because they need only one element to make noble gas structure.
Group 8A, the noble gases because they have high electron affinity.
The halogen with the least-negative electron affinity is astatine. Electron affinity and electronegativities decreases down a group. Since astatine is the last halogen located in Group 17 as you move down the column from fluorine, it has the least negative electron affinity.
Yes, that is part of the definition of electron affinity.
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.
The energy change that occurs when an electron is added to a neutral atom. This is usually exothermic. Noble Gases are excluded from this. Equation: X(element)+e-(electron)---------> X-1+ energy
Group 8A, the noble gases because they have high electron affinity.
Halogens have the highest electron affinity among all elements. This is because halogens have a strong tendency to gain an electron to achieve a full outer energy level and become stable.
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.
The elements to the left side of the periodic table in groups VIa and VIIa have high electron affinity, as they tend to gain electrons to achieve a stable octet configuration. Group VIIa elements (halogens) have the highest electron affinities in the periodic table.
The halogen group in the periodic table releases the most energy by gaining an electron because they have a high electron affinity and tend to form stable, energy-releasing compounds when they gain an electron to achieve a full outer electron shell.
The halogen with the least-negative electron affinity is astatine. Electron affinity and electronegativities decreases down a group. Since astatine is the last halogen located in Group 17 as you move down the column from fluorine, it has the least negative electron affinity.
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.)
Yes, that is part of the definition of electron affinity.
The electron affinity of germanium is considered to be moderate. Germanium is a metalloid element with an electron affinity that falls between that of metals and nonmetals.
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.
The halogens, specifically the group 17 elements, have the most negative electron affinities. This is because they have a strong attraction for gaining an electron to achieve a stable electron configuration with a full outer shell. Fluorine has the highest electron affinity among the halogens.
Gold; gold has the highest electronic affinity of any atom other than the halogens, due to relativistic effects.