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For electron affinity of halogens, which of the following is correct?
1. Br > F
2. F > Cl
3. Br > Cl
4. F > I

Which of the following has the highest electron affinity?
1. F^–
2. O^–
3. O
4. Na

Most basic oxide is
1. N₂O₃
2. N₂O₅
3. Bi₂O₅
4. Bi₂O₃

Which of largest in size?
1. Li⁺(aq)
2. Cs⁺(aq)
3. Li⁺(g)
4. Cs⁺(g)

The correct order of 3rd ionisation potential of Na, Mg, Al and Si is
1. Si > Al > Mg > Na
2. Mg > Si > Al > Na
3. Mg > Na > Si > Al
4. Mg > Na > Al > Si

Which pair has largest size difference?
1. Na and Na⁺
2. Na and K
3. Cl and Cl^–
4. Mg and Mg⁺

An element whose IUPAC name is ununtrium (Uut) belongs to:
1. s-block element
2. p-block element
3. d-block element
4. Transition element

The atomic species that has the maximum ionization energy is : 

If the ionic radii of K⁺ and F^- are nearly the same (i.e., 1.34 $\stackrel{\circ }{\mathrm{A}}$), then the atomic radii of K and F respectively are:
(1) 1.34 $\stackrel{\circ }{\mathrm{A}}$, 1.34 $\stackrel{\circ }{\mathrm{A}}$
(2) 0.72 $\stackrel{\circ }{\mathrm{A}}$, 1.96 $\stackrel{\circ }{\mathrm{A}}$
(3) 1.96 $\stackrel{\circ }{\mathrm{A}}$, 0.72 $\stackrel{\circ }{\mathrm{A}}$
(4) 1.96 $\stackrel{\circ }{\mathrm{A}}$, 1.34 $\stackrel{\circ }{\mathrm{A}}$

Which is the correct order of ionization energies?
(1) F^->F>Cl^->Cl
(2) F>Cl>Cl^->F^-
(3) F^->Cl^->Cl>F
(4) F^->Cl^->F>Cl

X_(g) $\to$X⁺_(g) + e^-, $∆$H=+720 KJ 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

Match the correct ionisation enthalpies and electron gain enthalpies of the
following elements.
Elements                                 $∆{\mathrm{H}}_1$                  $∆{\mathrm{H}}_2$                   ${∆}_{\mathrm{eg}}\mathrm{H}$
(i) Most reactive non metal      A.419                 3051                     -48
(ii) Most reactive metal            B. 1681               3374                     -328
(iii) Least reactive element        C. 738                 1451                      -40
(iv) Metal forming binary halide  D. 2372               5251                      +48
(1) (i)$\Rightarrow$A, (ii)$\Rightarrow$B, (iii)$\Rightarrow$C, (iv)$\Rightarrow$D
(2) (i)$\Rightarrow$B, (ii)$\Rightarrow$A, (iii)$\Rightarrow$D, (iv)$\Rightarrow$C
(3) (i)$\Rightarrow$D, (ii)$\Rightarrow$C, (iii)$\Rightarrow$A, (iv)$\Rightarrow$B
(4) (i)$\Rightarrow$C, (ii)$\Rightarrow$D, (iii)$\Rightarrow$B, (iv)$\Rightarrow$A

The electronic configuration of four elements are :
(I) [Kr]5s¹
(II) [Rn]5f¹⁴6d¹7s²
(III) [Ar]3d¹⁰4s²4p⁵
(IV) [Ar]3d⁶4s²
Consider the following statements :
(i) I Shows variable oxidation state
(ii) II is a d-block element
(iii) The compound formed between I and III is covalent
(iv) IV shows single oxidation state
Which statement is True (T) or False (F)?
1. FTFF
2. FTFT
3. FFTF
4. FFFF

Which of the following electronic configuration represents a sudden large gap
between the values of second and third ionisation energies of an element?
(1) 1s², 2s²2p³
(2) 1s², 2s²2p⁶, 3s²3p³
(3) 1s², 2s²2p⁶, 3s²3p¹
(4) 1s², 2s²2p⁶, 3s²