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The tenth element in the periodic table resides in:
1. the second period
2. the fourth period
3. the fifth period
4. the eight period

Which of the following order is not in accordance with the property stated against it?                                                                                                      
1. F₂ > Cl₂ > Br₂ > l₂ Oxidising Power
2. Hl > HBr >HCl >HF Acidic property in water
3. F₂ > Cl₂ > Br₂ > l₂ Electronegativity
4. F₂ > Cl₂ > Br₂ > l₂ Bond dissociation energy

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

The most non-metallic element among the following is:
1. Be
2. B
3. Mg
4. Al

Element ₅₈Ce belongs to:
1. s-block elements
2. p-block elements
3. d-block elements
4. f-block elements

How does the shielding effect of d-electrons compare to that of other electrons?
1. Weaker than s-electrons.
2. Stronger than s-electrons.  
3. Same as s-electrons.
4. Same as p-electrons.

Correct statement regarding transuranic elements is :
1. They have higher atomic number than uranium.
2. They are lighter than uranium.
3. They have lower atomic number than uranium.
4. They have same atomic number as uranium.

General electronic configuration of outermost and penultimate shell of an atom is
(n - 1)s² (n - 1) p⁶ (n - 1)d^x ns². If n = 4 and x = 5, the number of proton in the nucleus is:
1. > 25
2. < 24
3. 25
4. 30

The maximum number of valence electrons possible for atoms in the second period of the periodic table is:
1. 18
2. 10
3. 8
4. 2

The element having atomic number 19, is:
1. an inert gas
2. a metal with oxidation number +1
3. a non-metal with oxidation number -3
4. a metal with oxidation number -3

Which of the following has the least density?
1. Na
2. Li
3. Mg
4. K

The order of basic character of given oxides is:
1. Na₂O > MgO > Al₂O₃ > CuO
2. MgO > Al₂O₃ > CuO > Na₂O
3. Al₂O₃ > MgO > CuO > Na₂O
4. CuO > Na₂O > MgO > Al₂O₃

The low melting point of manganese in the 1st transition series is due to:
1. strong metallic bond due to d¹⁰ configuration
2. weak metallic bond due to d⁵ configuration
3. weak metallic bond due to d⁷ configuration
4. none of the above

An element R forms the highest oxide R₂O₅. R belongs to:
1. 13th  group
2. 15th group
3. 16 th group
4. 2nd group

Transition elements exhibit variable oxidation states because they release electrons from the following orbits:
1. ns and np orbits
2. (n-1)d and ns orbits
3. (n-1)d orbits
4. ns orbits

In II period most acidic oxide is formed by:
1. F
2. N
3. Zn
4. Li

The outer electronic configuration of Gd (Atomic no. 64) is:
1. 4f³ 5d⁵6d²
2. 4f⁸ 5d¹⁰6d²
3. 4f⁴ 5d⁴6d²
4. 4f⁷ 5d¹6s²

Which of the following transition metal ions has the lowest density?
1. Copper
2. Nickel
3. Scandium
4. Zinc

Ionic radii are :
1. Inversely proportional to the effective nuclear charge.
2. Inversely proportional to the square of effective nuclear charge.
3. Directly proportional to the effective nuclear charge.
4. Directly proportional to the square of effective nuclear charge.

Which one is a metalloid?
1. Tin
2. Germanium
3. Sulphur
4. Carbon

Elements with an electronic configuration 1s²  2s²  2p⁶  3s²  3p⁶  3d¹⁰ 4s²  4p⁶  4d¹⁰  5s²  5p³ belong to the group :

General electronic configuration of the transition elements is given by:
1. ns²nd^1-10
2. ns²np⁶nd^1-10
3. (n-1)d^1-10np⁶
4. (n-1)d^1-10ns^1-2
 

Which among the following options is a nonmetal?

The alkali metals have:
1. highest ionization energy
2. largest atomic radii
3. highest density
4. highest electronegativity

Which of the following statement is correct with respect to the property of elements with increase in atomic number in carbon family.
1. Their metallic character decreases
2. The stability of +2 oxidation state increases
3. Their ionisation energy increases
4. Their atomic size decreases

The graph of the first ionization enthalpy versus atomic number is as follows:

Which of the following statements is correct?

The electric charge for electrode deposition of 1g equivalent of a substance is:
1. 1 ampere per second
2. 96,500 coulomb per second
3. 1 ampere for 1 hour
4. charge on 1 mole of electrons

The electronic configuration of chalcogens in their outermost shell is : 
1. ${\mathrm{ns}}^2{\mathrm{np}}^3$ $$ $$ $$    
2. ${\mathrm{ns}}^2{\mathrm{np}}^4$ $$ $$ $$     
3. ${\mathrm{ns}}^2{\mathrm{np}}^5$           
4. ${\mathrm{ns}}^2{\mathrm{np}}^6$

Match list-I with list II and select the correct answer using codes given below:
1. List-I Ions                                List-II Radius (in pm)
(I) Li⁺                                         (a) 216
(II) Na⁺                                      (b) 195
(III) Br^-                                      (c) 60
(IV) I^-                                        (d) 95
     Codes:
      I   II   III   IV
1.   a   b    d    c
2.   b   c    a    d
3.   c   d    b    a
4.   d   c    b    a 

Increasing order of the ionic radii and decreasing order of protons of the given isoelectric species is:-
(1) Ca⁺², K⁺, Cl^-, S^-2
(2)Cl^-, Ca⁺², K⁺, S^-2
(3)S^-2, Cl^-, Ca⁺², K⁺,
(4)None of the above

Allred Rochow's scale is related to:
 
1. Electronegativity, radius, and Z^*
2. Resonance energy of the molecule, ionisation potential and electron affinity.
3. Bond Polarity, diagonal relationship and periodicity.
4. None of the above.

Atomic radius of Be, O, C, N, B are respectively (in pm) :-
(1) 111, 66, 77, 74, 88
(2) 74, 84, 111, 77, 66
(3) 111, 88, 77, 74, 66
(4) 111, 66, 88, 77, 74

Ionic radii are : 
1. Directly proportional to square of effective nuclear charge.
2. Inversely proportional to effective nuclear charge .
3. Inversely proportional to square of effective nuclear charge .
4. Directly proportional to effective nuclear charge.

Which of the following orders of ionic radii is correctly represented?
1. H^->H>$H^{+}$
2. Na⁺>F^->O^2-
3. F^->O^2->Na⁺
4. N^3->Mg²⁺<Al³⁺

Identify the wrong statement in the following:
1. Amongst isoelectronic species, smaller the positive charge on the cation, smaller is the
ionic radius
2. Amongst isoelectronic species, greater the negative charge on the anion, larger is the
ionic radius
3. Atomic radius of the elements increases as one moves down the first group of the
Periodic Table
4. Atomic radius of the elements decreases as one moves across from left to right in the
2nd period of the Periodic Table

The correct order of increasing electron gain enthalpy with a negative sign for the elements O, S, F, and Cl is : 
1. Cl < F < S < O                   
2. O < S < F < Cl
3. F < S < O < Cl                   
4. S < O < Cl < F

For following steps
$$\begin{gathered} {\mathrm{M}}_{\left(\mathrm{g}\right)}\to {\mathrm{M}}_{\left(\mathrm{g}\right)}^{+}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{e}}^{-},<mspace\; width="1em"></mspace>∆\mathrm{H}=100\mathrm{eV} \\ {\mathrm{M}}_{\left(\mathrm{g}\right)}\to {\mathrm{M}}^{+2}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{\mathrm{e}}^{-},<mspace\; width="1em"></mspace>∆\mathrm{H}=250\mathrm{eV} \\ \mathrm{Which}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>\mathrm{not}<mspace\; width="1em"></mspace>\mathrm{correct}? \\ 1.<mspace\; width="1em"></mspace>{\mathrm{IE}}_1<mspace\; width="1em"></mspace>\mathrm{of}<mspace\; width="1em"></mspace>{\mathrm{M}}_{\left(\mathrm{g}\right)}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>100<mspace\; width="1em"></mspace>\mathrm{eV} \\ 2.<mspace\; width="1em"></mspace>\mathrm{IE}<mspace\; width="1em"></mspace>\mathrm{of}<mspace\; width="1em"></mspace>{\mathrm{M}}_{\left(\mathrm{g}\right)}^{+}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>150<mspace\; width="1em"></mspace>\mathrm{eV} \\ 3.<mspace\; width="1em"></mspace>{\mathrm{IE}}_2<mspace\; width="1em"></mspace>\mathrm{of}<mspace\; width="1em"></mspace>{\mathrm{M}}_{\left(\mathrm{g}\right)}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>250<mspace\; width="1em"></mspace>\mathrm{eV} \\ 4.<mspace\; width="1em"></mspace>{\mathrm{IE}}_2<mspace\; width="1em"></mspace>\mathrm{of}<mspace\; width="1em"></mspace>{\mathrm{M}}_{\left(\mathrm{g}\right)}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>150<mspace\; width="1em"></mspace>\mathrm{eV} \end{gathered}$$

An element whose IUPAC name is Ununtrium (Uut) belongs to:
1. s-Block elements                       
2. p-Block elements
3. d-Block elements                              
4. Inner transition elements .

Consider the following electronic configuration of an element (P) :
$\left[\mathrm{Xe}\right]4{\mathrm{f}}^{14}5{\mathrm{d}}^{1}6{\mathrm{s}}^2$
The correct statement about element 'P' is :
1. It belongs to the 6th period and the 1st group.
2. It belongs to the 6th period and the 2nd group.
3. It belongs to the 6th period and the 3rd group.
4. None of the above.

Consider the following information about element P and Q :
                        Period number            Group number
P                               2                                 15
Q                               3                                 2
Then formula of the compound formed by P and Q element is :
(1) PQ         
(2) $P_3{Q}_2$           
(3)$Q_3{P}_2$            
(4)$P{Q}_2$

In alkaline earth metals, the properties, from the following, that will increase from Be to Ba are-
(i) Atomic radius       
(ii) Ionisation energy       
(iii) Nuclear charge

Aqueous solutions of two compounds $M_1-O-H<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>M_2-O-H$ are prepared in two different beakers. If, the electronegativity of $M_1=3.4<mspace\; width="1em"></mspace>,<mspace\; width="1em"></mspace>M_2=1.2,<mspace\; width="1em"></mspace>O=3.5<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>H=2.1,$ then the nature of two solutions will be respectively:
(a) acidic, basic             (b) acidic, acidic
(c) basic, acidic             (d) basic, basic

The process requiring the absorption of energy is :
1. $F\to F^{-}$
2. $H\to H^{-}$
3. $Cl\to C{l}^{-}$
4. $O\to O^{2-}$

The correct order among the following options is: 
1. F > N > C > Si > Ga - Non-metallic character.
2. F > Cl > O >N - Oxidising property.
3. C < Si > P > N  - Electron affinity value.
4. All of the above.