Transcript Atomic Orbitals

ATOMIC ORBITALS
Schrodinger’s Quantum Mechanics
Model
ORBITALS – AREAS WITHIN ATOMS WHERE
THERE IS A HIGH PROBABILITY OF
FINDING ELECTRONS
Principal Energy Levels - A region
around the nucleus of an atom
where the electron is likely to be
moving. (n = 1 , 2 , 3 , 4 , etc.)
 Number 1-7 on periodic table down side.
ENERGY SUBLEVELS
Energy sublevels can be thought of as a section of
seats in a theater. The rows that are higher up and
farther from the stage contain more seats, just as
energy levels that are farther from the nucleus
contain more sublevels.
Sublevels are labeled s, p, d, and f according to the
shapes of the atom’s orbitals.
ATOMIC ORBITALS
 Each orbital may contain at most 2 electrons.
 Each energy level may contain at most 1 s orbital, 3 p orbitals, 5
d orbitals, and 7 f orbitals. (all odd numbers) .
Energy Level
# of Sublevels
(types of orbitals present)
# of Orbitals
# of Electrons
1
s
1
2
2
s
p
1s
3p
8
3
s
p
d
1s
3p
5d
18
4
s
p
d
f
1s
3p
5d
7f
32
LABEL AND OUTLINE THE S, P, D, AND F BLOCKS
ON THE PT AS SHOWN BELOW (ANY 4
COLORS)
LABEL THE SUBLEVELS (1S, 2S, ……)
PRACTICE: READ LIKE A BOOK
 Hydrogen (1 electron) : 1s1
 Helium(2 electrons): 1s2
 Lithium(3 electrons): 1s2, 2s1
 Beryllium(4 electrons): 1s2. 2s2
 Carbon(6 electrons): 1s2, 2s2, 2p2
 Iron(26 electrons): 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d6
 You try: Sulfur ( ___ electrons): _____________________
 Bromine (___ electrons): _______________________
MORE PRACTICE
Do page 9 that you got yesterday.
“Practice #1 – electron configuration”