Chemical Bonding and Molecular Structure

In this hybridisation, one '2s' and three '2p' orbitals present in the valence shell of the excited carbon atom get hybridised to give rise to four new orbitals of equivalent energies. Each sp³ hybrid orbital is an average of one '2s' orbital and three '2p' orbitals having one fourth 's' character and three fourth 'p' character. 

In this type of hybridisation one '2s' and one '2px' orbitals get hybridised to form two equivalent orbitals called 'sp' hybrid orbitals. The remaining 2py and 2pz do not take part in hybridisation. The two unhybridised orbitals are directed along the 'y' and 'z' axes while the two hybridised orbitals are directed towards the 'x' axis. This hybridisation is often known as diagonal hybridisation as the two hybridised orbitals are at 180o due to mutual repulsion of their electron clouds. Each hybrid orbital has equal 's' and 'p' character.

In this type of hybridisation one '2s' and two 'p' orbitals (2px and 2py) get hybridised to form three equivalent orbitals called 'sp2' hybrid orbitals. Each hybrid orbital has one third 's' character and two third 'p' character. The bond angle between the two hybridised orbital is 120. The unhybridised orbital (2pz) of carbon is oriented in a plane at right angles to the plane containing the three hybridised orbitals.

In the formation of ethylene, each carbon atom undergoes sp² hybridisation leaving 2p_z orbital unhybridised. One of the sp² hybridised orbital of one carbon atom overlaps axially with sp² hybridised orbital of the other carbon atom to form a stable sigma bond (C-C). The remaining two sp² hybrid orbitals of both carbon overlap axially with the half filled '1s' orbital of hydrogen atoms forming four C-H sigma bonds. The unhybridised orbital (2p_z) of one carbon atom overlaps sidewise with the similar orbital of the other carbon atom to form a weak pi bond. Thus, in ethylene all the six atoms containing the sigma bonds lie in one plane, while the pi bond is at a plane perpendicular to the plane, of the six atoms.

This option is correct because all molecules have all three types of bonds, i.e., electrovalent, covalent and coordinate bonds.

This option is correct because all molecules exceed the octet rule, and hence all are hypervalent molecules.

This option is correct because boron and beryllium forms electron deficient compounds, so B₂H₆, BeCl₂ and BCl₃ all are electron deficient molecules.

Correct Answer: Molecule

This option is wrong because the acetophenone are treated with chorine in absence of catalyst to form phenacyl chloride. These are harmless, powerful lachrymator or tear gas, which is used by police to disperse mob.

This option is correct because bezene is aromatic, cyclooctatetraene is non-aromatic and cyclopropenyl anion is anti-aromatic.

A water molecule consists of two hydrogen atoms covalently bonded to a single central oxygen atom, forming a bent molecular geometry.

Water molecules are held together by hydrogen bonds, which are strong dipole-dipole attractions between the hydrogen atom of one molecule and the oxygen atom of another. Covalent bonds exist within the molecule, but the intermolecular force is hydrogen bonding.

The bonding between a molecule of water and a molecule of methanol is called intermolecular bonding, and it is a type of hydrogen bonding.

This option is correct because 1, 3 and 4 species are isoelectronic having 10 electrons.

This option is correct because the Stannic Chloride Pentahydrate is used for mordant in dyeing under the name oxymuriate of tin or butter tin.