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Generally electron affinity goes up as you go from left to right across the Periodic Table, and decreases as you go down a column.
There are exceptions however. See the Related Questions to the left for some examples of the exceptions as well as an explanation.
What else can I help you with?
Is electron affinity of N is greater than F?
No, it is not. Electron affinity follows a trend like electronegativity and hence increases as we move from left to right across a period. So, Fluorine has the highest electron affinity among 1st period elements.
What happens when the nuclear charge increases across a period?
As the nuclear charge increases across a period, the number of protons in the nucleus increases. This leads to a stronger attraction between the nucleus and the electrons in the atom, resulting in a greater effective nuclear charge. This can lead to an increase in the atomic size and higher electronegativity across a period.
Why does electron affinity increase going left to right?
In general, electron affinity does not increase steadily from left to right. Firstly, only non-metals have electron affinities greater than 0. Secondly, the ordering of these electron affinities is O<N<F; S<P<Cl
How does ionization enthalpy vary as you move across the periods vary from left to right?
in a period size decreases from left to right and hence electrons are more tightly held to the nucleus. so electron gain enthalpy increases across a period . down the period size increases and thus in general electron gain enthalpy decreses .
Do nonmetals have always higher electron affinity than metals?
No, nonmetals do not always have higher electron affinity than metals. Electron affinity depends on the specific element and its position in the periodic table. Some metals can have higher electron affinities than certain nonmetals.
How does electron affinity vary in periods?
Increases from left to right in a period
What is the trend for electrons?
As you go across a period; Left to right, the electron affinity increases. As you go down a group; top to bottom, the electron affinity decreases.
What are the trends and exceptions to the trends in electron affinity?
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)
Why does electron affinity tend to become more exothermic as you move right across a period?
Electron affinity tends to become more exothermic as you move right across a period because the effective nuclear charge increases, leading to a stronger attraction between the nucleus and the incoming electron. This results in a more stable electron configuration and a release of energy.
Is electron affinity of N is greater than F?
No, it is not. Electron affinity follows a trend like electronegativity and hence increases as we move from left to right across a period. So, Fluorine has the highest electron affinity among 1st period elements.
Which element has the lowest electron affinity Is it nitrogen?
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.)
What is electron affinity . write down its trend in periods and group?
The electronegativity increase in a period from left to right; in a group decrease by descending.
Electron affinity tends to what?
Electron affinity is an elements' ability to attract electrons and is variable for each element. Generally the more electronegative atoms are furthest to the right bottom of the periodic table and ascending to the left the elements lose their electron accepting ability.
What is the periodic trend for ionization energy and electron affinity?
Ionization energy increases from left to right across a period, and decreases down a group.
What happens when the nuclear charge increases across a period?
As the nuclear charge increases across a period, the number of protons in the nucleus increases. This leads to a stronger attraction between the nucleus and the electrons in the atom, resulting in a greater effective nuclear charge. This can lead to an increase in the atomic size and higher electronegativity across a period.
What periodic treds exist for ionization energy?
Ionization energy increases to the right and up on the periodic table. Ionization energy is the energy required to remove an electron. It can be conceptualized as the opposite of electron affinity, though this is not precisely true.
Why does electron affinity increase going left to right?
In general, electron affinity does not increase steadily from left to right. Firstly, only non-metals have electron affinities greater than 0. Secondly, the ordering of these electron affinities is O<N<F; S<P<Cl
