An electron in a(n) __________ subshell experiences the greatest effective nuclear charge in a many-electron atom. Question 18 options:
a) 4f
b) 4p
c) 4d
d) 4s
e) 5s
is the correct answer d)?
Yes, the correct answer is d) 4s.
In many-electron atoms, the effective nuclear charge experienced by an electron depends on its energy level and subshell. The effective nuclear charge increases across a period in the periodic table, meaning that the electrons in the inner shells shield the outer electrons from the full positive charge of the nucleus.
The 4s subshell is closer to the nucleus than the other subshells listed in the options, so the effective nuclear charge experienced by the electron in the 4s subshell is the greatest. Therefore, the electron in the 4s subshell experiences the greatest effective nuclear charge in a many-electron atom.
The correct answer is actually e) 5s.
In a many-electron atom, the subshells are filled in a specific order according to the aufbau principle, which states that electrons fill orbitals starting from the lowest energy level subshell to the highest.
The subshells are filled in the order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, etc.
As we move across periods in the periodic table, from left to right, the effective nuclear charge experienced by an electron in a subshell increases. This is because as the number of protons in the nucleus increases, the positive charge of the nucleus also increases, pulling the electrons closer and increasing the attraction.
In this case, the electron in the 5s subshell experiences the greatest effective nuclear charge in a many-electron atom. So, the correct answer is e) 5s.
To determine which subshell experiences the greatest effective nuclear charge in a many-electron atom, we need to consider the concept of shielding. Shielding occurs when inner-shell electrons repel outer-shell electrons, reducing the attractive force between the nucleus and the outer-shell electrons.
In general, electrons further away from the nucleus experience less effective nuclear charge because they are shielded by inner electrons. The order of the subshells from closest to furthest away from the nucleus is: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, and so on.
In this question, we are comparing the 4s, 4p, 4d, and 5s subshells.
The 4s subshell is closer to the nucleus than the 4p and 4d subshells. However, a 4s electron is shielded by the 3s and 3p electrons, which reduce the effective nuclear charge it experiences.
On the other hand, the 4p and 4d subshells are further away from the nucleus, but they are less shielded by inner electrons. Therefore, electrons in the 4p or 4d subshells experience a greater effective nuclear charge than an electron in the 4s subshell.
Therefore, the correct answer is not d) 4s. To determine the correct answer, we need to compare the 4p, 4d, and 5s subshells. Since the 5s subshell is further away from the nucleus than the 4p and 4d subshells, it experiences less effective nuclear charge due to shielding.
Thus, the correct answer is e) 5s.