Ionization energy of gaseous $Na$ atoms is $495.5 \ kJ \ mol^{-1}$. The lowest possible frequency of light that ionizes a sodium atom is $(h = 6.626 \times 10^{-34} \ J \ s, N_A = 6.022 \times 10^{23} \ mol^{-1})$.
- A$7.50 \times 10^4 \ s^{-1}$
- B$4.76 \times 10^{14} \ s^{-1}$
- C$3.15 \times 10^{15} \ s^{-1}$
- D$1.24 \times 10^{15} \ s^{-1}$
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The first ionization energy of magnesium is smaller as compared to that of elements $X$ and $Y$,but higher than that of $Z$. The elements $X$,$Y$ and $Z$,respectively,are :
The $CORRECT$ order of first ionisation enthalpy is:
Observe the following statements.
Statement $(A)$: In general,the ionisation potential value decreases on moving down in the group.
Statement $(B)$: The $1$st ionisation potential of sodium is greater than that of potassium.
Correct answer is:
Statement $(A)$: In general,the ionisation potential value decreases on moving down in the group.
Statement $(B)$: The $1$st ionisation potential of sodium is greater than that of potassium.
Correct answer is:
$A$ large difference between the fourth and fifth ionization energies indicates the presence of
Medium
View SolutionWould you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.
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