Electron affinity is maximum in

The correct option is B Cl Electron gain enthalpy α 1 A t o m i c S i z e Electron gain enthalpy α Effective nuclear charge Electron Affinity term can also be used to measure the ability of an atom to gain an electron. If energy is released when an electron is added to an atom, the electron affinity is taken as positive, contrary to thermodynamic convention. Then, I > Br > Cl > F [Atomic Radius] ⇒ It should be F > Cl > Br > I [EA] But as we know, electron gain enthalpy α 1 A t o m i c S i z e Therefore, F > Cl, but, fluorine is very small, therefore electron density is high and an increased electronic repulsion makes the addition of an electron to fluorine less favorable than that in the case of chlorine. Therefore, the order will be Cl > F > Br > I [EA]. ⇒ Cl has maximum electron affinity. Q. Read the following questions for N, P, C, Si elements. (i) Element which has least atomic radii (ii) Element which has maximum ionization energy (iii) Element which has least electron affinity (iv) Element which has Maximum electronegativity Select the correct code of elements for given questions respectively.

Electron affinity is defined as the quantitative measurement of the energy change that results from adding a new electron to a neutral atom or molecule in the gaseous state. The more negative the electron affinity value, the higher an atom’s affinity for electrons.The energy of an atom is stated when an atom loses or gains energy through chemical reactions that cause the loss or gain of electrons. The reaction that releases energy is called an ‘exothermic’ reaction and the reaction in which energy is absorbed is called an ‘endothermic’ reaction. Talking about energies, energy from an endothermic reaction is positive. Hence, given a positive sign whereas energy from an exothermic reaction is negative. It is given a negative sign. The energy is released when an electron is being added to a neutral atom. Thus first electron affinities are always negative whereas second electron affinity ( electron to negative ion ) is positive. The electron affinity is further discussed below: First Electron Affinity Negative energy because energy is released. X(g) + e- —> X⁻ (g) Second Electron Affinity: Positive energy because the energy needed is more than gained. X⁻(g) + e- —> X²⁻ (g) First Electron Affinity: The energies are always concerned by the formation of positive ions. The first electron affinity is the energy released when 1 mole of gaseous atoms acquire an electron to form 1 mole of gaseous -1 ions. Example: The first electron affinity of chlorine is -349 kJ mol⁻¹ The energy is ...

The electron affinity increases on moving from left to right along a period. Arrange the reasons in a proper sequence. (a) The amount of energy released during the addition of an electrons increases from left to right along a period. (b) Effective nuclear charge of the elements increases from left to right. (c) The atomic size of the elements decreases from left to right. (d) The tendency to gain electrons and form anion increases from left to right.

Solution: Generally, electron affinity decreases down the group but increases in a period. However, the electronegativity of Cl is more than F because of the smaller size of F, due to which their is a greater repulsion between the incoming electron and electrons present in its valence shell. Hence, Cl has the maximum electron affinity among halogens.

\( \newcommand\) • • • • • \[\ce\): This version of the periodic table displays the electron affinity values (in kJ/mol) for selected elements.: As we might predict, it becomes easier to add an electron across a series of atoms as the effective nuclear charge of the atoms increases. We find, as we go from left to right across a period, EAs tend to become more negative. The exceptions found among the elements of group 2 (2A), group 15 (5A), and group 18 (8A) can be understood based on the electronic structure of these groups. The noble gases, group 18 (8A), have a completely filled shell and the incoming electron must be added to a higher n level, which is more difficult to do. Group 2 (2A) has a filled ns subshell, and so the next electron added goes into the higher energy np, so, again, the observed EA value is not as the trend would predict. Finally, group 15 (5A) has a half-filled np subshell and the next electron must be paired with an existing np electron. In all of these cases, the initial relative stability of the electron configuration disrupts the trend in EA. We also might expect the atom at the top of each group to have the largest EA; their first ionization potentials suggest that these atoms have the largest effective nuclear charges. However, as we move down a group, we see that the second element in the group most often has the greatest EA. The reduction of the EA of the first member can be attributed to the small size of the n = 2 shell and the resulting la...

Electronegativity: The term electronegativity was first introduced by the scientist named Jöns Jacob Berzelius in the year 1811. In the year 1932, after many discoveries and discussions, Linus Pauling first discovered the property of electronegativity completely and he also created an electronegative scale that depends on the bond enthalpy. This has further helped in establishing the The property of attracting a shared pair of electrons towards itself is known as electronegativity. In simple words, electronegativity is the property and the ability to gain electrons from an When the atomic number increases, it means that the distance between the nucleus and the valence electron also increases and hence, the electronegativity also rises. Therefore, the atomic number and the location of the electron from the nucleus play a very important role in determining the electronegativity and are the factors that are affecting it. Also, the tendency of attraction of electrons increases with the increase in the number of protons which increases with the increase in the nuclear charge. When the two electronegative atoms are taken, with the increase in the difference between the electronegativity of the atoms, the polarity of the bond between them also increases. The atom that has the more electronegativity will gain a negative charge on it. The electronegativity usually increases along a period from left to right and decreases on passing through a group that is from up to down. According...

Electron affinity is the energy change that results from adding an electron to a gaseous atom. For example, when a fluorine atom in the gaseous state gains an electron to form F⁻( g), the associated energy change is -328 kJ/mol. Because this value is negative (energy is released), we say that the electron affinity of fluorine is favorable. Created by Jay. My understanding is that the potential energy is released as a photon. (I actually spent some time trying to confirm this, but without finding a reliable source.) The electron's kinetic energy is apparently converted into thermal energy (i.e. heat). Radioactivity is a very different process (involving changes in the nucleus) and so I am almost completely certain that it is not relevant. Boron is a very unusual element, with complicated properties. That is why Boron is not usually studied at an introductory level. So, that is part of the issue. Unlike electronegativity, the electron affinity does not have a strong periodic value. The electron affinity measures the energy released when an electron is captured by the atom (or a molecule), forming an anion with a 1− charge. This is not necessarily directly related to the "willingness" for the element to actually acquire an electron when forming a compound (as measured by electronegativity). There is some correlation, of course, but it is not a strict correspondence. So, these are rather different situations. With electron affinity you expose the atom to a source of electrons ...

Learning Objectives • To master the concept of electron affinity as a measure of the energy required to add an electron to an atom or ion. • To recognize the inverse relationship of ionization energies and electron affinities The electron affinity (\(EA\)) of an element \(E\) is defined as the energy change that occurs when an electron is added to a gaseous atom or ion: \[ E_\): Electron Affinities (in kJ/mol) of the s-, p-, and d-Block Elements. The s blocks are purple, the p blocks are green, the d blocks are red, and the f blocks are blue. Electron affinity increases from left to right and bottom to top. Atoms with the largest radii, which have the lowest ionization energies (affinity for their own valence electrons), also have the lowest affinity for an added electron. There are, however, two major exceptions to this trend: • The electron affinities of elements B through F in the second row of the periodic table are less negative than those of the elements immediately below them in the third row. Apparently, the increased electron–electron repulsions experienced by electrons confined to the relatively small 2 p orbitals overcome the increased electron–nucleus attraction at short nuclear distances. Fluorine, therefore, has a lower affinity for an added electron than does chlorine. Consequently, the elements of the third row ( n = 3) have the most negative electron affinities. Farther down a column, the attraction for an added electron decreases because the electron is e...