Gently knock on the standard primary battery.
And that definition of electrode potential.
Using a standard hydrogen electrode
Measuring the reduction potential of atoms of elements
Metal atoms in solution
Lose its electrons
Let it enter the ionic solution
With the flow of salt bridge
Metal elements become negative because of electrons.
Electrons go from negative electrode to positive electrode.
Ions flow into the salt bridge.
The anode and cathode of primary battery depend on oxidation.
The oxidant is the positive electrode.
The reducing agent is the negative electrode
Relates to redox reaction.
And its equation.
The role of salt bridge in it
Perfect the circuit
Blocking the reaction with ions
Remember the calculation of primary battery voltage.
Redox potential
The sum equals the voltage.
This is equivalent to battery energy.
Electrodes are divided into three categories.
Metal electrode, platinum electrode and graphite electrode
It depends on the type of electrode in the battery.
And electrodes between ions.
Platinum and graphite
Are all inert materials.
Platinum is used for gas ions
Graphite is used for liquids.
The role of salt bridge in it
Perfect the circuit
Blocking the reaction with ions
Remember the calculation of primary battery voltage.
Redox potential
The sum equals the voltage.
This is equivalent to battery energy.
Gently knock on the standard primary battery.
And that definition of electrode potential.
Using a standard hydrogen electrode
Measuring the reduction potential of elemental atoms
If the total voltage is zero
The battery cannot run.
Let the copper-zinc primary battery be used as
Examples of metal electrodes
The role of salt bridge in it
Perfect the circuit
Blocking the reaction with ions
Remember the calculation of primary battery voltage.
Redox potential
The sum equals the voltage.
This is equivalent to battery energy.
The role of salt bridge in it
Perfect the circuit
Blocking the reaction with ions
Remember the calculation of primary battery voltage.
Redox potential
The sum equals the voltage.
This is equivalent to battery energy.
The role of salt bridge in it
Perfect the circuit
Blocking the reaction with ions
Remember the calculation of primary battery voltage.
Redox potential
The sum equals the voltage.
This is equivalent to battery energy.
[00:32.410]Gently knock on the standard primary battery.
[00:36.030]And that definition of electrode potential.
[00:39.390]Using a standard hydrogen electrode
[00:41.460]Measuring the reduction potential of atoms of elements
[00:46.560]Metal atoms in solution
[00:49.890]Lose its electrons
[00:53.070]Let it enter the ionic solution
[00:56.520]With the flow of salt bridge
[01:01.410]Metal elements become negative because of electrons.
[01:04.770]Electrons go from negative electrode to positive electrode.
[01:08.190]Ions flow into the salt bridge.
[01:10.290]The anode and cathode of primary battery depend on oxidation.
[01:15.360]The oxidant is the positive electrode.
[01:18.660]The reducing agent is the negative electrode
[01:21.900]Relates to redox reaction.
[01:25.230]And its equation.
[01:30.570]The role of salt bridge in it
[01:32.280]Perfect the circuit
[01:33.900]Blocking the reaction with ions
[01:37.380]Remember the calculation of primary battery voltage.
[01:44.130]Redox potential
[01:45.720]The sum equals the voltage.
[01:50.670]This is equivalent to battery energy.
[01:57.270]Electrodes are divided into three categories.
[02:00.540]Metal electrode, platinum electrode and graphite electrode
[02:03.960]It depends on the type of electrode in the battery.
[02:07.560]And electrodes between ions.
[02:11.250]Platinum and graphite
[02:14.460]Are all inert materials.
[02:17.730]Platinum is used for gas ions
[02:21.000]Graphite is used for liquids.
[02:26.310]The role of salt bridge in it
[02:28.050]Perfect the circuit
[02:29.730]Blocking the reaction with ions
[02:33.510]Remember the calculation of primary battery voltage.
[02:39.930]Redox potential
[02:41.520]The sum equals the voltage.
[02:46.440]This is equivalent to battery energy.
[02:53.070]Gently knock on the standard primary battery.
[02:56.340]And that definition of electrode potential.
[02:59.790]Using a standard hydrogen electrode
[03:01.860]Measuring the reduction potential of elemental atoms
[03:07.020]If the total voltage is zero
[03:10.290]The battery cannot run.
[03:13.500]Let the copper-zinc primary battery be used as
[03:16.800]Examples of metal electrodes
[03:20.730]The role of salt bridge in it
[03:23.880]Perfect the circuit
[03:25.500]Blocking the reaction with ions
[03:29.010]Remember the calculation of primary battery voltage.
[03:35.700]Redox potential
[03:37.290]The sum equals the voltage.
[03:42.210]This is equivalent to battery energy.
[03:49.230]The role of salt bridge in it
[03:51.000]Perfect the circuit
[03:52.620]Blocking the reaction with ions
[03:56.100]Remember the calculation of primary battery voltage.
[04:02.760]Redox potential
[04:04.380]The sum equals the voltage.
[04:09.330]This is equivalent to battery energy.
[04:16.320]The role of salt bridge in it
[04:18.030]Perfect the circuit
[04:19.620]Blocking the reaction with ions
[04:23.130]Remember the calculation of primary battery voltage.
[04:29.760]Redox potential
[04:31.380]The sum equals the voltage.
[04:36.210]This is equivalent to battery energy.