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CHM103 Week 5 Class Notes (9/19-9/23)

by: askcch

CHM103 Week 5 Class Notes (9/19-9/23) 103

Marketplace > University of Miami > Chemistry > 103 > CHM103 Week 5 Class Notes 9 19 9 23
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About this Document

These notes cover 3.1-3.3
Chemistry for Life Sciences I (Lecture)
Elliot Atlas
Class Notes
Chemistry, CHM103
25 ?




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This 3 page Class Notes was uploaded by askcch on Friday September 23, 2016. The Class Notes belongs to 103 at University of Miami taught by Elliot Atlas in Fall 2016. Since its upload, it has received 12 views. For similar materials see Chemistry for Life Sciences I (Lecture) in Chemistry at University of Miami.


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Date Created: 09/23/16
  CHM103    Class     otes     eek      (9/19­9/23)  ________________________________________________________________________________  From     revious    ections   ­ 2.4­2.8  ­ Periodic   Table,  Characteristics  of  Different   Groups,   Electron   Configuration   ________________________________________________________________________________  Chapter   3: Ionic  Compounds  ­ 3.1   ons  ­ Alkali  metals   (group  1A)   form  compounds  with  halogens   (group  7A)  ­ Properties   of these   compounds   include:  ­ High   melting   points  ­ Stable,    hite,  crystalline   solids  ­ Soluble  in  water  ­ Conduct     lectricity   hen     issolved   in water  ­ * Electricity  can   only  flow  through   a medium  containing  charged   particles   (ions)   hat  are   ree  o  move  ­ An  ion  is formed   when   a neutral   atom   gains   or loses   electrons  ­ The   loss  of electron(s)   gives   a positively   charged  ion  called  a  cation  ­   ­ The   gain  of  electron(s)   gives   a negatively   charged   ion  called  an  anion  ­   ­ Positive   charge   =     ; Negative  charge   =     (which  n  is any  integer)     ­ 3.2 Ions   and    he    ctet  Rule  ­ Octet  rule:  Main  group   elements   tend   to undergo   reactions   that leave   them  with    ight valence  electrons  ­ E.g.  Alkali  metals   with   a single   valence   electron  react   with  halogens  with   seven  valence  electrons,  giving   both  ns np   6 configurations   with  eight   valence   electrons   (i.e. noble   gas   electron   configuration)  ­ E.g.  N:  1s 2s 2p  →     N  :  1s 2s 2p   6 ­ 3.3  ons   of Some     ommon   Elements  ­   ­ Transition   metals  form  cations,   but  they  can   lose  one   or  more  d  electrons  in addition  to  losing     alence   s electrons.    he  octet    ule  is not   ollowed.    ­ Metals   form   cations   by  losing   one  or  more   electrons  ­ Reactive   nonmetals   form   anions  by   gaining   one   or  more   electrons  to  achieve     noble     as    onfiguration  ­ Group   8A  elements   (noble   gases)   are    nreactive  ­ Ionic  charges  of  main   group   elements   can  be  predicted   using   the  group  number     nd the  octet   rule  ­ E.g.  1A   =      2A     X      ­ E.g.    A    X   , 6A  =         A    X          


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