Questions: Use Lewis theory to determine the chemical formula for the compound formed between Ba and O .

Solution Steps

Barium (Ba) is in Group 2 of the periodic table, so it has 2 valence electrons. Oxygen (O) is in Group 16, so it has 6 valence electrons.

Barium will lose its 2 valence electrons to achieve a stable electron configuration, forming a \( \text{Ba}^{2+} \) ion. Oxygen will gain 2 electrons to achieve a stable electron configuration, forming an \( \text{O}^{2-} \) ion.

To form a neutral compound, the total positive charge must balance the total negative charge. Since \( \text{Ba}^{2+} \) has a +2 charge and \( \text{O}^{2-} \) has a -2 charge, one \( \text{Ba}^{2+} \) ion will combine with one \( \text{O}^{2-} \) ion.

Final Answer