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1st Year Chemistry Short Questions (Chapter 6)

 If you are in 1st year class



And searching for important short questions for your exams preparation than read it out 


Here is some short questions from chapter 6 of 1st year

 


INTRODUCTION


1. Define chemical bond 


2. Why noble gases are most stable (least reactive)?


3. Explain octet rule. It is not universal. Comment 


4. Bond distance is a compromise distance b/w two bonded atoms


ATOMIC, IONIC & COVALENT RADIUS 


5. Define ionic and covalent radius.


6. Radius of an atom cannot be measured precisely. Give two reasons 


7. Write variation of atomic radius in periodic table?


8. Why ionic radius is greater than atomic radius (Why size of Cl' is greater than Cl)?


9. why size of cation is always smaller than neutral atom?


10. What is interionic distance. Explain with example


IONIZATION ENERGY, ELECTRON AFFINITY & ELECTRONEGATIVITY 


11. Define ionization energy How do it vary in periodic table?


12. Name four factors which effect ionization energy of atom


13. Why 2nd ionization energy is always greater than first ionization energy?


14. Ionization energy is the index of metallic character.


15. Define electron affinity. How do it vary in periodic table?


16. Why first electron affinity of atoms is negative while 2nd is positive?


17. Define electronegativity. How do it vary in periodic table? 


18. How does E.N difference decide the nature of ionic bond?


 TYPES OF BONDS 


19. Define ionic bond with example


20. No bond is 100% ionic. Justify 


21. Define covalent bond with examples


22. Compare polar and non-polar covalent bonds


23. Write the Lewis structures of NH4OH & H2SO.?


24. What is coordinate covalent bond. Give one example 


25. Why the distinction b/w covalent and coordinate covalent bond vanish after bond formation in H3O+ and NH4+ 


26. Discuss the formation of ammonium ion 


27. Lewis model seems to be over simplified. Justify (Limitation of Lewis model)


VSEPR THEORY 


28. What is VSEPR theory Write its two postulates


29. Why lone pair occupy more space than bond pair ?


30. What is order of repulsion b/w electron pairs?


31. Why the bond H2O & NH3 are not 109.5° like that of CH4, although O&N atoms are SP3 hybridized?


32. Why NH3 and NF3 have different bond angles?


33. Why NH3 & NH4+ have different structures?


VALENCE BOND THEORY


34. What is valence bond theory? Give two postulates


35. Differentiate sigma and Pi bonds.


36. Pi bonds are more diffused than sigma bonds. (Pi bonds are weaker than sigma bonds.) Why? 


37. Define hybridization, SP3, SP2, SP hybridization


MOLECULAR ORBITAL THEORY 


38. What is meant by the term bonding and anti-bonding molecular orbitals?


39. Why energy of anti-bonding molecular orbitals are higher than bonding molecular orbitals?


40. He2 molecule is not formed. Why?


41. Explain the term bond order.


42. Why MOT is superior to VBT 


43. Why oxygen is paramagnetic?


BOND ENERGY, BOND LENGTH & DIPOLE MOMENT 


44. Define bond energy. Write factors that determine the strength of bond energy.


45. Why abnormality in bond length and bond strength in HI is less prominent than HCI? 


46. What is dipole moment? Give its various units


47. How %age of ionic character in a bond is determined?


48. Why the dipole moment of CH4 is zero? 


49. The dipole moment of CO2 is zero and that of H20 is 1.85 D (Dipole moment of CO2 is zero but that of SO2 is 1.61 D).


50. Compare dipole moment of CO & CO2. Give reason 




REGARDS : TALHA 

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