Bond Polarity and Partial Charges Worksheet

Question 1

Which bond shares its electron pair equally in the simple model?

1. H–H
2. H–Cl
3. H–O
4. H–F

Question 2

In H–F, F has greater electronegativity than H. Place δ+ and δ− on the atoms and explain.

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Question 3

What does a δ− symbol on an atom in a polar bond mean?

1. The atom has gained exactly one electron as a separate ion.
2. The atom has lost all its valence electrons.
3. The bond has greater electron density near that atom.
4. The nucleus has gained a neutron.

Question 4

Carbon dioxide has two polar C=O bonds, and the molecule is linear. Explain why the two bonds do not produce a permanent molecular dipole.

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Question 5

Which bond in the set has the greatest electronegativity difference?

1. H–N
2. H–Cl
3. H–O
4. H–F

Question 6

Calculate the electronegativity difference for H–O. Identify which atom carries δ−.

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Question 7

Which bond has the smallest electronegativity difference in the set?

1. H–N
2. H–Cl
3. H–O
4. H–F

Question 8

A display places δ− on H in H–Cl. Correct the label and use the supplied data to explain.

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