Write the full electron configuration for the ground state of each of the following:
a. Ni
b. Ni2+
I'm not exactly sure what to do here, please help!
28Ni = 1s2 2s2 2p6 3s2 3p6 3d8 4s2.
Now you do the Ni++.
To determine the electron configuration of an atom or ion, we need to follow a specific order or filling sequence of the orbitals in the atom. The ordering of the orbitals is based on the Aufbau principle, which states that electrons fill the lowest energy orbitals first before occupying higher energy orbitals.
The electron configuration is usually written in a shorthand notation using the following format: 1s^2 2s^2 2p^6...
Now let's determine the electron configuration for each case:
a. Ni (nickel):
To find the electron configuration for nickel, we need to locate it on the periodic table. Nickel is located in the 4th period and belongs to the d-block elements.
The electron configuration can be obtained by filling the orbitals following the order of increasing energy levels and using the respective subshell notation. The order of the subshells is as follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, ...
The full electron configuration for nickel (Ni) is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^8.
b. Ni2+ (Nickel ion with a +2 charge):
When an atom forms a cation (positive ion), it loses one or more electrons from its neutral state. In the case of Ni2+, two electrons are lost from nickel.
To determine the electron configuration of Ni2+, start with the electron configuration of neutral Ni, and then remove two electrons from the highest energy level (4s):
Full electron configuration of Ni: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^8
Remove two electrons from 4s^2: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^8
Therefore, the electron configuration for Ni2+ is: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^8.
Remember that cations are formed by the loss of electrons, so the electron configuration for the ion will have fewer electrons compared to the neutral atom.
I hope this explanation helps! Let me know if you have any further questions.