A quantitative measure of the tendency o...

A quantitative measure of the tendency of an element to lose electron is given by its ionization enthalpy. It represents the energy required to remove an electron from an isolated gaseous atom (X) in its ground state. In other words, the first ionization enthalpy for an element X is the enthalpy change `(Delta_(i)H)` for the reaction depicted.
`X(g) rarr X^(+) (g)+e^(-)`
The ionization enthalpy is expressed in units of `kJ mol^(-1)`. We can define the second ionization enthalpy as the energy required to remove the second most loosely bound electron: it is the energy required to carry out the reaction,
`X^(+)(g) rarr X^(2+)(g) +e^(-)`
Consider following statements for the two uncharged gaseous species
Species -1 `=1s^(2),2s^(1)` Species -2 `=1s^(2),2p^(1)`
(P) Species-1 is ground state, species-2 is excited state of same atom
(Q) Species-1 is excited state, species-2 is ground state of same atom
(R) Ionization of species-1 is easier as compared to species-2
(S) Ionization of species-2 is easier as compared to species-1
Select correct statement(s)

P and R

Q and R

P and S

Q and S

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The correct Answer is:

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A quantitative measure of the tendency of an element to lose electron is given by its ionization enthalpy. It represents the energy required to remove an electron from an isolated gaseous atom (X) in its ground state. In other words, the first ionization enthalpy for an element X is the enthalpy change (Delta_(i)H) for the reaction depicted. X(g) rarr X^(+) (g)+e^(-) The ionization enthalpy is expressed in units of kJ mol^(-1) . We can define the second ionization enthalpy as the energy required to remove the second most loosely bound electron: it is the energy required to carry out the reaction, X^(+)(g) rarr X^(2+)(g) +e^(-) Largest energy is required for which change?

`Sc_((g)) rarr Sc_((g))^(+)`

`Sc_((g))^(+) rarr Sc_((g))^(+2)`

`Sc_((g))^(+2) rarr Sc_((g))^(+3)`

`Sc_((g))^(+3) rarr Sc_((g))^(+4)`

smaller than the first ionization enthalpy

salmost equal to the first ionizationn enthalpy

smallerr than the third ionization enthalpy

equal to the second electron gain enthalpy.

all positive quantities

all negative quantities

either positive or negative quantities

all netural quantities