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With reference to concept of ionisation potential, which one of the following sets are correct ?
1. Li > K> Cs
2.  B > U > K
3. Cs > U > B
4. None of the above

The correct order in which the first ionisation potential increases is :
1. K,Be,Na
2. Be,Na,K
3. K,Na,Be
4. Be,K,Na

Generally, the first ionisation energy increases along a period. But there are some exceptions. One which is not an exceptions is :
1. N and O
2. Na and Mg
3. Mg and Al
4. Be and B

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 X^- ions are subsequently converted to 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, EA = 11.83 eV
3. IP = 11.83 eV, EA = 11.83 eV
4. IP = 3.35 eV, EA = 3.35 eV

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

The elements X,Y,Z and J have the indicated electron configurations starting with the innermost shell. The most metallic element is :
1. X = 2,8,3
2. Y = 2,8,8
3. Z = 2,8,8,1
4. J = 2,8,8,7

Which one of these is amphoteric ?
1. ${\mathrm{CO}}_2$
2. ${\mathrm{SnO}}_2$
3. ${\mathrm{NO}}_2$
4. ${\mathrm{SO}}_2$

Which of the following pairs show reverse trend on moving along a period from left to right and from top 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 of the following properties show gradual decrease with increase in atomic number across a period in the periodic table ?
1. Electron affinity
2. Ionisation potential
3. Electronegativity
4. Size of atom 

In the following the element with the highest electropositivity is :
1. Copper
2. Cesium
3. Barium
4. Chromium

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 to each atom of mixture releases 68.8 kJ energy.  If IE per atom for F and Cl are $27.91\times {10}^{-22} \mathrm{kJ}$ and $20.77\times {10}^{-22} \mathrm{kJ}$. ${\mathrm{EA}}_1$ for F and Cl are $-5.53\times {10}^{-22} \mathrm{kJ} \mathrm{and} -5.78\times {10}^{-22} \mathrm{kJ}$  respectively. 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 of 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 enthalpy

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 electron configuration 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. ${\mathrm{M}}_{\left(\mathrm{g}\right)}^{-}\to {\mathrm{M}}_{\left(\mathrm{g}\right)}+\mathrm{e}$
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 ionization energy of nitrogen is more than oxygen because of :
1. more attraction of electrons 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 ${\mathrm{IP}}_1,{\mathrm{IP}}_2,{\mathrm{IP}}_3,{\mathrm{IP}}_4 \mathrm{and}\hspace{0.17em}{\mathrm{IP}}_5$ of an element are 7.1, 14.3, 34.5, 46.8, 162.2 eV respectively. The element is likely to be :
1. Na
2. Si
3. F
4. Ca

The first four ionisation energy values of an element are 191, 578, 872 and 5962 kcal. The number of valence electrons in the element is :
1. 1
2. 2
3. 3
4. 4

Which one of the following statements is incorrect in relation to ionisation enthalpy ?
1. Ionisation enthalpy increases for removal of each successive electron
2. The higher values of ionisation enthalpies are noticed on removal of electron from core noble gas configuration
3. End of valence electrons is marked by a big jump in ionisation enthalpy
4. Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value 

If ${\mathrm{E}}_{\mathrm{H}-\mathrm{H}}, {\mathrm{E}}_{\mathrm{C}-\mathrm{C}} \mathrm{and} {\mathrm{E}}_{\mathrm{C}-\mathrm{H}}$ values are 104.2, 83.1 and 98.8 kcal ${\mathrm{mol}}^{-1}$ respectively and ${\chi }_H$ (pauling) is 2.1, then ${\chi }_C$ (Pauling ) will be :
1. 2.158
2. 2.598
3. 3.0
4. data is sufficient 

In general, maximum difference in electronegativities is observed when we move :
1. from second to third period
2. from third to fourth period
3. from fourth to fifth period
4. from fifth to sixth period

The correct order of electronegativities of the groups given is :
1. $-{\mathrm{CH}}_3>-{\mathrm{CF}}_3>-\mathrm{CN}>-\mathrm{OH}$
2. $-\mathrm{OH}>-\mathrm{CN}>-{\mathrm{CF}}_3>-{\mathrm{CH}}_3$
3. $-{\mathrm{CF}}_3>-\mathrm{CN}>-\mathrm{OH}>-{\mathrm{CH}}_3$
4. $-{\mathrm{CF}}_3>-\mathrm{OH}>-\mathrm{CN}>-{\mathrm{CH}}_3$

The maximum tendency to form unipositive ion stands for the element with the electronic configuration :
1. $1{\mathrm{s}}^2, 2{\mathrm{s}}^{2}2{\mathrm{p}}^6, 3{\mathrm{s}}^2$
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. $1{\mathrm{s}}^2, 2{\mathrm{s}}^{2}2{\mathrm{p}}^6, 3{\mathrm{s}}^{2}3{\mathrm{p}}^3$

The correct order of ionic radii of ${\mathrm{Li}}^{+},{\mathrm{Al}}^{3+}, {\mathrm{K}}^{+} \mathrm{and} {\mathrm{Mg}}^{2+}$ is :
1. ${\mathrm{Li}}^{+}<{\mathrm{K}}^{+}<{\mathrm{Mg}}^{2+}<{\mathrm{Al}}^{3+}$
2. ${\mathrm{Al}}^{3+}<{\mathrm{Mg}}^{2+}<{\mathrm{K}}^{+}<{\mathrm{Li}}^{+}$
3. ${\mathrm{Li}}^{+}<{\mathrm{Al}}^{3+}<{\mathrm{Mg}}^{2+}<{\mathrm{K}}^{+}$
4. ${\mathrm{Li}}^{+}<{\mathrm{K}}^{+}<{\mathrm{Mg}}^{2+}<{\mathrm{Al}}^{3+}$

Select the correct relation 
1. ${\mathrm{IE}}_1\left(\mathrm{Cu}\right)<{\mathrm{IE}}_1\left(\mathrm{Zn}\right) \mathrm{but} {\mathrm{IE}}_2\left(\mathrm{Cu}\right)>{\mathrm{IE}}_2\left(\mathrm{Zn}\right)$
2. ${\mathrm{IE}}_1\left(\mathrm{Cu}\right)<{\mathrm{IE}}_1\left(\mathrm{Zn}\right) \mathrm{and} {\mathrm{IE}}_2\left(\mathrm{Cu}\right)<{\mathrm{IE}}_2\left(\mathrm{Zn}\right)$
3. ${\mathrm{IE}}_1\left(\mathrm{Cu}\right)>{\mathrm{IE}}_1\left(\mathrm{Zn}\right) \mathrm{and} {\mathrm{IE}}_2\left(\mathrm{Cu}\right)>{\mathrm{IE}}_2\left(\mathrm{Zn}\right)$
4. None

Consider the following conversions
$\left(\mathrm{i}\right)O\left(g\right)+e^{-}\to {\mathrm{O}}^{-}\left(\mathrm{g}\right) ;∆{\mathrm{H}}_1$
$\left(\mathrm{ii}\right) \mathrm{F}\left(\mathrm{g}\right)+{\mathrm{e}}^{-}\to {\mathrm{F}}^{-} ; ∆{\mathrm{H}}_2$
$\left(\mathrm{iii}\right) \mathrm{Cl}\left(\mathrm{g}\right)+{\mathrm{e}}^{-}\to {\mathrm{Cl}}^{-}\left(\mathrm{g}\right) ; ∆{\mathrm{H}}_3$
$\left(\mathrm{iv}\right) {\mathrm{O}}^{-}\left(\mathrm{g}\right)+{\mathrm{e}}^{-}\to {\mathrm{O}}^{2-}\left(\mathrm{g}\right) ; ∆{\mathrm{H}}_4$
According to the given information, the incorrect statement is:
1. $∆{\mathrm{H}}_3$ is more negative than $∆{\mathrm{H}}_1$ and $∆{\mathrm{H}}_2$
2. $∆{\mathrm{H}}_1$ is less negative than $∆{\mathrm{H}}_2$
3. $∆{\mathrm{H}}_1$,$∆{\mathrm{H}}_2$ and $∆{\mathrm{H}}_3$ are negative $∆{\mathrm{H}}_4$ is positive
4. $∆{\mathrm{H}}_1$ and $∆{\mathrm{H}}_3$ are negative whereas $∆{\mathrm{H}}_2$ and $∆{\mathrm{H}}_4$ are positive

What is the shielding constant experienced by a 3d electron in the Br (35)-atom?
1. 21.15
2. 20.80
3. 15.65
4. None of these

Consider the following elements with their electronegativity value 
Elements                 :      A       B       C       D
Electronegativity      :    3.77  1.12   2.25  3.10
Incorrect statement is :
1. AOH is more acidic than DOH
2. BOH is more basic than COH
3. 'AB' molecule is predominantly ionic.
4. 'D-OH' bond is more weaker than 
    'B-OH' bond in polar solvent

The value of four quantum number for the last electron of atom of element 'X' are n = 7 , l  =1, m = +1 and s = $+\frac{1}{2} or -\frac{1}{2}$ and  value of spin magnetic moment for element 'X' is zero
The incorrect statement regarding element 'X' is :
1. Element 'X' belongs to 18th group
2. Number of unpaired electrons in element 'X' is zero
3. Atomic number of element 'X' is 118
4. 'X' is representative element 

If the difference in atomic size of :
Na – Li = x                   K – Na = y                Fr – Cs = z
Then correct order will be:-
1. x = y = z 
2. x > y > z 
3. y > x > z 
4. x < y << z

Oxidising power of chlorine in aqueous solution can be determined by the parameters indicated below $\frac{1}{2}C{l}_2\left(g\right)\stackrel{\frac{1}{2}∆diss H^{⊝}}{\to }Cl\left(g\right)\stackrel{∆E_A{H}^{⊝}}{\to }C{l}^{-}\left(g\right)\stackrel{{∆}_{hyd}{H}^{⊝}}{\to }C{l}^{-}\left(aq\right)$
The energy involved in the conversion of $\frac{1}{2}C{l}_2\left(g\right) to C{l}^{-}\left(aq\right)$
using the data $\left({∆}_{\mathrm{diss}}{\mathrm{H}}_{{\mathrm{Cl}}_2}^{⊝}=240 \mathrm{kJ} {\mathrm{mol}}^{-1}, {∆}_{\mathrm{EA}}{\mathrm{H}}_{\mathrm{Cl}}^{⊝}=-349 \mathrm{kJ} {\mathrm{mol}}^{-1}, {∆}_{\mathrm{hyd}}{\mathrm{H}}_{\mathrm{Cl}}^{⊝}=-381 \mathrm{kJ} {\mathrm{mol}}^{-1}\right)$
1. +152 $\mathrm{kJ} {\mathrm{mol}}^{-1}$
2. -610 $\mathrm{kJ} {\mathrm{mol}}^{-1}$
3. -850 $\mathrm{kJ} {\mathrm{mol}}^{-1}$
4. +120 $\mathrm{kJ} {\mathrm{mol}}^{-1}$

Following statement regarding the periodic treads of chemical reactivity odf the alkali metals and the halogens are given, which of these statements give the correct picture?
1. The reactivity decreases in the alkali metals but increase in the halogens with increase in Atomic numbers down the groups
2. in both the alkali metals and the halogens the chemical reactivity decrease with increase in atomic numbers down the group
3. Chemical reactivity increases with decrease in atomic numbers down the group in both the alkali metals and halogens
4. In alkali metals the reactivity increases but in the halogens it deacrease4 with increase in atomic down the group

The atomic numbers of vanadium (V), chromium (Cr), manganese (Mn) and iron (Fe) are, respectively 23, 24, 25 and 26. Which one of these may be expected to have the highest second ionization enthalpy?
1. V 
2. Cr 
3. Mn 
4. Fe

Incorrect order among the following is:-
1. Electronegativity – P < N < O < F 
2. I^st ionisation potential – B < Be < O < N
3. Basic property – MgO > CaO > FeO > Fe₂O₃
4. Reactivity – Be < Li < K < Cs