oxidation-reduction.....aims
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oxidation-reduction.....aims |
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aim 1.....what are oxidation numbers? quiz
aim 2.....what is a redox reaction? quiz
aim 3.....what are electrochemical cells? quiz
aim 4.....what are electrolytic cells? quiz
cross-word puzzle
skills students should be able to do
skills students should be able to do
determine a missing reactant or product in a balanced equation
write and balance half-reactions for oxidation and reduction of free elements and their monatomic ions
identify and label the parts of a voltaic cell (cathode, anode, salt bridge) and direction of electron flow, given the reaction equation
use an activity series to determine whether a redox reaction is spontaneous
identify and label the parts of an electrolytic cell (anode, cathode) and direction of electron flow, given the reaction equation
compare and contrast voltaic and electrolytic cells
patina (copper-Statue of Liberty)
metallurgy of iron and steel
electroplating
smelting
leaching (refining of gold)
thermite reactions (reduction of metal oxides, e.g., aluminum)
recovery of active non- metals (I2)
electrochemical
corrosion
electrolysis
photography
rusting
Words: cathode, changes, electrochemical, electrolysis, electrolytic, half reaction, ions, lost, oxidation, redox, reduction, voltaic
An oxidation-reduction (_____) reaction involves the transfer of electrons (e-). ________ is the gain of electrons. A _______________ can be written to represent reduction. __________ is the loss of electrons. A half-reaction can be written to represent oxidation. In a redox reaction the number of electrons _____ is equal to the number of electrons gained. Oxidation numbers (states) can be assigned to atoms and ____. ________ in oxidation numbers indicate that oxidation and reduction have occurred. An ______________ cell can be either voltaic or electrolytic. In an electrochemical cell, oxidation occurs at the anode and reduction at the ________. A ________ cell spontaneously converts chemical energy to electrical energy. An ___________ cell requires electrical energy to produce chemical change. This process is known as ____________.