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$\mathrm{The} \mathrm{first}, \mathrm{second} \mathrm{and} \mathrm{third} \mathrm{ionisation} \mathrm{energies} ({\mathrm{E}}_1, {\mathrm{E}}_2 \& {\mathrm{E}}_3)$
$\mathrm{for} \mathrm{an} \mathrm{element} \mathrm{are} 7\mathrm{eV}, 12.5\mathrm{eV} \mathrm{and} 42.\mathrm{eV} \mathrm{respectively}.$
$\mathrm{The} \mathrm{most} \mathrm{stable} \mathrm{oxidation} \mathrm{state} \mathrm{of} \mathrm{the} \mathrm{element} \mathrm{will} \mathrm{be} :$
$\left(\mathrm{a}\right) +1$
$\left(\mathrm{b}\right) +4$
$\left(\mathrm{c}\right) +3$
$\left(\mathrm{d}\right) +2$

The element having electronic configuration [Kr]4d¹⁰4f¹⁴, 5s²5p⁶, 6s² belongs to:
1. s-block
2. p-block
3. d-block
4. f-block

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

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

Consider the following electronic configuration of an element (P) :
                 [Xe]4f¹⁴5d¹6s² 
Then correct statement about element 'P' is :
1. It belongs to 6th period and 1st group
2. It belongs to 6th period and 2nd group
3. It belongs to 6th period and 3rd group
4. None of these

Which of the following graph is correct representation between atomic number (Z) and magnetic moment of d-block elements? [Outer electronic configuration : (n-1)d^xns^{1 or 2}]

If IUPAC name of an element is "unununium" then correct statement regarding element is:
1. It is a inner transition element
2. It belongs to 8th period in periodic table
3. It is transition element
4. It is a non-transition element

Which property decreases from left to right across the periodic table and increases from top to bottom?
(i) Atomic radius
(ii) Electronegativity
(iii) Ionisation energy
(iv) Metallic character
1. (i) only
2. (i), (ii) and (iii)
3. (i), (iii) and (iv)
4. (i) and (iv)
 

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
 

Which of the following metal is expected to have the highest third ionization enthalpy?
1. Cr(Z = 24)
2. V(Z = 23)
3. Mn(Z = 25)
4. Fe(Z = 26)

Second ionisation 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

The first four I.E. values of an element are 284, 412, 656 and 3210 kJ mol^-1. The number of valence electrons in the element are :
1. one
2. two
3. three
4. four

The first I.E. of Na, Mg, Al and Si are in the order :
1. Na < Mg < Al < Si
2. Na < Al < Mg <Si
 

Which of the following isoelectronic ion has the lowest ionization energy?
1. K⁺
2. Cl^-
3. Ca²⁺
4. S^2-

The ionization potentials of Li and K are 5.4 and 4.3 eV respectively. The ionization potential of Na will be:
1. 9.7 eV
2. 1.1 eV
3. 4.9 eV
4. cannot be calculated

Which of the following order is incorrect?
1. Electronegativity of central atom :CF₄ > CH₄ > SiH₄
2. Hydration energy : Al³⁺ > Be²⁺ > Mg²⁺ > Na⁺
3. Electrical conductance : ${\mathrm{F}}_{\left(\mathrm{aq}\right)}^{-} > {\mathrm{Cl}}_{\left(\mathrm{aq}\right)}^{-}>{\mathrm{S}}_{\left(\mathrm{aq}\right)}^{2-}$
4. Magnetic moment : Ni⁴⁺ > V³⁺ > Sr²⁺

Which of the following is arranged in order of increasing radius ?
1. K⁺ (aq) < Na⁺ (aq) < Li⁺(aq)
2. Na⁺(aq) < K⁺ (aq) < Li⁺ (aq)
3. K⁺(aq) < Li⁺(aq) < Na⁺(aq)
4. Li⁺(aq) < Na⁺(aq) < K⁺(aq)

To which of the following atom, the attachement of electron is most difficult ?
1. Radon
2. Nitrogen
3. Oxygen
4. Radium

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

Among the following configurations, the element which has the higher electron affinity is :
1. [Ne]3s¹3p²
2. [Ne]3s²3p⁵
3. [Ne]3s²3p4
4. [Ne]3s²3p⁶3d⁵4s¹

The increasing order of electron affinity of the electron configurations of element is :
(I) $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^5$
(II) $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^3$
(III) $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^5$
(IV) $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^1$
1. II < IV < III < I
2. I < II < III < IV
3. I < III < II < IV
4. IV < III < II < I

Second electron gain enthalpy :
1. is always negative
2. is always positive
3. can be positive or negative
4. is always zero

Which of the following represents correct order of electron affinity?
1. Cl > F > S > O
2. F > O > S > Cl
3. F > Cl > S > O
4. Cl > S > O > F

The process requiring absorption of energy is:
1.  $\mathrm{N}\to {\mathrm{N}}^{-}$
2. $\mathrm{F}\to {\mathrm{F}}^{-}$
3. $\mathrm{Cl}\to {\mathrm{Cl}}^{-}$
4. $\mathrm{H}\to {\mathrm{H}}^{-}$

The electronegativity of the following elements increases in the order :
1. C < N < Si < P
2. Si < P < C < N
3. N < C < P < Si
4. C < Si < N < P 

Which of the following electronic configuration represents a sudden large gap between the values of second and third ionisation energies of an element?
1. ${1\mathrm{s}}^2, 2{\mathrm{s}}^{2}2{\mathrm{p}}^3$
2.${1\mathrm{s}}^2, 2{\mathrm{s}}^{2}2{\mathrm{p}}^6, 3{\mathrm{s}}^{2}3{\mathrm{p}}^3$
3. ${1\mathrm{s}}^2, 2{\mathrm{s}}^{2}2{\mathrm{p}}^6,3{\mathrm{s}}^{2}3{\mathrm{p}}^1$
4. ${1\mathrm{s}}^2, 2{\mathrm{s}}^{2}2{\mathrm{p}}^6,3{\mathrm{s}}^2$

Element having highest I.P value is :
1. Ne
2. He
3. Be
4. N

Which of the following atomic species has maximum ionisation energy?
1. O^-
2. S^-
3. Se^-
4. Te^-