Chem 121 1st Edition Lecture 12Outline of Last Lecture I. Chemical BondingII. Ionic BondingIII. Covalent BondingIV. Chemical FormulasV. Lewis Model/ Lewis Structures- Ionic/ Covalent BondingOutline of Current Lecture I. Nomenclature- Anions / Naming Simple CompoundsII. Formula for Ionic CompoundsCurrent LectureI. Monatomic- H (1A)- F, Cl, Br, I (7A)- S, O (6A)- N, P (5A)Polyatomic: cluster of atoms with “n __ ” charge- Peroxide- Hydroxide- Cyanide- Organic:o Acetateo OxalateOxoanions (Special group of polyatomic anions) with General formula: EOyn-- Prefixes:o per- (1 more oxygen)o hypo- (1 less oxygen)- Suffixes:These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.o –ate (more oxygen)o –ite (fewer oxygen)- If E is in group 7A, 7B (Mn, Cl, Br, I), max # of O = 4o 4 O: per- + (B.N. of E) + -ateo 3 O: (B.N. of E) + -ateo 2 O: (B.N. of E) + -iteo 1 O: hypo- + (B.N. of E) + -ite- If E is in period 2 (B, C, N), max # of O = 3o 3 O: (B.N. of E) + -ateo 2 O: (B.N. of E) + -ite- If E is other, max # of O = 4o 4 O: (B.N. of E) + -ateo 3 O: (B.N. of E) + -ite- Charge= group # of E + [(-2) x (max # of O in series)]- Hydrogen Oxoanions- with general formula HxEOym-o One hydrogen (treat H as H+) Hydrogen (name of oxoanion) or bi- + name of oxoaniono More than one hydrogen (H+) (Prefix + hydrogen)(Name of oxoanion)o Charge= charge of oxoanion + [(# of H) x (+1)]First Element: H- Acids (except H2O)- Acids: compounds dissolving in water, releasing H+ (aq)o A covalent compound with H as 1st element followed by (aq)o Naming acids: depends on name of anion Base Name ending with –ide- hydro + base name of nonmetal + -ic + acid Base Name ending with - ate- Base name of oxyanion+ -ic + acid Base Name ending with -ite- Base name of oxyanion + -ous + acid First Element: Nonmetal- Covalent Compounds- For all compounds: prefix + name of 1st element // Prefix + name of anion- Numerical prefixes:1 mono- 6 hexa-2 di- 7 hepta-B.N. – Base NameE- ElementO- Oxygen3 tri- 8 octa-4 tetra- 9 nona-5 penta- 10 deca-- Use prefix for 2 or more atoms of 1st E- With Oxide, o-, a- from prefix omittedFirst Element: Metal- Ionic Compounds- Type I Metals: metals forming only one cation (17)o Group 1A, 2A; GAS (Ga, Al, Sc); ZAC (Zn, Ag, Cd); NH4+o Charge: metals lose electrons by their group numberso Naming: name of cation (metal) + name of anion- Type II Metals: metals forming >1 cationso Rest of metals in periodic tableo Naming: name of cations (metals) + (charge of cation (metal) in roman numerals and parentheses) + name of aniono Charge of metal: Start with anion (charge is always known!) Count total negative charges by multiplying the charge by the subscript Total negative charge = total positive charges (compound: charge neutral) Charge of metal = total positive charge divided by subscript of metal- Hydrated Ionic Compounds: MXnH2Oo (Name of ionic compound)(Prefix+ hydrate)o Prefixes--- similar to those used in covalent compounds½ hemi- 5 penta-1 mono- 6 hexa-2 di- 7 hepta-3 tri- 8 octa-4 tetra-II.Formula for Ionic Compounds: Steps in writing formula for ionic compounds1. Determine ions and charges2. Swap charge numbers from one element to another as subscripts (crossing over)3. Reduce the subscripts to give a ratio with the smallest whole number4. Check charges for charge