E) Mg 2-
2) Based on the octet rule, phosphorus most likely forms a __________ ion.
A) P5B) 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]3s 23p3
B) [Ne]3s 23p1
C) [Ne]3s 2
D) [Ne]3p2
E) [Ne]3s 23p6
w.i
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1) Based on the octet rule, magnesium most likely forms a __________ ion.
B) Mg 6+
C) Mg 2+
D) Mg 6A) Mg -
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
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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 their
standard states
kaa
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
A) Ca
B) Rb
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8) Of the atoms below, __________ is the most electronegative.
C) S
D) Cl
E) Si
9) Electronegativity __________ from left to right within a period and __________ from top to bottom within a
group.
A) increases, increases
B) increases, decreases
C) decreases, increases
E) increases, stays the same
om
D) stays the same, increases
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10) The Lewis structure of AsH3 shows __________ nonbonding electron pair(s) on As.
A) 0
C) 2
D) 3
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B) 1
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.
B) N, 2
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A) C, 1
C) C, 2
D) N, 1
E) H, 1
12) The Lewis structure of N H shows __________.
2 2
A) each nitrogen has one nonbinding electron pair
B) each hydrogen has one nonbonding electron pair
C) each nitrogen has two nonbinding electron pairs
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D) a nitrogen-nitrogen single bond
E) a nitrogen-nitrogen triple bond
Consider the following species when answering the questions that follow:
(i) PCl
3
(ii) CH Cl
2 2
(iii) HCN
(iv) C2H4
(v) NH3
13) In which Lewis structure does the central atom have a non-zero formal charge?
A) (i)
B) (ii)
C) (iii)
kaa
D) (v)
E) none
D) +3
E) +2
14) The formal charge on carbon in the molecule below is __________.
A) 0
B) +1
C) -1
15) How many equivalent resonance forms can be drawn for SO without expanding octet on the sulfur atom
2
(sulfur is the central atom)?
B) 0
C) 4
D) 2
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A) 3
E) 1
For the questions that follow, consider the BEST Lewis structures of the following oxyions:
322(v) BrO
(iv) SO
(iii) SO3
(i) NO
(ii) NO
4
3
2
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)
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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)
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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
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C) (iv) only
D) (iii) and (iv)
E) (iii), (iv), and (v)
19) Lewis structures of which ions can be drawn with all formal charges being zero?
A) all
B) (i) and (ii)
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C) (ii) only
D) (iii), (iv), and (v)
E) none
20) The central atom in __________ does not violate the octet rule.
A) KrF
2
C) CF4
D) ICl 4
E) SF
4
Refer to Molecular Orbital Theory. What is the molecular orbital configuration of N2? a.
2
2
2
2
2
[core electrons] (σ2s) (σ*2s) (π2p) (σ2p) (σ*2p)
2
2
2
2
b. [core electrons] (σ2s) (σ*2s) (π2p) (σ2p) (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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21).
B) XeF
4
22) Using the table of average bond energies below, the DH for the reaction is __________ kJ.
Bond:
D (kJ/mol):
C”C
839
C=C
614
A) +506
B) -506
kaa
H-C”C-H (g) + H-I (g) ¬ H ChCHI (g)
2
H-I
299
C-I
240
C-H
413
C) -129
D) +129
E) -931
23) As the number of covalent bonds between two atoms increases, the distance between the atoms __________ and
the strength of the bond between them __________.
A) increases, increases
C) increases, decreases
D) decreases, increases
E) is unpredictable
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B) decreases, decreases
24) According to VSEPR theory, if there are three electron domains in the valence shell of an atom, they will be
arranged in a(n) __________ geometry.
A) trigonal bipyramidal
C) linear
D) octahedral
E) trigonal planar
om
B) tetrahedral
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25) According to VSEPR theory, if there are five electron domains in the valence shell of an atom, they will be
arranged in a(n) __________ geometry.
A) tetrahedral
B) linear
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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
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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.
B) XeF4
C) ICl3
+
28) The molecular geometry of the H O ion is __________.
3
A) trigonal pyramidal
B) octahedral
C) bent
E) linear
D) XeF2
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A) CCl4
E) PH3
D) tetrahedral
29) The molecular geometry of the CS2 molecule is __________.
B) T-shaped
D) trigonal planar
E) linear
C) bent
kaa
A) tetrahedral
30) The molecular geometry of the PF4+ ion is __________.
A) trigonal bipyramidal
B) tetrahedral
C) trigonal pyramidal
D) octahedral
A) NCl3
B) BCl3
C) PH3
D) ClF3
E) All of these will have bond angles of 120e.
32) The molecular geometry of the BrO
B) trigonal pyramidal
C) tetrahedral
D) bent
E) trigonal planar
3- ion is __________.
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A) T-shaped
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E) trigonal planar
31) Of the following species, __________ will have bond angles of 120e .
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33) The molecular geometry of the left-most carbon atom in the molecule below is __________.
A) octahedral
B) tetrahedral
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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.
B) 90e, 90e, 90e
C) 120e , 120e , 109.5e
D) 109.5e, 90e, 120e
E) 109.5e , 120e , 109.5e
bio
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A) 120e , 120e , 90 e
35) The central iodine atom in IF has __________ unbonded electron pairs and __________ bonded electron pairs
5
in its valence shell.
B) 4, 1
C) 1, 5
kaa
A) 1, 4
D) 0, 5
E) 5, 1
D) SF
6
E) CH4
D) NF
3
E) BF3
36) Of the molecules below, only __________ is polar.
A) SbF
5
B) I
C) AsH
2
3
37) Of the molecules below, only __________ is nonpolar.
A) IF
3
B) BrCl
3
C) PBr
3
D) seesaw, polar
E) tetrahedral, polar
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38) The molecular geometry of the CHF molecule is __________, and the molecule is __________.
3
A) seesaw, nonpolar
B) trigonal pyramidal, polar
C) tetrahedral, nonpolar
39) The electron-domain geometry of a carbon-centered compound is tetrahedral. The hybridization of the central
carbon atom is __________.
E) sp3d
B) sp
C) sp3d2
A) sp3
D) sp2
om
40) The hybridization of the carbon atom in carbon dioxide is __________.
A) sp3d
B) sp2
C) sp
D) sp3
E) sp3d2
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E) sp3 d
42) The sp3d2 atomic hybrid orbital set accommodates __________ electron domains.
A) 2
B) 3
C) 4
D) 5
E) 6
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41) The hybridization of the central atom in the XeF4 molecule is __________.
B) sp3d2
C) sp
D) sp3d
A) sp2
43) The hybridizations of iodine in IF and IF are __________ and __________, respectively.
3
5
3
A) sp3, sp3d
D) sp d2, sp3 2
C) sp3d, sp d2
B) sp3d, sp
d
3
3
44) The blending of one s atomic orbital and two p atomic orbitals produces __________.
A) two sp3 hybrid orbitals
2
E) sp d , sp3
3
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B) three sp2 hybrid orbitals
C) two sp 2 hybrid orbitals
D) three sp3hybrid orbitals
E) three sp hybrid orbitals
45) The angles between sp2 orbitals are __________.
A) 109.5e
B) 120e
C) 180e
D) 45e
E) 90e
A) three ionic bonds
C) three sigma bonds
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46) A typical triple bond consists of __________.
B) three pi bonds
D) two sigma and one pi bond
E) one sigma and two pi bonds
kaa
47) There is/are __________ s bond(s) in the molecule below.
A) 1
B) 2
C) 12
D) 13
E) 18
48) There is/are __________ p bond(s) in the molecule below.
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B) 1
C) 2
om
A) 0
D) 4
E) 16
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49. Which of the following is a correct Lewis structure for oxygen?
A.
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D.
C.
B.
E.
50. Which of the following is a correct Lewis structure for C2H6O?
B
w.i
A.
D. Answers a and c are correct.
C.
E. Answers a, b, and c are correct.
Which Lewis structure is possible for N2O?
A.
C.
D.
E.
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kaa
B.
52..
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51.
Which of the following is not a correct Lewis structure?
NO2
NO2NO
N2O
All of the above are correct structures.
om
A.
B.
C.
D.
E.
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53.
What is the correct Lewis structure of SF4?
A.
E.
kaa
54.
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D.
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C.
ww
B.
Which of the following are correct resonance structures of SO3?
(1) and (5)
(2) and (4)
(1), (2), and (4)
(2), (3) and (4)
(1), (2), (4), and (5)
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A.
B.
C.
D.
E.
om
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55.
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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
56.
b.
d.
e.
kaa
c.
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w.i
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
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
covalent bonds.
E. the difference between the number of valence electrons in a free atom and the number of
electrons assigned to the atom in a Lewis structure.
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
58. Using formal charges and the octet rule, determine which Lewis structure of OCN- is most stable.
a.
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
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
re.c
59.
om
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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
3
C. sp
D. sp3d
3 2
E. sp d
64.
What hybridization change does the carbon atom undergo in the combustion of methane?
ww
62.
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
65.
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A. sp → sp2
B. sp2 → sp3
C. sp3 → sp
D. sp2 sp
E. none
How many sigma and pi bonds are present in the following molecule?
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A. 8 sigma bonds and 1 pi bond
C. 10 sigma bonds and 2 pi bonds
E. 11 sigma bonds and 1 pi bond
B. 8 sigma bonds and 2 pi bonds
D. 11 sigma bonds and 2 pi bonds
Which element is the most
electronegative?
A. phosphorus
B. silicon
C. carbon
D. nitrogen
E. oxygen
67.
Which of the following compounds is expected to have the strongest ionic bonds?
A. RbF
B. NaF
C. NaI
D. CsBr
E. CsI
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.
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69.
kaa
66.
om
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
71.
sp
sp
sp
sp2
sp3
B. II and III
C. II only
D. III only
E. Iand IV
How many sigma (σ) bonds and pi (π) bonds are in the following molecule?
C. five σ and five π
kaa
B. five σ and three π
E. seven σ and three π
Which of the following characteristics apply to PCl3?
1. nonpolar molecule
2. polar bonds
3. trigonal-pyramidal molecular geometry
4. sp2 hybridized
B. 2 and 3
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A. 1 and 2
76.
B. only for molecules with nonpolar bonds.
D. only for molecules with metallic bonds.
Which of the following interactions are present between CO2 molecules?
I.
London forces
II. ion-dipole forces
III.
hydrogen bonding IV. dipole-dipole attractions
A. five σ and two π
D. seven σ and two π
75 .
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London forces exist
A. for all molecules.
C. only for molecules with polar bonds.
E. only for molecules with hydrogen bonding.
A. I only
74.
C4
sp3d
sp3
sp2
sp3
sp3
w.i
73.
C3
sp3
sp2
sp2
sp3
sp3
Which molecule is
polar?
A. BF3
B. H2Se
C. N2
D. GeF4
E. CO2
72.
C2
sp
sp
sp2
sp2
sp3
ww
a.
b.
c.
d.
e.
C. 3 and 4
D. 1, 2, and 3 E. 1, 2, 3, and 4
Which of the underlined atoms (C1, C2, N, and O) are sp2 hybridized?
C1 and C2
C1, N, and O
N and O
O and C2
O only
om
A.
B.
C.
D.
E.
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Molecular Orbital Theory
bio
w.i
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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.
77.According to molecular orbital theory, which of the following species is the most likely to exist?
78.
79.
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
Use molecular orbital theory to predict which species is
paramagnetic.
A . N2
B. O2
C. F2
D. Li2
E. H2
Which one of the following best defines the word “allotropes”?
A
B
Different structural forms of an element
+
A pair of substances that differ by H
re.c
80.
H22He2
Li2
Li22Be2
kaa
a.
b.
c.
d.
e.
om
C
Elements that possess properties intermediate between those of metals and nonmetals
D
Atoms of a given atomic number that have a specific number of neutrons E The different
phases (solid, liquid or gas) of a substance
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81.
A
2
B
8
C
10
D
16
E
18
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82.
2–
How many electrons are there in the valence shell of the O ion?
What is the formula of the compound formed between magnesium and oxygen?
A MgO
B Mg2O2
83.
222
A
Elements of the same group all have the same number of electrons in the outermost occupied electron shell.
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.
Rn is unstable and decays by losing 6 neutrons and 2 protons. What is the final decay product?
A
B
C
218
D
214
Po
E
212
Tl
Bi
Bi
216
Pb
216
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85.
Which one of the following statements concerning elements in the Periodic Table is correct?
kaa
84.
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C Mg2O3
D MgO2
E Mg2O
Which one of the following species has the least number of electrons?
35
17
Cl
B
39
18
Ar
C
40
D
40
18
20
E
35
17
Ar
Ca2+
Cl–
om
A
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86.
B
35
17
C
I2(g) and I2(s)
D
Mg2+ and Ne
E
F+ and F–
Cl
A
covalent bonds
B ionic bonds
D
dispersion forces
E dipole-dipole forces
C hydrogen bonds
How many protons (p), neutrons (n) and electrons (e) are present in
A
B
200 p
80 p
C
120 p
D
80 p
200 n
E
120 p
200 n
80 n
120 n
198 e
78 e
80 n
118 e
200
80
Hg2+?
78 e
118 e
Which symbol correctly represents an isotope with 14 protons and 15 neutrons?
Si
15
14
B
29
14
P
C
30
15
P
D
29
Si
29
15
P
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kaa
A
E
91.
37
17
Which one of the following describes the major intermolecular force in I2(s)?
14
90.
Cl and
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89.
O2 and O3
w.i
88.
A
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87.
Which one of the following pairs are isotopes?
How many bonding and non-bonding electron pairs are found in the BF3 molecule?
A 1 bonding and 3 non-bonding
B 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
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
om
D
Na and Cl
E Ne and Ne
3+
92. Which one of the following species has the same electron configuration as the Al
cation?
A
B
C
D
E
F–
Cl–
S2–
O–
Mg+
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ww
93.
Which one of the following elements has valence electrons in the n = 3 shell?
A beryllium
B oxygen
C silicon
D neon
E hydrogen
Which one of the following species contains a polar covalent bond?
A oxygen
B carbon dioxide
C sodium chloride
D magnesium fluoride
E helium
bio
95.
w.i
94.
Which one of the following structures represents a 2pz atomic orbital?
z
A.
z
B.
kaa
x
x
z
E.
z
y
x
What is the oxidation number of phosphorus in KH2PO4?
A
–VI
B
–II
C
0
D
+V
E
+VI
om
96.
x
re.c
y
x
y
y
y
D.
z
C.
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hydrogen bonding
B
dipole-induced dipole
C
ion-dipole
D
dipole-dipole
E
ionic
Which one of the following substances will form strong hydrogen bonds?
A
HCOOH
B
CH3CN
C
CCl4
D
SiH4
E
CH3OCH3
kaa
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99.
A
w.i
98.
Which force is most important in allowing ammonia, NH3, to dissolve in water?
ww
97.
Which one of the following statements regarding a catalyst is not correct?
An enzyme is a catalyst that only binds certain substrates.
B
An enzyme is a protein that is a highly efficient catalyst for one or more
chemical reactions in a living system.
C
Catalysts increase the rate of a reaction by altering the mechanism, thereby
increasing the activation energy.
D
Catalysts do not alter the equilibrium constant for a chemical reaction.
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A
100. Which one of the following statements is not correct?
Since voltage depends on concentrations, using standard conditions makes it
easier to compare different electrochemical reactions.
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.
The direction of a redox reaction can only be determined experimentally.
C
D
om
A
Half-cell potentials for half-reactions are determined by combining the relevant
half-cell with a standardised half-cell.
AIIMS,CBSE,AIPMT, AFMC,Bio.Tech & PMT, Contact :- 9438559863, Mail at :- [email protected],www.ibiokaare.com,compiled by AKB
Answer Key
3) B
4) E
5) B
41) B
42) E
43) C
44) B
47) C
9) B
48) C
10) B
49. A
50. D
51. B
52. C
53. B
54. B
55. B
56. E
57. A
58. B
59. A
60. D
61. E
62. A
63. B
64. C
65. E
66. E
67. B
68. E
69. C
13) E
14) A
15) D
16) C
17) B
18) E
19) E
20) C
21. C
22) C
23) D
24) E
25) E
26) C
27) B
28) A
29) E
30) B
31) B
32) B
94
B
95
B
96
D
97
A
98
A
100
C
80.A
81 B
82 A
83 A
84 D
85 A
86 B
87 D
88 B
89 D
om
33) B
34) E
35) C
36) C
37) E
38) E
39) A
40) C
93
C
re.c
46) E
92
A
kaa
7) B
8) D
91
C
bio
45) B
90
D
w.i
6) B
11) D
12) A
70. B
71. B
72. A
73. A
74. E
75. B
76. A
77. C
78. E
79.B
ww
1) C
2) D
AIIMS,CBSE,AIPMT, AFMC,Bio.Tech & PMT, Contact :- 9438559863, Mail at :- [email protected],www.ibiokaare.com,compiled by AKB
99
C