What happens to force of attraction down a group?

How does coulombic attraction change as you move down a group?

The bigger the size of the atom, the electrons, especially the valence electrons are further away from the nucleus. The nucleus is not able to pull the electrons, that are in orbitals further away from the nucleus, towards itself and the coulombic attraction decreases.

What happens to the force of attraction as you go down a column on the periodic table?

Ans: As you go down a column, the valence electrons are on levels that are further away from the nucleus. According to Coulomb’s law, the further the distance, the less force holding the electrons, so they are easier to lose. … The closer an electron is to the nucleus, the more energy required to remove it from the atom.

Does force of attraction decrease across a period?

Since the force of attraction between nuclei and electrons increases, the size of the atoms decreases. The effect lessens as one moves further to the right in a period because of electron-electron repulsions that would otherwise cause the atom’s size to increase.

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What happens to force of attraction as the atoms increase in size down a group?

Down a group, the number of energy levels (n) increases, and so does the distance between the nucleus and the outermost orbital. The increased distance and the increased shielding weaken the nuclear attraction, and so an atom can’t attract electrons as strongly.

How does the attractive force between the outermost electron and the nucleus change?

As you move from the smallest atom to the largest atom in Model 2, how does the distance between the outermost electron and the nucleus change? The outermost electron is further away in the larger atom. 9. … As more protons are added, the attractive force on the electron increases.

Why does the force of attraction between the nucleus and electrons decrease down a group?

The electrostatic attraction between nucleus and valence electrons is weaker and results in less energy needed to remove an electron from the outermost shell. Therefore a decrease in IE down a group.

What variables will affect the force of attraction between charged particles?

In an atom, the most important factors that influence the force, as calculated by Coulomb’s equation, are the nuclear charge and the distance from the nucleus to the electron of interest. The closer an electron is to a nucleus, the stronger the attractive force (i.e. the more negative F becomes).

Why do valence electrons decrease down a group?

What happens to the number of valence electrons as you go across a period? Number of valence electrons increases. … Decreases as you go down a group because electrons are close to the nucleus in smaller atoms making the attraction stronger.

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Why does reactivity decrease across a period?

Period – reactivity decreases as you go from left to right across a period. The farther to the left and down the periodic chart you go, the easier it is for electrons to be given or taken away, resulting in higher reactivity. … Group – reactivity decreases as you go down the group.