CHEM 101 1nd Edition Lecture 7 Outline of Last Lecture I. IonsII. What is the size of an atom?III. Ionic CompoundsIV. Writing Formulas for Ionic CompoundsV. Naming Ionic CompoundsOutline of Current Lecture I. List of Common Anions and CationsII. Naming Ionic CompoundsIII. Naming Covalent CompoundsIV. Chemical CompoundsCurrent LectureI. List of Common Anions and Cationsa. http://faculty.lacitycollege.edu/boanta/paperwork/iontable.htm II. Naming Ionic Compoundsa. Review of Rules i. If the anion is an element, change the ending to –ide.ii. If the anion is a polyatomic ion, simply write the name of the polyatomic ion.iii. If the cation can have more that one possible charge, write the charge as a Roman numeral in parentheses.b. Examplesi. HgBr21. Br had -1 charge, are are 2 molecules2. In order for it to have an equal charge, Hg must be 2+3. mercury (II) bromideii. FeS1. S has a -2 charge, 2. Iron must has exact opposite charge3. iron (II) sulfideiii. NH4CN1. NH4+, ammonium 2. CN-, cyanideThese 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.3. ammonium cyanideiv. Sn(OH)21. (OH)2, hydroxide has a -1 charge, since there are 2, it's a -2 charge2. Therefore Sn will have to have a +2 charge3. tin (II) hydroxidev. NaHSO41. Na will always be +12. HSO4, must have a -1 charge, but how do you name it?a. SO42- sulfate, when you add an hydrogen it changes the chargeb. HSO4-, hydrogen sulfate or bisulfate3. sodium hydrogen sulfatea. sodium bisulfatevi. TiCl21. Ti is variable, but Cl is always -1, contributing -22. Therefore Ti is contributing +23. titanium (II) chloridevii. Co2O31. O is -2 charged, contributing -62. Since there are 2 Co, it must be +3 charged3. cobalt (III) oxideIII. Naming Covalent Compoundsa. Moleculesi. Molecule: an aggregate of at least 2 atoms in a definite arrangement gel together by covalent chemical bonds1. Non-metals share covalent bondsii. Naming Binary Covalent Compounds1. A prefix is used to denote the number of atoms each element in the compounda. mono- id not used on the first element listed2. The ending on the more electronegative (2nd) element is changed to -idea. PCl3 = phosphorus trichlorideb. CO2 = carbon dioxidec. N2O5 = dinitrogen pentoxidei. When elements begging with a vowel, drop the vowel off of the end of the prefixd. SO2 = sulfur dioxidee. CO = carbon monoxideiii. Exceptions include:1. NH3 = ammonia2. PH3 = phosphine3. NO = nitric oxide4. N2O = nitrous oxide5. H2O = water6. N2H4 = hydrazineb. Naming Acidsi. Acid: hydrogen containing compounds that give off H+ in waterii. Why do we call H+ a proton?1. Recall that a.1H has 1 proton, 0 neutron, and 1 electronb.2D has 1 proton, 1 neutron, 2. If we then write H+, this mean we lost an electron and are only left with a proton.iii. ____ride -> add H+ -> hydro_____ic acid1. HF: hydrogen fluoride -> hydrofluoric acid2. HCN: hydrogen cyanide -> hydrocyanic acidiv. ____ate -> add H+ -> _______ic acid1. HNO3: nitrate -> nitric acid2. H2SO4: sulfate -> sulfuric acidv. _______ite -> add H+ -> _____ous acid1. HNO2: nitrite -> nitrous acid2. H2SO3: sulfite ->sulfurous acidIV. Chemical Compoundsa. Chemical Compounds: Formed from fixed ratios of atoms or ions i. C6H12O6, NaCl, H2O, Ca(NO3)2b. Ionic Compounds: are formed between cations and anionsi. metal ion + nonmetal ionii. polycation + nonmetal ioniii. metal ion +polyanionc. Covalent Compounds: are formed between nonmetal atomsi. Nonmetal +