Please be patient as the PDF generation may take upto a minute.

For Avogadro's no. of 'X' atoms, if half of the atoms of 'X' transfer one electron to the other half of 'X' atoms, 409 KJ must be added. If these ${\mathrm{X}}^{-}$ ions are subsequently converted to ${\mathrm{X}}^{+}$, an additional 733 KJ must be added. The IP and EA of X (in eV) are :
1. IP = 11.83 eV, EA = 3.35 eV
2. IP = 3.35 eV, IP = 11.83 eV
3. IP = 11.83 eV, EA = 11.83 eV
4. IP = 3.35 eV, IP = 3.35 eV

The least stable cation is :
1. ${\mathrm{Li}}^{+}$ 
2. ${\mathrm{K}}^{+}$
3. ${\mathrm{Al}}^{2+}$
4. ${\mathrm{Si}}^{2+}$

Which of the following pairs show reverse trend on moving along a period from left to right and from up to down in a group?
1. Nuclear charge and electron affinity
2. Ionisation energy and electron affinity
3. Atomic radius and electron affinity
4. None of these

Which will show maximum non-metallic character?
1. B
2. Be
3. Mg
4. Al

A mixture contains F and Cl atoms. The removal of an electron from each atom of the sample requires 284 KJ while addition of an electron of each atom of mixture releases 68.8 KJ energy.
If IE per atom for F and Cl are $27.91 \mathrm{x} {10}^{-22}$KJ and $20.77 \mathrm{x} {10}^{-22}$KJ. ${\mathrm{EA}}_1$ for F and Cl are $-5.53 \mathrm{x} {10}^{-22}$KJ and $-5.78 \mathrm{x} {10}^{-22}$KJ repectively. The % composition of mixture is :
1. 38% Cl, 62% F
2. 38% F and 62% Cl
3. 50% F and 50% Cl
4. can't be calculated

In which the following arrangements, the sequence is not strictly according to the property written against it?
1. ${\mathrm{Co}}_2 < {\mathrm{SiO}}_2 < {\mathrm{SnO}}_2 < {\mathrm{PbO}}_2$ : increasing oxidising power
2. HF < HCl <HBr < HI : increasing acid strength
3. ${\mathrm{NH}}_3 < {\mathrm{PH}}_3 < {\mathrm{AsH}}_3 < {\mathrm{SbH}}_3$ : increasing basic strength
4. B < C < O < N : increasing first ionisation enthaply
 

Which is not correct order for the stated property?
1. Ba > Sr > Mg : Atomic radius
2. F > O > N : First ionisation energy
3. Cl > F > I : Electron affinity
4. O > Se > Te : Electronegativity

The electronic confuguration of the element with maximum electron affinity is :
1. $1{\mathrm{s}}^2, 2{\mathrm{s}}^{2}2{\mathrm{p}}^3$
2. $1{\mathrm{s}}^2, 2{\mathrm{s}}^{2}2{\mathrm{p}}^5$
3. $1{\mathrm{s}}^2, 2{\mathrm{s}}^{2}2{\mathrm{p}}^6, 3{\mathrm{s}}^{2}3{\mathrm{p}}^5$
4. $1{\mathrm{s}}^2, 2{\mathrm{s}}^{2}2{\mathrm{p}}^6, 3{\mathrm{s}}^{2}3{\mathrm{p}}^3$

In which element shielding effect is not possible?
1. H
2. Be
3. B
4. N

Which transition involves maximum amount of energy :
1. ${\mathrm{M}}_{\left(\mathrm{g}\right)}^{-} \to {\mathrm{M}}_{\left(\mathrm{g}\right)} +\hspace{0.17em}\mathrm{e}$
2. ${\mathrm{M}}_{\left(\mathrm{g}\right)}^{-} \to {\mathrm{M}}_{\left(\mathrm{g}\right)}^{+} + 2\mathrm{e}$
3. ${\mathrm{M}}_{\left(\mathrm{g}\right)}^{+} \to {\mathrm{M}}_{\left(\mathrm{g}\right)}^{2+} + \mathrm{e}$
4. ${\mathrm{M}}_{\left(\mathrm{g}\right)}^{2+} \to {\mathrm{M}}_{\left(\mathrm{g}\right)}^{3+} + \mathrm{e}$

The ionisation energy of nitrogen is more than oxygen because of :
1. more attraction of electron by the nucleus
2. the extra stability of half filled p-orbitals
3. the size of nitrogen atom is smaller 
4. more penetrating effect

The first ionisation potential of aluminium is smaller than that of magnesium because :
1. atomic size of Al > Mg
2. atomic size of Al < Mg
3. Al has one electron in p-orbital
4. none of these

A sudden jump between the values of second and third ionization energies of an element would be associated with the electronic configuration :
1. $1{\mathrm{s}}^2, 2{\mathrm{s}}^2 2{\mathrm{p}}^6, 3{\mathrm{s}}^1$
2. $1{\mathrm{s}}^2, 2{\mathrm{s}}^2 2{\mathrm{p}}^6, 3{\mathrm{s}}^2 3{\mathrm{p}}^1$
3. $1{\mathrm{s}}^2, 2{\mathrm{s}}^2 2{\mathrm{p}}^6, 3{\mathrm{s}}^2 3{\mathrm{p}}^2$
4. $1{\mathrm{s}}^2, 2{\mathrm{s}}^2 2{\mathrm{p}}^6, 3{\mathrm{s}}^2$

The IP${}_1$, IP${}_2$, IP${}_3$, IP${}_4$ and IP${}_5$ of an element are 7.1, 14.3, 34.5, 46.8, 162.2 eV repectively. The element is likely to be :
1. Na
2. Si
3. K
4. Mg

When a ${\mathrm{F}}_{\left(\mathrm{g}\right)}$ atom is changed to ${\mathrm{F}}_{\left(\mathrm{g}\right)}^{-}$, its size increases from 72 pm to 136 pm. The % increase in terms of volume during the formation of F to ${\mathrm{F}}^{-}$ is :
1. 6.75
2. $5.75\times {10}^2$
3. $5.75\times {10}^6$
4. $6.75\times {10}^2$

If $1.96 \times {10}^4$ kJ energy is supplied to 1 mol ${\mathrm{Li}}_{\left(\mathrm{g}\right)}$, it ionised to ${\mathrm{Li}}^{3+}$. If $\mathrm{I}.\mathrm{E}{.}_1$ for Li is 520 kJ ${\mathrm{mol}}^{-1}$ and $\mathrm{I}.\mathrm{E}{.}_1$ for H is $2.18\times {10}^{-18}$ kJ ${\mathrm{atom}}^{-1}$. The $\mathrm{I}.\mathrm{E}{.}_2$ for Li will be :
1. 7270 kJ ${\mathrm{mol}}^{-1}$
2. $11.81\times {10}^3$ kJ ${\mathrm{mol}}^{-1}$
3. $6.54\times {10}^{-3} \mathrm{kJ} {\mathrm{mol}}^{-1}$
4. can't  be calculated 

How many ${\mathrm{Cs}}^{+}$ ions will be obtained if 1 joule energy is supplied to Cs-atoms, if ${\mathrm{IE}}_1$ for Cs is 376 $\mathrm{kJ} {\mathrm{mol}}^{-1}$ ?
1. 1
2. $1.60\times {10}^{18}$
3. $6.023\times {10}^{23}$
4. $3.76\times {10}^{23}$

The amount of energy liberated upon the complete conversion of 2g of chlorine into Cl⁻ is:
( The first electron gain enthalpy value for chlorine is 3.7 eV).
1. 2.4 kcal
2. 4.8 kcal
3. 7.4 kcal
4. 85.3 kcal

For chlorine atom, ${\mathrm{IE}}_1$ and $∆{\mathrm{H}}_{{\mathrm{EG}}_1}$ values are 13.0 eV and 3.60 eV respectively. If Avogadro number of atoms are converted into ${\mathrm{Cl}}^{-}$ by the reaction $\mathrm{Cl}+\mathrm{e}\to {\mathrm{Cl}}^{-}$. If the energy released in this reaction is used to ionise Cl-atoms as $\mathrm{Cl}\to {\mathrm{Cl}}^{+}+{\mathrm{e}}^{-}$. Then the number of Cl-atoms ionised is :
1. $1.667\times {10}^{23}$
2. $6.023\times {10}^{23}$
3. $3.2\times {10}^{23}$
4. can't be calculated

In the long form of periodic table, the elements having lowest ionisation potential are placed in :
1. I group
2. IV group
3. VII group
4. zero group