Sg Chemistry 2 blog of week 10/12

Sg Chem 2 reflection paper

Obi Ilozor 3rd hour

In this week of Sg Chemistry, we took 2 assessments and reviewed what we learned in the previous week. The only new concept that we learned about was the molecular formula and empirical formula. We reviewed conversions from moles to number of atoms, grams to moles, grams to number of atoms, and vice versa for all of these examples. We learned about relative mass  We also learned about diatomic atoms where they double in mass in a gaseous state. Finally, we learned about element composition in a compound. On Friday, we began chapter 6 with a discussion about what keeps atoms together and how H2O was separated by the electrolosis contraption. 

First, we reviewed relative mass in a worksheet. We were told to look back to our old relative mass lab with washers, nails, and hexes. All of the materials were measured relative to the mass of the lightest object which was the washer. We did this lab to relate to all elements whose masses are relative to hydrogen which is the smallest element on the periodic table

On friday, we discussed how the electrolosis machine worked. No real answer was given to us yet but I theorize that what keeps compounds together are electrical bonds. It has something to do with magnetism and what particles attract others. When water is put into the elctrolosis machine, a current is sent through it. The electrical current somehow breaks the electrical bonds by maybe reversing an elements polarity but whatever it does, it breaks the compounds into two different elements and then separates them.

Second, we reviewed the conversions for moles, number of atoms, and mass. It is a fairly simple concept where if you want to convert something to another, you must put the unit that will cancel out on the bottom and the unit you want on the top. One important thing is that you cannot skip moles in the conversion of mass to number of atoms and vice-versa. You must go through the middle man. 

Third, we learned about the empirical formula and molecular formula. The empirical formula is the most simple formula of a compound such as H2O. A molecular formula is a variation of the empirical formula except it is not the most simple. Such a formula, relative to the one presented previously in the paragraph, could be H6O3. It just has to maintain the same ratio. You can calculate a lot of problems using these two formulas. The mass to mole conversion is used in these problems and then you are supposed to eyeball the ratio at which these elements combine at.

Fourth, we learned about percent composition of an element by mass. This was by far the easiest concept and it just used simple division to see how much of an element is in a compound. In the case of H20, oxygen has a 33 percent element composition in that compound. As you can see, it is very simple.

This chapter was a fun chapter and to me, it was much easier than chapter four. The hardest concept of this chapter was the mole to gram coversion factors and those weren't even that hard. Overall, I liked this chapter the most out of all of them so far. Thanks for reading