PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion World of Chemistry: Chapter 4 Nomenclature HC 2 H 3 O 2 Acetic Acid Common Names Common Names A lot of chemicals have common lot of chemicals have common names as well as the proper names as well as the proper IUPAC IUPAC (International Union of Pure name. and Applied Chemistry) name. Chemicals that should always be Chemicals that should always be named by common name and never named by common name and named by the IUPAC method are: never named by the IUPAC H 2 O water, not dihydrogen method monoxide are: NH H 2 O water, 3 ammonia, not not dihydrogen nitrogen trihydride monoxide NH 3 ammonia, not nitrogen trihydride COMPOUNDS FORMED FROM IONS CATION + ANION COMPOUND Na + + Cl - NaCl Predicting Charges on Monatomic Ions KNOW THESE!!!! +1 +2 +3-3 -2-1 0 A neutral compound requires equal number of + and - charges. Cd +2 Binary Ionic Compounds contains positive ion(s) (cation) and negative ion(s) (anion) name the ions to name the ionic compounds Binary Ionic Compounds Two types metals that form only one cation (type I) metals that can form two or more cations (type II), usually transition metals 1
IONIC COMPOUNDS Some Ionic Compounds NH 4 + Cl - ammonium chloride NH 4 Cl Ca 2+ + 2 F - CaF 2 Mg 2+ + N 3- Mg 3 N 2 magnesium nitride Mg 2+ + Cl 1- MgCl 2 magnesium chloride calcium fluoride Formulas of Ionic Compounds Formulas of ionic compounds are determined from the charges on the ions. atoms ions e - Na + F Na + F - NaF sodium + fluorine sodium fluoride formula Charge balance: 1+ 1- = 0 Writing a Formula Write the formula for the ionic compound that will form between Ba 2+ and Cl. Solution: 1. Balance charge with + and ions 2. Write the positive ion of metal first, and then negative ion Ba 2+ Cl Cl 3. Write the number of ions needed as subscripts BaCl 2 Write the correct formula for the compounds containing the following ions: 1. Na +, S 2- a) NaS b) Na 2 S c) NaS 2 2. Al 3+, Cl - a) AlCl 3 b) AlCl c) Al 3 Cl 3. Mg 2+, N 3- a) MgN b) Mg 2 N 3 c) Mg 3 N 2 Naming Compounds Binary Ionic Compounds: 1. Cation first, then anion 2. Monatomic cation = name of the element Ca 2+ = calcium ion 3. Monatomic anion = root + -ide Cl - = chloride CaCl 2 = calcium chloride 2
Naming Binary Ionic Compounds Examples: NaCl sodium chloride Complete the names of the following binary compounds: Na 3 N sodium nitride ZnI 2 zinc iodide KBr potassium bromide Al 2 O 3 aluminum oxide Al 2 O 3 aluminum oxide MgS magnesium sulfide Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or 2+ 2+ or 3+ Cu +, Cu 2+ Fe 2+, Fe 3+ copper (I) ion iron (II) ion copper (II) ion iron (III) ion Names of Variable Ions These elements REQUIRE Roman Numerals because they can have more than one possible charge: anything except Group 1A, 2A, Ag, Zn, Cd, and Al (You should already know the charges on these!) Or another way to say it is: Transition metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral. FeCl 3 (Fe 3+ ) iron (III) chloride CuCl (Cu + ) copper (I) chloride SnF 4 (Sn 4+ ) tin (IV) fluoride PbCl 2 (Pb 2+ ) lead (II) chloride Fe 2 S 3 (Fe 3+ ) iron (III) sulfide Complete the names of the following binary compounds with variable metal ions: FeBr 2 Fe must +2 iron (II) bromide Roman numeral CuCl Cu must +1 copper (I) chloride indicates SnO 2 Sn charge must +4 tin (IV) NOT oxide Fe 2 O 3 quantity!!! Fe must +3 iron (III) oxide Hg 2 S Hg must +1 mercury (I) sulfide Polyatomic Ions charged entities composed of several atoms bound together assigned special names with specific charges the ionic charge is on the group of atoms 3
Polyatomic Ions 2- CO 3 2- carbonate ion Ternary Ionic Nomenclature Writing Formulas Write each ion, cation first. Don t show charges in the final formula. Overall charge must equal zero. If charges cancel, just write symbols. If not, use subscripts to balance charges. Use parentheses to show more than one of a particular polyatomic ion. Use Roman numerals indicate the ion s charge when needed (stock system) Ternary Ionic Nomenclature Sodium Sulfate Na + and SO 4-2 Na 2 SO 4 Iron (III) hydroxide Fe +3 and OH - Fe(OH) 3 Ammonium carbonate NH 4 + and CO 3 2 (NH 4 ) 2 CO 3 1. aluminum nitrate a) AlNO 3 b) Al(NO) 3 c) Al(NO 3 ) 3 2. copper (II) nitrate a) CuNO 3 b) Cu(NO 3 ) 2 c) Cu 2 (NO 3 ) 3. iron (III) hydroxide a) FeOH b) Fe 3 OH c) Fe(OH) 3 4. tin (IV) hydroxide a) Sn(OH) 4 b) Sn(OH) 2 c) Sn 4 (OH) Naming Ternary Compounds Contains at least 3 elements There MUST be at least one polyatomic ion (it helps to circle the ions) Examples: NaNO 3 Sodium nitrate K 2 SO 4 Potassium sulfate Al(HCO 3 ) 3 Aluminum bicarbonate or Aluminum hydrogen carbonate Match each set with the correct name: 1. Na 2 CO 3 a) magnesium sulfite MgSO 3 b) magnesium sulfate MgSO 4 c) sodium carbonate 2. Ca(HCO 3 ) 2 a) calcium carbonate CaCO 3 b) calcium phosphate Ca 3 (PO 4 ) 2 c) calcium bicarbonate 4
Mixed Practice! Name the following: 1. Na 2 O 1. sodium oxide 2. CaCO 3 2. calcium carbonate 3. PbS 2 3. lead (IV) sulfide 4. Sn 3 N 2 4. tin (II) nitride 5. Cu 3 PO 4 5. copper (I) phosphate 6. HgF 2 6. mercury (II) fluoride Mixed Up The Other Way Write the formula: 1. Copper (II) chlorate 2. Calcium nitride 3. Aluminum carbonate 4. Potassium bromide 5. Barium fluoride 6. Cesium hydroxide 1. Cu(ClO 3 ) 2 2. Ca 3 N 2 3. Al 2 (CO 3 ) 3 4. KBr 5. BaF 2 6. CsOH Naming Molecular Compounds CH 4 methane CO 2 Carbon dioxide BCl 3 boron trichloride All are formed from two or more nonmetals. Ionic compounds generally involve a metal and nonmetal (NaCl) Molecular (Covalent) Nomenclature for two nonmetals Prefix System (binary compounds) 1. Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Mono- is included on the SECOND element 2. Change the ending of the second element to -ide. Molecular Nomenclature Prefixes PREFIX monoditritetrapentahexaheptaoctanonadeca- NUMBER 1 2 3 4 5 6 7 8 9 10 Molecular Nomenclature: Examples CCl 4 carbon tetrachloride N 2 O dinitrogen monoxide SF 6 sulfur hexafluoride 5
More Molecular Examples arsenic trichloride AsCl 3 dinitrogen pentoxide N 2 O 5 tetraphosphorus decoxide P 4 O 10 Fill in the blanks to complete the following names of covalent compounds. CO carbon oxide mon CO 2 carbon dioxide PCl 3 phosphorus chloride tri CCl 4 carbon chloride tetra N 2 O nitrogen di mon oxide 1. P 2 O 5 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide A flow chart for naming binary compounds. 2. Cl 2 O 7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl 2 a) chlorine b) dichlorine c) dichloride Overall strategy for naming chemical compounds. Mixed Review Name the following compounds: 1. CaO a) calcium oxide b) calcium(i) oxide c) calcium (II) oxide 2. SnCl 4 a) tin tetrachlorideb) tin(ii) chloride c) tin (IV) chloride 3. N 2 O 3 a) nitrogen oxide b) dinitrogen trioxide c) nitrogen trioxide 6
Mixed Practice Mixed Practice 1. Dinitrogen monoxide 2. Potassium sulfide 3. Copper (II) nitrate 4. Dichlorine heptoxide 5. Chromium (III) sulfate 6. Iron (III) sulfite 7. Calcium oxide 8. Barium carbonate 9. Iodine monochloride 1. BaI 2 2. P 4 S 3 3. Ca(OH) 2 4. FeCO 3 5. Na 2 Cr 2 O 7 6. I 2 O 5 7. Cu(ClO 4 ) 2 8. CS 2 9. B 2 Cl 4 Acid Nomenclature Acids Compounds that form H + in water. Formulas usually begin with H. Examples: HCl (aq) hydrochloric acid HNO 3 nitric acid H 2 SO 4 sulfuric acid Now it s Study Time DONE 7