CHM 303 1st Edition Lecture1Outline of Current LectureDiscuss Course Syllabus, Objectives and ExpectationsChapter 1: Structure Determines PropertiesCurrent LectureView syllabusChapter 1: Structure Determines PropertiesStructure:A. Lewis Structure (LS); displays possible bonding sequencesB. Molecular Geometry (MG); example (Ex.); tetrahedral, linear, trigonal planarC. Formal ChargesD. Resonance Forms; two or more ways to draw LS, MG does NOTchangeE. Bond/Molecular Polarity; electronegativity*This is not everything regarding structure, but some of the key aspects*Properties:A. Physical1. Boiling Point and Melting Point2. Solubility; in water, ethanol, hexane, etc.B. Chemical1. Acidity/Basicity; can also be considered physical2. Reactivity These 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.Ex. Compound Bond Energy H—O—O—H O—O; 213 kJ/molH—N—N—H N—N; 275 kJ/mol H H H HH—C—C—H C—C; 347 kJ/mol H HC—C bond is much stronger than O—O or N—N because there are no lone pairs.Carbon:A. No Lone Pairs1. Because of this fact, it is possible to have tens of thou-sands of carbons in a single chain together, and it willstill remain stable. No other element is capable of doing this.B. Two Main Forms1. Diamond; cannot be broken due to 3-dimensional lattice2. Graphite; fused together hexagonal rings form sheets that can act like a lubricant, causing these sheets to slide.. . . .. . . .. . .