section 5.3 quantum numbers and atomic orbitals quantum numbers are numbers that specify the...
TRANSCRIPT
![Page 1: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/1.jpg)
Section 5.3Quantum numbers and Atomic Orbitals
• Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that orbital
• It’s the electrons “address”
![Page 2: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/2.jpg)
Four Quantum Numbers
• Principal quantum number
• Orbital quantum number
• Magnetic quantum number
• Spin quantum number
![Page 3: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/3.jpg)
Principal quantum number
• Symbol, n
• Indicates the main energy levels
• To this point, only 1-7
• Where do we see 7 main energy levels in this room?
![Page 4: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/4.jpg)
Orbital quantum number
• Shape of an orbital
• Four shapes• s, p, d, and f
• Within each main energy level there are different shapes of orbitals
![Page 6: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/6.jpg)
Shapes of d orbitals
![Page 7: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/7.jpg)
Examples of f-shaped orbitals
![Page 8: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/8.jpg)
Magnetic quantum number
• Indicates the orientation (or position) of an orbital around the nucleus– s orbital has 1 orientation– p orbitals have 3 orientations– d orbitals have 5 orientations– f orbitals have 7 orientations
• Each orbital can contain only 0, 1, or 2 electrons.
![Page 9: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/9.jpg)
Spin quantum number
• Indicates the spin of the electron– +1/2 – -1/2– So if there are two electrons in one orbital,
they spin in opposite directions
• *** no two electrons can have the same 4 quantum numbers***
![Page 10: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/10.jpg)
Electron configurations(electron arrangements)
• Pauli Exclusion Principle– No two electrons in the same atom will have
the same set of 4 quantum numbers
![Page 11: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/11.jpg)
How to “read” orbitals• How we determine which orbital gets filled with electrons first?
• Must follow the ________________:
– Orbital of Lowest energy gets filled before going to the next lowest energy orbital
– In other words we fill from lowest energy to highest energy
– “building up” principle: electrons occupy the lowest-energy orbital that is available.
– For example, Hydrogen’s electron goes into the __ orbital, because it is the lowest energy orbital
![Page 12: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/12.jpg)
Electron configurations(electron arrangements)
• How do we know which orbitals are higher or lower in energy?
– Read Periodic Table from Left to Right, Top to Bottom
![Page 13: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/13.jpg)
Periodic Table Sections
![Page 14: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/14.jpg)
3 types of notation
• Orbital Notation
• Electron-Configuration Notation
• Electron Dot Notation
![Page 15: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/15.jpg)
Orbital Notation
• Unoccupied orbital __• Orbital with1 e- ↑ or ↓• Orbital with 2 e- ↓↑
• Example: Hydrogen Example: Lithium
• Example: Helium Example: Oxygen
![Page 16: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/16.jpg)
Electron configurations(electron arrangements)
• Hund’s rule– Orbitals of equal energy are each occupied by 1
electron before a 2nd electron is added.
– All electrons in singly occupied orbitals must have the same spin
– For example, there are 3 p orbitals. If you have 3 electrons, there will be one in each orbital and all will have spin quantum number of +1/2 or -1/2
– Example N:
![Page 17: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/17.jpg)
Electron-Configuration notation
• Similar to orbital notation, but uses superscripts instead of lines
• Example: Hydrogen
• Example: Helium
• Example: Lithium
![Page 18: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/18.jpg)
Electron-Dot Notation
• Uses only the Valence electrons• Valence electrons = the electrons in the highest
(outermost) main energy level
• H
• He
• K
![Page 19: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/19.jpg)
Practice Problems (orbital and dot notation)
Carbon
Sodium
Sulfur
![Page 20: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/20.jpg)
Shorthand Notation
• Use the last noble gas before your element as a “building block”
• Example: Phosphorous
![Page 21: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/21.jpg)
Practice Problems (d and f orbitals)
Fe
Au
![Page 22: Section 5.3 Quantum numbers and Atomic Orbitals Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that](https://reader036.vdocuments.us/reader036/viewer/2022062308/56649ee65503460f94bf64fe/html5/thumbnails/22.jpg)
Trick to Electron Dot Notation
• Use the group number that the element is in
• Hydrogen is in group 1, 1 valence electron• Oxygen is in group 6, 6 valence electrons• These 8 groups are sometimes called the 8
“main groups”