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How does fluorine differ from iodine in the periodical table?
Fluorine is located to the left of iodine in the periodic table. Fluorine is a highly reactive nonmetal, while iodine is a less reactive nonmetal. Their chemical properties and reactivities differ due to their electron configurations and atomic sizes.
Why the electron affinity of fluorine is less than that of chlorine?
Generally electron affinity goes up as you go from left to right across the Periodic Table, and decreases as you go down a column. However, fluorine is an exception -- and the element with the highest electron affinity is chlorine (note that the most electronegative element is fluorine however).The reason that the electron affinity is not as high as might otherwise be predicted for fluorine is that it is an extremely small atom, and so it's electron density is very high. Adding an additional electron is therefore not quite as favorable as for an element like chlorine where the electron density is slightly lower (due to electron-electron repulsion between the added electron and the other electrons in the electron cloud).Note that there are a number of other exceptions to the general rule of electron affinity increasing towards the upper right corner -- see the Related Questions links to the left for an explanation of some of those other exceptions.See also the Web Links to the left for more information about electron affinities and the fluorine-chlorine exception.
What elements has the largest electron affinity?
AnswerElectron affinity is the energy released when we add an electron to the outermost orbit of the atom. Halogens are the higher in electron affinity, and chlorine has the higher electron affinity than rest of the halogens. The irregularity in the electron affinity trend between Cl and F is due to the small size of the F atom. Although F definitely has a higher attraction for an electron than Cl (as evidenced by its high electro negativity value), the small size of the F atom means that adding an electron creates significant repulsion. Since electron affinity is an energy measurement, the total energy associated with electron affinity winds up being the energy that is released by the electron binding to the nucleus, minus the energy involved in overcoming the electrical repulsion in the outer shell.This makes the fluoride anion so formed unstable due to a very high charge/mass ratio. Also, fluorine has no d electrons which limits its atomic size. As a result, fluorine has an electron affinity less than that of chlorine.
Which halogen has the lowest first ionization potential?
The outer electrons in bigger halogens are further from the nucleus and so they feel less attraction and so are easier to remove. Therefore, astatine has the lowest ionisation potential of the halogens.
What is the second electron affinity of chlorine?
Chlorine has a negative second electron affinity because it releases energy when gaining an additional electron. This makes it less likely to accept a second electron compared to its first electron affinity, which is positive.
How does fluorine differ from iodine in the periodical table?
Fluorine is located to the left of iodine in the periodic table. Fluorine is a highly reactive nonmetal, while iodine is a less reactive nonmetal. Their chemical properties and reactivities differ due to their electron configurations and atomic sizes.
Why the electron affinity of fluorine is less than that of chlorine?
Generally electron affinity goes up as you go from left to right across the Periodic Table, and decreases as you go down a column. However, fluorine is an exception -- and the element with the highest electron affinity is chlorine (note that the most electronegative element is fluorine however).The reason that the electron affinity is not as high as might otherwise be predicted for fluorine is that it is an extremely small atom, and so it's electron density is very high. Adding an additional electron is therefore not quite as favorable as for an element like chlorine where the electron density is slightly lower (due to electron-electron repulsion between the added electron and the other electrons in the electron cloud).Note that there are a number of other exceptions to the general rule of electron affinity increasing towards the upper right corner -- see the Related Questions links to the left for an explanation of some of those other exceptions.See also the Web Links to the left for more information about electron affinities and the fluorine-chlorine exception.
Who has higher electron affinity between bromine and Iodine?
According to Zumdahl, Group 7A elements (halogens) follow the expected behavior or periodicity as you follow top to bottom. The numbers (top to bottom) are getting closer to 0, so they are decreasing in electron affinity. Bromine has a higher negative # therefore it is a higher electron affinity.---papajohn
What elements has the largest electron affinity?
AnswerElectron affinity is the energy released when we add an electron to the outermost orbit of the atom. Halogens are the higher in electron affinity, and chlorine has the higher electron affinity than rest of the halogens. The irregularity in the electron affinity trend between Cl and F is due to the small size of the F atom. Although F definitely has a higher attraction for an electron than Cl (as evidenced by its high electro negativity value), the small size of the F atom means that adding an electron creates significant repulsion. Since electron affinity is an energy measurement, the total energy associated with electron affinity winds up being the energy that is released by the electron binding to the nucleus, minus the energy involved in overcoming the electrical repulsion in the outer shell.This makes the fluoride anion so formed unstable due to a very high charge/mass ratio. Also, fluorine has no d electrons which limits its atomic size. As a result, fluorine has an electron affinity less than that of chlorine.
Which has more electron affinity between cl2 and f2?
The reason that the electron affinity is not as high as might otherwise be predicted for fluorine is that it is an extremely small atom, and so it's electron density is very high. Adding an additional electron is therefore not quite as favorable as for an element like chlorine where the electron density is slightly lower (due to electron-electron repulsion between the added electron and the other electrons in the electron cloud).
Why is the electron affinity for clorine is greater than the electron affinity for iodine?
Generally electron affinity goes up as you go from left to right across the periodic table, and decreases as you go down a column. However, fluorine is an exception -- and the element with the highest electron affinity is chlorine.(Note that the most electronegative element is fluorine however; 'electronegativity' is not exactly the same as 'electron affinity'.)Electronegativity is the ability of an atom in a molecule to draw bonding electrons to itselfElectron affinity is a measure of the energy change when an electron is added to a neutral atom to form a negative ion.The reason that the electron affinity is not as high as might otherwise be predicted for fluorine, is that it is an extremely small atom, and so it's electron density is very high. Adding an additional electron is therefore not quite as favorable as for an element like chlorine where the electron density is slightly lower (due to electron-electron repulsion between the added electron and the other electrons in the electron cloud).
Which halogen has the lowest first ionization potential?
The outer electrons in bigger halogens are further from the nucleus and so they feel less attraction and so are easier to remove. Therefore, astatine has the lowest ionisation potential of the halogens.
What is the second electron affinity of chlorine?
Chlorine has a negative second electron affinity because it releases energy when gaining an additional electron. This makes it less likely to accept a second electron compared to its first electron affinity, which is positive.
Why EA of fluorine is less than chlorine?
Generally electron affinity goes up as you go from left to right across the periodic table, and decreases as you go down a column. However, fluorine is an exception -- and the element with the highest electron affinity is chlorine (note that the most electronegative element is fluorine however).The reason that the electron affinity is not as high as might otherwise be predicted for fluorine is that it is an extremely small atom, and so it's electron density is very high. Adding an additional electron is therefore not quite as favorable as for an element like chlorine where the electron density is slightly lower (due to electron-electron repulsion between the added electron and the other electrons in the electron cloud).Note that there are a number of other exceptions to the general rule of electron affinity increasing towards the upper right corner -- see the Related Questions links to the left for an explanation of some of those other exceptions.See also the Web Links to the left for more information about electron affinities and the fluorine-chlorine exception.
Why is the electron affinity of Mg lower than the electron affinity of K?
The electron affinity of magnesium (Mg) is lower than that of potassium (K) because Mg is a smaller atom with a fully-filled valence shell, making it less likely to accept an additional electron. In contrast, potassium is a larger atom with an electron configuration that benefits from gaining an electron to achieve a stable inert gas configuration.
Does chlorine have a high electron affinity or a low ionization energy?
Chlorine has a high electron affinity due to its tendency to gain an electron to achieve a stable electron configuration. It also has a relatively low ionization energy, meaning it takes less energy to remove an electron from a chlorine atom compared to other elements.
What is xenon electron affinity?
Xenon's electron affinity refers to the energy released when a neutral xenon atom gains an electron to form a xenide ion. Xenon's electron affinity is low compared to many other elements, meaning it is less likely to gain an electron and form negative ions.
