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(B) The atomic number of $K$ is $19$ with the electronic configuration $[Ar] 4s^1$.For $K \longrightarrow K^{+} + e^{-}$,the first ionization enthalpy

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$K$

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(B) The atomic number of $K$ is $19$ with the electronic configuration $[Ar] 4s^1$.For $K \longrightarrow K^{+} + e^{-}$,the first ionization enthalpy $\Delta_i H_1 = 419 \ kJ \ mol^{-1}$ is low because $K$ loses its valence electron easily to achieve a stable noble gas configuration.For $K^{+} \longrightarrow K^{2+} + e^{-}$,the second ionization enthalpy $\Delta_i H_2 = 3051 \ kJ \ mol^{-1}$ is very high because the electron is being removed from a stable,fully-filled noble gas core (argon configuration).Potassium is an alkali metal with low electron affinity,resulting in a low negative electron gain enthalpy $\Delta_{eg} H = -48 \ kJ \ mol^{-1}$.Thus,the given values correspond to $K$.

Which element among the following is most probable to have the following values?
$\Delta_i H_1 = 419 \ kJ \ mol^{-1}$
$\Delta_i H_2 = 3051 \ kJ \ mol^{-1}$
$\Delta_{eg} H = -48 \ kJ \ mol^{-1}$

Similar Questions

Which one of the following sets of ions represents the collection of isoelectronic species?

Choose the correct statement$(s)$.

Select the correct statements from the following:
$(a)$ Effective nuclear charge for nitrogen is $3.90$
$(b)$ $IP$ of $Ne$ is more than $Na^{+}$
$(c)$ Order of electronegativity $sp > sp^2 > sp^3$
$(d)$ Order of acidic character $NH_3 < PH_3 < AsH_3$

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

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Which element among the following is most probable to have the following values?$\Delta_i H_1 = 419 \ kJ \ mol^{-1}$$\Delta_i H_2 = 3051 \ kJ \ mol^{-1}$$\Delta_{eg} H = -48 \ kJ \ mol^{-1}$