Effective Nuclear Charge

[radhika singh 1A]

I don't really understand why atomic radii decrease across a period due to effective nuclear charge. I understand that the number of electrons that stay shielded is constant across a period, but the protons increase, so wouldn't the nucleus increase as well?

This is kind of regards to achieve hw 2 #27. any clarification would be super helpful!

[Charlotte McDonough 2B]

With a larger nucleus/more protons, the attractive force between the electrons and the nucleus increases and thus the radius decreases :)

[Charlotte McDonough 2B]

more protons, higher effective nuclear charge and constant shielding ---> more attractive force pulling electron cloud in tighter ---> smaller atomic radius across a period.

[Stephen_Kim_1D]

The atomic radius measures the radius of the entire atom (nucleus and electrons combined), not just the radius of the nucleus. Although the nucleus is larger, the greater number of protons means there is a greater electrostatic force attracting the electrons to the nucleus, which decreases the atomic radius.

[005683006]

It increases across the period, thus the atomic radii of the elements decrease correspondingly as well

[Noa Popko 3I]

Across a period, the number of protons increases meaning there is a greater positive charge (effective nuclear charge) that can pull all the electrons in. Thus, the atomic radius decreases.

[Sidharth Paparaju 3B]

The nucleus is the tiny center, so it doesn't contribute much to the radii. However, since the number of protons increases, the attractive force increases, pulling the electrons closer to the nucleus--reducing the radii.

[Sidharth Paparaju 3B]

The nucleus is the tiny center, so it doesn't contribute much to the radii. However, since the number of protons increases, the attractive force increases, pulling the electrons closer to the nucleus--reducing the radii.