Test: Chemical Bonding- 3
30 Questions MCQ Test Inorganic Chemistry | Test: Chemical Bonding- 3
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In B the central atoms are S and I+ respectively, having 6 e- each and the others are from G-VII. Hence, they will have the same lone pair repulsion.
Hence B is correct.
Among the following pairs, those in which both the species have the similar shape:
(I) N3-, XeF2
(II) [ClF2]+, [ICl2]+
(III) [ICl4]+, [PtCl4]2-
(IV) XeO3, SO3
According to VSEPR theory, the molecule/ ion having ideal tetrahedral shape is:
Which among are super valent species:
(I) NO
(II) NO2
(III) PCl5
(IV) SF6
Electronegativity decreases down the group, the electron density also decreases and consequently the repulsive interactions between the electron pairs also decrease thereby decreasing the bond angle H-M-H
The compound pair which shows correct order of angle:
(I) NH3 > PH3
(II) H2S < H2O
(III) NO2+ > NO2
(IV) NO2+ > NO2–
(V) NO2– > NO2+
a) NH3 ammonia has bond angle = 107.8 deg.
Bond angle of Ph3 = 93 deg.
NH3 > PH3 (True)
b) The bond angle of H2O is 105 deg
The bond angle of H2S is 90 deg
H2S < H2O (True)
c) bond angle of NO2+ is 180 deg
bond angle of NO2 is 134.4 deg
NO2+ > NO2 (True)
d) bond angle of NO2+ is 180 deg
bond angle of NO2- is 115 deg
NO2+ > NO2– (True)
The bond energies of H2, F2 and Cl2 decreases in the following order:
Arrange the following molecules in order of increasing bond polarity :
(I) H2O
(II) NH3
(III) PH3
(IV) H2S
Correct Answer :- c
Explanation : The bond polarity is directly proportional to the electronegativity of the atom.
As we move down the group, radius of elements increases and electronegativity decreases so bond angle decreases.
So, bond polarity will be : H2O < NH3< H2S < PH3
The element NaCl and Kr crystallizes in a cubic structure. While NaCl is a solid at room temperature, Kr is a gas? The reason for this is:
Which of the following molecules will have a permanent dipole moment?
Paramagnetism is due to the presence of at least one unpaired electron in the molecule. Though NO2 is paramagnetic, its dimer, N2O4, is diamagnetic. The two unpaired electrons in the two NO2 units get paired while forming the dimer, and so N2O4 is diamagnetic with even number of electrons.
Which is/are paramagnetic among:
(I) S2 gas
(II) O2
(III) NO2+
(IV) CaH2
Nitrogen forms N2 but phosphorus is converted into P4 from P2. The reason for this is:
Due to larger atomic size P is unable to form pi bond and so it is tetra-atomic in which each P atom is linked with 3 other P atoms by 3 sigma bonds.
But, due to smaller atomic size N forms 1 sigma and 2 pi bonds i.e. triple bonds with other N atom and exists as diatomic molecules. Hence the bonding is responsible for that.
Phosporous form P4 because in P2 pπ-pπ bond is weaker.
Boron trifluoride is planar and the bond angle is 120 degrees. This can be predicted from VSEPR theory. There are three bonding pairs of electrons and no lone pairs on the central atom
The correct order of bond angles θ1, θ2 and θ3 in the following is
PH5 and NI3 doesnt exist.
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