The document provides a tutorial on quantum numbers, electronic configuration, and de Broglie wavelength. It discusses:
1) Early models of the Bohr model and de Broglie's explanation of electrons as waves.
2) Heisenberg's uncertainty principle and how it means the exact position of an electron can never be known.
3) Schrodinger's wave function describes electrons mathematically using probability and orbital shapes rather than fixed orbits.
4) The four quantum numbers (n, l, ml, ms) that describe the specific states that electrons can occupy in an atom or molecule.
Introduction, measurement of uncertainty, Heisenberg microscope, challenges to Heisenberg principle, examples of Heisenberg uncertainty principle, applications of uncertainty principle
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for vedio click on this linkhttps://www.youtube.com/watch?v=ZzIxkWDlf5Q&feature=youtu.be
Organic compound nomenclature (ALkanes, ALKYL GROUP, ALKENE, ALKYNES)
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Report made by: Students of Sogod National High School STEM 9-Newton
Kyla Krystelle Salva
Krishia Belle Cambalon
Marycris Felicilda
Ester is one of the functional groups in organic chemistry. It is formed by combining alcohols and carboxylic acids in a process called esterification.
Organic compound nomenclature (ALkanes, ALKYL GROUP, ALKENE, ALKYNES)Tasneem Ahmad
for vedio click on this linkhttps://www.youtube.com/watch?v=ZzIxkWDlf5Q&feature=youtu.be
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The complete presentation on Organic Compound, IMPORTANCE, PROPERTIES, SOURCE, USED, Nomenclature Of Organic Compound
This is a report about Aldehydes. The content of this slideshow are as follows: What is an aldehyde, How to name aldehydes with IUPAC Nomenclature and Common Names, The Physical Properties of Aldehydes, and the examples of aldehyde and its uses. The main objective of this report is to widen the knowledge of the readers/learners concerning of the stated topic so that they can further understand the concept of aldehydes.
Report made by: Students of Sogod National High School STEM 9-Newton
Kyla Krystelle Salva
Krishia Belle Cambalon
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The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
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Macroeconomics- Movie Location
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Objective:
Prepare a presentation or a paper using research, basic comparative analysis, data organization and application of economic information. You will make an informed assessment of an economic climate outside of the United States to accomplish an entertainment industry objective.
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The Roman Empire, a vast and enduring power, stands as one of history's most remarkable civilizations, leaving an indelible imprint on the world. It emerged from the Roman Republic, transitioning into an imperial powerhouse under the leadership of Augustus Caesar in 27 BCE. This transformation marked the beginning of an era defined by unprecedented territorial expansion, architectural marvels, and profound cultural influence.
The empire's roots lie in the city of Rome, founded, according to legend, by Romulus in 753 BCE. Over centuries, Rome evolved from a small settlement to a formidable republic, characterized by a complex political system with elected officials and checks on power. However, internal strife, class conflicts, and military ambitions paved the way for the end of the Republic. Julius Caesar’s dictatorship and subsequent assassination in 44 BCE created a power vacuum, leading to a civil war. Octavian, later Augustus, emerged victorious, heralding the Roman Empire’s birth.
Under Augustus, the empire experienced the Pax Romana, a 200-year period of relative peace and stability. Augustus reformed the military, established efficient administrative systems, and initiated grand construction projects. The empire's borders expanded, encompassing territories from Britain to Egypt and from Spain to the Euphrates. Roman legions, renowned for their discipline and engineering prowess, secured and maintained these vast territories, building roads, fortifications, and cities that facilitated control and integration.
The Roman Empire’s society was hierarchical, with a rigid class system. At the top were the patricians, wealthy elites who held significant political power. Below them were the plebeians, free citizens with limited political influence, and the vast numbers of slaves who formed the backbone of the economy. The family unit was central, governed by the paterfamilias, the male head who held absolute authority.
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June 3, 2024 Anti-Semitism Letter Sent to MIT President Kornbluth and MIT Cor...Levi Shapiro
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The US House of Representatives is deeply concerned by ongoing and pervasive acts of antisemitic
harassment and intimidation at the Massachusetts Institute of Technology (MIT). Failing to act decisively to ensure a safe learning environment for all students would be a grave dereliction of your responsibilities as President of MIT and Chair of the MIT Corporation.
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unwillingness to rectify this violation through action requires accountability.
Postsecondary education is a unique opportunity for students to learn and have their ideas and beliefs challenged. However, universities receiving hundreds of millions of federal funds annually have denied
students that opportunity and have been hijacked to become venues for the promotion of terrorism, antisemitic harassment and intimidation, unlawful encampments, and in some cases, assaults and riots.
The House of Representatives will not countenance the use of federal funds to indoctrinate students into hateful, antisemitic, anti-American supporters of terrorism. Investigations into campus antisemitism by the Committee on Education and the Workforce and the Committee on Ways and Means have been expanded into a Congress-wide probe across all relevant jurisdictions to address this national crisis. The undersigned Committees will conduct oversight into the use of federal funds at MIT and its learning environment under authorities granted to each Committee.
• The Committee on Education and the Workforce has been investigating your institution since December 7, 2023. The Committee has broad jurisdiction over postsecondary education, including its compliance with Title VI of the Civil Rights Act, campus safety concerns over disruptions to the learning environment, and the awarding of federal student aid under the Higher Education Act.
• The Committee on Oversight and Accountability is investigating the sources of funding and other support flowing to groups espousing pro-Hamas propaganda and engaged in antisemitic harassment and intimidation of students. The Committee on Oversight and Accountability is the principal oversight committee of the US House of Representatives and has broad authority to investigate “any matter” at “any time” under House Rule X.
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IB Chemistry on Quantum Numbers, Electronic Configuration and De Broglie Wavelength
1. Tutorial on Quantum Number, Electronic
Configuration and De Broglie Wavelength.
Prepared by
Lawrence Kok
http://lawrencekok.blogspot.com
2. How electrons move?
•
•
Bohr Model
Electron as particle
Electron orbit in FIXED radius from nucleus
Electron – particle
Orbit
Bohr Model equation:
• Angular momentum, L = nh/2π
L=
nh
2p
mvr =
nh
2p
3. How electrons move?
•
•
Bohr Model
Electron as particle
Electron orbit in FIXED radius from nucleus
•
•
•
Quantum Model
Electron as standing wave around nucleus
Electron NOT in fixed position
ORBITAL – probability/chance finding electron
Electron – particle
Electron – Wave like nature
Orbit
Orbital
Bohr Model equation:
• Angular momentum, L = nh/2π
L=
nh
2p
mvr =
nh
2p
De Broglie wavelength equation • Electron -standing wave.
• E = mv2 and E = hf -> λ = h/mv
mv 2 = hf
mv 2 = h
v
l
Click here - electron wave
mv =
h
l
mv =
h
l
4. How electrons move?
•
•
Bohr Model
Electron as particle
Electron orbit in FIXED radius from nucleus
•
•
•
Quantum Model
Electron as standing wave around nucleus
Electron NOT in fixed position
ORBITAL – probability/chance finding electron
Electron – particle
Electron – Wave like nature
Orbit
Orbital
De Broglie wavelength equation • Electron -standing wave.
• E = mv2 and E = hf -> λ = h/mv
Bohr Model equation:
• Angular momentum, L = nh/2π
L=
nh
2p
mvr =
nh
2p
mv 2 = hf
mv 2 = h
v
l
Click here - electron wave
mv =
h
l
mv =
h
l
Combine Bohr and De Broglie
mvr =
nh
2p
h
l
r=
nh
2p
nl = 2p r
nλ = 2πr
What does, nλ = 2πr means ?
•
•
•
•
Orbit/circumference - exact multiples of electron wavelength
Circumference of orbit- equal t0 1x wavelength, 2x wavelength,
3x wavelength or multiple of its wavelength, nλ
Electron as standing wave around the nucleus
Wavelength fits around the circumference of the orbit
5. Electron Wavelength around orbit
•
•
•
•
Electron acts as standing wave surrounding the nucleus
Wavelength fits around the circumference of the orbit
Orbit/circumference - exact multiples of electron wavelength
Circumference of orbit- equal the wavelength, 2x wavelength, 3x wavelength or multiple of its wavelength, nλ
nλ = 2πr
n=1
1λ = 2πr1
ONE wavelength λ fits the 1st orbit
n=2
2λ = 2πr2
TWO wavelength λ fits the 2nd orbit
n=3
3λ = 2πr3
THREE wavelength λ fits the 3rd orbit
6. Electron Wavelength around orbit
•
•
•
•
Electron acts as standing wave surrounding the nucleus
Wavelength fits around the circumference of the orbit
Orbit/circumference - exact multiples of electron wavelength
Circumference of orbit- equal the wavelength, 2x wavelength, 3x wavelength or multiple of its wavelength, nλ
nλ = 2πr
n=1
1λ = 2πr1
ONE wavelength λ fits the 1st orbit
n=2
2λ = 2πr2
TWO wavelength λ fits the 2nd orbit
n=3
3λ = 2πr3
THREE wavelength λ fits the 3rd orbit
Standing wave around the circumference /circle
1λ
ONE wavelength λ fits the 1st orbit
1st Orbit
2λ
TWO wavelength λ fits the 2nd orbit
3λ
2nd Orbit
THREE wavelength λ fits the 3rd orbit
3rd Orbit
7. Electron Wavelength around orbit
•
•
•
•
Electron acts as standing wave surrounding the nucleus
Wavelength fits around the circumference of the orbit
Orbit/circumference - exact multiples of electron wavelength
Circumference of orbit- equal the wavelength, 2x wavelength, 3x wavelength or multiple of its wavelength, nλ
nλ = 2πr
n=1
1λ = 2πr1
ONE wavelength λ fits the 1st orbit
n=2
2λ = 2πr2
TWO wavelength λ fits the 2nd orbit
n=3
3λ = 2πr3
THREE wavelength λ fits the 3rd orbit
Standing wave around the circumference /circle
1λ
ONE wavelength λ fits the 1st orbit
1st Orbit
2λ
TWO wavelength λ fits the 2nd orbit
3λ
2nd Orbit
THREE wavelength λ fits the 3rd orbit
3rd Orbit
Relationship between wavelength and circumference
a o = 0.0529nm/Bohr radius
1λ
n=1
n=2
ONE wavelength λ
TWO wavelength λ
r n = n2 a 0
1λ1 = 2πr1
2λ
2λ2 = 2πr2
λ1 = 6.3 ao - 1st orbit
r n = n2 a 0
λ2= 12.6 ao - 2nd orbit
3λ
n=3
THREE wavelength λ
3λ3 = 2πr3
r n = n2 a 0
λ3 = 18.9 ao - 3rd orbit
8. Electron Wavelength around orbit
•
•
•
•
Electron acts as standing wave around the nucleus
Wavelength fits around circumference of orbit
Orbit/circumference - exact multiples of electron wavelength
Circumference of orbit- equal t0 1x wavelength, 2x wavelength, 3x wavelength or multiple of its wavelength, nλ
nλ = 2πr
ONE wavelength λ fits the 1st orbit
n=1
λ = 2πr1
n=2
2λ = 2πr2
TWO wavelength λ fits the 2nd orbit
n=3
3λ = 2πr3
THREE wavelength λ fits the 3rd orbit
Standing wave around the circumference /circle
λ
ONE wavelength λ fits the 1st orbit
1st Orbit
λ
TWO wavelength λ fits the 2nd orbit
λ
2nd Orbit
THREE wavelength λ fits the 3rd orbit
Click here to view video
Click here to view notes
Click here - electron wave simulation
9. Models for electronic orbitals
1913
1925
Bohr Model
De Broglie wavelength
Electron in fixed orbits
Electron form a standing wave
1927
Heisenberg Uncertainty principle
10. Models for electronic orbitals
1913
Bohr Model
1927
1925
De Broglie wavelength
Electron in fixed orbits
Electron form a standing wave
Heisenberg Uncertainty principle
•
•
Impossible to determine both the
position and velocity of electron at the same time.
Applies to electron, small and moving fast..
Probability/chance/likelyhood to find electron in space
ORBITAL is used to replace orbit
Δx = uncertainty in position
Δp = uncertainty in momentum/velocity
(ħ)= reduced plank constant
11. Models for electronic orbitals
1927
1913
1925
Bohr Model
De Broglie wavelength
Electron in fixed orbits
Heisenberg Uncertainty principle
•
Electron form a standing wave
•
Impossible to determine both the
position and velocity of electron at the same time.
Applies to electron, small and moving fast..
If we know position, x very precisely – we don’t know its momentum, velocity
Δp
electron
Δx
Big hole
electron
Δx
electron
Probability/chance/likelyhood to find electron in space
Δx
ORBITAL is used to replace orbit
Small hole
Reduce the hole smaller, x
Know precisely x, electron position
Uncertainty Δx is small ( Δx, Δp)
Δp is high so Δx Δp > h/2
Δp high – uncertainty in its velocity is high
Position of electron is unknown!
Δp = mass x velocity
Velocity is unknown
Δx = uncertainty in position
Δp = uncertainty in momentum/velocity
(ħ)= reduced plank constant
Probability/likelyhood to find an electron in space
12. Uncertainty for electron in space
1913
Bohr Model
1927
1925
De Broglie wavelength
Electron in fixed orbits
Electron form a standing wave
Heisenberg Uncertainty principle
•
•
Impossible to determine both the
position and velocity of electron at the same time.
Applies to electron, small and moving fast..
If we know position, x very precisely – we don’t know its momentum, velocity
Probability/chance/likelyhood to find an electron
ORBITAL is used to replace orbit
Excellent video on uncertainty principle
Click here video on uncertainty principle
Video on uncertainty principle
Click here to view uncertainty principle
Δx = uncertainty in position
Δp = uncertainty in momentum/velocity
(ħ)= reduced plank constant
14. Schrödinger's wave function.
1927
•
•
Schrödinger's wave function.
Mathematical description of electron given by wave function
Amplitude – probability of finding electron at any point in space/time
High probability
finding electron
electron density
•
•
•
Probability finding electron in space
Position electron unknown
Orbital ✔ NOT orbit ✗ used
is
•
•
•
Probability find electron distance from nucleus
Probability density used- Ψ2
Orbital NOT orbit is used
ORBITAL is used to replace orbit
ORBITAL• Mathematical description wavelike nature electron
• Wavefunction symbol – Ψ
• Probability finding electron in space
15. Schrödinger's wave function.
1927
•
•
Schrödinger's wave function.
Mathematical description of electron given by wave function
Amplitude – probability of finding electron at any point in space/time
High probability
finding electron
electron density
•
•
•
Bohr Model
✗
•
•
•
Probability finding electron in space
Position electron unknown
Orbital ✔ NOT orbit ✗ used
is
Schrödinger's wave function.
Probability find electron distance from nucleus
Probability density used- Ψ2
Orbital NOT orbit is used
✔
ORBITAL is used to replace orbit
ORBITAL• Mathematical description wavelike nature electron
• Wavefunction symbol – Ψ
• Probability finding electron in space
better description
electron behave
Click here to view simulation
16. Schrödinger's wave function.
1927
•
•
Schrödinger's wave function.
Mathematical description of electron given by wave function
Amplitude – probability of finding electron at any point in space/time
High probability
finding electron
electron density
•
•
•
Bohr Model
✗
•
•
•
Probability finding electron in space
Position electron unknown
Orbital ✔ NOT orbit ✗ used
is
Schrödinger's wave function.
Probability find electron distance from nucleus
Probability density used- Ψ2
Orbital NOT orbit is used
✔
ORBITAL is used to replace orbit
ORBITAL• Mathematical description wavelike nature electron
• Wavefunction symbol – Ψ
• Probability finding electron in space
better description
electron behave
Click here to view simulation
Click here to view simulation
Click here to view simulation
17. Four Quantum Numbers
•
•
•
1
Electrons arrange in specific energy level and sublevels
Orbitals of electrons in atom differ in size, shape and orientation.
Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ’ms’ - (n, l, ml, ms)
Principal Quantum Number (n): n = 1, 2, 3,.. ∞
• Energy of electron and size of orbital/shell
• Distance from nucleus, (higher n – higher energy)
• Larger n - farther e from nucleus – larger size orbital
• n=1, 1stprincipal shell ( innermost/ground shell state)
No TWO electron have same
4 quantum number
18. Four Quantum Numbers
•
•
•
Electrons arrange in specific energy level and sublevels
Orbitals of electrons in atom differ in size, shape and orientation.
Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ’ms’ - (n, l, ml, ms)
1
Principal Quantum Number (n): n = 1, 2, 3,.. ∞
• Energy of electron and size of orbital/shell
• Distance from nucleus, (higher n – higher energy)
• Larger n - farther e from nucleus – larger size orbital
• n=1, 1stprincipal shell ( innermost/ground shell state)
2
Angular Momentum Quantum Number (l): l = 0 to n-1.
• Orbital Shape
• Divides shells into subshells/sublevels.
• Letters (s, d, p, f)
s orbital
p orbital
d orbital
No TWO electron have same
4 quantum number
19. Four Quantum Numbers
•
•
•
Electrons arrange in specific energy level and sublevels
Orbitals of electrons in atom differ in size, shape and orientation.
Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ’ms’ - (n, l, ml, ms)
1
Principal Quantum Number (n): n = 1, 2, 3,.. ∞
• Energy of electron and size of orbital/shell
• Distance from nucleus, (higher n – higher energy)
• Larger n - farther e from nucleus – larger size orbital
• n=1, 1stprincipal shell ( innermost/ground shell state)
2
Angular Momentum Quantum Number (l): l = 0 to n-1.
• Orbital Shape
• Divides shells into subshells/sublevels.
• Letters (s, d, p, f)
s orbital
p orbital
d orbital
3
No TWO electron have same
4 quantum number
Magnetic Quantum Number (ml): ml = -l, 0, +l.
• Orientation orbital in space/direction
• mℓ range from −ℓ to ℓ,
• ℓ = 0 -> mℓ = 0
–> s sublevel -> 1 orbital
• ℓ = 1 -> mℓ = -1, 0, +1
-> p sublevel -> 3 diff p orbitals
• ℓ = 2 -> mℓ = -2, -1, 0, +1, +2 -> d sublevel -> 5 diff d orbitals
• (2l+ 1 ) quantum number for each ℓ value
20. Four Quantum Numbers
•
•
•
Electrons arrange in specific energy level and sublevels
Orbitals of electrons in atom differ in size, shape and orientation.
Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ’ms’ - (n, l, ml, ms)
1
Principal Quantum Number (n): n = 1, 2, 3,.. ∞
• Energy of electron and size of orbital/shell
• Distance from nucleus, (higher n – higher energy)
• Larger n - farther e from nucleus – larger size orbital
• n=1, 1stprincipal shell ( innermost/ground shell state)
2
Angular Momentum Quantum Number (l): l = 0 to n-1.
• Orbital Shape
• Divides shells into subshells/sublevels.
• Letters (s, d, p, f)
s orbital
p orbital
3
4
No TWO electron have same
4 quantum number
Magnetic Quantum Number (ml): ml = -l, 0, +l.
• Orientation orbital in space/direction
• mℓ range from −ℓ to ℓ,
• ℓ = 0 -> mℓ = 0
–> s sublevel -> 1 orbital
• ℓ = 1 -> mℓ = -1, 0, +1
-> p sublevel -> 3 diff p orbitals
• ℓ = 2 -> mℓ = -2, -1, 0, +1, +2 -> d sublevel -> 5 diff d orbitals
• (2l+ 1 ) quantum number for each ℓ value
Spin Quantum Number (ms): ms = +1/2 or -1/2
• Each orbital – 2 electrons, spin up/down
• Pair electron spin opposite direction
• One spin up, ms = +1/2
• One spin down, ms = -1/2
• No net spin/cancel out each other– diamagnetic electron
writing electron spin
electron spin up/down
d orbital
21. Principal and Angular Momentum Quantum numbers
•
•
•
Electrons arrange in specific energy level and sublevels
Orbitals of electrons in atom differ in size, shape and orientation.
Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ’ms’ - (n, l, ml, ms)
1
Principal Quantum Number (n): n = 1, 2, 3, …, ∞
• Energy of electron and size of orbital /shell
• Distance from nucleus, (higher n – higher energy)
• Larger n - farther e from nucleus – larger size orbital
• n=1, 1stprincipal shell ( innermost/ground shell state)
2
Angular Momentum Quantum Number (l): l = 0, ..., n-1.
• Orbital Shape
• Divides shells into subshells (sublevels)
• Letters (s,p,d,f)
• < less than n-1
Sublevels, l
22. Principal and Angular Momentum Quantum numbers
•
•
•
Electrons arrange in specific energy level and sublevels
Orbitals of electrons in atom differ in size, shape and orientation.
Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ’ms’ - (n, l, ml, ms)
1
Principal Quantum Number (n): n = 1, 2, 3, …, ∞
• Energy of electron and size of orbital /shell
• Distance from nucleus, (higher n – higher energy)
• Larger n - farther e from nucleus – larger size orbital
• n=1, 1stprincipal shell ( innermost/ground shell state)
2
Angular Momentum Quantum Number (l): l = 0, ..., n-1.
• Orbital Shape
• Divides shells into subshells (sublevels)
• Letters (s,p,d,f)
• < less than n-1
Sublevels, l
Quantum number, n and l
l=1
2p sublevel
l=0
2s sublevel
n= 2
n= 1
1
Principal
Quantum #, n
(Size , energy)
l=0
2
1s sublevel
Angular momentum
quantum number, l
(Shape of orbital)
1
Principal Quantum
Number (n)
2
Angular Momentum
Quantum Number (l)
23. Principal and Angular Momentum Quantum numbers
•
•
•
Electrons arrange in specific energy level and sublevels
Orbitals of electrons in atom differ in size, shape and orientation.
Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ’ms’ - (n, l, ml, ms)
1
Principal Quantum Number (n): n = 1, 2, 3, …, ∞
• Energy of electron and size of orbital /shell
• Distance from nucleus, (higher n – higher energy)
• Larger n - farther e from nucleus – larger size orbital
• n=1, 1stprincipal shell ( innermost/ground shell state)
2
Angular Momentum Quantum Number (l): l = 0, ..., n-1.
• Orbital Shape
• Divides shells into subshells (sublevels)
• Letters (s,p,d,f)
• < less than n-1
Sublevels, l
Quantum number, n and l
l=1
2p sublevel
l=0
2s sublevel
n= 2
n= 1
1
Principal
Quantum #, n
(Size , energy)
l=0
2
1s sublevel
Angular momentum
quantum number, l
(Shape of orbital)
2p sublevel – contain 2p orbital
2nd energy level
Has TWO sublevels
2s sublevel – contain 2s orbital
1st energy level
Has ONE sublevel
1s sublevel – contain 1s orbital
1
Principal Quantum
Number (n)
2
Angular Momentum
Quantum Number (l)
24. Electronic Orbitals
n = 1, 2, 3,….
Allowed values
Energy Level
n= 3
n= 2
n= 1
1
Principal
Quantum #, n
(Size , energy)
25. Electronic Orbitals
n = 1, 2, 3,….
Allowed values
l = 0 to n-1
l=2
3d sublevel
l=1
3p sublevel
l=0
3s sublevel
l=1
2p sublevel
l=0
2s sublevel
l=0
1s sublevel
Energy Level
n= 3
n= 2
n= 1
1
Principal
Quantum #, n
(Size , energy)
2
Angular momentum
quantum number, l
(Shape of orbital)
26. Electronic Orbitals
n = 1, 2, 3,….
Allowed values
l = 0 to n-1
Allowed values
ml = -l, 0, +l- (2l+ 1 ) for each ℓ value
ml =+2
ml =+1
ml = 0
l=1
3px orbital
ml = 0
3s sublevel
3py orbital
3s orbital
ml =+1
l=0
3pz orbital
ml = 0
3p sublevel
3dxy orbital
ml =-1
l=1
3dxz orbital
ml =+1
n= 3
3dz2 orbital
ml =-2
3d sublevel
3dyz orbital
ml =-1
l=2
Energy Level
3dx2 – y2 orbital
2py orbital
ml = 0
2p sublevel
2pz orbital
ml =-1
n= 2
2px orbital
l=0
1
Principal
Quantum #, n
(Size , energy)
2
ml =0
2s orbital
l=0
n= 1
2s sublevel
1s sublevel
ml =0
1s orbital
Angular momentum
quantum number, l
(Shape of orbital)
3
Magnetic Quantum
Number (ml)
(Orientation orbital)
27. Electronic Orbitals
Simulation Electronic Orbitals
n = 1, 2, 3,….
Allowed values
l = 0 to n-1
Allowed values
ml = -l, 0, +l- (2l+ 1 ) for each ℓ value
ml =+2
ml =+1
ml = 0
l=1
3px orbital
ml = 0
3s sublevel
3py orbital
3s orbital
ml =+1
l=0
3pz orbital
ml = 0
3p sublevel
3dxy orbital
ml =-1
l=1
3dxz orbital
ml =+1
n= 3
3dz2 orbital
ml =-2
3d sublevel
3dyz orbital
ml =-1
l=2
Energy Level
3dx2 – y2 orbital
2py orbital
ml = 0
2p sublevel
2pz orbital
ml =-1
n= 2
2px orbital
l=0
1
Principal
Quantum #, n
(Size , energy)
2
2s sublevel
ml =0
1s sublevel
ml =0
Click here to view simulation
2s orbital
l=0
n= 1
Click here to view simulation
1s orbital
Angular momentum
quantum number, l
(Shape of orbital)
3
Magnetic Quantum
Number (ml)
(Orientation orbital)
Click here to view simulation
30. Quantum Numbers and Electronic Orbitals
ml =+2
Energy Level
3dx2 – y2orbital
ml =+1
3dz2 orbital
3dxz orbital
ml =-2
3d sublevel
ml = 0
ml =-1
l=2
3dyz orbital
3dxy orbital
n= 3
ml =+1
l=1
3s sublevel
2p sublevel
n= 2
3pz orbital
3px orbital
ml = 0
3s orbital
ml =+1
l=0
3p sublevel
ml = 0
ml =-1
l=1
3py orbital
2py orbital
ml = 0
2pz orbital
ml =-1
2px orbital
l=0
n= 1
2s sublevel
ml =0
2s orbital
l=0
1s sublevel
ml =0
1s orbital
31. Quantum Numbers and Electronic Orbitals
ml =+2
3dx2 – y2orbital
Simulation Electronic Orbitals
Energy Level
ml =+1
3d sublevel
ml = 0
3dz2 orbital
ml =-1
l=2
3dyz orbital
3dxz orbital
Click here to view simulation
n= 3
ml =-2
3dxy orbital
ml =+1
3p sublevel
ml = 0
3pz orbital
ml =-1
l=1
3py orbital
3px orbital
Click here to view simulation
l=0
2p sublevel
n= 2
ml = 0
3s orbital
ml =+1
l=1
3s sublevel
2py orbital
ml = 0
2pz orbital
ml =-1
2px orbital
l=0
n= 1
2s sublevel
ml =0
2s orbital
l=0
1s sublevel
ml =0
1s orbital
Click here to view simulation
32. Concept Map
Quantum number
No TWO electron have same
4 quantum number
Quantum number = genetic code for electron
Electron has special number codes
33. Concept Map
No TWO electron have same
4 quantum number
Quantum number
Quantum number = genetic code for electron
What are these 4 numbers?
(1, 0, 0, +1/2) 0r (3, 1, 1, +1/2)
4 numbers
n
l
Size/distance
Shape
Number + letter
ml
Orientation
ms
Electron spin
Electron has special number codes
34. Concept Map
No TWO electron have same
4 quantum number
Quantum number
Quantum number = genetic code for electron
What are these 4 numbers?
(1, 0, 0, +1/2) 0r (3, 1, 1, +1/2)
4 numbers
n
l
Size/distance
Shape
ml
Orientation
Number + letter
1
Electron with quantum number given below
(n,l,ml,,ms) – (1, 0, 0, +1/2)
1s orbital
ms
Electron spin
Electron has special number codes
35. Concept Map
No TWO electron have same
4 quantum number
Quantum number
Quantum number = genetic code for electron
What are these 4 numbers?
(1, 0, 0, +1/2) 0r (3, 1, 1, +1/2)
4 numbers
n
l
Size/distance
Shape
ml
Orientation
Number + letter
1
Electron with quantum number given below
(n,l,ml,,ms) – (1, 0, 0, +1/2)
1s orbital
(n,l,ml,,ms) – (3, 1, 1, +1/2)
3py orbital
ms
Electron spin
Electron has special number codes
36. Concept Map
No TWO electron have same
4 quantum number
Quantum number
Quantum number = genetic code for electron
What are these 4 numbers?
(1, 0, 0, +1/2) 0r (3, 1, 1, +1/2)
4 numbers
n
l
Size/distance
Shape
ml
Orientation
ms
Electron has special number codes
Electron spin
Number + letter
1
Electron with quantum number given below
(n,l,ml,,ms) – (1, 0, 0, +1/2)
(n,l,ml,,ms) – (3, 1, 1, +1/2)
2
1s orbital
3py orbital
What values of l, ml, allow for n = 3? How many orbitals exists for n=3?
Video on Quantum numbers
For n=3 -> l = n -1 =2 -> ml = -l, 0, +l -> -2, -1, 0, +1, +2
• mℓ range from −ℓ to ℓ,
• ℓ = 0 -> mℓ = 0
–> s sublevel -> 1 orbital
• ℓ = 1 -> mℓ = -1, 0, +1
-> p sublevel -> 3 diff p orbitals
• ℓ = 2 -> mℓ = -2, -1, 0, +1, +2 -> d sublevel -> 5 diff d orbitals
• (2l+ 1 ) quantum number for each ℓ value
Answer = nine ml values – 9 orbitals/ total # orbitals = n 2
Click here video on quantum number
Click here video on quantum number
37. Acknowledgements
Thanks to source of pictures and video used in this presentation
Thanks to Creative Commons for excellent contribution on licenses
http://creativecommons.org/licenses/
Prepared by Lawrence Kok
Check out more video tutorials from my site and hope you enjoy this tutorial
http://lawrencekok.blogspot.com