Question

Help does anyone know this?

This is explained by the fact that at the top of the group, atoms are so the positive charge of the nucleus will be closer to any the atom may encounter as it seeks to fill its outer shell. This means the electrostatic force of between nucleus and electron will be greater. Additionally, for a smaller atom, there will be fewer inner shells of electrons to repel an incoming electron

Answer 1

Smaller for the first one

Electron for the second on

and Attract for the third one

Answer 2

Answers in order:

smaller

electron

attraction

Step-by-step explanation:

ok so we know that a positive proton attracts the negative electron and we know that protons, neutrons are found in nucleus while the electron orbits around it.

now let's imagine an atom, could you say that with the increasing number of protons as you go down the elements of the periodic table that there is also an increasing positive charge in the nucleus?

and we know that in elements the protons and electrons are equal since they attract each other and hence the element is neutral in charge.

Now let's imagine that larger size of positive charge versus the electrons in many shells orbit.

we know that there is a specific amount of electrons per each shell, but particularly the group 17 elements, their outer shell has 17 valence electrons.

Now could we also say that having such a high number of electron in their valence shell also mean that there is a great negative charge especially in that outer shell.

so now let's imagine, both these great negative and positive charges attracting eachother, wouldn't this attraction be more stronger as compared to lower positive and negative charge? Yes

Knowing this, we can explain the reason for the actual size of the entire atom, the shells are much closer together to the nucleus due to those forces of attraction hence the atomic radii is smaller. This is also why elements with a larger number of valence electrons tend to accept electrons rather than donate.

Also know that atomic radii increase going across a period from left to right, and decrease going down a group