Question Bank 2025

CLASS:-XIth SUB:- CHEMISTRY

Q.1. Select and write the correct answer for the following multiple choice type of questions:
1) A sample of pure water, whatever the source always contains by mass of oxygen and 11.1 % by mass of
hydrogen.
a. 88.8 b. 18 c. 80 d. 16
2) Which of the following temperature will read the same value on Celsius and Fahrenheit scales.
a. - 400 b. + 400 c. -800 d. -200
3) How many g of H2 O are present in 0.25 mol of it?
a. 4.5 b. 18 c. 0.25 d. 5.4
4) The energy difference between the shells goes on........... When moved away from the nucleus.
a. Increasing b. decreasing c. equalizing d. static
5) p-orbitals are....... in shape.
a. spherical b. dumb bell c. double dumbbell d. diagonal
6) Principal Quantum number describes.
a. shape of orbital b. size of the orbital c. spin of electron d. orientation of in the orbital electron
7) Which molecule is linear?
a. SO3 b. CO2 c. H2S d. Cl2O
8)Identify the odd one .
a. Rb b. Ra c. Sr d. Be
9)………is inorganic graphite,
a. borax b. diboran c. boron nitride d. colemanite
10) A compound contains atoms of three elements A, B and C. If the oxidation state of A is +2, B is +5 and that
of C is -2, the compound is possibly represented by
a. A2(BC3)2 b. A3(BC4)2 c. A3(B4C)2 d. ABC2
11) Oxidation number of carbon in H2 CO3 is
a. +1 b. +2 c. +3 d. +4
12) Which is the correct stock notation for magenese dioxide?
a. Mn(I)O2 b. Mn (II)O2 c. Mn (III)O2 d. Mn (IV)O2
13) The lanthanides are placed in the periodic table at
a. left hand side b. right hand side c. middle d. bottom

14) Which of the atomic number represent the s-block elements?

a. 7, 15 b. 3, 12 c. 6, 14 d. 9, 17
15) Consider the elements B, Al, Mg and K predict the correct order of metallic character:
a. B > Al > Mg > K b. Al > Mg > B > K c. Mg > Al > K > B d. K > Mg > Al > B
16) The unstable isotope of hydrogen is......
a. H-1 b. H-2 c. H-3 d. all the three
17) Which of the following is Lewis’s acid?
a. BaCl2 b. KCl c. BeCl2 d. LiCl
18) What happens when crystalline Na2 CO3 is heated?
a. releases CO2 b. loses H2O c. decomposes in NaHCO3 d. no change taken place.
19) Which of the following is not an allotrope of carbon?
a. bucky ball b. diamond c. graphite d. emerald
20) Which of the following shows most prominent inert pair effect?
a. C b. Si c. Ge d. Pb
21) Haber’s process is used for preparation of………….
a. HNO3 b. NH3 c. NH2CONH2 d. NH4OH
22) The geometry of a carbocation is......
a. linear b. planar c. tetrahedral d. octahedral
23) The homologous series of alcohols has general molecular formula.........
a. CnH2n+1OH b. CnH2n+2OH c. CnH2n-2OH d. CnH2nOH
24) The delocalization of electrons due to overlap between p-orbital and sigma bond is called
a. Inductive effect b. electronic effect c. Hyperconjugation d. Resonance
25) Acidic hydrogen is present in:
a. acetylene b. ethane c. ethylene d. dimethyl acetylene
26) Major product of chlorination of ethyl benzene is:
a. m-chloroethyl benzene b. p - chloroethyl benzene c. chlorobenzene d. o - chloroethyl benzene
27) 1 - chloropropane on treatment with alc. KOH produces:
a. propane b. propene c. propyne d. propyl alcohol

Q.2 Answer the following questions: (VSA)

1) How many particles are present in 1 mole of a substance?
2) What is the SI unit of amount of a substance?
3) If an element ‘X’ has mass number 11 and it has 6 neutrons, then write its representation.
4) Give the names of any one quantum numbers.
5)Name the Alkali metal with smallest atom.
6)Define isotopes.
7) Write the formula for the Mercury (II) chloride
8) Write the formula for the Thallium (I) sulphate
9) Select the smaller ion form each of the following pairs: a. K+, Li+ b. N3-, F-
10) Define Electronegativity.
11) Name the most abundant element in the universe.
12) Name the Radioactive alkali metal.
13)Define isobars.
14)Name the isotopes of hydrogen.
15) What is meant by homologous series?
16) Write the first four members of homologous series that begins with A. CH3 CHO
17) Name the type of hydrocarbon that is used as lubricant.
18) Write general formula of alkyne.

Q.3 Answer the following questions: (SA)

1) Calculate number of moles of hydrogen in 0.448 litre of hydrogen gas at STP.
2) Calculate the number of moles and molecules of acetic acid present in 22 g of it.
3) Write condensed orbital notation of electronic configuration of the following elements:
a. Silicon (Z=14) b. calcium (Z=20)

4) Make the pairs:

‘A’ ‘B’

a. Neutrons i. six electrons

b. p-orbital ii. -1.6×10-19 C

c. charge on electron iii. Spherical shape

d. d-orbital i v. Chadwick

v. ten electron
 5) Hydrogen shows similarity with alkali metals as well as halogens.

.6) Describe the diagonal relationship between Li and Mg with the help of two illustrative properties.
7) Provide the stock notation for the following compounds: Mn and CuO.

8) Provide the stock notation for the following compounds: FeO, Fe2O3
9) Why the second ionization enthalpy is greater than the first ionization enthalpy?
10) Compare chemical properties of metals and nonmetals.
11) Explain BeCl2 is covalent while MgCl2 is ionic.
12) Explain why Lithium floats on water while sodium floats and catches fire when put in water.
13) Draw the structure of the following.
A. Orthophosphoric acid
B. diborane
14) Draw Resonance structure of nitric acid.
15) Write bond line formulae and condensed formulae for the following compounds
a. 3-methyloctane b. hept-2-ene
16) Write bond line formulae and condensed formulae for the following compounds
a. 2, 2, 4, 4- tetramethyl pentane b. octa-1,4-diene c. methoxy ethane
17) Write IUPAC names of the products obtained by the reaction of cold concentrated sulphuric acid followed
by water with the following compounds. a. propene b. but-l-ene
18) How many monochlorination products are possible for a. 2-methylpropane? b. 2-methylbutane?
19) Explain wurtz reaction with suitable example?
20) Find out the difference between.
A. Diamond and Graphite
B. White phosphorus and Red phosphorus.
Q.4 Answer the following questions: (LA-I)
1) N. Calculate the number of moles of magnesium oxide, MgO in i. 80 g and ii. 10 g of the compound.
(Average atomic masses of Mg = 24 and O = 16)
2) What is volume of carbon dioxide, CO2 occupying by i. 5 moles and ii. 0.5 mole of CO2 gas measured at STP.
3) Write orbital notations for electrons in orbitals with the following quantum numbers.
a. n = 2, l =1 b. n =4, l = 2 c. n = 3, l = 2
4) Write electronic configurations of Fe, Fe2+, Fe3+
5) Draw Lewis dot diagrams for the following
a. Water (H2O) b. Carbon dioxide (CO2) c. Methane (CH4)
6) Draw Lewis electron dot structures of a. HF b. C2H6 c. C2H4 d. CF3Cl e. SO2
7) Balance the following reactions by oxidation number method
Bi(OH)3 (g) + Sn(OH)3- (aq) Bi (s) + Sn (OH)6 -2 (aq) (basic)
8) Balance the following reactions by oxidation number method
H2SO4 (aq) + C (s) CO2 (g) + SO2 (g) + H2O (l) (acidic)
9) Define ionization enthalpy. Name the factors on which ionisation enthalpy depends? How does it vary down
the group and across a period?
10) How the atomic size vary in a group and across a period? Explain with suitable example.
11) Describe the diagonal relationship between Li and Mg with the help of two illustrative properties.
12) Write balanced chemical equations for the Beryllium oxide is treated separately with aqueous HCl and
aqueous NaOH solutions.
13) Difference between Diamond and Graphite.
14) Difference between White phosphorus and Red phosphorus.
15) Draw resonance structures of Benzaldehyde and which type of effect it take place.
16) Draw resonance structures of the Phenol and which type of effect it take place.
17) Acetone and acetaldehyde are the ozonolysis products of an alkene. Write the structural formula of an
alkene and give IUPAC name of it.
18) An alkene ‘A’ an ozonolysis gives 2 moles of ethanal. Write the structure and IUPAC name of ‘A’.
Q.5Answer the following questions: (LA-II)

1) In two moles of acetaldehyde (CH3 CHO) calculate the following a. Number of moles of carbon b. Number
of moles of hydrogen c. Number of moles of oxygen d. Number of molecules of acetaldehyde
2) Calculate the mass of potassium chlorate required to liberate 6.72 dm3 of oxygen at STP. Molar mass of
KClO3 is 122.5 g mol-1.
3) Find the oxidation number of sulphur in a) Na2S2O3 b) H2SO4 c) SO2 d) SF6
4) Find the oxidation number of Manganese in a) KMnO4 b) MnO2 c) MnCl2 d)K2MnO4
5) Write the structural formulae for the following names and also write correct IUPAC names for them.
a. 5-ethyl-3-methylheptane b. 2,4,5-trimethylthexane c. 2,2,3-trimethylpentan-4-0l
6) What is a condition for aromatic and non-aromatic compound with one example each?
7) Predict the possible products of the following reaction.
a. Bromination of phenol b. nitration of toluene.

8. Give reasons.
A. Ga3⊕ salts are better reducing agent while Tl3⊕ salts are better oxidising agent.

B. PbCl4 is less stable than PbCl2

.
9) Predict the possible products of the following reaction.
a. chlorination of nitrobenzene b. Sulfonation of chlorobenzene.
10) Difference between aromatic and aliphatic compound.
11) With the help of an appropriate example, write the steps of the Markovnikov's rule mechanism.
12) Draw structure of IUPAC name
a) 3-ethyl-4, 4-dimethylheptane b) 2, 2–dimethyl propane c) 3-bromo-1-chlorocyclohexene
d) 4-Bromo-3-methylpent-2-ene.

13Match the pairs from column A and B..

A B
BCl3 Angular molecule
SiO2 linear covalent molecule
CO2 Tetrahedral molecule.
Planar trigonal molecule

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