1. Formation of MgO

2. Calculations Section 1.Balanced Equation 2Mg + O 2  2MgO (Starting Mass) + X  (ending Mass) 0.1+ X = 0.2 X (amt of O 2 ) = 0.1g 2.%Mg = (0.1/0.2) x 100 = 50% % O = (0.1/0.2) x 100 = 50% 3. % Error = ((0.1 – 0.1)/0.1) x 100 = 0% Perfect!

3. Conclusion Part 1 Magnesium Oxide was formed when Mg ribbon was heated and combined with oxygen in the air. The ionic compound was determined to be formed by the formation of white ash in the crucible after heating. The percent composition was determined to be 50% each of Mg and O, which is what is expected from the molecular formula.

4. Conclusion Part 2: Errors **** If your numbers worked out as ours did then you did not have any errors – state that your lab data was as expected, no errors. **** If your numbers did not work out as ours did then, possible sources of error were Not heating the ribbon hot enough Balance measuring error

5. Conclusion Part 3: Questions 1.Energy was released as heat and light 2.We know the reaction combined Mg and O due to the presence of white powder and an increase in product mass. 3.MgO 4.MgO, the white powder was present. 5.Our yield of MgO was exactly correct. The percent error was 0%.

6. Conclusion Part 4: Real World Application Ionic compounds have many useful applications in our everyday lives. MgO can be used in vitamin supplements to support healthy bones and muscles. Other ionic compounds using magnesium, such as magnesium chloride, can be used to melt snow and ice off sidewalks and roads.