Valence electrons are electrons that are on the outside "shell."
In Group (column) 1, there is only one valence electrons for each element. In Group (column) 2, there are two valence electrons.
Group 13: 3 valence electrons
Group 14: 4 valence electrons
Group 15: 5 valence electrons
Group 16: 6 valence electrons
Group 17: 7 valence electrons
Group 18: 8 valence electrons
There is no Group 19, so this list is done. For the metals, each element will need to be mapped out utilizing the Bohr Diagram design or something of the like as valence electrons are difficult to define due to the grouping on the Periodic Table.
The most valence electrons that can be in an outer shell is eight.
Barium (Ba) is in Group (column) 2, and thus has only two valence electrons.
Barium contains two valence electrons
56 ELECTRONS
Barium has two valence electrons.
6
There are 2 valence electrons in Barium.
This element is xenon.
Any neutral atom of barium contains 56 electrons, the counter charge for the 56 protons contained in the nucleus of a barium atom, as indicated by its atomic number, 56.
Neither..they both have approximately the same weight as electrons are virtually weightless.bt the ba2 plus wud have to combine with another element for charge stability and the compound it forms shud be heavier than ba.
2
6
Barium 137 has 56 protons and 56 electrons.
there are 54 electrons in Ba 2+. as the atomic no. of Ba is 56, so when it loses two of its electrons.. there are 54 electron left..
Examples: Ca, Mg, Ba, Sr, Ra, etc.
There are 2 valence electrons in Barium.
gain 2
Ba2+ is the ion of the Ba atom. That means it has given away two electrons to other atoms in order to reach a stable state with 8 electrons in its outer shell.
To attain the noble gas configuration, Ca would have to lose 2 electrons, Mg would have to lose 2 electrons, Ba would have to lose 2 electrons, and Be would have to lose 2 electrons.
Ba
This element is xenon.
Barium has two valence electrons, as can be deduced from its placement in Group 2 of the modern periodic table.