Introduction To Nomenclature. based on procedures created by IUPAC which stands for the International Union of Pure and Applied Chemistry

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1 Introduction To Nomenclature the skill of determining the name and/or chemical formula of a compound based on procedures created by IUPAC which stands for the International Union of Pure and Applied Chemistry allows us to distinguish one type of compound from another based on knowledge of ionic and covalent bonding necessary for writing and balancing word and chemical equations requires a solid grasp of rules to name various types of compounds like binary ionic multivalent ionic polyatomic ionic molecular

2 NOMENCLATURE OF COMPOUNDS compounds are pure substances that are made of more than one element some examples include: TYPES OF COMPOUNDS Ionic Compounds made up of metals and nonmetals valence electrons are transferred leading to ionic bonding Molecular Compounds made valence electrons are shared leading to covalent bonding Note: Whenever you see a compound (name or formula) you must classify it as either ionic or molecular. You must make this distinction for each compound.

3 NOMENCLATURE OF BINARY IONIC COMPOUNDS Characteristics of Binary Ionic Compounds made of ions from just two different elements one ion is a metallic cation with a positive charge the other ion is a non- metallic anion with a negative charge ions will combine in fixed ratios based on the charges of the ions present in the compound so that the overall charge on the compound is zero

4 NAMING PROCEDURES FOR BINARY IONIC COMPOUNDS 1. The name of the metal cation goes first and is not changed 2. The name of the nonmetallic anion goes next and the ending of its name is changed to ide. Element Name ELEMENT Symbol fluorine F chlorine Cl bromine iodine oxygen sulfur nitrogen phosphorus carbon Anion of the Element Name ANION Symbol MgI 2 MAGNESIUM IODIDE K 3 N POTASSIUM NITRIDE Ca 2 C CALCIUM CARBIDE

5 CHEMICAL FORMULA PROCEDURES FOR BINARY IONIC COMPOUNDS Name of BINARY IONIC Compound à Chemical Formula Method Simple Particles Lewis Dot Particles Cross- Over - Draw the Lewis Dot diagram for each ion and then Practice determine how many of each ion you will need to reach a combined charge of zero. - Use these numbers as subscripts in the chemical formula. Examples Note: Unless otherwise told, for all anions in binary ionic compounds, assume the charge is equal to the number electrons that would fill the outer shell, even though in some anions are multivalent (have more than one oxidation state). - Draw one simple colour particle with the charge of the ion in it for the cation and the anion - Add particles of each until you reach a combined charge of zero. - Write the chemical formula to show the ratio of the number of particles - Write the ion symbols side by side. - Circle the number of the charge for each ion. - Put the circled superscript number into the subscript of the other ion. - Always reduce to the lowest ratio. For example: even though sulfur has four valences, for our purposes, it s ionic charge would be 2. Chemical Name Chemical Formula lithium phosphide magnesium sulfide aluminum carbide NOTE FOR LOWEST RATIO

6 BINARY COMPOUND PRACTICE MgS potassium bromide Ba 3 N 2 aluminum oxide NaI strontium fluoride Li 2 S barium chloride CaO aluminum phosphide K 2 S lithium iodide Mg 3 P 2 barium nitride NaBr magnesium fluoride Na 2 O calcium sulfide Na 3 N cesium chloride

7 NAMING PROCEDURES FOR MULTIVALENT IONIC COMPOUNDS A multivalent ionic compound is one in which the metallic element can stably form more than one cation. The Classical System You will have to memorize the Classical metals. These are the multivalent metals that will only form two cations. There are others but we will only cover these because the Classical System is not used so much anymore. Element Latin Name Lower Charge Ion Higher Charge Ion Copper cuprum cuprous Iron ferric Lead plumbum Tin stannous NOTE: you must first determine the charge of the cation before naming a multivalent Cu 2 S PbCl 4

8 The Stock System For multivalent metals that form two or more stable cations, The Stock System for naming applies. Follow the procedure below to give a Stock Name to a multivalent ionic compound. 1. First determine the charge of the cation. 2. Then write the English name of the cation followed by the value of its charge in Roman numerals in brackets. 3. Then follow proper rules to name the anion within the compound. NOTE: Copper, iron and lead can be named by both systems. Multivalent metals that form more than two cations can only be named by the stock system Fe 2 O 3 MnN 2

9 CHEMICAL FORMULA PROCEDURES FOR MULTIVALENT IONIC COMPOUNDS 1. Determine the charge on the cation as indicated by the name. 2. Proceed with the approach you like best out of the three methods presented previously. Method Simple Particles Lewis Dot Particles Cross- Over Practice Examples - Draw one simple colour particle with the charge of the ion in it for the cation and the anion - Add particles of each until you reach a combined charge of zero. - Write the chemical formula to show the ratio of the number of particles (remember the brackets around the polyatomic ion if necessary) - Draw the Lewis Dot diagram for each ion and then determine how many of each ion you will need to reach a combined charge of zero. - Use these numbers as subscripts in the chemical formula. (remember brackets around the polyatomic ion if necessary) - Write the ion symbols side by side. - Circle the number of the charge for each ion. - Put the circled superscript number into the subscript of the other ion. (remember the brackets around the polyatomic ion if necessary) - Always reduce to the lowest ratio. Chemical Name Chemical Formula manganese (III) phosphide cupric chloride copper (II) chloride lead (IV) oxide plumbic oxide

10 Multivalent Practice CuS plumbic bromide Pb 3 N 2 ferric oxide FeI 2 stannic phosphide Cu 2 S tin (II) chloride HgO lead (II) iodide CuCl 2 cuprous bromide PbO iron (III) sulfide NiCl 2 stannous oxide Cu 2 O plumbous fluoride NiO 2 tin (iv) sulfide

11 NAMING PROCEDURES FOR POLYATOMIC IONIC COMPOUNDS Chemical Formula à Name of POLYATOMIC IONIC Compound This kind of naming requires that you memorize the table below to recognize polyatomic (many atom) ions when you see them in compounds. Other than this, the rules are similar to naming binary ionic compounds. 1. The name of the metallic cation goes first and is not changed 2. The name of the non- metallic polyatomic ion goes next. NOTE THE EXCEPTION: - all polyatomic ions in the table are anions except for ammonium which is a cation so if it is found in a compound, even though it is non- metallic, the compound is still ionic. eg. Ammonium chlorate COMMON POLYATOMIC IONS NAME FORMULA ammonium hydroxide carbonate bicarbonate sulfate bisulfate nitrate phosphate chlorate

12 CHEMICAL FORMULA PROCEDURES FOR POLYATOMIC IONIC COMPOUNDS Method Simple Particles Lewis Dot Particles Cross- Over - Draw one simple colour particle with the charge of the - Draw the Lewis Dot diagram for each ion and then Practice ion in it for the cation and the anion determine how many of each ion you will need to reach a - Add particles of each until you reach a combined charge combined charge of zero. of zero. - Use these numbers as subscripts in the chemical formula. Examples - Write the chemical formula to show the ratio of the (remember the brackets around the polyatomic ion if number of particles (remember the brackets around the necessary) Note: polyatomic ion if necessary) brackets ( ) are required around all polyatomic ions, except when there is only one of them, so subscripts for these ions go after the close bracket - Write the ion symbols side by side. - Circle the number of the charge for each ion. - Put the circled superscript number into the subscript of the other ion. (remember the brackets around the polyatomic ion if necessary) - Always reduce to the lowest ratio. eg. magnesium hydroxide: Mg(OH)2 Chemical Name Chemical Formula lithium phosphate magnesium sulfate calcium carbonate NOTE FOR LOWEST RATIO

13 POLYATOMIC IONIC COMPOUND NAMING PRACTICE AlPO 4 potassium nitrate NaHCO 3 calcium carbonate Mg(OH) 2 barium chlorate K 2 SO 4 sodium bicarbonate NH 4 NO 3 tin (II) nitrate FePO 4 Watch out for multivalent compounds in here too. Cu 2 SO 4 ammonium sulfate Pb(OH) 4 cupric phosphate FeSO 4 potassium chlorate SnSO 4 lead (II) nitrate Mg 3 (PO 4 ) 2 ferric bicarbonate Na 2 CO 3

14 NOMENCLATURE PROCEDURES FOR MOLECULAR COMPOUNDS A molecular compound is one in which there are no metallic elements and the particles are called molecules which are held together by covalent bonds. 1. The first name usually begins with the element that is more left on the periodic table. 2. The second name ends in - ide just like in binary ionic compounds. 3. Greek prefixes are used in the name to tell how many atoms of each element are present in the compound. 4. The prefixes tell you the subscripts for the chemical formula of molecular compounds. Note: the prefix mono is omitted for the FIRST element in a molecular compound. eg. N 2 O 5 SO 3 carbon tetrachloride NUMBER OF ATOMS PREFIX

15 Molecular Practice BrO 3 dinitrogen trioxide NI 3 sulfur hexaflouride PCl 3 carbon monoxide PCl 5 diphosphorous pentoxide SO 2 Silicon dioxide CO 2 Sulfur trioxide NO tricarbon octahydride

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