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NCERT solutions Chemistry Textbook for Class 11 Part 1 chapter 4 Chemical Bonding and Molecular Structure

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Chapter 4 - Chemical Bonding and Molecular Structure

Pages 129 - 131

Explain the Formation of a Chemical Bond.

Q 1 | Page 129 | view solution

Write Lewis dot symbols for atoms of the following elements: Mg, Na, B, O, N, Br.

Q 2 | Page 129 | view solution

Write Lewis symbols for the following atoms and ions: S and S2–

Q 3.1 | Page 129 | view solution

Write Lewis symbols for the following atoms and ions: Al and Al3+

Q 3.2 | Page 129 | view solution

Write Lewis symbols for the following atoms and ions H and H

Q 3.3 | Page 129 | view solution

Draw the Lewis structures for the following molecules and ions: H2S

Q 4.1 | Page 129 | view solution

Draw the Lewis structures for the given molecules and ions: SiCl4

Q 4.2 | Page 129 | view solution

Draw the Lewis structures for the given molecules and ions BeF2

Q 4.3 | Page 129 | view solution

Draw the Lewis structures for the given molecules and ions `CO_3^(2-)`

Q 4.4 | Page 129 | view solution

Draw the Lewis structures for the following molecules and ions HCOOH

Q 4.5 | Page 129 | view solution

Define octet rule

Q 5.1 | Page 129 | view solution

Write its significance and limitations octet rule

Q 5.2 | Page 129 | view solution

Write the favourable factors for the formation of the ionic bond.

Q 6 | Page 129 | view solution

Discuss the shape of the following molecules using the VSEPR model:

BeCl2, BCl3, SiCl4, AsF5, H2S, PH3

Q 7 | Page 130 | view solution

Although geometries of NH3 and H2O molecules are distorted tetrahedral, bond angle in water is less than that of ammonia. Discuss.

Q 8 | Page 130 | view solution

How do you express the bond strength in terms of bond order?

Q 9 | Page 130 | view solution

Define the bond length.

Q 10 | Page 130 | view solution

Explain the important aspects of resonance with reference to the `CO_3^(2-)` ion.

Q 11 | Page 130 | view solution

H3PO3 can be represented by structures 1 and 2 shown below. Can these two structures be taken as the canonical forms of the resonance hybrid representing H3PO3? If not, give reasons for the same.

Q 12 | Page 130 | view solution

Write the resonance structures for SO3

Q 13.1 | Page 130 | view solution

Write the resonance structures for NO2

Q 13.2 | Page 130 | view solution

Write the resonance structures for `NO_3^(-)`

Q 13.3 | Page 130 | view solution

Use Lewis symbols to show electron transfer between the following atoms to form cations and anions:-

K and S

Q 14.1 | Page 130 | view solution

Use Lewis symbols to show electron transfer between the following atoms to form cations and anions:

Ca and O

Q 14.2 | Page 130 | view solution

Use Lewis symbols to show electron transfer between the following atoms to form cations and anions:

Al and N

Q 14.3 | Page 130 | view solution

Although both CO2 and H2O are triatomic molecules, the shape of H2O molecule is bent while that of CO2 is linear. Explain this on the basis of dipole moment.

Q 15 | Page 130 | view solution

Write the significance/applications of dipole moment.

Q 16 | Page 130 | view solution

Define electronegativity

Q 17.1 | Page 130 | view solution

 How does electronegativity differ from electron gain enthalpy?

Q 17.2 | Page 130 | view solution

Explain with the help of suitable example polar covalent bond.

Q 18 | Page 130 | view solution

Arrange the bonds in order of increasing ionic character in the molecules: LiF, K2O, N2, SO2 and ClF3.

Q 19 | Page 130 | view solution

The skeletal structure of CH3COOH as shown below is correct, but some of the bonds are shown incorrectly. Write the correct Lewis structure for acetic acid.

Q 20 | Page 130 | view solution

Apart from tetrahedral geometry, another possible geometry for CH4 is square planar with the four H atoms at the corners of the square and the C atom at its centre. Explain why CH4 is not square planar?

Q 21 | Page 130 | view solution

Explain why BeH2 molecule has a zero dipole moment although the Be–H bonds are polar.

Q 22 | Page 130 | view solution

Which out of NH3 and NF3 has higher dipole moment and why?

Q 23 | Page 130 | view solution

What is meant by hybridisation of atomic orbitals?

Q 24.1 | Page 130 | view solution

Describe the shapes of sp, sp2,sp3 hybrid orbitals.

Q 24.2 | Page 130 | view solution

Describe the change in hybridisation (if any) of the Al atom in the following reaction.

`AlCl_3 + Cl^(-) -> AlCl_4^(-)`

Q 25 | Page 130 | view solution

Is there any change in the hybridisation of B and N atoms as a result of the following reaction?

BF3 + NH3 → F3B.NH3

Q 26 | Page 130 | view solution

Draw diagrams showing the formation of a double bond and a triple bond between carbon atoms in C2H4 and C2H2 molecules.

Q 27 | Page 131 | view solution

What is the total number of sigma and pi bonds in the following molecules?

(a) C2H2 (b) C2H4

Q 28 | Page 131 | view solution

Considering x-axis as the internuclear axis which out of the following will not form a sigma bond and why? (a) 1and 1(b) 1and 2px (c) 2py and 2py (d) 1and 2s.

Q 29 | Page 131 | view solution

Which hybrid orbitals are used by carbon atoms in the following molecules?

CH3–CH3; (b) CH3–CH=CH2; (c) CH3-CH2-OH; (d) CH3-CHO (e) CH3COOH

Q 30 | Page 131 | view solution

What do you understand by bond pairs and lone pairs of electrons? Illustrate by giving one example of each type.

Q 31 | Page 131 | view solution

Distinguish between a sigma and a pi bond.

Q 32 | Page 131 | view solution

Explain the formation of H2 molecule on the basis of valence bond theory.

Q 33 | Page 131 | view solution

Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.

Q 34 | Page 131 | view solution

Use molecular orbital theory to explain why the Be2 molecule does not exist.

Q 35 | Page 131 | view solution

Compare the relative stability of the following species and indicate their magnetic properties; `O_2, O_2^+, O_2^-`(superoxide), `O_2^(2-)`(peroxide)

 

Q 36 | Page 131 | view solution

Write the significance of a plus and a minus sign shown in representing the orbitals.

Q 37 | Page 131 | view solution

Describe the hybridisation in case of PCl5. Why are the axial bonds longer as compared to equatorial bonds?

Q 38 | Page 131 | view solution

Define hydrogen bond. Is it weaker or stronger than the van der Waals forces?

Q 39 | Page 131 | view solution

What is meant by the term bond order? Calculate the bond order of: N2, O2, `O_2^+`and `O_2^-`

Q 40 | Page 131 | view solution

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