Hence, the incoming electron is not accepted with the same ease as is the case with chlorine. 23. However, when we add the second electron to the negatively charged ion, this addition of electron will be strongly opposed due to the coulomb forces of repulsion. Atomic and Physical Properties and Their Trends Atomic and Ionic Radii . Explain why second or higher electron gain enthalpy will have positive value. The concept of atom efficiency has proven to be a popular tool in the evaluation of the “greenness” of a chemical process [1], which revealed a comparison between various sectors of chemical manufacturing.In pharmaceutical and fine chemicals manufacturing, the high value of the product has been particularly a significant feature in the establishment of many highly (atom) inefficient processes. 1 answer. Students can solve NCERT Class 12 Chemistry The p-Block Elements MCQs Pdf with Answers to know their preparation […] As we move down the group, the outer electrons, which are to be removed, are farther from the nucleus and there is an increasing screening of the nuclear charge by the electrons in the inner shells. Check important questions and answers for Class 12 Chemistry Board Exam 2020 from Chapter 7 - The p-Block Elements. 27. This is due to the fact that group 15 element have extra stable half-filled p orbitals electronic configurations. Therefore, the electron gain enthalpy of such elements is substantially large in value. The atoms of group 17 elements are only one electron short of attaining stable noble gas configurations. sehgalmilan29 sehgalmilan29 4 hours ago Chemistry Secondary School +6 pts. Therefore, the latter two factors more than compensate for the less negative electron gain enthalpy of fluorine. However, the bond dissociation energy of fluorine is much lesser than that of chlorine. This is because of increasing in size from F to I. Why? Electron Gain Enthalpy H 2S is less acidic than H 2Te. How much energy in kJ is released when 17.5 g of chlorine is completely . The electron gain enthalpy of an atom can be considered as a measure to gain an electron and form an anion. Ionisation enthalpy: Ionisation enthalpy of elements of group 16 is lower than group 15 due to half filled p-orbitals in group 15 which are more stable. The electron gain enthalpy of chlorine is more negative than that of fluorine. Group 13 is the first group to span the dividing line between metals and nonmetals, so its chemistry is more diverse than that of groups 1 and 2, which include only metallic elements. These questions are based on the latest CBSE Class 12 Chemistry Syllabus. Log in. Electron Affinity of Lithium is 59.6 kJ/mol. Elements of groups 16 and 17 have more negative values of electron gain enthalpies hence they have a tendency to form ionic compounds. Ionization Enthalpy. Electron Affinity. The elements of the second period have the smallest atomic size among the elements in their respective group. When a single electron is added to a gaseous atom, it forms a monovalent anion and the enthalpy released is called the first electron gain enthalpy. However, the element of group 16 has lower ionisation enthalpy values as compared to those of group 15 in the corresponding periods. But the element Ga has ten 3d electrons present in the 3d sub-shell which do not screen as much as is done by s and p electrons. asked Aug 30, 2018 in Chemistry by Sagarmatha (54.4k points) the p block … When a single electron is added to a gaseous atom, it forms a monovalent anion and the enthalpy released is called the first electron gain enthalpy. However F has less electron gain enthalpy than Cl due to its small size and high electron density. In other words, the neutral atom's likelihood of gaining an electron. Step 3: (For the shielding experienced by d- or f- electron): all other electrons in the (ns, np) group contribute shielding to the extent of 0.35 each to the screening constant. this is because,as we go down the group both atomic size and nuclear charge increases,but the effect of atomic size is more prominent than that of nuclear charge. This is due to the fact that group 15 element have extra stable half-filled p orbitals electronic configurations. Chemistry MCQs for Class 12 Chapter Wise with Answers PDF Download was Prepared Based on Latest Exam Pattern. This is on the grounds that Oxygen, because of its compressed nature encounter more repulsion between the electrons effectively present and the approaching electron. Ionization energy: If we compare ionization energy of group 17 and group 16 we see that group 17 has higher energy than group 16 because of smaller size of group 17 elements. Electronegativity of Lithium is 0.98. Group 16 elements have 6 electrons in their valence shell and their general electronic configuration is ns 2 np 4. Solution. It is due to increase in size. Ionisation enthalpy decrease down the group. Electron Gain Enthalpy. (i) Al has lower ionization enthalpy than B due to larger size. give reasons. Element: Electronic Configuration: Oxygen [He] 2s 2 2p 4: Sulphur [Ne] 3s 2 3p 4: Selenium [Ar] 3d 10 4s 2 4p 4: Tellurium [Kr] 4d 10 5s 2 5p 4: Polonium [Xe] 4f 14 5d 10 6s 2 6p 4: Atomic and Physical Properties and the Trends of Group 16 elements. Because of this, the electron-electron repulsions in 2p sub-shell are quite high. Elements of Group 16 generally show lower value of first ionisation enthalpy compared to the corresponding periods of group 15. Among all the elements which one has the highest value of electronegativity? The electron gain enthalpy of fluorine is less negative than chlorine owing to a smaller size where the electron-electron repulsion is comparatively smaller. Ionization enthalpy decreases with increase in size of the central atom as we move down. The repulsive forces between electrons imply low negative electron gain enthalpy value. Electron Affinity and Electronegativity of Lithium. Electron Gain Enthalpy of Halogen Family. The value of electron gain enthalpy with negative sign for sulphur is higher than that for oxygen . Ask your question. Ans: Due to extra stable half-filled p orbital electronic configurations of Group 15 elements, larger amount of energy is required to remove electrons compared to Group 16 elements. All alkali metals have negative electron gain enthalpy. Question Papers 172. Thus, these elements have a maximum negative electron gain enthalpy in the corresponding periods. Therefore the incoming electron is not accepted with the same ease as in the case of chlorine which the atomic size is bigger (atomic radius 99 pm) and the electron crowding is comparatively less. However, ionization enthalpy decreases down the group. Electron gain enthalpy becomes less negative as we move down the group. 1 answer. Electron affinity (data page) Jump to navigation Jump to search This page deals with the electron affinity as a ... 16 O Oxygen: 1.461 113 6(9) 140.976 0(2) 8 17 O Oxygen: 1.461 108 (4) 140.975 5(3) 8 18 O Oxygen: 1.461 105(3) 140.975 2(3) 9: F: Fluorine: 3.401 189 8(24) 328.164 9(3) 10: Ne: Neon-1.2(2)-116(19) est. Ionisation of sodium(or any atom) is endothermic process (495.8 KJ/mol), meaning, in isolated gaseous state, neutral atom is more stable, Electron gain process of Na+ is obviously an exothermic process (reverse of ionisation) due to attraction of Positively charged, Na+ for a free electron. Log in. Fig. 24th September 2018 12:09 PM Answered by Expert Variation in electron gain enthalpies across the period (2 nd period) and down the group (16 th and 17 th group) Anomalous behaviour down the group: Electron gain enthalpy of O (-141 kJ/mol) is less negative than that of S (-200 kJ/mol) and the electron gain enthalpy of F (-328 kJ/mol) is less negative than that of Cl (-349 kJ/mol). The reason for that, the atomic size of oxygen is quite small. Also, because of its small size, the hydration energy of fluorine is much higher than that of chlorine. Generally the first ionization enthalpy decreases down a group in the periodic table. Elements of Group 16 generally show lower value of first ionization enthalpy compared to the corresponding periods of group 15. All the electrons in a group lying left of (nd, nf) group contribute 1.0 each to the screening effect. The electron gain enthalpy of groups 16 and 17 varies to become less negative as you move down a group, because of the change in the atomic size, nuclear charge. why 15 group low velctron gain enthalpy than 16 group Asked by kunalkumarshah123456! Share with your friends. Why? In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as:. Ask your question. Join now. note that for 1s this value is 0.30. The higher the energy released during this process, the easier will be the formation of an anion. The electron gain enthalpy of chlorine is 348 kJ mol^-1 . Electron gain enthalpy of chlorine is more negative as compared to fluorine. However, the element of this group has lower ionisation enthalpy values compared to those of group 15 in the corresponding periods. Electron Gain Enthalpy in Period and Group. Why? The value of electron gain enthalpy of {eq}Na^+ {/eq} will be (1) 5.1 eV (2) 10.2 eV (3) + 2.55 eV (4) 2.55 eV. Join now. In periodic table, down in the group means from "top to bottom", the electron gain enthalpy becomes "less negative". the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion. 3: Electronic Configuration of Group 16 Elements. The first ionisation enthalpy values (kJ mol-1) of group 13 elements are : How would you account for their deviation from the general trend ? Comparing Group 16 and Group 17 values; Second Electron Affinity; Practice Problems ; Answers; References; Contributors and Attributions; Electron affinity is defined as the change in energy (in kJ/mole) of a neutral atom (in the gaseous phase) when an electron is added to the atom to form a negative ion. (ii) Ga has slightly higher ionization enthalpy than Al due to ineffective shielding by 3d electrons. asked May 27 , 2019 in Chemistry by AashiK (75.6k points) p-block element; class-12; 0 votes. Except for the lightest element (boron), the group 13 elements are all relatively electropositive; that is, they tend to lose electrons in chemical reactions rather than gain them. Click here to get an answer to your question ️ explain changes of value of electron gain enthalpy of period and groups 1. Electron Gain Enthalpy: The electron gain enthalpy decreases with increase in the size of the central atom moving down the group.Oxygen molecule has a less negative electron gain enthalpy than sulfur. Answer: The decrease in ∆ i H 1 value from B to Al is quite expected because of the bigger size of Al atom. 1. Electron gain enthalpy: Along period it is more negative because of attraction towards electron as of increased nuclear charge. Consequently the removal of electrons becomes easier down the group. Free PDF Download of CBSE Chemistry Multiple Choice Questions for Class 12 with Answers Chapter 7 The p-Block Elements. Explain why second or higher electron gain enthalpy will have positive value. Electron gain enthalpy: Oxygen has less negative electron gain enthalpy than S because of small size of O. asked Sep 26, 2020 in Periodic Classification of Elements by Manish01 (47.5k points) periodic classification of elements; class-11; 0 votes. Share 6. Textbook Solutions 8602. The first ionization enthalpy values (in kJ mol-1) of group 13 elements are : B Al Ga In Tl 801 577 579 558 589 How would you explain this deviation from the general trend? Which of the following has highest electron gain enthalpy? The atomic and ionic radius increasesas we move from oxygen to polonium. "Electron gain enthalpy" is termed as the energy change when we add "electron to the valence shell" to a gaseous atom which is neutral. The negative electron gain enthalpies are large for elements of group 16.
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