Consider the following ionization enthalpies | vedclass

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(A) The large jump between the $2^{nd}$ and $3^{rd}$ ionization enthalpies for both elements ($A: 1757$ to $14847$; $B: 1450$ to $7731$) indicates tha

Vedclass · Accepted Answer

Both $A$ and $B$ belong to group $2$ where $B$ comes below $A$.

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(A) The large jump between the $2^{nd}$ and $3^{rd}$ ionization enthalpies for both elements ($A: 1757$ to $14847$; $B: 1450$ to $7731$) indicates that both elements have $2$ valence electrons,placing them in group $2$ (alkaline earth metals).Ionization enthalpy decreases down a group as the atomic size increases.Since the ionization enthalpy values for element $B$ are lower than those for element $A$,element $B$ must be located below element $A$ in group $2$.

Element	Ionization enthalpy $(kJ \ mol^{-1})$ $(1^{st}, 2^{nd}, 3^{rd})$
$A$	$899, 1757, 14847$
$B$	$737, 1450, 7731$

Consider the following ionization enthalpies of two elements $A$ and $B$.

Element Ionization enthalpy $(kJ \ mol^{-1})$ $(1^{st}, 2^{nd}, 3^{rd})$

$A$ $899, 1757, 14847$

$B$ $737, 1450, 7731$

Which of the following statements is correct?

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The successive ionization enthalpy values for an unknown element are $\Delta_i H_1 = 899 \ kJ/mol$,$\Delta_i H_2 = 1757 \ kJ/mol$,$\Delta_i H_3 = 14847 \ kJ/mol$,and $\Delta_i H_4 = 17948 \ kJ/mol$. To which group of the periodic table does this element belong?

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Consider the following ionization enthalpies of two elements $A$ and $B$. Element Ionization enthalpy $(kJ \ mol^{-1})$ $(1^{st}, 2^{nd}, 3^{rd})$ $A$ $899, 1757, 14847$ $B$ $737, 1450, 7731$ Which of the following statements is correct?