HBSE Class 11 Chemistry Question Paper 2022 Answer Key

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HBSE Class 11 Chemistry Question Paper 2022 Answer Key

Q1. Number of moles in 54g of Water are :

(A) 2.0

(B) 2.5

(C) 3.0

(D) 3.5 

Ans. (C) 3.0

18g = 1 mole

No. of moles = 54/18 = 3 moles


Q2. Find number of unpaired electrons in Oxygen atom :

(A) 1

(B) 2

(C) 3

(D) 4

Ans. (B) 2


Q3. Arrange B, Al, Mg and K in correct order of their metallic character :

(A) B > Al > Mg > K

(B) Al > Mg > B > K

(C) Mg > Al > K > B

(D) K > Mg > Al > B

Ans. (D) K > Mg > Al > B


Q4. How many vertical columns in Modern Periodic table ?

(A) 2

(B) 8

(C) 32

(D) 18

Ans. (D) 18


Q5. Which compound do not show zero dipole moment ?

(A) CO2

(B) BF3

(C) H2O

(D) CCl4

Ans. (C) H2O


Q6. Which type of intermolecular force exists in Cl2 and CCl4 ?

(A) dipole-dipole forces 

(B) dipole-induced dipole forces

(C) dispersion forces

(D) hydrogen bonds

Ans. (C) dispersion forces


Q7. The temperature at which the volume of gas is zero ?

(A) 0°C

(B) O K

(C) O°F

(D) None of these

Ans. (B) O K


Q8. For the process to occur under adiabetic conditions, the correct condition is :

(A) ∆T = 0

(B) ∆P = 0

(C) ∆q = 0     

(D) w = 0 

Ans. (C) ∆q = 0

∆q = 0 means there is no exchange of heat.


Q9. The pH of Human Saliva is :

(A) 7.9

(B) 9.2

(C) 7.8

(D) 6.8

Ans. (D) 6.8

pH of human saliva = 6.2 to 7.6 


Q10. The oxidation number of Cl in KClO3 is :

(A) +5

(B) +3

(C) +1

(D) -1 

Ans. (A) +5

+1 + x +3(-2) = 0

1 + x – 6 = 0

x = +5 


Q11. The oxidation number of Sulphur in SO4²- is :

(A) -2

(B) +6

(C) +3

(D) +4 

Ans. (B) +6

x + 4(-2) = -2 

x = -2 + 8 = +6 


Q12. How many isotopes of Hydrogen ?

(A) 2

(B) 3

(C) 5

(D) 4

Ans. (B) 3

The hydrogen element has three isotopes : hydrogen, deuterium, and tritium.


Q13. Standard electrode potential of Hydrogen is :

(A) 0.0 V

(B) 1.0 V

(C) -1.0 V

(D) 2.0 V

Ans. (A) 0.0 V


Q14. What is formula of Caustic Soda ?

(A) Ca(OH)2

(B) NaOH


(D) Na2CO3

Ans. (B) NaOH


Q15. Which alkali metal having least melting point ?

(A) Na

(B) K

(C) Rb 

(D) Cs

Ans. (D) Cs

Caesium (Cs) has large size and weaker metallic bond. 


Q16. Thermodynamically the most stable form of Carbon is :

(A) Diamond

(B) Graphite

(C) Fullerenes

(D) Coal

Ans. (B) Graphite


Q17. CnH2n-2 is general formula of : 

(A) Alkanes

(B) Arenes

(C) Alkenes

(D) Alkynes

Ans. (D) Alkynes


Q18. Heating a mixture of sodium acetate with soda-lime gives :

(A) Propane

(B) Ethane

(C) Methane 

(D) Butane

Ans. (C) Methane


Q19. Round up 34.216 upto three significant figures.

Ans. 34.2


Q20. Which of the following species will have largest size ?

Mg, Mg²+, Al, Al³+ 

Ans. Mg

Mg > Al > Mg²+ > Al³+ 


Q21. Write general electronic configuration of p-block elements.

Ans. ns² np¹-⁶


Q22. What is Boyle’s Law ?

Ans. The pressure and volume of a gas are inversely proportional to each other as long as the temperature and the quantity of gas are kept constant.

P ∝ 1/V  (Temperature = Constant) 

P1/P2 = V2/V1 = constant 


Q23. What is constant in Charle’s Law ?

Ans. Charles’s law states that if a given quantity of gas is held at a constant pressure, its volume is directly proportional to the absolute temperature.

V ∝ T  (Pressure = Constant) 


Q24. What is oxidation process ? 

Ans. Oxidation is a process which involves the addition of oxygen or any electronegative element or the removal of hydrogen or any electropositive element.

(Removal of hydrogen or addition of oxygen)


Q25. Which is reducing agent in the following reaction ?

Zn + CuSO4 → ZnSO+ Cu 

Ans. Zinc(Zn) is reducing agent.


Q26. Why is Na less reactive than K ?

Ans. Because Na has small size and large ionisation energy than K.


Q27. 1 kilometer = ……… millimeter or …….. millimeter 

Ans. 1000000 mm or 10⁶ mm


Q28. Binary compound formed by Li and O is ………… 

Ans. Li2O


Q29. Each line of V Vs. P graph at constant temperature is called ………… 

Ans. isotherm or isothermal


Q30. In a reaction acceptor of electrons called ………… 

Ans. oxidising agent


Q31. ………. number of hydrogen bonded water molecules in CuSO4.5H2O. 

Ans. One


Q32. Group 13 hydrides called ………….. 

Ans. Electron Deficient Hydrides


Q33. ……….. is oxidation state of K in KO2.

Ans. +1


Q34. Group 1 Li, Na, K, Rb, Cs are called ……….. metals. 

Ans. Alkali


Q35. The type of hybridization of carbon in diamond is ……….. 

Ans. sp³


Q36. Calculate the molarity of NaOH in the solution prepared by dissolving its 4g NaOH in water to form 250mL of solution. 

Ans. Weight of NaOH (W) = 4g

Molecular weight of NaOH (MW) = 40g 

Volume of solution (V) = 250mL 

Molarity (M) = W/MW × 1000/V = 4/40 × 1000/250 = 4/10 = 0.4 M 


Q37. What will be the wavelength of a ball of mass 0.1 kg moving with a velocity of 10ms-¹ ? 

Ans. Wavelength, λ = h/mv = (6.626×10-³⁴) ÷ (0.1×10) = 6.626 × 10-³⁴ metre

(h = de-broglie constant, m = mass, v = velocity) 


Q38. What is enthalpy of formation ? Give one example. 

Ans. Heat evolved or absorbed when 1 mole of the substance is formed form its elements under given conditions of temperature and pressure.

e.g.  C (graphite) + 2H2 (g) → CH4 (g)   ΔfH° = – 74.81 kJmol-¹


Q39. What will be the conjugate acids for the Bronsted bases NH3 and HCOO- ? 


Conjugate Acid  → Bronsted Base 

NH3                       → NH2– 

HCOO-                 → HCOOH 


Q40. What are Electrophiles ? Give its types with examples. 

Ans. Electrophiles are electron deficient species and can accept an electron pair from electron rich species. e.g. Br+, Cl+, CH3+


Q41. Explain Hund’s rule of maximum multiplicity with example. 

Ans. Hunds Rule of Maximum Multiplicity rule states that for a given electron configuration, the term with maximum multiplicity falls lowest in energy. According to this rule electron pairing in p, d and f orbitals cannot occur until each orbital of a given subshell contains one electron each or is singly occupied.


Q42. Define closed system, intensive properties and internal energy. 

Ans. Closed system– The system which allows the exchange of energy not of matter with the surroundings is called a closed system.

Intensive properties– The properties which do not depend upon the quantity of matter or substance present in the system. 


Internal Energy– Internal energy is the inherent microscopic energy of a system associated with the random motion of its molecules.


Q43. Define acid and base with example in Bronsted-Lowry concept. 


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