Chapter 7 - Oxidation And Reduction Flashcards
Give the oxidation state of manganese in the MnO4− ion (1)
+7
X - 8 = -1
Write the simplest ionic equation for the reaction of chlorine with bromide ions. (1)
Cl2 + 2Br- —> 2Cl− + Br2
In terms of electrons, state the meaning of the term oxidising agent. (1)
-accepts electrons
In sunlight, chlorine can also oxidise water slowly to form oxygen. Write an equation for this reaction. (2)
2Cl2 + 2H2O —> 4HCl + O2
Ferrovanadium is produced by the reaction of aluminium with a mixture of V2O5 and iron(III) oxide.
Write an equation for the reaction of aluminium with iron(III) oxide.
State the change in oxidation state of aluminium in this reaction. (2)
2Al + Fe2O3 —> 2Fe + Al2O3
Write an equation for the reaction of iron with antimony sulfide (Sb2S3) to form antimony and iron(II) sulfide. (1)
3Fe + Sb2S3 —> 3FeS + 2Sb
.Which of these species is the best reducing agent?
A Cl2
B Cl−
C I2
D I−
I-
Describe oxidation in terms of oxygen, hydrogen and electrons (3)
-addition of oxygen,
-loss of electrons,
-loss of hydrogen
Describe reduction in terms of oxygen, electrons , oxidation number and hydrogen (3)
-loss of oxygen,
-decrease in oxidation number
-gain of hydrogen,
-gain of electrons
Describe oxidation and reduction in terms of oxidation state (2)
-reduction = decrease in oxidation state,
-oxidation = increase in oxidation state
Describe oxidizing agents and reducing agents (2)
-oxidizing agents = oxidizes another atom and reduces itself,
-reducing agents = reduces another atom and oxidizes itself, its oxidation state will increase
Oxidation state of S in SO2 …………………………………………………………..
Oxidation state of S in H2SO4 …………………………………………………….. (2)
SO2 = 4,
H2SO4 = 6
With reference to electrons, give the meaning of the term reducing agent (1)
Electron donor
Give the oxidation state of phosphorus in each of the following. P4 …………………………………………………….
H3PO4 ……………………………………………… (2)
P4 = 0
H3PO4 = 5
