SG Chem Reflection Week 5

This week we have had a homework assignment that was due Monday, a quiz, review guide and a final test on Friday.  Throughout this more stressful week, we began with the continuous study of mole conversations, finding atoms, and the amount of a specific element in a compound.  Along with theses studies, we have been able to expand our knowledge further than just the basics of each of theses topics. Starting with the beginning of the week we were able to comprehend how to find the amount of moles in a compound given a mass.

After completing the homework from the previous weekend that was due Monday, I felt more confident understanding how to complete the concept of finding moles due to the fact I was able to get a majority or the answers correct.  One of the more common questions on the worksheet but with more challenging numbers and a more challenging compound was number 9.  This problem allowed us to expand our knowledge on calculating moles and finding atoms in a given compound.  Therefore, this is how the chemical equation would be set up for problem 9.

After we were given the review guide, we managed to go over the answers as a class.  Without white boarding out all the answers, we managed to have the correct answers due to the fact the review guide was given to us on Moodle.  Beginning with definitions and ending with percentages, we covered everything we learned over the unit.  The newest lesson we were introduced to was the empirical and molecular formula.  Defining the empirical formula is only based on the data in specific situations.  On the other hand, the molecular formula is the same as or multiple of the empirical formula.  In most situations, you will have two or more elements with a given amount of mass, then you will use the mole conventions for each substance.  Therefore, you will use the periodic table to find the atomic mass for each substance and solve the equation like a regular mole problem.  Next, use the lowest number and divide each of the answers found to complete the problems.  After figuring out what the answer is after dividing the lowest number, is it a simple task to find the empirical formula.  For example, if the number is one, then you only have on of the certain substance.  Below is a visual example of how to use the empirical formula.  

Beginning the topic of molar mass was also a simple lesson to handle.  Due to the fact the molar mass of a compound is the atomic number of each substance added together.  A few examples of finding the molar masses in each compound is NaCl.  To find the correct molar mass, you add the atomic number of Na which is sodium to the atomic number of Cl which is chlorine.  Here are a few examples of the compounds from the review guide and calculating there molar masses.  

Finally the last unit we touched base on this week was the molecular formula.  Combining the topic of empirical formula and the molar mass, you have the ability to come the conclusion on the molar mass.  The empirical formula is the compound you are able to come to the conclusion on after using the mol formulas. Then after finding the molar mass of the compound, you divide the original mass given by the molecular formula.  Then you use that number to multiply the empirical formula after simply divided the molar mass by the original mass.