Ionisation Energy

Q. Which of the following species has lowest ionisation enthalpy?

1. $O$
2. $O^{-}$
3. $O^{2-}$
4. $O^{+}$

Q. The correct order of ionization energy for the isoelectronic species among the following is:

1. 
   $N{a}^{+}>O^{2-}$
2. 
   All of the above
3. 
   $K^{+}>C{l}^{-}$
4. 
   $Ne>F^{-}$

Q. Highest amount of energy will be required to remove an electron from:
(for the same value of n)

1. $s-\text{subshell}$
2. $p-\text{subshell}$
3. $d-\text{subshell}$
4. $f-\text{subshell}$

Q. $I{E}_2$ for an element is invariably higher than $I{E}_1$ because

1. The size of cations is smaller than its atom
2. It is difficult to remove electron from cations
3. Ionization energy is endothermic
4. All of the above

Q. The factors that influence the ionization energy are :

1. Size of the atom
2. The inner electrons which effectively screen the nuclear charge
3. All of the above.
4. Charge on the nucleus

Q. Which of the following has the largest ionization enthalpy?

1. $Mg$
2. $P$
3. $Ar$
4. $F$

Q. Choose the correct ionization potential among the following:

1. 
   $O^{-}>O$
2. 
   $N^{-}>O$
3. 
   None of the above
4. 
   $H^{-}>H$

Q. Energy of an electron in the ground state of the hydrogen atom is -$2.18\times {10}^{-18}J.$ The ionization enthalpy of atomic hydrogen is $a\times {10}^{5}J/mol$. Then $‘a^{\prime }$ is: (Take $N_A=6\times {10}^{23}$)

Q. The ionic bonds $X^{+}{Y}^{-}$ are formed when:

1. Electron affinity of $Y$ is high and ionisation energy of $X$ is low
2. None of these
3. Electron affinity of $Y$ is low and ionisation energy of $X$ is high
4. Lattice energy of $XY$ is low

Q. $\frac{N_0}{2}$ atoms of $X\left(g\right)$ are converted into $X^{+}\left(g\right)$ by absorbing $E_1$ energy. $2N_0$ atoms of $X\left(g\right)$ are converted into $X^{-}\left(g\right)$ by releasing $E_2$ energy. Calculate the ionisation enthalpy and electron gain enthalpy of $X\left(g\right)$ per atom.

1. $I.E.=\frac{2E_1}{N_0},{\Delta }_{eg}H=-\frac{E_2}{2N_0}$
2. $I.E.=\frac{E_2}{2N_0},{\Delta }_{eg}H=-\frac{2E_1}{N_0}$
3. $I.E.=\frac{E_1}{2N_0},{\Delta }_{eg}H=-\frac{E_2}{N_0}$
4. $I.E.=\frac{N_0}{E_1},{\Delta }_{eg}H=-\frac{2N_0}{E_2}$

Q. Correct increasing order of $1st$ ionisation energy:

1. $Be<C<B$
2. None of the above
3. $B<Be<C$
4. $Be<B<C$

Q. Which of the following statement(s) is/(are) correct?

1. The electron affinity for Sulphur is more exothermic than that for Oxygen
2. Successive ionization energies of an atom always increase.
3. First ionization energy of $N$ is greater than that of $O$
4. Chlorine has larger atomic size as well as electron afinity than that of fluorine.

Q. The decreasing order of the first ionization energy of group 16 elements is:

1. $O>S>Se<Te>Po$
2. $O>S>Se>Te>Po$
3. $O<S<Se<Te<Po$
4. None of the above

Q.

What is an ionisation energy?

Q. Select the incorrect statement(s).

1. $I{E}_1$ of Nitrogen atom is less than $I{E}_1$ of Oxygen atom.
   
2. Electron gain enthalpy of Oxygen is less negative than Selenium.
   
3. Electronegativity on Pauling scale is 2.8 times the electronegativity on Mulliken scale.
   
4. $C{r}^{6+}$ is smaller than $C{r}^{3+}$.
   

Q. $I{E}_1$ and $I{E}_2$ of $Mg$ are $178$ and $348\text{kcal}$ respectively. The energy required for the following reaction is:
$Mg\to M{g}^{2+}+2e^{-}$
(Where $IE$ = ionization energy)

1. $+170\text{kcal}$
2. $+526\text{kcal}$
3. $-170\text{kcal}$
4. $-526\text{kcal}$

Q. The successive ionization energies for element $X$ are given below:
$I{E}_1=250{\text{kJ mol}}^{-1}$
$I{E}_2=820{\text{kJ mol}}^{-1}$
$I{E}_3=1100{\text{kJ mol}}^{-1}$
$I{E}_4=1400{\text{kJ mol}}^{-1}$
Find out the number of valence electrons from the element $X$.

1. $3$
2. $4$
3. $2$
4. $1$

Q. The ionization energy of sodium is $495kJ/mol$. How much energy is needed to convert atoms present in 2.3 $mg$ of sodium into sodium ions?

1. 4.95 $J$
2. 49.5 $J$
3. 495 $J$
4. 0.495 $J$