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UGA CHEM 1211 - Chapter 8

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Slide 1Slide 2Slide 3Slide 4Slide 5Slide 6Slide 7Slide 8Slide 9Slide 10Slide 11Slide 12Slide 13Slide 14Slide 15Slide 16Slide 17Slide 18Slide 19Slide 20Slide 21Slide 22Slide 23Formal ChargeSlide 25Slide 26Slide 27Slide 28Slide 29ResonanceSlide 31Slide 32Slide 338.5 Exceptions to the Octet RuleSlide 35Slide 36Slide 37Slide 38Slide 39Slide 40Slide 41Slide 42Slide 43Slide 44Slide 45Slide 46Electron Pair GeometriesSlide 48Slide 49Slide 50Slide 51Slide 52Slide 53ElectronegativitySlide 55Slide 56ElectronegativitySlide 58Slide 59Slide 60Polar Molecules: The Influence of shapeSlide 62Slide 63Slide 64Slide 65Slide 66Slide 67Slide 68Slide 69Slide 70Slide 71Slide 72Slide 73Slide 74Slide 75Slide 76Slide 77Slide 78Slide 79Slide 80Slide 81Slide 82Slide 83Slide 84Slide 85Slide 86Slide 87Slide 88Slide 89Slide 90Slide 91Slide 92Slide 93Slide 94Slide 95Slide 96Slide 97Slide 98Slide 99Slide 100Slide 101Slide 102Slide 103Slide 104Slide 105Slide 106Octahedral electronic arrangement: AB6, AB5U, and AB4U2Octahedral electronic arrangement: AB6, AB5U, and AB4U2Octahedral electronic arrangement: AB6, AB5U, and AB4U2Slide 110Octahedral electronic arrangement: AB6, AB5U, and AB4U2Octahedral electronic arrangement: AB6, AB5U, and AB4U2Octahedral electronic arrangement: AB6, AB5U, and AB4U2Octahedral electronic arrangement: AB6, AB5U, and AB4U2Octahedral electronic arrangement: AB6, AB5U, and AB4U2Slide 116Slide 117Slide 118Slide 119Slide 120Slide 121Slide 122Bond EnergiesBond EnergiesSlide 125Slide 126Slide 127Slide 128Slide 129Slide 130Ch. 8 Bonding and Molecular Structure8.1 Chemical Bond Formation2 general types of bonds:1. Ionic: forms when one or more valence electrons is transferred from one atom to another, creating negative and positive ions; occurs between a metal and a nonmetal2. Covalent: involves sharing of valence electrons between atoms; occurs between 2 nonmetals1Ionic bonding:Examples:2Covalent bonding:Examples:3In most chemical compounds, electrons are shared unequally, with the extent of sharing varying widely from very little sharing (largely ionic) to considerable sharing (largely covalent).48.2 Covalent Bonding and Lewis StructuresValence Electrons and Lewis Symbols for AtomsValence electrons: the electrons found in the outermost shell (usually the highest n number)Core Electrons: the electrons in the inner shells (usually the last noble gas configuration)Chemical reactions result in the loss, gain, or rearrangement of valence electrons.Core electrons are not involved in bonding or chemical reactions.5Useful guideline for main group elements is that the number of valence electrons is equal to the group number.Elements in a periodic group/family have the same number of valence electrons which accounts for the similarity of chemical properties in a family.Valence e- for transition elements include the electrons in the ns and (n-1)d orbitals.6Examples of valence e-:Clicker Q: How many valence e- does Iodine have?7Lewis dot structureNamed after American chemistry Gilbert Lewis.Octet of electrons: 8 dots around element, most stable (just like noble gases)8Where is the following element found? What is the group number?Draw a Lewis dot structure with dots for e9Lewis Electron Dot Structures and the Octet RuleCovalent bonding: a bond results when one or more electron pairs are shared between 2 atoms. 10Bond pair: the electrons in the bondSingle bond: shares 2 e- (CH4)Double bond: shares 4 e- (CH2CH2, O2, CO2)Triple bond: shares 6 e- (N2, C2H2)Lone pairs: nonbonding electrons, not involved in bonding.11Octet rule: the tendency of molecules and polyatomic ions to have structures in which eight electrons surround each atom, just like the noble gasesethaneetheneethyne12Drawing Lewis Electron Dot Structures1. Determine the arrangement of atoms within a molecule; central atom is usually the one with the lowest affinity for electrons (least EN).2. Determine total number of valence e-3. Place one pair of electrons between each pair of bonded atoms to form a single bond4. Use any remaining pairs as lone pairs around each terminal atom (except H – can only have 2 e-), so that each terminal atoms is surrounded by 8 e-.135. If the central atom doesn’t have eight e-, change one or more lone pairs on the terminal atoms into a bonding pair, to make double or triple bonds 1415Write Lewis dot formula for C3H8.Write Lewis dot formula for NO3 – (pretend that was a superscript)Write a Lewis dot structure for dimethyl ether (CH3-O-CH3).Write a Lewis dot structure for n-propylamine, CH3CH2CH2NH21617Lewis formulas can also be drawn for polyatomic ions.One example is the ammonium ion , NH4+.Predicting Lewis StructuresHydrogen Compounds1819Oxoacids and Their AnionsAll covalent compounds, but since they are acidic they must loose H+.2021Write Lewis dot formula for the sulfite ion, SO32-.Isoelectronic SpeciesReminder: isoelectronic means “same # of electrons”228.3 Atom Formal Charge in Covalent Molecules and IonsFormal charge: charge that would reside on an atom in a molecule or polyatomic ion if we assume that all bonding e- are shared equally (not a real charge)FC = group number –(# of unshared e- + # of bonds )2324Formal Charge•Calculation of a formal charge on a molecule is a mechanism for determining correct Lewis structures.•The formal charge is the hypothetical charge on an atom in a molecule or polyatomic ion.•The best Lewis structures will have formal charges on the atoms that are zero or nearly zero.25Rules for Assigning Formal Charge (FC)1. FC = grp number – (# of bonds + # of unshared e-)2. An atom that has the same number of bonds as its periodic group number has a formal charge of 0.3. a. The formal charges of all atoms must sum to 0 in molecules.b. The formal charges must sum to the ion’s charge for a polyatomic ion.PO43-26Cl N OCl N OConsider nitrosyl chloride, NOClDo Lewis structures for CO2, do formal charges. Which one is better?27Cyanite ion do Lewis structures (OCN-) page 374288.4 ResonanceResonance is a means of representing the bonding in a molecule or polyatomic ion when a single Lewis structure fails to give an accurate picture.2930Resonance•There are three possible structures for SO3.–The double bond can be placed in one of three places.When two or more Lewis formulas are necessary to show the bonding in a molecule, we must use equivalent resonance structures to show the molecule’s structure.Double-headed arrows are used to indicate resonance


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UGA CHEM 1211 - Chapter 8

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