How much energy is required to move the electron of the hydrogen atom from the 1s to the 2s orbital
The "gas" needed for the electron transport chain is Hydrogen. In the electron transport chain its not Hydrogen gas H2 but a Hydrogen Ion H negative that flows across the membrane to produce engery.
For example when the electron absorb energy.
Briefly, it is the energy required to completely remove a valence (outer shell) electron from its atom when forming an ionic bond.See related links below for more info
Since work function is the energy needed to dislodge the electron, I'd say that the unit is Joules or eV (electron Volts).
Ionization energy
bond energy
Each energy level corresponds to an exact amount of energy needed by the electron to orbit the nucleus. Transitions from a higher energy level to a lower energy level correspond to the difference in the energy needed for an electron to occupy those two energy levels. This difference creates the emission spectrum.
The "gas" needed for the electron transport chain is Hydrogen. In the electron transport chain its not Hydrogen gas H2 but a Hydrogen Ion H negative that flows across the membrane to produce engery.
Hydrogen because it has one electron in one energy level and is needed to make water (essential liquid).
The amount of energy needed to move an electron from one energy level to another is called a quantum.
There is an attraction of the nucleus for electrons. This attractive force must be overcome to remove an electron. The energy to overcome this attraction and remove an electron from the atom is 'ionization energy'.
The energy needed to remove an electron from an atom (in the gaseous state) is called the IONIZATION ENERGY.
For example when the electron absorb energy.
1.94 x 10-18 Joules
One atom is needed to full the outer shell of a hydrogen atom, this is bacuse in GCSE terms electrom structure goes 2,8,8,2 and hydrogen only has one shell, so it would need 2 to complete this shell. This is the same for A-level however we refer to electron structure in spd, the electron structure of hydrogen then would be 1s1.
Light or photons are little packets of energy. When this energy is absorbed by an electron it boots the electrons energy and the electron jumps to a higher orbital shell position (which must be vacant of its electron). The electron can only do this when the energy needed for the jump and the energy in the incoming photon match. Thus specific colours of light are absorbed depending on the element present.
This is the energy needed to extract an electron from an atom in gaseous phase, to form a cation.