Redox💃
Substance A undergo oxidation.
Substance A is ___
reducing agent
Substance B undergo reduction.
Substance B is ___.
oxidising agent
Mg + CuO ---> MgO + Cu
-CuO lose ___.
-CuO undergo ___.
-CuO is ___.
-CuO is ___.
-oxygen
-reduction reaction
-reduced
-oxidising agent
Mg + CuO ---> MgO + Cu
-Mg gains ___.
-Mg undergo ___.
-Mg is ___.
-Mg is ___.
-oxygen
-oxidation reaction
-oxidised
-reducing agent
H2S + Cl2 ---> HCL + S
-Cl2 gain ___.
-Cl2 undergo ___.
-Cl2 is ___.
-hydrogen
-reduction reaction
-oxidising agent
H2S + Cl2 ---> HCL + S
-H2S lose ___.
-H2S undergo ___.
-H2S is ___.
-hydrogen
-oxidation reaction
-reducing agent
2NH3 + 3CuO ---> N2 + 3H2O + 3Cu
-CuO lose ___.
-CuO undergo ___.
-CuO is ___.
-oxygen
-reduction reaction
-oxidising agent
Oxidation number for element always ___.
zero
Na oxidation number
0
O2 oxidation number
0
S8 oxidation number
0
Oxidation for ion (got charge) always ___as their charge
same
Na+ oxidation number
+1
Oxidation number for oxygen when pair with other always ___.
-2
H2O2 hydrogen peroxide
Oxidation number of oxygen is ___.
-1
Oxidation number for hydrogen when pair with others is always ___.
+1
Metal hydride is ___
metal + hydrogen
Metal hydride oxidation number is ___.
-1
Sodium hydride oxidation number is ___.
-1
H2 + Cl2 ---> 2HCL
-Oxidation number of H ___ from __ to __.
-H2 molecule undergo ___.
-H2 is ___.
-increases, 0, +1
-oxidation reaction
-reducing agent
2NH3 + 3CuO ---> N2 + 3H2O + 3Cu
-NH3 lose ___.
-NH3 undergo ___.
-NH3 is a ___.
-hydrogen
-oxidation reaction
-reducing agent
H2 + Cl2 ---> 2HCL
- Oxidation number of Cl ___from __to__.
-Cl2 molecule undergo ___.
-Cl2 molecule is ___.
-decreases, 0, -1
-reduction reaction
-oxidising agent
Zn + Br2 ---> ZnBr2
-Oxidation number of Zn ___, from ___ to ___.
-Zn undergo ___.
-Zn is a ___.
-increases, 0, +2
-oxidation reaction
-reducing agent
Zn + Br2 ---> ZnBr2
-Oxidation number of Br ___ from ___ to ___.
-Br2 undergo ___.
-Br2 is a ___.
-decreases, 0, +2
-reduction reaction
-oxidising agent
What is the oxidation number of Mn in MnO^- 4 ?
+7
What is the oxidation number of N in N^+ 4 ?
-3
What is the oxidation number of Cr in K2Cr2O7?
+6
Mg + CuSO4 ---> MgSO4 + Cu
Give the ionic equation and the two half equation.
-Mg + Cu^2+ ---> Mg^2+ + Cu
-Mg ---> Mg^+2 + 2e
-Cu^2+ + 2e ---> Cu
Zn + 2HNO3 ---> Zn(NO3)2 + H2
Give the ionic equation and the two half equation.
-Zn + 2H^+ ---> Zn^+2 + H2
-Zn ---> Zn^2+ + 2e
-2H^+ + 2e ---> H2
Ca + 2AgNO3 ---> Ca(NO3)2 + 2Ag
Give the ionic equation and the two half equation.
-Ca + 2Ag^+ ---> Ca^2+ + 2Ag
-Ca ---> Ca^2+ + 2e
-Ag^+ + e ---> Ag
In half equation if electron is found on the left undergo ___.
reduction reaction
In half equation if electron is found on the right undergo ___.
oxidation reaction
Electrochemical Series:
K
___
Ca
___
Al
Na, Mg
Electrochemical series:
Zn
___
Sn
___
H
__
Ag
Fe, Pb, Cu
Fe^2+ to ___.
Fe^3+
Oxidising agent:
1. Chlorine ,___
2. Bromine,___
3. Acidified potassium manganate (VII) solution,___
4. Acidified potassium dichromate (VI) solution,___
5. Hydrogen peroxide,___
-Cl2
-Br2
-KMnO4
-K2Cr2O7
-H2O2
Conversion of Fe^2+ to Fe^3+ refer to ___. Now!
modul
Colour of Fe^3+
Brown
Colour of Fe^2+
Green
Colour of chlorine water
Pale yellow
Colour of bromine water
Brown
Colour of Iodine water
Brown
MnO^- 4 to ___
Mn^2+
Cr2O^2- 7 to ___
Cr^3+
Colour of Cu^2+
Blue
Colour of MnO^- 4
Purple
Colour of Cr2O^2- 7
Orange
Colour of Cr^3+
Green
Fe^3+ to __
Fe^2+
3 reducing agent:
1. Magnesium,___
2. Zinc,___
3. All halide ion (Group 17 ion),___
-Mg
-Zn
-Cl^-, Br^-, I^-
Convertion of Fe^3+ to Fe^2+ refer to ___. Now!
modul
In half equation, metal dissolve to become ___.
ion
Ignore K^+, SO^2- 4, NO^- 3 because they are ___.
spectator ions
All metals dissolve to ion are ___ except ___ is brown solid.
grey solid, copper
Halogen is group 17 ____ molecule.
neutral
Examples of group 17 :
-___, Cl2
-___,Br2
-___,I2
-Chlorine
-Bromine
-Iodine
Halide is group 17 ___.
ion
Example of halide :
-___,Cl^-
-___,Br^-
-___,I^-
-Chloride ion
-Bromide ion
-Iodide ion
Halogen ascending order gangster.
I, Br, Cl, F
Cl2 + 2 KI ---> ____
2KCl + I2
Br2 + KCl ---> ___
No reaction
Halide displacement essay refer to ___.
modul
Cl2 colour
Pale yellow
Br2 colour
Brown
I2 colour
Brown
All halide ions are ___.
Colourless
U-tube refer to ___.
modul
The function of salt bridge is to allow ___ to pass through to ___ the ___.
ions, complete, circuit
Suggest suitable material to be used as salt bridge.
-Dilute sulphuric acid
-Soluble salt (sodium chloride, potassium nitrate)
Half cell is a combination of a___ with a ___ that contain ___ ion.
metal, solution, metal
SEP refer to ___.
modul
-More positive E°
-Keen to___electron
-Easy to undergo ___
-Strong___agent
-receive
-reduction
-oxidising
-More negative E°
-Keen to ___ electron
-Easy to undergo ___
-Strong ___agent
-release
-oxidation
-reducing
State 3 standard conditions for half cell.g
-Temperature : 25°C
-Pressure : 1 atm
-Concentration : 1 mol dm^-3
Function of Voltaic cell/ Electrochemical cell/ Chemical cell/ Galvanic cell.
Generate electricity
Energy changes of Voltaic cell/ Electrochemical cell/ Chemical cell/ Galvanic cell.
Chemical energy ---> Electricity energy
2 types of Voltaic cell.
Simple cell and Daniel cell
Function of porous pot is to allow ___to pass through to ___ the ___.
ions, complete, circuit
Anode : Where electron is ___.
donated
Cathode : Where electron is ___.
received
Voltaic cell refer to __.
modul
For metal half cell :
metal + metal ion solution
For non-metal half cell :
non-metal + non-metal ion solution
Metal half cell use metal ____.
electrode
Non-metal half cell use ___ electrode.
platinum
Function of electrolytic cell.
Use electricity to breakdown compound.
Electrolytic cell converts
Electrical energy ---> Chemical energy
Function of battery/ dry cell.
Supply electricity
Electrolysis of molten use___.
crucible and heat
Electrolysis of aqueous solution use ___.
beaker and water
Electrolyte is the substance that able to conduct ____ in ___ state or ___ state and undergo ___ change.
electricity, molten, aqueous, chemical
Pure metal is not consider as electrolyte. Why ?
Pure metal is a conductor
Conductor :
-Able to conduct electricity in ___ form or ___ form.
-Do not undergo ____ changes
-Example : All ___, ___ (graphite)
-Able to conduct ___ due to free ____
-solid, molten
-chemical
-metals, carbon
-electricity, moving electrons
Electrolyte :
-Able to conduct electricity in ___ form or ___ form.
-Undergo ___ changes.
-Example : All ___&____, ____ compound (metal+non-metal)
-Able to conduct __ due to free ___.
-molten, aqueous
-chemical
-acid, alkali, ionic
-electricity, moving ions
Electrolysis of Molten Compound refer to ___.
modul
Cl2 gas colour
Greenish-yellow gas
Br2 gas colour
Brown gas
I2 gas colour
Purple gas
O2 & H2 gas colour
Colourless gas
At voltaic cell, negative terminal is ___& positive terminal is ___.
anode, cathode
In electrolytic cell, negative terminal is ___& positive terminal is ____.
cathode, anode
3 factor that affects electrolysis of aqueous solution.
E° value, concentration, type of electrode used