Electron Arrangements
Schrodinger proposed a theory that more specifically described the location of the electrons into orbitals. This provided chemists the ability
to write an electron configuration for an atom, and use this configuration to explain many of the chemical properties of an atom.
Whole numbers are used to denote the main energy level. Level 1 is lower in energy than level 2, and level 2 is lower than 3, etc. Within the
main energy level are sublevels that more accurately describe the electron’s orbital. These are labeled s, p, d, f, etc. The s orbital fills first,
then the p, and so on.
Finally we use a superscript number to represent how many electrons are actually in that orbital.
↿⇂
↿⇂
↿⇂ ↿⇂ ↿⇂
↿⇂
↿⇂ ↿⇂ ↿⇂
↿
↿
↿
↿⇂
Vanadium has 23 electrons
In a Orbital Filling Diagram:
In Electron Configuration:
In Dot Diagram
1s2 2s2 2p6 3s2 3p6 4s2 3d3
4s2 = · V ·
Only the s and p electrons of the biggest quantum number count towards valence electrons. Dots 1-4
are spread to the four sides of the symbol, and then dots 5-8 double up.
Assignment:
For each element listed below:
1) Fill in the Orbital Filling Diagram – go in the order on the P.T., not the order of the boxes
2) Write the electron configuration
3) Draw electron dot diagrams
Then answer the questions.
Assortment #1.
1. Barium (Ba)
2. Chromium (Cr)
3. Fluorine (F)
4. Gadolinium (Gd)
5. Mercury (Hg)
6. Nitrogen (N)
7. Platinum (Pt)
8. Plutonium (Pu)
9. Scandium (Sc)
10. Silicon (Si)
Assortment #2
1. Aluminum (Al)
2. Arsenic (As)
3. Calcium (Ca)
4. Copper (Cu)
5. Gallium (Ga)
6. Iodine (I)
7. Krypton (Kr)
8. Radon (Rn)
9. Rhodium (Rh)
10. Samarium (Sm)
Be sure to complete your assigned assortment!
Assortment #3
1. Americium (Am)
2. Chlorine (Cl)
3. Germanium (Ge)
4. Europium (Eu)
5. Phosphorus (P)
6. Silver (Ag)
7. Strontium (Sr)
8. Tin (Sn)
9. Xenon (Xe)
10. Zirconium (Zr)
Assortment #4
1. Argon (Ar)
2. Berkelium (Bk)
3. Bromine (Br)
4. Chromium (Cr)
5. Magnesium (Mg)
6. Palladium (Pd)
7. Promethium (Pm)
8. Antimony (Sb)
9. Yttrium (Y)
10. Zinc (Zn)
Assortment #5
1. Astatine (At)
2. Beryllium (Be)
3. Bismuth (Bi)
4. Californium (Cf)
5. Molybdenum (Mo)
6. Neodymium (Nd)
7. Neon (Ne)
8. Nickel (Ni)
9. Technetium (Tc)
10. Titanium (Ti)
Assortment #6
1. Boron (B)
2. Cadmium (Cd)
3. Indium (In)
4. Iron (Fe)
5. Manganese (Mn)
6. Radium (Ra)
7. Sodium (Na)
8. Sulfur (S)
9. Tungsten (W)
10. Uranium (U)
1.
Element Name =
a. orbital notation =
b. electron configuration =
c. dot diagram =
2. Element Name =
a. orbital notation =
b. electron configuration =
c. dot diagram =
3. Element Name =
a. orbital notation =
b. electron configuration =
c. dot diagram =
4. Element Name =
a. orbital notation =
b. electron configuration =
c. dot diagram =
5. Element Name =
a. orbital notation =
b. electron configuration =
c. dot diagram =
6. Element Name =
a. orbital notation =
b. electron configuration =
c. dot diagram =
7. Element Name =
a. orbital notation =
b. electron configuration =
c. dot diagram =
8. Element Name =
a. orbital notation =
b. electron configuration =
c. dot diagram =
9. Element Name =
a. orbital notation =
b. electron configuration =
c. dot diagram =
10. Element Name =
a. orbital notation =
b. electron configuration =
c. dot diagram =
Answer the following questions using a complete sentence.
1. The orbital filling diagram has arrows pointing in opposite directions when two electrons occupy the same orbital. What do these arrows
indicate?
2. How many electrons do the elements in group IIA of the periodic table have in their electron dot diagram?
3. Element X has a dot diagram with 5 dots. Name at least two elements that could be element X.
4. Which element would have the following orbital filling diagram?
↿⇂ □□□
↿⇂ ↿ ↿
…□
5s
5p
5. What will be the importance of the valence (outer most) electrons, which are the only ones shown in question 4 and are the only ones
included in the electron dot diagrams?