Ionization Energy

[805594676]

Why do ionization energy and atomic radius have an inverse relationship?

[205793570]

he smaller the radius, the higher the ionization energy. This is because the electrons are being held in closer to the protons, which have opposing charges and therefore hold on to them, in an atom with a small radius.

[Charmaine Ho 2G]

Ionization energy is the energy required to remove an electron. The closer the electron is to the nucleus, the smaller the atomic radius is, and the more energy is required to remove it.

[Shannon Clark 1F]

The ionization energy is the energy need to remove an electron. It has an inverse relationship with atomic radius because the smaller the radius, the closer the electrons are held to the central atom. The pull is strong, so it would take more energy to remove an electron.

[Alison King 3L]

As atomic radius decreases, this means that the effective nuclear charge is increasing and thus electrons are being held more tightly by the atom. As a result, it is harder to remove these tightly held electrons and ionization energy increases.

[Katryn Heine 3A]

So ionization energy is the amount of energy required to remove the outermost electron from an atom. Atom with smaller atomic radius are more tightly bond and therefore it is harder to remove the outermost electron. Large atoms have more electron repulsion and are less tightly bound so it'll take less energy to remove the electron.

[905715668]

Ionization energy is the amount of energy needed to remove an e- from an atom. When an atom is larger, the valence electrons are held less tightly and thus easier to pull out of an atom's valence shell. The greater the atomic size the less energy is needed to remove an electron.

[305692127]

Why do ionization energy and atomic radius have an inverse relationship?

If you you think about it that way yes because the ionization energy increases as you move right and up the periodic table. Meanwhile the atomic radius moves down the periodic table and to the left.

[Sophia Dominguez 3I]

Ionization energy and atomic radius are inversely proportional because as the atomic radius increases, less ionization energy is required to remove an electron. When the atomic radius is smaller, the closer the electrons are to the central atom, requiring more ionization energy to remove the electron.

[Daniel Tabibian 3K]

The smaller the atomic radius, the closer the electrons are being held by the atom and the higher ionization energy it would take to remove them.

[Emma Goellner 2I]

The closer the electrons are being pulled in towards the positively charged nucleus, the harder they are to remove, and thus there is a higher ionization energy. The electrons have a stronger pull when the radius is smaller, because they are closer to the nucleus. When the radius is larger, the ionization energy is lower, since it is easier to remove an electron.

[Nathalia Garibay 1D]

this is from the textbook:
The first and second ionization energies of phosphorus, sulfur, and chlorine atoms are listed in the following table. Explain why the first ionization energies of phosphorus and sulfur are nearly the same, whereas the second ionization energy of sulfur is much greater than that of phosphorus.

How are first and second ionization energies different from each other? Why is the second ionization of sulfur much greater than that of phosphorous?

[705676154]

What is the trend for ionization energy.

[Matthew Nguyen 3G]

As the atomic radius decreases the amount of energy to remove the outermost electron or the ionization energy increases. This inverse relationship is due to the Atoms with a smaller atomic radius being more tightly bonded thus harder to break apart.

[Kelly McFarlane]

Ionization energy is the energy required to remove an electron so when the atom is large and the electrons are far from the nucleus, the ionization energy is small.

[Nataly Antonova 1B]

The smaller is the atom, the closer the electrons are to the nucleus and so are held more tightly (more difficult to remove). The bigger is the atom, the less attraction is experienced by the electrons (easier to remove).

[105605391]

The smaller the radius the stronger the nuclear charge is being felt by other species causing the atom to want to pull in more electrons and not want to give up any that it already has.