Light, as a photon, as the ability to energize an electron bringing them to the Excited level/state. However, staying excited is temporary, and as
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1 Light, as a photon, as the ability to energize an electron bringing them to the Excited level/state. However, staying excited is temporary, and as the electron returns to the ground state, it emits a specific wave of light.!
2 Niels Bohr later described the type of light that the electron was giving off as something proportional to the different energy levels an electron can take form as. This describes the behaviour of Bohr s Hydrogen model.!! EXCITED! STATE!!! H! E! GROUND! STATE!!
3 What is certainty?!
4 The point of Neils Bohr s Model was to show that there are only allowed places where electrons can be energy levels!! EXCITED! STATE!!! H! E! GROUND! STATE!!
5 de Broglie proposed that if light, which is a wave, can energize/interact with electrons, do electrons also have wave properties? This lead to the conclusion of Matter Waves - that all things behave like a wave.!
6 For electrons which can only be found in the energy levels, de Broglie proposed that their movement as a waves are being done at the specific energy levels stated by Bohr.!
7 There is no 1 proponent/scientist who takes claim on the Electron cloud model. There will be several more but today, we ll only discuss 2.! Karl Heisenberg! Erwin Schrödinger!
8 Heisenberg believed that for small things that travel very fast, it is impossible to know 1) where something is & 2) how fast it s going at the SAME TIME.!
9 Schrödinger proposed that an electron can only be in probable spaces at a certain time. However, as the electron is energized, it is able to move from one level to the other.!
10
11 Bohr = Electrons can only be found in energy levels! de Broglie = Electrons move in form of waves! Heisenberg = Fast and small moving things like electrons are impossible to exactly find or know where it s going! Schrödinger = Even if you can t find where it is specifically, you can find where it PROBABLY is!
12 With Schrödinger s description of where in the cloud the electron can be located, gives the basis why we call this the ELECTRON CLOUD MODEL!
13 As mathematical equations are used to show shapes on an axis!
14 In the ELECTRON CLOUD MODEL, you can use Schrödinger s equation to show different shapes of cloud - sub-levels/orbitals!
15 Orbitals v.s. Orbits: Bohr s model focuses on electrons traveling circular paths around the nucleus. An orbital is the approximation/estimated area of space an electron can most likely be found.! Orbits! Orbitals!
16 Each shape is a sub-level/orbital and has: (A) a configuration on the 3D axis, and (B) Its own set of configurations which correspond to shells (each shell capable of housing 2 electrons)! S! P! D! F!
17 In the ELECTRON CLOUD MODEL, you can use Schrödinger s equation to show different shapes of cloud - sub-levels/orbitals! - THE S SUB LEVEL! Has only 1 shell! Houses at most 2 electrons!
18 In the ELECTRON CLOUD MODEL, you can use Schrödinger s equation to show different shapes of cloud - sub-levels/orbitals! - THE P SUB LEVEL! - Has 3 shells! - Houses at most 6 electrons!
19 In the ELECTRON CLOUD MODEL, you can use Schrödinger s equation to show different shapes of cloud - sub-levels/orbitals! - THE D SUB LEVEL! - Has 5 shells! - Houses 10 electrons!
20 In the ELECTRON CLOUD MODEL, you can use Schrödinger s equation to show different shapes of cloud - sub-levels/orbitals! - THE F SUB Level! - Has 7 shells! - Houses at most 14 electrons!
21 In the ELECTRON CLOUD MODEL, you can use Schrödinger s equation to show different shapes of cloud we call them sub-levels or orbitals! Each shape is a sub-level/orbital and has: (A) a configuration on the 3D axis, and (B) Its own set of configurations which correspond to shells (each shell capable of housing 2 electrons)! - THE S ORBITAL! - Has only 1 shell! - Houses at most 2 electrons! - THE D ORBITAL! - Has 5 shells! - Houses 10 electrons! - THE P ORBITAL! - Has 3 shells! - Houses at most 6 electrons! - THE F ORBITAL! - Has 7 shells! - Houses 14 electrons!
22 After discussing what the different orbitals are, it s now a matter of placing electrons where they are supposed to be located. This is the business done during electron configuration.!
23 The Electron Configuration is a way of organizing electrons based on their energy from lowest to highest. This follows the principle of Bohr that electrons can only be found on energy levels.!
24 As each energy level has sub-levels/orbitals, we label each specific orbital as the ENERGY LEVEL and the ORBITAL.! 1! s! 2! s! 2! p! 3! s! 3! p! 3! d! 4! s! 4! p! 4! d! 4! f!
25 Now that we ve labelled each energy level with their corresponding orbitals, there is a way that them in increasing energy.!
26 For particles in general, especially those with a lot of electrons, their electrons fill orbital with the lowest energy orbital to the highest. This is commonly known as the filling order. This follows the Aufbau principle.!
27 Like filling a empty barrel, the Aufbau principle, (German: to build up ) follows that the bottom levels get filled up first before you move to the higher levels! {! 1s! 2s! 2p! 3s! electrons!
28 To memorize the arrangement of the orbitals from lowest energy to highest energy, the following images are used for mnemonics.!
29 To memorize the arrangement of the orbitals from lowest energy to highest energy, the following images are used for mnemonics.!
30 To designate the number of electrons found in each orbital, we place the number of electrons it has on the upper right hand side of the orbital. An orbital can have electrons fewer than its capacity.! 1s! 2! 6! 10! 2p! 3d! 4f! 14! 3! 1! 3p! 4s!
31 It s important to remember when filling up the orbitals with electrons that: Each orbital has a specific number of shells and each shell can only contain 2 electrons. Thus, an orbital can t have more than its capacity.! X! 1s! 4! X! 2p! 8! X! 5f! X! 3d! 11! 20!
32 So for particles with a lot of electrons, we can list their orbitals and their corresponding number of electrons depending on all of the electrons they have.! # Electrons" Electron Configuration" 9" 17" 35" 53"
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