atomic orbitals where do we put all of the electrons?
TRANSCRIPT
Atomic Orbitals
Where do we put all of the electrons?
Different Models of Same Atom
Reality Check• Lewis structures don’t represent what is going
on inside atoms with 100% accuracy. • But Lewis structures are useful tools that can
help us figure out chemical structures maybe 95% of the time.
• To understand what is really going on with the electrons inside of atoms we need to delve into quantum mechanics.
Quantum Mechanics• quantum – a small but incremental amount of
energy.• mechanics – study of motion and the causes
of motion.
• Weird Stuff – Quantum Leaps, You can’t pay me in pennies, Certain Uncertainty, Zombie cats, We are all made of Waves
Potential (aka Positional) Energy
It takes a certain amount of energy to move away from something that is pulling you.
• Potential Energy – the energy related to something’s position.
• Potential Energy – the energy related to something’s position.
• Objects have greater potential energy when they are further away from the Earth.
What about Potential Energy in Atoms?
• Potential Energy – the energy related to something’s position.
• Objects have greater potential energy when they are further away from the Earth.
• Electrons have greater potential energy when they are further away from the nucleus.
Quantum Leapabsorbed energy from light allows an electron to jump to a higher energy level
quantum – a distinct energy amount (no more, no less).
light
Quantum Dropreleased energy from light allows an electron to fall to a lower energy level
light
Quantum Dropreleased energy from light allows an electron to fall to a lower energy level
light
Einstein’s Photoelectric Effectphoto – having to do with light.electric – having to do with electrons.
The Photoelectric Effect
The Photoelectric Effect
Einstein’s Photoelectric Effect• Even though more red light hits the metal,
only the higher energy blue light causes the electrons to be leave the metal.
Einstein’s Photoelectric Effectphoton – a single particle (or packet) of light
Einstein’s Photoelectric Effectphoton – a single particle (or packet) of light
Orbitals• 2 electrons per orbital.
• Different shapes and energy levels.
s-orbitals
p-orbitals
px-orbital
x-axis
y-axis
z-ax
is
py-orbital
x-axis
y-axisz-
axis
pz-orbital
x-axis
y-axisz-
axis
d-orbitals
f-orbitals
So how many electrons can they hold?
Orbital Type
# of orbitals per energy
level
Full # of electrons
abbrev.
s-orbitals 1 2 e- s2
p-orbitals 3 6 e- p6
d-orbitals 5 10 e- d10
f-orbitals 7 14 e- f14
Where do they put all of these electrons?!
Where do they put all of these electrons?!
Where do they put all of these electrons!
Where do they put all of these electrons?!
Where do they put all of these electrons?!
Where they put all of these electrons?!
s-block
p-block
d-block
f-block
1 s orbital = 2 electrons
2e–
2e– 2e– 2e–
2e– 2e– 2e– 2e– 2e–
2e– 2e– 2e– 2e– 2e– 2e– 2e–
3 p orbitals = 6 electrons
5 d orbitals = 10 electrons
7 f orbitals = 14 electrons
7s 7p 7d 7f6s 6p 6d 6f5s 5p 5d 5f4s 4p 4d 4f3s 3p 3d2s 2p1s
Incr
easi
ng E
nerg
y
7s 7p 7d 7f6s 6p 6d 6f5s 5p 5d 5f4s 4p 4d 4f3s 3p 3d2s 2p1s
Incr
easi
ng E
nerg
y
?
8s 8p 8d 8f 7g 6g
5g ?
?
Incr
easi
ng E
nerg
y
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
3d
4d
5d
5f
4f
n = 1
n = 2
n = 3
n = 4
n = 5
n = 6
n = 7
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s1
H
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s2
He
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s1
Li
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s2
Be
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p1
B
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p2
C
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p3
N
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p4
O
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p5
F
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p6
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s1
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s2
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p1
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p2
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p3
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p4
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p5
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p6
Electron Configuration RulesPauli exclusion principle – no more than 2
electrons per orbital (no 2 electrons in an atom have same 4 quantum numbers).
Hund’s rule – electrons fill all of the suborbitals one at a time before they double up (favors having the same spin).
aufbau principle – electrons fill the orbitals with the lowest energy first.
2p
4 Quantum Numbers
(n, l, ml , ms )
Energy level (1, 2, 3, …)
Orbital shape or sublevel (s, p, d, f)
Orbital direction (px , py , pz)
Spin(+ ½, - ½)
Hybrid orbitals
• Example: tangerine + pomelo =
Sometimes atoms transform their own electron orbitals into hybrid orbitals so they can covalently bond with other atoms.
• hybrid – a mixture of 2 different types of something.
• Example: donkey + horse = • Example: gasoline
engine + electric motor =
tangelomule
hybrid car
s and p orbital hybridization1 s + 1 p = 2 sp orbitals
1 s + 2 p = 3 sp2 orbitals
1 s + 3 p = 4 sp3 orbitals
Weekend Homework Contest• In your home, find the most bizarre ionic
compound that you can:
• Write down: 1) where it was found (food, cleaning supply, etc.)
2) ingredient name on the label3) ionic formula (or what you
think it is)
• Example: 1) Chlorox Bleach2) sodium hypochlorite3) NaClO
NeFONCBBe
He
Li
H
Kr
ArCl
Br
XeI
SPSiMg Al
Ca
Na
K
NeFONCBBe
He
Li
H
Kr
ArCl
Br
XeI
SPSiMg Al
Ca
Na
K
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p6
4 e– in valence shell
So how many electrons can they hold?
Orbital Full # of type electrons abbrev.s-orbital 2 electrons s2
p-orbitals 6 electrons p6
d-orbitals 10 electrons d10
f-orbitals 14 electrons f14
C CH H