CBSE Class 11 Chemistry Chemical Bonding and Molecular Structure Worksheet Set A

Question. In PO₄^3–ion, the formal charge on each oxygen atom and P—O bond order respectively are
(a) –0.75, 1.25
(b) –0.75, 1.0
(c) –0.75, 0.6
(d) –3, 1.25 
Answer. A

Question. Among LiCl, BeCl₂, BCl₃and CCl₄, the covalent bond character follows the order
(a) BeCl₂> BCl₃ > CCl₄ < LiCl
(b) BeCl₂ < BCl₃ < CCl₄ < LiCl
(c) LiCl < BeCl₂ < BCl₃ < CCl₄
(d) LiCl > BeCl₂ > BCl₃ > CCl4
Answer. C

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

Question. Which of the following, set of molecules will have zero dipole moment?
(a) Ammonia, beryllium difluoride, water,1, 4-dichlorobenzene
(b) Boron trifluoride, hydrogen fluoride, carbon dioxide, 1, 3-dichlorobenzene
(c) Nitrogen trifluoride, beryllium difluoride, water, 1, 3-dichlorobenzene
(d) Boron trifluoride, beryllium difluoride, carbon dioxide, 1, 4-dichlorobenzene
Answer. B

Question. Which of the following is the correct order of dipole moment ?
(a) NH₃< BF₃< NF₃ < H₂O
(b) BF₃ < NF₃ < NH₃ < H₂O
(c) BF₃ < NH₃ < NF₃ < H₂O
(d) H₂O < NF₃ < NH₃ < BF₃ 
Answer. D

Question. The species, having bond angles of 120° is
(a) ClF₃
(b) NCl₃
(c) BCl₃
(d) PH₃
Answer. B

Question. Consider the molecules CH₄, NH₃and H₂O. Which of the given statements is false?
(a) The H — O — H bond angle in H₂O is smaller than the H — N — H bond angle in NH₃.
(b) The H — C — H bond angle in CH₄is larger than the H — N — H bond angle in NH₃.
(c) The H — C — H bond angle in CH₄, the H — N — H bond angle in NH₃, and the H — O — H bond angle in H2O are all greater than 90°.
(d) The H — O — H bond angle in H₂O is larger than the H — C — H bond angle in CH₄.
Answer. C

Question. Which of the following molecules has the maximum dipole moment?
(a) CO₂
(b) CH₄
(c) NH₃
(d) NF₃
Answer. D

Question. The correct order of increasing bond length of C – H, C – O, C – C and C C is
(a) C – H < C C < C – O < C – C
(b) C – C < C C < C – O < C – H
(c) C – O < C – H < C – C < C C
(d) C – H < C – O < C – C < C C 
Answer. C

Question. The correct order of increasing bond angles in the following triatomic species is
(a) NO₂⁺< NO₂< NO₂^–
(b) NO₂⁺ < NO₂^– < NO₂
(c) NO₂^– < NO₂⁺ < NO₂
(d) NO₂^– < NO₂ < NO₂⁺
Answer. A

Question. The correct order of C – O bond length among CO,CO₃^2–, CO₂is
(a) CO < CO₃^2– < CO₂
(b) CO₃ ^2– < CO₂ < CO
(c) CO < CO₂ < CO₃^2–
(d) CO₂ < CO₃ ^2– < CO
Answer. D

Question. The electronegativity difference between N and F is greater than that between N and H yet the dipole moment of NH3 (1.5 D) is larger than that of NF3 (0.2 D). This is because
(a) in NH₃ the atomic dipole and bond dipole are in the opposite directions whereas in NF₃ these are in the same direction
(b) in NH₃ as well as in NF3 the atomic dipole and bond dipole are in the same direction
(c) in NH₃ the atomic dipole and bond dipole are in the same direction whereas in NF₃ these are in opposite directions
(d) in NH₃as well as in NF3 the atomic dipole and bond dipole are in opposite directions. 
Answer. C

Question. The correct order in which the O – O bond length increases in the following is
(a) O₂ < H₂O₂ < O₃
(b) O₃ < H₂O₂ < O₂
(c) H₂O₂ < O₂ < O₃
(d) O2 < O₃ < H₂O₂
Answer. D

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. Which of the following would have a permanent dipole moment?
(a) SiF4
(b) SF4
(c) XeF4
(d) BF3
Answer. B 

Question. H₂O is dipolar, whereas BeF₂ is not. It is because
(a) the electronegativity of F is greater than that of O
(b) H₂O involves hydrogen bonding whereas BeF₂ is a discrete molecule
(c) H₂O is linear and BeF₂ is angular
(d) H₂O is angular and BeF₂ is linear. 
Answer. A

Question. Which of the following molecules does not possess a permanent dipole moment?
(a) CS₂
(b) SO₃
(c) H₂S
(d) SO₂ 
Answer. D

Question. The table shown below gives the bond dissociation energies (Ediss) for single covalent bonds of carbon (C) atoms with element A, B, C and D. Which element has the smallest atoms?
Bond   Ediss(kJ mol^–1)
C-A       240
C-B       328
C-C       276
C-D       485
(a) C
(b) D
(c) A
(d) B
Answer. D

Question. Strongest bond is in between
(a) CsF
(b) NaCl
(c) both (a) and (b)
(d) none of the above.
Answer. D

Question. Which of the following bonds will be most polar?
(a) N – Cl
(b) O – F
(c) N – F
(d) N – N
Answer. C

Question. In the structure of ClF₃, the number of lone pairs of electrons on central atom ‘Cl’ is
(a) one
(b) two
(c) four
(d) three 
Answer. C

Question. Predict the correct order among the following :
(a) bond pair - bond pair > lone pair - bond pair > lone pair - lone pair
(b) lone pair - bond pair > bond pair - bond pair > lone pair - lone pair
(c) lone pair - lone pair > lone pair - bond pair > bond pair - bond pair
(d) lone pair - lone pair > bond pair - bond pair > lone pair - bond pair
Answer. B

Question. Which of the following species contains three bond pairs and one lone pair around the central atom?
(a) H₂O
(b) BF₃
(c) NH₂^–
(d) PCl₃ 
Answer. A

Question. Which of the following is not a correct statement?
(a) Multiple bonds are always shorter than corresponding single bonds.
(b) The electron-deficient molecules can act as Lewis acids.
(c) The canonical structures have no real existence.
(d) Every AB5 molecule does in fact have square pyramid structure. 
Answer. B

Question. Which of the following is not isostructural with SiCl₄?
(a) NH₄ ⁺
(b) SCl₄
(c) SO₄ ^2–
(d) PO₄ ^3– 
Answer. C

Question. In which of the following molecules all the bonds are not equal?
(a) NF₃
(b) ClF₃
(c) BF₃
(d) AlF₃
Answer. C

Question.Which of the following molecules has trigonal planar geometry?
(a) BF₃
(b) NH₃
(c) PCl₃
(d) IF₃ 
Answer. C

Question. In a regular octahedral molecule, MX6 the number of X – M – X bonds at 180° is
(a) three
(b) two
(c) six
(d) four. 
Answer. B

Question. In BrF₃  molecule, the lone pairs occupy equatorial positions to minimize
(a) lone pair - bond pair repulsion only
(b) bond pair - bond pair repulsion only
(c) lone pair - lone pair repulsion and lone pair - bond pair repulsion
(d) lone pair - lone pair repulsion only. 
Answer. A

Question. In NO₃^– ion, number of bond pair and lone pair of electrons on nitrogen atom are
(a) 2, 2
(b) 3, 1
(c) 1, 3
(d) 4, 0. 
Answer. C

Question. In which of the following bond angle is maximum?
(a) NH₃
(b) NH₄⁺
(c) PCl₃
(d) SCl₂ 
Answer. D

Question. The BCl₃ is a planar molecule whereas NCl₃ is pyramidal because
(a) nitrogen atom is smaller than boron atom
(b) BCl₃ has no lone pair but NC₃l has a lone pair of electrons
(c) B—Cl bond is more polar than N—Cl bond
(d) N—Cl bond is more covalent than B—Cl bond.
Answer. C

Question. In compound X, all the bond angles are exactly 109°28′, X is
(a) chloromethane
(b) carbon tetrachloride
(c) iodoform
(d) chloroform.
 Answer. D 

Question. Which of the following species contains equal number of s and p-bonds?
(a) (CN)₂
(b) (CH)₂(CN)₂
(c) HCO₃^–
(d) XeO₄,
Answer. D

Question. Which one of the following molecules contains no p bond?
(a) SO₂
(b) NO₂
(c) CO₂
(d) H₂O 
Answer. D

Question. Which one of the following statements is not correct for sigma- and pi- bonds formed between two carbon atoms?
(a) Sigma-bond is stronger than a pi-bond.
(b) Bond energies of sigma- and pi-bonds are of the order of 264 kJ/mol and 347 kJ/mol, respectively.
(c) Free rotation of atoms about a sigma-bond is allowed but not in case of a pi-bond.
(d) Sigma-bond determines the direction between carbon atoms but a pi-bond has no primary effect in this regard. 
Answer. B

Question. Main axis of a diatomic molecule is z, molecular orbital px and py overlap to form which of the following orbitals?
(a) p molecular orbital
(b) s molecular orbital
(c) d molecular orbital
(d) No bond will form. 
Answer. A

Question. Which statement is not correct?
(a) A sigma bond is weaker than a pi bond.
(b) A sigma bond is stronger than a pi bond.
(c) A double bond is stronger than a single bond.
(d) A double bond is shorter than a single bond.
Answer. A

Question. Linear combination of two hybridized orbitals belonging to two atoms and each having one electron leads to the formation of
(a) sigma bond
(b) double bond
(c) co-ordinate covalent bond
(d) pi bond. 
Answer. A

Question. Which of the following does not apply to metallic bond?
(a) Overlapping valence orbitals
(b) Mobile valence electrons
(c) Delocalized electrons
(d) Highly directed bonds 
Answer. D

Question. The angle between the overlapping of one s-orbital and one p-orbital is
(a) 180°
(b) 120°
(c) 109°28′
(d) 120°, 60° 
Answer. A

Question. Which of the following pairs of compounds is isoelectronic and isostructural?
(a) TeI₂, XeF₂
(b) IBr₂^–, XeF₂
(c) IF₃, XeF₂
(d) BeCl₂, XeF₂
Answer. None

Question. The hybridizations of atomic orbitals of nitrogen in NO⁺₂, NO^–3 and NH⁴⁺ respectively are
(a) sp, sp³ and sp²
(b) sp², sp³ and sp
(c) sp, sp² and sp³
(d) s^p2, sp and sp³
Answer. C

Question. Which of the following pairs of ions is isoelectronic and isostructural?
(a) CO₃^2–, NO₃^–
(b) ClO₃^–, CO₃^2–
(c) SO₃^2–, NO₃^–
(d) ClO₃^–, SO₃^2–
Answer. A,D

Question. The correct geometry and hybridization for XeF₄ are
(a) octahedral, sp³d²
(b) trigonal bipyramidal, sp³d
(c) planar triangle, sp³d³
(d) square planar, sp³d². 
Answer. A

Question. Among the following, which one is a wrong statement?
(a) PH5 and BiCl₅ do not exist.
(b) pp-dp bonds are present in SO₂.
(c) SeF₄ and CH₄ have same shape.
(d) I₃ ⁺ has bent geometry.
Answer. C

Question. In which of the following pairs, both the species are not isostructural?
(a) Diamond, Silicon carbide
(b) NH₃, PH₃
(c) XeF₄, XeO₄
(d) SiCl₄, PCl₄ ⁺ 
Answer. C

Question. Maximum bond angle at nitrogen is present in which of the following?
(a) NO₂⁺
(b) NO₃^–
(c) NO₂
(d) NO₂^–
Answer. A

Question. Which one of the following species has planar triangular shape?
(a) N₃
(b) NO₃^–
(c) NO₂^–
(d) CO₂ 
Answer. B

Question. XeF₂ is isostructural with
(a) SbCl₃
(b) BaCl₂
(c) TeF₂
(d) ICl₂^– 
Answer. D

Question. Which of the following is a polar molecule?
(a) SiF₄
(b) XeF₄
(c) BF₃
(d) SF₄
Answer. D

Question. The outer orbitals of C in ethene molecule can be considered to be hybridized to give three equivalent sp2 orbitals. The total number of sigma (s) and pi (p) bonds in ethene molecule is
(a) 3 sigma (s) and 2 pi (p) bonds
(b) 4 sigma (s) and 1 pi (p) bonds
(c) 5 sigma (s) and 1 pi (p) bonds
(d) 1 sigma (s) and 2 pi (p) bonds.
Answer. C

Question. Identify a molecule which does not exist.
(a) He₂
(b) Li₂
(c) C₂
(d) O₂
Answer. A

Question. Which of the following diatomic molecular species has only p bonds according to Molecular Orbital Theory?
(a) Be₂
(b) O₂
(c) N₂
(d) C₂ 
Answer. D

Question. Which of the following is paramagnetic?
(a) N₂
(b) H₂
(c) Li₂
(d) O₂
Answer. D

Question. Decreasing order of stability of O₂, O₂^–, O²⁺ andO₂^2– is
(a) O₂^2– > O₂^– > O₂ > O₂⁺
(b) O₂ > O₂⁺ > O₂^2– > O₂^–
(c) O₂– > O₂^2– > O₂⁺ > O₂
(d) O₂+ > O₂ > O₂^– > O₂^2–
Answer. D

Question. The correct bond order in the following species is
(a) O₂⁺ < O₂^– < O₂²⁺
(b) O₂– < O₂⁺ < O₂²⁺
(c) O₂²⁺ < O₂⁺ < O₂^–
(d) O₂²⁺ < O₂^– < O₂⁺
Answer. B

Question. Bond order of 1.5 is shown by
(a) O₂⁺
(b) O₂^–
(c) O₂^2–
(d) O₂
Answer. B

Question. Which of the following has the minimum bond length?
(a) O₂⁺
(b) O₂^–
(c) O₂^2–
(d) O₂
Answer. A

Question. The pairs of species of oxygen and their magnetic behaviour are noted below. Which of the following presents the correct description?
(a) O₂–, O₂^2– - Both diamagnetic
(b) O⁺, O₂^2– - Both paramagnetic
(c) O₂⁺, O₂ - Both paramagnetic
(d) O, O₂^2– - Both paramagnetic
Answer. C

Question. Which one of the following species does not exist under normal conditions?
(a) Be₂⁺
(b) Be₂
(c) B₂
(d) Li₂
Answer. B

Question. According to MO theory which of the lists ranks the nitrogen species in terms of increasing bond order?
(a) N₂^2– < N₂^– < N₂
(b) N₂ < N₂^2– < N₂^–
(c) N₂– < N₂^2– < N₂
(d) N₂ – < N₂ < N₂ ^2–
Answer. A

Question. Right order of dissociation energy N₂ and N₂⁺ is
(a) N₂> N₂⁺
(b) N₂= N₂⁺
(c) N₂⁺ > N₂
(d) none.
Answer. A

Question. N₂ and O₂ are converted into monocations, N₂⁺ andO₂⁺ respectively. Which is wrong?
(a) In O⁺₂ paramagnetism decreases.
(b) N₂⁺ becomes diamagnetic.
(c) In N₂⁺, the N–N bond weakens.
(d) In O₂⁺, the O–O bond order increases. 
Answer. B

Question. N₂ and O₂ are converted into monoanions N₂^– andO₂^– respectively, which of the following statements iswrong?
(a) In O₂^–, bond length increases.
(b) N₂^– becomes diamagnetic.
(c) In N₂^–, N–N bond weakens.
(d) In O₂^–, the O–O bond order decreases. 
Answer. B

Question. The ground state electronic configuration of valence shell electrons in nitrogen molecule (N2) is written as KK, s2s², s*2s², p²px² = p²py 2s²pz². Hence the bond order in nitrogen molecule is
(a) 2
(b) 3
(c) 0
(d) 1 
Answer. B

Question. Which of the following molecules has the highest bond order?
(a) O₂^–
(b) O₂
(c) O₂⁺
(d) O₂^2– 
Answer. C

Question. Which one of the following compounds shows the presence of intramolecular hydrogen bond?
(a) H₂O₂
(b) HCN
(c) Cellulose
(d) Concentrated acetic acid 
Answer. C

Question. What is the dominant intermolecular force or bond that must be overcome in converting liquid CH₃OH to a gas?
(a) Dipole-dipole interaction
(b) Covalent bonds
(c) London dispersion force
(d) Hydrogen bonding 
Answer. D

Question. In X – H Y, X and Y both are electronegative elements. Then
(a) electron density on X will increase and on H will decrease
(b) in both electron density will increase
(c) in both electron density will decrease
(d) on X electron density will decrease and on H increases. 
Answer. A

Question. Strongest hydrogen bond is shown by
(a) water
(b) ammonia
(c) hydrogen fluoride
(d) hydrogen sulphide.
Answer. C

Question. Which one shows maximum hydrogen bonding?
(a) H₂O
(b) H₂Se
(c) H₂S
(d) HF
Answer. A

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