Quiz for ions.pdf

Type II Cations (1 of 2) Two Table 4.3 Some Metals That Form Cations with Different Charges Metal Ion Name Older Name* Chromium Cr 2  C r s...

Type II Cations (1 of 2) Two Table 4.3 Some Metals That Form Cations with Different Charges Metal Ion Name Older Name* Chromium Cr 2  C r super 2 plus Chromium(II) Chromium 2 Chromous Chromium Cr 3  C r super 3 plus Chromium(III) Chromium 3 Chromic Iron Fe2  F e super 2 plus lron(II) Iron 2 Ferrous Iron Fe3  F e super 3 plus lron(III) Iron 3 Ferric Cobalt Co3  C o super 2 plus Cobalt(II) Cobalt 2 Cobaltous Cobalt Co2  C o super 3 plus Cobalt(III) Cobalt 3 Cobaltic Copper Cu C u super plus Copper(I) Copper 1 Cuprous Copper Cu2 C u super 2 plus Copper(II) Copper 2 Cupric © McGraw-Hill Education  Type II Cations (2 of 2) Two Table 4.3 [Continued] Metal Ion Name Older Name* Tin Sn2  S n super 2 plus Tin(II) Tin 2 Stannous Tin Sn4  S n super 4 plus Tin(IV) Tin 4 Stannic Mercury Hg22  H g sub 2 super 2 plus Mercury(I) Mercury 1 Mercurous Mercury Hg2  H g super 2 plus Mercury(II) Mercury 2 Mercuric Lead Pb2  P b super 2 plus Lead(II) Lead 2 Plumbous Lead Pb 4  P b super 4 plus Lead(IV) Lead 4 Plumbic * An older naming system substitutes the names found in this column for the name of the metal and its charge. Under this system, chromium(II) oxide is named chromous oxide. In this system, the suffix-ous indicates the ion with the lesser charge, and-ic indicates the ion with the greater charge. We will not use the older system in this text. © McGraw-Hill Education  Common Monoatomic Anions Table 4.2 Some Common Monoatomic Anions Nonmetal Symbol for Ion Base Name Anion Name Fluorine F minus F Fluor Fluoride Chlorine Cl C l minus Chlor Chloride Bromine Br  B r minus Brom Bromide Iodine I I minus Iod Iodide Oxygen O2  O, 2 minus Ox Oxide Sulfur S2  S, 2 minus Sulf Sulfide Nitrogen N3  N, 3 minus Nitr Nitride Phosphorus P3  P, 3 minus Phosph Phosphide © McGraw-Hill Education  Hydrates Common hydrate prefixes Other common hydrated ionic hemi ½ compounds and their names are as follows: mono = 1 CaSO4  ½H2O is named di = 2 tri = 3 calcium sulfate hemihydrate. tetra = 4 BaCI2  6H2O is named barium penta = 5 chloride hexahydrate. hexa = 6 CuSO4  5H2O is named hepta = 7 copper(II) sulfate pentahydrate. octa = 8 © McGraw-Hill Education  Covalent Bonding in Ionic Species: Polyatomic Ions—Common Polyatomic Ions (Anions) © McGraw-Hill Education 42  (x) Using Mass Percent Composition to Determine Empirical Formula—Example 2 2 1 mol C 1 mol H 53.31 g C   4.439 mol C 11.19 g H   11.10 mol H 12.01 g C 1.008 g H 1 mol O 35.51 g O   2.219 mol O 16.00 g O This gives us a preliminary result of C4.439H11.10O2.219. We reduce the subscripts to whole numbers as follows: we first identify the smallest number of moles and divide each of the numerical results by it: C(4.439/2.219) H (11.10/2.219) O(2.219/2.219) We then use the results to write the correct empirical formula, which in this case is C2H5O. © McGraw-Hill Education 68