2) Based on the charges of magnesium and oxygen ions (see above), what would one predict for the formula of magnesium oxide? Mg ^2++ 02- MgO 2. Below are some reasons why you may not have gotten the correct Mg/O ratio. Explain whether these mistakes will cause the Mg/O ratio to be too large, too small, or if the error would not affect the ratio at all. For example: Not heating the Mg as hot as in the instructions say. Answer: If not heating the Mg as hot as instructed, not all of the Mg will be reacting with oxygen to become MgO, which would cause a lower mass of MgO. Since the mass of O (mass of MgO-mass of Mg), the mass and the number of moles of O will be lowered. It will hence increase the Mg/O ratio making it higher than expected. Mistake 1: Spilling a little of the ash residue before the final weighing Mistake 2: The residue at the end still has some water absorbed on it 3. Use the formula of magnesium oxide you derived in Question #1 to write out a balanced chemical equation of the burning of magnesium metal in oxygen gas to generate magnesium oxide. Make sure to indicate the physical state (s, 1, g, or aq) for each of the substances in the equation. 4. Classify the above reaction in question #3 in as many ways as possible. Circle the correct answer(s). If needed, review Chapter 7 section "Classify Chemical Reactions". acid-basecombination/synthesiscombustion decompositionoxidation-reductionprecipitation Footer