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CHEM-001 Chapter 06 Nomenclature of Inorganic Compounds Chapter 6 Hein and Arena Eugene Passer Chemistry Department Version 1.1 Bronx Community1 College © John Wiley and Sons, Inc Elements and Ions 2 The formula for most elements is the symbol of the element. Sodium Na Potassium K Zinc Zn Argon Ar Mercury Hg Lead Pb Calcium Ca 3 These 7 elements are found in nature as diatomic molecules. Hydrogen H2 Nitrogen N2 Oxygen O2 Fluorine F2 Chlorine Cl2 Bromine Br2 Iodine I2 4 Formation of Ions 5 Positive Ion Formation: Loss of an Electron(s) From a Neutral Atom Na Na+ + e- Ca Ca2+ + 2e- Al Al3+ + 3e- 6 Naming Cations 7 Cations are named the same as their parent atoms. 8 Atom sodium (Na) Cation Na+ Name of sodium ion Cation 9 Atom calcium (Ca) Cation Ca2+ Name of calcium ion Cation 10 Negative Ion Formation: Gain of an Electron(s) by a Neutral Atom Cl + e- Cl- O + 2e- O2- N + 3e- N3- 11 Naming Anions 12 A monatomic anion consists of one element and has the stem of the parent element name with an –ide ending 13 Atom fluorine (F) Anion F- stem Name of fluoride ion Anion 14 Atom oxygen (O) Anion O2- stem Name of oxide ion Anion 15 Ions are always formed by adding or removing one or more electrons to or from a neutral atom. 16 Most often ions are formed when metals combine with nonmetals to form ionic solids with ionic bonds. 17 The charge on an ion can be predicted from its position in the periodic table. 18 elements of elementselements elementsof of of elements of Group Group IIA have Groupa Group VAGroup have VIA haveVIIAa havea a IA have a +1 charge +2 charge -3 charge-2 charge-1 charge 19 Writing Formulas From Names of Compounds 20 A chemical compound must have a net charge of zero. 21 If the compound contains ions, then the charges on all of the ions must add to zero. 22 Write the formula of calcium chloride. Step 1. Write down the formulas of the ions. Ca2+ Cl- Step 2. Combine the smallest numbers of Ca2+ and Cl- so that the sum of the charges The cationThe is anion is writtenequalswritten first. zero.second. (Ca2+) + 2(Cl-) = 0 (2+) + 2(1-) = 0 The lowest common multiple The correct formula is CaCl2 of +2 and –1 23is 2 Write the formula of barium phosphide. Step 1. Write down the formulas of the ions. Ba2+ P3- Step 2. Combine the smallest numbers of Ba2+ and P3- so that the sum of the charges The cationThe anionis is writtenwrittenequals first. second.zero. 3(Ba2+) + 2(P3-) = 0 3(2+) + 2(3-) = 0 The lowest common multiple The correct formula is Ba3P2 of +2 and –3 24is 6 Binary Compounds 25 Binary compounds contain two different elements only. 26 Naming Binary Compounds 27 Binary ionic compounds consist of a metal combined with a non-metal. 28 Binary Ionic Compounds Containing a Metal Forming Only One Type of Cation 29 • The chemical name is composed of the name of the metal followed by the name of the nonmetal which has been modified to an identifying stem plus the suffix –ide. • The number of atoms of each element present is not expressed in the name. 30 Name of Metal + Stem of Nonmetal with -ide ending 31 Examples 32 Compound NaCl name of metal Name sodium chloride nonmetal stem 33 Compound MgCl2 name of metal Name magnesium chloride nonmetal stem 34 Binary Ionic Compounds Containing a Metal That Can Form Two or More Types of Cations 35 The Stock System 36 In IUPACthe Stock devisedSystem thethe Stockcharge Systemon theof cation is designatednomenclatureby toa nameRoman compoundsnumeral placed of in parenthesesmetals thatimmediately have more thanfollowing one typethe ofname of thecation.metal. Cation +1 +2 +3 +4 +5 Charge Roman I II III IV V Numeral The stem of the nonmetal name ends in -ide37 . Stock System LowerLower ChargeCharge HigherHigher Charge Charge Element Formula Name Formula Name Copper Cu+ copper (I) Cu2+ copper (II) Iron Fe2+ iron(II) Fe3+ iron(III) Lead Pb2+ lead (II) Pb4+ lead(IV) 2+ 2+ Mercury Hg2 mercury(I) Hg mercury(II) Tin Sn2+ Tin(II) Sn4+ Tin (IV) 38 Examples 39 iron(II) chloride FeCl2 +2 -1 iron(II) chloride compoundionion charge name name iron(III) chloride FeCl3 +3 -1 iron(III) chloride40 Binary Compounds Containing Two Nonmetals 41 Compounds between nonmetals are molecular, not ionic. 42 In a compound formed between two nonmetals, the element that appears first in the formula is named first. 43 Prefixes 44 Prefixes are used in a name to denote the number of atoms of each element present in a formula unit. Mono is rarely used when naming the first element, but mono is used in naming the second element (e.g. CO is carbon monoxide). • mono = 1 • hexa = 6 • di = 2 • hepta = 7 • tri = 3 • octa = 8 • tetra = 4 • nona = 9 • penta = 5 • deca = 10 45 Examples 46 dinitrogen trioxide N2O3 indicates two indicates three nitrogen atoms oxygen atoms 47 dichlorine heptaoxide Cl2O7 indicates two indicates seven chlorine atoms oxygen atoms Why does chlorine appear first in the formula and oxygen second? Oxygen is more electronegative than chlorine; the more electronegative element appears second in the formula and the name. Electronegativity is the relative ability of an atom in a bond to attract the bonding electrons toward itself and away from the atom it is bonded to. 48 Electronegativity increases from the lower left to the upper right for representative elements. 49 Step by Step Approach to Naming a Binary Molecular Compounds, PCl5 Step 1 • Phosphorous and chlorine are nonmetals so the rules for naming a binary molecular compound applies. • Phosphorous is named first and chlorine second. (recall Cl is more electronegative: See 11.6). Therefore, in the name, phosphorous remains phosphorous and chlorine becomes chloride. 50 Step by Step Approach to Naming Binary Molecular Compounds, Cont. Step 2 • No prefix is needed for phosphorous because there is only one phosphorous atom. The prefix penta- is used with chloride because there are 5 chlorine atoms present. Step 3 • The name is phosphorous pentachloride. 51 Examples 52 Cl2O3 dichlorine trioxide 53 N2O3 dinitrogen trioxide 54 Acids Derived from Binary Compounds of Hydrogen 55 Certain binary hydrogen compounds, when dissolved in water, form solutions that have acid properties. • The aqueous solutions of these compounds are given acid names. 56 Pure solid or gaseous compound HCl Hydrogen Chloride Dissolved in water HCl Hydrochloric acid 57 • To write the formula of binary acids write the symbol of hydrogen first. • After hydrogen, write the symbol of the second element; typically a nonmetal. • To name binary acids, place the prefix hydro- in front of the stem of the nonmetal name. • Then place the suffix -ic after the stem of the nonmetal name followed by acid. 58 Examples 59 Pure Solid or Gaseous Compound HCl hydrogen chloride 60 Dissolved in Water HCl hydrochloric acid 61 Pure Solis or Gaseous Compound HI hydrogen iodide 62 Dissolved in Water HI hydroiodic acid 63 Naming Compounds Containing Polyatomic Ions 64 A polyatomic ion is an ion that contains two or more elements. The nitrate anion is an example. - NO3 65 66 • When naming a compound containing a polyatomic ion, name the cation first and then name the anion. Na23 CO In writing the formula, the cation(s) appears first followed by the polyatomic ion. 67 Oxy-acids 68 Oxy-acids contain hydrogen, a nonmetal, or a metal, and oxygen. HClO3 or H2CrO4 69 Hydrogen in an The word acid in oxy-acid is not the name indicates expressed in the the presence of acid name. hydrogen. 70 Naming Oxy-Acids of Chlorine HClO4 Perchloric Acid +1 oxygen HClO3 Chloric Acid Root Acid HClO2 Chlorous Acid - 1 oxygen HClO Hypochlorous Acid -2 oxygens HCl Hydrochloric Acid No oxygen* * Please note HCl is not an oxy-acid Prefixes and Suffixes of Oxy-anions 72 Naming Oxy-Anions of Chlorine - ClO4 Perchlorate +1 oxygen - ClO3 Chlorate Root Base - ClO2 Chlorite - 1 oxygen ClO- Hypochlorite -2 oxygens Cl- Chloride No oxygen* * Please note Cl- is not an oxy-anion 74 75.
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