[Xe]
Normally the electronic configuration for Barium would be [Xe] 6s2, but since you want it for Ba2+, you're missing two electrons. You get rid of the 6s2 and get [Xe].
"Shantell12: Light up the Darkness with barium my favorite element B''
The electronegativity of barium is less than that of strontium.
Because Strontium and Barium provide brilliant red and orange colors.
No. Barium and magnesium and calcium are in group 2A but potassium is in group 1A.
It is usually a barium or iodine dye
Barium is divalent; the ion is Ba2+.
None. Barium is in group 2. the electronic configuration is [Xe] 6s2.
Barium forms a divalent cation and no anions.
Yes, barium is divalent with two electrons in the outer shell.
2
Two electrons are donated by Barium to an oxidant (nonmetal, eg. O2) by which barium gets oxidised.Ba --> Ba2+ + 2e-This is because Ba is in group 2 of the periodic system, belonging to the 'earth alkali' metals and so it has 2 electrons (2e-) in its valency (or outer) shell (2,8,18,18,8,2). Hence Ba2+ configuration is (2,8,18,18,8,-), with an empty (-) 6th shell (the 'P' shell) like Xenon.
Ba(NO3)2. Barium forms divalent cations, and the nitrate polyatomic anion has only one negative charge.
There is no noble gas with the same electronic configuration as the element barium (Ba). But Ba2+ ion and the noble gas xenon (Xe) will have the same number of electrons (54 electrons each).
2 electrons as barium has 56 electrons so it will lose two electrons to reach the electronic structure of the nearest noble gas which is xenon 54 electrons
[Kr]4d105s25p6
Cesium(I), Cs+1 is an iso-electronic ion to Ba2+ and also iodine, I-1 ions and xenon, Xe0 atoms are iso-electronic to Ba2+ ions.They all have the [Xe] electron configuration: [2, 8, 18, 18, 8], 0
barium chloride