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NEET Chemistry MCQ
Molecular Bonding Mcq Neet Chemistry
Quiz 2
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Q.1
Number of electrons that are paired in oxygen molecule is .. [ Kerala CEE 2000]
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a) 16
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b) 8
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c)14
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d)12
Explanation
O2 have 2 unpaired and 14 paired electronsAnswer: (c)
Q.2
the correct order of increasing C-O bond length of CO, CO32-, CO2 is ... [ IIT 1999]
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a)CO32- < CO2 < CO
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b) CO2 < CO32- < CO
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c)CO < CO32- < CO2
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d)CO < CO2 < CO32-
Explanation
Bond length is determined by number of bonded electrons (the bond-order) Higher the bond-order, shorter will be the bond-length. OR Smaller the bond-order longer will bond length. (i) Number of bonds in CO Total number of bonds between C and O=3 Number of resonating structures=1 B.O.=Total number of bonds / number of resonating structures=3/1=3 (ii) Number of Bonds CO2 Number of bonds=4 resonating structures=2 B.O=4/2=2(iii) Number of bonds CO32-, Three are three resonating structures Number of bonds=4 B.O=4/3=1.33Answer: (d)
Q.3
Sulphuric acid provides a simple example of ..
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a) co-ordinate bonds
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b) covalent compound
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c) covalent ion
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d) non-covalent ion
Explanation
Here, hydrogen, sulphur and oxygen are non-metals. It is not form by transfer of electrons, from atom to another, by sharing of electrons between unifing atoms. They bond formed by sharing of e- is known as covalent bond. Coordinate bond are formed by donation of a pair of e- to the central atom atom. In sulphuric acid, sulphur form only covalent bond. There is no coordination bond in sulphure. Answer: (b)
Q.4
The nodel plane in the π-bond of ethene is located in ... [ IIT screening 2002]
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a) the molecular plane
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b) a plane parallel to molecular plane
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c)a plane perpendicular to the molecular plane which bisects the carbon-carbon sigma bond at right angles
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d)a plane perpendicular to the molecular pane which contains the carbon carbon σ bond
Explanation
Nodel pane do not have any electron density, and molecular plane do not have electron density Answer:(a)
Q.5
The value of electronegativity atom A and B are 1.20 and 4.0 respectively. the percentage of ionic character of A-B bond is [ DCE 2000]
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a) 50%
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b) 72.24%
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c)55.3%
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d)43.0%
Explanation
By Hanny and Smith equation % ionic character=16( xA - xB) +.3 (xA - xB)2Where xA and xB are electronegativities of atom A and B respectively.% ionic character=16( 4-1.2) + 3.5(4-1.2)2 % ionic character=44.8 +27.44=72.24Answer: (b)
Q.6
Which of the following substance has the east ionic character? [ Kerala MEE 2000]
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a)FeCl2
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b) ZnCl2
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c)MgCl2
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d)HgCl2>2
Explanation
ZnCl2 Transition metal halide Atomic size of Zn is highest and less electro positive, thus have more covalent characterAnswer: (b)
Q.7
In OF2, number of bond pairs and lone pairs of electrons are respectively [ DPMT 2002]
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a) 2, 6
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b) 2, 8
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c) 2, 10
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d) 2, 9
Explanation
Two bonded and 8 lone pairs Answer: (b)
Q.8
Chemical bond implies [ KCET 2002]
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a) repulsion
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b) attraction
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c)attraction and repulsion balanced at a particular distance
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d)attraction and repulsion
Explanation
Chemical bond is an attraction between atoms that allows the formation of chemical substances. The bond will be formed where attraction forces due to opposite charges were balanced by repulsion forces due to similar charge. Answer:(c)
Q.9
Which of the following arrangements of molecules's is correct on the order of their dipole moment
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a) BF3 > NF3 > NH3
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b) NF3 > BF3 >NH3
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c)NH3 >BF3 > NF3
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d)NH3 > NF3 > BF3
Explanation
Dipole moment of BF3 is zero because of trigonal symmetry, While NH3 have higher dipole moment than NF3 magnetic dipolemoment of NH3 = 1.46D magnetic dipolemoment of NF3 = 10.24D Answer: (d)
Q.10
The hybridization of atomic orbitals of nitrogen in NO2+, NO3- and NH4+ are .. [ iit screening test 2000)
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a)sp2, sp3 and sp2 respectively
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b) sp, sp2, and sp3 respectively
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c)sp2, sp and sp3 respectively
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d)sp2, sp3, and sp respectively
Explanation
NO2+ umber of valance electrons=5+6+6-1=16 Now 16 ÷ 8=2(Q1) + 0(R1) total of Q1 + R1=2 sp hybridization By using same procedure find Hybridization of NO3- as sp2 Hybridization of NH4+ is sp3 Thus option b' is correctAnswer: (b)
Q.11
The boiling point of p-nitrobenzene is higher than that of o-nitrobenzene because .. [ CBSE PMT 1994]
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a) NO2 group at p-position behaves in a different way from that at o-position
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b) intramolecular hydrogen bonding exists in p-nitophenol
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c) there is intermolecular hydrogen bonding in p-nitrophenol
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d) p-nitrophenol has higher molecular weight than o-nitrophenol
Explanation
in o-nitrophenol there is intra molecular bonding while in p-nitrobenznene there is intermolecular bonding hence higher boiling point Answer: (c)
Q.12
The correct order of decreasing polarisabile ions is
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a) Cl-, Br-, I-, F-
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b) F-, I-, Br-, Cl-
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c)F-, Cl-, Br-, I-
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d)I-, Br-, Cl-, F-
Explanation
According to Fajan's rule. Greater anion size has more covalent charcter. Polarisability: measure of covalent character in case of anion Size order: I- > Br- > Cl- > F- Charge is same in all, higher the size more the polarisabile ion Answer:(d)
Q.13
In which of the following hydrogen bonding is not possible .. [ AMU 1997]
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a) NH3, NH3
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b) NH3, NCH4
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c)H2O, CH3OCH3
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d)CH3OH, CH3OCH3
Explanation
H bonding is possible only if molecule contains N, O, F , Now CH3 do not contains any of the listed atomAnswer: (b)
Q.14
The following molecule is not linear in shape .. [ CPMT 1996]
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a)HgCl2
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b) Hg2Cl2
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c)CO2
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d)SnCl2
Explanation
SnCl2 has 18 valence electrons Now 18 ÷ 8=2(Q1) + 2(R1 and 2 ÷2=1(Q2 ) + 0(R2) Thus Q1 + Q2 + R2=2 +1 + 0=3 sp2 hybridization. thus angular shape Answer: (d)
Q.15
Which of the following has least covalent P-H bond? [ CPMT 1996]
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a) PH3
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b) P2H6
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c) P2H5
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d) PH6+
Explanation
PH6+, P-H bond will be ionic due to electron attracting tendency of P. Thus P-H bond PH6+ is least covalent. Due to +ve charge on P of PH6+ it attracts electrons of the P-H bonds towards it self. As a result its has some ionic character. thus P-H bond in PH6+ is least covalent Answer: (d)
Q.16
The sulphate of a metal has the formula M2(SO3)The formula of its phosphate will be ... [ MPPMT 1995]
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a) M(HPO4)2
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b) M3(PO4)2
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c)M2(PO4)3
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d)MPO4
Explanation
Valancy of M is +3 and PO4 is trivalent , and thus option 'd' is correct Answer:(d)
Q.17
Bond order is a concept in the molecular orbital theory. It depends on the number of electrons in the bonding and antibonding orbitals. Which of the following statements is true about it? [ AIIMS 1994]
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a) Bond order cannot be negative
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b) Bond order have always an integral value
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c)Bond ordercan assumes any value, positive or negative integral or fractional, including zero
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d)Bond orderis non -zero quantity
Explanation
Bond order is half of difference between Bonding electrons and antibonding electrons. thus bond order can not be negative because Bonding electrons are always more than antibonding electronsAnswer: (a)
Q.18
For two ionic solids, CaO and KI. Identify the wrong statement among the following .. [ CBSE PMT 1997]
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a)Lattice energy CaO is much higher than that of KI
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b) KI is soluble in benzene
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c)CaO has higher melting point
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d)KI has lower melting point
Explanation
CaO has higher melting point due to higher charges Due to lowe lattice enthalpy of KI compared to CaO benzene in non polar solvent while KI is ionic which is soluble only in polar solventsAnswer: (b)
Q.19
The structure and hybridization of Si(CH3)4 is ... [ CBSE PMT 1996]
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a) bent, sp
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b) trigonal, sp2
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c)octahedral, sp3d
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d)tetrahedral, sp3
Explanation
Answer:(d)
Q.20
Which of the following species has lowest ionization potential
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a) O
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b) O2
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c) O2+
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d) O2-
Explanation
The electronic configuration of the O2- ion containing 18e- can be written as O2- have three electrons in antibonding orbitals and hence have highest energy and least ionization potential. Answer: (d)
Q.21
Molecule having dipole moment is ... [ AFMC 1994]
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a) 2,2-dimethylpropane
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b) trans-2-pentene
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c)neopentane
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d)2,2,3,3-tetranethylbutane
Explanation
Because of +I effect of they group is more than CH3 group, the two dipole moment do not cancel our and hence trans-2pentene has a resultant finite dipolemoment Answer:(b)
Q.22
Bonding in Ferric chloride is ... [ Pb CET 1997]
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a) Covalent
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b) Ionic
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c)CO-ordinate
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d)None of the above
Explanation
Ferric chloride, FeCl3 , have three +ve charge on Fe ion ion thus more in covalent character according to Fajan rule which states more the charge on cation more covalent natureAnswer: (a)
Q.23
Polarization power of cation increases when .... [ AMU 1997]
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a)Charge on the cation increases
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b) size of the cation increases
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c)charge on the cation decreases
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d)has no relation to its size or charge
Explanation
Polarization power of cation is ability of cation of distort an anion. (Charge/Radius) ∝ polarization. Increase in charge of cation and decrease in radius will increase in polarization power Answer: (a)
Q.24
Which of the following ion does not have bond order of 2.5? [ Raj.PMT 1998]
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a) O2-
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b) O2+
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c) N2+
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d) N2-
Explanation
Number of electrons
B.O.
10
1
11
1.5
12
2
13
2.5
14
3
15
2.5
16
2
17
1.5
18
1
Bond order of O2- is 1.5 While remaining ion bond order 2.5 Bond order ∝ stability B.O. = ½(Nb-Na) N2- = electrons 7+7+1 =15 ⇒ B.O. = 2.5 N2+ = electrons 7+7-1 =13 ⇒ B.O. = 2.5 O2+ = electrons 8+8-1 =15 ⇒ B.O. = 2.5 Answer: (a)
Q.25
2 and O2 are converted into monocations, N2+ and O2+ respectively. Which of the following 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+ paramagnetism decreases
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d)N2+ becomes diamagnetic
Explanation
Number of electrons in N2+=7+7-1=13 which is odd thus paramagnetic, option 'd' is wrong Answer:(d)
Q.26
Which of the following is the correct electron dot structure of N2O molecule .... [MP PET 1996] (I) Formal charge helps us which structure is most correct. Where choosing the best structure, based on following rules (a) Smaller formal charge are more favourable. (b) More electronegative atoms should have negative formal charge. (II) In option (b) Formal charge of centre Nitrogen is +1 and formal charge of oxygen is -1 Following the eule that more electro-negative atome should have negative formal charge. Oxygen is more electronegative atom and has negative charge.
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a)
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b)
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c)
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d)
Explanation
(I) Formal charge helps us which structure is most correct. Where choosing the best structure, based on following rules (a) Smaller formal charge are more favourable. (b) More electronegative atoms should have negative formal charge. (II) In option (b) Formal charge of centre Nitrogen is +1 and formal charge of oxygen is -1 Following the eule that more electro-negative atome should have negative formal charge. Oxygen is more electronegative atom and has negative charge. Only in option(b) octet of N and O are completeAnswer: (b)
Q.27
Which of the following hydrogen halide have lowest boiling point? [ AIIMS 1994]
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a)HF
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b) HCl
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c)HBr
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d)HI
Explanation
As the size of halide increases van der waal force increases hence increasing in boiling point. Accordingly HF should have lowest boiling point but HF shows hydrogen bond. Now there is no hydrogen bond in HCl thus HCl have lower boiling point than HF.Answer: (b)
Q.28
Average distance of single covalent bond of carbon and oxygen is ... [ Pb CET 1998]
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a) 1.34 A°
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b) 1.54 A°
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c) 1.77 A°
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d) 1.91 A°
Explanation
Answer: (a)
Q.29
On the basis of ionic potential, the tendency to form covalent bond in a group ... [ BHU 1994]
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a) Increases
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b) Decreases
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c)remains unchanged
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d)shows erratic change
Explanation
More the ionic potential more is the tendency to form a covalent bonds. In group electronegativity decreases hence ionic potential Therefore tendency to form covalent character decreases Answer:(b)
Q.30
Which of the following molecular orbitals has two nodal planes ... [ Haryana CEET 1996]
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a) σ2s
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b) π2py
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c)π*2py
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d)σ*2px
Explanation
π*2py have two nodel plane one passing through intermolecular axis and one passing through y axisAnswer: (c)
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