The successive ionization energies of an element $(A)$ are given as $IE_1 = 20 \ eV, IE_2 = 45 \ eV, IE_3 = 150 \ eV, IE_4 = 900 \ eV, IE_5 = 1800 \ eV$. What is the formula of the halide of $(A)$?
- A$AX$
- B$AX_3$
- C$AX_4$
- D$AX_5$
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The first three ionisation energies (in $kJ/mol$) of three representative elements are given below:
Element $IE_1$ $IE_2$ $IE_3$ $P$ $495.8$ $4562$ $6910$ $Q$ $737.7$ $1451$ $7733$ $R$ $577.5$ $1817$ $2745$
Which of the following options is incorrect?
| Element | $IE_1$ | $IE_2$ | $IE_3$ |
| $P$ | $495.8$ | $4562$ | $6910$ |
| $Q$ | $737.7$ | $1451$ | $7733$ |
| $R$ | $577.5$ | $1817$ | $2745$ |
Which of the following options is incorrect?
Difficult
View SolutionIdentify the elements $X$ and $Y$ using the ionisation energy values given below :
Element Ionization energy $1^{st}$ $(kJ/mol)$ Ionization energy $2^{nd}$ $(kJ/mol)$ $X$ $495$ $4563$ $Y$ $731$ $1450$
| Element | Ionization energy $1^{st}$ $(kJ/mol)$ | Ionization energy $2^{nd}$ $(kJ/mol)$ |
| $X$ | $495$ | $4563$ |
| $Y$ | $731$ | $1450$ |
The first four $I.E.$ values of an element are $284, 412, 656$ and $3210 \ kJ \ mol^{-1}$. The number of valence electrons in the element are
Difficult
View SolutionWhich of the following electronic configurations represents the atom with the lowest first ionization enthalpy?
Medium
View SolutionThe correct sequence of elements in decreasing order of first ionisation energy is
Easy
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