f.describe the shapes of electron density plots (or maps) for s and p orbitals
description
Transcript of f.describe the shapes of electron density plots (or maps) for s and p orbitals
![Page 1: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/1.jpg)
f. describe the shapes of electron density plots (or maps) for s and p orbitalsg. predict the electronic structure and configuration of atoms of the elements
from hydrogen to krypton inclusive using 1s …notation and electron-in-boxes notation (recall electrons populate orbits singly before pairing up)
3: Filling orbitals and shells
Connector – use the 1s2 … notation to:(a) Write the electronic configurations of the following atoms:
lithium, nitrogen and sulphur. (b)
i. Write the electronic configuration of the following ions: fluoride, lithium and oxide.
ii. What do you notice about the electronic configuration of ions?
iii. Suggest why this is so.
(c) Identify the following atoms:
![Page 2: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/2.jpg)
![Page 3: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/3.jpg)
Write the electronic configuration of the following ions:
Ions have the electronic configuration of the STABLE NOBLE GASES.
![Page 4: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/4.jpg)
Arrangement of Electrons in Arrangement of Electrons in AtomsAtoms
Arrangement of Electrons in Arrangement of Electrons in AtomsAtoms
Electrons in atoms are arranged asElectrons in atoms are arranged as
SHELLSHELL (n) (n)
SUBSHELLSSUBSHELLS
ORBITALSORBITALS
Each type of subshell (s,p,d,f) contains one or more orbitals.An Orbital represents the region in space where it is most likely to find an electron.
![Page 5: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/5.jpg)
Shells, subshells and orbitals
• ‘s’ subshell has 1 orbital, ‘p’ subshell has 3 orbitals, ‘d’ subshell has 5 orbitals, ‘f’ subshell has 7 orbitals.
• Copy and complete the following table:
- - - - - - - - - -
Each orbital can hold maximum of 2 electrons. What will be the maximum number of electrons in each subshell and shell?
![Page 6: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/6.jpg)
Energy level diagram
As the principal quantum number ‘n’ increases, the energy gap between successive shells decreases. As a result, neighbouring subshells overlap and have a different order of increasing energy in subshells.
![Page 7: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/7.jpg)
Shapes of Orbitals Orbitals have different shapes
is an area of zero probability of finding an electron
![Page 8: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/8.jpg)
Home Learning Research task
Use The Heisenberg Uncertainty Principle to explain the impossibility of drawing orbits for electrons.i.e.Why is this wrong?
But this is correct?
Due date: Next Lesson
![Page 9: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/9.jpg)
Shapes of p Orbitals
planar node
Typical p orbital
planar node
Typical p orbitalp sublevel has 3 orbitals p sublevel has 3 orbitals – – ppxx,p,pyy,p,pzz
There is a PLANAR NODE thru the nucleus, which is an area of zero probability of finding an electron
![Page 10: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/10.jpg)
Shapes of d Orbitalstypical d orbital
planar node
planar noded sublevel has 5 orbitalsd sublevel has 5 orbitals – – ddxyxy, d, dxzxz, d, dyzyz, d, dx - yx - y, d, dzz 2 2 2
![Page 11: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/11.jpg)
Filling the orbitals• An atom is in it’s lowest energy state (ground state)
when it’s electrons are in the orbitals with the lowest possible energy level.
• One of the factors influencing the filling of orbitals is Electron spin.
An electron can either have clockwise or anticlockwise spin.Two electrons in the same orbital MUST have opposite spin*. Represented by:
* Pauli exclusion principle
![Page 12: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/12.jpg)
Copy and complete the table by filling the correct number of orbitals with electrons.
Filling the orbitals
![Page 13: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/13.jpg)
Electrons will fill the lowest energy orbital first, then the remaining number of orbitals with increasing energy.
Hund's Rule - Electrons occupy all the orbitals of a given sublevel singly before pairing begins.
Spins of electrons in different incomplete orbitals are parallel in the ground state.
The most stable arrangement of electrons in the subshells is the one with half filled or completely filled orbitals.
Rules for filling the orbitals
![Page 14: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/14.jpg)
Complete the orbital diagram from H to Ne
•Hund's Rule - Electrons occupy all the orbitals of a given sublevel singly before pairing begins.
•Spins of electrons in different incomplete orbitals are parallel in the ground state.
![Page 15: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/15.jpg)
Complete the electronic configuration and orbital diagram from O to Ar.
1s 2s 2p
This is called Shorthand notation
Hund’s rule
![Page 16: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/16.jpg)
Complete the electronic configuration and orbital diagram from K to Cr.
![Page 17: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/17.jpg)
Complete the electronic configuration and orbital diagram from Mn to Kr.
![Page 18: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/18.jpg)
ELECTRON CONFIGURATIONS OF IONS
• For an ion, you simply add or subtract the right number of electrons from the outermost shell – taking electrons for a positive ion and adding electrons for a negative ion.
• For example, write the electronic configuration for V and then for V
• Write the electronic configuration for O and Ca
2+
2- 2+
![Page 19: f.describe the shapes of electron density plots (or maps) for s and p orbitals](https://reader035.fdocuments.in/reader035/viewer/2022062301/56815735550346895dc4d5d7/html5/thumbnails/19.jpg)
Try Some Ions! (Grade A/A*)
• Write the longhand notation for these:
F-
Li+
Mg+2
• Write the shorthand notation for these:
Br-
Ba+2
Al+3