Which explains the change in ionization energy that occurs between removing the first and second electrons from an atom?

AThe ionization energy decreases because the ratio of the protons to electrons increases.
BThe ionization energy increases because the ratio of the protons to electrons increases.
CThe ionization energy decreases because the ratio of the protons to electrons decreases.d)The ionization energy increases because the ratio of the protons to electrons decreases.

Question

maduAntinn maduAntinn

19-05-2016
Chemistry

Answered

Which explains the change in ionization energy that occurs between removing the first and second electrons from an atom?

AThe ionization energy decreases because the ratio of the protons to electrons increases.
BThe ionization energy increases because the ratio of the protons to electrons increases.
CThe ionization energy decreases because the ratio of the protons to electrons decreases.d)The ionization energy increases because the ratio of the protons to electrons decreases.

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Anonymous Anonymous · Answer 1 · 2016-05-26T06:58:05-04:00

The change in ionization energy that occurs between removing the first and second electrons from an atom is best described by b. The ionization energy increases because the ratio of the protons to electrons increases. Removing electrons from an atom makes it more positive, making the attractive forces between protons and neutrons stronger. This makes it harder to remove the succeeding electrons, resulting to a higher ionization energy.

AarushiAanand AarushiAanand · Answer 2 · 2022-06-15T14:36:44-04:00

The first and second electrons from an atom can be explained by "the ionization energy decreases because the ratio of the protons to electrons increases."

What is ionization energy?

Ionizations energy, also referred as ionization potential, is the amount of energy necessary to remove an electron from an isolated atom or molecule.

What is electrons?

The electron is just a subatomic particle with a negatively fundamental charged. Consider the nuclear charge of the atom to understand this. The greater the number of protons in the nucleus, the stronger the nucleus's attraction to electrons. This increased affinity makes removing electrons more challenging. The ionization energy reduces within a group as the atom size increases.

The ionization energy falls as the proton-to-electron ratio grows. When electrons are removed from an atom, it becomes more positive, increasing the attraction interactions between protons and neutrons. This makes removing the succeeding electrons more difficult, resulting in a larger ionization energy.

Hence the correct option is a.

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