Which of the electrons in the following orbitals will experience the greatest nuclear attraction?
1s electron of helium
1s electron of potassium
23 electron of boron
2s electron of carbon
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B.
in both He and K the 1s electron is located in the First shell, However while the the 1s electron of He is attracted by nuclear charge of 2 (atomic number), that of K is attracted by 19 (atomic number). according to Slater's rule, effective nuclear charge=nuclear charge -shielding constant. for any 1s electron, shieding constant = 0.3 no matter the element, therefore, effective nuclear charge for 1s electron of He = 2 - 2(0.3) = 1.4 while for K = 19 - 2(0.3) = 18.4. thus K(18.4) > He(1.4).
NOTE: The effective nuclear charge is the actual charge an electron experiences in an atom with multiple electrons.
Myschool is right, the correct answer is A. Because Helium has a small atomic radius, which means its 1s electron is closer to the nucleus, and even 1s electron is the only electron that Helium has, so it doesnt have to share the nuclear attraction with other electrons. In contrast, Potassium has a latrger atomic radius, so its 1s electron is farther from the nucleus and 1s electron shares the nuclear attraction with other 17 electrons. i hope this settles the case. Best regards @JOHNJESUS
@ 2stringS nuclear attraction (attraction between the Particles in nucleus and the electron in in orbit) is greater when the electron is closer to the nucleus and from the options above the 1s electron of helium is the closest to the nucleus putting into consideration atomic radius
in this case helium has a smaller atomic radius than potassium meaning there is an increased nuclear attraction than in potassium so helium os the ans
the greater the atomic radius the greater the nuclear attraction.going by periodic properties potassium has the greatest atomic radius among the listed options,so potassium should be the right answer
