Question 8 of 34beginner🔧 ApplyVery Short1 mark

Predict the number of unpaired electrons in the square planar [Pt(CN)4]2- ion.

Correct Answer

Zero (no unpaired electrons).

Exercise: Intext Questions | Q: 5.9 | (Page Page 18)
For More Understanding

Explanation

The textbook explicitly states in section 5.9 that for square planar shape, the hybridisation is dsp². In [Pt(CN)₄]²⁻, the unpaired electrons in the 5d orbital pair up to make one d orbital empty for dsp² hybridisation. Thus, there is no unpaired electron, making the complex diamagnetic. This is similar to [Ni(CN)₄]²⁻ mentioned in the context, which is also square planar with dsp² hybridisation and is diamagnetic due to the absence of unpaired electrons.

Solution Steps

  1. Step 1: Identify the geometry as square planar, which requires dsp² hybridisation.

  2. Step 2: For dsp² hybridisation, one d orbital must be empty.

  3. Step 3: The unpaired electrons in the 5d orbital pair up to create this empty d orbital.

  4. Step 4: Since all electrons are paired, the number of unpaired electrons is zero.

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