Orbital Diagrams and Electron Configuration Notations

In summary, the conversation discusses the electron configuration notation and the significance of the principal quantum number, angular momentum quantum number, and the number of electrons on the orbital. The shorthand notation [Xe] is explained as well as the exceptions to the normal behavior of shell filling with electrons. The conversation also mentions a helpful website and a thread on the stability of electron orbitals for further understanding.
  • #1
Mk
2,043
4
I used to understand this -- a few years ago -- but it has completely slipped my mind. What is going on with al this 1s2 and Like Cs[Xe]6s1?

Thanks a lot,
Mk
 
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  • #2
Principal quantum number, angular momentum quantum number and the number of electrons on the orbital specified by n and l. [Xe]6s1 means that you have the closed shell structure of Xenon and one electron in the n=6, l=0 state or in other words Cesium.
 
  • #3
It is all a way of categorizing where the electrons are around the atom, putting them into "Shells", "SubShells", and "Orbitals".

http://en.wikipedia.org/wiki/Electron_configuration

Every electron around an atom has 4 quantum numbers, n (the principle quantum number), l (for angular momentum), m sub l (for its atomic orbital), and m sub s (the spin, either + or - 1/2).
No two electrons can have the exact same 4 quantium numbers.

The [Xe] is a shorthand notation, meaning that the electron configuration is the same as Xenon's up to that point, and then it contunues with a 6s1, to make it have an electron configuration of Cessium
 
  • #4
Thank you very much for the replies, how can you write the electron configuration notation using only a periodic table?
 
  • #5
This site has a nice visual for this.

http://www.matter-antimatter.com/electronic_configurations.htm
 
Last edited by a moderator:
  • #6
Mk said:
Thank you very much for the replies, how can you write the electron configuration notation using only a periodic table?

Usually you don't. Not entirely correctly, that is. There are some exceptions from the "normal" behavior of shell filling with electrons. Vanadium, copper, zinc, silver, paladium, hydrargirum...and a lot among the lantanoids & actinoids.

Daniel.
 
  • #7
If you want an explanation for what dexitroby( Sorry for misspelling) said I started a thread about the stability of electron orbitals, in atoms, moloceuls, and solids. Towards the end Gukul( Sorry potential misspelling) explained why transition metals fill up differently. The thread is towards the bottom and titled 'Stability of a full valence shell' or something like that. Hopefully this will help a little bit. I am sorry that I was too stupid to know how to create a link.
-Scott
 

Related to Orbital Diagrams and Electron Configuration Notations

What is an orbital diagram?

An orbital diagram is a visual representation of the arrangement of electrons within an atom's orbitals. Each orbital is represented by a box and the electrons are shown as arrows, with their spin indicated.

How do you write electron configuration notations?

Electron configuration notation is written by listing the energy level and sublevel, followed by the number of electrons in that sublevel. For example, the electron configuration for carbon is 1s2 2s2 2p2, indicating that there are 2 electrons in the 1s sublevel, 2 electrons in the 2s sublevel, and 2 electrons in the 2p sublevel.

What is the difference between orbital diagrams and electron configuration notations?

The main difference between orbital diagrams and electron configuration notations is the way they represent the arrangement of electrons. Orbital diagrams show the orientation of the electrons in terms of their spin, while electron configuration notations simply list the number of electrons in each sublevel.

How do you determine the electron configuration of an element?

The electron configuration of an element can be determined by using the Aufbau principle, which states that electrons fill orbitals in order of increasing energy. The Pauli exclusion principle and Hund's rule can also be used to determine the specific arrangement of electrons within an element's orbitals.

How do you use orbital diagrams and electron configuration notations to predict chemical properties?

The arrangement of electrons in an atom's orbitals determines its chemical properties. By looking at the number of electrons in each energy level and sublevel, as well as the number of unpaired electrons, chemists can predict an element's reactivity, bonding behavior, and other chemical properties.

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