Atomic Radii & Ionization Potential

Q.

Why do noble gases have comparatively large atomic sizes?

Q. The correct order of first ionization energy is(1) Fe >Co > Ni(3) Co > Fe > No52.Ni>Co > Fe(4) Ni> Fe> Co

Q. The element having greatest difference between its first and second ionization energies, is:

1. $Ca$
2. $Sc$
3. $K$
4. $Ba$

Q.

The size of isoelectronic species — $F^{–}$ , Ne and $N{a}^{+}$ is affected by
(a) Nuclear charge (Z )
(b) Valence principal quantum number (n)
(c) Electron-electron interaction in the outer orbitals
(d) None of the factors because their size is the same.

Q. Arrange the following in decreasing order of their atomic radii: B, O, N, F.

1. $B>O>N>F$
2. $B>N>O>F$
3. $F<O<N<B$
4. $F<N<O<B$

Q.

Explain why chlorine can be converted into chloride ion more easily as compared to 2 fluoride ion from fluorine.

Q. Size of the following isoelectronic species increase in the order:

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

Q. Arrange the following in increasing order of their size: Be, Ca, Ba, Sr.

1. $Ca<Ba<Be<Sr$
2. $Be<Sr<Ba<Ca$
3. $Be<Ca<Sr<Ba$
4. $Ba<Sr<Ca<Be$

Q. Highest size will be of

1. $B{r}^{-}$
2. $I$
3. $I^{-}$
4. $I^{+}$

Q. Account for the following:
(i) Schottky defects lower the density of related solids.
(ii) Conductivity of silicon increases on doping it with phosphorus.

Q.

__________gas is used to obtain very low temperature.

Q. Which of the following option is correct for ionic radii?

1. $K^{+}$ > $C{l}^{-}$
2. $P^{+3}$ > $P^{+5}$
3. $T{i}^{+4}$ < $M{n}^{+7}$
4. ${}^{35}C{l}^{-}$ < ${}^{37}C{l}^{-}$

Q. Which of the following noble gases is the least polarized?

1. Radon
2. Krypton
3. Xenon
4. Helium

Q.

Are all the cations in the periodic table are smaller in size with respect to all anions in the periodic table

Q. Which of the follwing atoms has the highest first ionization energy?

1. $Na$
2. $K$
3. $Sc$
4. $Rb$

Q. The element which has the highest first ionization energy is:

1. hydrogen
2. xenon
3. fluorine
4. helium

Q. If $I_{Mg}=\text{First ionization energy of Mg}$
$I{I}_{Mg}=\text{Second ionization energy of Mg}$
$I_{Na}=\text{First ionization energy of Na}$
$I{I}_{Na}=\text{Second ionization energy of Mg}$
Choose the correct option:

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

Q. Ionization energy of noble gas is very high. Why?

Q. Why Noble gases are usually have large atomic size in the period?

Q. Assertion :Helium has the highest value of ionisation energy among all the elements known. Reason: Helium has the highest value of electron affinity among all the elements known.

1. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
2. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
3. Assertion is correct but Reason is incorrect
4. Both Assertion and Reason are incorrect

Q. Match List-I with List-II.

	List-I		List-II
	Electonic configuration of elements		${\Delta }_{1}H\text{(}inkJmo{l}^{-1})$
(a)	$1s^{2}2s^2$	(i)	$801$
(b)	$1s^{2}2s^{2}2p^4$	(ii)	$899$
(c)	$1s^{2}2s^{2}2p^3$	(iii)	$1314$
(d)	$1s^{2}2s^{2}2p^1$	(iv)	$1402$

Choose the most appropriate answer from the options given below:

1. $\left(a\right)\to \left(i\right),\left(b\right)\to \left(iii\right),\left(c\right)\to \left(iv\right),\left(d\right)\to \left(ii\right)$
2. $\left(a\right)\to \left(i\right),\left(b\right)\to \left(iv\right),\left(c\right)\to \left(iii\right),\left(d\right)\to \left(ii\right)$
3. $\left(a\right)\to \left(iv\right),\left(b\right)\to \left(i\right),\left(c\right)\to \left(ii\right),\left(d\right)\to \left(iii\right)$
4. $\left(a\right)\to \left(ii\right),\left(b\right)\to \left(iii\right),\left(c\right)\to \left(iv\right),\left(d\right)\to \left(i\right)$

Q.

What is the vanderwall radius periodicity along A period and down the group in the periodic table

Q. Amongst the following elements (whose electronic configuration are given below) the one having the highest ionization energy is-

1. $\left[Ne\right]3s^{2}3p^1$
2. $\left[Ne\right]3s^{2}3p^3$
3. $\left[Ne\right]3s^{2}3p^2$
4. $\left[Ne\right]3d^{10}4s^{2}4p^3$

Q. The atomic numbers of $V,Cr,Mn$ and $Fe$ are respectively $23,24,25\text{and}26$. Which one of these is expected to have the highest second ionization energy ?

1. $Cr$
2. $Mn$
3. $Fe$
4. $V$

Q.

Two p-block elements x(outer electronic configuration ${ns}^2$, ${np}^3$) and z (outer configuration ${ns}^2$, ${np}^4$) occupy neighbouring positions in a period. Using this information which of the following is correct with respect to their ionisation potential $I_x$ and $I_z$.

1. I_z = I_x

2. Relation between I_x and I_z is uncertain

3. I_x > I_z

4. I_z > I_x

Q. Which of the following is the correct order of ionic radii?

1. 
   $T{i}^{4+}<M{n}^{7+}$
2. $C{l}^{-}<K^{+}$
3. $C{a}^{2+}<K^{+}$
4. $O^{2-}<F^{-}$

Q. Assertion (A): Noble gases have highest ionization energies in their respective periods.
Reason (R): The outermost shell of noble gases is completely filled.

1. Both $A$ and $R$ are correct and $R$ is the correct explanation of $A$.
2. Both $A$ and $R$ are correct and $R$ is not the correct explanation of $A$.
3. $A$ is true but $R$ is false.
4. $A$ is false but $R$ is true.

Q. The electron configuration for the noble gas with the highest first ionization energy is:

1. $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^2$
2. $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^1$
3. $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$
4. $1s^2$
5. $1s^{2}2s^{2}2p^{6}3p^1$

Q.

The number of peroxide bonds in perxenate ion $[Xe{O}_6{]}^{4-}$ is:

1. $3$
2. $1$
3. $0$
4. $2$

Q. The noble gas with highest ionization energy is :

1. He
2. Ar
3. Kr
4. Xe