Periodic Table & Periodicity

PERIODIC TABLE & PERIODICITY

CLASS : XI | TARGET : NEET (UG)

PRACTICE TEST PAPER

Max. Marks : 180 Max. Time : 1 Hr.

Important Instructions :
1. The test duration is 1 hour and maximum marks 180.
2. The test consists 45 SCQ questions 4 marks each
3. 1 mark will be deducted for incorrect answer. No deduction of marks from the total score will be made for
an un-attempted question.
SINGLE CHOICE QUESTIONS

1. The elements which exhibit both vertical and horizontal similarities are :
(1) inert gas elements (2) representative elements
(3) transition elements (4) none of these

2. Of the following pairs, the one containing examples of metalloid elements is :

(1) B and Al (2) Ga and Ge (3) Al and Si (4) As and Sb

3. Which of the following is the wrong statement ?

(1) All the actinide elements are radioactive.
(2) Alkali and alkaline earth metals are s-block elements.
(3) Pnicogens and halogens are p-block elements.
(4) The first member of the lanthanide series is lanthanum.

4. Atomic number of 15, 33, 51 represents the following family :

(1) carbon family (2) nitrogen family (3) oxygen family (4) None of these

5. In a given energy level, the order of penetration effect of different orbitals is :

(1) f < p < d < s (2) s < p < d < f (3) f < d < p < s (4) s = p = d = f

6. Which of the following is correct order of Zeff :

(1) I– > I > I+ (2) Mg2+ > Na+ > F– (3) P5+ < P3+ (4) Li > Be >B

7. In Sodium atom on 3s electron the screening is due to :

(1) 3s2, 3p6 (2) 4s1 (3) 1s2, 2s2, 2p6 (4) 3s1

8. Which of the following elements can have negative oxidation states.

(1) Al (2) Ca (3) Fe (4) B
9. What is correct order of reducing capacity :
(1) Ye2+ > Sn2+ > Pb2+ (2) Ye2+ < Sn2+ < Pb2+ (3) Ye2+  Sn2+  Pb2+ (4) Pb2+ > Ye2+ > Sn2+

10. Inert pair effect is observed in elements of which block :

(1) s (2) p (3) d (4) f

11. Which of the following order of radii is correct :

(1) Li < Be < Mg (2) H+ < Li+ < H– (3) O < F < Ne (4) Li < Na < K < Cs < Rb

12. The lanthanide contraction refers to :

(1) radius of the series. (2) valence electrons of the series.
(3) the density of the series. (4) electronegativity of the series.
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Periodic Table & Periodicity
13. Which of the following statement is correct with respect to the property of elements in the carbon family
with an increase in atomic number, their :
(1) Atomic size increases (2) Ionization energy increases
(3) Metallic character decreases (4) Stability of + 4 oxidation state increases

14. Which group of atoms have nearly same atomic radius :

(1) Na, K, Rb, Cs (2) Li, Be, B, C (3) Fe, Co, Mn (4) F, Cl, Br, I
15. The incorrect order of radius is/are :
(1) Cu– > Cu > Cu+ (2) Sc3+ > K+ > S2– (3) Ni < Cu < Zn (4) All of these

16. The second ionization enthalpies of elements are always higher than their first ionization enthalpies
because:
(1) cation formed always have stable half filled or completely filled valence shell electron configuration.
(2) it is easier to remove electron from cation.
(3) ionization is an endothermic process.
(4) the cation is smaller than its parent atom.

17. A large difference between the third and fourth ionization energies indicates the presence of :
(1) 4 valence electrons in an atom (2) 5 valence electrons in an atom
(3) 3 valence electrons in an atom (4) 2 valence electrons in an atom

18. The ionization enthalpy will be highest when the electron is to be removed from .............. if other factors
are equal : 
(1) s-orbital (2) p-orbital (3) d-orbital (4) f-orbital

19. The atomic number of Vanadium (V), Chromium (Cr), Manganese (Mn) and Iron (Fe) are respectively
23, 24, 25 and 26 which one of these may be expected to have the highest second Ionization enthalpy.
(1) V (2) Cr (3) Mn (4) Fe

20. For which of the following species 2nd IE < 1st IE

(1) Be (2) Ne (3) Na+ (4) None of these

21. With reference to 1st IP which are correct.

(1) Li < C (2) O < N (3) Be < N < Ne
(1) a, b only (2) b, c only (3) a, c only (4) a, b & c

22. Values of 1st four ionisaiton energies (kJ/mol) of an element are respectively 496, 4563, 6913, 9541 ;
the electronic configuration of that element can be.
(1) 1s2, 2s1 (2) 1s2 2s2 2p1 (3) 1s2, 2s2, 2p6 3s1 (4) (3) and (2) both

23. Which one of the following statements is correct ?

(1) The elements having large negative values of electron gain enthalpy generally act as strong
oxidising agents.
(2) The elements having low values of ionisation enthalpies act as strong reducing agents.
(3) The formation of S2–(g) from S(g) is an endothermic process.
(4) All of these.

24. For magnitude of electron gain enthalpy of chalcogens and halogens, which of the following options is
correct?
(1) Br > F (2) S > F (3) O < Cl (4) S < Se

25. The correct order of electron gain enthalpy (most endothermic first and most exothermic last) is :
(1) Be < B < C < N (2) Be < N < B < C (3) N < Be < C < B (4) N < C < B < Be
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Periodic Table & Periodicity
N0
26. atoms of X (g) are converted into X– (g) by absorbing E1 energy. 2N0 atoms of X (g) are converted
2
into X–(g) by releasing E2 energy. Calculate ionisation enthalpy and electron gain enthalpy of X(g) per
atom.
2E1 E E 2E
(1) I.E. = , eqH = – 2 (2) I.E. = – 2 , eqH = 1
N0 2N0 2N0 N0
E1 E2 N0 2N0
(3) I.E. = , eqH = – (4) I.E. = , H=–
2N0 2N0 2E1 eq E2

27. The formation of the oxide ion, O2–(g), from oxygen atom requires first an exothermic and then an
endothermic step as shown below :
O(g) + e– —O–(g) ; egH = – 141 kJmol–1
O–(g) + e– —O2–(g) ; egH = + 780 kJmol–1
Thus process of formation of O2– in gas phase is unfavourable even though O2– is isoelectronic with
neon. It is due to the fact that :
(1) oxygen is more electronegative.
(2) addition of electron in oxygen results in larger size of the ion.
(3) electron repulsion outweighs the stability gained by achieving noble gas configuration.
(4) O– ion has comparatively smaller size than oxygen atom.
28. The properties which are not common to both groups 1 and 17 elements in the periodic table are :
(1) Elelctropositive character increase down the gorups.
(2) Reactivity decrease from top to bottom in these groups.
(3) Atomic radii increase as the atomic number increase.
(4) Electronegativity decrease on moving down a group.
29. The correct set of decreasing order of electronegativity is :
(1) Li, H, Na (2) Na, H,Li (3) H, Li, Na (4) Li, Na, H
30. Which of the following is most electronegative in p-block elements
(1) Oxygen (2) Chlorine (3) Fluorine (4) Phosphorus
31. The IP1, IP2, IP3, IP4 and IP5 of an element are 7.1, 14.3, 34.5, 46.8, 162.2 eV respectively. The element
is likely to be
(1) Na (2) Si (3) F (4) Ca

32. IE1 and IE2 of Mg are 178 and 348 K, cal mol–1. The enthalpy required for the reaction Mg —Mg2+ +
2e– is
(1) +170 K. cal (2) +526 K.cal (3) –170 K.cal (4) –526 K.cal
33. The correct order of decreasing first ionization energy is :
(1) Si > Al > Mg > Na (2) Si > Mg > Al > Na (3) Al > Si > Mg > Na (4) none of these
34. In which of the following configuration, there will be large difference between second and third
ionisation energies ?
(1) 1s2, 2s2, 2p6,3s1 (2) 1s2, 2s2, 2p6,3s2, 3p1 (3) 1s2, 2s2, 2p6,3s2, 3p6 (4) 1s2, 2s2, 2p6,3s2
35. Elements which occupied position in the Lother Maeyer curve, on the peaks, were :
(1) Alkali metals (2) Highly electro positive elements
(3) Elements having large atomic volume (4) All
36. Which of the following is not isoelectronic series ?
(1) Cl–, P3–, Ar (2) N3–, Ne, Mg2+ (3) B3+, He, Li+ (4) F–, S2–, N3–

37. Correct orders of 1st ionisation energies are :

(i) Li < B < Be < C (ii) O < N < F (iii) Be < N < Ne
(1) (i), (ii) (2) (ii),(iii) (3) (i),(iii) (4) (i),(ii),(iii)
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Periodic Table & Periodicity
38. Which is a true statement ?
(1) Larger is the value of ionisation energy easier is the formation of cation.
(2) Larger is the value of electron affinity easier is the formation of anion.
(3) Larger is the value of ionisation energy as well as electron affinity the smaller is the electronegativity
of atom.
(4) Larger is the Zeff larger is the size of atom.

1 2 3 4 5
39. HC  C– CH  CH – CH3 Which carbon atom will show minimum electronegativity :
(1) Fifth (2) Third (3) First (4) Second

40. Arrange F, C, N, O in the decreasing order of electronegativity :

(1) O > F > N > C (2) F > N > C > O (3) C > F > N > O (4) F > O > N > C

41. Among O,C,F,Cl,Br the correct order of increasing atomic radii is :

(1) F < O < C < Cl < Br (2) F < C < O < Br < Cl
(3) F < Cl < Br < O < C (4) C < O < F < Cl < Br

42. The values of IE(I), IE(II), IE(III), and IE(IV),of an atom are respectively 7.5 eV, 25.6 eV, 48.6 eV and
170.6 eV. The electronic configuration of the atom will be :
(1) 1s2, 2s2, 2p6, 3s1 (2) 1s2, 2s2, 2p6, 3s2, 3p1
(3) 1s , 2s , 2p , 3s , 3p
2 2 6 2 3
(4) 1s2, 2s2 , 2p6, 3s2

43. The first (IE1) and second (IE2) ionization energies (kJ/mol) of a few elements designated by Roman
numerals are given below. Which of these would be an alkali metal ?
IE1 IE2 IE1 IE2
(1) I 2372 5251 (2) II 520 7300
(3) III 900 1760 (4) IV 680 7800

44. In the formation of a chloride ion, from as isolated gaseous chlorine atom, 3.8 eV energy is released,
which would be qual to :
(1) Electron affinity of Cl– (2) Ionisation potential of Cl
(3) Electronegativity of Cl (4) Ionisation potential of Cl–

45. Ionisation potential of Na would be numerically the same as :

(1) electron affinity of Na+ (2) electronegativity of Na+
(3) electron affinity of He (4) ionisation potential of Mg

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