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A diatomic molecule has a dipole moment of 1.2 D. If its bond distance is equal to 2.0Å then the % of ionic character in the diatomic molecular is :
  • a)
    12.5% 
  • b)
    37% 
  • c)
    52% 
  • d)
    42% 
Correct answer is option 'A'. Can you explain this answer?
Verified Answer
A diatomic molecule has a dipole moment of 1.2 D. If its bond distance...
Assuming complete charge transfer then dipole moment = (4.8 x 10-10 esu) (10-8 cm) x 2 = 9.6 D
so % ionic character = 12.5% 
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Most Upvoted Answer
A diatomic molecule has a dipole moment of 1.2 D. If its bond distance...
Angstroms, what is the magnitude of the partial charge on each atom?

The dipole moment (μ) of a diatomic molecule is given by:

μ = q × d

where q is the magnitude of the partial charge on each atom and d is the bond distance.

We can rearrange this equation to solve for q:

q = μ / d

Plugging in the given values, we get:

q = 1.2 D / 2.0 Å

Converting D to C-m and Å to m, we get:

q = (1.2 × 10^-30 C-m) / (2.0 × 10^-10 m)

Simplifying, we get:

q = 6 × 10^-21 C

Since the diatomic molecule is neutral overall, each atom must have an equal but opposite partial charge of:

± 3 × 10^-21 C

Therefore, the magnitude of the partial charge on each atom is 3 × 10^-21 C.
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A diatomic molecule has a dipole moment of 1.2 D. If its bond distance is equal to 2.0Å then the % of ionic character in the diatomic molecular is :a)12.5%b)37%c)52%d)42%Correct answer is option 'A'. Can you explain this answer?
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