Qualification > Sciences
IGCSE CHEMISTRY DOUBTS HERE !!!!
elemis:
I have no idea of the answers to Question 3. I've just started my AS Level. SO forgive me :P
Question 6
a) http://www.periodictable.com/Elements/028/data.html Click on the elements at the top of the page to view the Electronic Config.
b) I dont understand what they are ak
elemis:
QUestion 5
elemis:
4 a) The amount of energy needed to remove an electron from one mole of an atom of a gaseous element.
Ivo:
--- Quote from: Ari Ben Canaan on October 05, 2010, 04:09:09 pm ---I have no idea of the answers to Question 3. I've just started my AS Level. SO forgive me :P
Question 6
a) http://www.periodictable.com/Elements/028/data.html Click on the elements at the top of the page to view the Electronic Config.
b) I dont understand what they are ak
--- End quote ---
For Question 6) b):
i) The 4s orbital will fill before a 3d orbital, because the 4s orbital is at a lower energy level than a 3d orbital. The order of filling orbitals based on their energy level is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, ...
ii) It is strange that the 4s orbital has not been completely filled up before moving on to the 3d orbital (which incidently is full - filled with 10 electrons). This is because copper is one of the exceptions to Hund's rule, where one of the 4s electrons moves into the last 3d orbital. This is known to be because there is more stability if it is arranged in this way - a full 3d subshell.
iii) Chromium is the other exception, arranged in a similar way - with having a half full 3d subshell, which appear to be associated with greater stability.
Deadly_king:
--- Quote from: Ivo on October 10, 2010, 10:49:56 am ---For Question 6) b):
i) The 4s orbital will fill before a 3d orbital, because the 4s orbital is at a lower energy level than a 3d orbital. The order of filling orbitals based on their energy level is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, ...
ii) It is strange that the 4s orbital has not been completely filled up before moving on to the 3d orbital (which incidently is full - filled with 10 electrons). This is because copper is one of the exceptions to Hund's rule, where one of the 4s electrons moves into the last 3d orbital. This is known to be because there is more stability if it is arranged in this way - a full 3d subshell.
iii) Chromium is the other exception, arranged in a similar way - with having a half full 3d subshell, which appear to be associated with greater stability.
--- End quote ---
Hehe......this whole paper was already answered in another thread. ;)
Anyway thanks for the help :)
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