Correct order of electron affinity
WebJan 15, 2024 · Electron affinity, often abbreviated as EA, is the energy released when an electron is added to a valence shell of the atom. F (g) + e- -> F-(g) EA = -328 kJ/mol [When an electron is added to an atom, energy is given off. This process is exothermic. ] The electron affinity (Eea) of an atom or molecule is defined as the amount of energy released when an electron attaches to a neutral atom or molecule in the gaseous state to form an anion. X(g) + e → X (g) + energy This is not the same as the enthalpy change of electron capture ionization, which is defined as negative when energy is released. In other words, the enthalpy change and the electron affinity …
Correct order of electron affinity
Did you know?
WebCorrect option is D) The correct order of electron affinity is Cl>F>O. On moving from left to right across a period, the electron affinity becomes more negative. On moving from … WebSelect the clement you would expect to have the greatest electron affinity. Show transcribed image text Best Answer 100% (10 ratings) a) K (48)
WebJan 8, 2016 · Electron affinity is defined as. The amount of energy released when an electron is added to a neutral atom to form an anion. … WebThe correct order of electron affinity among the following is: A Se>O B P >N C Cl>F D All of the above Solution The correct option is D All of the above The electron affinity generally decreases down the group. However, due to the small sizes of O, N and F, their electronaffinities will be less than expected. Hence all of the above are correct.
WebApr 25, 2024 · The correct order of electron affinity is: WebElectron affinity can be defined in two equivalent ways. First, as the energy that is released by adding an electron to an isolated gaseous atom. The second (reverse) definition is that electron affinity is the energy required to remove an electron from a singly charged gaseous negative ion. The latter can be regarded as the ionization energy ...
Web1. odd number of electrons 2. octet deficient molecules (B, Al) 3. valence shell expansion (elements with n greater or equal to 3 have empty d orbitals which means more than 8 electrons can fit around the central atom) AX2 (Steric number, geometry, bond angle (s), polarity) SN: 2 Geometry: linear Bond angle: 180 Polarity: nonpolar
WebSep 14, 2024 · Periodic trends are specific patterns that are present in the periodic table that illustrate different aspects of a certain element, including its size and its electronic properties. Major periodic trends include: electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. colin muthWebOct 8, 2024 · What is the correct order of electron affinities? Therefore, the correct order of electron affinity is Cl > F > Br. Hence, option C is the required answer. Note: You should know that mercury has the lowest electron affinity. colin murray portsoyWebApr 6, 2024 · Hint: In the modern periodic table, the elements are arranged in an increasing order of their atomic numbers. We know that the energy released when one electron is added to a neutral gaseous atom in its ground state is known as electron affinity. When an electron is added to a neutral gaseous atom the atom forms an anion. Complete solution: dr olson ophthalmology orlandoWebApr 9, 2024 · Therefore, combining the effect of size and electron gain enthalpy the electron affinity of Sulphur is a bit higher than selenium and that of oxygen is least in the group. Hence, The correct order of electron affinity is O < S e < S . So, the correct answer is “Option B”. dr olson pediatrics fargoWebJan 30, 2024 · The electron affinity of metals is lower than that of nonmetals. Nonmetals: Nonmetals like to gain electrons to form anions to have a fully stable octet. They release energy (exothermic) to gain electrons to form an anion; thus, electron affinity of … dr olson perrysburg pediatricsWebApr 7, 2024 · Hence, order of electron affinity is So, the correct answer is “Option B”. Note: 1. Electron affinity increases upward for the groups and from left to right across the period of a periodic table because the electrons added to energy levels become closer to the nucleus, thus a stronger attraction is seen between the nucleus and its electron. 2. dr olson orthopedic renoWeb1 Answer. The amount of screening is the same in the two groups but the effective positive charge that the incoming electron feels is stronger in Group 7. and 8 protons. The effective positive charge that pulls the incoming electron (which approaches the second level) is 8 − 2 = 6. and 9 protons. The effective positive charge is 9 − 2 = 7. colin narbeth \u0026 son limited