P Block Elements Class 12 Important Questions

P Block Elements Class 12 Important Questions are very important for NEET, JEE as well as AIIMS exam. These P Block Elements Class 12 Important Questions will help you to score more marks.

These P Block Elements Class 12 Important Questions is very useful for those students who are preparing for NEET, JEE as well as AIIMS Exam. These P Block Elements Class 12 Important Questions will be very useful for those students who are preparing with complete devotion and hard work.

P Block Elements Class 12 Important Questions

These P Block Elements Class 12 Important Questions contains following topics:

P Block Important Questions (Group 15 Elements)
P Block NEET Questions (Dinitrogen)
P Block Elements NEET Questions (Ammonia)
P Block JEE Mains Questions (Oxides of Nitrogen)
P Block Previous Year Questions JEE Mains (Nitric Acid)
P Block Elements Class 11 NEET Questions (Phosphorus – Allotropic Forms)
P Block Elements JEE Mains Questions (Phosphine)
P Block JEE Advanced Questions (Phosphorus Halides)
P Block MCQ For NEET (Oxoacids of Phosphorus)
P Block Questions For JEE Mains (Group 16 Elements)
P Block Elements Questions For NEET (Dioxygen)
P Block Class 11 NEET Questions (Simple Oxides)
P Block Elements MCQ For NEET (Ozone)
P Block Elements Class 12 MCQ For NEET (Sulphur – Allotropic Forms)
P Block Elements Important Question (Sulphur Dioxide)
P Block Elements Class 12 Questions And Answers (Oxoacids of Sulphur)
P Block Questions (Sulphuric Acid)
MCQ On P Block Elements Class 12 (Group 17 Elements)
P Block Elements MCQ (Chlorine)
P Block Elements Class 12 MCQ (Hydrogen Chloride)
Important Questions From P Block Elements Class 12 (Oxoacids of Halogens)
P Block MCQ (Interhalogen Compounds)
Important Questions Of P Block Class 12 (Group 18 Elements)

P Block Elements Class 12 Important Questions

1. Which of the following is radioactive in nature?

a) Oxygen

b) Sulphur

c) Tellurium

d) Polonium

Answer: Polonium

2. Which of the following does not exist as an octatomic solid?

a) Sulphur

b) Tellurium

c) Selenium

d) Oxygen

Answer: Oxygen

3. Which group 16 element has the highest tendency for catenation?

a) Oxygen

b) Sulphur

c) Selenium

d) Polonium

Answer: Sulphur

4. Which group 16 element has 8 allotropic forms?

a) Sulphur

b) Oxygen

c) Selenium

d) Polonium

Answer: Selenium

5. What is the most reactive element of group 16?

a) Oxygen

b) Sulphur

c) Tellurium

d) Selenium

Answer: Oxygen

6. Among the following, which one is a wrong statement.

(a) PH5 and BiCl5 do not exist.

(b) pπ-dπ bonds are present in SO2

(c) SeF4 and CH4 have same shape.

(d) I3 has bent geometry.

Answer: SeF4 and CH4 have same shape.

7. Which one of the following order is correct for the bond dissociation enthalpy of halogen molecule?

(a) Br2 > I2 > F2 > Cl2

(b) F2 > Cl2 > Br2 > I2

(c) I2 > Br2 > Cl2 > F2

(d) Cl2 > Br2 > F2 > I2

Answer: Cl2 > Br2 > F2 > I2

8. Which is strongest acid in the following:

(a) HClO4

(b) H2SO3

(c) H2SO4

(d) HClO3

Answer: HClO4

9. The correct order of oxidising power is

(a) HClO4 > HClO3 > HClO2 > HCIO

(b) HOCl > HClO2 > HClO3 > HClO4

(c) HClO3 > HClO4 > HClO2 > HClO

(d) HCIO2 > HOCl > HClO3 > HClO4

Answer: HOCl > HClO2 > HClO3 > HClO4

10. The correct order of acid strength is

(a) HClO4 < HClO3 < HClO2 < HClO

(b) HCIO < HClO2 < HClO3 < HClO4

(c) HClO4 < HClO < HClO2 < HClO3

(d) HClO2 < HClO3 < HClO4 < HClO

Answer: HCIO < HClO2 < HClO3 < HClO4

11. Among the following which is strongest oxidising agent.

(a) Br2

(b) I2

(c) Cl2

(d) F2

Answer: F2

12. When Cl2 reacts with hot and cone. NaOH, the oxidation number of chlorine changes from

(a) zero to +1 and zero to +5

(b) 0 to -1 and 0 to +5

(c) zero to -1 and zero to +3

(d) 0 to +1 and 0 to -3

Answer: 0 to -1 and 0 to +5

13. Acidity of diprotic acid in aqueous solution increases in the order.

(a) H2S < H2Se < H2Te

(b) H2Se < H2S < H2Te

(c) H2Te < H2S < H2Se

(d) H2Se < H2Te < H2S

Answer: H2S < H2Se < H2Te

14. Which of the following statement is incorrect?

(a) ONF is isoelectronic with NO2

(h) OF2 is an oxide of fluoride

(c) Cl2O7 is an anhydride of perchloric acid

(d) O3 molecule is bent

Answer: OF2 is an oxide of fluoride

15. Chlorine reacts with excess of NH3 to form

(a) NH4Cl

(b) N2 + HCl

(c) N2 + NH4Cl

(d) NCl3 + HCl

Answer: N2 + NH4Cl

16. Which of the following reactions is an example of redox reaction?

(a) XeF4 + O2F2 → XeF6 + O2

(b) XeF2 + PF5 → [XeF]+ [PF6]

(c) XeF6 + H2O → XeOF4 + 2HF

(d) XeF6 + 2H2O → Xeo2F2 + 2HF

Answer: XeF4 + O2F2 → XeF6 + O2

17. On addition of cone. H2SO4 to a chloride salt, colourless fumes are evolved but in case of iodide salt, violet flames come out. This is because [NCERT Exemplar]

(a) H2SO4 reduces HI to I2

(b) HI is of violet colour

(c) HI gets oxidised to I2

(d) HI changes to HIO3

Answer: HI gets oxidised to I2

18. Affinity for hydrogen decreases in the group from fluorine to iodine. Which of the halogen acids should have highest bond dissociation enthalpy? [NCERT Exemplar]

(a) HF

(b) HCl

(c) HBr

(d) HI

Answer: HF

19. Hot cone. H2SO4 acts as moderately strong oxidising agent. It oxidises both metals and non-metals. Which of the following element is oxidised by cone. H2SO4 into two gaseous products?

(a) Cu

(b) S

(c) C

(d) Zn

Answer: atomic number of sulphur is higher than oxygen.

20. H2S is more acidic than H2O because

(a) oxygen is more electronegative than sulphur.

(b) atomic number of sulphur is higher than oxygen.

(c) H — S bond dissociation energy is less as compared to H — O bond.

(d) H — O bond dissociation energy is less also compared to H — S bond.

Answer: atomic number of sulphur is higher than oxygen.

21. The boiling points of hydrides of group 16 are in the order

(a) H2O > H2Te > H2S > H2Se

(b) H2O > H2S > H2Se > H2Te

(c) H2O > H2Te > H2Se > H2S

(d) None of these

Answer: H2O > H2S > H2Se > H2Te

22. In the manufacture of sulphuric acid by contact process Tyndall box is used to

(a) convert SO2 and SO3

(b) test the presence of dust particles

(c) filter dust particles

(d) remove impurities

Answer: test the presence of dust particles

23. Fluorine differs from rest of the halogens in some of its properties. This is due to

(a) its smaller size and high electronegativity.

(b) lack of d-orbitals.

(c) low bond dissociation energy.

(d) All of the these.

Answer: lack of d-orbitals.

24. The set with correct order of acidity is

(a) HClO < HClO2 < HClO3 < HClO4

(b) HClO4 < HClO3 < HClO2 < HClO

(c) HClO < HClO4 < HClO3 < HClO2

(d) HClO4 < HClO2 < HClO3 < HClO

Answer: HClO4 < HClO3 < HClO2 < HClO

25. When chlorine reacts with cold and dilute solution of sodium hydroxide, it forms

(a) Cl and ClO

(b) Cl and ClO2

(c) Cl and ClO3

(d) Cl and ClO4

Answer: Cl and ClO

26. The formation of O2+ [PtF6] is the basis for the formation of first xenon compound. This is because

(a) O2 and Xe have different sizes.

(b) both O2 and Xe are gases.

(c) O2 and Xe have comparable electro-negativities.

(d) O2 and Xe have comparable ionisation enthalpies.

Answer: O2 and Xe have comparable ionisation enthalpies.

27. Partial hydrolysis of XeF4 gives

(a) XeO3

(b) XeOF2

(c) XeOF4

(d) XeF2

Answer: XeOF2

28. Helium is preferred to be used in balloons instead of hydrogen because it is

(a) incombustible

(b) lighter than hydrogen

(c) more abundant than hydrogen

(d) non polarizable

Answer: incombustible

29. The increasing order of reducing power of the halogen acids is

(a) HF < HCl < HBr < HI

(b) HI < HBr < HCl < HF

(c) HBr < HCl < HF < HI

(d) HCl < HBr < HF < HI

Answer: HF < HCl < HBr < HI

30. What product is formed when iron metal is dipped into concentrated nitric acid?

a) Iron (III) nitrate + NO2

b) Iron (II) nitrate + NO

c) Iron (III) oxide

d) Iron (III) nitrite

Answer: Iron (III) oxide

31. Which of the following processes involves heating a carbonate ore to form metal oxide?

a) Leaching

b) Smelting

c) Ore Reduction

d) Calcination

Answer: Calcination

32. Which of the following metals does not react with hot water to form an oxide?

a) Calcium

b) Magnesium

c) Iron

d) Lithium

Answer: Iron

33. What is formed when amphoteric oxides react with an alkali solution?

a) Salt only

b) No reaction

c) Acid

d) Salt and water

Answer: Salt and water

34. What type of oxides is formed by metals?

a) Oxides with pH = 7

b) Oxides with pH > -log10[1 x 10-7]

c) Oxides with pH <= -log10[1 x 10-7]

d) Amphoteric oxides

Answer: Oxides with pH > -log10[1 x 10-7]

35. What type of oxides is formed by non-metals?

a) Oxides with pH <=7

b) Amphoteric oxides

c) Oxides with pH > 7

d) Oxides which are acidic

Answer: Oxides which are acidic

FAQs on P Block Elements

What are P block elements give example?

The p-block elements are found on the right side of the periodic table. They include the boron, carbon, nitrogen, oxygen and flourine families in addition to the noble gases. The noble gases have full p-orbital’s and are nonreactive. When electrons fill shells they must do so under certain restrictions. These restrictions include: Having both s and p orbitals available (in compliance with the octet rule) Being able to keep a full or almost full valence shell (to meet valence shell electron pair repulsion; VSEPR theory)

What is P block elements Class 12?

We can see various elements in P block on right hand side side of periodic table. These elements are known as p-block elements. It consists of the Boron, Carbon, Nitrogen, Oxygen, Halogen and Noble gas family.

Why it is called p-block?

The names s-block and p-block refer to the electron configurations assumed by elements in these respective blocks. In the s-block, all elements have their valence electrons in s orbitals. The p-block, on the other hand, contains elements with their valence electrons in p orbitals.

Is helium p-block?

The p-block is on the right side of the standard periodic table and encompasses elements in groups 13 to 18. Helium, though being the first element in group 18, is not included in the p-block. Elements in this block are called p-block because all these elements have a valance shell of s subshells while no other subshell is present.

What is meant by inert pair effect?

The inert pair effect is the tendency of the two electrons in the outermost atomic s-orbital to remain unshared in compounds of post-transition metals. As a result, the inert pair of ns electrons remains more tightly held by the nucleus and hence participates less in bond formation. The following properties arise as a consequence: Rule for filling d-electron level: Since one electron is already paired and another electron would be anti-bonding, only one additional electron will enter the d-orbital. This electron will be added as tightly as possible to an already occupied orbital, rather than occupying a new unoccupied orbital.

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