Consider the following statements:

(I) Rutherford name was associated with the development of periodic table.

(II) A metal M having electronic configuration 1s2, 2s2, 2p2, 3s2, 3d10, 4s1 is d-block element.

(III) Diamond is not an element.

(IV) The electronic configuration of the most electronegative elements is 1s2, 2s2, 2p5, and select the correct one from the given codes.

(A) I, II, IV                                      (B) I, II, III, IV

(C) II, IV                                         (D) I, III, IV

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There are four elements 'p', 'q', 'r' and 's' having atomic number Z-1, Z, Z+1 and Z+2 respectively. If there element 'q' is an inert gas, select the correct answers from the following statements.

(i) 'p' has most negative electron gain enthalpy in the respective period.

(ii) 'r' is an alkali metal.

(iii) 's' exists in +2 oxidation state.

(A) (i) and (ii)                      (B) (ii) and (iii)

(C) (i) and (iii)                     (D) (i), (ii) and (iii)

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Which of the following orders is correct for the size?

(1) Mg2+<Na+<F-Al

(2) Al3+<Mg2+Li+<K+

(3) Fe4+<Fe3+<Fe2+<Fe

(4) Mg>Al>Si>P

(A) (1), (2) & (3)                          (B) (2), (3) & (4)

(C) (1), (3) & (5)                          (D) (1), (2), (3) & (4)

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Which of the following orders are correct for the ionization energies?

(1)  Ba < Sr < Ca                       (2) S2-<S <S2+

(3) C < O<N                            (4) Mg < Al < Si

(A) 1, 2 and 4                              (B) 1, 3 and 4

(C) 1, 2 and 3                              (D) 1, 2, 3 and 4

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Ionization Energy (IE)
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The electron gain enthalpies of halogens in kJ mol-1 are as given below.

F =-332, Cl =-349, Br =-234, I =-295.

The least negative value for F as compared to that of Cl is due to:

(A) Strong electron-electron repulsions in the compact 2p-subshell of F.

(B) Weak electron-electron repulsions in the bigger 3p-subshell of Cl.

(C) Smaller electronegativity value of F than Cl.

(D) (A) & (B) both 

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Electron Affinity (EA)
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Which of the following statements are correct ?

(i) Generally the radius trend and the ionization energy trend across a period are exact opposites.

(ii) Electron affinity values of elements may be exothermic (negative) or endothermic (positive)

(iii) The first ionization energy of sulphur is higher than that of phosphorus ?

(iv) Te2->I->Cs+>Ba2+ represents the correct decreasing order of ionic radii.

(A) (i), (iii) and (iv)                          (B) (ii), (iii) and (iv)

(C) (i), (ii) and (iv)                           (C) (i), (ii) and (iii)  

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Which of the following statements is not correct?

(A) The first ionization energies (in KJ mol-1) of carbon, silicon, germanium, tin, and lead are 1086, 786, 761, 708 and 715 respectively.

(B) Down the group, electronegativity decreases from B to Tl in boron family.

(C) Among oxides of the elements of carbon family, CO is neutral, GeO is acidic and SnO is amphoteric.

(D) The 4f- and 5f- inner transition elements are placed separately at the bottom of the periodic table to maintain its structure.

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Ionization Energy (IE)
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The correct order of acidic strength is :

(A) Cl2O7>SO2>P4O10                   (B) CO2>N2O5>SO3

(C) Na2O>MgO>Al2O3                   (D) K2O>CaO>MgO

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Nature of Compound
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Which of the following orders is correct?

(A) F>N>C>Si>Ga -non-metallic character.

(B) F>Cl>O>N - oxidising property.

(C) C<Si>P>N - electron affinity value.

(D) All of these.

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Nature of Compound
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If the same element is forming oxides in different oxidation states then :

(A) that oxides will be neutral in nature in which element will be in its highest oxidation state.

(B) that oxide will be highest acidic in nature in which element will be in this highest oxidation state.

(C) that oxide will be amphoteric in nature in which element will be in its highest oxidation state.

(D) that oxide will be highly basic in nature in which element will be in its highest oxidation state.

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Nature of Compound
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