Ionisation Energy

Q. Which of the following configurations represents atoms of the elements having the highest second ionization energy?

1. $1s^{2}2s^{2}2p^{6}3s^2$
2. $1s^{2}2s^{2}2p^6$
3. $1s^{2}2s^{2}2p^4$
4. $1s^{2}2s^{2}2p^{6}3s^1$

Q. Choose the correct ionization potential among the following:

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

Q. Which of the following relation is correct with respect to $I^{st}$ and $2^{nd}$ Ionization energy of Sodium and Magnesium?

1. $I_{Mg}=I{I}_{Na}$
2. $I{I}_{Na}>I{I}_{Mg}$
3. $I{I}_{Mg}>I{I}_{Na}$
4. $I_{Na}>I{I}_{Mg}$

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 $J$

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

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

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

Q. Which of the following isoelectronic ions have lowest ionization?

1. $N{a}^{+}$
2. $M{g}^{2+}$
3. $F^{-}$
4. $O^{2-}$

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

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

Q. What is the correct order of increasing second ionisation energies for the elements $Be,B,C,N$ and $F?$

1. $Be<C<B<N<F$
2. $F<C<B<N<Be$
3. $Be<B<C<N<F$
4. $Be<C<N<B<F$

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

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