________________ CaSO4 ___________________________________________ FeCl2 _______________________________________ SnF4 ________________________________________ FeS ________________________________________ Ni2O3 ________________________________________ Be(NO3)2 ______________________________________ Ni2S3 _________________________________________ K2O __________________________________________ AgBr __________________________________________ Zn3(PO4)\2_______________________________________ CuCO3 __________________________________________ NiSe ___________________________________________ Mn(CO3)2_______________________________________ Pb3N4_________________________________________ 5 Sn(OH)2 _______________________________________ 6