Ch 07 HW Periodic Trends in Relative Electron Affinity Resources a previous | 5

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Ch 07 HW Periodic Trends in Relative Electron Affinity Resources a previous | 5 of 7 |next » Periodic Trends in Relative Electron Affinity Part A Electron affinity, EA, is the energy required to add an electron to a neutral gaseous atom and is related to an element's position on the periodic table. Electron affinities can be positive, negative, or zero, as shown in the table For the elements with the electron affinities given in the table in the introduction, which element is most likely to accept an electron? Hints Mg Electron affinity Element As (arsenic) F (fluorine) Mg (magnesium) As (kJ/mol) -78 328 Submit My Answers Give Up Part B Rank the following elements by electron affinity, from most positive to most negative EA value Rank from most positive to most negative. To rank items as equivalent, overlap them. Hints Reset Help fluorinepotassium phosphorus neon sulfu Most positive Most negative

Explanation / Answer

A. Fluorine,

higher the negative electro affinity value , the higher the value of low exothermic it is the stronger the attractive force exterted on the electrons. electron affinity in kj/mol means that for every mole of an atom there requires that certain amount of energy for all particles of that element to gain an electron.

B. potassium electron affinity = -48 kj/mol

phophorous 72 kj/mol

neon= 0( zero kj/mol)

sulfur = -200 kj/mol

fluorine = -328 kj/mol

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