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NEET Chemistry MCQ
Molecular Bonding Mcq Neet Chemistry
Quiz 1
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Q.1
Identify a molecule which does not exist. .... [NEET 2020]
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a) C2
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b) O2
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c) He2
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d) Li2
Explanation
(i) He2 Z for He = 2 He2 = 4e- E.C = σ1s2 σ*1s2 Bond order = ½ (Nb - Na = ½ (2-2) = 0 (ii) Li2 Z=3 valence e- = 3×2 = 6e- E.C = σ1s2 σ*1s2 σ2s2 Bond order = ½ (4-2) =2 (Li - Li) (iii) C2 Z = 6 Valence e- = 6 × 2 = 16e- E.C. = σ1s2 σ*1s2 σ2s2 σ*2s2 π2px2=π2py2 Bond order = ½ [8-4] = 2 (iv) O2 Z=8 Valance electrons = 8 ×2 = 16e- E.C. = σ1s2 σ*1s2 σ2s2 σ*2s2 π2px2=π2py2π*2px1=π*2py1 Bond order = ½[10-6]=2 Answer: (c)
Q.2
Which of the following diatomic molecular species has only π bonds according to Molecular Orbital Theory? [NEET 2019]
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a) O2
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b) N2
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c)C2
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d)Be2
Explanation
Answer:(c)
Q.3
Which one of the following elements is unable to form MF63- ion ? [NEET 2018]
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a) B
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b) Al
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c) Ga
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d) In
Explanation
Answer: (a)
Q.4
Consider the following species : CN+, CN-, NO and CN Which one of these will have the highest bond order ? [NEET 2018]
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a) CN+
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b) CN–
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c)NO
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d)CN
Explanation
a) CN+ = 12e- electron ≤ 14 E.C. = σ1s2 σ*1s2 σ2s2 σ*2s2 π2px2=π2py2=2pz BO = ½ [8-4] = 2 b) CN- = 14e- B.O = ½ [10-4] = 3 c) NO = 15e- electron > 14e- E.C. = σ1s2 σ*1s2 σ2s2 σ*2s2 σ2pz2 π2px2=π2py2 π*2px1=π*2py σ*2pz B.O = ½[10-5] = 2.5 d) CN = 13e- B.O. = ½(9-4) = 2.5 Answer: (d)
Q.5
Which of the following molecules represents the order of hybridisation sp2, sp2, sp, sp from left to right atoms ? [NEET 2018]
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a) CH2 = CH – CH = CH2
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b) CH2 = CH – C ≡ CH
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c) HC ≡ C – C≡ CH
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d) CH3 – CH = CH – CH3
Explanation
Answer: (b)
Q.6
Which of the following set of molecules will have zero dipole moment? [NEET 2020]
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a) Nitrogen trifluoride, beryllium difluoride, water, 1,3-dichlorobenzene
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b) Boron trifluoride, beryllium difluoride, carbon dioxide, 1,4-dichlorobenzene
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c) Ammonia, beryllium difluoride, water, 1,4-dichlorobenzene
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d) Boron trifluoride, hydrogen fluoride, carbon dioxide, 1,3-dichlorobenzene
Explanation
µ = dipole moment Answer:(b)
Q.7
Identify the incorrect statement related to PCl5 from the following: [NEET 2019]
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a) Three equatorial P–Cl bonds make an angle of 120° with each other
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b) Two axial P–Cl bonds make an angle of 180&dge with each other
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c) Axial P–Cl bonds are longer than equatorial P–Cl bonds
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d) PCl5 molecule is non-reactive
Explanation
PCl5 Hybridiztion = ½ [5+5] = 5 ⇒ sp3 Shape is Trigonal bipyramidal equitoral = 120° , axial = 180° In PCl5 , 2-axial P-Cl bond are weak and they make PCl5 highly reactive. PCl5 → PCl2 + Cl2 Answer: (d)
Q.8
The shape of gaseous SnCl2 is (kerala MEE 2000]
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a)Tetra hedral
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b) Linear
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c)Angular
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d)T-shaped
Explanation
Sn in SnCl2 has sp2 hybridized and has has angular shapeAnswer: (c)
Q.9
Sodium chloride is an ionic compound where as hydrogen chloride is mainly covalent because.. [ KCET 2002]
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a) sodium is less reactive
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b) Hydrogen is non-metal
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c) Hydrogen chloride is a gas
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d) Electronegativity difference in the case of Hydrogen and chloride is less than 2.1
Explanation
electronegativity
types of bond
0.0 to 0.2
non-polar covalent
0.3 to 1.4
polar covalent
(I) Type of bpnding between atom is dependent on combining atom's electronegativity and its electronegativity difference. (II) In NaCl, Na is a metal with electronegativity 1.0 and Cl is non metal with electronegativity 3.0 The difference is > 15 ∴ NaCl is ionic compound. In HCl, H is non-metal with electronegativity 2.1. The electronegativity difference is 0.9 ∴ HCl is polar covaleant. (III) To conclude (a) Bond betwwen metal and non-metal are usually ionic (b) Bond between two non-metal are polar, covalent or non-polar covalent. Answer: (b)
Q.10
The electronic configuration of metal M is 1s22s22p63sthe formula of its oxide will be ... [ MP PMT 1998]
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a) MO
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b) M2O
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c)M2O3
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d)MO2
Explanation
Metal have only one electron in its valance shell hence formula for metal oxide is M2O Answer:(b)
Q.11
Which of the following molecule is linear? [ MP PMT 2000]
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a) SO2
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b) NO2 +
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c)NO2 -
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d)SCl2
Explanation
NO2 +have sp hybridization, hence linearAnswer: (b)
Q.12
Among H2O, H2, H2Se and H2 Te, the one with highest boiling point is
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a)H2O because of hydrogen bonding
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b) H2Te because of higher molecular weight
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c)H2S because of hydrogen bonding
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d)H2Se because of lower molecular weight
Explanation
Oxygen is more electronagtive thus have strong hydrogen bondAnswer: (a)
Q.13
Which of the following molecular species has unpaired electron(s)? [ IIT screening 2002]
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a) N2
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b) F2
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c)O2-
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d)O22-
Explanation
O2- have one unpaired electron in π*2p orbital Answer:(c)
Q.14
The bond length in LiF will be ... [CPMT 2000]
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a) Less than that of NaF
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b) equal to that of KF
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c)more than that of KF
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d)equal to that of NaF
Explanation
1) Bond length is approximately sum of covalent radii of two atoms 2) Size of Na+, K+ > Li+ As we go down the group size increase 3) Bond length of LiF < NaF < KF Answer: (a)
Q.15
The compound MX4 is tetrahedral. the number of ∠XMX formed in such compound is .. [ DEC 2000]
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a)Three
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b) Four
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c)Five
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d)Six
Explanation
Since MX4 is tetra hedral number of ∠XMX are six Six angles are as follows ∠AMB ∠AMC ∠AMD ∠BMC ∠BMD ∠CMD Answer: (d)
Q.16
Which of the following has zero dipole moment? [ MP PMT 2002]
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a) ClF
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b) PCl3
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c) SiF4
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d) CFCl3
Explanation
ClF: difference in electronegative µ ≠ 0 PCl : polar structure µ ≠ 0 CFCl3 &rAaa non symmetric arrangement µ ≠ 0 Due to symmetric arrangement SiF4 has zero dipole moment Answer: (c)
Q.17
A lone pair of electron in an atom implies [ KCET 2002]
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a) a pair of valence electrons
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b) a pair of electrons
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c)a pair of electrons involved in bonding
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d)a pair of valence electron not involved in bonding
Explanation
Answer:(d)
Q.18
Consider the following states. The common features of the molecules BF3, CO and NO are that I. All are Lewis acids II. all are gaseous in nature III. all contain unpaired electrons IV. all do not conform to the octet rule [SCRAE 2000]
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a) I and II
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b) III and IV
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c)I and III
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d)II and IV
Explanation
BF3
Lewis acid
Gaseous
Un-Paired electrons
Do not confirm Octate rule
CO
Lewis acid
Gaseous
Un-Paired electrons
Do not confirm Octate rule
NO
Lewis base
Gaseous
Paired electrons
Do not confirm Octate rule
(I) Lewis acid : accepts electron pair and hence vacant orbital. (II) Lewis base: donates electron pair and will have lone pair electrons. All are gaseous molecules and do not confirm to the octet rule BF3 and CO are Lewis acid but NO is Lewis base. BF3 and CO contain unpaired e’s but NO contains pair electrons. Answer: (d)
Q.19
Number of possible resonance structure of CO3-2 are ... [ MP PMT 2000]
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a)2
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b) 3
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c)6
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d)9
Explanation
Answer: (b)
Q.20
Fluorine molecule is formed by [ Kerals MEE 2001]
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a) the axial p-p orbital overlap
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b) the sideways p-p orbital overlap
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c) the s-s orbital overlap
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d) the overlap of s-p orbitals
Explanation
Answer: (a)
Q.21
In NO3- ion, number of bond pairs and lone pairs of electrons on nitrogen atom are .. [ CBSE PMT 2002]
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a) 2, 2
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b) 3, 1
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c)1, 3
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d)4, 0
Explanation
Thus four bonded pairs and no loan pairs Answer:(d)
Q.22
A molecule has seven bond pairs around the central atom, the shape associated with the molecule is
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a) heptagonal
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b) octahedral
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c) pentagonal pyramidal
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d) pentagonal bipyramidal
Explanation
Answer: (d)
Q.23
Two ice cubes are pressed over each other until they unit to form one block. Which one of the following forces dominates for holding then together? [ kerala CEE 2000]
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a)Dipole -dipole interaction
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b) van der Waal's force
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c)Hydrogen bond formation
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d)Covalent attraction
Explanation
Answer: (c)
Q.24
Which of the following has pπ - dπ bonding? [ CBSE PMT 2002]
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a) NO3-
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b) SO32-
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c) BO33-
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d) CO32-
Explanation
Answer: (b)
Q.25
Covalent compounds have low melting point because [ KCET 2002]
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a) covalent molecules have definite shape
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b) covalent bond is weaker than ionic bond
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c)covalent bond is less exothermic
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d)covalent molecules are held by weak van der Waals force of attraction
Explanation
Covalent compound molecules are held together by van der Waals force of attraction. Thus energy require required to break bond is less and have low melting point Answer:(d)
Q.26
N2 and O2 are converted into monoanions N2- , O2-respectively. Which of the following statement is wrong? .. [ CBSE PMT 1997]
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a) In N2-, N - N bond weakens
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b) In O2- bond order increases
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c) In O2- bond order decreases
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d) In ON2- become paramagnetic
Explanation
Bond order of O2-=1.5 while for O2 it is 2.0 Answer: (b)
Q.27
Which of the following molecule will have unequal bond lengths? [ Kerala MEE 2000]
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a) NF3
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b) BF3
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c)PF5
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d)SF4
Explanation
PF5 have triogonal bipyramidal geometry. Here all P-F bonds are not equal. Axial P-F bond is longer than equatorial P-F bond Hybridization: mixing of 2 orbital to form new hybrid orbital. NF3 = ½[5+3]= 4 ⇒ sp3 1 lone pair, 3 bond pair, bond length equal BF3 = ½[3+3] = 3 ⇒ sp2 ⇒ Trigonal planer structure, Bond length equal PF5 = ½[5+5] = 5 ⇒ sp3d ⇒ TBP Bond are not equal. Axial P-F bond is longer than equitorial P-F bond. Bond length not equal. SF6 = ½[6+6] = 6 ⇒ sp3d2. Bond length equal. Answer: (c)
Q.28
The type of forces between molecules of C6H6 are ... [ BHU 2000]
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a)Dipole -dipole interaction
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b) Dispersible forces
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c)H-bonding
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d)van der Waals force
Explanation
C6H6 is non polar molecules, thus have momentary dipole-in-induced dipole. It is dispersive forceAnswer: (b)
Q.29
Number of sigma bonds in P4O10 is ..[ AIEEE2002]
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a) 6
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b) 7
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c) 17
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d) 16
Explanation
Each P atom forms 4 sigma bonds Total sigma bonds=16 Answer: (d)
Q.30
Molecule having non-zero dipole moment is ... [ kerala CEE 2000]
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a) H2O2
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b) CH4
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c)BF4-
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d)B2H2
Explanation
µ = 0 ( non-polar), µ ≠ 0 (polar) Except H2O2 all have symmetric structure and hence zero dipole moment. H2O2 is has a non planar structure and hence has a finite dipole moment Answer:(c)
0 h : 0 m : 1 s
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