1. Dry ice is
a) solid \[NH_{3}\]
b) solid \[SO_{2}\]
c) solid \[CO_{2}\]
d) solid \[N_{2}\]
Explanation: Dry ice is solid \[CO_{2}\]
2. Quartz is extensively used as piezoelectric material, it
contains __________ .
a) Pb
b) Si
c) Ti
d) Sn
Explanation: Quartz is extensively used as piezoelectric material, it contains "Si"
3. Which of the following is most electronegative?
a) Pb
b) Si
c) C
d) Sn
Explanation: Electronegativity decreases down the group
4. The most stable +2 oxidation state is exhibited by
a) Fe
b) Sn
c) Pb
d) Si
Explanation: Inert pair effect increases down the group. Hence for Pb2+, O.S. is most stable.
5. The electronic configuration of four different elements is
given below. Identify the group 14 element among these
a) \[\left[He\right] 2s^{1}\]
b) \[\left[Ne\right] 3s^{2}\]
c) \[\left[Ne\right] 3s^{2}3p^{2}\]
d) \[\left[Ne\right] 3s^{2}3p^{5}\]
Explanation: Valence shell electronic configuration of group 14 elements is ns2p2
6. The catenation tendency of C,Si and Ge is in the order Ge
< Si < C.The bond energies (in kJ mol-1 ) of C-C , Si-Si and Ge-
Ge bonds, respectively are
a) 167,180,348
b) 180,167,348
c) 348,167,180
d) 348,180,167
Explanation: The more the bond energy, the more is the catenation
7. Ge(II)compounds are powerful reducing agents
whereas Pb(IV)compounds are strong oxidants .It is because
a) Pb is more electropositive than Ge
b) ionization potential of lead is less than that of Ge
c) ionic radii of Pb2+ and Pb4+ are larger than those of \[Ge^{2+}\]
and \[Ge^{4+}\]
d) of more pronounced inert pair effect in lead than
in Ge
Explanation: Ge(II) tends to acquire Ge (IV) state by loss of electrons. Hence it is reducing in nature. Pb (IV) tends to acquire Pb (II) O.S. by gain of electrons. Hence it is oxidising in nature. This is due to inert pair effect.
8. Which among CH4, SiH4, GeH4, SnH4 is most volatile?
a) \[CH_{4}\]
b) \[SiH_{4}\]
c) \[GeH_{4}\]
d) \[SnH_{4}\]
Explanation: The lower the mol. wt. The more is the volatile character
9. Which of the following halides is the most stable?
a) \[CF_{4}\]
b) \[Cl_{4}\]
c) \[CBr_{4}\]
d) \[CCl_{4}\]
Explanation: Since bond energy of C-F >C-Cl > C-Br > C-I Hence CF4 is most stable
10. Which of the following conceivable structures for CCl4 will
have a zero dipole moment ?
a) Square planar
b) Square pyramid (carbon at apex)
c) Irregular tetrahedron
d) None of these
Explanation: CCl4 is tetrahedral in nature.