Chemical Bonding Online Test

Element X is strongly electropositive and element Y is strongly electronegative. Both are univalent. The compound formed would be
X+Y-
X-X+
X-Y
X(Y
Which of the following is soluble in water
CS2
C2H2OH
CCI4
CHCI3
The correct order of the O-O bond length in O2, H2O2 and O3 is:
H2O2 > O3 > O2
O2 > O3 > H2O2
O2 > H2O2 > O3
O3 > H2O2 > O2
PbCI4 exists but PbBr4 and PBI4 do not because of:
Br- and I- ions are bigger in size
chlorine is a gas
Br2 and I2 are more electronegative
inability of bromine and iodine to oxidize Pb2+ to Pb4+
Which is/are correct statements?
A solute will dissolve in water if hydration energy is greater than lattice energy
If the anion is large compared to the cation, the lattice energy wil remain almost constant
Solubility of II A hydroxide is in order. Be(OH)2 < Mg(OH)2 < Ca(OH)2 < Sr(OH)2
none is correct
Above three are correct
In which molecule is the van der Waals force likely to be most important in determining m.p. and b.p.?
IC1
Br2
H2S
CO
In the following case (s),, hybridization of the underlined atom is affected:
PC15 (solid) dissociates into PC1+4 and PC1-6
LiH reacts with AIH3 forming Lia1H4
NH3 is protonated
H3PO2 is heated forming PH3 and H3PO3
PC15 (solid) dissociates into PC1+4 and PC1-6, LiH reacts with AIH3 forming Lia1H4
The bond between two identical non-metal atoms has a pair of electrons:
Unequally shared between the two
Transferred fully from one atom to another
With identical spins
Equally shared between them
The types of bonds present in CuSO4.5H2O are only
Electrovalent and covalent
Electrovalent and coordinate covalent
Electrovalent and covalent and coordinate covalent
Covalent and coordinate covalent
If a molecule MX2 has zero dipole moment, the sigma bonding orbits used by M (atomic number<21)are
pure P
sp hybrid
sp2 hybrid
sp3 hybrid
The number and type of bonds between two carbon atoms in CaC2 are:
One sigma (() and one Pi (() bonds
One sigma (() and two Pi (() bonds
One sigma (() and one and a half Pi (() bonds
One sigma (() bond.
The cyanide ion, CN- and N2 are isoelectronic. But in contrast to CN-, N2 is chemically inert, because of
Low bond energy
Absence of bond polarity
Unsymmetrical electron distribution
Presence of more number of electrons in bonding orbitals
The molecule which has zero dipole moment is:
CH2CI2
BF3
NF3
CIO2
Specify the coordination geometry around and hybridisation of N and b atoms in a 1 : 1 complex of BF3 and NH3
N : tetrahedral in a 1 : 1 complex of BF3 and NH3
N : pyramidal, sp3, B : pyramidal, sp3
N : pyramidal, sp3, B : planar, sp2
N : pyramidal, sp3, B : tetrahedral, sp3
The correct order of hybridization of the central atom in the following species NH3, [PtCI4]2-, PCI5 and BCI3 is
Dsp2, dsp3, sp2 and sp3
Sp3, dsp3, dsp3, sp2
Dsp2, sp2, sp3, dsp3
Dsp2, sp3, sp2, dsp3
The common features among the species CN-, CO and NO+ are
Bond order three and isoelectronic
Bond order three and weak field ligands
Bond order two and (-acceptors
Isoelectronic and weak field ligands
Read the following statement and explanation and answer as per the options given below:
If both assertion and reason are correct and reason is the correct explanation of the assertion
If both assertion and reason are correct, but reason is not the correct explanation of the assertion
If assertion is correct but reason is incorrect.
If assertion is incorrect but reason is correct
The critical temperature of water is higher than that of O2 because the H2O molecule has
Fewer electrons than O2
Two covalent bonds
V-shape
Dipole moment.
Which contains both polar and non-polar bonds?
NH4CI
HCN
H2O2
CH4
The structure of  is ____.
Planar
Non-planar
Spherical
Linear
Which one is false in the following statements?
The geometry and the type of hybrid orbital present about the central atom in BF3 is
Linear, sp
Trigonal planar, sp2
Tetrahedral, sp3
Pyramidal, sp3
Among the fooling, the paramagnetic compound is
Na2O2
O3
N2O
KO2
Witch species has the maximum number of lone pair of electrons on the central atom?
|CIO3
XeF4
SF4
[I3]
Carbon atoms in diamond are bonded to each other in a configuration ____.
Tetrahedral
Planar
Linear
Octahedral
Among the following compounds which is planar in shape?
Methane
Acetylene
Benzene
Isobutene
As compared to pure atomic orbitals, hybrid orbitals have ____.
Low energy
Same energy
High energy
None of the above
Which of the following formula does not correctly represent the bonding capacity of the atom involved?
The valency of carbon is four. On what principle it can be explained in a better way?
Resonance
Hybridization
Electron transfer
None of the above
In which of the following pairs, molecules/ions have similar shape?
CO2 and H2O
BF3 and (CH3)3C(
CCI4 and PtCI4
NH3 and BF3
Polarizing action of Cd2+ on anions is stronger than that of Ca2+ because:
the charges of the ions are same
their radii are same (Ca2+ = 0.104 nm; Cd2+ = 0.099 nm)
the Ca2+ ion has a noble-gas electron configuration, and the Cd2+ ion, an 18-electron configuration of its outer shell
all are correct
Azide ion (N-3) exhibits an N-N bond order of 2 and may be represented by resonance structures I, II and III given below: - + - .. + + .. :N=N=N:( 2-:N-N(N:(:N ( N-N:2- .. .. .. I II III Select correct statements:
Structures I and II make greater contributions than III
Structures II and III make greater contributions than I
Structures I and III make greater contributions than II
All three structures make equal contributions
The correct order of increasing C-O bond length of CO, CO2-3, CO2 is:
CO2-3 < CO2 < CO
CO2 < CO2-3 < CO
CO < CO2-3 , CO2
CO < CO2 < CO2-3
Select correct statement(s) about C4-3 ion:
It reacts with H2O forming C3H6
It reacts with H2O forming C3H4
It has two sigma and two pi bonds
It has three sigma and one pi bonds
It reacts with H2O forming C3H4, It has two sigma and two pi bonds
Metallic bonding is explained by:
band model
electron-sea model
both (a) and (b)
none of these
Energy gaps between the highest filled band and the lowest empty bands in elements A, B, C and D are 0, 70, 530 and 110 kJ mol-1. Thus:
element A is metal
element C is insulator
element B and D can be semiconductors
all are correct conclusions about elements A, B, C and D
Solutions of alkali metals in liquid ammonia at –330C conduct electricity without chemical reaction at the electrodes. Hence, conductivity should:
increase as temperature is lowered
decrease as temperature is lowered
remain constant on changing the temperature
there is always interaction of alkali metal with liquid ammonia
The hybridization scheme for the central atom includes a d-orbital contribution in:
I-3
PC13
NO-3
H2Se
A substance in which large energy gap separates the valence and conduction band is a/an:
metal
metalloid
semi-conductor
insulator
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DIPANKAR DAS
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