CHEM 333 1nd Edition Lecture 2 Outline of Last Lecture I. What are Organic Elements?II. Components of an AtomOutline of Current Lecture I. Atoms and Filling RulesII. Lewis StructuresIII. Octet RuleIV. BondingV. ElectronegativityCurrent LectureI. Atoms contain electronselectrons have quantum levels shells - 1,2,3,4 (*Bolded are what we focus on in organic chemistry)Orbitals - s,p,d,f,gFilling rules: Afbau: Electrons fill orbitals starting at the lowest available energy levels before filling higher levelsHund: Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.Pauli: When filling sublevels other than s, electrons are placed in individual orbitals before they are paired up. II. Lewis Structuresbased on valence electronsCarbon: 4 valence electrons, 4 bonds Nitrogen: 5 valence electrons, 3 bonds 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.Oxygen: 6 valence electrons, 2 bonds III. Octet Rule: Every atom wants to have eight valence electrons in its outermost electron shell. IV. Bonding: Two main types of bonds1. Ionic: Electrons are transferred (Salts)a. Gain electrons-anionb. Lose electrons-cations2. Covalent: Electrons are shareda. Not always shared equallyb. Creates polarityV. ElectronegativityElectronegativity is the tendency of an atom to attract electrons, the more electronegative, the more strongly it attracts them.Bond polarity is caused by differences in electronegativity Ex. C-H bonds have almost no electronegativity difference, but C-F bonds do. This causes C-H bonds to be more stable than the C-F bond.Electronegativity trend Bonds:Ionic- two elements from opposite sides of the periodic tablePolar Covalent- two elements from the same rowNonpolar Covalent- two elements from the same column or a C-H