Chemical Bonding and Molecular Structure

These measure the tendency of an atom to accept electrons. The atoms with high electronegativity and electron affinity readily form anion and hence ionic compounds.

An atom with low ionization energy, readily loses electron. So it forms the cation readily and produce ionic compounds. Ex: Potassium gives the cation more readily than sodium because the ionization potential of potassium is less than the sodium atom.

In a triple bond, six electrons attract the nuclei with greater force, out of the three types of bond length. This decreases the distance of separation between the two nuclei the most. Hence the bond length is shortest in triple bond.Since, a shorter bond means greater bond strength hence, the energy required to separate the bonded atoms is maximum.

A line is drawn by joining 2 points. In the same way a molecule is formed by the combination of two atoms.

Trinitrotoluene (TNT) is used to measure the strength of bombs.

This option is correct. In Pb⁺² inert pair effect is there i.e. because of lanthanoid contraction , poor shieding effect of  4f¹⁴  electrons . The effective nuclear charge increases and after removal of two  electrons it becomes really hard to remove the other two electrons . Hence, Pb⁺² is most stable among its group because lanthanoids contraction observe in this atom only .

This option is correct because , in ClOH chlorine has three lone pair and the electron on O^- is unable to delocalise itself . Hence, it will remain on oxygen atom and  has the highest basicity among the given options .  

This option is correct because , during the hydrolysis ,  water being neucleophile always prefer to attack the central atom first . it will attack the central atom  only when it posses vacant orbitals . If the central atom doesn't posses vacant orbital then attack  of water molecules taken place on peripheral atom provided they also posses vacant orbitals . in this case niether central nor peripheral atom posses vacant orbital hence hydroysis doesn't takes place in this molecule . 

This option is correct. Bond order of N₂ = 3. Bond order of N₂⁺ = 2.5. Bond order of N₂^- = 2.5. Since bond order of N₂⁺ and N₂^- is the same, but the effective nuclear charge of N₂⁺ is more than that of N₂^-, so the correct order is N₂ > N₂⁺ > N₂^-.

You might have remembered  this logic  , if the total number of electrons comes out to be 50  the hybridisation is capped octahedral i.e. sp³d² or distorted octahedral .  

XeF₂ has three lone pairs of electrons with linear geometry.

SF₄ has one lone pair of electrons with seesaw geometry.

I^3- and XeF₂ both have three lone pair of electrons with linear geometry. HgCl₂ has zero lone pair of electrons with linear geometry. SO₂ has one lone pair of electron with bent shape.  Hence, 1, 2, 3 all molecules have linear geometry.

P. NH₃ and PCl₃ both molecules have one lone pair of electrons with trigonal pyramidal geometry. S. CO₂ has zero lone pair of electrons with linear geometry. XeCl₂ has three lone pairs of electrons with linear geometry. Hence, P and S statements are incorrect.

According to VSEPR theory, BrF₄^- and XeF₄ both have four bond pair of electrons and two lone pair of electrons with square planar shape. TeCl₄ has four bond pair of electrons and one lone pair of electrons with distorted trigonal bipyramidal shape.  Hence, 1 and 2 have square planar shape.