Redoxtest
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Showing posts with label redox. Show all posts
Showing posts with label redox. Show all posts
Wednesday, March 10, 2010
Monday, March 8, 2010
Redox Review
For today's class we did the exercise from page 29 on Balancing Redox Equations for Reactions Run in Acidic Conditions, letters c and d.
We learned that there are general steps:
- Write out which ones are oxidized and reduced and how many electrons are gained and lost.
- Balance out the elements other than the H and O.
- Balance the oxygen atoms by adding H2O molecules where needed.
- Balance hydrogen atoms by adding H+ ions where needed.
- Balance the charge by adding electrons, e-.
- Multiply one or both the half-reactions by a number that will equal both gained and lost electrons. (This is when the number of electrons lost in oxidation is not equal to the number of electrons gained in reduction.)
- Add the two reactions. Cancel electrons and cancel the same formulas found on opposite sides.
- Lastly, make sure that the charges and atoms balance out on both sides.
We also did the exercise on page 32 about Balancing Redox equations Run in Basic Conditions Using Half-reaction Technique.
We learn that there are also steps for these:
-First, do the same steps provided from above. Afterwards, proceed to the following steps given below.
-Add enough Hydroxide ions(OH-) to cancel the H+ ions. (Make sure its still balanced.)
-Combine H+ ions and OH- ions to form water then combine H2O (water molecules).
-Make sure its balanced :)
We also did the chapter 20 study guide sheet about Oxidation and Reaction.
**Btw, we have a test tomorrow on redox reactions. OMG :)
>> Next scribe is Janine Dolor.
We learned that there are general steps:
- Write out which ones are oxidized and reduced and how many electrons are gained and lost.
- Balance out the elements other than the H and O.
- Balance the oxygen atoms by adding H2O molecules where needed.
- Balance hydrogen atoms by adding H+ ions where needed.
- Balance the charge by adding electrons, e-.
- Multiply one or both the half-reactions by a number that will equal both gained and lost electrons. (This is when the number of electrons lost in oxidation is not equal to the number of electrons gained in reduction.)
- Add the two reactions. Cancel electrons and cancel the same formulas found on opposite sides.
- Lastly, make sure that the charges and atoms balance out on both sides.
We also did the exercise on page 32 about Balancing Redox equations Run in Basic Conditions Using Half-reaction Technique.
We learn that there are also steps for these:
-First, do the same steps provided from above. Afterwards, proceed to the following steps given below.
-Add enough Hydroxide ions(OH-) to cancel the H+ ions. (Make sure its still balanced.)
-Combine H+ ions and OH- ions to form water then combine H2O (water molecules).
-Make sure its balanced :)
We also did the chapter 20 study guide sheet about Oxidation and Reaction.
**Btw, we have a test tomorrow on redox reactions. OMG :)
>> Next scribe is Janine Dolor.
Wednesday, March 3, 2010
march 2, 2010
On tuesday's class we went over questions 2-11 on page 21
We also learned how to determine the following:
-which element is being oxidized or reduced
-an element is being oxidized if it has a loss in electrons. The charge becomes more positive
-an element is being reduced if it has a gain in electrons. The charge becomes more negative
-which substances are the oxidizing or reducing agent
For hand in we had to do questions 12-17 on page 21
We also learned how to determine the following:
-which element is being oxidized or reduced
-an element is being oxidized if it has a loss in electrons. The charge becomes more positive
-an element is being reduced if it has a gain in electrons. The charge becomes more negative
-which substances are the oxidizing or reducing agent
For hand in we had to do questions 12-17 on page 21
Monday, March 1, 2010
Redox
Today, Ms. K went over the Rules for Determining Oxidation Numbers, we also went over the homework that was assigned for us on Friday. The worksheet question 1-4: Assigning Oxidation Numbers -- Practice.
Oxidation - involves an increase in oxidation
Reduction - involves a decrease in oxidation #
We also learn, how to indicate whether or not the reaction is a Redox reaction
& we were asked to work on our yellow Booklet on page 21 question #2-17, for tomorrow.
- the next scribe will be JulieAnneNavea:)
Oxidation - involves an increase in oxidation
Reduction - involves a decrease in oxidation #
We also learn, how to indicate whether or not the reaction is a Redox reaction
Example of Reduction:
0 +1+5 -2--------> 0 +2 +5 -2
Cu + AgNO3------->Ag + Cu(NO3)
- Ag gain 1 electrons (Reduction)
- Cu loss of 2 electrons (Oxidation)
& we were asked to work on our yellow Booklet on page 21 question #2-17, for tomorrow.
- the next scribe will be JulieAnneNavea:)
Friday, February 26, 2010
February 26, 2010
Today, we got our Aqueous Reactions Test returned to us... or was that yesterday? I don't remember. Either way, the answers for the said test is posted up here; uploaded via slideshare.
We did some work on Oxidation and Reduction by going over pages 18 to 21 in the Aqueous Reactions Unit booklet. Remember that oxidation is the loss of electrons, and reduction is the gain of electrons and that the exchanging of electrons in a redox reactions occur simultaneously.
We went over the rules for assigning Oxidation Numbers. Note that the diatomic elements H2O2F2Br2I2N2Cl2 and pure elements have an oxidation number of zero. Also consider that the sum of the oxidation numbers in any neutral molecule is zero and that the sum in any ion is equal to the charge on the ion.
We were told to do questions 1 to 3, on the given practice worksheet "Assigning Oxidation Numbers". Also, Ms. Kozoriz swore by accident today. Just putting it out there.
Our next scribe will be the lovely Bernadette! :D
We did some work on Oxidation and Reduction by going over pages 18 to 21 in the Aqueous Reactions Unit booklet. Remember that oxidation is the loss of electrons, and reduction is the gain of electrons and that the exchanging of electrons in a redox reactions occur simultaneously.
We went over the rules for assigning Oxidation Numbers. Note that the diatomic elements H2O2F2Br2I2N2Cl2 and pure elements have an oxidation number of zero. Also consider that the sum of the oxidation numbers in any neutral molecule is zero and that the sum in any ion is equal to the charge on the ion.
We were told to do questions 1 to 3, on the given practice worksheet "Assigning Oxidation Numbers". Also, Ms. Kozoriz swore by accident today. Just putting it out there.
Our next scribe will be the lovely Bernadette! :D
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