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(D) The graph shows that the value of $Y$ increases as the atomic number $(X)$ increases for the alkali metals $Li$,$Na$,and $K$. $1$. $IE_1$ (first i

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$\frac{1}{	ext{electronegativity}}$

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(D) The graph shows that the value of $Y$ increases as the atomic number $(X)$ increases for the alkali metals $Li$,$Na$,and $K$. $1$. $IE_1$ (first ionization energy) decreases down the group as atomic size increases. $2$. Electron affinity generally decreases down the group. $3$. $Z_{eff}$ (effective nuclear charge) calculated using Slater's rule for valence electrons in alkali metals remains approximately constant ($Z_{eff} \approx 1.30$ for $Li$,$Na$,$K$). $4$. Electronegativity decreases down the group,so $\frac{1}{	ext{electronegativity}}$ increases down the group. Therefore,the value of $\frac{1}{	ext{electronegativity}}$ increases as we move from $Li$ to $Na$ to $K$.

If coordinate $X$ is atomic number,then select the best option for the $Y$ coordinate based on the given graph for $Li$,$Na$,and $K$.

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If coordinate $X$ is atomic number,then select the best option for the $Y$ coordinate based on the given graph for $Li$,$Na$,and $K$.

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Among the following,the pairs of elements having approximately the same electronegativity values are:
$I$. $H$ and $P$
$II$. $Be$ and $Al$
$III$. $N$ and $Cl$
$IV$. $C$ and $P$