CHAPTER 1 PERIODIC CLASSIFICATION OF ELEMENTS AND PERIODICITY
1. The number of shells in an element reflects its: (a) Period number (b) Group number (c) Both (d) None
2. The number of electrons in valence shell of an element reflects its: (a) Period number (b) Group number (c) Both (d) None
3. Generally metals form oxides: (a) Acidic (b) Basic (c) Amphoteric (d) None
4. Variable valency is shown by: (a) Group 1A (b) Group IIA (c) Group VIIA (d) Group IB
5. Hydrogen can be placed above the groups of the periodic table: (a) IA, IVA and VIIA elements (b) VIIA Elements (c) IIIA, IVA and VA elements (d) IIA, IIIA and VIIA elements
6. Members of group IA are called: (a) Alkali metals (b) Alkaline earth metals (c) Halogens (d) Noble gases
7. Members of group IB are called: (a) Alkali metals (b) Alkaline earth metals (c) Halogens (d)tyCoinage metals
8. Keeping in view the sizes of atoms, which order is the correct one: (a) Mg>Sr (b) Ba > Mg (c) Be>Mg (d) Ra>Ba
9. Which one of the following oxides is Amphoteric in nature: (a) MgO (b) Na2O (c) SO2 (d) ZnO
10. According to Newland’s arrangement of elements recurrence (periodicity) of properties take place at every: (a) 8th element (b) 10mth element (c) 18th element (d) None
11. Atomic number was discovered by Mosley in: (a) 1913 (b) 1914 (c) 1915 (d) 1916
12. Total groups in modern periodic table: (a) 7 (b) 8 (c) 10 (d) 18
13. Non-metals usually exist as: (a) Liquids (b) Gases (c) Liquids or gases (d) Waxy solids
14. The Ionization energy of Sodium is: (a) 500 K.J mol-1 (b) 513 K.J mol-1 (c) 496 K.J mol-1 (d) 480 K.J mol-1
15. SnCl4 is a: (a) Co-ordinate Covalent Compound (b) Ionic compound (c) Covalent Compound (d) None of these
16. Ga has oxidation state: (a) +3 (b) +2 (c) +4 (d) +1
17. Hydrides can be classified into: (a) Two types (b) Three types (c) Four types (d) Five types
18. Which of the following represents elements in order of increasing atomic radii: (a) I>Br> Cl (b) Li>Na>K (c) He>Ne>Ar (d) None
19. The decrease in nuclear force on valence electrons, because of the increase in number of shells containing electrons and layering above is known as: (a) Resonance effect (b) Shielding effect (c) Inductive effect (d) None
20. Number of elements present in the 5th period of periodic table is: (a) 8 (b) 10 (c) 18 (d) 32
21. Which element has the largest first ionization energy: (a) Li (b) Na (c) K (d) Rb
22. Which of the following pairs are chemically dissimilar: (a) Na and K (b) Ba and Sr (c) Zr and Hf (d) Ca and Zn
23. Which of the following elements is most electronegative: (a) Oxygen (b) Chlorine (c) Nitrogen (d) Fluorine
24. Which of the following has greatest metallic character: (a) Mg (b) Ca (c) Al (d) Cs
25. Highest Hydration energy is shown by: (a) Na+ (b) Mg+2 (c) Al+3 (d) Ga+3
26. Which of the following has highest value of Ionization Energy: (a) Na+ (b) Al+ (c) Al+2 (d) Al+3
27. The valence shell electronic structure of an element is ns2 np5. The element will belong to the group: (a) IA (b) IIA (c) VA (d) VIIA
28. Which of the following pair of atomic numbers represents IIA elements: (a) 3, 11 (b) 3, 12 (c) 4, 20 (d) 3, 20
29. Among the following elements the highest value of electron affinity is shown by: (a) F (b) Cl (c) Br (d) I
30. The force of attraction of an element on shared pair of electron is known as: (a) Covalent bond (b) Ionization potential (c) Electron affinity (d) Electronegativity
31. Alkali metals in each period have: (a) Smallest size (b) Lowest Ionization Energy (c) Highest Ionization Energy (d) Lowest atomic radius
32. The correct order of electron afmfinity among the following is: (a) F > Cl > Br (b) Br > Cl > F (c) Cl > F > Br (d) F > Br > Cl
33. Which of the followlineg does not exhibit the “periodicity” in properties of the elements: (a) Ionization energy (b) n/p ratio (c) Electronegativity (d) Atomic radius
34. Polymeric (Intermediate) hydride shall be formed by: (a) Na (b) K (c) Be (d) C
35. The highetst acidity is shown by: (a) Mn2O7 (b) Mn2O3 (c) MnO2 (d) MnO
36. The covalent hydrides are usually: (a) Liquids (b) Gases (c) Volatile Liquids or gases (d) Waxy solids
37. Which of the following is not iso-electronic with others: (a) Na+ (b) Mg2+ (c) O2 (d) Cl
38. Which of the following oxides is Amphoteric in character: (a) CaO (b) CO2 (c) SiO2 (d) Sb2O3
39. The melting point is lowest for: (a) Be (b) Mg (c) Ca (d) Sr
40. Which of the following in not true for metalloids: (a) They are borderline elements that exhibit both metallic and non-metallic properties (b) They usually act as electron donors to non-metals (c) They usually act as electron acceptors from metals (d) They are good conductor of heat and electricity
41. Among the pure ionic compounds, the ------- have the highest lattice energies: (a) Fluorides (b) Chlorides (c) Bromides (d) Iodides
42. Which electronic sub-shell in lanthanides is incompletely filled: (a) 4f (b) 5f (c) 6f (d) All
43. The number of elements in fourth period of periodic table is: (a) 32 (b) 18 (c) 10 (d) 8
44. The basis of modern periodic law is: (a) Electron affinity (b) atomic mass (c) Ionization energy (d) atomic number
45. The highest ionization energy is possessed by: (a) Nitrogen (b) Phosphorous (c) Bismuth (d) Antimony
46. The decrease in atomic sizes is much prominent across rows containming elements of: (a) s & p-block (b) d-block (c) f-block (d) All
47. Mark the correct statement: (a) All lanthanides are present in the same group (b) All halogens are present in the same period (c) All the alkali metals are present in the same group (d) All the noble gases are present in the same period.
48. Encircle the correct statement: (a) Metallic character increases down the group (b) Metallic character increases along a period (c) Metallic character remains the same along a period (d) Metallic character remains the same down the group
49. In Potassium super oxide (KO2) oxidation state of O is: (a) -1 (b) -2 (c) -1/2 (d) -4
50. Hydrogen can be placed with the element of group (IV-A) because both: (a) Act as strong oxidizing agent (b) Act as strong reducing agent (c) Possess the property of catenation (d) Form neutral oxides
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Chemistry