The successive ionisation energy values for an element $X$ are given below. Element $X$ belongs to which group?
$1^{st} \text{ IE} = 410 \ kJ \ mol^{-1}$
$2^{nd} \text{ IE} = 820 \ kJ \ mol^{-1}$
$3^{rd} \text{ IE} = 1100 \ kJ \ mol^{-1}$
$4^{th} \text{ IE} = 1500 \ kJ \ mol^{-1}$
$5^{th} \text{ IE} = 3200 \ kJ \ mol^{-1}$
$1^{st} \text{ IE} = 410 \ kJ \ mol^{-1}$
$2^{nd} \text{ IE} = 820 \ kJ \ mol^{-1}$
$3^{rd} \text{ IE} = 1100 \ kJ \ mol^{-1}$
$4^{th} \text{ IE} = 1500 \ kJ \ mol^{-1}$
$5^{th} \text{ IE} = 3200 \ kJ \ mol^{-1}$
- A$14$
- B$13$
- C$15$
- D$12$
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Similar Questions
Consider the elements $Ne$,$Na$,and $Mg$. The element with the highest first ionization enthalpy and the element with the lowest second ionization enthalpy,respectively,are:
Consider the following ionisation reactions:
$A_{(g)} \to A^{+}_{(g)} + e^-, \ A_1$ $B_{(g)} \to B^{+}_{(g)} + e^-, \ B_1$ $B^{+}_{(g)} \to B^{2+}_{(g)} + e^-, \ B_2$ $C_{(g)} \to C^{+}_{(g)} + e^-, \ C_1$ $C^{+}_{(g)} \to C^{2+}_{(g)} + e^-, \ C_2$ $C^{2+}_{(g)} \to C^{3+}_{(g)} + e^-, \ C_3$
If the monovalent positive ion of $A$,divalent positive ion of $B$,and trivalent positive ion of $C$ have zero electrons,then which of the following is the incorrect order of the corresponding $I.E.$?
| $A_{(g)} \to A^{+}_{(g)} + e^-, \ A_1$ | $B_{(g)} \to B^{+}_{(g)} + e^-, \ B_1$ |
| $B^{+}_{(g)} \to B^{2+}_{(g)} + e^-, \ B_2$ | $C_{(g)} \to C^{+}_{(g)} + e^-, \ C_1$ |
| $C^{+}_{(g)} \to C^{2+}_{(g)} + e^-, \ C_2$ | $C^{2+}_{(g)} \to C^{3+}_{(g)} + e^-, \ C_3$ |
If the monovalent positive ion of $A$,divalent positive ion of $B$,and trivalent positive ion of $C$ have zero electrons,then which of the following is the incorrect order of the corresponding $I.E.$?
Arrange $S, P, As$ in order of increasing ionisation energy.
Easy
View SolutionWhich of the following orders is correct for the property mentioned in brackets?
Difficult
View SolutionGiven below are two statements:
Statement $I$: The first ionization energy of $Pb$ is greater than that of $Sn$.
Statement $II$: The first ionization energy of $Ge$ is greater than that of $Si$.
In the light of the above statements,choose the correct answer from the options given below:
Statement $I$: The first ionization energy of $Pb$ is greater than that of $Sn$.
Statement $II$: The first ionization energy of $Ge$ is greater than that of $Si$.
In the light of the above statements,choose the correct answer from the options given below:
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