MCQ Questions For Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure

MCQs Class 11

Please refer to MCQ Questions Chemical Bonding and Molecular Structure for Chapter 4 Class 11 Chemistry given below. All MCQ questions are provided with answers. These MCQ Questions for Class 11 Chemistry are designed based on the chapters given in your CBSE NCERT Textbook for Class 11 Chemistry. These MCQ Questions are expected to come in your class 11 Board exams.

Question. Who provide explanation of valence based on intertness of noble gases ?
(a) Lewis
(b) Kossel-Lewis
(c) Langmuir
(d) Sidgwick & Powell

Answer

B

Question. In the formation of a molecule which of the following take part in chemical combination?
(a) cation
(b) anion
(c) valence electron
(d) inner shell electron

Answer

C

Question. The bond formed as a result of the electrostatic attraction between the positive and negative ions is termed as …
(a) Chemical bond
(b) Electrovalent bond
(c) Co-ordinate bond
(d) Covalent bond

Answer

B

Question. Cation and anion combines in a crystal to form following type of compound
(a) ionic
(b) metallic
(c) covalent
(d) dipole-dipole

Answer

A

Question. The attractive force which holds various constituents (atoms, ions etc.) together in different chemical species is called a
(a) chemical bond
(b) chemical compound
(c) ionic bond
(d) covalent bond

Answer

A

Question. The evolution of various theories of valence and the interpretation of the nature of chemical bonds have closely been related to the developments in the understanding of
(a) structure of atom
(b) electronic configuration of elements
(c) periodic table
(d) All of the above

Answer

D

Question. Who introduced the term covalent bond ?
(a) Lewis
(b) Langmuir
(c) Nyholm and Gillespie
(d) Heitler and London

Answer

B

Question. Which of the following is/are not the condition(s) for Lewis dot structure?
(i) Each bond is formed as a result of sharing of an electron pair between the atoms.
(ii) From the two combining atoms only one atom contribute electron(s) to the shared pair.
(iii) The combining atoms attain the outer shell noble gas configurations as a result of the sharing of electrons.
(a) (i) and (iii)
(b) (ii) and (iii)
(c) (ii) only
(d) (iii) only

Answer

C

Question. In N2molecule, the number of electrons shared by each nitrogen atom is
(a) 1
(b) 2
(c) 3
(d) 5

Answer

C

Question. The lowest energy structure is the one with the ………. formal charges on the atoms.
(a) smallest
(b) highest
(c) zero
(d) negative

Answer

A

Question. Electrovalence of calcium and chlorine respectively is
(a) + 2, – 1
(b) + 1, – 1
(c) + 1, – 2
(d) + 2, – 2

Answer

A

Question. When a metal atom combines with non-metal atom, the non-metal atom will
(a) lose electrons and decrease in size
(b) lose electrons and increase in size
(c) gain electrons and decrease in size
(d) gain electrons and increase in size

Answer

D

Question. In PO43– ion, the formal charge on each oxygen atom and P—O bond order respectively are
(a) –0.75, 0.6
(b) – 0.75, 1.0
(c) – 0.75, 1.25
(d) –3, 1.25

Answer

C

Question. In the cyanide ion, the formal negative charge is on
(a) C
(b) N
(c) Both C and N
(d) Resonate between C and N

Answer

B

Question. Among the following the electron deficient compound is
(a) BCl3
(b) CCl4
(c) PCl5
(d) BeCl2

Answer

A

Question. Which of the following is the electron deficient molecule?
(a) C2H6
(b) B2H6
(c) SiH4
(d) PH3

Answer

B

Question. Which of the following compounds does not follow the octet rule for electron distribution?
(a) PCl5
(b) PCl3
(c) H2O
(d) PH3

Answer

A

Question. A pair of compound which have odd electrons in the group NO, CO, ClO2, N2O5, SO2 and O3 are
(a) NO and ClO2
(b) CO and SO2
(c) ClO2 and CO
(d) SO2 and O3

Answer

A

Question. What are the exceptions of the octet rule ?
(a) The incomplete octet of central atom
(b) An odd number of electrons on central atom.
(c) Expanded octet of the central atom
(d) All of these

Answer

D

Question. In which of the following molecules octet rule is not followed?
(a) NH3
(b) CH4
(c) CO2
(d) NO

Answer

D

Question. Which of the following statements is incorrect ?
(a) The formation of ionic compounds depend upon the ease of formation of the positive and negative ions from the respective neutral atoms.
(b) Formation of ionic compounds depend upon arrangement of the positive and negative ions in the solid.
(c) Formation of positive ion involves addition of electron(s) while that of negative ion involves removal of electron(s).
(d) None of these

Answer

C

Question. The effect of more electronegative atom on the strength of ionic bond
(a) increases
(b) decreases
(c) remains the same
(d) decreases slowly

Answer

A

Question. Which of the following combination will form an electrovalent bond ?
(a) P and Cl
(b) NH3 and BF3
(c) H and Ca
(d) H and S

Answer

C

Question. Among the following which compound will show the highest lattice energy ?
(a) KF
(b) NaF
(c) CsF
(d) RbF

Answer

B

Question. Which of the following bond will have highest ionic character?
(a) H–I
(b) H–F
(c) H–Cl
(d) H–Br

Answer

B

Question. Which of the following pairs will form the most stable ionic bond ?
(a) Na and Cl
(b) Mg and F
(c) Li and F
(d) Na and F

Answer

B

Question. In ionic solids how crystal structure get stabilized
(a) By the energy released in the formation of crystal lattice.
(b) By achieving octet of electrons around the ionicspecies in gaseous state. 
(c) By electron gain enthalpy and the ionization enthalpy.
(d) None of these

Answer

A

Question. Energy required to completely separate one mole of a solid ionic compound into gaseous constituent ions is called ………. .
(a) Ionisation enthalpy
(b) Electron gain enthalpy
(c) Bond dissociation enthalpy
(d) Lattice enthalpy

Answer

D

Question. Which of the following methods is used for measuringbond length ?
(a) X-ray diffraction
(b) Electron-diffraction
(c) Spectroscopic techniques
(d) All of these

Answer

D

Question. ………. is measured as the radius of an atom’s core which is in contact with the core of an adjacent atom in a bonded situation.
(a) van der Waal’s radius
(b) Bond length
(c) Covalent radius
(d) Ionic radius

Answer

C

Question. The number of possible resonance structures for 2 CO32− is
(a) 2
(b) 3
(c) 6
(d) 9

Answer

B

Question. Which one of the following is not the resonance structure of CO2?
(a) O = C = O
(b) O – C ≡ O+
(c) + O ≡ C – O
(d) O ≡ C = O

Answer

D

Question. All the bond lengths of sulphur – oxygen in sulphate ion, are equal because of:
(a) symmetry
(b) resonance
(c) high electronegativity of oxygen
(d) None of these

Answer

B

Question. Resonance is due to
(a) delocalization of sigma electrons
(b) delocalization of pi electrons
(c) migration of protons
(d) Both (a) and (b)

Answer

B

Question. Which one of the following pairs of molecules will have permanent dipole moments for both members ?
(a) NO2 and CO2
(b) NO2 and O3
(c) SiF4 and CO2
(d) SiF4 and NO2

Answer

B

Question. The molecule which has zero dipole moment is
(a) CH3Cl
(b) NF3
(c) BF3
(d) ClO2

Answer

C

Question. Which of the following statement is correct?
(a) Amount of energy required to break one mole of bonds of a particular type between two atoms in a gaseous state is called bond enthalpy.
(b) The unit of bond enthalpy is kJ mol–1
(c) Larger the bond dissociation enthalpy, stronger will be the bond in the molecule
(d) All of these

Answer

D

Question. Complete the following statements. With A in bond order, B increases and C decreases.
(a) A = increase, B = bond length, C = bond enthalpy
(b) A = decrease, B = bond enthalpy, C = bond length
(c) A = increase, B = bond enthalpy, C = bond length
(d) A = increase, B = bond angle, C = bond enthalpy

Answer

C

Question. Which of the following has dipole moment?
(a) CO2
(b) p-dichlorobenzene
(c) NH3
(d) CH4

Answer

C

Question. Identify the non polar molecule in the following compounds
(a) H2
(b) HCl
(c) HF and HBr
(d) HBr

Answer

A

Question. Which one of the following molecules is expected to have zero dipole moment?
(a) H2O
(b) CO2
(c) SO2
(d) CaF2

Answer

B

Question. The correct order of dipole moments of HF, H2S and H2O is
(a) HF < H2S < H2O
(b) HF < H2S < H2O
(c) HF < H2S < H2O
(d) HF < H2O < H2S

Answer

A

Question. The most polar bond is
(a) C – F
(b) C – O
(c) C – Br
(d) C – S

Answer

A

Question. According to Fajan’s rule, covalent bond is favoured by
(a) Large cation and small anion
(b) Large cation and large anion
(c) Small cation and large anion
(d) Small cation and small anion

Answer

C

Question. The correct sequence of increasing covalent character is represented by
(a) LiCl < NaCl < BeCl2
(b) BeCl2 < LiCl < NaCl
(c) NaCl < LiCl < BeCl2
(d) BeCl2 < NaCl < LiCl

Answer

C

Question. A neutral molecule XF3 has a zero dipole moment. The element X is most likely
(a) chlorine
(b) boron
(c) nitrogen
(d) carbon

Answer

B

Question. Among the following, the molecule of high dipole moment is
(a) CCl4
(b) NH3
(c) H2O
(d) CHCl3

Answer

C

Question. Which of the following salt shows maximum covalent character?
(a) AlCl3
(b) MgCl2
(c) CsCl
(d) LaCl3

Answer

A

Question. Polarisibility of halide ions increases in the order
(a) F, I –, Br, Cl
(b) Cl , Br –, I, F
(c) I , Br , Cl, F
(d) F, Cl, Br, l

Answer

D

Question. Sodium chloride is an ionic compound whereas hydrogen chloride is mainly covalent because
(a) sodium is less reactive
(b) hydrogen is non-metal
(c) hydrogen chloride is a gas
(d) electronegativity difference in the case of hydrogen and chlorine is less than 2.1.

Answer

B

Question. CO2 is isostructural with
(a) C2H2
(b) SnCl2
(d) MgCl2
(c) NO2         

Answer

A

Question. Which species has the maximum number of lone pair of electrons on the central atom ? 
(a) [CIO3]
(b) XeF4
(c) SF4
(d) [I3]         

Answer

D

Question. InP4O10 the
(a) second bond in P = O is formed by pn-dn back bonding
(b) P = 0 bond is formed by pn-pn bonding
(c) P = 0 bond is fo1med dn-dn bonding
(d) P = 0 bond is formed by dn-dn- 30′ back bonrung     

Answer

C

Question. Which of the following molecules bas pyramidal shape?
(a) PCI3
(b) SO3
(c) CO32-
(d) NO3         

Answer

A

Question. Amongst the following, the molecule that is linear is
(a) SO2
(b) BeH2
(c) ClO2
(d) NO2     

Answer

B

Question. How manycr and n-bonds are present in toluene?
(a) 3n + 8σ
(c) 3n + 15σ
(e) 6n+ 6σ
(b) 3n + l0σ
(d) 6n + 3σ     

Answer

C

Question. Which of the following is a linear molecule? 
(a) BeCl2
(b) H2O
(c) SO2
(d) CH4         

Answer

A

Question. Pair of species having identical shapes for molecules is
(a) CF4, SF4
(b) BF3, PCI
(c) XeF2, CO
(d) PF5, IF7     

Answer

C

Question. The number of lone pairs of Xe in XeF2 , XeF4 and XeF6 respectively are 
(a) 3,2, l
(b) 2,4, 6
(c) 1,2,3
(d) 6,4,2         

Answer

A

Question. A square planar complex is formed by hybridisation of the following atomic orbitals 
(a) s, px, Py , Pz
(b) s, px, Py, Pz, d
(c) d, S, Px, Py       
(d) s, Px, Py, pz, d, d   

Answer

C

Question. Number of P—0 bonds in P4O10 is 
(a) 17
(b) 16
(c) 15
(d) 6       

Answer

B

Question. Hydrogen bonding plays a central role in the following phenomena 
(a) ice floats in water
(b) higher Lewis basicity of primary amines than tertiary amines in aqueous solutions
(c) formic acid is more acidic than acetic acid
(d) dimerisation of acetic acid in benzene     

Answer

A.B.D

Question. Which of the following hydrogen bonds are strongest in vapour phase? 
(a) HF …… HF
(b) HF ….. . HCI
(c) HCI. ….. HCI
(d) HF …… Hl       

Answer

A

Question. Which of the following compounds would have the highest boiling point ? 
(a) CH3CH2CH2CH3
(b) CH3NH2
(c) CH3OH
(d) CH2F2       

Answer

C

Question. Which of the following has strongest hydrogen bonding?
(a) Ethylamine
(b) Ammonia 
(c) Ethyl alcohol
(d) Diethyl ether           

Answer

C

Question. The maximum number of hydrogen bonds that a molecule of water can have is 
(a) 1
(c) 3
(b) 2
(d) 4       

Answer

D

Question. Malleability and ductility of metals can be accounted due to
(a) the presence of electrostatic force
(b) the crystalline stmcture in metal
(c) the capacity of layers of metal ions to slide over the other
(d) the interaction of electrons with metal ions in the lattice     

Answer

C

Question. Unusually high boiling point of water is result of
(a) intermolecular hydrogen bonding 
(b) intramolecular hydrogen bonding
(c) both intra and inter molecular hydrogen bonding
(d) high specific heat     

Answer

A

Question. Glycerol is more viscous than ethanol due to 
(a) high molecular weight
(b) high boiling point
(c) many hydrogen bonds per molecule
(d) Fajan’s rule     

Answer

C

Question. Oxygen and sulphur both are the member of same group in Periodic Table but H2O is liquid while H2 Sis gas because
(a) molecular weight of water is more
(b) electronegativity of sulphur is more
(c) H2S is weak acid
(d) water molecules are having strong hydrogen bonds between them     

Answer

D

Question. NH3 has much higher boiling point than PH3 because
(a) NHhas larger molecular weight 
(b) NHundergoes umbrella inversion
(c) NHforms hydrogen bond
(d) NHcontains ionic bonds whereas PH3 contains covalent bonds       

Answer

C

Question. Which compound is soluble in water? 
(a) CS2
(b) C2H5OH
(c) CCI4
(d) CHCI3     

Answer

B

Question. I. 1, 2-dihydroxy benzene
II. 1, 3-dihydroxy benzene
III. I, 4-dihydroxy benzene
IV. Hydroxy benzene
The increasing order of boiling points of above mentioned alcohols is
(a) I < II < ill< IV
(b) I< II < IV<ill
(c) IV < I < II < Ill
(d) IV < II < I < ill     

Answer

C

Question. Which molecule has hydrogen bonding?
(a) CH4
(b) CH3COOH
(c) GeH4
(d) H2Te       

Answer

B

Question. H-bond is not present in
(a) water
(b) glycerol
(c) hydrogen fluoride
(d) hydrogen sulphide       

Answer

D

Question. Metallic lusture is explained by
(a) diffusion of metal ions
(b) osci Ila ti on of loose electrons
(c) excitation of free protons
(d) existence of bee lattice     

Answer

B

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