11th Chemistry Chapter 6 Notes

Important Complete Computerized 11th Chemistry Chapter 6 Notes written by Professor Mr. Adnan Haider Suib. These notes are very helpful in the preparation of 11th Chemistry Chapter 6 Notes for the students of the intermediate and these are according to the paper patterns of all Punjab boards.

Summary and Contents:

Topics which are discussed in the notes are given below:

Important Fill in the blanks with answers of Chapter Number 6: Chemical Bonding of First-year Chemistry Punjab Textbook Boards.
Why Noble gases don't form chemical bonds?
Define octet rule. Give two examples of compounds which do not obey this rule.
What is the cause for chemical change?
Why the atoms of the elements other than noble gases combine with one another?
Define bond energy with two parameters which determine its strength?
Compare bond strength of polar and non−polar molecules?
Why the covalent compounds show isomerism, but ionic compounds do not?
Write short note on atomic radii and ionic radii. Give example.
Why atomic radius is greater than cationic radius?
Why cationic radii are smaller than anionic radii?
Why cationic radius is smaller than parent atom?
Define electronegativity and electron affinity of an atom?
Name the factors influencing the electron affinity.
How electron affinity changes in a group?
Fluoride has electron affinity less than the chloride. Give reason.
Why anionic radius is larger than atomic radius?
Why the atomic radii of the atoms cannot be determined precisely?
Why the atomic radii increase down the group?
Why the atomic radius decreases along period and increases along group?
The size of chlorine 𝐂𝐥 atom is smaller than 𝐂𝐈 − ion. Justify it?
Define electronegativity. Give its trend in periodic table.
The size of anion is greater than its parent atom. Justify.
Define ionization energy and electron affinity with one example in each case.
1st ionization energy of Mg is lower than the 2nd ionization energy. Explain.
How ionization energy does vary in periodic table?
Ionization energy decreases down the group although atomic number is increased. Explain it.
Why the ionic radius of Cl− ion increases from 99 pm to 181 pm?
Electronegativity increase from left to right in the periodic table. Give reason.
How electronegativity values of elements help ds in understanding the nature of chemical bond?
Ionization Energy is an Index to the metallic character. Justify it.
Define shielding effect and how it varies along period.
How does Shielding effect affect ionization energy?
The difference in E.N of bonded atoms is index of polar nature of covalent bond.
Define Covalent bond. Give two examples.
Define ionic and covalent radii.
Differentiate between polar and non-polar covalent bond.
Define polar covalent bond with two examples.
No bond in chemistry is 100% ionic.
How coordinate covalent bonds differ from covalent bond?
Why polar bond is stronger than non−polar bond?
Why CO2 and CS2 have linear structures?
NH3 can form coordinate covalent bond with H+ ion. Explain.
What is coordinate covalent bond? Give example.
Why ionic bond is stronger than covalent bond?
Explain the limitations of Lewis model.
Lone pair of electrons on an atom occupies more space. Give reasons.
Write order of repulsion between electron pairs according to VSEPR theory.
What is the basic assumption for Valence Shell Electron Pair Repulsion (VSEPR) theory?
Draw and explain the geometry of NH3 molecule according to valence shell electron pair repulsion theory.
Define lone pair and bond pair of electrons.
Discuss AB2 type molecules in the light of VSEPR theory. Give two examples.
Write the Lewis structures for the following compounds (a) HCN (b) CCl4
Write the Lewis structures for the following compounds (a) BF3 (b) CH4
Why BF3 molecule is triangular planar.
Explain the structure of NH3 molecule on the basis of VSEPR theory.
Deviation in bond angle in water H2O molecule is more than in ammonia NH3 molecule although both have tetrahedral structures.
Give any two postulates of valence shell electron pair repulsion theory.
Explain geometry of H2S molecule on the basis of VSEPR Theory.
Both NH3 and BF3 are tetra atomic but different geometries why?
Write two points of valence Bond Theory.
Sigma Bond is stronger than Pi−Bond. Why?
Tell the number of electron pairs shared in CH4 and how many bonds are polar?
Draw the structure of H2O Molecule on the basis of VBT and explain it.
Define orbital hybridization of orbitals.
How bond length is affected by change of hybridization state?
𝝅 −bonds are more diffused than sigma bonds. How?
Define degenerate orbitals. How degeneracy of orbitals can be lifted?
Differentiate between bonding and anti−bonding molecular orbitals.
Why the energy of anti−bonding molecular orbital is higher than corresponding bonding molecular orbitals?
Draw molecular orbital picture of N2molecule and also calculate its bond order.
Why oxygen molecules show paramagnetic behavior?
Discuss He-molecules on the basis of MOT. OR Why He2 does not exist under Normal Condition?
Represent the molecular orbitals of N2 molecule in the increasing order of energy.
Draw the hypothetical orbital picture of He2 molecule according to M.0.T.
Differentiate between atomic and molecular orbital.
MOT is Superior to VBT explain.
Bond distance is compromise distance between two atoms. Explain with reason.
The abnormality of bond length and bond strength in Hl is less prominent than that of HCI. Why?
How the criteria of electronegativity help us to understand the nature of bond?
What is difference between bond length and bond energy?
Why CH4 molecule is called tetrahedral? Mention maximum number of bond angles in it?
Define Covalent Radius with an example.
Why sigma bond is stronger than Pi−bond?
Differentiate between Sigma and Pi−bond.
What information about the molecular structure are obtained from the dipole moment?
Why BF3 is non−polar but SO2 is polar?
Define "Dipole Moment" and give its mathematical form and S.I unit.
Why the dipole moment of SO2 is 1.61 D but that of SO3 is zero?
CO2 molecules have linear structure while H2O have angular structure. Comment.
Why the dipole moment of CH4 is zero?
The dipole moment of CO2 is zero but that of CO is 0.12 D. Give reason. OR Why CO is polar and CO2 is non-polar?
Why no bond can have 100% ionic character?
Why CO2 has zero dipole moment and that of water has value of dipole moment 1.85 D?
Why the melting points, boiling points, heat of sublimation and heat of vaporization of electrovalent compounds are higher as compared with those of covalent compounds?
Why covalent compounds react slowly than the ionic compounds?
Reactions between ionic compounds are very rapid, give reason.
What is the effect of bonding on solubility of a compound?
Ionic compounds are mostly soluble in water but insoluble in non−polar solvents. Give reason.
Explain important points of molecular orbit theory and draw structure of nitrogen (N2) molecule according to this theory.
Define dipole moment. Give its Sl units. Also write its significance. Explain the geometry of CO2, BF3 and H2O by dipole moment.
Define Sp² hybridization and on its basis explain the structure of ethane.
Define hybridization of atomic orbitals. Discuss Sp3 hybridization in detail. Draw the structure of methane.
Calculate the bond order of O2 molecule by making energy level diagram. Also show that it is paramagnetic.

Loading your document...

Download PDF