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UNT CHEM 1415 - Lewis Dot Structure
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CHEM 1415 1st EditionLecture 6Unit: Chemical Bonding, Lewis Dot StructuresOutline of Current Lecture I. Review of Quantum NumbersII. Quantum Numbers of ElementsIII. Octet RuleIV. Lewis Dot Structurea. Examplesi. Methaneii. Carbon Tetrachlorideiii. Wateriv. Dinitridev. Carbon DioxideCurrent LectureReview of Quantum Numbers:l Orbital Number in a set0 s Spherical 1 Size, energy1 p dumbbell 3 Shape of the thumbnail2 d 5 Orientation of thumbnail3 fQuantum Numbers of Elements:H1 s1He1 s2These 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.Li1 s22 s1[He]2 s1Be1 s22 s2[He]2 s2B1 s22 s22 p1[He]2 s22 p1C1 s22 s22 p2N1 s22 s22 p3O1 s22 s22 p4F1 s22 s22 p5[He]2 s22 p5Ne1 s22 s22 p6[He]2 s22 p6Na1 s22 s22 p63 s1Mg1 s22 s22 p63 s2Sc[Ar]4s23 dSn[Kr]5s24 d105 p2La[Xe] 6s25 d1Hf[Xe] 6s25 d14 f14U[Rn]7s26 d15 f3Octet Rule:- An atom will form covalent bonds to achieve a complement of eight valence electronsLewis Dot Structure:1. Draw a trial structure with an octet of electrons around every atom except hydrogen2. Adjust as necessary relative to the number of valence electrons availableExamples:Methane C H4H↓H ↔ C ↔ H↑HThis is the trial structure, the arrows represent 2 atoms bonding, we have 8 available electrons and 8 of them are bonded.Carbon Tetrachloride C Cl4Trial StructureC: 1 * 4 = 4Cl: 7 * 4 = 28Electrons available = 32Water H2OTrial StructureH: 1 * 2 = 2O: 6 * 1 = 6Electrons available = 8N2N: 5 * 2 = 10Electrons available = 10- The most you can have is triple bondsCarbon Dioxide C O2C: 4 * 1 = 4O: 6 * 2 = 12Electrons available =


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