For the spectroscopic notation:

2-8-18-5

1)What does the element do to make the outer shell complete?
2) What would be the charge on the ion the forms as a result?
3) What is the spectroscopic notation fpr each shell

Thanks!

1) In order to make the outer shell complete, the element will typically gain or lose electrons. In this case, the element with the spectroscopic notation 2-8-18-5 will most likely lose 5 electrons.

2) The charge on the ion that forms as a result of losing 5 electrons would be +5 (positive five). This is because the element started with 5 valence electrons and lost them to achieve a complete outer shell.

3) The spectroscopic notation for each shell in this case would be:

- Shell 1: 2 electrons (2)
- Shell 2: 8 electrons (2-8)
- Shell 3: 18 electrons (2-8-18)
- Shell 4: 5 electrons (2-8-18-5)

1) In the given spectroscopic notation 2-8-18-5, the element has a total of 33 electrons. To make its outer shell complete, the element will need to gain or lose electrons. Generally, elements tend to either lose electrons to achieve a stable outer shell with fewer electrons or gain electrons to achieve a stable outer shell with more electrons. By following the octet rule, which states that most elements strive to have 8 electrons in their outer shell, we can determine the element's behavior.

2) To determine the charge on the ion that forms as a result, we need to consider the element's position in the periodic table. In this case, since we don't know the specific element, we can't determine the exact charge. However, if the element is located in Group 1 (1 valence electron) or Group 2 (2 valence electrons), it tends to lose those electrons and form ions with charges of +1 or +2, respectively. On the other hand, if the element is located in Groups 15 (5 valence electrons) or 16 (6 valence electrons), it tends to gain 3 or 2 electrons, respectively, forming ions with charges of -3 or -2.

3) The spectroscopic notation for each shell represents the number of electrons in each electron shell or energy level. In the notation 2-8-18-5, the first shell (closest to the nucleus) has 2 electrons, the second shell has 8 electrons, the third shell has 18 electrons, and the outermost fourth shell has 5 electrons. The notation is based on the Aufbau principle, which states that electrons fill the lowest available energy levels first before moving to higher ones.

I don't consider 2-8-18-5 a spectroscopic notation.

In order:
1. It adds three electrons to make 3 in the last shell.

2. If it adds three electrons, each with a -1 charge, then there will be a charge of -3 on the ion.

3. Since I, obviously, don't know what you mean by spectroscopic notation you will need to figure this one out. I would write the orbital notation as
1s2 2s2 2p6 3s2 3p6 3d10 2s2 2p6 for the -3 ion (after the three electrons have been added).