1. IonicCovalentMetallic Chemical Bonds  e- transfer  Crystal lattice  ions  Na + Cl Na + Cl -  “salts”  very strong bonds generally between metals and non metals.  Solids at room temp.  Poor conductors of electricity in a solid state +-  sharing  “molecules”  hypothetical charge  H + H H H. orbital overlap  Bonding e- are localized between two atoms  Formed between two nonmetals  “sea” of e-  e- are delocalized. “glue” Bonds

2. Nomenclature

3. Assigning Oxidation States The concept of oxidation numbers (or oxidation states) was devised as a simple way of keeping track of electrons in reactions. We use the following rules for assigning oxidation numbers: Free Elements (Na, O 2, etc.)0 Group 1 Elements in a compound 1 +1 Group 2 Elements in a compound+2 Group 3 Elements in a compound+3 “O” in a compound 2 -2 “F” in a compound-1 1 Exception to this rule occurs for hydrogen in hydrides (e.g. LiH, where the oxidation state of hydrogen is –1). 2 Exception to this rule occurs in peroxides (e.g. H 2 O 2, where the oxidation state of oxygen is –1).

4. NOTE: Three transition metals, Cd 2+, Zn 2+ and Ag +, are understood to exist in these oxidation states (numbers); therefore, Roman numerals are NOT included in parentheses. Also note that the mercury(I) ion is written as a diatomic ion (dimer): Hg 2 +2. WorkShop Determine the oxidation state of each underlined atom: KMnO 4, ClO 4 -, and S 2 O 3 2-.

5. Common Polyatomic Ions – YOU MUST MEMORIZE THESE!!! acetateC 2 H 3 O 2 - hydrogen phosphateHPO 4 2- ammoniumNH 4 + hydrogen sulfateHSO 4 - carbonateCO 3 2- hydroxideOH - chromateCrO 4 2- nitrateNO 3 - hypochloriteClO - nitriteNO 2 - chloriteClO 2 - oxalateC 2 O 4 2- chlorateClO 3 - permanganateMnO 4 - perchlorateClO 4 - peroxideO 2 2- cyanideCN - phosphatePO 4 3- dichromateCr 2 O 7 2- sulfateSO 4 2- dihydrogen phosphateH 2 PO 4 - sulfiteSO 3 2- hydrogen carbonateHCO 3 - thiocyanateSCN -

6. Naming Acids There are two main types of acids that we will encounter at the onset of this course, binary acids, and oxoacids. 1. Binary Acids – certain compounds of H with other nonmetal atoms. Examples: HF(aq) = hydrofluoric acid HCl(aq) = hydrochloric acid HBr(aq) = hydrobromic acid HI(aq) = hydroiodic acid H 2 S(aq) = hydrosulfuric acid 2. Oxoacids – Hydrogen with two other nonmetals, one of which is oxygen. Examples:HClO = hypochlorous acid HClO 2 = chlorous acid HClO 3 = chloric acid HClO 4 = perchloric acid HNO 2 = nitrous acid HNO 3 = nitric acid

7. Naming Hydrates and Simple Organic Compounds Hydrates Hydrates are ordinary chemical substances that have associated with them a certain number of water molecules. For example, CuSO 4  5H 2 O is read copper(II) sulfate pentahydrate. As we will see in section 2, when determining the overall molecular weight of this particular compound, you ADD five water molecules to the initial CuSO 4 (as opposed to multiply, where the “  ” is commonly misinterpreted by beginner chemistry students; more on this later)! When dealing with organic (or carbon-containing) compounds, we refer to the following prefixes: Number of CarbonsPrefix 1Meth- 2Eth- 3Prop- 4But- 5Pent- 6Hex- 7Hept- 8Oct- 9Non- 10Dec-

8. Naming Simple Organic Compounds Compounds containing only carbon and hydrogen are called hydrocarbons. Hydrocarbons that contain only carbon-carbon single bonds are called alkanes. The simplest alkane is methane (CH 4 ), followed by ethane (C 2 H 6 or CH 3 CH 3 ), etc. The names of the alkanes are composed of two parts: a prefix indicating the number of carbon atoms, and the suffix “-ane” indicating that the molecule contains only carbon-carbon single bonds. Hydrocarbons that contain only carbon=carbon double bonds are called alkenes. The simplest alkene is ethene (C 2 H 4 or CH 2 CH 2 ) followed by propene (C 3 H 6 ).

9. Workshop on Nomenclature 1.Name each of the following compounds: A.KClO 4 G.KMnO 4 B.Ca 3 (PO 4 ) 2 H.K 2 Cr 2 O 7 C.Al 2 (SO 4 ) 3 I.CH 3 CH 2 CH 2 CH 2 CH 3 D.Pb(NO 3 ) 2 J.Li 2 C 2 O 4 E.BaSO 3 K.TiO 2 F.NaNO 2 L.BaCl 2  8H 2 O 2.Name each of the following compounds: A.NaClG.NO B.MgCl 2 H.NaHSO 4 C.RbBrI.N 2 F 4 D.CsFJ.FePO 4 E.AlI 3 K.SiF 4 F.V 2 O 5 L.Ca(HSO 3 ) 2

10. Workshop continued: 3.Write formulas for the following compounds: A.potassium dichromateG.ammonium acetate B.sulfur hexafluorideH.ammonium hydrogen sulfate C.sodium dihydrogen phosphateI.cobalt(III) nitrate D.lithium nitrideJ.mercury(I) chloride E.chromium(III) carbonateK.potassium chlorate F.octaneL.cobalt(II) chloride heptahydrate 4.Write formulas for the following compounds: A.sodium hydroxideG.potassium hypochlorite B.aluminum hydroxideH.lead(IV) oxide C.hydrogen cyanideI.ammonium chromate D.sodium peroxideJ.copper(I) bromide E.copper(II) acetateK.germanium dioxide F.carbon tetrafluorideL.butane

11. 5.The formulas and common names for several substances are given below. What are the systematic names for these substances? A.sugar of leadPb(C 2 H 3 O 2 ) 2 B.blue vitrolCuSO 4 C.quicklimeCaO D.milk of magnesiaMg(OH) 2 E.laughing gasN 2 O 6. Writing Names and Formulas of Compounds i. Write the formula of each of the following compounds. A.Calcium hydroxide____________________ B.Nickel(II) phosphate____________________ C.Beryllium iodide____________________ D.Chromium(III) sulfide____________________ E.Diphosphorus tetroxide____________________ F.Aluminum oxide____________________ G.Ammonium nitrate____________________ H.Phosphorus pentachloride _________________

12. ii. Name each of the following compounds. A.Na 3 PO 4 ________________________________ B.PF 5 ________________________________ D.FeBr 3 ________________________________ E.Cu 2 O________________________________ F.Cr(OH) 3 ________________________________ G.Rb 2 SO 4 ________________________________ H.N 2 O________________________________ I.HI________________________________ J.KH________________________________ K.Cr 2 O 3 ________________________________ L.MgSO 4  6H 2 O________________________________ M.CH 3 CH 2 CH 3 ________________________________