Saturday, May 24, 2008
Fri-Day 1
Bio- For the rest of the school year, bring in your Glencoe Living Environment Review books for Regents review in class!
We took our Ecology/Human Impacts exam, which I'll return to you on Wednesday after the makeups are given on Tuesday.
We then began Regents exam review by emphasizing the ULTRA-important test-taking skills that you MUST use on your Regents exam in order to maximize your score and effort.
We dissected each question by 1. topic , 2. key terms, 3. predicted answer, and 4. finding the matching or synonymous answer choice.
I'll post the rest of that Regents on Blackboard so that we can go over it at extra help on Tuesday morning. Complete that test this weekend so that you can identify your strengths and weaknesses; we can efficiently address any questions that were difficult for you.
Chem 7- On Blackboard, check out the link to the interactive Voltaic cell!
We built a spontaneous Voltaic/Galvanic cell, labeled its parts, and explained how the two half reactions were used to generate electricity.
We then built a cell that is the OPPOSITE of a spontaneous cell: the ELECTROLYTIC cell, one that REQUIRES a battery/voltage source in order to CAUSE a nonspontaneous reaction to occur.
However, reduction still occurs at the CATHODE (RED CAT) and oxidation still occurs at the anode BUT the + and - signs are changed in an electrolytic cell (anode is now (+) and cathode is now (-), by definition).
We then saw how to use Table J to predict whether a given reaction is spontaneous or not. If the MORE active (higher on the chart) metal LOSES electrons in the reaction, then the reaction is spontaneous/natural.
Chem 8/9- On Blackboard, check out the link to the interactive Voltaic cell!
We built a spontaneous Voltaic/Galvanic cell, labeled its parts, and explained how the two half reactions were used to generate electricity.
We then built a cell that is the OPPOSITE of a spontaneous cell: the ELECTROLYTIC cell, one that REQUIRES a battery/voltage source in order to CAUSE a nonspontaneous reaction to occur.
However, reduction still occurs at the CATHODE (RED CAT) and oxidation still occurs at the anode BUT the + and - signs are changed in an electrolytic cell (anode is now (+) and cathode is now (-), by definition).
We then saw how to use Table J to predict whether a given reaction is spontaneous or not. If the MORE active (higher on the chart) metal LOSES electrons in the reaction, then the reaction is spontaneous/natural.
We then did a little lab that tested whether the above predictions were observed in practice by performing 6 single replacement reactions.
We took our Ecology/Human Impacts exam, which I'll return to you on Wednesday after the makeups are given on Tuesday.
We then began Regents exam review by emphasizing the ULTRA-important test-taking skills that you MUST use on your Regents exam in order to maximize your score and effort.
We dissected each question by 1. topic , 2. key terms, 3. predicted answer, and 4. finding the matching or synonymous answer choice.
I'll post the rest of that Regents on Blackboard so that we can go over it at extra help on Tuesday morning. Complete that test this weekend so that you can identify your strengths and weaknesses; we can efficiently address any questions that were difficult for you.
Chem 7- On Blackboard, check out the link to the interactive Voltaic cell!
We built a spontaneous Voltaic/Galvanic cell, labeled its parts, and explained how the two half reactions were used to generate electricity.
We then built a cell that is the OPPOSITE of a spontaneous cell: the ELECTROLYTIC cell, one that REQUIRES a battery/voltage source in order to CAUSE a nonspontaneous reaction to occur.
However, reduction still occurs at the CATHODE (RED CAT) and oxidation still occurs at the anode BUT the + and - signs are changed in an electrolytic cell (anode is now (+) and cathode is now (-), by definition).
We then saw how to use Table J to predict whether a given reaction is spontaneous or not. If the MORE active (higher on the chart) metal LOSES electrons in the reaction, then the reaction is spontaneous/natural.
Chem 8/9- On Blackboard, check out the link to the interactive Voltaic cell!
We built a spontaneous Voltaic/Galvanic cell, labeled its parts, and explained how the two half reactions were used to generate electricity.
We then built a cell that is the OPPOSITE of a spontaneous cell: the ELECTROLYTIC cell, one that REQUIRES a battery/voltage source in order to CAUSE a nonspontaneous reaction to occur.
However, reduction still occurs at the CATHODE (RED CAT) and oxidation still occurs at the anode BUT the + and - signs are changed in an electrolytic cell (anode is now (+) and cathode is now (-), by definition).
We then saw how to use Table J to predict whether a given reaction is spontaneous or not. If the MORE active (higher on the chart) metal LOSES electrons in the reaction, then the reaction is spontaneous/natural.
We then did a little lab that tested whether the above predictions were observed in practice by performing 6 single replacement reactions.
# posted by C @ 11:33 AM 
