# How does coulombic attraction impact the atomic size?

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## What is coulombic attraction How does it relate to atoms?

Coulombic attraction is the attraction between oppositely charged particles. For example, the protons in the nucleus of an atom have attraction for the electrons surrounding the nucleus. This is because the pro- tons are positive and the electrons are negative. The attractive force can be weak or strong.

## How does Coulomb’s law relate to atomic radius?

Atomic radius increases from top to bottom within a group because: There is bigger distance between the protons in the nucleus and the outer electrons, decreasing the attraction forces according to Coulomb’s Law.

## How will that attraction affect the size of the atom’s radius?

The greater attraction draws the electrons closer to the protons, decreasing the size of the particle. Therefore, the atomic radius decreases. Down the groups, atomic radius increases. This is because there are more energy levels and therefore a greater distance between protons and electrons.

## How would you describe the coulombic attraction between the nucleus of the atom and the two electrons in the 4s sublevel?

How would you describe the Coulombic attraction between the nucleus of the atom and the two electrons in the 4s sublevel? The attractive force is equal for both electrons. … The attractive force between the valence electrons and the nucleus decreases.

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## How does coulombic force affect periodic trends?

The Coulombic attraction of the nucleus of an atom for its electrons is referred to as the electronegativity of the atom. Exercise 3 Within a given group (column) of the periodic table, the general trend is that the radii of the atoms increase as their atomic numbers .

## How does Coulomb’s law affect periodic trends?

8.6 Periodic Trends in the Size of Atoms

According to Coulomb’s Law, the attraction is stronger as the charge on the nucleus (Z) increases, and as the electron gets closer to the nucleus.

## How does Coulombic attractive forces affect ionization energy?

The greater the ionization energy, the more difficult it is to remove an electron. Using the same Coulombic attraction ideas, we can explain the first ionization energy trends on the periodic table. … The greater an atom’s electronegativity, the greater is its ability to attract electrons to itself.

## What factors affect the atomic size?

The actual trends that are observed with atomic size have to do with three factors. These factors are: the number of protons in the nucleus (called the nuclear charge). the number of energy levels holding electrons and the number of electrons in the outer energy level.

## What causes a larger atomic radius?

In general, atomic radius decreases across a period and increases down a group. … Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius.

## How does atomic size increase?

Summary: Atomic size increases as you go down a column because of the addition of another electron shell and electron shielding. Atomic size decreases as you go right across a row because of increased protons.

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