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The D-And-f-Block Elements

Question
CBSEENCH12010621
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The pair in which phosphorous atoms have a formal oxidation state of +3 is:

  • Pyrophosphorous and hypophosphoric acids

  • Orthophosphorous and hypophosphoric acids

  • Pyrophosphorous and pyrophosphoric acids

  • Orthophosphorous and pyrophosphorous acids

Solution

D.

Orthophosphorous and pyrophosphorous acids

Orthophosphorous H3PO4

H3PxO3 = 3 +x + 3(-2) = 0 x = +3

pyrophosphorous acids H4P2O6


H4P2xO5 = 4 + 2x + 5 (-2) = 0
4 + 2x -10 = 0
x = +3

Some More Questions From The d-And-f-Block Elements Chapter

In the series Sc (Z = 21) to Zn(Z = 30), the enthalpy of atomisation of zinc is the lowest i.e., 26, kJ mol. Why?

The E° (M2+/M) value for copper is positive (+ 0.34 V). What is possibility the reason for this? 

How would you account for the irregular variation of ionisation enthalpies (first and second) in the first series of the transition elements?

Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?

Which is a stronger reducing agent Cr2+ or Fe2+ and why?

Explain why Cu+ ion is not stable in aqueous solutions?

Actinoid contraction is greater from element to element than lanthanoid contraction. Why?

On what ground can you say that scandium (Z = 21) is a transition element but zinc (Z = 30) is not?

The outer electronic configuration of copper is 3d10 4s1, yet it is considered transition element. Why?

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