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Published on: 27/08/2019
Chemical Bonding and Molecular Structure
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Questions + Answers key
Take MCQ Chemistry Test
1.
Arrange the following, according to increasing covalent nature.
NaCl, MgCl2, AICl3
2.
What is meant by bond pairs of electrons?
3.
Use molecular orbital theory to explain why the Be2 molecule does not exist.
4.
Can we have a diatomic molecule with its ground state molecular orbitals full with electrons? Give a reason for your answer.
5.
What type of atomic orbitals can overlap to form molecular orbitals?
6.
A molecule or ion is stable if: ______.
Nb = Na
Nb < Na
Na < Nb
Na - Nb =+ve
7.
In SO2 molecule, S atom is: ______.
sp3 hybridized
sp hybridized
sp2 hybridized
d sp2 hybridized
8.
The axial overlap between the two orbitals leads to the formation of a: ______.
sigma bond
pi bond
multiple bond
none of these
9.
The species CO, CN- and N2 are ______.
isoelectronic
having coordinated bond
having polar bond
having low bond energies
10.
A co-ordinate bond is formed by ______.
sharing of electrons contributed by both the atoms
complete transfer of electrons
sharing of electrons contributed by one atom only
none of these
1.
NaCl < MgCl2 < AlCl3
2.
The electron pairs involved in the bond formation are known as bond pairs or shared pairs.
3.
Electronic configuration of Be2 molecule (4 + 4 = 8)
σ1s2,σ1s2,σ1s2,σ1s2
Bond order=1/2[Nb−Na]=1/2(4−4)=0
Since, bond order in zero, so Be2 does not exist.
4.
No, because bond order becomes zero, e.g in case of He2, Be2, Ne2 etc. Note that in H2 ,σ1s molecular orbitals is full but σ1s is empty.
5.
Atomic orbitals with comparable energies and proper orientation overlap to form molecular orbitals
6.
(c)
Na < Nb
7.
(c)
sp2 hybridized
8.
(a)
sigma bond
9.
(a)
isoelectronic
10.
(c)
sharing of electrons contributed by one atom only
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