Atomic Orbitals Where do we put all of the electrons?
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Transcript of Atomic Orbitals Where do we put all of the electrons?
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Atomic Orbitals
Where do we put all of the electrons?
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Different Models of Same Atom
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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.
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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
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Potential (aka Positional) Energy
It takes a certain amount of energy to move away from something that is pulling you.
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• Potential Energy – the energy related to something’s position.
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• Potential Energy – the energy related to something’s position.
• Objects have greater potential energy when they are further away from the Earth.
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What about Potential Energy in Atoms?
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• 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.
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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
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Quantum Dropreleased energy from light allows an electron to fall to a lower energy level
light
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Quantum Dropreleased energy from light allows an electron to fall to a lower energy level
light
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Einstein’s Photoelectric Effectphoto – having to do with light.electric – having to do with electrons.
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The Photoelectric Effect
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The Photoelectric Effect
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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.
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Einstein’s Photoelectric Effectphoton – a single particle (or packet) of light
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Einstein’s Photoelectric Effectphoton – a single particle (or packet) of light
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Orbitals• 2 electrons per orbital.
• Different shapes and energy levels.
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s-orbitals
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p-orbitals
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px-orbital
x-axis
y-axis
z-ax
is
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py-orbital
x-axis
y-axisz-
axis
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pz-orbital
x-axis
y-axisz-
axis
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d-orbitals
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f-orbitals
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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
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Where do they put all of these electrons?!
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Where do they put all of these electrons?!
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Where do they put all of these electrons!
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Where do they put all of these electrons?!
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Where do they put all of these electrons?!
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Where they put all of these electrons?!
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s-block
p-block
d-block
f-block
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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
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7s 7p 7d 7f6s 6p 6d 6f5s 5p 5d 5f4s 4p 4d 4f3s 3p 3d2s 2p1s
Incr
easi
ng E
nerg
y
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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 ?
?
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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
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Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
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Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s1
H
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Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s2
He
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Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s1
Li
![Page 52: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/52.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s2
Be
![Page 53: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/53.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p1
B
![Page 54: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/54.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p2
C
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Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p3
N
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Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p4
O
![Page 57: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/57.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p5
F
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Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p6
![Page 59: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/59.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s1
![Page 60: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/60.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s2
![Page 61: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/61.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p1
![Page 62: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/62.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p2
![Page 63: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/63.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p3
![Page 64: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/64.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p4
![Page 65: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/65.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p5
![Page 66: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/66.jpg)
Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p6
![Page 67: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/67.jpg)
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
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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)
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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
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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
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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
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NeFONCBBe
He
Li
H
Kr
ArCl
Br
XeI
SPSiMg Al
Ca
Na
K
![Page 74: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/74.jpg)
NeFONCBBe
He
Li
H
Kr
ArCl
Br
XeI
SPSiMg Al
Ca
Na
K
![Page 75: Atomic Orbitals Where do we put all of the electrons?](https://reader036.fdocuments.in/reader036/viewer/2022062314/56649e755503460f94b76ab8/html5/thumbnails/75.jpg)
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Incr
easi
ng E
nerg
y
1s
2s
3s
2p
3p
n = 1
n = 2
n = 3
electron configuration:
1s22s22p63s23p6
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4 e– in valence shell
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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
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C CH H