Single Choice

Which of the following pairs of compounds is isoelectronic and isostructural?

A$$IF_{3}, XeF_{2}$$
B$$BeCl_{2}, XeF_{2}$$
C$$TeI_{2}, XeF_{2}$$
D$$I{Br}_{2}^{-}, XeF_{2}$$
Correct Answer

Solution

The compounds $$\displaystyle I{Br}_{2}^{-}$$ and $$XeF_{2}$$ are isostructural. Both have the same number of valence electrons. Both have linear geometry as they have 3 lone pairs and 2 bond pairs of electrons. Electron pair geometry is trigonal bipyramidal and molecular geometry is linear.

Note: Isoelectronic compounds have the same number of electrons. This includes core electrons and valence electrons.

SIMILAR QUESTIONS

p - block Elements

The hybridization of Chlorine atom in $$ClF_{3}$$ molecule is:

p - block Elements

The shape of $$ClF_{3}$$ molecule is:

p - block Elements

The hybridization of iodine in $$\mathrm{IF}_{5}$$ is :

p - block Elements

Shapes of certain interhalogen compounds are stated below. Which one of them is not correctly stated?

p - block Elements

Match the interhalogen compounds of column I with the geometry in column II and assign the correct code. Column I Column II (a) $$XX'$$ (i) T-shape (b) $$XX_{3}'$$ (ii) Pentagonal bipyramidal (c) $$XX_{5}'$$ (iii) Linear (d) $$XX_{7}'$$ (iv) Square - pyramidal (v) Tetrahedral

p - block Elements

Answer the following question: $$ClF_{3}$$ exists but $$FCl_{3}$$ does not. Explain.

p - block Elements

Which bond do you expect to be stronger in each of the following cases and why ? (i) $$H - H, Cl - Cl$$ (ii) $$O_{2}, N_{2}$$ (iii) $$F - F, Cl - Cl$$

p - block Elements

Out of $$P-F, F-F, S-F$$ and $$Cl-F$$ bonds, which bond is the least ionic ?

p - block Elements

In which of the following molecules, central atom involve expansion of octet?

p - block Elements

The species which is not tetrahedral in structure :

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