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 electron configuration of beryllium is written as [He] 2s2. This means that it has 2s2 electrons above the configuration of Helium.
VanadiumAtomic number: 23Symbol: VAtomic weight: 50.9415(1)Electron configuration: [Ar]3d34s2Group: 5BPeriod: 4
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 Rb+1 or Kr
Orbital notation shows how the electrons are arranged in the orbitals of the sublevels. Electron configuration shows only how many electrons are in each sublevel.
its because some are naturally stable like helium, when some like hydrogen have an extra electron in their electron clouds. That's why they are unstable. When they meet with an element with one extra electron they can be stable because the first electron cloud holds 2 electrons. ex. : hydrogen - 1 electron hydrogen - 1 electron adding both together will give you a full eletron cloud. Hope this helps!
Tin. {http://en.wikipedia.org/wiki/Tin}.
It could be either Sn2+ ion (stannous ion) or Sn4+ ion (stannic ion)
The electron configuration of tin(II) cation is [Kr]5s2.4d10.
Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration. Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration.
Na+ is the formula of the ion formed when sodium achieves a stable electron configuration.
The group of elements that have a stable electron configuration are the noble gases.
The electronic configuration of tin is: [Kr]D10.5s2.5p2.The electronic configuration of chromium(2+) is correct.
What symbol would represent a chlorine ion that has ionized to have a stable electron configuration?
They achieve stable configuration by sharing their electrons in their outermost shell.
Oxygen atoms need to share or gain two electrons in order to achieve a stable electron configuration.
The electron configuration of copper is: [Ar]4s13d10. It isn't 4s23d9 because Cu is able to obtain a more stable electron configuration when it takes an electron from the 4s and adds it to 3d. A half filled 4s and a completely filled 3d is more stable.
A stable electron configuration.