N + e â â N â â âH = Affinity = 7 kJ/mol. Electron affinity is the attraction a neutral atom has for a non-bonding electron. Question: Of The Group 15 Elements On The Periodic Table (periods 2 Through 6), Select The Element With The Greatest Electron Affinity, The Smallest Atomic Radius, And The Largest Ionic Radius According To Periodic Trends. Electron affinities are given in kj/mol (joules per mole), a measurement of given energy per amount of material. Electron affinity decreases or increases across a ⦠Data taken from John Emsley, The Elements, 3rd edition.Oxford: Clarendon Press, 1998. There are also increasing numbers of electrons between the nucleus and those outer electrons. An electron affinity > 0 indicates that the negative ion is higher in energy than the separated atom and electron. A negative electron affinity means energy must be input in order to attach an electron to the ion. Solution. Absorbing an additional electron requires energy because a negatively charged particle is not naturally attracting to a neutral atom. The value may be either positive or negative. The electron affinity of an element is the energy change which accompanies the addition of an electron to an atom in the gas phase to produce a negatively charged anion:. The first electron affinity is always exothermic that is negative the second electron affinity of the same element will be positive or endothermic. Nitrogen having a lower electron affinity compared to oxygen actually follows the periodic trend! This is because going from left to right and bottom to top, the atomic radius decreases so it is easier for the nucleus to attract negative electrons. (a) Define the term electron affinity. Thus, electron affinity decreases down the group. Ionisation paotential and electron affinity of fluorine are `17.42` and `3.45eV` respectively .Calculate the electronegativity of fluorine on Mulliken scale and Pauling scale . THe electron affinity is the nergy required to detach an electron from the singly charged negative ion (energy for the process X -> X + e). Electron affinity of group 15 i.e. Electron affinities are measured in the gaseous state. Check Answer and Solution for above question from Chemistry in Class And the added electron will have to go to the n-p orbital of higher energy. Because this value is negative (energy is released), we say that the electron affinity of fluorine is favorable. The general trend for electron affinity down the group is that it decreases because of the increase in atomic radius.The exception of $\ce{Cl}>\ce{F}$, I can understand is because fluorine has a high electron density and it is unfavourable to add more electrons as it would only increase the electron -electron repulsion. Second electron affinity. The halogens are a group of elements who share the property of needing a single electron to become stable. Following the trend, one would expect carbon to have a lower electron affinity than nitrogen. Madhya Pradesh PMT 1998: The correct order of electron affinity of B, C, N, O is (A) O > C > N > B (B) B > N > C > O (C) O > C > B > N (D) O > B > C > That means that the electrons occupying the most outlying orbitals are farther away from the nucleus. The first electron affinity is the energy released when 1 mole of gaseous atoms each acquire an electron to form 1 mole of gaseous 1- ⦠Electron affinity is the energy change that results from adding an electron to a gaseous atom. -15-121 +31-142 â333 +99: The exception mentioned above can be readily explained. The electron affinity cannot be determined directly but is obtained indirectly from the Born-Haber cycle. #Delta"E"# is negative, the electron affinity will be positive.. Electron affinity follows a trend on the periodic table. Defining first electron affinity. Name the elements which do not follow the trend in this period. CS â, CSe â, SiO â, and GeO â are found to support dipole-bound anion states with electron affinities on the order of 0.01 eV. The equivalent more common definition is the energy released (E initial + E final) when an additional electron is attached to a neutral atom or molecule. X(g) + e- ® X-(g) The electron affinity for elements in Group 15 is much lower than elements in Group 14, 16, or 17 because elements in Group 15 have a half filled p subshell which is more stable than having an electron in Px, Py but not Pz orbital, or having not a full 6 electron p subshell. Arrange the following in the decreasing order of electron affinity: B, C, N, O. As for example the electron affinity of oxygen to add two electrons are: O (g) + e â â O â (g) EA 1 = -142 Kj mol-1 The change is small and there are many exceptions. The addition of an electron makes for a more unfavorable change; therefore, the electron affinity is lower in group 15 when compared to group 14. It increases moving down a column or group and also increases moving from left to right across a row or period (except for the noble gases). As the principal quantum number increases, the size of the orbital increases and the affinity for the electron is less. This is so because the second electron has to be forced to enter the mono negative ion. Helium is a member of this block. So in Group 15 elements as you would move down a group, starting with the lightest element and finishing with the heavy ones; youâd notice a general flow in properties as you move down the order. Here are the electron affinities of the 16th and 17th groups. Electronic Configuration of p-block Elements. When halogens get electrons they give up energy. 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