What is the period 3 element whose 2+ ion is isoelectronic with neon?
How can I find the solution?
Thanks
It's tough to explain without a board but look at Mg. Period 3 has Ar as the "end" element. So if you want it to be isoelectronic with Ne, the element must be in period 3 but lose electrons which makes it Na, Mg, Al etc. Mg is the only one of those that forms a 2+ ion to make it isoelectronic with Ne. .
Ah, period 3 and isoelectronic with neon? Well, that's quite a zesty question! So, let's put on our detective hats and search for the solution, shall we?
In period 3, we have elements from sodium (Na) to argon (Ar), and we're on the hunt for an element with a 2+ ion that has the same number of electrons as neon (Ne).
Now, remember that ions gain or lose electrons to achieve a stable electron configuration, which is the goal here. Neon (Ne) has 10 electrons, so we need to find an element with 12 electrons after losing 2.
If you take a gander at the periodic table, you'll soon stumble upon magnesium (Mg) as the element you seek! When it loses 2 electrons, it happily becomes Mg2+, having the same electron configuration as neon (Ne).
So, there you have it! The element you're looking for is none other than our comedic friend magnesium (Mg). I hope you enjoyed the hunt and, most importantly, the laughter along the way!
To find the period 3 element whose 2+ ion is isoelectronic with neon, you can follow these steps:
1. Determine the electron configuration of neon (Z = 10). Neon's electron configuration is 1s^2 2s^2 2p^6.
2. Remove 2 electrons from the outermost shell (valence electrons) of neon. Since neon has a full outer shell, it loses its valence electrons in the 2p orbital.
3. Now, you need to find a period 3 element whose 2+ ion has the same electron configuration as neon's. The period 3 elements include sodium (Na), magnesium (Mg), aluminum (Al), silicon (Si), phosphorus (P), sulfur (S), chlorine (Cl), and argon (Ar).
4. Let's check the electron configurations of the period 3 elements and see which one matches neon's 2+ ion.
- Sodium (Na) loses one electron from the 3s orbital, resulting in 1s^2 2s^2 2p^6. It is not isoelectronic with neon.
- Magnesium (Mg) loses two electrons from the 3s orbital, resulting in 1s^2 2s^2 2p^6. It is not isoelectronic with neon.
- Aluminum (Al) loses three electrons from the 3s and 3p orbitals, resulting in 1s^2 2s^2 2p^6. It is not isoelectronic with neon.
- Silicon (Si) loses four electrons from the 3s and 3p orbitals, resulting in 1s^2 2s^2 2p^6. It is not isoelectronic with neon.
- Phosphorus (P) loses five electrons from the 3s and 3p orbitals, resulting in 1s^2 2s^2 2p^6. It is not isoelectronic with neon.
- Sulfur (S) loses six electrons from the 3s and 3p orbitals, resulting in 1s^2 2s^2 2p^6. It is not isoelectronic with neon.
- Chlorine (Cl) loses seven electrons from the 3s and 3p orbitals, resulting in 1s^2 2s^2 2p^6. It is not isoelectronic with neon.
- Argon (Ar) loses eight electrons from the 3s, 3p, and 3d orbitals, resulting in 1s^2 2s^2 2p^6. It is isoelectronic with neon's 2+ ion.
Therefore, the period 3 element whose 2+ ion is isoelectronic with neon is Argon (Ar).
I hope this helps! Let me know if you have any further questions.
To find the answer to this question, we need to understand the concept of isoelectronicity. Isoelectronic species are atoms, ions, or molecules that have the same number of electrons. In this case, we're looking for an element from period 3 whose 2+ ion has the same number of electrons as neon.
To get started, let's first determine the electronic configuration of neon. Neon is located in period 2 of the periodic table, which means it has two electron shells. Its electronic configuration is 1s²2s²2p⁶, where the superscripts represent the number of electrons in each atomic orbital.
Now, we need to find an element from period 3, which means it will have three electron shells. Since we're looking for the 2+ ion of this element, it means we need to remove two electrons from its neutral state. This will correspond to removing the two valence electrons from the outermost shell.
To find out which element fills these criteria, we can look at the periodic table to identify the elements in period 3. These include sodium (Na), magnesium (Mg), aluminium (Al), silicon (Si), phosphorus (P), sulfur (S), chlorine (Cl), and argon (Ar).
Next, we can determine the electronic configurations of the 2+ ions of each of these elements by removing the two valence electrons. Once we have these configurations, we can compare them to the electronic configuration of neon.
When we go through this process, we find that the electronic configuration of the 2+ ion of sulfur (S^2+) is 1s²2s²2p⁶. This is the same as the electronic configuration of neon (Ne).
Therefore, sulfur (S) is the element from period 3 whose 2+ ion is isoelectronic with neon.