Question

For any electron, how do 1) electrons further than it & 2) electrons closer than it affect Zeff?

A) 1) Increase, 2) Decrease
B) 1) Decrease, 2) Increase
C) 1) Increase, 2) Increase
D) 1) Decrease, 2) Decrease

Answer 1

Electrons that are closer to the nucleus than the electron of interest decrease its effective nuclear charge through shielding, while electrons further away do not affect this shielding and thus do not increase the effective nuclear charge. The answer to how nearby and distant electrons affect Zeff is B) 1) Decrease, 2) Increase.

Step-by-step explanation:

The question you've asked pertains to how electrons closer or further from an electron of interest affect its effective nuclear charge (Zeff). Zeff is defined as the net positive charge experienced by an electron in a polyelectronic atom. The shielding effect plays a crucial role here.

Electrons that are closer to the nucleus than the electron of interest will shield the nuclear charge, thereby decreasing the Zeff experienced by that electron. On the other hand, electrons that are further away do not affect the shielding encountered by the electron of interest, and can't increase its Zeff. Therefore, the correct answer is B) 1) Decrease, 2) Increase.