I forget how to determine the charge of an element based on its electron configurationI know it has to do with how electrons fill outer orbitals, but I have seen too many conflicting 'methods' and now i am confusedFor example, what is the predicted charge on a molecule that has the electron configuration of (1s2)(2s2)(2p6)(3s2) The answer key say +2, but I don't see itHow would you figure it out if you were given the electron configuration for aluminum or fluoride?Thanks
YOU GO GIRL/MAN!:) solar power lighting?! a tatttoo of GO GREEN on you !3 peace love greeen
Bike whenever you can instead of drivingThat makes a big differenceAlso, carpooling is a good idea.
The highest energy sub-level is the 3s where there are two electronsWhen a metal ionizes then the electrons are lost from the highest sub-level(s), hence the +2 chargeAluminum has three electrons in the highest energy level (n3) - [Ne] 3s2 3p1 - so it will have a charge of +3Fluorine is a halogen, and forms a negatively charged ionIt has the configuration 1s2, 2s2 2p5It can gain one electron to have a filled p-sublevel and a -1 charge.
YOU GO GIRL/MAN!:) solar power lighting?! a tatttoo of GO GREEN on you !3 peace love greeen
Bike whenever you can instead of drivingThat makes a big differenceAlso, carpooling is a good idea.
The highest energy sub-level is the 3s where there are two electronsWhen a metal ionizes then the electrons are lost from the highest sub-level(s), hence the +2 chargeAluminum has three electrons in the highest energy level (n3) - [Ne] 3s2 3p1 - so it will have a charge of +3Fluorine is a halogen, and forms a negatively charged ionIt has the configuration 1s2, 2s2 2p5It can gain one electron to have a filled p-sublevel and a -1 charge.
