WorksheetsChemical Bonding
Total questions: 20
Worksheet time: 11mins
In N0–3 ion, the number of bond pairs and lone pairs of electrons on nitrogen atom are,
2, 2
3, 1
1,3
4, 0
Which of the following angle corresponds to sp2 hybridisation?
90°
120°
180°
109°
Polarity in a molecule and hence the dipole moment depends primarily on electronegativity of the constituent atoms and shape of a molecule. Which of the following has the highest dipole moment?
CO2
HI
H2O
(a) SO2
Which of the following is the correct order of dipole moment ?
NH3 < BF3 < NF3 < H2O
BF3 < NF3 < NH3 < H2O
BF3 < NH3 < NF3 < H2O
H2O < NF3 < NH3 < BF3
The species, having bond angles of 120° is
ClF3
NCl3
BCl3
PH3
The electronegativity difference between N and F is greater than that between N and H yet the dipole moment of NH3 (1.5 D) is larger than that of NF3 (0.2 D). This is because
In NH3 the atomic dipole and bond dipole are in the opposite directions whereas in NF3 these are in the same direction
In NH3 as well as in NF3 the atomic dipole and bond dipole are in the same direction
In NH3 the atomic dipole and bond dipole are in the same direction whereas in NF3 these are in opposite directions
In NH3 as well as in NF3 the atomic dipole and bond dipole are in opposite directions.
H2O is dipolar, whereas BeF2 is not. It is because
The electronegativity of F is greater than that of O
H2O involves hydrogen bonding whereas BeF2 is a discrete molecule
H2O is linear and BeF2 is angular
H2O is angular and BeF2 is linear
Predict the correct order among the following :
Bond pair - bond pair > lone pair - bond pair > lone pair - lone pair
Lone pair - bond pair > bond pair - bond pair > lone pair - lone pair
Lone pair - lone pair > lone pair - bond pair > bond pair - bond pair
Lone pair - lone pair > bond pair - bond pair > lone pair - bond pair
Which of the following species contains three bond pairs and one lone pair around the central atom?
H2O
BF3
NH3
CO2
Which of the following is not a correct statement?
Multiple bonds are always shorter than corresponding single bonds
The electron-deficient molecules can act as Lewis acids.
The canonical structures have no real existence.
Every AB5 molecule does in fact have square pyramid structure
Which of the following molecules has trigonal planar geometry?
BF3
NH3
PCl3
IF3
Which one of the following molecules contains no pi bond?
SO2
NO2
CO2
H2O
Which statement is not correct?
A sigma bond is weaker than a pi bond.
A sigma bond is stronger than a pi bond.
A double bond is stronger than a single bond.
A double bond is shorter than a single bond.
Linear combination of two hybridized orbitals belonging to two atoms and each having one electron leads to the formation of,
Sigma bond
Double bond
Co-ordinate covalent bond
Pi bond.
According to VSEPR theory the geometry of a covalent molecules depends upon
The number of bond pairs of electrons
The number of lone pairs of electrons
The number of electron pairs present in the outer shell of the central atom
All the above
A molecule has two lone pairs and two bond pairs around the central atom. The molecule shape is expected to be
V-shaped
triangular
Linear
Tetrahedral
The nature of hybridisation in the ammonia molecule is
sp2
sp2d
sp
sp3
A sp3 -hybrid orbital contains
25% s-character
75% s-character
50% s-character
25% p-character
The types of hybridisation of the five carbon atoms from left to right in the molecule CH3 — CH = C = CH — CH3 are
sp3 , sp2 , sp2 , sp2 , sp3
sp3 , sp, sp2 , sp2 , sp3
sp3 , sp2 , sp, sp2 , sp3
sp3 , sp2 , sp2 , sp, sp3
Which one of the following is not correct in respect of hybridization of orbitals?
The orbitals present in the valence shell only are hybridized
The orbitals undergoing hybridization have almost equal energy
Promotion of electron is not essential condition for hybridization
Pure atomic orbitals are more effective in forming stable bonds than hybrid orbitals
