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What ion of barium is most stable? Chemistry Matter Elements. 1 Answer anor277 Jan 7, 2017 ...
In this redox reaction, barium starts as a neutral solid but becomes an aqueous ion with a #2^+# charge. Hydrogen begins as an aqueous ion with a #1+# charge and becomes a neutral gas. Thus, two hydrogen atoms steal a total of two electrons from one barium atom, resulting in the formation of neutral hydrogen gas and a barium ion with a #2 ...
The formula for the barium ion is "Ba"^(2+)". Fluorine is a group 17 element. Group 17 elements form anions with a 1^- charge. The formula for the fluoride ion is "F"^(-)". Ionic compounds are neutral, so the charges of the positive and negative ions must equal zero when added. So for every "Ba"^(2+)" ion, two "F"^(-)" ions are needed.
The salt derives barium ion, Ba^(2+), and phosphate ion, PO_4^(3-). A neutral salt is formed from the formulation Ba_3(PO_4)_2. Most of the time, we probably deal with the bisphosphate, BaHPO_4.
The Barium ion in this molecule would have +2 charge. Barium is in the 6th energy level of the periodic table in the second column, with an electron configuration of Ba = [Xe] 6s^2 Barium would lose two electrons to follow the Rule of Octet and become Ba^+2 = [Kr] 5s^2 4d^10 5p^6 The Barium ion is Ba^+2 The Chloride ion is Cl^-1 It takes two -1 Chloride ions to balance the one +2 Barium ions ...
The dose of barium ion must be about 200 mg/(kg·day) to see adverse effects. For a 50 kg individual, this corresponds to 10 g/day of barium. Barium sulfate is highly insoluble in water.
Barium atoms are able to form ions, which is known as the barium ion. Specifically, a barium ion is formed when the barium atom gives up its two valence (or outermost) electrons. The resulting ion ...
Barium is an "alkaline-earth metal".....i.e. "Group 2". And thus barium commonly forms a Ba^(2+) ion, just as the halogen bromine, commonly forms a Br^-. And hence the salt formed is BaBr_2.
Barium oxide is an ionic compound, compromised of a barium metal cation, and an oxygen non-metal anion. Looking at the periodic table, oxygen is in group #6# or #16#, and will therefore have an oxidation number of #-2#, while barium sits in group #2#, and will have an oxidation number of #+2#.
The bromate ion is BrO_3^-. The alkaline earth barium commonly forms a Ba^(2+) ion. And thus the formula for barium bromate is Ba(BrO_3)_2. All I have done is cross multiply the charges so I get a neutral salt.