Wednesday, May 16, 2007
Wednes-Day 1
Regents and Honors class:
By Monday, you must take your first of MANY practice Regents exams. The instructions for this Regents exam will be posted by tomorrow. You must show your work for each question on separate paper, which will be graded based on quality of effort and accuracy.
Do NOT be foolish with these practice tests! I am supplying the (minimal) answer key for each test. If you simply copy the key, you will learn NOTHING and you will go into the Regents unprepared and you will likely fail.
If you need to use a key to CHECK your work or reasoning AFTER you have done the test, that is fine, of course. However, you MUST keep track, for yourself, of the questions/topics that you need help with. Furthermore, many of the answer Regents answer keys give the ABSOLUTE bare MINIMUM of what qualifies for a correct answer. DO NOT lower yourself to such low quality answers or you will find that you are not prepared for this year's Regents. It is easy to dumb yourself down on Regents day, it is not possible to suddenly increase your knowledge of things that you did not prepare for on that day.
Honors: we looked at a couple of ways to predict whether a redox reaction occurs spontaneously: we looked at the standard reduction potential chart and connected the REACTANTS. If the line connecting the reactants goes uphill (positive slope), the reaction is NOT spontaneous, if the line goes downhill, the reaction IS spontaneous. You can add up the reduction potential of the reactant that gets reduced and the OXIDATION potential (the opposite sign of the reduction potential) of the reactant that gets oxidized; if the sum is positive, the reaction is spontaneous.
We also looked at the activity series Table J (I will show this method to D period on Monday) to see which metals are more active (oxidized more easily) and which nonmetals are more active (more easily reduced) and applied this to predict whether a redox/single replacement is spontaneous.
We then discussed electroplating and forcing a nonspontaneous reaction to occur via an electroLYTIC cell. These cells use electricity (electrical energy) to force/cause a nonspontaneous chemical reaction to occur.
Regents: We also looked at the activity series Table J to see which metals are more active (oxidized more easily) and which nonmetals are more active (more easily reduced) and applied this to predict whether a redox/single replacement is spontaneous. We then began to discuss "electrolytic" cells.
By Monday, you must take your first of MANY practice Regents exams. The instructions for this Regents exam will be posted by tomorrow. You must show your work for each question on separate paper, which will be graded based on quality of effort and accuracy.
Do NOT be foolish with these practice tests! I am supplying the (minimal) answer key for each test. If you simply copy the key, you will learn NOTHING and you will go into the Regents unprepared and you will likely fail.
If you need to use a key to CHECK your work or reasoning AFTER you have done the test, that is fine, of course. However, you MUST keep track, for yourself, of the questions/topics that you need help with. Furthermore, many of the answer Regents answer keys give the ABSOLUTE bare MINIMUM of what qualifies for a correct answer. DO NOT lower yourself to such low quality answers or you will find that you are not prepared for this year's Regents. It is easy to dumb yourself down on Regents day, it is not possible to suddenly increase your knowledge of things that you did not prepare for on that day.
Honors: we looked at a couple of ways to predict whether a redox reaction occurs spontaneously: we looked at the standard reduction potential chart and connected the REACTANTS. If the line connecting the reactants goes uphill (positive slope), the reaction is NOT spontaneous, if the line goes downhill, the reaction IS spontaneous. You can add up the reduction potential of the reactant that gets reduced and the OXIDATION potential (the opposite sign of the reduction potential) of the reactant that gets oxidized; if the sum is positive, the reaction is spontaneous.
We also looked at the activity series Table J (I will show this method to D period on Monday) to see which metals are more active (oxidized more easily) and which nonmetals are more active (more easily reduced) and applied this to predict whether a redox/single replacement is spontaneous.
We then discussed electroplating and forcing a nonspontaneous reaction to occur via an electroLYTIC cell. These cells use electricity (electrical energy) to force/cause a nonspontaneous chemical reaction to occur.
Regents: We also looked at the activity series Table J to see which metals are more active (oxidized more easily) and which nonmetals are more active (more easily reduced) and applied this to predict whether a redox/single replacement is spontaneous. We then began to discuss "electrolytic" cells.
# posted by C @ 2:20 PM 
