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#### Periodic Classification Of Elements frequently asked one mark questions

11th Standard

Reg.No. :
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Chemistry

Time : 00:40:00 Hrs
Total Marks : 75

Part - A

75 x 1 = 75
1. The first ionisation potential ofNa is 5.1 eY. The value of electron gain enthalpy is

(a)

+2.55 eV

(b)

-2.55 eV

(c)

-5.1 eV

(d)

-10.2 eV

2. Electronegativity of the following elements increases in the order

(a)

C, N, Si, P

(b)

N, Si, C, P

(c)

Si, P, C, N

(d)

P,Si, N, C

3. Consider the following elements: B, AI, Mg and K.

(a)

B >AI > Mg> K

(b)

Al > Mg > B > K

(c)

Mg >Al > K > B

(d)

K> Mg > AI> B

(1) inverse proportion to the effective nuclear charge
(2) inverse proportion to the square of the effective nuclear charge.
(3) direct proportion to the screening effect.
(4) direct proportion to the square of screening effect

(a)

1,2

(b)

1,3

(c)

2,3

(d)

2,4

5. The chemical symbol of carbon and cobalt are______

(a)

Ca and CO

(b)

Ca and Cl

(c)

C and CO

(d)

Cr and Cb

6. Consider the following statements.
(i) The chemical symbol of nickel is N.
(ii) An element is a material made up of different kind of atoms.
(iii) The physical state of bromine is liquid.
Which of the above statement is/are not correct?

(a)

(i) and (iii)

(b)

(iii) only

(c)

(ii) and (iii)

(d)

(i) and (ii)

7. Match the list-I and list-II using the correct code given below the list.

 List-I List -II A. Jewels 1. 1.Sodium chloride B. Bolts and cot 2. Copper C. Table salt 3. Gold D. Utensils 4. Iron
(a)
 A B C D 3 4 1 2
(b)
 A B C D 4 1 3 2
(c)
 A B C D 1 4 2 3
(d)
 A B C D 2 3 4 1
8. The law of triads is not obeyed by______

(a)

Ca, Sr, Ba

(b)

CI, Br, I

(c)

Li, Na, K

(d)

Be, B, C

9. The law of triads is obeyed by________

(a)

Fe, CO, Ni

(b)

C, N, O

(c)

He, Ne, Ar

(d)

AI, Si, P

10. Match the list-I and list-II using the code given below the list

 List-I List-II A.Law of triads 1.Chancourtois B.Law of octaves 2.Henry Moseley C.First periodic law 3.Newland D.Modem periodic law 4.Johann Dobereiner
(a)
 A B C D 4 3 1 2
(b)
 A B C D 3 4 2 1
(c)
 A B C D 1 3 4 2
(d)
 A B C D 2 3 1 4
11. Consider the following statements
(i) In Chancourtois classification, elements differed from each other in atomic weight by 16 or multiples of 16 fell very nearly on the same vertical line.
(ii) Mendeleev's periodic law is based on atomic weight.
(iii) Mendeleev listed the 117 elements known at that time and are arranged in the order of atomic numbers.
Which of the following statement is/are not correct?

(a)

(i) only

(b)

(ii) and (iii)

(c)

(iii) only

(d)

(i),(ii) ,(iii)

12. Which of the following elements were unknown at that time of Mendeleev?

(a)

Na, Mg

(b)

Fe, CO

(c)

K, Cu

(d)

Ga, Ge

13. Consider the following statements.
(i) Position of hydrogen could not be made clear.
(ii) Isotopes find correct place in Mendeleev's periodic table.
(iii) Mendeleev's periodic table could not explain the variable valencies of elements.
Which of the above statement is/are not correct?

(a)

(i) only

(b)

(i) and (iii)

(c)

(ii) only

(d)

(i), (ii), (iii)

14. According to modern periodic law, the physical and chemical properties of the elements are periodic functions of their_______

(a)

atomic volume

(b)

atomic numbers

(c)

atotnic weights

(d)

valency

15. Which period contain 32 elements?

(a)

Period 1

(b)

Period 4

(c)

Period 5

(d)

Period 6

16. There are horizontal rows of the periodic table known as_____

(a)

groups

(b)

periods

(c)

families

(d)

chalcogens

17. The shortest period contains______elements.

(a)

H, He

(b)

Li, Be

(c)

B,C

(d)

He, Ar

18. The longest form of periodic table was constructed by______

(a)

Dmitri Mendeleev

(b)

Henry Moseley

(c)

Lothar Meyer

(d)

Newlands

19. Match the list-land list-II using the correct code given below the list.

 List-I List-II A. Z = 100 1. Mendelevium B Z = 101 2. Lawrencium C. Z = 102 3. Fermium D. Z = 103 4. Nobelium
(a)
 A B C D 4 3 2 1
(b)
 A B C D 3 1 4 2
(c)
 A B C D 4 1 3 2
(d)
 A B C D 3 2 1 4
20. Which one of the following is the first transition series?

(a)

Sc

(b)

Zn

(c)

Ti

(d)

Cu

(a)

4th period

(b)

7th period

(c)

6th period

(d)

3rd period

22. Which one of the following is called halogen family?

(a)

Group 17

(b)

Group 16

(c)

Group 1

(d)

Group 2

23. Group 16 constitutes_____family.

(a)

halogen

(b)

nobel gas

(c)

chalcogen

(d)

alkali metals

24. Consider the following statements.
(i) The valency of the elements increases from left to right in a period.
(ii) Valency decreases from 7 to 1 with respect to oxygen.
(iii) The metallic character of the elements decreases across a period.
Which of the above statement is/are not correct?

(a)

(i) only

(b)

(ii) only

(c)

(i) and (iii)

(d)

(i) (ii) and (iii)

25. Match the list-I and list-II using the correct code given below the list.

 List-I List-II A. Li 1. 2,8,8,1 B. Na 2. 2,1 C. K 3. 2,8,18,18,8,1 D. Cs 4. 2,8,1
(a)
 A B C D 3 4 1 2
(b)
 A B C D 2 4 1 3
(c)
 A B C D 1 3 2 4
(d)
 A B C D 4 2 1 3
26. What will be the change in valency down the group in the periodic table?

(a)

increases

(b)

decreases

(c)

remains same

(d)

zero

27. Which one of the following is a metalloid?

(a)

N

(b)

P

(c)

Bi

(d)

Sb

28. Which one of the following is a metal?

(a)

N

(b)

Br

(c)

Bi

(d)

As

29. Match the list-I and list-II using the correct code given below the list.

 List-I List-II A. Alkali metal 1. ns2 np1-6 B. Alkaline earth metals 2. ns1 C. d-block elements 3. ns2 D. p-block elements 4. (n-1)d1-10 ns0-2
(a)
 A B C D 2 3 4 1
(b)
 A B C D 3 4 2 1
(c)
 A B C D 4 2 3 1
(d)
 A B C D 1 4 2 3
30. Consider the following statements.
(i) Oxidation character increases from left to right in a period.
(ii) Reducing character increases from left to right in a period.
(iii) Metallic character increases from left to right in a period.
Which of the above statement is/are not correct?

(a)

(i) only

(b)

(i) and (ii)

(c)

(ii) and (iii)

(d)

(i),(ii),(iii)

31. Consider the following statements.
(i) d-block elements show variable oxidate states.
(ii) Mostly d-block elements form colourless compounds.
(iii) Mostly d-block elements are diamagnetic due to paired electrons.
Which of the above statement is/are not correct?

(a)

(i) only

(b)

(ii) only

(c)

(i) and (ii)

(d)

(ii) and (iii)

32. All the s-block and p-block elements excluding 18th group are called______elements

(a)

representative

(b)

transition

(c)

inner-transition

(d)

transuranium

33. Which of the following is the correct electronic configuration of noble gases?

(a)

ns2 np6 nd10

(b)

ns2 np5

(c)

ns2 np6

(d)

ns2 np3

34. Group numbers 13 to 12 in the periodic table are called______

(a)

inner transition elements

(b)

representative elements

(c)

synthetic elements

(d)

transition dements

35. Which one of the following is in solid state at room temperature?

(a)

Bromine

(b)

Mercury

(c)

Bismuth

(d)

Gallium

36. Which of the following is not a metalloid (or) semi-metal?

(a)

Silicon

(b)

Arsenic

(c)

Germanium

(d)

Sodium

37. Which of the following metal is not in liquid state?

(a)

Gallium

(b)

Aluminium

(c)

Mercury

(d)

Caesium

38. Which of the following is not a periodic property?

(a)

(b)

Ionization enthalpy

(c)

Electron affinity

(d)

Oxidation number

39. Which of the following property increases as we go down the group in the periodic property?

(a)

Ionization energy

(b)

Electronegativity

(c)

(d)

Electron affinity

40. The metallic radius of copper is_____

(a)

0.99 $\mathring { A }$

(b)

1.28 $\mathring { A }$

(c)

1.98 $\mathring { A }$

(d)

2.56 $\mathring { A }$

41. Consider the following statements.
(i) Atomic radius of elements increases with increase in atomic number as we go down the group.
(ii) Atomic radius of elements increases with increase in atomic number as we go across the period.
(iii) Atomic radius of elements decreases as we go from left to right in a period.
Which of the above statement is/are not correct?

(a)

(i) only

(b)

(i) and (ii)

(c)

(ii) only

(d)

(i) and (iii)

42. Which one of the following is not an isoelectronic ion?

(a)

Na+

(b)

Mg2+

(c)

Cl-

(d)

O2-

43. Which one of the following is not an isoelectronic ion?

(a)

Al3+

(b)

N3-

(c)

Mg2+

(d)

K+

44. Which of the following possess almost same properties due to lanthanide contraction?

(a)

Zr,HF

(b)

Na,K

(c)

Zn,Cd

(d)

Ag,Au

45. Consider the following statements.
(i) Ionization is always an exothermic process.
(ii) Ionization energies always increase in the order LE1> I.E2 > I.E3.
(iii) Ionization energy measurements are carried out with atoms in the solid state.
Which of the above statement is/are not correct?

(a)

(i) only

(b)

(i) and (ii)

(c)

(iii) only

(d)

(i), (ii) and (iii)

46. Which of the following does not have zero electron gain enthalpy?

(a)

Be

(b)

Cl

(c)

Mg

(d)

N

47. Which of the following have zero electron gain enthalpy?

(a)

Halogens

(b)

Noble gases

(c)

Chalcogens

(d)

Gold

48. Which of the following have the highest value of electronegativity?

(a)

Halogens

(b)

Alkali metals

(c)

Alkaline earth metals

(d)

Transition metals

49. Among all the elements which one has the highest value of electronegativity?

(a)

Chlorine

(b)

Bromine

(c)

Fluorine

(d)

Iodine

50. Among the alkali metals which one form compounds with more covalent character?

(a)

Sodium

(b)

Potassium

(c)

Rubidium

(d)

Lithium

51. Which of the following pair is not diagonally related?

(a)

Li, Mg

(b)

Li, Na

(c)

Be, Al

(d)

B, Si

52. In the modern periodic table, the period indicates the value of____

(a)

atomic number

(b)

mass number

(c)

principal quantum number

(d)

azimuthal quantum number

53. Which of the following statements related to the modern periodic table is incorrect?

(a)

The p-block has 6 columns, because a maximum of 6 electrons can occupy all the orbitals in a p-subshell.

(b)

The d-block has 8 columns, because a maximum of 8 electrons can occupy all the orbitals in a d-subshell.

(c)

Each block contairis a number of columns equal to the number of electrons that can occupy that subshell.

(d)

The block indicates value of azimuthal quantum number (1) for the last subshell that received electrons in building up the electronic configuration.

54. The size of isoelectronic species- F-, Ne and Na+ is affected by

(a)

nuclear charge (Z)

(b)

valence principal quantum number (n)

(c)

electron-electron interaction in the outer orbitals

(d)

none of the factors becausetheir size is the same

55. Which of the following statements is incorrect in relation to ionization enthalpy?

(a)

Ionization enthalpy increases for each successive electron.

(b)

The greatest increase in ionization enthalpy is experienced on removal of electrons from core noble gas configuration.

(c)

End of valence electrons is marked by a big jump in ionization enthalpy.

(d)

Removal of electron from orbitals bearing lower n value is easier than from orbital having high n value.

56. Considering the elements F, CI, O and N, the correct order of their chemical reactivity in terms of oxidizing property is_____

(a)

F > CI > O > N

(b)

F > O > CI > N

(c)

CI > F > O > N

(d)

0 > F > N > CI

57. The highest ionization energy is exhibited by_________

(a)

halogens

(b)

alkaline earth metals

(c)

transition metals

(d)

noble gases

58. Which of the following is arranged in order of increasing radius?

(a)

K+ (aq) < Na+ (aq) < Li+ (aq)

(b)

K+ (aq) > Na+ (aq) > Zn+ (aq)

(c)

K+ (aq) > Li+ (aq) > Na+ (aq)

(d)

Li+ (aq) < Na+ (aq) < K+ (aq)

59. Among the following elements, which has the least electron affinity?

(a)

Phosphorous

(b)

Oxygen

(c)

Sulphur

(d)

Nitrogen

60. Which one of the following is isoelectronic with Ne?

(a)

N3-

(b)

Mg2+

(c)

Ag3+

(d)

All the above

61. Which element has smallest size?

(a)

B

(b)

N

(c)

Al

(d)

P

62. In halogens, which of the following decreases from iodine to fluorine?

(a)

Bond length

(b)

Electronegativity

(c)

Ionization energy

(d)

Oxidizing power

63. What is the electronic configuration of the elements of group 14?

(a)

ns2 np4

(b)

ns2 np6

(c)

ns2 np2

(d)

ns2

64. Consider the isoelectronic species Na+, Mg2+, F- and O2-. The correct order of increasing length of their radii is:

(a)

F- < O2- < Mg2+< Na+

(b)

Mg2+ < Na+ < F- < O2-

(c)

O2- < F- < Na+ < Mg2+

(d)

O2- < F- < Mg2+ < Na+

65. The order of screening effect of electron of s, p, d and f orbits of a given shell of an atom on its outershell electrons is:

(a)

s > p > d> f

(b)

f>d>p>s

(c)

P>d>s>f

(d)

f>p>s>d

66. The first ionization enthalpy of Na, Mg, AI and Si are in order.

(a)

Na<Mg<AI>Si

(b)

Na>Mg>AI>Si

(c)

Na<Mg<Al<Si

(d)

Na>Mg>Al<Si

67. Among halogens, the correct order of amount of energy released in electron gain is:

(a)

F>CI>Br>I

(b)

F<CI<Br<I

(c)

F<CI>Br>I

(d)

F<CI<Br>I

68. Hydrogen by donating one electron forms H+. In this property, it resembles with__________.

(a)

Transition metals

(b)

Alkaline earth metals

(c)

Alkali metals

(d)

Halogens

69. On moving from left to right across a period in the periodic table, the metallic character__________.

(a)

increases

(b)

decreases

(c)

remains constant

(d)

first increases and then decreases

70. The most electronegative element possess the electronic configuration______.

(a)

ns2 np2

(b)

ns2 np4

(c)

ns2 np5

(d)

ns2 np3

71. Choose the correct order of ionization energy.

(a)

N>O>F

(b)

F>O>N

(c)

N>O<F

(d)

O>F>N

72. The element with highest electron affinity belongs to___________.

(a)

period 1 group 1

(b)

period 3 group 17

(c)

period 2 group 17

(d)

period 2 group 16

73. Which of the following ions are not isoelectronic with Ar?

(a)

Na+

(b)

Ca2+

(c)

Cl-

(d)

K+

74. Statement-I: Ionization enthalpy of Be is greater than that of B.
Statement-:II: The nuclear charge of B is greater than that of Be.

(a)

Statement-I and II are correct and statement-II is the correct explanation of statement-I.

(b)

Statement-I and statement-II are correct but statement-II is not the correct explanation of statement-I.

(c)

Statement-I is correct but statement-II is wrong.

(d)

Statement-I is wrong but statement-II is correct.

75. Statement-I: Ionization enthalpy of nitrogen is greater than that of oxygen.
Statement-II: Nitrogen has exactly half filled electronic configuration which is more stable than electronic configuration of oxygen.

(a)

Statement-I is wrong but statement-II is correct.

(b)

Statement-I is correct but statement-II is wrong.

(c)

Statement-I and II are correct and statement-II is the correct explanation of statement-I.

(d)

Statement-I and II are correct but statement-II is not the correct explanation of statement-I.