molecule with covalent bond o Formula unit with ionic bond * Molecules: formed by covalent bonds * Lattice energy is the energy released in the formation of an ionic compound. DEFINITION: The formation of an IONIC BOND is the result of the transfer of one or more electrons from a metal onto a non-metal. Characteristics of both bonds: * Occur between 2 atoms * Composed of 2 electrons * Have both ionic and covalent characteristics * Together = 100% * Both bonds are measured on
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Free rotation about the single C-C bond prevents it. 33) 2-methyl propene has the Lewis structure: Is cis-trans isomerism possible for this oxalic acid? 34) For each pair of bonds‚ predict which will be the shorter. (a) B-Cl or Ga-Cl (b) C-O or Sn-O (c) P-S or P-O (d) the C=C or the C=O bond in acrolein H2O=CH-C=OH 35) For each pair of bonds‚ predict which will be the shorter. (a) Si-N or P-O (b) Si-O or C-O (c) C-F or C-Br (d) the C=C bond or the C=N bond in acrylonitrile‚ H2C=CH-C=N 37)
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Building materials of a cell are composed of two atoms that form molecules. A chemical bond is created when two atoms share an electron. Also called covalent bond because they share valence electrons. A covalent bond‚ which is the strongest bond‚ takes action when two atoms valence overlap. For example‚ there are two suns and the light that shines from the two solid spheres forms many rays making a radiant cloud around each of the two. If these suns move closer together the radiant shine would
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Chem 201 /HW#10 Chapter 9 Electronegativity Table: use this table to answer Q [pic] 1. Bromine tends to form a monatomic ion which has the electronic configuration of a noble gas. What is the electron configuration of that noble gas? a. 1s2 2s2 2p6 3s2 3p6 3d10 4p6 b. 1s2 2s2 2p6 3s2 3p6 4p6 4d10 c. 1s2 2s2 2p6 3s2 3p6 4s2 4p6 d. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 e. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 2. Which ion of
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http://wwwchem.uwimona.edu.jm:1104/courses/CFT.html Galvanic Cell animation Acid base animations Crystal field theory Audio Visual Aids Sr No AV-1 AV-2 (AV aids) (only if relevant to the course) http://ocw.mit.edu/courses/chemistry/5-111-principles-of-chemical-science-fall2008/video-lectures/lecture-2/ Salient Features video on
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Element: Simplest form of matter to have unique chemical properties. Atom: The smallest particles with unique chemical identities. Nucleus: Center of an atom (composed of protons and neutrons). Proton: Have a single positive charge (+1). Neutron: Have no charge. Electron: Tiny particles with a single negative charge and very low mass (-1)/determines chemical bonding properties of an atom. Atomic Number: Number of protons in the nucleus. Atomic Mass: Approximate number of protons and neutrons
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Chapter 1 Carbon Compounds and Chemical Bonds. (Covered material: 1.1 - 1.8; 1.12 - 1.17) 1. Structural Theory – most fundamental theory of Organic Chemistry (developed independently by A. Kekule‚ A. Couper and A. Butlerov between 1858 and 1861). Organic Compounds – compounds of carbon and hydrogen. Other elements frequently found in organic compounds are: oxygen‚ nitrogen and halogens (F‚ Cl‚ Br‚ I); less frequently found are: sulfur and phosphorus. Review Periodic Table for determining valence
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Chapter 2 The Chemical Context of Life PowerPoint Lectures for Biology‚ Seventh Edition Neil Campbell and Jane Reece Copyright © 2005 Pearson Education‚ Inc. publishing as Benjamin Cummings • Overview: Chemical Foundations of Biology Copyright © 2005 Pearson Education‚ Inc. publishing as Benjamin Cummings • The bombardier beetle uses chemistry to defend itself Figure 2.1 Copyright © 2005 Pearson Education‚ Inc. publishing as Benjamin Cummings • Concept 2.1: Matter consists
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Year 11 Module 1 – The Chemical Earth The Earth is made up of a large number of different substances: elements‚ compounds & mixtures We can classify elements & compounds as pure substances. These are always HOMOGENEOUS. Mixtures are not pure substances and can be either homogeneous or HETEROGENEOUS. Pure substances have a fixed composition eg copper metal‚ sulfur‚ carbon dioxide (CO2)‚ methane (CH4). Mixtures have variable composition and can also be separated into its components relatively
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MULTIPLE BOND PRESENTED BY: WASIQUE AZHAR MSC CHEM (2 SEM) Some basic concept Electrophile : a species with a region of positive or partial positive charge electron-poor Nucleophile: a species with a region of negative or partial negative charge electron-rich TO LERN OBJECTIVE : Elecrophilic Addition to carbon-carbon double bond Stereochemistry of Elecrophilic addition reaction Hydrogenation of double and triple bond Nucleophilic Addition to carbon-carbon double bond Regio and
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