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- B) Mg6+ C) Mg2+ D) Mg6- E) Mg2-
2) Based on the octet rule, phosphorus most likely forms a __________ ion.
A) P5- B) P5+ C) P+ D) P3- E) P3+
3) Which ion below has a noble gas electron configuration?
A) B2+ B) Be2+ C) C2+ D) N2- E) Li2+
4) The electron configuration of the phosphide ion (P3-) is __________.
A) [Ne]3s23p3 B) [Ne]3s23p1 C) [Ne]3s2 D) [Ne]3p2 E) [Ne]3s23p6
5) The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively.
A) 8, 2, and 3 B) 7, 1, and 2 C) 2, 7, and 4 D) 2, 4, and 6 E) 1, 5, and 7
6) Lattice energy is __________.
A) the sum of electron affinities of the components in an ionic solid
B) the energy required to convert a mole of ionic solid into its constituent ions in the gas phase
C) the sum of ionization energies of the components in an ionic solid
D) the energy given off when gaseous ions combine to form one mole of an ionic solid
E) the energy required to produce one mole of an ionic compound from its constituent elements in theirstandard states
7) In which of the molecules below is the carbon-carbon distance the shortest?
A) H3C-CH3
B) H-C”C-H
C) H2ChChCH2
D) H3C-CH2-CH3
E) H2ChCH2
8) Of the atoms below, __________ is the most electronegative.
A) Ca B) Rb C) S D) Cl E) Si
1) Based on the octet rule, magnesium most likely forms a __________ ion.
A) Mg
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9) Electronegativity __________ from left to right within a period and __________ from top to bottom within agroup.
A) increases, increases
B) increases, decreases
C) decreases, increases
D) stays the same, increases
E) increases, stays the same
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10) The Lewis structure of AsH3 shows __________ nonbonding electron pair(s) on As.
A) 0
B) 1
C) 2
D) 3
E) This cannot be determined from the data given.11) The Lewis structure of HCN (H bonded to C) shows that __________ has __________ nonbonding electron
pairs.
A) C, 1 B) N, 2 C) C, 2 D) N, 1 E) H, 1
12) The Lewis structure of N2H2 shows __________.
A) each nitrogen has one nonbinding electron pair
B) each hydrogen has one nonbonding electron pair
C) each nitrogen has two nonbinding electron pairs
D) a nitrogen-nitrogen single bond
E) a nitrogen-nitrogen triple bond
(i) PCl3
(ii) CH2 2
(iii) HCN (iv) C2H4 3
13) In which Lewis structure does the central atom have a non-zero formal charge?
A) (i) B) (ii) C) (iii) D) (v) E) none
14) The formal charge on carbon in the molecule below is __________.
A) 0 B) +1 C) -1 D) +3 E) +2
without expanding octet on the sulfur atom(sulfur is the central atom)?
A) 3 B) 0 C) 4 D) 2 E) 1
15) How many equivalent resonance forms can be drawn for SO2
(v) NH
Consider the following species when answering the questions that follow:
Cl
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16) The central atoms in __________ cannot expand octet.
A) (i) only B) (ii) only C) (i) and (ii) D) (ii) and (iii) E) (iii) and (iv)
2
For the questions that follow, consider the BEST Lewis structures of the following oxyions:
17) The Lewis structure of __________ cannot be drawn without a non-zero formal charge on the central atom.
A) (i) B) (ii) C) (iii) D) (iv) E) (v)
-32-(v) BrO(iv) SO
432-
(iii) SO-(ii) NO
3-(i) NO
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18) Lewis structures of which ions can be drawn with and without expanding the octet on the central atom?
A) (i) and (ii)
B) (iii) only
C) (iv) only
D) (iii) and (iv)
E) (iii), (iv), and (v)
20) The central atom in __________ does not violate the octet rule.
A) KrF2 B) XeF4 C) CF4
D) ICl4- E) SF
4
19) Lewis structures of which ions can be drawn with all formal charges being zero?
A) all
B) (i) and (ii)
C) (ii) only
D) (iii), (iv), and (v)
E) none
21). Refer to Molecular Orbital Theory. What is the molecular orbital configuration of N2? a. [core electrons] (σ2s)2 (σ*2s)2 (π2p)2 (σ2p)2 (σ*2p)2 b. [core electrons] (σ2s)2 (σ*2s)2 (π2p)2 (σ2p)2 (π*2p)2 c. [core electrons] (σ2s)2 (σ*2s)2 (π2p)4 (σ2p)2 d. [core electrons] (σ2s)2 (σ*2s)2 (π2p)4 (σ2p)2 (π*2p)4 e. [core electrons] (σ2s)2 (σ*2s)2 (π2p)4 (π*2p)2
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22) Using the table of average bond energies below, the DH for the reaction is __________ kJ.
A) increases, increases
B) decreases, decreases
C) increases, decreases
D) decreases, increases
E) is unpredictable
23) As the number of covalent bonds between two atoms increases, the distance between the atoms __________ andthe strength of the bond between them __________.
A) +506 B) -506 C) -129 D) +129 E) -931
Bond: C”C C=C H-I C-I C-HD (kJ/mol): 839 614 299 240 413
ChCHI (g)2H-C”C-H (g) + H-I (g) ¬ H
A) trigonal bipyramidal
B) tetrahedral
C) linear
D) octahedral
E) trigonal planar
24) According to VSEPR theory, if there are three electron domains in the valence shell of an atom, they will bearranged in a(n) __________ geometry.
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25) According to VSEPR theory, if there are five electron domains in the valence shell of an atom, they will bearranged in a(n) __________ geometry.
A) tetrahedral
B) linear
C) octahedral
D) trigonal planar
E) trigonal bipyramidal
26) The electron-domain geometry and molecular geometry of iodine trichloride are __________ and __________,respectively.
A) T-shaped, trigonal planar
B) trigonal planar, trigonal planar
C) trigonal bipyramidal, T-shaped
D) tetrahedral, trigonal pyramidal
E) octahedral, trigonal planar
27) The molecular geometry of __________ is square planar.
A) CCl4 B) XeF4 C) ICl3 D) XeF2 E) PH3
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28) The molecular geometry of the H
A) trigonal pyramidal B) octahedral
C) bent D) tetrahedral
E) linear
A) T-shaped
B) trigonal pyramidal
C) tetrahedral
D) bent
E) trigonal planar ion is __________.-3
32) The molecular geometry of the BrO
3
E) All of these will have bond angles of 120e.
3
D) ClF
3
C) PH
3
B) BCl
31) Of the following species, __________ will have bond angles of 120e.
A) NCl
ion is __________.+430) The molecular geometry of the PF
229) The molecular geometry of the CS
ion is __________.O+
3
molecule is __________.
A) tetrahedral B) T-shaped C) bent
D) trigonal planar E) linear
A) trigonal bipyramidal B) tetrahedral
C) trigonal pyramidal D) octahedral
E) trigonal planar
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33) The molecular geometry of the left-most carbon atom in the molecule below is __________.
A) octahedral
B) tetrahedral
C) trigonal planar
D) T-shaped
E) trigonal bipyramidal
34) The bond angles marked a, b, and c in the molecule below are about __________, __________, and __________,respectively.
A) 120e, 120e, 90eB) 90e, 90e, 90eC) 120e, 120e, 109.5eD) 109.5e, 90e, 120eE) 109.5e, 120e, 109.5e
35) The central iodine atom in IF5 has __________ unbonded electron pairs and __________ bonded electron pairsin its valence shell.
A) 1, 4 B) 4, 1 C) 1, 5 D) 0, 5 E) 5, 1
36) Of the molecules below, only __________ is polar.
A) SbF5 B) I2
C) AsH3 D) SF6 E) CH4
37) Of the molecules below, only __________ is nonpolar.
A) IF3 B) BrCl
3 C) PBr3 D) NF E) BF3
38) The molecular geometry of the CHF3 molecule is __________, and the molecule is __________.
3
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A) seesaw, nonpolar B) trigonal pyramidal, polar C) tetrahedral, nonpolar
D) seesaw, polar E) tetrahedral, polar
B) sp C) sp
23dE) sp2 C) sp D) sp3ps)d B3
40) The hybridization of the carbon atom in carbon dioxide is __________.
A) sp
3dE) sp2D) spd
233A) sp
39) The electron-domain geometry of a carbon-centered compound is tetrahedral. The hybridization of the centralcarbon atom is __________.
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41) The hybridization of the central atom in the XeF4 molecule is __________.
A) sp2 B) sp d2 C) sp D) sp d E) sp3
42) The sp3d2 atomic hybrid orbital set accommodates __________ electron domains.
A) 2 B) 3 C) 4 D) 5 E) 6
3 and IF5
are __________ and __________, respectively.
A) sp3, sp3d B) sp3d, sp3 3d, sp3d2 D) sp
3 , sp3d
2 E) sp3d
2, sp3
d
2 hybrid orbitals
C) two sp hybrid orbitals
D) three sp hybrid orbitals
E) three sp hybrid orbitals45) The angles between sp2 orbitals are __________.
A) 109.5e B) 120e C) 180e D) 45e E) 90e
47) There is/are __________ s bond(s) in the molecule below.A) 1 B) 2C) 12 D) 13
E) 18
44) The blending of one s atomic orbital and two p atomic orbitals produces __________.
A) two sp
32
hybrid orbitals
B) three sp
3
43) The hybridizations of iodine in IF
C) sp d2
3 3
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46) A typical triple bond consists of __________.
A) three ionic bonds B) three pi bonds
C) three sigma bonds D) two sigma and one pi bond
E) one sigma and two pi bonds
A) 0 B) 1 C) 2 D) 4 E) 16
48) There is/are __________ p bond(s) in the molecule below.
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49. Which of the following is a correct Lewis structure for oxygen?
A. B.
C.
D.
E.
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50. Which of the following is a correct Lewis structure for C2H6O?
D. Answers a and c are correct. E. Answers a, b, and c are correct.
51. Which Lewis structure is possible for N2O?
C.
E.
D.
B.
A.
C.
B A.
D. N2O E. All of the above are correct structures.
A. NO2 B. NO2
- C. NO
52.. Which of the following is not a correct Lewis structure?
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53. What is the correct Lewis structure of SF4?
A.
B.
C.
D.
E.
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54. Which of the following are correct resonance structures of SO3?
A. (1) and (5) B. (2) and (4) C. (1), (2), and (4) D. (2), (3) and (4) E. (1), (2), (4), and (5)
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electrons assigned to the atom in a Lewis structure.
b.
c.
d.
e.
55. How many lone pairs of electrons are on the sulfur atom in sulfite ion, SO32-?
A. 0 B. 1 C. 2 D. 3 E. 4
covalent bonds. E. the difference between the number of valence electrons in a free atom and the number of
57. What is the formal charge on each atom in dichloromethane, CH2Cl2?A. C = 0, H = 0, Cl = 0 B. C = 0, H = -1, Cl = +1 C. C = 0, H = +1, Cl = -1 D. C = -2, H = +1, Cl = +1 E. C = +4, H = -1, Cl = -1
on any atom in a Lewis structure. C. the difference between the number of valence electrons and the number of protons in any given atom. D. equal to the number of valence electrons in a free atom minus the number of shared in
58. Using formal charges and the octet rule, determine which Lewis structure of OCN- is most stable. a.
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56. Formal charge is A. the absolute value of the charge on a polyatomic anion or cation. B. the difference between the number of lone pairs of electrons and shared pairs of electrons
61. Which of the following species have the same molecular geometry: CO2, H2O, BeCl2, and N2O? A. CO2 and N2O only B. H2O and N2O only C. H2O and BeCl2 only D. CO2 and BeCl2 only E. CO2, BeCl2, and N2O
59. Use VSEPR theory to predict the molecular geometry of BH3. A. triangular planar B. triangular pyramidal C. linear D. tetrahedral E. triangular bipyramidal
60. Use VSEPR theory to predict the molecular geometry of ICl3.A. triangular planar B. triangular pyramidal C. triangular bipyramidal D. t-shaped E. octahedral
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65. How many sigma and pi bonds are present in the following molecule?
A. sp → sp2
62. What are the bond angles in SF6?A. 90º and 180º B. 109.5º C. 120º D. 90º and 120º E. 180º
63. What is the hybridization of the carbon atoms in benzene, C6H6? A. sp B. sp2 C. sp3 D. sp3d E. sp3d2
64. What hybridization change does the carbon atom undergo in the combustion of methane? CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
B. sp2 → sp3 C. sp3 → sp D. sp2 sp E. none
A. 8 sigma bonds and 1 pi bond B. 8 sigma bonds and 2 pi bonds C. 10 sigma bonds and 2 pi bonds D. 11 sigma bonds and 2 pi bonds E. 11 sigma bonds and 1 pi bond
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67. Which of the following compounds is expected to have the strongest ionic bonds? A. RbF B. NaF C. NaI D. CsBr E. CsI
66. Which element is the most electronegative?A. phosphorus B. silicon C. carbon D. nitrogen E. oxygen
68. The central atom in XeF4 is surrounded by A. 3 single bonds, 1 double bond, and no lone pairs of electrons. B. 2 single bonds, 2 double bonds, and no lone pairs of electrons. C. 3 single bonds, 1 double bond, and 1 lone pair of electrons. D. 4 single bonds, no double bonds, and no lone pairs of electrons. E. 4 single bonds, no double bonds, and 2 lone pairs of electrons.
69. Which one of the following molecules has a dipole moment? A. CI4 B. PF5 C. NCl3 D. SO3 E. O2
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70. Label the hybridization at C#1, C#2, C#3, and C#4 in the molecule. C1 C2 C3 C4 a. sp sp sp3 sp3d b. sp sp sp2 sp3 c. sp sp2 sp2 sp2 d. sp2 sp2 sp3 sp3 e. sp3 sp3 sp3 sp3
71. Which molecule is polar?A. BF3 B. H2Se C. N2 D. GeF4 E. CO2
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72. London forces exist A. for all molecules. B. only for molecules with nonpolar bonds. C. only for molecules with polar bonds. D. only for molecules with metallic bonds. E. only for molecules with hydrogen bonding.
73. Which of the following interactions are present between CO2 molecules? I. London forces II. ion-dipole forces III. hydrogen bonding IV. dipole-dipole attractionsA. I only B. II and III C. II only D. III only E. Iand IV
74. How many sigma (σ) bonds and pi (π) bonds are in the following molecule?
A. five σ and two π B. five σ and three π C. five σ and five π D. seven σ and two π E. seven σ and three π
75. Which of the following characteristics apply to PCl3? 1. nonpolar molecule 2. polar bonds 3. trigonal-pyramidal molecular geometry 4. sp2 hybridized A. 1 and 2 B. 2 and 3 C. 3 and 4 D. 1, 2, and 3 E. 1, 2, 3, and 4
A. C1 and C2 B. C1, N, and O C. N and O D. O and C2 E. O only
76. Which of the underlined atoms (C1, C2, N, and O) are sp2 hybridized?
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2- e. Be2
2- a. H2
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79. Use molecular orbital theory to predict which species is paramagnetic.A. N2 B. O2 C. F2 D. Li2 E. H2
78. According to molecular orbital theory, what is the bond order of nitrogen, N2? A. 1 B. 3/2 C. 2 D. 5/2 E. 3
77.According to molecular orbital theory, which of the following species is the most likely to exist?
b. He2 c. Li2 d. Li2
Molecular Orbital Theory The following molecular orbital diagram may be used for the following problems. For oxygen and fluorine, the σ2p orbital should be lower in energy than the π2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.
phases (solid, liquid or gas) of a substance
metals D Atoms of a given atomic number that have a specific number of neutrons E The different
B A pair of substances that differ by H+ C Elements that possess properties intermediate between those of metals and non-
A Different structural forms of an element
80. Which one of the following best defines the word “allotropes”?
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85. Which one of the following species has the least number of electrons?
17 Cl–
20 Ca2+
E 35
18 Ar
D 40
18 Ar
C 40
A 3517 Cl
B 39
D 214Po
E 212Tl
A 218Bi B 216Bi C 216Pb
84. 222Rn is unstable and decays by losing 6 neutrons and 2 protons. What is the final decay product?
83. Which one of the following statements concerning elements in the Periodic Table is correct?
B Elements of Group 16 occur as cations in ionic compounds.C Oxides of elements in Groups 16 and 17 are basic. D The halogens (Group 17) are all gases at room temperature. E The Group 13 elements are all metals.
A Elements of the same group all have the same number of electrons in the outermost occupied electron shell.
C Mg2O3D MgO2 E Mg2O
A MgOB Mg2O2
82. What is the formula of the compound formed between magnesium and oxygen?
81. How many electrons are there in the valence shell of the O2– ion?
10 D 16 E 18
C B 8
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A O2 and O3
B 3517Cl and 3717Cl
C I2(g) and I2(s)
D Mg2+ and Ne E F+ and F–
80Hg2+?
A 1514Si
B 29
15P
D 29
14Si
E 2915P
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86. Which one of the following pairs are isotopes?
87. Which one of the following describes the major intermolecular force in I2(s)?
A covalent bonds B ionic bonds C hydrogen bonds
D dispersion forces E dipole-dipole forces
88. How many protons (p), neutrons (n) and electrons (e) are present in 200
A 200 p 80 n 198 e B 80 p 120 n 78 e C 120 p 80 n 118 e D 80 p 200 n 78 e E 120 p 200 n 118 e
89. Which symbol correctly represents an isotope with 14 protons and 15 neutrons?
14 P
C 30
90. How many bonding and non-bonding electron pairs are found in the BF3 molecule?
A 1 bonding and 3 non-bondingB 2 bonding and 2 non-bonding C 3 bonding and 1 non-bonding
D 3 bonding and 0 non-bonding E 4 bonding and 0 non-bonding
91. Which one of the following pairs of atoms would form a non-polar covalent bond? A C and O B N and O C Cl and Cl D Na and Cl E Ne and Ne
92. Which one of the following species has the same electron configuration as the Al3+ cation?
A F – B Cl– C S2– D O– E Mg+
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A –VI B –II
C 0 D +V
E +VI
96. What is the oxidation number of phosphorus in KH2PO4?
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D. E.
A. B. C.
y y
y y y
z z
z z z
x x
x x x
93. Which one of the following elements has valence electrons in the n = 3 shell?
95. Which one of the following structures represents a 2pz atomic orbital?
A oxygen B carbon dioxideC sodium chloride D magnesium fluorideE helium
94. Which one of the following species contains a polar covalent bond?
A beryllium B oxygenC silicon D neon E hydrogen
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A Since voltage depends on concentrations, using standard conditions makes it easier to compare different electrochemical reactions.
C The direction of a redox reaction can only be determined experimentally.
D Half-cell potentials for half-reactions are determined by combining the relevant half-cell with a standardised half-cell.
99. Which one of the following statements regarding a catalyst is not correct?
100. Which one of the following statements is not correct?
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B We have to measure the cell potential to obtain the difference in potential energy because the potential of half-reactions cannot be measured directly.
D Catalysts do not alter the equilibrium constant for a chemical reaction.
C Catalysts increase the rate of a reaction by altering the mechanism, thereby increasing the activation energy.
B An enzyme is a protein that is a highly efficient catalyst for one or more chemical reactions in a living system.
A An enzyme is a catalyst that only binds certain substrates.
A HCOOH B CH3CN
C CCl4 D SiH4
E CH3OCH3
98. Which one of the following substances will form strong hydrogen bonds?
A hydrogen bonding
B dipole-induced dipole C ion-dipole
D dipole-dipole E ionic
97. Which force is most important in allowing ammonia, NH3, to dissolve in water?
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1) C2) D3) B4) E
5) B
6) B
Answer Key
7) B8) D
9) B
10) B
11) D12) A13) E
14) A
15) D
16) C17) B18) E19) E20) C
41) B42) E
43) C
44) B
45) B
46) E
47) C48) C
21. C
49. A
50. D 51. B
52. C 53. B
54. B 55. B 56. E 57. A
59. A 60. D
58. B
61. E 62. A
63. B 64. C 65. E 66. E
67. B 68. E 69. C
70. B 71. B 72. A 73. A 74. E
81
82
83
84
85
86
87
88
89
A
B
80.A
A
D A
B
D
B
D23) D24) E
22) C
25) E
26) C
27) B
28) A29) E30) B
31) B32) B
33) B34) E35) C36) C37) E38) E39) A40) C
79.B
75. B 76. A 77. C 78. E
90 91 92 93 94 95 96 97 98 99D C A C B B D A A C 100C
AIIMS,CBSE,AIPMT, AFMC,Bio.Tech & PMT, Contact :- 9438559863, Mail at :- [email protected],www.ibiokaare.com,compiled by AKB
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