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
Bromine has a higher electron affinity than iodine. This is because bromine has a smaller atomic size, resulting in a stronger attraction for electrons compared to iodine.
Iodine's electron configuration is 2, 8, 18, 18, 7; bromine's is 2, 8, 18, 7. At the simplest level of modelling there is one more electron shell occupying space in an iodine atom than in one of bromine.
Bromine will form a more polar bond with phosphorus compared to iodine. This is because bromine is more electronegative than iodine, resulting in a greater difference in electronegativity between bromine and phosphorus, making the bond more polar.
Bromine has a SMALLER atomic radius because it has one more electron shell than Iodine. On the periodic table, atomic radius of an atom decreases across a period and increases down a group. Since Bromine and Iodine are in the same group, you know Bromine has a smaller atomic radius because it is in a lower period.
An iodine atom has the same number of electrons as a bromine ion. Both elements belong to the halogen group and have seven valence electrons. When bromine gains one electron to become an ion, it will have a full outer shell with eight electrons, the same electron configuration as iodine.
Bromine has a higher electron affinity than iodine. This is because bromine has a smaller atomic size, resulting in a stronger attraction for electrons compared to iodine.
Yes. It's true. Chlorine has the highest electron affinity, then Fluorine, Bromine and Iodine
Bromine has more nuclear charge as compared to iodine. So, bromine easily attracts an electron and hence more reactive.
Iodine's electron configuration is 2, 8, 18, 18, 7; bromine's is 2, 8, 18, 7. At the simplest level of modelling there is one more electron shell occupying space in an iodine atom than in one of bromine.
The Halogens, Fluorine, Chlorine, Bromine, Iodine and Astatine.
Iodine is the largest atom among bromine, fluorine, iodine, and chlorine. It has more electron shells and a larger atomic radius compared to the other three elements.
Bromine will form a more polar bond with phosphorus compared to iodine. This is because bromine is more electronegative than iodine, resulting in a greater difference in electronegativity between bromine and phosphorus, making the bond more polar.
A similar element to bromine in the periodic table is iodine. Both bromine and iodine are halogens, located in the same group (Group 17) of the periodic table. They share similar chemical properties due to their valence electron configuration.
Bromine has a SMALLER atomic radius because it has one more electron shell than Iodine. On the periodic table, atomic radius of an atom decreases across a period and increases down a group. Since Bromine and Iodine are in the same group, you know Bromine has a smaller atomic radius because it is in a lower period.
An iodine atom has the same number of electrons as a bromine ion. Both elements belong to the halogen group and have seven valence electrons. When bromine gains one electron to become an ion, it will have a full outer shell with eight electrons, the same electron configuration as iodine.
The formula for bromine is Br2 and the formula for iodine is I2.
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).