What is the definition of ionization energy for an atom?
- AThe energy required to remove an electron from the outermost shell of an isolated gaseous atom in its ground state.
- BThe energy released when an electron is added to an isolated gaseous atom.
- CThe energy required to excite an electron from the ground state to an excited state.
- DThe energy change when an atom gains a proton.
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Similar Questions
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 $(A)$?
Medium
View Solution$X_{(g)} \to X^{+}_{(g)} + e^-$,$\Delta H = +720 \ kJ \ mol^{-1}$
Calculate the amount of energy required to convert $110 \ mg$ of $X$ atom in gaseous state into $X^{+}$ ion .................... $kJ$ (Atomic weight for $X = 7 \ g \ mol^{-1}$)
Calculate the amount of energy required to convert $110 \ mg$ of $X$ atom in gaseous state into $X^{+}$ ion .................... $kJ$ (Atomic weight for $X = 7 \ g \ mol^{-1}$)
The elements which occupy the peaks of the ionisation energy curve are
Easy
View SolutionAssertion $(A)$: First ionisation enthalpy of oxygen is less than that of nitrogen.
Reason $(R)$: Atoms with half-filled or completely filled orbitals are less stable.
The correct option among the following is:
Reason $(R)$: Atoms with half-filled or completely filled orbitals are less stable.
The correct option among the following is:
Which of the following transitions involves the maximum amount of energy?
DifficultAIIMS 1992
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