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(N/A) Electron gain enthalpyElectronegativity$1$. It can be measured.$1$. It cannot be measured.$2$. The change in enthalpy when $1$ electron is added

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(N/A) Electron gain enthalpyElectronegativity$1$. It can be measured.$1$. It cannot be measured.$2$. The change in enthalpy when $1$ electron is added to a gaseous atom is known as electron gain enthalpy.$2$. The capacity to attract a shared pair of electrons in a covalent bond is known as electronegativity.$3$. It represents the enthalpy change of the reaction $X_{(g)} + e^{-} \rightarrow X^{-}_{(g)}$.$3$. Its value is relative and denoted by scales like Pauling's scale (electronegativity of fluorine is $4.0$).$4$. It indicates the energy released or absorbed when an electron is added.$4$. It indicates the relative tendency of an atom to attract shared electrons.$5$. Its value is a property of an isolated gaseous atom.$5$. Electronegativity is not constant; it depends on the chemical environment and the atom it is bonded to.

What is the basic difference between the terms electron gain enthalpy and electronegativity?

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Electron gain enthalpy	Electronegativity
$1$. It can be measured.	$1$. It cannot be measured.
$2$. The change in enthalpy when $1$ electron is added to a gaseous atom is known as electron gain enthalpy.	$2$. The capacity to attract a shared pair of electrons in a covalent bond is known as electronegativity.
$3$. It represents the enthalpy change of the reaction $X_{(g)} + e^{-} \rightarrow X^{-}_{(g)}$.	$3$. Its value is relative and denoted by scales like Pauling's scale (electronegativity of fluorine is $4.0$).
$4$. It indicates the energy released or absorbed when an electron is added.	$4$. It indicates the relative tendency of an atom to attract shared electrons.
$5$. Its value is a property of an isolated gaseous atom.	$5$. Electronegativity is not constant; it depends on the chemical environment and the atom it is bonded to.