Answer:
A) The energy of a given orbital increases as the nuclear charge Z increases.
Explanation:
The energy of an orbital is as higher as the attraction force between protons and electrons is lower. So, as far as from nuclei, the orbital is more energetic. When Z increases, that means that the number of protons increases, so the attraction force increases, then the energy of a given orbital decrease.
Letter "b" is correct because of the Linus Pauling diagram in which the levels and sublevels are displaced to know its energy. The sublevel 3d is more energetic than the sublevel 4s, so it's necessary both quantum numbers.
Letter "c" is correct because the electrons at the same orbital have a greater repulsive force, so they can't shield electrons at the same orbital. But the inner electrons are attracted to the nuclei, so the repulsive force, plus the distance, will be less effective.
Letter "d" is correct because the penetration effect means the ability of an orbital to attract an electron. So, when the division in sublevels can explain that energy from the orbitals.
Letter "e" is correct because in the hydrogen atom there is only one orbital with one quantum number n and one quantum number l, which are n = 1, l = s, so the energy depends only on the quantum number n.
The statement that is not true about orbital energies is the energy of a given orbital increases as the nuclear charge Z increases.
The Orbital energy is the energy required by an Orbital to take an electron present in it to infinity or it is the energy released when there is addition of and electron the orbital from infinity.
The energy of the orbital depends on the values of both the principal quantum number (n) and the azimuthal quantum number (l).
Therefore, The statement that is not true about orbital energies is the energy of a given orbital increases as the nuclear charge Z increases.
Learn more about orbital energies here.
https://brainly.com/question/6202988.
