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4.12, , 363. H-Bonding is exhibited by, , 364., , 365., , 366., , (A) all the molecules containing H-atoms, (B) molecules in which H_ is covalently, bonded to electronegative atoms F, O, or, , N <, , (C) molecules in which t Si atoms are, , present “, , (D) molecules in whigh? H is bonded to, atoms with lessefelectronegativity, , When H - F bongtiformed, (A) hydrogen |= cquires partial negative, , charge (@nd fluorine acquires partial, positive-charge, (B) hydrogen acquires partial positive, ge and fluorine acquires partial, gative charge, (Qs neither hydrogen nor fluorine acquires, any kind of charge, (D) shared electrons are present exactly at, the center of the bond, , Two ice cubes are pressed over each other, until they unite to form one block. Which one, of the following forces dominates for holding, them together? [Kerala CEE 2000}, (A) Dipole-dipole interaction, , (B) Vander Waals’ forces, , (C) Hydrogen bond, , (D) Covalent attraction, , Number of hydrogen bonds formed by one, molecule of water are, , (A) 1 (B) 2, , (CC) 3 (b) 4
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367., , 368., , 369., , 370., , 371., , 372., , 373., , Which of the following molecules cannot form, hydrogen bond?, , (A) H,0 (B) H-F, , (C) CHs (D) NHs, , NH; has higher boiling point than expected, because ‘, (A) NHs is nonpolar, , (B) it has strong intermolecular hydrogen, bonds, , it has strong intermolecular van der, Waal’s forces, , none of these, , (C), , (D), There is no hydrogen bonding in :, , (A) acetic acid (B) ammonia, , (C) ethyl alcohol (D) diethyl ether, The bond that determines the secondary, , structure of a protein is ;, [NCERT 1984; MP PET 1996], , (A) coordinate bond (B) covalent bond, , (C) hydrogenbond (D)_ ionic bond, , Water (H,0) is liquid while hydrogen sulphi, , (HLS) is a gas because - [(CPMT, , (A) water has higher molecular weight, , (B) hydrogen sulphide is a weak a, , (C) sulphur has high electron than, oxygen =, , water molecules ee, , hydrogen bondin, , The hydrides of the “SS, , 15-17, namely, , show abnormall, boiling points,, , @), , t elements in groups, and HF respectively, values for melting and, is due to 7, , [WB JEEM 2014], small size of N, O and F, the ability to form extensive, intermolecular H-bonding, the ability to form extensive, intramolecular H-bonding, effective van der Waals interaction, , , , , , (A), (B), , (C), , @), , HCI is a gas but HF is a low boiling liquid., , This is because INCERT 1984], , (A) H-F bond is strong, , (B) H-F bond is weak, , (C) molecules aggregate, hydrogen bonding, , (D) HF is a weak acid, , because of, , , , , 374., , 375., , 378,, , 379,, , , , Which of the following has the Strongeg, , H-bond? [WB JEE 2019;, (A) O-H--S, (B) S-H:-O, (C) FHF, (D) F-H:-0, , Hydrogen bonds are formed in many, compounds e. , HF, NH. The boiling, point of such jpounds depends to a large, , extent on trength of hydrogen bond ang, the on of hydrogen bonds. The, COR decreasing order of the boiling, points O£ above compounds is, [NCERT Exemplar|, HF > H,O > NH;, H2O > HF > NH;, , ), ce NH; > HF > H,O, , >, , 76., , (D) NH;>H,0>HF, , In which of the following substances will, hydrogen bond be strongest?, , [NCERT Exemplar], (B) H,0, , (@) HS, , (A) HCl, (C) HI, , . The boiling point of p-nitrophenol is higher, , than that of o-nitrophenol because:, (A) intramolecular hydrogen bonding exists, in p-nitrophenol. ‘, , (B) there is intermolecular hydrogen, bonding in p-nitrophenol., , (C) p-nitrophenol has a higher molecular, weight than o-nitrophenol., , (D) none of these., , Which of the following compound shows, intramolecular hydrogen bonding?, , (A) 0-nitrophenol, , (B) p-nitrophenol, , (C) phenol, , (D) methanol, , In which of the following compounds, intramolecular hydrogen bond is present?, , [MP PMT 19941, , (A) Ethyl alcohol, , (B) Water, , (C) Salicylaldehyde, (D) Hydrogen sulphide
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“ane oiling Point OF methanol is greater than, fy methylthiol because, 0), , there is intramolecular hydrogen, bonding in methanol and intermolecular, i hydrogen bonding in methylthiol, i) there is intermolecular hydrogen, bonding in methanol and no hydrogen, ponding in methylthiol, there is no hydrogen bonding «in, i methanol and intermolecular hydrogen, bonding in methylthiol, (D) there is intramolecular hydrogen, bonding in methanol and no hydrogen, bonding in methylthiol, , ig), Methanol and Ethanol are miscible in water, because of, , (B) hydrogen bonding, methanol/ethanol and water, , (C) ionic character of water, , (D) covalent character of water, , between, , 382. Acetic acid exists as dimer in benzene due to, 3 [CPMT 1982], (A) condensation reaction, (B) hydrogen bonding, (C) presence of carboxyl group, (D) none of the above, , 383. Water has high boiling point er, hydrides of VI group elements\\ This is, , because it is * Y, tur, , (A) liquid at the room tem, (B) covalent in nature, (C)_ associated trough Fone bonding, 4 (D) nota gas at roo! perature, NH Kx sling point than PHs, Shea a much hi oiling . aie, (A) NH; has larger molecular weight, , (B) NH, undergoes umbrella inversion, , (©) NH; forms hydrogen bond, drogen, (D) NH; contains ionic bonds whereas PH;, , contains covalent bonds, , 38 ., ® Which one has the highest ae point?, f, , , , (A) covalent character of methanol and ethanol, , >, , , , 386., , 387., , The boiling points of methanol, water and, diethyl ether are respectively 65 °C, 100 °C, and 34.5 °C. Which of the following best, explains these wide variations in b.p.?, , (A) The molecular mass increases from, , water (18) to methanol (32) to diethyl], ether (74)., , (B) The extent of H-bonding decreases from, water to methanol while it is absent in, ether., , (C) The extent of i olecular H-bonding, decreases from methanol to water., , (D) The number o} atoms per molecule, increases ter to methanol to ether., , Density of, ies ess’ than that of water, because of, , , , , , odification of ice, , porous structure of ice due to, ogen bonding, , ifference in the physical states, , a, Tf the electronic configuration of an element is, , o>, , 389., , 390., , 391., , 1s? 2s? 2p® 3s” 3p® 3d” 4s”, the four electrons, involved in chemical bond formation will be, , from [NCERT Exemplar], 3 6 3 6 2, , oe B) 3p. 4s,, , (C) 3p’, 3d (D) 3d’, 4s, , Amongst the following elements whose, electronic configurations are given below, the, one having the highest ionization enthalpy is, , : [NCERT Exemplar], (A) [Ne}3s'3p!, , (B) [Ne]3s°3p°, (C) [Ne]3s*3p*, (D) [Ar]3d'°4s74p°, , Helium molecule is monoatomic because, , , , (A) duplet state of He atom is fulfilled, , (B) _ it does not contain unpaired electrons, , (C) potential energy for the He-He system is, very high, , @), , all of the above, Which of the following compounds contain(s), , PMT 2002] no covalent bond(s)?, (A) Acet KCl, PHs, O2, BrHs, H2SO,, lone, i) [JEE (Main) Offline 2, © peetetes (A) KCl, BiH, PH; (B) KCLELSO., ©) Chloroform i ket ®) KCIBH,, , , , etme
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115. Bond length is, , (A) the equilibrium distance between the, nuclei of two bonded atoms in a molecule, , (B) the average distance between the centres, of nuclei of the two bonded atoms, , (C) the sum of the radius of the two, covalently bonded atoms i.e. r+ 1, , (D) all of the above, , 116. Carbon to carbon bond in acetylene is, (A) weaker than C - C bond, ‘(B)_ weaker than C = C bond, (C) longer than C - C bond, (D) _ shorter than C = C bond, , 117. In the series, ethane, ethylene and acetylene,, the carbon-hydrogen bond length is, (A) equal in all the three, (B) the largest in ethane, (C) _ the smallest in ethylene, (D) the largest in acetylene, , 118. Amongst the following molecules, the one, with the largest distance between the two, adjacent carbon atoms is, , , , (A) ethane (B) ethene, , (C) ethyne (D) benzene Oo, 119. The molecule with the shortest di, , between the two adjacent carbon a is, , (A) ethane (B) ethend_), , (C)_ ethyne ©) re, 120, Which among the fl od length, , - between poe atoms i sleet?, , |, (A) -C= 6., , |, © ae @) -e-6, 121. Bond energy is le of, (A) _ the energy required to break one mole 0, bonds of a diatomic molecule in gaseous, state into its constituent atoms, (B) average of the bond energies of the, constituent molecules, , , , (A) (i) and (ii), XN (C) (i) and (iii), , NY, , , , 122. The amount of energy given off or released, , per mole at the time of overlapping of orbitals, to form a bond is, , (A) _ bond energy, , (B) _ lattice energy, (C) nuclear energy, (D) activation energy, , 123. As the number of covalent bonds increases,, bond energy, (A) _ increases, (B) decreases, , (C) remains consta:, , (D) reduces to minim, 124. Bond energie: fNe N, H - H and Cl - Cl, and 243 kJ respectively., , , , , , Then, , 0) e reactive than H2 and Cl,, (ii) more reactive than Cl, and N2, (iii is more reactive than H), , 2 is more reactive than N2 but less, reactive than Cl,, , Be TRUE statements are, , (B) Gilly and (iv), , (D) only (iv), , 25. The bond energy is inversely proportional to, , (A) _ bond polarity, , (B) bond length, , (C) _ percent of s—character, (D) unsaturation character, , 126. In a covalent bond, the bond length, is the energy required to break the, bond., (A) | shorter ; greater, (B) | shorter ; smaller, (C) _ longer ; greater, (D) _ irrespective of ; same, 127. The bond energy of H; is greater than that of, I, because of __., (A) smaller bond Tength of Hydrogen, (B) _ larger bond length of Hydrogen, (C) no difference in the electronegativity of, I, molecule, (D) large value of electronegativity of iodine, 128. The bond energies of F2,Cl, Br: and I, are 37,, 58, 46, and 36 kcal/mol respectively. The, , (C) energy required to form excited state of strongest bond is poe —, the atom (A) Bre B) lL, (D) none of these © Ch @) F,
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129. C-—H bond energy among ethane, ethene and, , ethyne is, , (A) _ equal in all the three compounds, , (B) maximum in ethane, , (C) maximum in ethene, , (D) maximum in ethyne, , 130. Which of the following statements regarding, bond energies is FALSE?, , (A) Bond energy increases from a single, bond to a triple bond., , (B) The homolytic and heterolytic bond, dissociation energies for a given, molecule are considerably different., , (C) As the number of lone pairs on the, bonded atom increases, the bond energy, decreases., , (D) The bond energy decreases as the hybrid, orbitals have greater amount of, ‘s orbital contribution., , 131. Total energy required to break all the bonds in, , the molecule AB, is x kJ mol”. Then the bond, energy of bond A — B in the molecule will be, , , , = 7 mole, , (A) @®), , (C) 2xkJ mole (@) x - mi, Energy required to dissociate 4 g o: us, hydrogen into free gaseous atoms js*208 kcal, at 25°C. The bond energy of H = md will, , be s, 104 kcal mol! (B .4 kcal mol!, kcal mol"!, , (A), 1040 keal mol, e, The order of bond en H-F,H-Cl,, H-Br,H-lis:, , (C), , (A) H-F>H- -Br>H-I, (B) H-Cl> >H-Br>H-I, (©) H-I> r>H-Cl>H-F, (D) H-Br>H-I>H-CI>H-F, , Average bond energy values can be used to, calculate which of the following?, , (A) The energy content of the molecule, , (B) Heat of formation, , (C) Heat of reaction, , (D) All ofthese, , ~ kJ mole”, 2, , 132., , , , 133., , 134., , 135. The bond angle in a water molecule is, (A) 120° (B) 180°, , (C) 109°28' (D) 104°35", , 136., , RO, , 4 oO en), S, , 140., , 141,, , 142,, , , , 137., , 138., , ©, , 139., , As the s-character of hybridization orbj, increases, the bondangle, , (A) increases (B) decreases, (C) doesnot change (D) becomes Zero, , Due to the presence of unhybridized Orbitals,, the bondangle_, , (A) increases, (B) decreases, (C) remains sami, (D) doesn’t de on unhybridized Orbitals, Consider th moNectiles CHa, NH3 and H,0,, Which of thigh statements is FALSE?, , ‘ [NEET P-I 2016), (A) — O — H bond angle in H,0 jg, , aller than the H — N — H bond angle, H3., , H — C — H bond angle in CH, is, larger than the H — N — H bond angle in, NH., C) The H —-C-—H bond angle in CHy, the, H — N -H bond angle in NHs, and the, H — O —H bond angle in H,0O are all, greater than 90°., The H — O — H bond angle in H,0 is, larger than the H — C — H bond angle in, CH4., , In which of the following is the angle between, the two covalent bonds greatest?, , [NCERT 1975; AMU 1982; MNR 1987;, , IIT 1981; CPMT 1988; MP PMT 1994], (A) CO, (B) CH,, (©) NH; (D) #20, The CORRECT order of bond angles (smallest, first) in H.S, NH3, BF; and SiH, is:, , [AIEEE 2004], , (A) HS < NH; < SiH, < BF;, (B) NH3<H2S < SiH, < BF;, (C) HS < SiH, < NH; <BF;, (D) HS <NH3< BF3< SiHy, , The order of increasing bond angle in the, molecules BeCl,, BC]; and CCL is___, , (A) CCl, < BCl < BeCh, , (B) BeCh <BCl <CCh, , (C) CCk <BeCh < BCI, , (D) BCh<BeCh <CCL, , Higher the bond order, greater is, (A) _ bond dissociation energy, (B) bond length, , (C) both (A) and (B), , (D) neither (A) nor (B), , ita]
