1. Upload a periodic table that has the following charges indicated A. Metals that form only one cation: Gorup I cations (+), Group II cations (2+) and the TM with a most common, or only, ion Ag+, Zn2+, Cd2+, Al3+, Sc3+, Y3+. B. The charge of the halogens (-) C. Oxide, sulfide, selenide and telluride ions (2-) D. Nitride, phosphide and arsenide ions (3-) E. Write the prefixes from one to ten to name binary molecular compounds. F. Indicate which ones are the transition metals (TM) but do not write their charges. The charge of the TM is figured out with the anion of the compound to be named. 2. Upload the polyatomic ions chart color coded a) Polyatomic ions ending in ITE b) Polyatomic ions ending in ATE c) All others (special names) d) Write on the table, the codes ITE-OUS ATE-IC , to name acids with polyatomic ions 3. Compounds that contain metals that form only one cation and a non metal (ide), or, a polyatomic ion (ite , ate and special names). A. Name the cation then the anion (IDE ending) Examples NaCl = (binary compound (only two types of elements) The anion is Cl-. Sodium chlorIDE NaClO= (more than two types of atoms, one of them is a polyatomic ion find the name of ClO- in the polyatomic ions table) sodium hypochlorite Name these compounds 1. Li2S 2. Al2S3 3. K2SO4 4. Sc2(SO3)3 B Write the formulas Example Scandium oxide = look at the charge of the cation and anion in the labeled periodic table: Sc3+, O2- Balance the positive charges with negative charges: Need Sc3+, Sc3+, O2- , O2- , O2- to cancel the charges, write the number of each as a subscript and omit the charges= Sc2O3 If one of them is a polyatomic ion and require more than one, write it in parenthesis. Example aluminum sulfate. Ions Al3+. and SO42-. Need: Al3+, Al3+, SO42-, SO42-, SO42- Write Al2(SO4)3 Write the formula for these compounds 1. Silver bromIDE 2. Zinc hypobromITE 3. Cadmium bromITE 4. Calcium bromATE 4. A. Compounds that contain a TM: To name them, find the charge of the TM with the charge of the anion and write it as a roman numeral in parenthesis Examples: AuCl3, Au is a TM and chloride is -1 (labeled periodic table). There are three Cl-; total negative charges are -3. The gold has to have 3+ to cancel those charges. Name: Gold (III) chloride Au2SO4 Au is a TM, more than two types of elements then one is a polyatomic ion. Sulfate is -2 (in polyatomic ions table). We need 2+ to cancel the charge of sulfate 2 -. But there are two golds, each one of them gets a +. Au+, Au+ and SO42- Name: Gold (I) sulfate Name this compounds 1. Fe2O3 2. FeS 3.Fe2(SO4)3 4.FeSO3 B. Write the formula The roman numeral indicates the charge of the TM Examples Chromium (III) oxide. Cr is 3+ (from the name) Oxide 2- (from labelled periodic table). Need Cr3+, Cr3+, O2-, O2-,O2-to cancel charges. Formula Cr2O3 Chromium (I) nitrate Cr is + , nitrate is – . Need one of each. Formula CrNO3 Write the formula for these compounds 1. Copper (I) oxIDE 2. Copper (II) oxIDE 3. Copper (II) phosphATE 4. Copper (II) phosphIDE Binary molecular compounds (other than acids)contain two non metals. Indicate the number of each atom with prefixes. If the first atom is one, there is no need to say mono. Use mono for the second element if there is only one atom. 1 mono; 2 di; 3 tri; 4 tetra; 5 penta; 6 hexa; 7 hepta; 8 octa; 9 nona, 10 deca, 11 undeca, 12 dodeca, 13 trideca, 14 tetradeca, etc 1. CO 2. SO3 3. P4O5 4. CCl4 B. Write the formula. Write the number of each atom indicated by the prefix. 1. Carbon dioxide 2. Sulfur dioxide 3. Dinitrogen dioxide 4. Dinitrogen monosulfide 5. Binary acids (contain only two types of elements) Acids are molecular compounds but dissociate in water giving hydrogen ions (H+) There will be as many hydrogens as necessary to cancel the charge of the anions. It is not necessary to specify the number of each. These are molecular compounds when pure (neat) and ionic when dissolved in water (aq). A. Name the binary (neat) acids. Use Hydrogen STEMide Examples HCl = hydrogen chloride H2S = hydrogen sulfide Name these compounds 1. HBr 2. H2Se B. Name the aqueous acids: When the acids are in water (aq) use hydroSTEMic acid Examples HCl (aq) = hydroCHLORic acid H2S (aq) = hydroSULFURic acid Name these binary acids in aqueous solition 1. HBr(aq) 2. H2Se (aq) C. Write the formula of the acids. Find the charge of the anion in your labelled periodic table and use enough H+ to balance the charge of the anion. Write (aq) when in water) 1. Hydrogen iodide 2. Hydroiodic acid 3. Hydrogen telluride 4. Hydrotelluric acid 7. Acids that contain a polyatomic ion A. Name the acids: If the Polyatomic ion ends in ITE change the name to OUS. If the polyatomic ion end in ATE change the name to IC Examples H2SO4 = sulfuric acid H2SO3 = sulfurous acid Name these acids that contain a polyatomic ion 1. H2CO3 2. HClO2 3. HClO4 B. Write the formula for the acids: If the acid ends in IC find the ATE polyatomic ion. If the acid ends in OUS find the ITE polyatomic ion. To write the formula add enough H+ to cancel the charge of the polyatomic ion Example Selenic acid comes form Selenate, SeO42-. Two H+ are needed to cancel the charges H2SeO4. Always write the cation first then the anion. Write the formula for these acids that contain a polyatomic ion 1. Phosphoric acid 2. Arsenous acid 3. Hypoiodous acid 4 Perbromic acid
