MSE101

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Department
Materials Science & Engineering
Course
MSE101H1
Professor
Scott Ramsay
Semester
Spring

Description
Atomic  Structure  and  Interatomic  Bonding     Fundamental  Concepts     Atomic  number  (Z)  –  number  of  protons     Atomic  mass  (A)  –  sum  of  masses  of  protons  and  neutrons  within  nucleus     Atomic  weight  –  weighted  average  of  the  atomic  masses  of  an  atom’s  naturally   occurring  isotopes     Bohr  atomic  model  –  electrons  assumed  to  revolve  around  atomic  nucleus  in   discrete  orbitals.  Wavicle  model  was  later  adopted  (lol  visit  dennismercier.com)     Principal  quantum  number  (n)  –  shell  of  electron  (n  =  1,2,3,4…)     Angular  quantum  number  (l)  -­‐  shape  of  the  orbital   Magnetic  quantum  number  (m)  -­‐  number l of  orbitals  and  their  orientation  within  a   subshell   Electron  spin  quantum  number  (m )  -­‐  designstes  the  direction  of  the  electron  spin   and  may  have  a  spin  of  +1/2,  represented  by↑,  or  –1/2,  represented  by  ↓     Bonding  Forces  and  Energies         Primary  Interatomic  Bonds       Ionic  Bonding     ▯ For  attractive  energy:  𝐸 =▯ −   ▯ ▯ For  repulsive  energy:  𝐸 = ▯   ▯▯   Covalent  Bonding     -­‐sharing  of  electrons  between  adjacent  atoms     -­‐covalent  bond  is  directional     %  𝑖𝑜𝑛𝑖𝑐  𝑐ℎ𝑎𝑟𝑎𝑐𝑡𝑒𝑟 = 1 − exp − 0.25 𝑋 − 𝑋 ▯ ▯ ▯  ×  100     Metallic  Bonding     -­‐valence  electrons  form  an  electron  cloud     -­‐remaining  non-­‐valence  electrons  and  atomic  nuclei  form  ion  cores,  which  posses  a   net  positive  charge  equal  in  magnitude  to  total  valence  electron  charge  per  atom     -­‐non-­‐directional:  free  electrons  shield  positively  charged  ion  cores  from  mutually   repulsive  electrostatic  forces    
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