CHEMICAL BONDING - 10 ICSE CHAPTER WISE QUESTIONS

2. CHEMICAL BONDING

BONDING
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           Short answer questions

 1.   What kind of elements from positively charged ions?

 2.   What kind of elements from negatively charged ions?

 3.   Why sodium ion is not reactive, but Na metal is very reactive?

 4.   “atoms and ions differ in their physical as well as chemical properties.” Give example to

        support this statement.

 5.   A.Name the covalent compound, which dissolves in water and conducts electricity.

       B. which one property of the above compound, which agrees with it being a covalent  

            compound?

 6.   State the types of bonds present in a. sodium chloride   b. methane       c. carbon

        tetrachloride.           d. calcium oxide   e. Ammonium ion       f. Ammonium chloride.

 7.   What type of bonding is expected in a metallic chloride?

 8.   Acids dissolve in water to produce positively charged ions. Draw the structure of the

      positive ion.

 9.   What is a lone pair of electrons? Name a neutral covalent molecule which contains a lone

      pair of electrons.

 10.  Why is it that metals form positive ions and non metals form negative ions?

 11.  Among the following: NaCl, CCl4, HCl and CH4, which is polar molecule?

 12.  Which among the following: H2O, NH3, BF3 and NH4+ possesses a co-ordinate bond?

 13.  Which one of the following is non polar: CH4, H2O, NH3, HCl

Long answer questions

 1.   Define the following terms:                                                                                                   

         a. electrovalency                                       b. electrovalent or ionic bond.           

         c. electrovalent or ionic compound.        d. valence shell electrons

 2.   Draw the electron dot structures of the following                                                                             a. NaCl            b. MgCl2       c. CaO

 3.   A. what are ions? Define the i. Anion and      ii. Cation.                              

       B. what are the difference between a Na atom and Na+ ion?

 4.   Define the following on the basis of electronic concept:                                                                  
       a. oxidation     b. reduction         c. oxidizing agent        d. reducing agent.

 5.   Identify the following reactions as either oxidation or reduction:                                                    
             a. Mg – 2e-   --->               Mg        b. Fe+2 – e-    --->             Fe+3   

            c. Cl + e-      --->                Cl-         d. O + 2 e-      --->             O-2

 6.   Define the following terms:    a. covalency    b. covalent bond   c. covalent compound

 7.   Draw the electron dot structures of the following: H2O, NH3, CH4, N2, CCl4 and Cl2

 8.   State three differences between the properties of ionic and covalent compounds.

 9.   Explain giving suitable examples: a. polar covalent molecule   b. non polar molecule

10.  Explain with the help of a suitable electron dot structure diagrams the formation of          

        a. A non polar covalent compound, e.g., CCl4                                                         

        b. A polar covalent compound, e.g, HCl

 11.  Define co-ordinate bond.

 12.  Draw the electron dot structure of the following also stating the types of bonds involved:  

         a. NH4+                      b. H3O+

 13.  Explain giving reasons for the following:

        a.   Solid NaCl does not conduct electricity but its aqueous solution conducts electricity.

        b.   Ionic compounds generally have high melting and boiling points.

        c.   Ionic compounds are soluble in polar solvents but insoluble in non polar solvents.

        d.  Covalent compounds do not conduct electricity.

        e.  Covalent compounds usually have low melting and boiling points.

         f.  Covalent compounds are generally liquids or gases.

 14.  What do you understand by the term “electrolytic dissociation”?  How does it differ from    

       ionization?

 15.  An element C has electronic configuration of (2,8,18,8,1). Without identifying C,        

       a.  predict the sign and charge on simple ion of C.                                                       

       b.  state wheather you would except the element C metal or a non metal.                       

       c. write the probable formula of chloride of C. State the type of bonding inovolved.

 16.  The electron arrangement of atoms of three elements A, B and C is A(2,8,1); B(2,8,6) 

       C(2,8,7).                                                                                                  

       a.    Write down the formula of molecule of B and its electron dot diagram. Mention the 

           type of bonding

        b.   Write down the formula of compound formed between A and C and type of bonding.

        c.    Calssify the elements A, B and C as metals and non metals.

        d.   Which element is likely to be a good conductor of electricity and why?

 17.  The electronic configuration of element X is 2,8,5 and the e.configuration of element Y is 

      2,8,7. What is the likely formula of the compound containing only X and Y?

 18.  Use the following information to answer the questions given below about the element A, B,

        C & D:                                                                                                                               

       element                                                A                       B         C              D                           

        e. configuration                               2,8,8                   2,6     2,8,2       2,8,8,l 

a.    What type of bonding exists between B and D gap?

b.   Which element is not likely to form bonds with other elements?

c.    Name any two elements which form ions having the same electronic configuration as neon.

       a19.  The electronic configuration of the atoms P,Q and R are given

       below:                                

                     P = 2,1             Q = 2,6            &         R = 2,7

 a.    What types of bonds are formed between                  i. P & Q   ii. P & R      iii. Q & R?

 b.   What are the formulae of the compound formed between i. P & Q  ii. P & R

 20.  Elements A, B and C have atomic numbers 8, 10 and 13, respectively. Identify the one

        that (a) forms a cation     (b) forms an anion            (c) does not form an ion.

Conceptual questions 

1.   An element A has four electrons in the outermost shell of its atom and combine with another element B, having seven electrons in the outermost shell of its atom. The compound does not conduct electric current and fails to give a precipitate with a solution of AgNO3. What is the nature of the chemical bond in the compound? Write the electron dot structure of its molecule.

2.   NaCl is a electrovalent compound while hydrogen chloride is a covalent compound. But both form ions in their aqueous solution. explain.

3.   An element M burns in oxygen to form an electrovalent compound MO. What compounds do you expect if the element is made to combine with chlorine and sulphur?

4.    

Element	Atomic number
A	Z-1
B	Z
C	Z+1
D	Z-1

 

In the table given above, A, B, C and D are elements. Given B is an inert gas ( not Helium), what type of bonding would take place between. A) A and C, and B) A and D?

5.   Why NaCl gives a white precipitate with AgNO3 but CCl4 does not?

6.   An element ‘X’ has two electrons in the outermost shell of its atom and combines with an element having seven electrons in the outermost shell of its atom.                                                  
 A. Write the formula of the compound formed.            
 B. What type of bond will be formed between X and Y?           
 C. is it soluble in water or benzene

7.   Why HCl molecule is polar while Cl2 molecule is non polar?

8.   Why is HCl predominantly covalent in gaseous state but it ionizes in aqueous solution?

Previous Years ICSE Examination Questions

Short Answer Questions

1.   Name a covalent compound which behaves like an ionic compound in aqueous solution.

2.   A. What is a lone pair of electrons?    B. Draw an electron dot diagram of a hydronium ion

       and label the lone pair of electrons.

3.   Name a neutral covalent molecule which contains a lone pair of electrons.

4.   Identify the following reactions as either oxidation or reduction.   

               A. O    +            2electrons     -->               O-2      B. K – 1 electron  -->        K+1                

               C. Fe+3           +          1electron        -->                Fe+2

 5.   Compound X consists of molecules. Answer the following by choosing the correct

       answer from the choices given below:                     

      a. The type of bonding in X will be – Ionic, Covalent, electrovalent or molecular bond    

      b. X is likely to have a  

               i. low M.P and high B.P         ii. High M.P and low B.P                                            

               iii. Low M.P and low B.P       iv. High M.P and high B.P                        

     c. In the liquid state, X will                   

           i. become ionic.                       ii. Be an electrolyte                                                              

          iii. Conduct electricity              iv. Don’t conduct electricity

 6.   Explain why solid NaCl does not allow electricity to pass through it.

 7.   Electrons are getting added to an element y.      

     a. Is Y getting oxidized or reduced? 

     b. What charge will y have after the addition of electrons/   

     c. which electrode will Y migrate to during the process of electrolysis.

 

 Long Answer Questions

 1.   A. In covalent compounds, the bond is formed due to the ___________ electrons.

   (a)  Electrovalent compounds have a _________ B.P.

   (b) a molecule of __________  contains a triple bond.                                                      

   (c) By drawing an electron dot diagram, show the lone pair effect leading to the formation of

         ammonium ion from ammonia gas and hydrogen ion.

   (d) Give reasons why HCl can be termed as a polar covalent compound.

 2.    Consider the section of the Periodic table given below:                                                           

Group number	IA	IIA	IIIA	IVA	VA	VIA	VIIA	0 group
	1	2	13	14	15	16	17	18
	Li		D			O	J	Ne
	A	Mg	E	Si		H	K
	B	C		F	G			L

        Some elements are given in their own symbols and position in the P.table while others are shown with a letter. With reference to the above table, answer the following questions:                     

       a. Which is the most electronegative element?                                                                   

       b. How many valence electrons are present in G?                                                                

       c. Write the formula of the compound between B and H.                                                   

       d. In the compound between F and J, what type of bond will be formed?                          

       e. Draw electron-dot structure for the compound formed between C and K.

 3.   Methane is the first member of alkane family when it is treated with excess of Cl2 in the

       presence of diffused sunlight if forms Carbon tetrachloride. Draw appropriate formula of

      Carbon tetrachloride and state the type of bond present in it.

 4.   A. Name the charged particles which attracts one another to form electrovalent

       compounds.                                                                                                                  

      B. In the formation of electrovalent compounds, electrons are transferred from one element

      to another. How are electrons involved in the formation of a covalent compound           

      C. The electronic configuration of Nis 2,5. How many electrons in the outer shell of a N atom

       are not involved in the formation of a nitrogen molecule?                                            

      D. In the formation of MgCl2, name the substance that is oxidized and the substance that is

      reduced.

5.   A. Acids dissolve in water to produce positively charged ions. Draw the structure of these

     positively charged ions.                                                                                                        

      B. Explain why carbon tetrachloride does not dissolve in water.                                         

      C. Elements Q and S react together to form an ionic compound. Under normal conditions,

           which physical state will the compound QS exist in? Can Q and S, both be metals? Justify your answer.

 6.   Element X is a metal with a valency 2. Element Y is a non metal with a valency 3.                 

      A. Write the chemical equations to show how X and Y form ions.                                       

      B. If Y is a diatomic gas, write the chemical equation for the direct combination of X and Y

           to form a compound.                                                                                             

      C. If the compound formed between X and Y is melted and an electric current passed

           through the molten compound, the element will be obtained at the __________ and Y at

           the ____________ of the electrolytic cell.

7.   Copy and complete the following table:                                                                                    

Property	Sodium	Phosphorus
Formula of chloride
Physical state of Chloride at room temperature
Nature of bonding in chloride