The ionization energy of an element is defined as:
- AThe same as the electron affinity of the element
- BEqual in magnitude but of opposite sign to the electron affinity of the element
- CThe energy released when an electron is added to an atom of the element
- DThe energy required to remove the outermost electron of an atom of the element
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Similar Questions
In the second period of the modern periodic table,two elements $X$ and $Y$ have higher first ionization enthalpy values than the preceding and succeeding elements. $X$ and $Y$ are respectively
Which is the correct order of ionization energies?
Difficult
View SolutionThe first ionization potential $(IP)$ of $Be$ $(Z=4)$ is higher than which of the following elements?
$(a) B (Z=5)$
$(b) Mg (Z=12)$
$(c) Li (Z=3)$
$(d) Al (Z=13)$
$(e) K (Z=19)$
$(a) B (Z=5)$
$(b) Mg (Z=12)$
$(c) Li (Z=3)$
$(d) Al (Z=13)$
$(e) K (Z=19)$
Medium
View SolutionThe 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 $(A)$?
Medium
View SolutionThe increasing order of the first ionization enthalpies of the elements $B$,$P$,$S$ and $F$ (lowest first) is:
MediumAIEEE 2006
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