Tin.
{http://en.wikipedia.org/wiki/Tin}.
Each element has a specific electron configuration.
The electronic configuration of tin is: [Kr]D10.5s2.5p2.The electronic configuration of chromium(2+) is correct.
5s25p2 The 2's are exponents on the s and the p
Shouldn't you do the homework yourself. Teach your teacher!
The noble gas configuration for tin (Sn) is [Kr] 5s^2 4d^10 5p^2, where [Kr] represents the electron configuration of krypton.
In the electron configuration of tin (Sn), the 3d electrons are not present. Tin has a configuration of [Kr] 5s2 4d10 5p2, which means it has 2 electrons in the 5s orbital, 10 electrons in the 4d orbital, and 2 electrons in the 5p orbital.
Tin has 4 valence electrons. Because of this, Tin needs to lose the 4 electrons to make it stable. Thus the answer is SN4+
The element with this electron configuration is tin (Sn), which has an atomic number of 50. The electron configuration provided corresponds to the electron distribution in its various electron orbitals.
Mg
Tin typically has a configuration of [Kr] 5s^2 4d^10 5p^2 when it is a neutral atom. If tin forms an ion by losing two electrons, it would have a configuration of [Kr] 5s^2 4d^10, as it would lose its two outermost electrons from the 5p orbital.
The electron configuration that ends with np² corresponds to elements in Group 14 of the periodic table. This configuration is typically seen in elements like silicon (Si) and tin (Sn), which have the electron configurations ending in 3p² and 5p², respectively. In general, the full electron configuration for these elements includes all preceding orbitals filled according to the Aufbau principle.
It could be either Sn2+ ion (stannous ion) or Sn4+ ion (stannic ion)