CHM 130 Naming & Writing Chemical Formulas

Transcription

1 CHM 130 Naming & Writing Chemical s PRE - LAB Section 1: Naming Monatomic Cations Group IA and IIA cations form only one stable charge and are named for the parent metal followed by the word ion. Many other metals, especially the transition metals, can form cations with variable charges (oxidation states) so it is necessary to include a Roman numeral in parentheses to indicate the charge of the cation. Copper, for example, can form either Cu +, which we name copper (I), and Cu 2+, which we name copper (II). The aluminum ion (Al 3+ ), zinc ion (Zn 2+ ) and silver ion (Ag + ) are exceptions for transition metals and do not require the Roman numeral to be added to the name of the cation. Cr 2+ chromium (II) ion _ Al 3+ _ aluminum ion _ Co 3+ _ cobalt (III) ion _ Cu 1+ _ copper (I) ion _ Ca 2+ _ calcium ion _ Sn 4+ _ tin (IV) ion _ K + _ potassium ion _ Ni 3+ _ nickel (III) ion _ Fe 2+ _ iron (II) ion _ Pb 2+ _ lead (II) ion _ Ag + _ silver ion _ Zn 2+ _ zinc ion _ Section 2: Naming Monatomic Anions Nonmetal ions are named using the nonmetal stem plus the suffix ide. For example, Cl - is named chloride ion; N 3- is named nitride ion. O _ oxide ion _ Br - _ bromide ion _ H - _ hydride ion _ I - _ iodide ion _ S _ sulfide ion _ P 3- _ phosphide ion _ Section 3: Naming Polyatomic Ions Polyatomic anions generally contain one or more elements combined with oxygen and are often called oxyanions. The most common oxyanions have the name ending in ate (root form) SO 4 _ sulfate ion _ PO 4 3- _ phosphate ion _ CO 3 _ carbonate ion _ NO 3 - _ nitrate ion _ BrO 3 1- ClO 3 1- bromate ion IO 3 1- chlorate ion iodate ion _ 1

2 The prefix hypo- with ending - ite indicates two less oxygen atom than the oxyanion ending in ate (the root form); The ending ite indicates one less oxygen atom than the oxyanion ending in ate (the root form); The root form of the oxyanions as listed in the section 3 ending with -ate; The prefix per- with ending -ate indicates one more oxygen atom than the oxyanion ending in ate (the root form) ClO 4 - _ perchlorate ion_ ClO 3 - _ chlorate ion _ ClO 2 - _ chlorite ion _ SO 4 _ sulfate ion _ SO 3 _ sulfite ion _ SO 2 _ hyposulfite ion _ ClO - _ hypochlorite ion _ Anions derived by adding H + to an oxyanion are named by adding as a prefix the word hydrogen or dihydrogen, as appropriate. The charge on the ion will increase by + 1 for each hydrogen added to the base oxyanion. HSO 4 - _ hydrogen sulfate ion _ HCO 3 - _ hydrogen carbonate ion _ HPO 3 _ hydrogen phosphate ion _ H 2 PO 4 - _ dihydrogen phosphate ion _ Polyatomic anions that are exceptions and do not fit into any of the above: CN - _ cyanide ion _ OH - _ hydroxide ion _ C 2 _ carbide ion _ O 2 _ peroxide ion _ There is only one polyatomic cation we need to know for now: NH + 4 _ ammonium ion _ 2

3 LAB REPORT NAME: Section 4: Writing s of Ionic Compounds from the Monatomic Ions. The charges of the ions must sum to equal zero for the ionic compound. Write the name of each compound using the IUPAC rules for naming binary compounds with a single-charge metal. Cl O N 3- Se As 3 Na + Cl Na + O Na + N 3- Na + Se Na + As 3 Na + NaCl Na 2 O Na 3 N Na 2 Se Na 3 As Sodium Chloride Ca 2+ Cl Sodium Oxide Ca 2+ O Sodium Nitride Ca 2+ N 3- Sodium Selenide Ca 2+ Se Sodium Arsenide Ca 2+ As 3 Ca 2+ CaCl 2 CaO Ca 3 N 2 CaSe Ca 3 As 2 Calcium Chloride Al 3+ Cl Calcium Oxide Al 3+ O Calcium Nitride Al 3+ N 3- Calcium Selenide Al 3+ Se Calcium Arsenide Al 3+ As 3 Al 3+ AlCl 3 Al 2 O 3 AlN Al 2 Se 3 AlAs Aluminum Chloride Aluminum Oxide Aluminum Nitride Aluminum Selenide Aluminum Arsenide Section 5: Writing s of Ionic Compounds Formed with Polyatomic Ions. The charges of the ions must sum to equal zero for the ionic compound. If more than one of the polyatomic ions is required, parentheses should be added around the formula of the polyatomic ion and a subscript placed after the parentheses to allow the charges in the ionic compound to sum to zero. Write the name of each compound using the rules for naming of compounds in IUPAC category two ternary ionic compounds. CO 3 OH - PO 3-4 SO 4 NO 3 Cu + CO 3 Cu + OH - Cu + PO 3-4 Cu + SO 4 Cu + NO 3 Cu + Cu 2 CO 3 CuOH Cu 3 PO 4 Cu 2 SO 4 CuNO 3 Copper (I) Carbonate NH 4 + CO 3 Copper (I) Hydroxide NH 4 + OH - Copper (I) Phosphate NH 4 + PO 4 3- Copper (I) Sulfate NH 4 + SO 4 Copper (I) Nitrate NH 4 + NO 3 NH 4 + (NH 4 ) 2 CO 3 NH 4 OH (NH 4 ) 3 PO 4 (NH 4 ) 2 SO 4 NH 4 NO 3 Ammonium Carbonate Pb 2+ CO 3 Ammonium Hydroxide Pb 2+ OH - Ammonium Phosphate Pb 2+ PO 4 3- Ammonium Sulfate Pb 2+ SO 4 Ammonium Nitrate Pb 2+ NO 3 Pb 2+ PbCO 3 Pb(OH) 2 Pb 3 (PO 4 ) 2 PbSO 4 Pb(NO 3 ) 2 Lead (II) Carbonate Al 3+ CO 3 Lead (II) Hydroxide Al 3+ OH - Lead (II) Phosphate Al 3+ PO 4 3- Lead (II) Sulfate Al 3+ SO 4 Lead (II) Nitrate Al 3+ NO 3 Al 3+ Al 2 (CO 3 ) 3 Al(OH) 3 AlPO 4 Al 2 (SO 4 ) 3 Al(NO 3 ) 3 Aluminum Carbonate Aluminum Hydroxide Aluminum Phosphate Aluminum Sulfate Aluminum Nitrate 3

4 the following ionic compounds. Watch out for metals that can take a variable oxidation state. NH 4 Br _ ammonium bromide _ CrO 3 _ chromium (VI) oxide _ Co(NO 2 ) 2 _ cobalt (II) nitrite _ CaCO 3 _ calcium carbonate _ KCl _ potassium chloride _ FeSO 4 _ iron (II) sulfate _ MgCl 2 _ magnesium chloride _ FeCl 3 _ iron (III) chloride _ Zn 3 (PO 5 ) 2 _ zinc perphosphate _ Al(OH) 3 _ aluminum hydroxide _ CuC 2 H 3 O 2 _ copper (I) acetate _ NaClO _ sodium hypochlorite _ Fe 2 O 3 _ iron (III) oxide _ NaHSO 4 _ sodium hydrogen sulfate _ Mg(NO 3 ) 2 _ magnesium nitrate _ CuSO 5 _ copper (II) persulfate _ NaHCO 3 _ sodium hydrogen carbonate _ NiBr 3 _ nickel (III) bromide _ Be(NO 3 ) 2 _ beryllium nitrate _ AuCl 3 _ gold (III) chloride _ Cu 3 P _ copper (I) phosphide _ NH 4 NO 2 _ ammonium nitrite _ Cu(C 2 H 3 O 2 ) 2 _ copper (II) acetate _ PbSO 3 _ lead (II) sulfite _ SnS 2 _ tin (IV) sulfide _ (NH 4 ) 3 PO 4 _ ammonium phosphate _ Write the chemical formula for the following ionic compounds: magnesium sulfate _ MgSO 4 _ silver sulfide _ Ag 2 S _ ammonium perphosphate _ (NH 4 ) 3 PO 5 _ iron (III) oxide _ Fe 2 O 3 _ potassium nitrite _ KNO 2 _ aluminum hyposulfite _ Al 2 (SO 2 ) 3 _ lead (IV) peroxide _ Pb(O 2 ) 2 _ aluminum sulfite _ Al 2 (SO 3 ) 3 _ barium hydrogen carbonate _Ba(HCO 3 ) 2 _ lead (II) nitrate _ Pb(NO 3 ) 2 _ iron (II) oxide _ FeO _ calcium chloride _ CaCl 2 _ magnesium hydroxide _ Mg(OH) 2 _ copper (II) hypochlorite _Cu(ClO) 2 _ potassium carbide _ K 2 C 2 _ lithium cyanide _ LiCN _ 4

5 Binary Molecular Compounds Section 6: the Following Binary Molecular Compounds. A binary molecular compound is composed of two nonmetal elements. (Nonmental elements usually found to the right of the staircase in the periodic table) The first element in the compound is named using the parent name and the second element in the formula uses the stem of the parent name with the suffix ending with ide. The number of atoms of each element is indicated by Greek prefixes with an exception being the prefix mono- is never used in naming the first element. For example, P 4 S 7 is named tetraphosphorus heptasulfide. Write the name of each binary molecular compound. Watch out for names from the Internet! SO 3 _ sulfur trioxide _ NO _ nitrogen monoxide _ N 2 O 5 _ dinitrogen pentoxide _ PCl 5 _phosphorous pentachloride _ SCl 6 _ sulfur hexachloride _ CCl 4 _ carbon tetrachloride _ CS 2 _ carbon disulfide _ N 2 O _ dinitrogen monoxide _ N 2 O 4 _ dinitrogen tetroxide _ PCl 3 _ phosphorous trichloride _ NH 3 _ nitrogen trihydride (ammonia is OK)_ P 2 O 5 _ diphosphorous pentoxide _ SiO 2 _ silicon dioxide _ OF 2 _ oxygen difluoride _ Write the chemical formula for the following binary molecular compounds: carbon monoxide _ CO _ dinitrogen pentoxide _ N 2 O 5 _ tetraphosphorous decoxide _ P 4 O 10 _ nitrogen tribromide _ NBr 3 _ octaselenium pentoxide _ Se 8 O 5 _ tetraiodine decoxide _ I 4 O 10 _ boron trichloride _ BCl 3 _ silicon dioxide _ SiO 2 _ disulfur hexaiodide _ S 2 I 6 _ triiodine nonafluoride _ I 3 F 9 _ dibromine tetroxide _ Br 2 O 4 _ dioxygen heptafluoride _ O 2 F 7 _ 5

6 Binary Acids. A binary acid is an aqueous solution of a compound containing hydrogen and a nonmetal. A more inclusive definition of a binary acid is an acid that does not contain oxygen. The chemical formula always begins with H and must include (aq) at the end. The binary acids are systematically named by using the prefix hydro- before the nonmetal stem and adding the suffix ic acid. For example, HCl (aq) is named hydrochloric acid. or write the formula for the following binary acids: HF(aq) _ hydrofluoric acid _ H 2 S(aq) _ hydrosulfuric acid _ HI(aq) _ hydroiodic acid _ hydrochloric acid _ HCl _ hydrophosphoric acid _ H 3 P _ hydrobromic acid _ HBr _ Oxyacids. An oxyacid is a compound containing hydrogen and an oxyanion. The chemical formula always begins with H and ends with O. The oxyacid are named systematically as follows: Hydrogen always represents as an acid, the nonmetal stem ending of the oxyanion in an acid form will transform from -ate to ic; -ite to ous. For example: H 2 CO 3 -- H + represents the acid -- CO 3-2 is carbonate ion, replace ate with ic ---Carbonic acid H 2 SO 2 -- H + represents the acid -- SO 2 is hyposulfite ion, replacing ite with ous -- hyposulfurous acid. the following oxyacids: HNO 2 _ nitrous acid _ HNO 3 _ nitric acid _ HBrO_ hypobromous acid _ HBrO 3 _ bromic acid _ H 3 PO 4 _ phosphoric acid _ H 2 SO 3 _ sulfurous acid _ HBrO 2 _ bromous acid _ HBrO 4 _ perbromic acid _ Write the formula for the following oxyacids: sulfuric acid _ H 2 SO 4 _ nitric acid _ HNO 3 _ hypoiodous acid _ HIO _ perchloric acid _ HClO 4 _ acetic acid _ HC 2 H 3 O 2 _ phosphorous acid _ H 3 PO 3 _ carbonic acid _ H 2 CO 3 _ nitrous acid _ HNO 2 _ 6