PPT-CHE2060 Topic 1: Atoms, orbitals & bonding

Atoms Orbitals amp Bonding Topics Very quick history of chemistry What is organic chemistry Atomic models nuclear to quantum All about orbitals How orbitals fill electron configuration. (. Benzene. ). 140 pm. 140 pm. 140 pm. 140 pm. 140 pm. 140 pm. All C—C bond distances = 140 pm. Benzene. empirical formula. = CH. 140 pm. 140 pm. 140 pm. 140 pm. 140 pm. 140 pm. . 146 pm. 134 pm. 10. Molecular Geometry and Bonding Theory. 2. The subject of molecular geometry deals with shapes of molecules. Recall that a Lewis structure is a two-dimensional representation of a molecule or ion; its intent is to show how the valence electrons of atoms are distributed in the molecule. A Lewis structure does not necessarily have to depict the actual shape of the molecule or ion, but we can use it deduce what the actual shape is.. Elements with high electronegativities (non-metals) will not give up electrons. Bonds are not formed by a transfer of electrons, they are formed by sharing electrons.. Molecules are neutral groups of covalently bonded atoms. Chapter 9. Molecular Geometry and Bonding Theories. Molecular Geometry . The three-dimensional arrangement of atoms in a molecule .  . molecular geometry. Lewis structures can’t be used to predict geometry. The . attractive force which holds . various constituents . (atoms, . ions, etc. .) together in . different chemical . species is called a chemical bond.. KÖSSEL-LEWIS APPROACH TO. CHEMICAL BONDING. Atoms, Orbitals & Bonding Topics:. Very quick history of chemistry…. What is organic chemistry?. Atomic models: nuclear to quantum. All . about . orbitals. How . orbitals fill: electron . configuration. Prepared By:-. Swastik Mishra Upasana Nath. Rahul Kanungo Pratik Patnaik. 1. st. Shift. Kendriya Vidyalaya No-1, . BHubaneswar. Kossel Lewis Approach. Kossel Lewis Approach To Chemical Bonding. In 1916, Kossel and Lewis were the first to become independently successful in giving a satisfactory explanation about the formation chemical bond in terms of electrons. . ▪. . Each of the following counts as a single . electron group: . a lone pair, a single bond, a. double bond, a triple bond, or a single electron (as in a free radical. ).. ▪. . Electron groups. ▪. . Each of the following counts as a single . electron group: . a lone pair, a single bond, a. double bond, a triple bond, or a single electron (as in a free radical. ).. ▪. . Electron groups. NH. NH. 2. NH. 3. Thanks for participating in today’s session! We’ve been developing a new approach for teaching about bonding and molecules in General Chemistry courses like . Chem. 102. Our objective is to determine if the material makes sense to students.. Text:. Ch 8 (all except sections 4,5 & 8). Ch 9.1 & 9.5. Ch 10.1-10.7. My Name is Bond. Chemical Bond. PART 3: Hybridization & . Delocalization of Electrons. Hybridization . Hybridization:. 288 1 reactions catalyzed have lead to the large perturbation to activate of giving an incoming ligand. the d metal orbital Mulliken population the fragment, quite characteristic a phosphine ligand w DE Chemistry. Dr. Walker. Hybridization and the Localized Electron Model. Hybridization. The . mixing of two or more atomic orbitals of similar energies on . the same . atom . to . produce new orbitals of equal . Nature of coordinative bond. Back-bonding. Bonding of metals to . p. -systems. Valence bond and hybridization. Each bond treated independently from the environment. Resonance concept. Impossibility to explain molecular geometries.