Chapter 3 Homework #13

Moderators: Chem_Mod, Chem_Admin

Dan_Jin_1K
Posts: 15
Joined: Wed Sep 21, 2016 2:59 pm

Chapter 3 Homework #13

Postby Dan_Jin_1K » Mon Oct 24, 2016 8:47 pm

Hi everyone!

Could someone explain to me how to find the answers for this question?

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.

Thank you!

Logan 3C
Posts: 22
Joined: Wed Sep 21, 2016 2:57 pm

Re: Chapter 3 Homework #13

Postby Logan 3C » Mon Oct 24, 2016 9:16 pm

Its asking you to determine what orbital the highest energy valence electron is in. For example, to make Zn an ion, you would need to remove an electron from its 3d orbital to give it a +1 charge.

Navarro_Bree_1D
Posts: 24
Joined: Wed Sep 21, 2016 3:00 pm

Re: Chapter 3 Homework #13

Postby Navarro_Bree_1D » Wed Oct 26, 2016 10:17 am

In addition, you must remove an electron from the orbital with the highest energy level because these electrons are the easiest to remove compared to the electrons from orbitals with lower energy levels.

The electron configuration of Cl is [Ne]3s^2 3p^5.
--The highest energy level is 3p.
--Therefore, you remove an electron from the 3p orbital.

Note: You do NOT remove an electron from the 3s orbital because the ionization energy would be significantly greater at the 3s orbital than the 3p orbital.


Return to “Ionic & Covalent Bonds”

Who is online

Users browsing this forum: No registered users and 1 guest