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The atomic radius actually decreases across a period because the number of protons increases. The increase in number of protons increases the nuclear charge (basically makes the positive charge in the nucleus more intense) and thus because of electrostatic attraction, the protons will pull in the electrons even closer, resulting in a smaller radius.
The atomic radii decreases because since there is more protons, there is a stronger pull on the electrons towards the nucleus. All of the elements in that period have the similar electron configurations so the added protons attract the electrons more, creating a smaller atomic radii.
Atomic radii decrease as you go across a period in the periodic table as the increased amount of protons in the nucleus has a stronger pull on the electrons. This stronger pull decreases the size of the radii by a very small, but quantifiable amount.
The atomic radii decrease as you go across a period because the increased number of protons has a greater effect on the electrons around it (essentially the more protons there are, the more they pull on the electrons to move closer in, thereby decreasing the atomic radii).
The atomic radii decrease even though the number of protons increases as the increase in protons increases the effective nuclear charge on the electrons in the atom and pulls them in closer. This decreases the atomic radius.
Since there are more protons across a period, there is a larger positive charge in the nucleus that will pull the electrons in closer to the nucleus. This results in a smaller radii as electrons are more tightly held which is why the atomic radii decreases across a period.
As we go across the period, the atomic radius decrease because protons will be added to the element/atom. As more protons increase the more positive the nuclear charge is. As a result, electrons will be closer to the nucleus resulting it to have a smaller radius.
Sophia Dinh 1D wrote:Why does atomic radii decrease even though the number of protons increase as you go across a period?
I agree with the previous responses! I wanted to add that, in general, electrons repel each other and are attracted to protons. Having more protons in the nucleus, and thus a higher/more positive charge, will draw electrons toward the nucleus and decrease the atomic radius. On the other hand, having more electron shells will cause electron-electron repulsion, which will make it easier to remove a valence electron. These rules play into a lot of periodic trends, so it's a good idea to familiarize yourself with them :) I hope this helps!
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