Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy ΔG0 for the following r
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The electron transfer from n = 1 to n = 3 occurs the greatest energy change
<h3>Further explanation</h3>In an atom, there are energy levels in the skin and sub skin.
This energy level is expressed in terms of electron configurations.
Writing the electron configuration starts from the lowest to the highest subshell's energy level. There are 4 sub-shells in an atom's shell, namely s, p, d, and f. The maximum number of electrons for each subshell is
- s: 2 electrons
- p: 6 electrons
- d: 10 electrons and
- f: 14 electrons
The filling of electrons uses the following sequence:
1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.
Each sub-shell also has orbitals drawn in the form of a square box in which there are electrons symbolized by half arrows.
Each orbital in an atom consists of 4 quantum numbers, namely the main quantum number (n), the azimuth quantum number (l), and the magnetic quantum number (m) and the spin quantum number (s)
- Value of n: positive integer
- value of l: between 0 to n-1
- m value: between -l to + l
- value s: +1/2 or -1/2
Determination of electron configurations based on principles:
- 1. Aufbau: Electrons occupy orbitals of the lowest energy level
- 2 Hund: electron fills orbitals with the same energy level
- 3. Pauli: there are no electrons that have 4 equal quantum numbers
Bohr's atomic model has shown the energy levels of electrons in the path of the atomic shell
The greater the value of n (the atomic shell, the main quantum number), the greater the energy level
In normal circumstances, electrons fill the skin at the lowest energy level starting from the skin K, L M and then N
When an atom gets energy from outside, the electrons will absorb energy so it moves to higher energy. This situation is called excited
Electrons will return to the original path or a lower energy level because the excited state is unstable. In this condition, the electron will release energy
The electron energy at the nth path can be formulated:
En = -Rh / n²
Rh = constant 2.179.10⁻¹⁸ J
So the electron transfer energy (delta E)
delta E = E end - E start
From the electron transfer available, because the value of the Rh constant is the same, the effect is the value of n (skin) ---> 1/n²
- 1. n = 3 to n = 5
then the value of E is
delta E = -1/25 +1/9 = 0.07
- 2. n = 1 to n = 3,
then the value of E is
delta E = -1/9 + 1/1 = 0.89
- 3.n = 3 to n = 2,
then the value of E is
delta E = -1 / 9 + 1/16 = 0.14
- 4. n = 2 to n = 1
then the value of E is
delta E = -1/4 + 1 = 0.75
These 4 values indicate that regardless of the sign that there is an electron transfer from n = 1 to n = 3 the greatest energy change occurs
<h3>Learn more</h3>
statement about electrons and atomic orbitals
Effective nuclear charge
statement about subatomic particles is true
Keywords: electron transfer, quantum number, electron shell
