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

Further explanation

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 electronsp: 6 electronsd: 10 electrons andf: 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 integervalue of l: between 0 to n-1m value: between -l to + lvalue s: +1/2 or -1/2

Determination of electron configurations based on principles:

1. Aufbau: Electrons occupy orbitals of the lowest energy level2 Hund: electron fills orbitals with the same energy level3. 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

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Keywords: electron transfer, quantum number, electron shell

I'm not sure but i will try to find out

the catch is that the top numbers are atomic masses the bottom numbers are the numbers of protons and electrons in an uncharged atom. they are the number of that atoms as you would find them on the periodic table. further, the numbers on the left are used to determine the missing numbers on the right

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer