Class: XI
Subject:
√ Chemistry
Topic: Chemical Bonding and Molecular Structure
No. of Questions: 27
Q1. Which of the following bonds is the most stable?
1s – 1s
2p – 2p
2s – 2s
1s – 2p
ns
A.
B.
C.
D.
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Right Answer Explanation: A
The more closer are the shells to the nucleus, more will be the overlapping and the stability.
Q2. Which of the following bonds are present in dry ice?
IT
Ionic bonds
Covalent bonds
Hydrogen bonds
None of the above
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A.
B.
C.
D.
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Right Answer Explanation: B
Dry ice is solid CO2, which has C – O covalent bond.
Q3. Which structure will the compounds formed by sp3d hydbridisation have in the absence of a
lone pair?
A.
B.
C.
D.
Planar
Pyramidal
Angular
Trigonal bi pyramidal
Right Answer Explanation: D
In the absence of a lone pair, sp3d hybridsation gives trigonal bi pyramidal geometry.
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Q4. Which of the following is least ionic?
A.
B.
C.
D.
AgCl
KCl
BaCl2
NaCl
Right Answer Explanation: A
Alkali and alkaline earth metal salts are strongly ionic. AgCl is not an alkali or alkaline earth
metal salt.
Therefore, it is least ionic.
Ionic bond
Ion-dipole
Dipole-dipole
London dispersive
IT
Right Answer Explanation: A
Ionic bonding is strong among these all
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A.
B.
C.
D.
ns
Q5. Which of the following forces between atoms or ions or molecules is the strongest?
1
2
4
3
as
A.
B.
C.
D.
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Q6. How many electrons are needed by Phosphorus to attain the configuration of nearest noble gas?
Right Answer Explanation: D
Phosphorus has electronic configuration as 1s2 2s2 2p6 3s2 3p3.It needs three electrons to attain
stable noble gas configuration of argon.
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Q7. _______ is an electron deficient molecule.
A.
B.
C.
D.
CCl4
PCl5
BF3
SF6
ns
Right Answer Explanation: C
The compounds in which central atom has less than 8 electrons in their valence shell are
electron deficient compounds.
IT
ia
Boron (central atom) has 6 electrons in valence shell, 3 from boron and one each from three
fluorine atoms.
Boron in BF3 has less than 8 electrons.
It is electron deficient molecule and is correct answer.
A.
B.
C.
D.
4
1
2
3
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Q8. How many total electron pairs are present in valence shell of oxygen in water molecule?
as
Right Answer Explanation: A
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Q9. Which of the following geometrical configurations corresponds to dsp2 hybridization?
A.
B.
C.
D.
Tetrahedral
Square planar
Trigonal bi pyramidal
Octahedral
Right Answer Explanation: B
Square planar geometry corresponds to dsp2 hybridization.
Q10. How many electrons take part in the formation of bond in N2?
ia
ns
A. 6
B. 4
C. 2
D. 10
Right Answer Explanation: A
IT
Six electrons take part in the formation of N2 molecule.
2 and 2
1 and 2
3 and 1
4 and 0
as
A.
B.
C.
D.
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Q11. The numbers of bond pairs and lone pairs in ammonia molecule are _______, respectively.
Right Answer Explanation: C
Ammonia or azane is a compound of nitrogen and hydrogen with the formula NH3. It is a
colourless gas with a characteristic pungent odor. The numbers of bond pairs and lone pairs in
ammonia molecule are 3 and 1, respectively.
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Q12. Which substance would you expect to have the highest melting point?
A.
B.
C.
D.
NaF
NaCl
NaBr
Nal
Right Answer Explanation: A
NaF is ionic as the high electronegativity difference of sodium and fluorine creates a strong
ionic bond between them. That's why it has highest melting point.
Q13. Which of the following contains both covalent and ionic bonds?
CCl4
CaCl2
NH4Cl
SiCl4
ns
A.
B.
C.
D.
as
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IT
ia
Right Answer Explanation: C
N forms covalent bonds with hydrogen and ionic bonds with chlorine.
Q14. Which of the following has the greatest covalent character?
A.
B.
C.
D.
LiCl
NaCl
KCl
RbCl
Right Answer Explanation: A
Smaller the size of cation, higher will be the covalent character of molecule. As the ionic size
increases down the group, the correct order of covalent character will be LiCl>NaCl>KCl>RbCl.
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Q15. The correct order of bond angles in H2O, NH3, CH4 and CO2 is
A.
B.
C.
D.
H2O > NH3 > CO2 > CH4
CH4 > CO2 > NH3 > H2O
CO2 > CH4 > H2O > NH3
CO2 > CH4 > NH3 > H2O
Right Answer Explanation: D
Bond angle decreases with increase in the number of lone pairs on the central atoms.
Q16. Which one of the following is a correct set with respect to molecule, hybridisation and shape?
ns
as
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Right Answer Explanation: (iv)
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(i)
(ii)
(iii)
(iv)
BeCl2, sp, linear
BeCl2, sp2, trigonal planar
BCl3, sp2, trigonal planar
BCl3, sp3, tetrahedral
A and B
B and C
C and D
A and C
IT
A.
B.
C.
D.
Q17. Which of the following compounds/ions will have the maximum bond angle?
A.
B.
C.
D.
SO2
CH4
H2S
H3O+
Right Answer Explanation: A
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ia
ns
By looking at the following structure, it is clear that sulphur dioxide will have the maximum
bond angle.
P2H2
H2P
PH3
PH
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A.
B.
C.
D.
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Q18. Phosphorus (atomic number 15) and hydrogen elements combine to form a compound whose
formula is
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Right Answer Explanation: C
Phosphorus has three unpaired electrons which will combine with three hydrogen atoms to
form PH3 molecule.
Q19. Which of the following statements about electrovalent substances is false?
A.
B.
C.
D.
Electrovalent substances are made up of ions held together by strong electrostatic forces.
Electrovalent substances have high melting and boiling points.
Electrovalent compounds can conduct electricity in solid state.
None of these
Right Answer Explanation: C
Electrovalent or ionic compounds can conduct electricity only in the molten state. They will not
conduct electricity in the solid state.
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Q20. Which of the following is not a characteristic of covalent compound?
A.
B.
C.
D.
They are good conductors of electricity.
They are soluble in non polar solvents.
They have low melting and boiling point.
None of these
Right Answer Explanation: A
Electrons are not free in covalent compounds so conduction of electricity is not a property of
covalent compounds.
Q21. Write the favourable factors for the formation of ionic bond.
ns
Ans:
IT
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An lonic bond is formed by the transfer of one or more electrons from one atom to another.
Hence, the formation of ionic bonds depends upon the ease with which neutral atoms can lose
or gain electrons. Bond formation also depends upon the lattice energy of the compound
formed.
(i)
Low ionization enthalpy of metal atom.
(ii)
High electron gain enthalpy (∆egH) of a non-metal atom.
(iii)
High lattice energy of the compound formed.
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Ans:
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Q22. Although geometries of NH3 and H2O molecules are distorted tetrahedral, bond angle in water
is less than that of ammonia. Discuss.
The molecular geometry of NH3 and H2O can be shown as:
The central atom (N) in NH3 has one lone pair and there are three bond pairs. In H2O, there
are two lone pairs and two bond pairs.
The two lone pairs present in the oxygen atom of H2O molecule repel the two bond pairs.
This repulsion is stronger than the repulsion between then lone pair and the three bond
pairs on the nitrogen atom.
Since the repulsions on the bond pairs in H2O molecule are greater than that in NH3, the
bond angel in water is less than of ammonia.
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23. Write the significance / applications of dipole moment.
Ans: In heteronuclear molecules, polarization arises due to a difference in the electronegativities of
the constituents of atoms. As a result, one end of the molecule acquires a positive charge while the
other end becomes negative. Hence, a molecule is said to possess a dipole. The product of the
magnitude of the charge and the distance between the centres of positive-negative charges is called
the dipole moment ( ) of the molecule. It is a vector quantity and is represented by an arrow with
its tail at the positive centre and head pointing towards a negative centre.
Diploe moment ( ) = charge (Q) x distance of separation (r) the SI unit of a dipole moment is ‘esu’.
1 esu = 3.335 x10-30cm
IT
ia
ns
Dipole moment is the measure of the polarity of a bond. It is used to differentiate between polar and
non- polar bonds since all non – polar molecules (e.g. H2, O2) have zero dipole moments. It is also
helpful in calculating the percentage ionic character of a molecule.
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Q24. Arrange the bonds in order of increasing ionic character in the molecules: LiF, K2O, N2, SO2 and
CIF3.
as
Ans: The ionic character in a molecule is dependent upon the electronegativity difference
between the constituting atoms. The greater the difference, the greater will be the ionic character of
the molecule. On this basis, the order of increasing ionic character in the given molecules is
N2 < SO2 < ClF3 < K2O < LiF.
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Q25. DIstnguish between a sigma and a pi bond.
Ans: The following are the differences between sigma and pi-bonds:
Pi (n)Bond
It is formed by the lateral overlap of orbitals.
These bonds are formed by the overlap of p-p
orbitals only.
It is weak bond.
The electron cloud is not symmetrical.
There are two electron clouds lying above and
below the plane of the atomic nuclei.
Rotation is restricted in case of pi- bonds.
ns
Sigma ( ) Bond
(a) It is formed by the end to end overlap of
orbitals.
(b) The orbitals involved in the overlapping
are s-s, s-p, or p-p.
(c) It is a strong bond.
(d) The electron cloud is symmetrical about
the line joining the two nuclei.
(e) It consists of one electron cloud, which is
symmetrical about the internuclear axis.
(f) Free rotation about bonds is possible.
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Q26. Explain the formation of H2 molecule on the basis of valence bond theory.
IT
Write the important conditions required for the linear combination of atomic orbitals to
form molecular orbitals.
Ans: The given conditions should be satisfied by atomic orbitals to form molecular orbitals:
(iii)
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(ii)
The combining atomic orbitals must have the same or nearly the same energy. This
means that in a homonuclear molecule, the 1s-atomic orbital of an atom can
combine with the 1s-atomic orbital of another atom, and not with the 2s-orbital.
The combining atomic orbitals must have proper orientation to ensure that the
overlap is maximum.
The extent of overlapping should be large.
as
(i)
Q27. Write the significance of a plus and a minus sign shown in representing the orbitals.
Ans: Molecular orbitals are represented by wave functions. A puls sign in anorbital indicates
a postive wave function while a minus sign in an orbital represents a negative wave
function.
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