Oxidation/Reducion + Quantitative Chemistry
Redox Equations
Reactivity
Voltaic Cells
Electrolytic Cells
100
The loss of electrons is _____. The gain of electrons is ______.
Oxidation and Reduction
100
A blank is chemical reaction in which changes in the oxidation number occurs ____.
Redox Reaction
100
More reactive metals are more likely to _____ electrons. More reactive non-metals are more likely to _____ electrons.
Lose and Gain
100
A voltaic cells converts _____ energy to _______ energy.
chemical to electrical energy. (spontaneous) The energy is postive.
100
An electrolytic cell converts _____ energy to ______ energy.
Electrical to chemical energy. (non-spontaneous) The energy is negative.
200
What is formula for percent error?
| Theoretical - Experimental | / |Theoretical | X100
200
An oxidizing agent is _____ during a reaction. A Reducing agent is ______ during a reaction.
Reduced and Oxidized.
200
On the standard electrode potentials chart (Date Booklet Table 14) if the half-equation is undergoing oxidation do you change the sign value or does it stay the same?
Yes. Change it.
200
What is the device that is needed to connect the two half-cells?
A salt bridge.
200
The electrolyte must be at what state of matter to conduct electricity?
Liquid, metals need to be molten and ionic compounds need to be aqueous.
300
Oxidation number for uncombined elements is always ____. Group elements always have the oxidation number of ____. Group two elements always have an oxidation number of _____. Oxygen is usually ____ only _____ in peroxids. Group seven non-metals are ___ in compounds with lower electronegativity. Hydrogen is ____ except in certain metal hydrides where the oxidation number is ____.
0 +1 +2 -2, -1 -1 +1 , -1
300
In redox reactions ______ and ______ occur at the same time.
oxidation and reduction.
300
What are the standard conditions for energy plymsol?
1. 25 Degrees Celsius 2. 101 Kpa 3. Standard State 4. 1.0M/1.0 moles dm -3
300
Oxidation occurs at the ____. Reduction occurs at the ______.
Anode and Cathode. (Same for electrolytic cell)
300
Electrons flow from ____ to _____.
Anode to cathode. (Same for voltaic cell)
400
Give the oxidation number of nitrogen in: HNO3
+5
400
When solving acidic redox reactions, what are the steps to solving the problem? 1.) Assign _______ numbers. 2.) Write ______ half-equations. 3.) Balance ______. 4.) Balance oxygens with _____. 5.) Balance hydrogen with _____. 6.) Balance _______. 7.) Equalize ______ before adding _______equations. 8.) Add ____ equations and add _____ of matter.
1.) Oxidation 2.) seperate 3.) atoms 4.) H20 5.) H+ 6.) electrons 7.) electrons , half 8.) half, states
400
Is this reaction possible? Cl2 + KF --> F2 + KCl
No.
400
What is the equation to determine the energy in the voltaic cell?
E oxidation +E reduction= E cell
400
In and electrolytic cell, what are the half-equations for the reactions of molten NaCl?
Na is attracted to (-). Reducing. Na(+) + 1e- ---> Na(0) Cl (-) to the anode. Oxidized. Cl (-) -----> 1/2 Cl (0) + 1e-
500
Give the oxidation number for chromium: [Cr(H2O)6] 3+
-3
500
What is the oxodizing agent? 2 Mg + O2 --> 2 MgO
Oxygen
500
Free pass: YOU GET 500 points.........if you can name all the polyatomic ions!
(OH)- (NO3)- (SO4) 2- (CO3) 2- (PO4) 3- (NH4) + (HC03) - (CH3COO)-
500
The anode is _____ charged. The cathode is _____ charged.
Anode is negative. Cathode is postive.
500
The anode is _____ charged. The cathode is _____ charged.
Anode is postive. Cathode is negative.
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