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Understanding Covalent Bonding and Hybridization in Molecular Geometry

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bryce
14 diapositives · 282 Views · Aug 07, 2014

This guide explores the concepts of covalent bonding and hybridization of central atoms in molecules. We define hybridization types: sp, sp2, and sp3, explaining how electron sharing alters the shapes of s and p orbitals, resulting in linear, trigonal planar, and tetrahedral geometries. The process of naming covalent compounds is described, including the use of prefixes to denote atom quantities (mono, di, tri, etc.). Additionally, the naming conventions for acids, including those with and without oxygen, are outlined to assist in the identification of various chemical structures.

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  1. Covalent Bonding

  2. If three elements combine to share electrons, the shapes of the s orbital and p orbitals of the central atom change. • We call the new shape an sp1 hybrid • recall, the original s orbital is a spherical shape • the original p orbital is a sort of dumbell shape. Hybridization of Central Atom

  3. the new sp1 hybrid looks like a weighted dumbell, • the electrons are being pulled toward the other atom they are being shared with. Hybridization of Central Atom

  4. to make a new shared linear shape – see your hand-out Hybridization of Central Atom

  5. If central atom shares with three other atoms, • it creates an sp2 orbital hybrid, • because it involves changing the shapes of the central atom’s s-orbital • and 2 of its p-orbitals. • the new compound shape is trigonal planar. Hybridization of Central Atom

  6. If the central atom shares with four other atoms, or has a free pair of electrons, we get an sp3 hybrid, • because the s orbital and all 3 p orbitals shapes are hybridized. • This creates a tetrahedral shape of the molecule. Hybridization of Central Atom

  7. P 104 in text book • Use full name for first element and • add “ide” to second (just like you do for ionic formulas) • BUT…unlike for ionic formulas… • Prefixes are used to denote how many of each atom the prefix is in front of Naming of covalent compoundsNon-metals

  8. mono = 1 • di = 2, ex: CO2 = carbon dioxide • Notice in above example that “mono” is not used in front of the carbon. “Mono” is implied in front of the first element. • Tri = 3, ex: BF3 = boron trifluoride Naming Covalent Compounds

  9. tetra = 4 • penta = 5 • hexa = 6 • hepta = 7 • octa = 8 • try naming: N2O5 • dinitrogenpentoxide • notice that we drop the “a” ending of penta when the next word starts with a vowel. • This is the case for all endings with vowels, except di, as in dioxide, and tri, as in trioxide. Naming Covalent Compounds

  10. Text reference: p 113 – 114 • Acids – substances that release H+ ions (protons) when dissolved in water. • First element is always hydrogen • 2 types: • contain oxygen or • don’t contain oxygen Naming Acids

  11. Prefix “hydro” • Suffix “ic” • “Acid” at end • Ex: HCl = hydrochloric acid • You try: HCN • hydrocyanic acid • H2S • hydrosulfuric acid Naming Acids not Containing Oxygen

  12. 2 types of oxyanions: • oxyanion ends in “ate” • ex: sulfate, fluorate • oxyanion ends in “ite” • ex: sulfite, fluorite Naming Acids whose anions contain oxygen (oxyanions)

  13. Acids whose oxyanions end with “ate”: • use root name of oxyanion + “ic” • then add “acid” • think – “I ate that acid … ic!” • H2SO4 • SO42- = sulfate • sulfuric acid • you try: H3PO4 • phosphoric acid • HC2H3O2 • acetic acid Naming Acids With “ate” Oxyanions

  14. Acids whose oxyanions end with “ite”: • use root name of oxyanion + “ous” • then add “acid” • ex: H2SO3 • SO32- = sulfite • sulfurous acid • You try: HNO2 • nitrous acid • HClO • hypochlorous acid Naming Acids With “ite” Oxyanions