JEE Chemistry Chemical Bonding and Molecular Structure MCQs Set 52

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Multiple Choice Questions

Question 1: The incorrect order of solubility in water is:
(a) Ca(OH)2 < Sr(OH)2 < Ba(OH)2
(b) Li2CO3 < Na2CO3 < K2CO3
(c) AgF < AgCl < AgBr
(d) BaSO4 < MgSO4
Show Answer & Explanation

Answer: (c) AgF < AgCl < AgBr

Explanation:
1. AgF is very soluble in water, whereas AgCl and AgBr are sparingly soluble, so the order should be AgF > AgCl > AgBr.
2. The other orders are correct.
3. Answer: (c)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 2: Which of the following statements is incorrect?
(a) In O2- and O2+ the magnetic behaviour is not changed
(b) In N2+ and N2- the magnetic moment remains unchanged
(c) If the z-axis is the overlapping axis, the px orbital of one atom and the dxy orbital of another atom result in an antibonding molecular orbital
(d) None of these
Show Answer & Explanation

Answer: (c) If the z-axis is the overlapping axis, the px orbital of one atom and the dxy orbital of another atom result in an antibonding molecular orbital

Explanation:
1. The px and dxy orbitals have a net overlap of zero along the z-axis, so they form no bonding or antibonding combination.
2. O2+ and O2- are both paramagnetic and N2+ and N2- each have one unpaired electron, so statements (1) and (2) are correct.
3. Answer: (c)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 3: Which statement is correct in the following?
(a) NH3 > NF3 : bond angle
(b) NH3 > NF3 : reactivity towards Lewis acids
(c) NH3 > NF3 : dipole moment
(d) All are correct
Show Answer & Explanation

Answer: (d) All are correct

Explanation:
1. NH3 has a bond angle of 107° against 102° for NF3, it is a much better donor to Lewis acids, and its dipole moment (1.47 D) is higher than that of NF3 (0.24 D).
2. Answer: (d)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 4: The species having no pπ–pπ bond but with bond order equal to that of O2 is:
(a) XeO3
(b) ClO3-
(c) PO43-
(d) SO42-
Show Answer & Explanation

Answer: (a) XeO3

Explanation:
1. In XeO3 three dπ–pπ bonds are shared by three Xe–O bonds, giving an order of 2 and no pπ–pπ bond.
2. The bond orders of the others are 5/3, 5/4 and 3/2.
3. Answer: (a)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 5: Which has a giant covalent structure?
(a) PbO2
(b) SiO2
(c) NaCl
(d) AlCl3
Show Answer & Explanation

Answer: (b) SiO2

Explanation:
1. SiO2 is a three-dimensional network of Si–O covalent bonds.
2. NaCl is ionic and AlCl3 is molecular (dimeric); PbO2 is largely ionic.
3. Answer: (b)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 6: A molecule which cannot exist theoretically is:
(a) SF4
(b) OF2
(c) OF4
(d) O2F2
Show Answer & Explanation

Answer: (c) OF4

Explanation:
1. Oxygen is in period 2 with no d-orbitals, so it cannot expand its octet to form OF4.
2. SF4, OF2 and O2F2 exist.
3. Answer: (c)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 7: Select the correct relation between the dipole moments of CH3OH and CH3SH.
(a) μ(CH3OH) = μ(CH3SH)
(b) μ(CH3OH) > μ(CH3SH)
(c) μ(CH3OH) < μ(CH3SH)
(d) Cannot be compared
Show Answer & Explanation

Answer: (b) μ(CH3OH) > μ(CH3SH)

Explanation:
1. Oxygen is more electronegative than sulphur, so the C–O–H unit is more polar.
2. μ(CH3OH) is about 1.7 D against 1.5 D for CH3SH.
3. Answer: (b)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 8: Which of the following species has the same number of σ and π bonds?
(a) C2H6
(b) C2(CN)4
(c) C2H4
(d) HC≡CH
Show Answer & Explanation

Answer: (b) C2(CN)4

Explanation:
1. C2(CN)4: σ bonds = 1 (C=C) + 4 (C–CN) + 4 (C≡N) = 9; π bonds = 1 + 8 = 9.
2. The others have 7σ and 0π, 5σ and 1π, and 3σ and 2π.
3. Answer: (b)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 9: In which of the following pairs are the two species iso-structural?
(a) SO32- and NO3-
(b) BF3 and NF3
(c) BrO3- and XeO3
(d) SF4 and XeF4
Show Answer & Explanation

Answer: (c) BrO3- and XeO3

Explanation:
1. BrO3- and XeO3 are both pyramidal with one lone pair.
2. SO32- is pyramidal and NO3- planar, BF3 planar and NF3 pyramidal, SF4 see-saw and XeF4 square planar.
3. Answer: (c)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 10: The hybridisation of P in the phosphate ion (PO43-) is the same as that of:
(a) I in ICl4-
(b) S in SO3
(c) N in NO3-
(d) S in SO32-
Show Answer & Explanation

Answer: (d) S in SO32-

Explanation:
1. P in PO43- has four sigma bonds and no lone pair: sp3.
2. S in SO32- has three sigma bonds and one lone pair: sp3; I in ICl4- is sp3d2, and S in SO3 and N in NO3- are sp2.
3. Answer: (d)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 11: The bond order of NO is:
(a) 1.0
(b) 1.5
(c) 2.0
(d) 2.5
Show Answer & Explanation

Answer: (d) 2.5

Explanation:
1. NO has 15 electrons in total (11 valence); the molecular orbital configuration gives (8 – 3)/2 = 2.5.
2. Answer: (d)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 12: Two ice cubes pressed together unite to form one cube. Which force is responsible for holding them together?
(a) van der Waals forces
(b) Covalent attraction
(c) Hydrogen bond formation
(d) Dipole–dipole attraction
Show Answer & Explanation

Answer: (c) Hydrogen bond formation

Explanation:
1. Water molecules at the two surfaces form hydrogen bonds with one another, joining the cubes (regelation).
2. Answer: (c)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 13: If d represents the bond length, select the correct relation.
(a) d(N2) = d(N2+) and d(O2) = d(O2+)
(b) d(N2) < d(N2+) and d(O2) > d(O2+)
(c) d(N2) < d(N2+) and d(O2) < d(O2+)
(d) d(N2) > d(N2+) and d(O2) > d(O2+)
Show Answer & Explanation

Answer: (b) d(N2) < d(N2+) and d(O2) > d(O2+)

Explanation:
1. Removing a bonding electron from N2 lowers the bond order from 3 to 2.5, so the bond lengthens.
2. Removing an antibonding electron from O2 raises the order from 2 to 2.5, so the bond shortens.
3. Answer: (b)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 14: Which of the following conducts electricity?
(a) Diamond
(b) KCl
(c) KCl (fused)
(d) BaSO4
Show Answer & Explanation

Answer: (c) KCl (fused)

Explanation:
1. Fused KCl contains mobile K+ and Cl- ions.
2. Diamond has no free electrons and solid KCl and BaSO4 have immobile ions.
3. Answer: (c)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 15: What hybridisation is expected on the central atom of each of the following molecules? (i) BeH2 (ii) CH2Br2 (iii) PF6- (iv) BF3
(a) sp2, sp, sp3, sp2
(b) sp, sp3, sp3d, sp2
(c) sp, sp3, sp3d2, sp2
(d) sp2, sp, sp2, sp3
Show Answer & Explanation

Answer: (c) sp, sp3, sp3d2, sp2

Explanation:
1. BeH2 has 2 bond pairs: sp. CH2Br2 has 4: sp3.
2. PF6- has 6: sp3d2. BF3 has 3: sp2.
3. Answer: (c)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 16: What is the value of 1 debye in SI units?
(a) 3.336 × 10-30 C m
(b) 33.36 × 10-30 C m
(c) 333.6 × 10-30 C m
(d) None of these
Show Answer & Explanation

Answer: (a) 3.336 × 10-30 C m

Explanation:
1. 1 D = 10-18 esu cm = 3.336 × 10-30 C m.
2. Answer: (a)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 17: Which of the following molecules has a planar structure?
(a) O2SF2
(b) OSF2
(c) XeF4
(d) ClO4-
Show Answer & Explanation

Answer: (c) XeF4

Explanation:
1. XeF4 is square planar.
2. O2SF2 and ClO4- are tetrahedral and OSF2 is pyramidal.
3. Answer: (c)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 18: Which type of shape is found in the SF2 molecule?
(a) V-shaped
(b) Bipyramidal
(c) Linear
(d) Irregular tetrahedron
Show Answer & Explanation

Answer: (a) V-shaped

Explanation:
1. SF2 has two bond pairs and two lone pairs (sp3), so it is bent (V-shaped).
2. Answer: (a)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 19: The hybridisation of the central atom in XeF2, XeF4 and XeF6 respectively is:
(a) sp3d3, sp3d2, sp3d
(b) sp3d, sp3d3, sp3d2
(c) sp3, sp3, sp3
(d) sp3d, sp3d2, sp3d3
Show Answer & Explanation

Answer: (d) sp3d, sp3d2, sp3d3

Explanation:
1. The numbers of electron pairs around Xe are 5, 6 and 7.
2. These give sp3d, sp3d2 and sp3d3.
3. Answer: (d)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 20: The correct sequence of decreasing bond angle of the following hydrides is:
(a) NH3 > PH3 > AsH3 > SbH3
(b) SbH3 > AsH3 > PH3 > NH3
(c) PH3 > AsH3 > SbH3 > NH3
(d) PH3 > NH3 > AsH3 > SbH3
Show Answer & Explanation

Answer: (a) NH3 > PH3 > AsH3 > SbH3

Explanation:
1. Bond angles: NH3 107°, PH3 93.5°, AsH3 91.8°, SbH3 91.3°.
2. The angle falls as the central atom becomes less electronegative and larger.
3. Answer: (a)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 21: Which of the following is soluble in water?
(a) CS2
(b) C2H5OH
(c) CCl4
(d) CHCl3
Show Answer & Explanation

Answer: (b) C2H5OH

Explanation:
1. Ethanol forms hydrogen bonds with water and is miscible with it.
2. CS2, CCl4 and CHCl3 are non-polar or weakly polar and dissolve very little.
3. Answer: (b)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 22: Which of the following is correct?
(a) SOF2 > SOCl2 > SOBr2 (F–S–X bond angle)
(b) SF4 > XeF4 (dipole moment)
(c) BF3 < BCl3 < BBr3 (bond angle)
(d) PO43- < SO42- < ClO4- (bond length)
Show Answer & Explanation

Answer: (b) SF4 > XeF4 (dipole moment)

Explanation:
1. SF4 is see-saw and polar, while XeF4 is square planar with zero dipole moment.
2. The X–S–F angles rise from SOF2 to SOBr2, all boron trihalides have 120°, and the bond lengths fall from PO43- to ClO4-.
3. Answer: (b)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 23: Which molecule has the highest dipole moment?
(a) CH3Cl
(b) CH2Cl2
(c) CHCl3
(d) CCl4
Show Answer & Explanation

Answer: (a) CH3Cl

Explanation:
1. Dipole moments (D): CH3Cl 1.86, CH2Cl2 1.60, CHCl3 1.04, CCl4 0.
2. Answer: (a)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 24: The carbon atoms in C2(CN)4 are:
(a) sp-hybridised
(b) sp2-hybridised
(c) sp- and sp2-hybridised
(d) sp-, sp2- and sp3-hybridised
Show Answer & Explanation

Answer: (c) sp- and sp2-hybridised

Explanation:
1. The two carbons of the C=C bond are sp2.
2. The four nitrile carbons (C≡N) are sp.
3. Answer: (c)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

Question 25: How many bond pairs and lone pairs surround the central atom in the I3- ion?
(a) 2 bond pairs and 2 lone pairs
(b) 2 bond pairs and 3 lone pairs
(c) 3 bond pairs and 2 lone pairs
(d) 4 bond pairs and 3 lone pairs
Show Answer & Explanation

Answer: (b) 2 bond pairs and 3 lone pairs

Explanation:
1. The central I has 7 + 1 (charge) + 2 (from the end atoms) = 10 electrons, or 5 pairs.
2. Two are bond pairs and three are lone pairs, giving a linear shape.
3. Answer: (b)

Teacher's Note:
1. Work through each option against the rule or structure involved before choosing. Remember the exceptions your textbook lists.

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Multiple Choice Questions (MCQs) for JEE Chemistry Chemical Bonding and Molecular Structure

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