Fluorine flourine is the most electronegative element
Down the group electron affinity decreases Across a period electron affinity increases. However, it should be noted that chlorine is having higher electron affinity than flourine due to the small size of fluorine atom)
Halogens in group 7A have high electron affinities because they have only one electron missing to achieve a stable electron configuration. By gaining an electron, they can fill their outer energy level and become more stable. This strong attraction for an additional electron results in high electron affinities.
No, nitrogen does not have a low electron affinity. Electron affinity increases as you go up and to the right on the periodic table. Thus, Groups I and II elements (ex. Cs, Ba, Sr, etc.) have LOW electron affinities and the halogens in Group VII (Br, Cl, F, etc) have the HIGHEST electron affinities. Chlorine has the HIGHEST electron affinity on the periodic table.(Fluorine is an exception in this case.)
Barium (Ba) is the element in group 2 that is most likely to lose an electron, as it is the most reactive element in this group due to having the lowest ionization energy. This makes it easier for barium to lose its outermost electron to form a 2+ cation.
That element would be in the Alkali Metals (group one)
Aluminum has the lowest electron affinity in Group 13 because it is the most electropositive element in this group due to its position in the periodic table. Electropositive elements tend to have lower electron affinities.
The group that has a substantial affinity for electrons is group 17, the halogens. These elements have 7 valence electrons which makes them have the highest affinity for electrons.
Down the group electron affinity decreases Across a period electron affinity increases. However, it should be noted that chlorine is having higher electron affinity than flourine due to the small size of fluorine atom)
Halogens in Group 7A have high electron affinities because they have a strong desire to gain an electron to achieve a stable electron configuration with a full outer shell. This results in the release of significant energy when an electron is added, leading to high electron affinities for these elements.
Halogens in group 7A have high electron affinities because they have only one electron missing to achieve a stable electron configuration. By gaining an electron, they can fill their outer energy level and become more stable. This strong attraction for an additional electron results in high electron affinities.
No, nitrogen does not have a low electron affinity. Electron affinity increases as you go up and to the right on the periodic table. Thus, Groups I and II elements (ex. Cs, Ba, Sr, etc.) have LOW electron affinities and the halogens in Group VII (Br, Cl, F, etc) have the HIGHEST electron affinities. Chlorine has the HIGHEST electron affinity on the periodic table.(Fluorine is an exception in this case.)
Halogens in group 7 have high electron affinities because they only need to gain one electron to achieve a stable octet electron configuration, which is energetically favorable. This makes them highly reactive in forming stable compounds with metals that can donate an electron to satisfy their electron needs.
Barium (Ba) is the element in group 2 that is most likely to lose an electron, as it is the most reactive element in this group due to having the lowest ionization energy. This makes it easier for barium to lose its outermost electron to form a 2+ cation.
That element would be in the Alkali Metals (group one)
This group has the electron configuration of sulfur. The element sulfur has 16 electrons, and its electron configuration is 1s2 2s2 2p6 3s2 3p4.
8
the element belongs to 4th period, 9th group, it is a d block element. the element is cobalt