Why does the distance between the valence shell and nucleus decrease as there are more protons?

A higher effective nuclear charge causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius. Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital.

Why does the distance between energy levels decrease?

The further away an electron is from the nucleus, the less force it feels from the electron, so the less energy is needed to “pop it off” the atom. The value of the energy level is exactly this amount of energy, so the smaller it is, the smaller the difference with neighboring levels will be.

What happens when you move further away from the nucleus of an atom?

Electrons further away from the nucleus will have higher energy. An atom’s electron shell can accommodate 2n2 electrons (where n is the shell level). In a more realistic model, electrons move in atomic orbitals, or subshells. An electron will move to the orbital with lowest energy.

What happens to the distance between consecutive Bohr’s orbit as we move away from the nucleus?

Energy of orbit decreases as we move away from nucleus because orbit closer to nucleus are attracted towards nucleus, as nucleus posses positive charge and electron posses negative charge. As we move further from nucleus the attraction between the outer orbital and nucleus decreases.

What happens as the distance of the shells start increasing from the nucleus?

Explanation: As the electron goes far from the nucleus, the nuclear force of attraction on the electron decreases. As a result, the electron revolves around with lesser velocities. Therefore, the total energy of the electron increases with increase in distance from the nucleus.

Why does the energy of an electron increase as it moves to shells that are farther from the nucleus?

The nucleus and electrons have opposite charge and are attracted (with a force, just like gravity.) Thus, the further you pull the electron and the nucleus apart, the more energy you put into the system.

What can affect the distance between the nucleus and the electrons?

The greater attraction between the increased number of protons (increased nuclear charge) and electrons, pulls the electrons closer together, hence the smaller size. As you move down a group in the periodic table, the covalent radius increases. Atoms increase in size.

How does the distance between adjacent orbits in a hydrogen atom vary with increasing values of the orbital number N?

The distance difference between adjacent orbit radii remains constant with increasing values of the principal quantum number. The distance difference between adjacent orbit radii decreases with increasing values of the principal quantum number. Consider the hydrogen atom.

What determines the distance of the electrons from the nucleus?

In an atom, an electron is attracted to the nucleus by the “electromagnetic force”, similar to your rubber band. Like your baseball, the faster the electron goes, the farther away from the nucleus it is. The electrons in an atom are moving pretty fast, so they are far away from the nucleus.

What causes an electron distance from the nucleus to increase?

The energy of electrons increases with distance from the nucleus because electrons have an attractive force towards the nucleus, so the farther away…