Retro (Past 13 Years) JEE Main (Chemical Bonding) - JEE MCQ

groups do not cancel their dipole moments and hence exists as different conformations.

Since, all the electrons are paired, it is a diamagnetic specie

It is also a diamagnetic specie because of the absence of un paired electrons.

Since, O₂ or S₂ contain 2 unpaired electrons, therefore they are paramagnetic.

Species having zero or negative bond order do not exist.

Bond order = 0

Stability order is    have more number of electrons in antibonding orbitals which destabilises the species).

MCl₃ has sp³ hybridise  M-element with one lone pair.
Lone-pair and bond pair repulsion decreases bond angle. However, the bond pairs of electrons are much farther away from the central atom than they are in NCI₃. Thus, lone pair causes even greater distortion in PCI₃, AsCI₃ and SbCI₃.

Thus, bond angle decreases from NCI₃ (maximum) to SbCI₃ (minimum).

Covalent character is favoured by Fajans ’ rule.
(i) Larger the charge on the ions,
(ii) Smaller the size of cations,
(iii) Larger the size of anions,
(iv) Cation with 18-electrons structure (e.g.Cu⁺),
then larger the polarising power and the covalent character is favoured.
In all the given compounds , anion is same (Cl^-), hence polarising power is decided by size and charge of cation.
Al³⁺ with maximum charge and smallest size has maximum polarising power hence, AICI₃ is maximum covalent.

Count σ -bond , lone pairs and unpaired electrons or count number of atoms directly attached, lone pairs and unpaired electrons.

 IF₇ Outer orbital diagram of I



Seven sp³d³ hybrid orbitalsforming s-bonds with F-atoms,

In carbide ion, two carbon atoms are joined by triple bond (It is isoelectronic with N2)

with two π and one σ-bonds.

Higher the bo nd order, shorter is the bond length  has the shortest bond length (BO = 3).
Bond order of remaining species are

Isoelectronic species have same number of electron,   and N₂ all have 14 electrons.

CN^- and NO⁺ both have same number of electrons and same bond order (3)

The correct option   This species has 18 electrons, which are filled in such a way that all molecular orbitals are fully filled, so diamagnetic.

Electron is taken away from non-bonding molecular orbital, thats why bond order increases.

Since, H - bond is the electrostatic force of attraction between H -atom and electronegative element. Thus, fluorine being the most electronegative element forms stronger H -bonds. On the other hand, H-—F possesses larger electronegative difference than O—H.
Therefore, H - F molecule is more polarised than O—H, due to which H -atom of H—F bears larger amount of partial charge than that of O—H. This suggests H - atom of H—F attracts more strongly F -atom than that of O—H.
Hence, H—F forms more stronger H - bonds with fluorine than that of O—H.

SF₄ has trigonal bipyramidal geometry, lone pair of electrons repels the axial bond pair and decreases the bond angle to 173°,

As the electronegativity of central atom increases, bonded electron polarise towards central atom more, so repulsion increases and bond angle increases.

Molecular orbital configuration of given molecules are
  (Total number of electrons = 18)




Thus, does not contain any unpaired electron.

Greater the charge and smaller the radius, larger the polarising power and thus, greater the covalent nature. This leads to increase in lattice energy.

A species is said to be diamagnetic, if it has ail paired electrons.

sp³d² hybridisation has octahedral structure such that four hybrid orbitals are at 90° wrt each other and others two at 90° with first four.

Tetrahedral structure is associated with sp³ hybridised central atom without any lone pair. The structure of all the compounds given are as follows

Boron has three bonds thus sp2 hybridised. Each oxygen has two lone pairs hence sp³ hybridised.

Bond length is inversely proportional to bond order. Bond order in NO⁺ = 3 and NO = 2.5.
Thus, bond length in NO > NO⁺

XeF₂ contains sp³d hybridised Xe atom with three lone pairs of electrons. Fluorine atoms occupy axial positions while three lone pairs of elelctrons occupy equatorial positions in trigonal bipyramid to minimise repulsion.
Since, lone pair of electrons do not considered for the shape of the molecule, thus, shape of XeF₂ comes out to be linear. While C- atom of CO₂ is sp hybridised and thus, possesses a linear shap.