CBSE Class 11 Chemistry Chemical Bonding And Molecular Structure Worksheet Set B

Read and download free pdf of CBSE Class 11 Chemistry Chemical Bonding And Molecular Structure Worksheet Set B. Students and teachers of Class 11 Chemistry can get free printable Worksheets for Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure in PDF format prepared as per the latest syllabus and examination pattern in your schools. Class 11 students should practice questions and answers given here for Chemistry in Class 11 which will help them to improve your knowledge of all important chapters and its topics. Students should also download free pdf of Class 11 Chemistry Worksheets prepared by school teachers as per the latest NCERT, CBSE, KVS books and syllabus issued this academic year and solve important problems with solutions on daily basis to get more score in school exams and tests

Worksheet for Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure

Class 11 Chemistry students should refer to the following printable worksheet in Pdf for Chapter 4 Chemical Bonding and Molecular Structure in Class 11. This test paper with questions and answers for Class 11 will be very useful for exams and help you to score good marks

Class 11 Chemistry Worksheet for Chapter 4 Chemical Bonding and Molecular Structure

Chemical Bonding and Molecular Structure MCQ Questions with Answers Class 11 Chemistry

Question. Which species does not exhibit paramagnetism?

(1) N 2+

(2) O 2

(3) CO

(4) NO

Answer (3)

 

Question. Which one of the following species does not exist under normal conditions?

(1) Li2

(2) Be2-

(3) Be 2

(4) B 2

Answer (3)

 

Question. The maximum number of 180° angle possible between X-M-X bond for compounds with sp3d2 and sp3 dhybridisation respectively are

(1) 3, 3

(2) 3, 1

(3) 1, 3

(4) 3, 0

Answer (2)

 

Question. Which of the following molecule stabilizes by removal of electron?

(1) C 2

(2) O 2

(3) N 2

(4) H 2

Answer (2)

 

Question. In NO 3 – ion number of bond pair and lone pair of electrons on nitrogen atom are

(1) 2, 2

(2) 3, 1

(3) 1, 3

(4) 4, 0

Answer (4)

 

Question. Which of the following statement is correct?

(1) The hybridisation of Cl in ClF 3 is sp 2

(2) The number of lone pairs and bond pairs in I 3 – are 2 and 2 respectively

(3) The shape of XeF 6 is distorted square bipyramidal

(4) Hybridisation of S is sp 3 in SO 2

Answer (3)

 

Question. Which of the following is not a correct statement?

(1) Multiple bonds are always shorter than corresponding single bonds

(2) The electron-deficient molecules can act as Lewis acids

(3) The canonical structures have no real existence

(4) Every AB 5 molecules does in fact have square pyramid structure

Answer (4)

 

Question. A certain diatomic molecule, AB has dipole moment 1.6 D and the internuclear distance is 100 pm. The percentage of electronic charge existing on more electronegative atom is

(1) 33%

(2) 25%

(3) 50%

(4) 10%

Answer (1)

 

Question. The hybrid orbital having only 20% d character

(1) CCl 4

(2) SF6

(3) SF4

(4) Cl2O

Answer (3)

 

Question. Which of the following is correct for XeO2F2 and PCl5 ?

(1) Both have same hybridisation and shape

(2) Both have same hybridisation but different geometry

(3) Both have different hybridisation but same shape

(4) Both have same hybridisation but different shape

Answer (4)

 

Question.Which one of the following has the strongest O – O bond?

(1) O2+

(2) O2
(3) O2

(4) O2 2–

Answer (1)

 

Question. Some of the properties of the two species, NO3- and H 3 O+ are described below. Which one of them is correct?

(1) Dissimilar hybridization for the central atom with different structures

(2) Isostructural with same hybridization for the central atom

(3) Isostructural with different hybridization for the central atom

(4) Similar hybridization for the central atom with different structures

Answer (1)

 

Notes for Class 11 Chemistry Chemical Bonding

A chemical bond is defined as the force of attraction between any two atoms in a molecule to maintain stability.
 
Noble Gases
 Have stable electronic configuration, i.e. their outermost shell is complete.
 They have 2 electrons in the outermost shell or 8 electrons in the outermost shell.
 They do not lose, gain or share electrons and are inert or unreactive.
 
Atoms of Elements – Other than Noble Gases
 Have unstable electronic configuration, i.e. their outermost shell is incomplete.
 They can lose, gain or share electrons and are chemically reactive.
 
Reasons for Chemical Bonding
 The driving force for atoms to combine is related to the tendency of each atom to attain stable electronic configuration of the nearest inert noble gas.
 For an atom to achieve stable electronic configuration, it must have
 
Two electrons in the outermost shell (nearest noble gas He) – Duplet rule
Eight electrons in the outermost shell (all noble gases other than He) – Octet rule
 
Methods for achieving Chemical Bonding
There are three methods in which atoms can achieve a stable configuration:
 Electrovalent bond
 Covalent bond
 Coordinate bond
 
Electrovalent (or Ionic) Bond
¶ Ionic bond
The chemical bond formed between two atoms by transfer of one or more electrons from the atom of a metallic electropositive element to an atom of a non-metallic electronegative element.
¶ Ionic compound
The chemical compound formed as a result of transfer of one or more electrons from the atom of a metallic electropositive element to an atom of a non-metallic electronegative element.
¶ Electrovalency
The number of electrons donated or accepted by the valence shell of an atom of an element so as to achieve stable electronic configuration is called electrovalency.
 
Conditions for the formation of an Ionic Bond
Ionisation potential (IP): Lower the value of IP of a metallic atom, greater the ease of formation of the cation.
Electron affinity: Higher the value of EA of a non-metallic atom, greater the ease of formation of the anion.
Electronegativity: Larger the differences in electronegativity between the combining atoms, greater the ease of electron transfer.
 
Formation of electrovalent compounds
Formation of Sodium Chloride

N

Covalent Bond 
¶ Covalent bond: The chemical bond formed due to mutual sharing of electrons between the given pairs of atoms of non-metallic elements. 
¶ Covalent compound: The chemical compound formed due to mutual sharing of electrons between the given pairs of atoms, thereby forming a covalent bond between them. 
¶ Covalency: The number of electron pairs which an atom shares with one or more atoms of the same kind or different kind to achieve stable electronic configuration is called covalency. 
¶ Non-polar covalent compounds: Covalent compounds are said to be non-polar when the shared pair of electrons are equally distributed between the two atoms. 
Examples: H2, Cl2, O2, N2, CH4, CCl4 
¶ Polar covalent compounds: Covalent compounds are said to be polar when a shared pair of electrons are unequally distributed between the two atoms. 
Examples: H2O, NH3, HCl 
 
Conditions for formation of covalent compound 
Ionisation potential, electron affinity and electronegativity: High between both the atoms. 
Electronegativity difference: Should be negligible between the two combining atoms.
 
Formation of methane molecule – Non-polar covalent compound
A
 
One atom of carbon shares four electron pairs, one with each of the four atoms of hydrogen.
A-
 
Coordinate Bond
The bond formed between two atoms by sharing a pair of electrons provided entirely by one of the combining atoms but shared by both is called a coordinate bond or dative bond.
Examples: Ammonium ion (NH4+), hydronium ion (H3O+)
A coordinate bond has properties of both covalent and ionic bonds. So, it is also called a co-ionic bond.
¶ Lone pair of electrons: A pair of electrons which is not shared with any other atom is known as a lone pair of electrons. It is provided to the other atom for the formation of a coordinate bond.
¶ Conditions for the formation of coordinate bond
1. One of the two atoms must have at least one lone pair of electrons. Examples: Ammonia (NH3), water (H2O)
2. Another atom should be short of at least one lone pair of electrons. Example: Hydrogen ion (H+)

Aa

 

Redox Reaction 
 Oxidation: When an atom or ion loses an electron or electrons, oxidation takes place. 
 Reduction: When an atom or ion gains an electron or electrons, reduction takes place. 
 Oxidising agents: The atom or ion which gains an electron or electrons is an oxidising agent. 
 Reducing agents: The atom or ion which loses an electron or electrons is a reducing agent. 
¶ Redox reaction: A chemical reaction in which the loss and gain of electrons take place simultaneously is called a redox reaction. 
Example:

Aa-

 

Instructions:

1. All questions are compulsory.

2. Please give the explanation for the answer where applicable.

Q1 - What is hydrogen bonding? Name the two types of hydrogen bonding?

Q2 -Find

(i) Formal charge on S in HSO4-

(ii) Formal charge on P in orthophosphoric acid

Q3 - Which of the following bond is most polar?

(i) Cl-F

(ii) Br-F

(iii) I-F

(iv) F-F

Q4 - Which of the following compound will have highest solubility in water CCl4, CHCl3, CS2,C2H5OH.

Q5 - Name the type of hybridisation in each carbon atom of the following compounds —

(i) 1, 2 – butadiene

(ii) Propyne

Q6 - Find the bond order of NO and CO.

Q7 - How is bond order related to the stability of a molecule?

Q8 - What is the maximum number of hydrogen bonds in which a water molecule can participate?

Q9 - Arrange F2, N2, Cl2, O2 in increasing order of bond strengths.

Chapter 03 Classification of Elements and Periodicity in Properties
CBSE Class 11 Chemistry Classification Of Elements And Periodicity Worksheet
Chapter 12 Organic Chemistry – Some Basic Principles & Techniques
CBSE Class 11 Chemistry Organic Chemistry Worksheet

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