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Chemical Bonding and Molecular Structure

Long Answer Type

181. Discuss in brief the various types of hybridisation involving d-orbitals.

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182.

State and explain the geometric arrangements possible in sp³d and sp³d² hybridisation. Name the d-orbitals involved in these.

187 Views

183.

On the basis of hybridisation, explain the shape of phosphorus penta fluoride (PF₅).

932 Views

184.

Discuss the shape of:
$space left parenthesis straight i right parenthesis space PCl subscript 5 space space space left parenthesis ii right parenthesis space SF subscript 6$
on the basis of hybridization.

331 Views

185.

Which hybrid orbitals are used by carbon atoms in the following molecules ?

(a) CH₃ – CH₃(b) CH₃ – CH = CH₂(c) CH₃ – CH₂ - OH
(d) CH₃ - CHO
(e) CH₃COOH

516 Views

Short Answer Type

186.

Describe the change in hybridization (if any) of the Al atom in the following reaction:

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230 Views

187.

Is there any change in the hybridisation of B and N atoms as a result of the following reaction?
BF₃ + NH₃ → F₃B.NH₃?

680 Views

Long Answer Type

188.
What are non-polar and polar covalent bonds? Give examples.

(i) Non-polar covalent bond. If a covalent bond is formed between two identical atoms, the shared pair of electrons is attracted equally by both the atoms and lies exactly midway between them, such a bond is called a non-polar covalent bond. For example, in a molecule of H₂ or Cl₂, the shared pair of electrons is attracted equally between the two hydrogen atoms or chlorine atoms and hence the resulting bond is non-polar.

(ii) Polar covalent bond. If a covalent bond is formed between two dissimilar (non-identical) atoms having different electronegativities, the shared pair of electrons is pulled closer towards more electronegative atom, such a bond is called the polar covalent bond. The more electronegative atom acquires partial negative charge (δ–) while less electronegative atom acquires a partial positive charge (δ⁺). For example, hydrogen fluoride molecule has a polar covalent bond.