SCH4U - Atomic Structure Unit Outline

• Atomic models (Dalton, Thomson, Rutherford, Chadwick & Bohr)
• sketch of the model and a brief description of each model (epn anyone?)
• Blackbody radiation & photoelectric effect
• Spectral lines leading to Bohr
• bright and dark line spectrum of hydrogen
• 
  
  connecting the both line spectra to the Bohr model
• Spectral line splitting
• further refinements of the Bohr model
• in terms of orbitals, what does each type of spectral line splitting identify?

• Energy level diagrams
• fill according to the order of filling (spdf blocks on the periodic table)

• Electron configurations (complete, kernel, special cases, ions)
• use the periodic table of elements as an aid [see Nelson page 188 for two helpful diagrams]
• should be able to write the actual electron configuration for any element [includes the two columns of exceptions]
• from electron configuration (either complete or kernel) identify the appropriate electron changes to achieve an ion charge
• Quantum Numbers {n, l, m, s} and quantum model
• know the orbital significance of each quantum number
• be able to write the complete set of quantum numbers for an element
• Lewis Structure [following the rules]
• if you are going to follow the rules, then you had better know the rules, right? [Nelson text page 229]
• Atomic Modeling [Building, 3D shapes, names, bond angles]
• memorize the basic attributes of the various shapes [Nelson text pages 243-245]
• Hybridization (sp3, sp2 and sp) - connection to molecular shapes (if you know the shape you know the type of hybridization)
• sigma and pi bonds
• sketch the hybridization
• label hybrid orbitals
• Liquid state bonding (London, dipole-dipole, hydrogen bonding)
• can you distinguish between a polar molecule and a nonpolar molecule?
• H-N, H-O and/or H-F
  
  Solid state bonding [ionic, metallic, molecular & covalent network]
• know the properties of each type of solid [summary Nelson text page 273]
• covalent network - memorize a few of them

Galvanic Cell

A few reminders:
LEO says GER
AN OX CAn'T REaD (anode = oxidation; cathode = reduction)

Copper/Zinc Galvanic cell:
http://www.ausetute.com.au/voltcell.html  (nice little animation or just look below)

• chart on page 805 identifies Cu as more likely to be reduced (it's higher on the chart) Cu2+(aq)  + 2e- --> Cu(s)
• Zn will be oxidized (Zn(s) --> Zn2+(aq)  +  2e-
• Cu = cathode; Zn = anode
• Cu2+(aq) ions in solution will attach to the Cu eletrode as Cu(s)
• Zn(s) electrode will slowly dissolve creating Zn2+(aq) ions
• Salt bridge ions move to create electrically neutral solutions, soooo K+(aq) ions to copper solution (replacing Cu2+(aq) ions that left; Cl-(aq) ions move to electrical neutralize the added Zn2+(aq) ions)
• electrons flow to the copper electrode (afterall, the copper ions are being reduced GER!)
• standard cell notation Zn(s)|Zn2+(aq)||Cu2+(aq)|Cu(s)
• overcell reaction shown below

Anode:     Zn  ---> Zn2+ + 2e          Eo = -0.76V
Cathode: Cu2+ + 2e ---> Cu           Eo = +0.34V
--------------------------------------------------------------------------------
Cell: Zn + Cu2+ ---> Zn2+ + Cu    Eocell = +1.10V (0.34V- (-0.76V))
(V used values agree with Nelson text)

The following site also gives a nice overview of the galvanic cell. There a few sample questions (with answers) on the site as well.
http://www.science.uwaterloo.ca/~cchieh/cact/c123/battery.html

And now for something unrelated to elctrochemical cells: Q: Are polar bears expensive to keep as pets? A: NO! They live on ice! [Such a cool joke, eh?]