1s2 2x2 2p6 3s2 3p6 is the electron configuration ofr for which ion?
I believe your 2x2 should be 2s2. You have 18 electrons in filled orbitals. That could be a +1 charged element 19 (K+) or a +2 charged element 20 (Ca++) \, for example. In either case, it is a very stable ion because of the filed orbitals.
The electron configuration 1s2 2s2 2p6 3s2 3p6 corresponds to the ion with 18 electrons. Since the configuration indicates that all orbitals up to and including the 3p orbitals are filled, this ion has a completely filled valence shell.
Based on the number of electrons, this ion could be the potassium ion (K+) or the calcium ion (Ca2+). Potassium (atomic number 19) has 19 electrons, so removing one electron would result in a +1 charged ion. Calcium (atomic number 20) has 20 electrons, so removing two electrons would result in a +2 charged ion.
Therefore, the electron configuration 1s2 2s2 2p6 3s2 3p6 corresponds to either the potassium ion (K+) with a +1 charge or the calcium ion (Ca2+) with a +2 charge. Both ions are highly stable due to their filled valence shells.
To determine the ion for which the given electron configuration belongs to, we need to analyze the number of electrons in the orbitals. Let's break down the electron configuration:
1s2 2s2 2p6 3s2 3p6
The superscript numbers indicate the number of electrons in each orbital.
In the first shell (1s), there are 2 electrons (1s2).
In the second shell, the 2s orbital has 2 electrons (2s2), and the 2p orbital has 6 electrons (2p6).
In the third shell, the 3s orbital has 2 electrons (3s2), and the 3p orbital has 6 electrons (3p6).
By summing up the number of electrons in each shell, we find that there are a total of 18 electrons in filled orbitals.
Based on this, we can consider two possibilities:
1. If the element has an atomic number of 19, it would have one valence electron. By losing this electron, it would become a +1 charged ion (K+).
2. If the element has an atomic number of 20, it would have two valence electrons. By losing these electrons, it would become a +2 charged ion (Ca++).
Both potassium (K) and calcium (Ca) have 18 electrons in filled orbitals, making them very stable ions. Either of these ions, K+ or Ca++, could have the given electron configuration.
However, I noticed a mistake in the information you provided. The 2x2 should actually be 2s2 (2 electrons in the 2s orbital), not 2x2. Please double-check the electron configuration to ensure accurate analysis.