Information Required for MemorizationYour students are required to memorize the following information for Chem 10. This information must not besupplied on Cheat Sheets for your Semester Exams or Final Exam.SI PrefixesPrefixes greater than theBase UnitSymbolScientific NotationTeraT1012GigaG109MegaM106kilok103hectoh102dekada101Prefixes less than theBase UnitSymbolScientific Notationdecid10-1centic10-2millim10-3microµ10-6nanon10-9picop10-12femtof10-15Element Symbols and NamesGroup 1A: H, Li, Na, K, Rb, CsGroup 2A: Be, Mg, Ca, Sr, BaGroup 3A: B, Al, GaGroup 4A: C, Si, Ge, Sn, PbGroup 5A: N, P, As, SbGroup 6A: O, S, Se, TeGroup 7A: F, Cl, Br, IGroup 8A: He, Ne, Ar, Kr, Xe, RnGroup 3B: ScGroup 4B: TiGroup 5B: VGroup 6B: Cr, WGroup 7B: MnGroup 8B: Fe, Co, NiGroup 1B: Cu, Ag, AuGroup 2B: Zn, Cd, HgMonatomic IonsNon-metal AnionsNon-metals will form anions with only one possible negative charge. The names of these anions are based on theelement root name, but the ending is changed to – ide. The following Periodic Table shows the charges for non-metal anions commonly found in ionic compounds.1A2A 3A4A5A6A7A8A H-1 BC-4N-3O-2F-1 SiP-3S-2Cl-1 AsSe-2Br-1 TeI-1 At Metal CationsMost (but not all) main group metals will form cations with only one possible charge. Most (but not all) transitionmetals will form cations with more than one possible charge. Metal cation names are the same as the originalelement names. When metals form more than one cation, then the cation charge must be indicated in the name asRoman Numerals in brackets. The following Periodic Table shows the charges for metal cations commonly foundin ionic compounds:1A2A3A4A5AH+1(acids)Li+1Be+2Na+1Mg+2 Transition Metals (B)Al+3K+1Ca+2Ti+2Ti+4Cr+2Cr+3Cr+6Mn+2Mn+3Mn+4Fe+2Fe+3Co+2Co+3Ni+2Ni+3Cu+1Cu+2Zn+2Ga+3Rb+1Sr+2Ag+1Cd+2In+1In+3Sn+2Sn+4Cs+1Ba+2Au+1Au+3Hg+2Pb+2Pb+4Bi+3Bi+5Polyatomic Ions OH-1HydroxideO2-2PeroxideCN-1CyanideCO3-2CarbonateSCN-1ThiocyanateSO3-2SulfiteHCO3-1Hydrogen Carbonate (Bicarbonate)SO4-2SulfateHSO3-1Hydrogen Sulfite (Bisulfite)S2O3-2ThiosulfateHSO4-1Hydrogen Sulfate (Bisulfate)C2O4-2OxalateC2H3O2-1AcetateCrO4-2ChromateNO2-1NitriteCr2O7-2DichromateNO3-1Nitrate MnO4-1PermanganatePO3-3PhosphiteClO-1HypochloritePO4-3PhosphateClO2-1Chlorite ClO3-1ChlorateNH4+1AmmoniumClO4-1PerchlorateHg2+2Mercury (I)Rules for Assigning Oxidation NumbersThis is a prioritized list. If two rules contradict each other, follow the rule that appears higher on the list.1. The atoms in pure elements are assigned an oxidation number of zero.2. Monatomic ions are assigned an oxidation number equal to their charge.3. For atoms in covalent molecules and polyatomic ions:a. The sum of all the oxidation numbers of the atoms in a covalent molecule must equal zero. The sum of all theoxidation numbers of the atoms in a polyatomic ion must equal the charge on the ion.b. Fluorine is assigned an oxidation number of –1.c. Oxygen is assigned an oxidation number of –2 (an exception to this is when oxygen occurs as the peroxideion, O2-2, where it is assigned an oxidation number of –1).d. Hydrogen is assigned an oxidation number of +1.e. For all other elements: the element with the greater electronegativity is typically assigned a negative oxidationnumber equal to its charge as an anion in ionic compounds.The Half Reaction Method for Balancing Redox Reactions in Acidic SolutionThis method assumes the reaction occurs in aqueous, acidic solution where H2O and H+ are plentiful.1. Write two half-reactions, one for oxidation and one for reduction.2. Balance each half-reaction as follows:a. Balance all elements other than oxygen and hydrogen.b. Balance oxygen by adding the appropriate number of water molecules (H2O).c. Balance hydrogen by adding the appropriate number of hydrogen ions (H+).d. Balance the charge by adding the appropriate number of electrons (e-).3. Multiply each half-reaction by a whole number so that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction.4. Add the two half reactions together, keeping all the reactants together on the left of the yield arrow and all theproducts together on the right of the yield arrow. The electrons will cancel out so they are not shown in thefinal equation.5. Cancel any species that appear on both sides of the equation.VSEPR Theory# of effectiveelectron groupsElectronic GeometryMolecular Shape2bond angles =180°Linearbond angles =180°Linearbond angles =120°Trigonal Planar3bond angles =120°Trigonal Planarbond angles <120°Bent (or V-shaped)bond angles =109.5°Tetrahedralbond angles <109.5°Trigonal Pyramidal4bond angles =109.5°Tetrahedralbond angles <109.5°Bent (or