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Which of the following arrangements shows the correct order of decreasing paramagnetism?
1. N > Al > O > Ca
2. N > O > Al > Ca
3. O > N > Al > Ca
4. O > N > Ca > Al

The outer electronic structure of lawrencium (atomic number 103) is:
1. $\mathrm{Rn} 5 {\mathrm{f}}^{13}7s^{2}7p^2$
2. $\mathrm{Rn} 5 {\mathrm{f}}^{13}6d^{2}7s^{1}7p^2$
3. $\mathrm{Rn} 5 {\mathrm{f}}^{14}7s^{1}7p^2$
4. $\mathrm{Rn} 5 {\mathrm{f}}^{14}6d^{1}7s^2$

Which of the following pairs of molecules have the almost identical bond dissociation energy?
1. F₂ and H₂
2. N₂ and CO
3. F₂ and I₂
4. HF and O₂

Zn and Cd metals do not show variable valency because:
1. They have only two electrons in the outermost subshells
2. Their d-subshells are completely filled
3. Their d-subshells are partially filled
4. They are relatively soft metals

To which group does the element named ununtrium (Uut) belong according to the IUPAC naming convention?
1. s-block element
2. p-block element
3. d-block element
4. Actinoids

Which of the following anion has the smallest radius?
1. H^-
2. F^-
3. Cl^-
4. Br^-

The correct order of increasing atomic radius of the following elements is:
1. S < O < Se < C
2. O < C < S < Se
3. O < S < Se < C
4. C < O < S < Se

The correct order of atomic/ionic radii is:
1. Sc > Ti > V > Cr
2. Co > Ni > Cu > Zn
3. S^2- > Cl^- > O^2- > N^3-
4. None of these

The first, second and third ionisation energies (E1, E2 and E3) for an element are 7 eV, 12.5 eV and 42.5 eV respectively. The most stable oxidation state of the element will be:
1. +1
2. +4
3. +3
4. +2

The order of ionisation potential between He⁺ ion and H-atom (both species are in gaseous state) is:
1. I.P. (He⁺) = I.P. (H)
2. I.P. (He⁺) < I.P. (H)
3. I.P. (He⁺) > I.P. (H)
4. cannot be compared

Second ionization potential of Li, Be and B is in the order:
1. Li > Be > B
2. Li > B > Be
3. Be > Li > B
4. B > Be > Li

Which of the following atomic species has maximum electron affinity?
1. O
2. S
3. Se
4. Te

The correct order of I.E.₂. is:
1. Na > F > O > N
2. O > F > Ne > N
3. Ne > O > F > N
4. O > Ne > F > N

Which of the following processes involves absorption of energy?
1. $\mathrm{S}\left(\mathrm{g}\right)+{\mathrm{e}}^{-}\to {\mathrm{S}}^{-}\left(\mathrm{g}\right)$
2. ${\mathrm{S}}^{-}+{\mathrm{e}}^{-}\to {\mathrm{S}}^{2-}\left(\mathrm{g}\right)$
3. $\mathrm{Cl}\left(\mathrm{g}\right)+{\mathrm{e}}^{-}\to {\mathrm{Cl}}^{-}\left(\mathrm{g}\right)$
4. None of these

Arrange N, O and S in order of decreasing electron affinity:
1. S > O > N
2. O > S > N
3. N > O > S
4. S > N > O

Which of the following order is incorrect?
1. Electronegativity of central atom : ${\mathrm{CF}}_4>{\mathrm{CH}}_4>{\mathrm{SiH}}_4$
2. Hydration energy : ${\mathrm{Al}}^{3+}>{\mathrm{Be}}^{2+}>{\mathrm{Mg}}^{2+}>{\mathrm{Na}}^{+}$
3. Electrical conductance : ${\mathrm{F}}_{(\mathrm{aq}.)}^{-}>{\mathrm{Cl}}_{(\mathrm{aq}.)}^{-}>{\mathrm{S}}_{(\mathrm{aq}.)}^{2-}$
4. Magnetic moment : ${\mathrm{Ni}}^{4+}>{\mathrm{V}}^{3+}>{\mathrm{Sr}}^{2+}$

A compound contains three elements A, B and C, if the oxidation number of A = +2, B = +5 and C = -2, the possible formula of the compound is:
1. ${\mathrm{A}}_3{(\mathrm{B}}_{}$₄C)2
2. ${\mathrm{A}}_3{(\mathrm{BC}}_{}$₄)2
3. ${\mathrm{A}}_2{(\mathrm{BC}}_{}$₃)2
4. ${\mathrm{ABC}}_2$

Cosider the following four elements, which are represented according to long form of periodic table. 

Here W, Y and Z are left, up and right elements with respect to the element 'X' and 'X' belongs to 16th group and 3rd period. Then according to given information the incorrect statement regarding given elements is:
1. Maximum electronegativity : Y
2. Maximum catenation property : X
3. Maximum electron affinity : Z
4. Y exhibits variable covalency

What is the atomic number of the element with the maximum number of unpaired 4p electrons?
1. 33
2. 26
3. 23
4. 15

The electronic configuration of four elements are:

Consider the following statements:

Which statement is True (T) or False (F)?
1. FTFF
2. FTFT
3. FFTF
4. FFFF

The set representing the correct order of ionic radius is:
1. ${\mathrm{Na}}^{+}>{\mathrm{Mg}}^{2+}>{\mathrm{Al}}^{3+}>{\mathrm{Li}}^{+}>{\mathrm{Be}}^{2+}$
2. ${\mathrm{Na}}^{+}>{\mathrm{Li}}^{+}>{\mathrm{Mg}}^{2+}>{\mathrm{Al}}^{3+}>{\mathrm{Be}}^{2+}$
3. ${\mathrm{Na}}^{+}>{\mathrm{Mg}}^{2+}>{\mathrm{Li}}^{+}>{\mathrm{Al}}^{3+}>{\mathrm{Be}}^{2+}$
4. ${\mathrm{Na}}^{+}>{\mathrm{Mg}}^{2+}>{\mathrm{Li}}^{+}>{\mathrm{Be}}^{2+}$

If the ionic radii of K⁺ and F^- are nearly the same (i.e., 1.34 Å), then the atomic radii of of K and F respectively are:
1. 1.34 Å, 1.34 Å
2. 0.72 Å, 1.96 Å
3. 1.96 Å, 0.72 Å
4. 1.96 Å, 1.34 Å

Incorrect order of ionic size is:
1. ${\mathrm{La}}^{3+}>{\mathrm{Gd}}^{3+}>{\mathrm{Eu}}^{3+}>{\mathrm{Lu}}^{3+}$
2. ${\mathrm{V}}^{2+}>{\mathrm{V}}^{3+}>{\mathrm{V}}^{4+}>{\mathrm{V}}^{5+}$
3. ${\mathrm{Tl}}^{+}>{\mathrm{In}}^{+}>{\mathrm{Sn}}^{2+}>{\mathrm{Sb}}^{3+}$
4. ${\mathrm{K}}^{+}>{\mathrm{Sc}}^{3+}>{\mathrm{V}}^{5+}>{\mathrm{Mn}}^{7+}$

${\mathrm{X}}_{\left(\mathrm{g}\right)}\to {{\mathrm{X}}^{+}}_{\left(\mathrm{g}\right)}+{\mathrm{e}}^{-}, △\mathrm{H}=+720 \mathrm{kJ} {\mathrm{mol}}^{-1}$
Calculate the amount of energy required to convert 110 mg of 'X' atom in gaseous state into X⁺ ion. (Atomic wt. for X=7 g/mol)
1. 10.4 kJ
2. 12.3 kJ
3. 11.3 kJ
4. 14.5 kJ

The third ionization energy is maximum for:
1. Nitrogen
2. Phosphorus
3. Aluminium
4. Boron

First three ionisation energies (in kJ/mol) of three representative elements are given below:
Element   IE1     IE2    IE3
P           495.8  4562  6910
Q          737.7  1451  7733
R           577.5  1817  2745
Then incorrect option is :
1. Q: Alkaline earth metal
2. P: Alkali metals
3. R: p-block element
4. They belong to same period