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Byju's Answer
Standard XII
Chemistry
Ionization Enthalpy
The first ion...
Question

The first ionization enthalpy of Ca is greater than that of potassium because for Ca


A

The electron is removed from S- subshell

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B

The effective nuclear charge is higher

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C

The electron is removed from a P-subshell

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D

The removal of electron does not give noble gas configuration

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Solution

The correct option is B

The effective nuclear charge is higher


Higher the effective nuclear change, greater is the ionization enthalpy.


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Q.

Which one of the following statements is incorrect in relation to ionization enthalpy?

(a) Ionization enthalpy increases for each successive electron.

(b) The greatest increase in ionization enthalpy is experienced on removal of electron from core noble gas configuration.

(c) End of valence electrons is marked by a big jump in ionization enthalpy.

(d) Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value.

Q. Which one of the following statements is incorrect in relation to ionization enthalpy?
(a) Ionization enthalpy increases for each successive electron.
(b) The greatest increases in ionization enthalpy is experienced on removal of electron from core noble gas configuration.
(c) End of valence electrons is marked by a big jump in ionization enthalpy.
(d) Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value.
Q. Assertion :Third ionisation energy of phosphorus is larger than sulphur. Reason: There is a larger amount of stability associated with filled s- and p-subshells (a noble gas electron configuration) which correspond to having eight electrons in the valence shell of an atom or ion.
Q. I. The electron configuration of copper is [Ar]4s13d10.
II. A subshell which is 100% full or 50% full is more stable than subshells which are partially filled with a number of electrons less than or greater than half the number of electrons which can be held by the subshell.
Q. Assertion :Element has a tendency to lose the electron(s) to attain the stable configuration. Reason: Ionization enthalpy is the energy released to remove an electron from an isolated gaseous atom in its ground state.
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