Why does Li have a greater electron affinity than be?

Therefore, lithium has an incompletely filled 2s subshell while beryllium has a filled subshell. Lithium can affinity to receive electrons in 2s sub-shell but for beryllium, a still higher energy 2p level. Hence beryllium resists to gaining extra electrons in higher energy levels or 2p orbitals.

Why does lithium have higher electron affinity than sodium?

Because the attraction between that electron and its nucleus is less because it’s a larger atom. So smaller atoms generally are going to have more electron affinity. Which is why lithium has more electron affinity than sodium.

Why is electron affinity of phosphorus greater than nitrogen?

This means phosphorus has more occupied electron shells than nitrogen. So nitrogen will have a smaller atomic radius. This means the electrons are closer together. So, the reason that the change in energy for both electron affinities is lower for atoms of phosphorus than for atoms of nitrogen is answer choice (B).

Why do some atoms have a greater electron affinity than others?

Answers. Energy is released when a electron is added to a nonmetal. Nonmetals have a greater electron affinity than metals because their atomic structure allows them to gain electrons rather than lose them.

Which element has the smallest electron affinity?

mercury
What is the lowest electron affinity? Metals are more likely to lose electrons than they are to gain them. Of the metals, mercury has the lowest electron affinity.

Why does phosphorus have a negative electron affinity?

Phosphorus will have a less negative Eeas because P has an electronic configuration in which the 3p orbital is half filled, a very favorable configuration. Adding an electron will disrupt this half filled configuration. The elements on either side of P, Si and S , do not have this electronic configuration.

Why does nitrogen have less electron gain enthalpy than phosphorus?

N2 is less reactive than P4 due to high value of bond dissociation energy which is due to presence of triple bond between two N2 atoms of Ng molecule.

Why does electron affinity increase across a period and decrease down a group?

This is because as you go down the period table, new valence shells are added increasing the atomic radius. The new orbital is further away from the nucleus, meaning the attraction between the positively charged nucleus and the new electron decrease. Thus, electron affinity decreases.

Which of the following has the most negative electron affinity value greatest affinity to electrons?

This means Cl has the highest/most negative electron affinity.

What does it mean when electron affinity is negative?

This means that if energy is released when an atom is added to the atom, i.e. ΔE is negative, the electron affinity will be positive. Likewise, if energy is required to add an electron to an atom, i.e. ΔE is positive, then electron affinity will be negative.

How does effective nuclear charge affect electron affinity?

It goes without saying that the higher the effective nuclear charge, the more attracted to the nucleus an incoming electron will be, and the more negative the electron affinity of the atom will be. Now, what happens when you need energy to add an electron to an atom?

Why does sodium have a higher electron affinity than Al?

Aspects of Sarthak Srivastava’s answer are correct, however, sodium does have a higher electron affinity than Al. What influences electron affinity is the stability of the electron in its new position.

Why does oxygen have a higher electron affinity than nitrogen?

In case of Nitrogen (7) and Oxygen (8) ……the oxygen atom have more attracting power of electrons towards its nucleus than nitrogen, so, it will be more electron affinity than nitrogen. And the second factor is electronic state as oxygen have two p…