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The chemical formula for barium peroxide is BaO2.
Barium peroxide has a total of 14 valence electrons: 2 from the barium atom and 6 from each oxygen atom.
To determine the Lewis structure of barium peroxide, start by drawing the skeletal structure with the barium atom in the center and the oxygen atoms surrounding it. Then, distribute the valence electrons around the atoms, making sure each atom has a full outer shell. Remember to follow the octet rule, with the exception of the central barium atom which can hold up to 8 electrons in its outer shell.
The formal charge of the barium atom in barium peroxide is 0, as it has 2 valence electrons and is sharing 2 electrons with each oxygen atom. The formal charge of each oxygen atom is -1, as they each have 6 valence electrons and are sharing 2 electrons with the barium atom.
Yes, the Lewis structure of barium peroxide is stable. Each atom has a full outer shell and there are no lone pairs on the central atom. Additionally, the formal charges are all 0 or -1, which is a more stable arrangement than having formal charges of +1 or -2.