Carbon has an atomic number of 6, but the following orbital notation for carbon is incorrect. Explain the error in terms of the rules for electron arrangements.
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how does hunds rule help me find the answer? I don't understand the arrows and boxes thing.
well the electrons repel each other( due to charge) so the the outer shell , will have one electron in each box
According to Hund's rule.. the electron in 2px orbital can't be paired up until 2py and 2pz orbitals get filled up ! :)
Each S can hold two electrons total and a #S subshells has one orbital.
Each P can hold six electrons total and a #P subshell has three orbitals.
Each D can hold ten electrons total and a #D subshell has five orbitals.
Each F can hold fourteen electrons total and a #F subshell has seven orbitals.
Each orbital " in your example the squares represent your orbitals for that # subshell (S, P, etc.) & can hold two electrons (represented by the arrows) BUT....
Hund's rule says: every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied.
When they say in Hund's rule singly that means you have to fill each subshells orbital with UP ARROWS FIRST and if you have anymore left you need to represent then you come back in and fill the downward pointing arrows till you reach the total you need.
up then down up then down up only up only
_____ _______ ______ _______ ______
1S 2S 3P
2 e's + 2 e's + 2e's = 6 e's = carbon|dw:1348311532379:dw|