4compared to the energy and charge of the electrons in the first shell of a be atom, the electrons in the second shell of this atom have
(1) less energy and the same charge
(2) less energy and a different charge
(3) more energy and the same charge
(4) more energy and a different charge

The electrons in the second shell of this atom have (3) more energy and the same charge compared to the first shell

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 shell at the lowest energy level starting from the shell 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:

Rh = constant 2.179.10⁻¹⁸ J

So the electron transfer energy (ΔE)

ΔE = E end - E initial

From the electron transfer available, because the value of the Rh constant is the same, the effect is the value of n (shell) ⇒ 1 / n²

Electron configuration of Be (Beryllium) with atomic number 4

1s² 2s² or [He] 2s²

So in the first shell E = -1(n=1), the second shell E = -1/4 (n=2)

So the energy value in the second shell is greater than the first shell

While the electron charge is still the same(-1) (such as protons with + charges and neutrons with neutral charges / 0)

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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the answer would be c