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2A. 13 Question

Posted: Sun Oct 27, 2019 10:35 pm
by Aashka Popat 1A
This question asks which orbital which type of orbital will need to be removed in order to form a +1 electron (For each of the following ground-state atoms, predict the type of orbital (1s, 2p, 3d, 4f, etc.) from which an electron will need to be removed to form the +1 ions: (a) Zn; (b) Cl; (c) Al; (d) Cu.)

I'm not sure how to approach this problem, would it be helpful to find the electron configuration first?

Re: 2A. 13 Question

Posted: Sun Oct 27, 2019 10:38 pm
by Anish Patel 4B
Writing the electron configuration first is a good way to go because you need to determine what sublevel each atom has valence electrons in. When you form a positive ion, you take away electrons from the valence level first.

Re: 2A. 13 Question

Posted: Sun Oct 27, 2019 10:58 pm
by Michelle Song 1I
Adding on to what the person above me said, it's also important to remember that transition metals in the d-block will lose electrons in the s-orbital first.

Re: 2A. 13 Question

Posted: Sun Oct 27, 2019 11:04 pm
by Eesha Sohail 1D
This goes slightly outside the scope of the question, but do all elements follow the same pattern of removal of electrons? Like, would removing an electron from Ag work the same way as one from Cu save for being at one higher energy level?

Re: 2A. 13 Question

Posted: Mon Oct 28, 2019 10:52 am
by Maya Beal Dis 1D
It helps me to think of which block on the periodic table the element sits in. If the element is in the third row of the p block, the valence electron will generally be removed from the 3p shell.

Re: 2A. 13 Question

Posted: Mon Oct 28, 2019 10:54 am
by Maya Beal Dis 1D
For part d of this problem, why would an electron be removed from the 4s subshell as opposed to the 3d subshell? Wouldn't it be more stable to remove and electron from the subshell that is already only partially filled as opposed to removing an electron from the filled 4s shell?