Question

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Question :- Electron affinity....( )

a)Decreases accross a period and increases down the group
b)Decreases down the group and increases across a period
c)Increases both across period and group
d)Decreases both across period and down the group

Answer 1

$\mathfrak{Answer}$ :-

Option b

*Decreases across a group and increases in a period*

$\boxed{Explanation}$ :-

•Electron Affinity :-

The electron affinity of an element is defined as the energy liberated when an electron is added to its neutral gaseous atom.

•Electron affinity is also called as ELECTRON GAIN ENTHALPY.

•Electron gain enthalpy :-

>> In a group :- DECREASES

>>In a period :- INCREASES from left to right.

•Metals have low electron gain enthalpy values.

>>Factors influencing electron gain enthalpy are <<

—-• Nuclear Charge

—-•Screening Effect

—-•Penetration power of orbitals

—-• Stable Electronic configuration and

—-• Atomic radius

Answer 2

Answer:-

b)Decreases down the group and increases across a period

Explanation:-

$\texttt{\green{Electron \: Affinity:-}}$

• Electron affinity can be defined as the the amount of energy lost when electron is added to an atom.

• Electron affinity is also called as $\texttt{\blue{Electron \: gain \: Enthalpy}}$

• The term enthalpy refers to energy.

• Electron Affinity decreases down the group, due to $\texttt{\blue{increase \: in \: size}}$ of atom

• Electron Affinity increases from left to right in period , due to $\texttt{\blue{decrease \: in \: size}}$ of atom

• EA is opposite to the Ionization energy.. Which is defined as, the energy required to remove electron from valency shell from a NEUTRAL GASEOUS ATOM

• EA depends on the factors like, atomic Size, nuclear charge, Sccreening effect, Stable configuration etc..

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