The document discusses the quantum numbers that describe the electron states in an atom. It explains that each electron is labeled by four quantum numbers: principal (n), angular momentum (l), magnetic (ml), and spin (ms). The Pauli Exclusion Principle states that no two electrons can occupy the same quantum state, which explains the filling order of atomic shells in the periodic table.
Quantum Numbers
Wave nature of electrons
atomic structure
principle Quantum number
Azimuthal quantum number
magnetic quantum number
spic quantum number
shapes of orbitals
Quantum Numbers
Wave nature of electrons
atomic structure
principle Quantum number
Azimuthal quantum number
magnetic quantum number
spic quantum number
shapes of orbitals
This Presentation was prepared to help the readers to get the basic ideas for learning about the concepts of Quantum Numbers in Elementary Partcles ...
This presentation describes about the 4 Quantum Numbers.
This presentation will be helpful in determining the possible permitted values for Shells, Subshells, Electrons and the Shapes of Orbitals
This presentation is about the ionisation of energy of hydrogen, way to compute the value of ionisation energy of hydrogen, quantum numbers and a brief description of Schrodinger Equation.
This Presentation was prepared to help the readers to get the basic ideas for learning about the concepts of Quantum Numbers in Elementary Partcles ...
This presentation describes about the 4 Quantum Numbers.
This presentation will be helpful in determining the possible permitted values for Shells, Subshells, Electrons and the Shapes of Orbitals
This presentation is about the ionisation of energy of hydrogen, way to compute the value of ionisation energy of hydrogen, quantum numbers and a brief description of Schrodinger Equation.
The Aufbau Principle requires that the electrons occupy the lowest possible energy level before filling up the next.
Pauli’s Exclusion Principle posits that no two electrons can have the same set of four quantum number; the spin quantum number limits the number of electrons in an orbital to a maximum of two.
Hund’s Rule requires that the electrons fill the orbitals in a subshell one by one, before pairing the electrons in an orbital spin in opposite directions.
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https://sectrio.com/resources/ot-threat-landscape-reports/sectrio-releases-ot-ics-and-iot-security-threat-landscape-report-2024/
LF Energy Webinar: Electrical Grid Modelling and Simulation Through PowSyBl -...DanBrown980551
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The modern software delivery process (or the CI/CD process) includes many tools, distributed teams, open-source code, and cloud platforms. Constant focus on speed to release software to market, along with the traditional slow and manual security checks has caused gaps in continuous security as an important piece in the software supply chain. Today organizations feel more susceptible to external and internal cyber threats due to the vast attack surface in their applications supply chain and the lack of end-to-end governance and risk management.
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Bob Boule
Robert Boule is a technology enthusiast with PASSION for technology and making things work along with a knack for helping others understand how things work. He comes with around 20 years of solution engineering experience in application security, software continuous delivery, and SaaS platforms. He is known for his dynamic presentations in CI/CD and application security integrated in software delivery lifecycle.
Gopinath Rebala
Gopinath Rebala is the CTO of OpsMx, where he has overall responsibility for the machine learning and data processing architectures for Secure Software Delivery. Gopi also has a strong connection with our customers, leading design and architecture for strategic implementations. Gopi is a frequent speaker and well-known leader in continuous delivery and integrating security into software delivery.
2. From last lecture – Bohr model L n = nh /2 π Angular momentum is quantized Energy is quantized Radius is quantized n = 1, 2, 3 ... Linear momentum too Bohr model is incorrect!
3.
4. ACT: Quantum numbers For which state of hydrogen is the orbital angular momentum required to be zero? 1. n=1 2. n=2 3. n=3
5. Spectroscopic Nomenclature l =0 is “ s state ” l =1 is “ p state ” l =2 is “ d state ” l =3 is “ f state ” l =4 is “ g state ” 1 electron in ground state of Hydrogen: n=1, l =0 is denoted as: 1s 1 “ Subshells ” “ Shells ” n =1 is “ K shell ” n =2 is “ L shell ” n =3 is “ M shell ” n =4 is “ N shell ” n =5 is “ O shell ” Example n=1 l =0 1 electron
6. Electron orbitals In correct quantum mechanical description of atoms, positions of electrons not quantized, orbitals represent probabilities
7. Quantum Numbers How many unique electron states exist with n=2 ? l = 0 : m l = 0 : m s = ½ , -½ 2 states l = 1 : m l = +1: m s = ½ , -½ 2 states m l = 0: m s = ½ , -½ 2 states m l = -1: m s = ½ , -½ 2 states 2s 2 2p 6 There are a total of 8 states with n=2 Example
8. ACT: Quantum Numbers How many unique electron states exist with n=5 and m l = +3 ? A) 0 B) 4 C) 8 D) 16 E) 50
9. Preflight 25.2 What is the maximum number of electrons that can exist in the 5g (n=5, l =4) subshell of an atom?
10. Pauli Exclusion Principle In an atom with many electrons only one electron is allowed in each quantum state (n, l , m l , m s ). This explains the periodic table!
11. Electron Configurations Atom Configuration H 1s 1 He 1s 2 Li 1s 2 2s 1 Be 1s 2 2s 2 B 1s 2 2s 2 2p 1 Ne 1s 2 2s 2 2p 6 1s shell filled 2s shell filled 2p shell filled etc (n=1 shell filled - noble gas) (n=2 shell filled - noble gas) p shells hold up to 6 electrons s shells hold up to 2 electrons
12. The Periodic Table What determines the sequence? Pauli exclusion & energies s ( l =0) p ( l =1) d ( l =2) f ( l =3) n = 1, 2, 3, ... Also s
13. Shell Ordering Why do s shells fill first before p ? r 2p P(r) 2 s electrons can get closer to nucleus, which means less “shielding” from the 1s electrons r 2s P(r) 1s 1s
14. Sequence of Shells Sequence of shells: 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d ... 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, Pneumonic: ... 4s electrons get closer to nucleus than 3d
15.
16. Transition elements Recall torque on current loop from B-field: = I A B sin( ) I A = -ep/(2 rm) ( r 2 ) = -(e/2m)rp = -(e/2m)L T = 2 r/v = 2 r/v = 2 rm/p In 3d shell we are putting electrons into l = 2; all atoms in middle are strongly magnetic . Why? High angular momentum Strongly magnetic! Use Bohr model: Ze e – This looks like a current loop! I = -e/T A = r 2 r I Angular momentum!
17. Sodium Na 1s 2 2s 2 2p 6 3s 1 Many spectral lines of Na are outer electron making transitions www.WebElements.com Example Yellow line of Na flame test is 3p 3s Neon - like core Single outer electron
18.
Editor's Notes
Start by asking students to name seat (use row and number) make analogy with Quantum numbers. Why Lz? HUP tells us we can know one (and only one) component of L
Note it isn’t electron charge that keeps them from being in the same state!
