The most negative electron affinity is most likely associated with which type of atoms?

large nonmetal atoms
small nonmetal atoms
large metal atoms
small metal atoms

The most negative electron affinity is most likely associated with small nonmetal atoms

Elements based on electrical conductivity can be divided into two elements, namely metal elements (conductors) and non-metals (non-conductors/insulators)

In modern periodic systems, the metal element is generally located on the left while the non-metal is on the right. So that from left to right the metal's properties are reduced, and in one group from top to bottom the metal's properties are getting bigger

While in one group the atomic radius increases from top to bottom and in one period from left to right the radius of the atom decrease. So that the size of the elements getting smaller from right to left and getting bigger from top to bottom

Electron affinity indicates the energy released if an atom attracts electrons. The greater the energy released (negative value), the greater the tendency of the atom to attract electrons and become negative ions

In one group, electron affinity tends to decrease from top to bottom, whereas in one period, from left to right, affinity tends to increase

From the above statement, it can be concluded that the largest electron affinity (the most negative) is owned by the elements located on the upper right in the period system, namely the element F- or Cl- which is a non-metallic element and is small in size (the radius of the atom is small)

the element would most likely have an electron affinity

Ionization energy and electron affinity

the trend in electron affinity

Keywords: electron affinity, periodic system, atomic radius, metal, nonmetal

The most negative electron affinity is most likely associated with small nonmetal atoms.

Further explanation:

Electron affinity:

Electron affinity is the release of energy when an electron is added to a neutral atom to form an anion. Greater the energy released, greater will be the ability of neutral atom to attract electrons and become negatively charged.

The reaction for electron affinity is as follows

Here, X is a neutral atom.

Electron affinity depends upon the size of atom. More the size less will be the attraction to the nucleus as the distance between the nucleus and outermost electron will be more.

As we move down the group, as atomic radius increases from top to bottom, the attraction of electrons to the nucleus will be less resulting in decrease electron affinity.

As we move along the period, as the atomic radius decreases from left to right, the attraction of electrons to the nucleus will be more and hence electron affinity will increase.

Electrons affinity increases from metal to nonmetal as metal is on the left side of the periodic table while nonmetals are present on the right side of the periodic table.

Large nonmetal has electron affinity more than metal because of the small size of nonmetals as compared to metals. On the other hand, large nonmetals are large in size as compared to small nonmetal and therefore has less electron affinity compared to small nonmetal.

Small nonmetal has large electron affinity than metal because of the small size of nonmetals as compared to metals. On the other hand, small nonmetals are small in size as compared to large nonmetal and therefore has more electron affinity compared to large nonmetal.

Large metals lie on the left side of the periodic table and have small size and therefore less negative electron affinity as compared to nonmetals. While the large metals are large in size as compared to small metal and therefore has less electron affinity compared to small metal.

Small metals lie on the left side of the periodic table and have small size and therefore less negative electron affinity as compared to nonmetals. While the small metals are small in size as compared to large metal and therefore has more electron affinity compared to large metal.

Therefore, small nonmetals have most negative electron affinity.

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Answer details

Grade: High school

Subject: Chemistry

Chapter: Periodic properties

Keywords: Electron affinity, metals, nonmetals, group, period, increases, decreases valence electrons, and size.