name formula name formula ammonium Hydrogensulfate (or permanganate MnO 4 bisulfate) HSO 4 cyanide CN cyanate OCN oxalate

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1 Dr. Abel 1 Chemical Nomenclature Summary A. elements 1 through 94 You will be expected to know the names and symbols on the periodic table throughout the semester. Review these using the table in your textbook if necessary. B. common cations and anions 1. monatomic cations/anions Monatomic ions formed from elements in the main groups of the periodic table can be obtained from their position in the periodic table. Monatomic anions have the ide suffix while monatomic cations simply have the word ion at the end. For example, chloride is Cl and oxide is O 2, while lithium ion is Li + and calcium ion is Ca 2+. Monatomic ions from the transition metal and inner-transition metal groups usually have several different (and often difficult-to-predict) oxidation states and generally need a roman numeral to differentiate them [e.g. iron (II) chloride vs iron (III) chloride]. Notable exceptions are Zn 2+, Cd 2+ and Ag +, which are always found in these states when ionic and therefore do not require roman numeral designations. 2. polyatomic cations/anions You should know common polyatomic ions. It is critical not only to know the name and formula of each ion, but also its charge. Your success in lab and lecture will be substantially affected by your mastery of these formulas. name formula name formula ammonium + NH 4 carbonate 2 CO 3 mercury I**** Hg 2 2+ mercury II Hg 2+ (or bicarbonate) Hydrogencarbonate HCO 3 acetate*** C 2 H 3 O 2 chromate 2 CrO 4 hydroxide OH dichromate 2 Cr 2 O 7 hypochlorite* ClO phosphate 3 PO 4 chlorite* ClO 2 hydrogenphosphate 2 HPO 4 chlorate* ClO 3 dihydrogenphosphate H 2 PO 4 perchlorate* ClO 4 phosphite 3 PO 3 nitrite NO 2 sulfite 2 SO 3 nitrate NO 3 sulfate 2 SO 4 Hydrogensulfate (or permanganate MnO 4 bisulfate) HSO 4 cyanide CN cyanate OCN oxalate 2 C 2 O 4 thiocyanate** SCN hydride H - peroxide 2 O 2 * the same pattern exists for the bromine & iodine analogs (for example, BrO 3 is bromate and IO 4 is periodate). ** the prefix thio indicates that an oxygen has been replaced by a sulfur atom in the root ion *** acetate is also commonly written as CH 3COO **** note that the ion Hg + does not exist (the dimer is always found in nature instead)

2 Dr. Abel 2 C. names of compounds [ionic compounds, binary covalent compounds, and acids] 1. Ionic compounds (metal and nonmetal) Fundamental Rules: Formula must reflect electroneutrality Name (and write) metal first Indicate charge on variable metals using Roman numerals in parentheses A. binary (composed of two types of atoms, usually a metal and a non-metal) B. polyatomic (composed of more than two types of atoms) Examples: AgCl silver chloride Na 3 PO 4 sodium phosphate Fe(OH) 2 Iron (II) hydroxide FeAsO 4 Iron (III) arsenate 2. Hydrated Ionic Compounds - these are ionic compounds that have a specific number of water molecules associated with each formula unit. Fundamental Rules: Hydrates are named by attaching the word hydrate with a Greek numerical prefix to the systematic name of the ionic compound. The Greek prefix tells how many waters are associated with each formula unit of the compound. For example: Example MgSO 4 7 H 2 O Magnesium sulfate heptahydrate 3. Acids (one or more H + plus anion in an aqueous solution) Fundamental Rules: Formula must reflect electroneutrality The anion dictates the acid name Anion ends in Acid name (using the anion name in the blank ) -ate ic acid -ite ous acid -ide Examples: HNO3 (aq) nitric acid HNO2 (aq) nitrous acid HCl (aq) hydrochloric acid H3PO4 (aq) phosphoric acid hydro ic acid 4. Covalent compounds (non-metals) Fundamental Rules: Formula must reflect electroneutrality Name (and write) more electropositive element first More electronegative element name ends in -ide Indicate number of each element with Greek prefixes, except when redundant one mono, mon (before vowels) two di three tri four tetra five penta, pent (before vowels) six hexa, hex (before vowels) seven hepta, hept (before vowels) eight octa, oct (before vowels) nine nona, non (before vowels) ten deca, dec (before vowels) Examples: CO2 carbon dioxide CO carbon monoxide HCl hydrogen chloride H2S dihydrogen sulfide P2O5 diphosphorus pentoxide SF6 sulfur hexafluoride

3 Dr. Abel 3 Nomenclature Practice 1. Name the following ionic compounds. Remember to include Roman Numerals for transition metals: (a) K2O (b) MgH2 (c) Na3N (d) BeBr2 (e) CaO (f) AgI (g) CuF2 (h) Fe2O3 (i) CrCl3 (j) Al2S3 2. Name the following acids: (a) HI (aq) (b) HC2H3O2 (aq) (c) HClO3 (aq) 3. Write formulas for the following ionic compounds: (a) Barium chloride (e) Aluminum nitride (b) Sodium selenide (f) Copper(II) sulfide (c) Potassium phosphide (g) Calcium nitride (d) Manganese(IV) oxide (h) Aluminum hydride 4. Name the following ionic compounds which include polyatomic ions: (a) LiNO3 (b) K3PO4 (c) CuSO4 (d) NH4NO3

4 Dr. Abel 4 (e) NaH2PO4 (f) Sn(ClO3)2 (g) Fe2(CO3)3 5. Name the following molecular compounds: (a) P2O5 (b) SO2 (c) N2O (d) P4O7 (e) SF4 (f) N2O3 (g) S2Cl2 6. Give formulas for the following molecular compounds and acids: (a) Nitrogen triiodide (b) Iodine monochloride (c) Carbon monoxide (d) Tetraphosphorus hexoxide (e) Disulfur difluoride (f) Sulfur hexafluoride (g) Hydrofluoric acid (h) Hypochlorous acid 7. Give names for the following hydrates: (a) Ba(OH) 2 8H 2 O (b) Cu(ClO 4 ) 2 6H 2 O 8. Give formulas for the following hydrates: (a) chromium(iii) bromide hexahydrate (b) copper(ii) acetate monohydrate

5 Dr. Abel 5 9. Fill in the following table by providing the compound name or the chemical formula: NAME SYMBOL or FORMULA 1 Mn(OH) 2 2 MoPO 3 3 yttrium (III) sulfate octahydrate 4 N 2 O 4 5 chromium (II) nitride 6 B 2 O 3 7 P 2 S 5 8 Kr 9 Palladium 10 CoF 2.5H 2 O 11 Re(NO 2 ) 4 12 Lead (II) hypobromite 13 HClO 2 (aq) 14 nitric acid 15 Fe 3 (PO 4 ) 2 16 Zn(CN) 2 17 cyanic acid 18 sodium bicarbonate 19 Hg 2 C 2 O 4 20 ammonium acetate 21 iodide trichloride 22 rubidium sulfate 23 magnesium dichromate 24 sodium carbonate decahydrate 25 hydrosulfuric acid

6 Dr. Abel 6 KEY 1. Name the following ionic compounds. Remember to include Roman Numerals for transition metals: (a) K2O (b) MgH2 (c) Na3N (d) BeBr2 (e) CaO (f) AgI (g) CuF2 (h) Fe2O3 (i) CrCl3 (j) Al2S3 potassium oxide magnesium hydride sodium nitride beryllium bromide calcium oxide silver iodide copper (II) fluoride iron (III) oxide chromium (III) chloride aluminum sulfide 2. Name the following acids: (a) HI hydroiodic acid (b) HC2H3O2 acetic acid (c) HClO3 chloric acid 3. Write formulas for the following ionic compounds: (a) Barium chloride BaCl 2 (e) Aluminum nitride AlN (b) Sodium selenide Na 2 Se (f) Copper(II) sulfide CuS (c) Potassium phosphide K 3 P (g) Calcium nitride Ca 3 N 2 (d) Manganese(IV) oxide MnO 2 (h) Aluminum hydride AlH 3 4. Name the following ionic compounds which include polyatomic ions: (a) LiNO3 (b) K3PO4 (c) CuSO4 (d) NH4NO3 lithium nitrate potassium phosphate copper (II) sulfate ammonium nitrate

7 Dr. Abel 7 (e) NaH2PO4 sodium dihydrogen phosphate (f) Sn(ClO3)2 (g) Fe2(CO3)3 tin (II) chlorate iron (III) carbonate 5. Name the following molecular compounds: (a) P2O5 (b) SO2 (c) N2O (d) P4O7 (e) SF4 (f) N2O3 (g) S2Cl2 diphosphorous pentoxide sulfur dioxide dinitrogen monoxide tetraphosphrous heptoxide sulfur tetrafluoride dinitrogen trioxide disulfur dichloride 6. Give formulas for the following molecular compounds and acids: (a) Nitrogen triiodide NI 3 (b) Iodine monochloride (c) Carbon monoxide ICl CO (d) Tetraphosphorus hexoxide P 4 O 6 (e) Disulfur difluoride S 2 F 2 (f) Sulfur hexafluoride SF 6 (g) Hydrofluoric acid (h) Hypochlorous acid HF (aq) HClO (aq) 7. Give names for the following hydrates: (a) barium hydroxide octahydrate (b) copper(ii) perchlorate hexahydrate 8. Give formulas for the following hydrates: (a) CrBr 3 6H 2 O (b) Cu(CH 3 CO 2 ) 2 H 2 O

8 Dr. Abel 8 9. Fill in the following table by providing the compound name or the chemical formula: NAME SYMBOL or FORMULA 1 manganese (II) hydroxide Mn(OH) 2 2 Molybdenum (III) phosphite MoPO 3 3 yttrium (III) sulfate octahydrate Y 2 (SO 4 ) 3-8H 2 O 4 dinitrogen tetroxide N 2 O 4 5 chromium (II) nitride Cr 3 N 2 6 diboron trioxide B 2 O 3 7 diphosphorus pentasulfide P 2 S 5 8 Krypton Kr 9 Palladium Pd 10 cobalt (II) fluoride pentahydrate CoF 2.5H 2 O 11 rhenium (IV) nitrite Re(NO 2 ) 4 12 Lead (II) hypobromite Pb(BrO) 2 13 chlorous acid HClO 2 (aq) 14 nitric acid HNO 3 (aq) 15 iron (II) phosphate Fe 3 (PO 4 ) 2 16 zinc cyanide Zn(CN) 2 17 cyanic acid HOCN (aq) 18 sodium bicarbonate NaHCO 3 19 Mercury (I) oxalate Hg 2 C 2 O 4 20 ammonium acetate NH 4 C 2 H 3 O 2 21 iodide trichloride ICl 3 22 rubidium sulfate Rb 2 SO 4 23 magnesium dichromate MgCr 2 O 7 24 sodium carbonate decahydrate Na 2 CO 3-10H 2 O 25 hydrosulfuric acid H 2 S (aq)