For a hydrogen- like atom, classify these electron transitions by whether they result in the absorption or emission of light: n=3 to n=5, n=1 to n=3, n=3 to n=2, n=2 to n=1? ignoring the sign, which transition was associated with the greatest energy change

The electron transfer from n = 1 to n = 3 occurs the greatest energy change

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

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)

Determination of electron configurations based on principles:

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

then the value of E is

delta E = -1/25 +1/9 = 0.07

then the value of E is

delta E = -1/9 + 1/1 = 0.89

then the value of E is

delta E = -1 / 9 + 1/16 = 0.14

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

 statement about electrons and atomic orbitals

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Effective nuclear charge

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statement about subatomic particles is true

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Keywords: electron transfer, quantum number, electron shell

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8