Final answer:
The metal with a 4+ charge in a metallic oxide that is 36.81% oxygen by mass is determined through stoichiometry and molar mass calculations to be titanium (Ti⁴+).
Step-by-step explanation:
To find the metal with a 4+ charge in a metallic oxide that is 36.81% oxygen by mass, we'll use stoichiometry and the concept of molar mass. If we know the oxide is 36.81% oxygen, then the remainder (100% - 36.81% = 63.19%) is the mass percentage of the metal. Since oxygen has a molar mass of approximately 16 g/mol, and each oxygen has a -2 charge, the formula of the oxide would require two oxygen atoms to balance out the 4+ charge from the metal, resulting in a metallic oxide formula of M(4+)O₂(2-).
Let's consider the molar mass of this metallic oxide. We have 2 moles of oxygen, which equals to 32 g/mol. Since 36.81% is the mass of the oxygen, we can calculate the total molar mass of the compound: (32 g/mol / 0.3681 = 86.94 g/mol approximately). Now, subtracting the mass of oxygen (32 g/mol) from the total molar mass (86.94 g/mol), we get the molar mass of the metal, which is approximately 54.94 g/mol. The metal with a molar mass close to this and having a common 4+ charge is titanium (Ti), with a molar mass of about 47.87 g/mol.
Therefore, the metal in the oxide, having a 4+ charge, is Ti⁴+.