Free NEET Chemistry multiple-choice questions on VSEPR Theory. Attempt each question and reveal the answer with a full explanation.
The species, having bond angles of 120 ∘ is: BCl 3 PH 3 ClF 3 NCl 3 The shape of the hydronium ion ( H 3O + ) is: Pyramidal Tetrahedral Trigonal planar Bent The bond angle in Cl 2O is 110.9 , which is larger than the bond angle in H 2O ( 104.5 ). This is primarily due to: Steric repulsion between the large Chlorine atoms Higher electronegativity of Oxygen in Cl 2O Stronger lone pair-lone pair repulsion in H 2O p - d back bonding in Cl 2O The geometry and hybridization of the XeF 5 + ion are: Square pyramidal, sp 3d 2 Octahedral, sp 3d 2 Trigonal bipyramidal, sp 3d Pentagonal planar, sp 3d 3 In the ClO 2 molecule, the O-Cl-O bond angle is 118 . This value, being larger than expected, is explained by: Repulsion involving the single unpaired electron on Chlorine Stronger O-O repulsion Perfect sp 2 hybridization Absence of lone pairs The correct order of bond angles for the phosphorus trihalides is: PI 3 > PBr 3 > PCl 3 > PF 3 PF 3 > PCl 3 > PBr 3 > PI 3 PCl 3 > PF 3 > PI 3 > PBr 3 PF 3 > PI 3 > PBr 3 > PCl 3 Match the species in List-I with their geometry in List-II. A-IV, B-III, C-I, D-II A-III, B-IV, C-I, D-II A-III, B-I, C-II, D-IV A-III, B-II, C-I, D-IV In the white phosphorus ( P 4 ) molecule, the P-P-P bond angle is: 60 90 109 28' 120 The number of lone pairs on the central Bromine atom in BrF 5 is: 1 2 0 3 The H-N-H bond angle in NH 4 + is higher than in NH 3 because: In NH 4 + , there are no lone pairs to repel the bond pairs Nitrogen is sp 2 hybridized in NH 4 + NH 4 + has a square planar shape NH 4 + has more electrons Which of the following is linear? CO 2 SO 2 NO 2 ClO 2 Which of the following molecules has trigonal planner geometry ; NH3 BF3 PCl3 IF3 Which of the following would have a permanent dipole moment - BF3 SF4 SiF4 XeF4 Which of the following species has a linear shape:- NO2- SO2 NO2+ O3 Which of the following is not isostructural with SiCl4 :- SCl4 SO4 2- PO4 3- NH4+ In which of the following molecules / ions BF 3 , NO 2 - , NH 2 - and H 2O , the central atom is sp 2 hybridized ? BF 3 and NO 2 - NO 2 - and NH 2 - NH 2 - and H 2O NO 2 - and H 2O The correct order of bond angles in CH 4 , NH 3 , and H 2O is: CH 4 > NH 3 > H 2O H 2O > NH 3 > CH 4 NH 3 > CH 4 > H 2O CH 4 = NH 3 = H 2O XeF2 is isostructural with TeF2 ICl2 - SbCl3 BaCl2 Which one of the following species has plane triangular shape ? N3 - NO3 - NO2 - CO2 Consider the molecules CH4 , NH3 and H2O . Which of the given statements is false ? 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 The H-O-H bond angle in H2O is larger than the H-C-H bond angle in CH4 . The H-O-H bond angle in H2O is smaller than the H-N-H bond angle in NH3 . The H-C-H bond angle in CH4 is larger than the H-N-H bond angle in NH3 . Predict the correct order among the following :- lone pair - lone pair > lone pair - bond pair > bond pair - bond pair lone pair - lone pair > bond pair - bond pair > lone pair - bond pair bond pair - bond pair > lone pair - bond pair > lone pair - lone pair lone pair - bond pair > bond pair - bond pair > lone pair - lone pair Which of the following hydrides has the largest bond angle? H2Se H2S H2Te H2O In the structure of ClF3 , the number of lone pair of electrons on central atom 'Cl' is Four Two One Three Identify the incorrect statement related to PCl5 from the following: PCl5 molecule is non-reactive Three equatorial P–Cl bonds make an angle of 120° with each other Two axial P–Cl bonds make an angle of 180° with each other Axial P–Cl bonds are longer than equatorial P–Cl bonds BF3 is planar and electron deficient compound. Hybridization and number of electrons around the central atom, respectively are : sp 3 and 6 sp 2 and 6 sp 2 and 8 sp 3 and 4 Amongst the following which one will have maximum ‘lone pair - lone pair’ electron repulsions? IF5 SF4 XeF2 ClF3 Match List I with List II. array ll List I (Compound) & List II (Shape/geometry) A. NH3 & I. Trigonal Pyramidal B. BrF5 & II. Square Planar C. XeF4 & III. Octahedral D. SF6 & IV. Square Pyramidal array Choose the correct answer from the options given below: A-I, B-IV, C-II, D-III A-II, B-IV, C-III, D-I A-III, B-IV, C-I, D-II A-II, B-III, C-IV, D-I Among the following, which one is a planar molecule? XeF 4 NF 3 PH 3 SiF 4 Identify the correct statement about ClF3 from the following options : It has T-shaped geometry with three lone pairs on Cl atom. It has T-shaped geometry with two lone pairs on Cl atom. It has a trigonal pyramidal geometry with two lone pairs on Cl atom. It has a planar trigonal geometry with two lone pairs on Cl atom. The shape of the SnCl 2 molecule in the gaseous state is: Bent Linear Tetrahedral T-shaped Which of the following molecules is isostructural with BF 3 ? NO 3 - NH 3 PCl 3 NF 3 Which of the following species has a linear shape despite having lone pairs on the central atom? I 3 - ClO 2 SO 2 O 3 In BrF 3 , the central Bromine atom has how many lone pairs and what is the shape? 2 lone pairs, T-shaped 1 lone pair, Trigonal Planar 2 lone pairs, Trigonal Pyramidal 3 lone pairs, Linear Which one of the following is not isostructural with SiCl 4 ? SCl 4 NH 4 + PO 4 3- SO 4 2- Which of the following has the maximum number of lone pairs on the central atom? XeF 2 I 3 - ClF 3 XeF 2 and I 3 - both The geometry of BeCl 2 in the solid state is: Chain structure Linear Dimer Tetrahedral Which of the following pairs is isostructural and isoelectronic? ClO 3 - and XeO 3 CO 3 2- and SO 3 2- ClO 3 - and CO 3 2- SO 3 and NO 3 - The shape of XeO 3 molecule is: Pyramidal Trigonal planar T-shaped Square planar Which of the following molecules has a zero dipole moment? PCl 5 PCl 3 SF 4 ClF 3 The species ICl 2 - has a linear shape. The number of lone pairs on the central Iodine atom is: 3 2 1 0 The bond angle in OF 2 is less than 109 28' because of: Lone pair - Lone pair repulsion Bond pair - Bond pair repulsion Electronegativity of Fluorine All of the above Among the following, the pair in which the two species are NOT isostructural is: SiF 4 and SF 4 IO 3 - and XeO 3 BH 4 - and NH 4 + PF 6 - and SF 6 The geometry and hybridization of the central atom in the XeO 2F 2 molecule are respectively: Seesaw, sp 3d Trigonal bipyramidal, sp 3d Square planar, sp 3d 2 Tetrahedral, sp 3 Which of the following pairs of species has the same shape (isostructural)? ClO 3 - and SO 3 2- CO 3 2- and SO 3 2- BF 3 and NF 3 CF 4 and SF 4 In which of the following molecules/ions is the central atom sp 3 hybridized but the molecular shape is not tetrahedral? ClO 2 - BF 4 - NH 4 + CH 4 The molecular geometry of TeCl 4 is: Seesaw Square planar Tetrahedral Octahedral According to VSEPR theory, the geometry of the ICl 4 - ion is: Square planar Tetrahedral Octahedral Pyramidal Which of the following pairs has the same number of lone pairs on the central atom? XeF 2 and I 3 - ClF 3 and XeF 4 SF 4 and XeF 2 NH 3 and H 2O Which of the following describes the shape and hybridization of the I 3 + ion? Bent, sp 3 Linear, sp 3d Linear, sp Bent, sp 2 In the structure of ClF 3 , the number of lone pairs of electrons on central atom 'Cl' is: 2 3 4 1 In SF 4 , the F axial -S-F axial bond angle is approximately 173 instead of 180 . This distortion is due to: Lone pair-Bond pair repulsion Bond pair-Bond pair repulsion Lone pair-Lone pair repulsion Reduction in electronegativity of Sulfur The dihedral angle of H 2O 2 in the gaseous phase is approximately: 111.5 90.2 104.5 180 The bond angle in NCl 3 is 107 , while in NF 3 it is 102 . This difference is because: Electronegativity of F is higher than Cl , pulling bond pairs away from N Electronegativity of Cl is higher than F Lone pair on N is more active in NCl 3 Size of F is larger than Cl The dipole moment of SO 2 is non-zero ( 1.63 D ), but that of SO 3 is zero ( 0 D ). This is because: SO 3 is trigonal planar and symmetric, whereas SO 2 is bent SO 2 is linear and SO 3 is trigonal planar Sulfur has a higher oxidation state in SO 3 S-O bonds in SO 2 are more polar In which of the following molecules is the bond angle F-O-F smallest? OF 2 OCl 2 H 2O SF 2 The geometry of PbCl 2 in the gaseous phase is: Bent (V-shaped) Linear Tetrahedral Trigonal planar In the gas phase, PCl 5 has a trigonal bipyramidal geometry. The two axial P-Cl bonds are longer than the three equatorial P-Cl bonds because: Axial bonds suffer more repulsion from equatorial bonds Equatorial bonds suffer more repulsion from axial bonds Axial bonds have more s-character Equatorial bonds have more d-character The molecular geometry of XeO 3F 2 is: Trigonal bipyramidal See-saw Square pyramidal Octahedral Which of the following pairs is isostructural? ClO 3 - and XeO 3 CO 2 and SO 2 BF 3 and NF 3 ClF 3 and BF 3 In the BrF 5 molecule, the F axial -Br-F equatorial bond angles are: Less than 90 Exactly 90 Exactly 180 Greater than 90 Which of the following molecules has a pentagonal bipyramidal geometry? IF 7 SF 6 PCl 5 BF 3 In the linear XeF 2 molecule, the three lone pairs on the Xenon atom are arranged: In the equatorial positions of a trigonal bipyramid In the axial positions of a trigonal bipyramid At the corners of an equilateral triangle around the axis Randomly around the nucleus The F-Cl-F bond angle in ClF 3 is slightly less than 90 (approx 87.5 ) due to: Lone pair-lone pair repulsion Bond pair-bond pair repulsion Lone pair-bond pair repulsion The presence of d-orbitals Which of the following species is linear? N 3 - NO 2 - O 3 SO 2 The number of lone pairs of electrons on the central atoms of XeF 2 , XeF 4 and XeF 6 are respectively: 3, 2 and 1 2, 3 and 1 2, 3 and 0 3, 2 and 0 The molecular geometry and hybridization of the Xenon atom in XeO 4 are respectively: Tetrahedral, sp 3 Square planar, sp 3d 2 Trigonal bipyramidal, sp 3d Pyramidal, sp 3 Which of the following pairs of ions are isostructural? SO 4 2- and ClO 4 - SO 3 2- and NO 3 - ClO 3 - and CO 3 2- CO 3 2- and SO 3 2- The shape of the azide ion ( N 3 - ) is: Linear Bent Trigonal planar T-shaped The I-I-I bond angle in the triiodide ion ( I 3 - ) is: 180 120 109 28' 90 Which of the following are the bond angles present in the SF 6 molecule? 90 and 180 120 and 90 109 28' 90 only The molecular geometry and the hybridization of the central Iodine atom in the IF 4 - ion are: Square planar, sp 3d 2 Octahedral, sp 3d 2 Tetrahedral, sp 3 See-saw, sp 3d The number of lone pairs on the central Xenon atom in XeF 6 is: 1 2 3 0 Which of the following pairs is isostructural with N 2O ? CO 2 NO 2 SO 2 O 3 Which of the following species has the smallest bond angle? H 2S NH 3 CH 4 H 2O The species ICl 2 - is isostructural with: XeF 2 ICl 2 + SnCl 2 SO 2 Which of the following molecules has a zero dipole moment due to its symmetrical structure? XeF 4 SF 4 NF 3 H 2O Which of the following pairs of ions are isoelectronic and isostructural? CO 3 2- , NO 3 - ClO 3 -, CO 3 2- SO 3 2- , NO 3 - ClO 3 -, SO 3 2- The geometry of XeF 4 is: Square Planar Octahedral Trigonal Bipyramidal Tetrahedral In which of the following molecules all the bonds are not equal? PCl 5 CH 4 BF 3 SF 6 Which of the following has a square pyramidal shape? BrF 5 XeF 4 PCl 5 SF 6 Which molecule has the smallest bond angle? H 2S H 2O NH 3 CH 4 The geometry of the SF 4 molecule, according to VSEPR theory, is described as: See-saw Tetrahedral Square planar Trigonal bipyramidal The molecular geometry of TeF 6 is: Octahedral Pentagonal bipyramidal Square pyramidal Trigonal bipyramidal Which of the following molecules has a square pyramidal shape? BrF 5 PCl 5 XeF 4 SF 6 In the PCl 5 molecule, the axial P-Cl bonds are longer than the equatorial P-Cl bonds because: Axial bonds suffer more repulsion from equatorial bond pairs Equatorial bonds suffer more repulsion from axial bond pairs Axial bonds have more s-character Equatorial bonds have more p-character In which of the following molecules all the bonds are not equal:- ClF3 BF3 AlF3 NF3 Which of the following is not a correct statement:- The electron-deficient molecules can act as Lewis acids The canonical structures have no real existence Every AB5 molecule does infact have square pyramid structure Multiple bonds are always shorter than corresponding single bonds In which of the following pairs, the two species are iso-structure? SO3 2- and NO3 - BF3 and NF3 BrO3 - and XeO3 SF4 and XeF4 Match the compounds given in column I with the hybridisation and shape given in column II and mark the correct option. array llll ; & Column-I & ; & Column-II (a) & XeF6 & (i) & Distorted octahedral (b) & XeO3 & (ii) & Square planar (c) & XeOF4 & (iii) & pyramidal (d) & XeF4 & (iv) & Square pyramidal array a-i, b-iii, c-iv, d-ii a-i, b-ii, c-iv, d-iii a-iv, b-iii, c-i, d-ii a-iv, b-i, c-ii, d-iii The ionic radii of A+ and B- ions are 0.98 10 -10 m and 1.81 10 -10 m . The coordination number of each ion in AB is :- 6 4 8 2 Which of the following pair of species is not iso-structural? BrO3 - , XeO3 ICl4 - , XeF4 ClO3 - , CO3 2- IBr2 - , XeF2 The structures of beryllium chloride in solid state and vapour phase, are : Linear in both Dimer and Linear, respectively Chain in both Chain and dimer, respectively Match List-I with List-II. array ll List-I & List-II (a) PCl5 & (i) Square pyramidal (b) SF6 & (ii) Trigonal planar (c) BrF5 & (iii) Octahedral (d) BF3 & (iv) Trigonal bipyramidal array Choose the correct answer from the options given below. (a)-(ii), (b)-(iii), (c)-(iv), (d)-(i) (a)-(iii), (b)-(i), (c)-(iv), (d)-(ii) (a)-(iv), (b)-(iii), (c)-(ii), (d)-(i) (a)-(iv), (b)-(iii), (c)-(i), (d)-(ii) In the dimer of Aluminum chloride ( Al 2Cl 6 ), the number of bridge and terminal Al-Cl bonds are respectively: 2 and 4 4 and 2 3 and 3 2 and 6 Match List-I with List-II array ll List-I & List-II A. XeO3 & (I) sp 3d ; linear B. XeF2 & (II) sp 3 ; pyramidal C. XeOF4 & (III) sp 3d 3 ; distorted octahedral D. XeF6 & (IV) sp 3d 2 ; square pyramidal array Choose the correct answer from the options given below : A-IV, B-II, C-I, D-III A-II, B-I, C-IV, D-III A-II, B-I, C-III, D-IV A-IV, B-II, C-III, D-I The molecular geometry of XeF 6 is best described as: Distorted octahedral Octahedral Pentagonal bipyramidal Square pyramidal The correct order of bond angles for the following species is: NO 2 + > NO 2 > NO 2 - NO 2 + > NO 2 - > NO 2 NO 2 > NO 2 + > NO 2 - NO 2 - > NO 2 > NO 2 + The bond angle H-O-H in water is 104.5 , but in H 2S , the H-S-H bond angle is approximately 92 . This is because: Sulfur is less electronegative than Oxygen, so bond-pair bond-pair repulsion is less. Sulfur has larger size, increasing lone-pair lone-pair repulsion. Sulfur uses pure p-orbitals for bonding instead of sp 3 hybrids. Oxygen has a higher degree of s-character in its bonds. The species XeF 5 - has which of the following geometries according to VSEPR theory? Pentagonal planar Pentagonal bipyramidal Octahedral Square pyramidal Which of the following molecules has a bond angle of approximately 101.5 , which is less than the tetrahedral angle due to lone pair-bond pair repulsion, but larger than the angle in H 2O ? NF 3 NH 3 H 2O BF 3 Which of the following is the correct order of bond angles for the nitrogen species provided? NO 2 + > NO 2 > NO 2 - NO 2 + > NO 2 - > NO 2 NO 2 - > NO 2 > NO 2 + NO 2 > NO 2 + > NO 2 - The bond angle in NH 3 ( 107 ) is significantly larger than in NF 3 ( 102 ). This is primarily because: Nitrogen is more electronegative than Hydrogen, shifting bond pairs closer to Nitrogen Fluorine is more electronegative than Nitrogen, shifting bond pairs away from Nitrogen The lone pair on Nitrogen in NF 3 repels more than the lone pair in NH 3 The size of the Fluorine atom is larger than the Hydrogen atom In the molecule PCl 3F 2 , according to Bent's Rule, where are the fluorine atoms most likely to be positioned in the trigonal bipyramidal geometry? Both at the axial positions Both at the equatorial positions One axial and one equatorial position Fluorine atoms do not occupy specific positions In the solid state, Phosphorus pentabromide ( PBr 5 ) exists as: [PBr 4] + Br - [PBr 4] + [PBr 6] - [PBr 3] + [PBr 7] - P 2Br 10 molecules