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Chapters
2: Introduction to Analytical Chemistry
3: Basic Analytical Techniques
4: Structure of Atom
▶ 5: Chemical Bonding
6: Redox Reactions
7: Modern Periodic Table
8: Elements of Group 1 and 2
9: Elements of Group 13, 14 and 15
10: States of Matter
11: Adsorption and Colloids
12: Chemical Equilibrium
13: Nuclear Chemistry and Radioactivity
14: Basic Principles of Organic Chemistry
15: Hydrocarbons
16: Chemistry in Everyday Life
![Balbharati solutions for Chemistry [English] 11 Standard chapter 5 - Chemical Bonding - Shaalaa.com](/images/chemistry-english-11-standard_6:1ddd95908cb04440a83d42566c3337de.jpg "Balbharati solutions for Chemistry [English] 11 Standard chapter 5 - Chemical Bonding")
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Solutions for Chapter 5: Chemical Bonding
Below listed, you can find solutions for Chapter 5 of Maharashtra State Board Balbharati for Chemistry [English] 11 Standard.
Balbharati solutions for Chemistry [English] 11 Standard 5 Chemical Bonding Exercises [Pages 79 - 80]
Select and write the most appropriate alternatives from the given choices.
Which molecule is linear?
SO3
CO2
H2S
Cl2O
Select and write the most appropriate alternatives from the given choices.
When the following bond types are listed in decreasing order of strength (strongest first). Which is the correct order?
covalent > hydrogen > vander waal’s
covalent > vander waal’s > hydrogen
hydrogen > covalent > vander waal’s
vander waal’s > hydrogen > covalent
Select and write the most appropriate alternatives from the given choices.
Valence Shell Electron Pair repulsion (VSEPR) theory is used to predict which of the following:
Energy levels in an atom
the shapes of molecules and ions
the electrone getivities of elements
the type of bonding in compounds
Select and write the most appropriate alternatives from the given choices.
Which of the following is true for CO2?
C = O bond CO2 molecule polar non-polar C = O bond CO2 molecule non-polar polar C = O bond CO2 molecule polar polar C = O bond CO2 molecule non-polar non-polar
Select and write the most appropriate alternatives from the given choices.
Which O2 molecule is paramagnetic. It is explained on the basis of ______.
Hybridization
VBT
MOT
VSEPR
Select and write the most appropriate alternatives from the given choices.
The angle between the two covalent bonds is minimum in:
CH4
C2H2
NH3
H2O
Draw Lewis dot diagram for the following.
Hydrogen (H2)
Draw Lewis dot diagram for the following.
Water (H2O)
Draw Lewis dot diagram for the following.
Carbon dioxide (CO2)
Draw Lewis dot diagram for the following.
Methane (CH4)
Draw Lewis dot diagram for the following.
Lifthium Fluoride (LiF)
Draw diagram for bonding in ethene with sp2 Hybridisation.
Draw Lewis electron dot structure of HF
Draw Lewis electron dot structure of C2H6
Draw Lewis electron dot structure of C2H4
Draw Lewis electron dot structure of CF3Cl
Draw Lewis electron dot structure of SO2
Draw an orbital diagram of Fluorine molecule
Draw an orbital diagram of Hydrogen fluoride molecule
Distinguish between sigma and pi bond.
Display electron distribution around the oxygen atom in the water molecule and state the shape of the molecule, also write the H-O-H bond angle.
State octet rule.
Explain inadequacies octet rule with respect to
- Incomplete octet
- Expanded octet
Explain in brief with one example of an ionic bond.
Explain in brief with one example of a covalent bond
Explain in brief with one example of coordinate bond
Give reasons for need of Hybridization
Explain geometry of methane molecule on the basis of Hybridization.
In Ammonia molecule the bond angle is 107° and in water molecule it is 104°35', although in both the central atoms are sp3 hybridized Explain.
Give a reason for the sigma (σ) bond is stronger than the Pi (π) bond.
Give a reason for HF is a polar molecule
Give a reason for carbon is tetravalent in nature.
Which type of hybridization is present in the ammonia molecule?
Write the geometry and bond angle present in ammonia.
Identify the type of overlap present in H2. Explain diagrammatically.
Identify the type of overlap present in F2. Explain diagrammatically.
Identify the type of overlap present in H-F molecule. Explain diagrammatically.
F-Be-F is a liner molecule but H-O-H is angular. Explain.
BF3 molecule is planar but NH3 pyramidal. Explain.
In the case of bond formation in Acetylene molecule: How many covalent bonds are formed?
In the case of bond formation in Acetylene molecule: State number of sigma and pi bonds formed.
In the case of bond formation in Acetylene molecule: Name the type of Hybridization.
Define Bond Enthalpy
Define Bond Length
Predict the shape and bond angles in the following molecule:
CF4
Predict the shape and bond angles in the following molecule:
NF3
Predict the shape and bond angles in the following molecule:
HCN
Predict the shape and bond angles in the following molecule:
H2S
Using data from the Table, answer the following:
| Examples | C2H6 Ethane | C2H4 Ethene | C2H2 Ethyne |
| Structure |
\[\begin{array}{cc} \backslash \phantom{......}/\phantom{.}\\ \ce{—C – C —}\\ /\phantom{......}\backslash\phantom{.}\end{array}\] |
\[\begin{array}{cc} \backslash \phantom{......}/\\ \ce{C \text{=} C}\\ /\phantom{......}\backslash\end{array}\] |
\[\ce{- C ≡ C -}\] |
| Type of bond between carbons | single | double | triple |
| Bond length (nm) | 0.154 | 0.134 | 0.120 |
| Bond Enthalpy kJ mol-1 | 348 | 612 | 837 |
- What happens to the bond length when unsaturation increases?
- Which is the most stable compound?
- Indicate the relationship between bond strength and Bond enthalpy.
- Comment on the overall relation between Bond length, Bond Enthalpy, and Bond strength and stability.
Complete the flow chart.
| Molecular Formula | Structural Formula | Shape/ Geometry | Bond angle |
| BeCl2 | 180° | ||
| O=C=O | Linear | ||
| C2H2 |
Complete the following Table.
| Molecule | Type of Hybridization | Type of bonds | Geometry | Bond angle |
| CH4 | - | 4C-H 4σ bonds |
Tetrahedral | - |
| NH3 | sp3 | 3N-H 3σ bonds 1 lone pair |
- | - |
| H2O | - | - | angular | 104.5° |
| BF3 | sp2 | - | - | 120° |
| C2H4 | - | - | - | 120° |
| BeF2 | - | 2 Be-F | Linear | - |
| C2H2 | sp | (3σ+2π) 1C-C σ 2C-H σ 2C-C π |
- | - |
Indicate the factor on which stability of ionic compound is measured?
Arrange the following compounds on the basis of lattice energies in decreasing (descending) order:
BeF2, AlCl3, LiCl, CaCl2, NaCl
Give the total number of electrons around sulfur (S) in SF6 compound.
Answer in one sentence:
Covalent bond is directional in nature. Justify.
What are the interacting forces present during the formation of a molecule of a compound?
Give the type of overlap by which the pi (π) bond is formed.
Mention the steps involved in Hybridization.
Write the formula to calculate the bond order of molecule.
Why is O2 molecule paramagnetic?
What do you mean by formal charge?
Explain the significance of formal charge with the help of a suitable example
Solutions for 5: Chemical Bonding
Balbharati solutions for Chemistry [English] 11 Standard chapter 5 - Chemical Bonding
Shaalaa.com has the Maharashtra State Board Mathematics Chemistry [English] 11 Standard Maharashtra State Board solutions in a manner that help students grasp basic concepts better and faster. The detailed, step-by-step solutions will help you understand the concepts better and clarify any confusion. Balbharati solutions for Mathematics Chemistry [English] 11 Standard Maharashtra State Board 5 (Chemical Bonding) include all questions with answers and detailed explanations. This will clear students' doubts about questions and improve their application skills while preparing for board exams.
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Concepts covered in Chemistry [English] 11 Standard chapter 5 Chemical Bonding are Introduction of Chemical Bonding, Kossel-lewis Approach to Chemical Bonding - Octet Rule, Kossel and Lewis Approach to Chemical Bonding, Kossel-lewis Approach to Chemical Bonding - Formal Charge, Kossel-lewis Approach to Chemical Bonding - Limitations of the Octet Rule, Valence Shell Electron Pair Repulsion Theory (VSEPR), Valence Bond Theory, Molecular Orbital Theory, Parameters of Covalent Bond, Dipole Moment, Resonance.
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