#8 Write the electron configuration
for each atom.
a. carbon
1s22s22p2
http://cwx.prenhall.com/bookbind/pubbooks/hillchem3/medialib/media_portfolio/08.
#8b. argon
argon has 18 electrons
1s22s22p63s23p6
#8c. nickel
nickel has 28 electrons
2
2
6
2
6
2
8
1s 2s 2p 3s 3p 4s 3d
or it can be written:
2
2
6
2
6
8
2
1s 2s 2p 3s 3p 3d 4s
#9a. boron
boron has 5 electrons
2
2
1
1s 2s 2p
#9b. silicon
silicon has 14 electrons
2
2
6
2
2
1s 2s 2p 3s 3p
#10
aufbau principle
Pauli exclusion principle
Hund’s rule
Aufbau Principle
Think: “falling off the bow to the
lowest bottom. (of the lake)”
Link to Orbital Diagram Practice Page
More Electron Configuration practice LINK
Pauli exclusion principle
Think: “exclusive dinner for only
two”
Hund’s Rule
Think: “the Huns wanted
more space”
http://intro.chem.o
#11 Explain why the actual electron
configurations for some elements
differ from those assigned using
the aufbau principle.
You can see it in this
website (click on the pic.
when filling the 3d orbitals)
#12. Use fig 5.7 to arrange the following
sublevels in order of decreasing energy
2p, 4s, 3s, 3d, 3p.
3d
4s
3p
3s
2p
#13 Why does one electron in a
potassium atom go into the fourth
energy level instead of squeezing
into the third energy level along
with the eight already there?
2
2
6
2
6
1
1s 2s 2p 3s 3p 4s
Because the sublevels, 3s and 3p
are already filled. The next electron
has to find a slightly higher
energy level to go to.