BIOL 1441 1ST Edition Lecture 2 Outline of Last Lecture I Structure II Energy III Chemical properties Outline of Current Lecture I Bonds Current Lecture I Bonds i Unpaired electrons reactive ii Combine other atoms to fill valence shells iii 3 main types 1 covalent strongest like marriage 2 ionic positive and negative chill next to each other dating 3 hydrogen weakest one night stand a covalent bonds i pair of valence electrons is shared 1 orbitals overlap ii molecule 2 or more atoms held together by a covalent bond iii compound consists of 2 or more different atoms 1 water molecule iv single covalent bond hydrogen molecule share 1 electron 1 H H v Double covalent bond oxygen molecule 1 O O vi Bonding capacity valence 1 Valence number of electrons it takes to fill the valence shell periodic table trick vii Nonpolar covalent bond electros are shared equally no charge 2 atoms of the same element 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 viii Polar covalent bond electrons NOT shared equally charged water molecule ix Electronegativity attraction of an atom for the electrons in a covalent bond CANT CHANGE 1 The more electronegative an atom more strongly it pulls shared electrons to itself a Oxygen and nitrogen very electronegative High electronegativity Oxygen Nitrogen Non polar Low electronegativity Carbon Hydrogen Polar O O N N C C H H C H water molecule molecule H2O o Delta partial charge O C O H N C N H b Ionic bonds between oppositely charged molecules or atoms i Ion charged atom or molecule lose gain electron ii More electronegative atom strips an electron completel away from another making it an ion 1 Lose electron positive charge cation 2 Gain electron negative charge anion iii TRANSFERRING THE ELECTRON IS NOT THE FORMATION OF AN IONIC BOND iv Transfer of electron creates two ions v Ionic compounds salts 1 In nature found as crystals 3D lattice 2 Only has a ratio of element a NaCl 1 1 b MgCl2 1 2 c NH4Cl 1 1 c Hydrogen bond bond between polar molecules i Hydrogen atom covalently bonded to one electronegative atom in anoter polar covalent bond ii Easy to pull apart to replicate iii Weak interactionsd
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