Bond polarity by electronegativity: Practice Questions

A covalent bond is considered non-polar when the electronegativity difference between the two bonded atoms is approximately:

In the molecule \(H_2O\) , which atom carries the partial positive charge? (Electronegativity: O \(\approx\) 3.44, H \(\approx\) 2.20)

Given the approximate Pauling electronegativity values: F (3.98) and Cl (3.16).

Which of the following statements about the polarity of chlorine trifluoride (\(ClF_3\)) is correct?

Given the approximate Pauling electronegativity values:
C (2.55), O (3.44), N (3.04), H (2.20), Cl (3.16), F (3.98).

Which of the following covalent bonds is considered a non-polar covalent bond?

Given the approximate Pauling electronegativity values: H (2.2), C (2.55), N (3.04), O (3.44), Cl (3.16).

Which of the following covalent bonds has the LEAST polarity?

a) Define electronegativity and explain how the difference in electronegativity between two bonded atoms leads to the formation of a polar covalent bond.

b) Consider the covalent bond between hydrogen (\(H\), electronegativity = 2.20) and oxygen (\(O\), electronegativity = 3.44) in a water molecule.

i) Determine the polarity of the \(H-O\) bond.

ii) Indicate the partial charges (\(\delta+\) and \(\delta-\)) on the hydrogen and oxygen atoms in the \(H-O\) bond.

(a) Define electronegativity and explain how a difference in electronegativity between two bonded atoms leads to the formation of a polar covalent bond.

(b) Consider the molecules hydrogen sulfide ($$H_2S$$) and methane ($$CH_4$$).

(i) Predict the molecular shape of each molecule using VSEPR theory.

(ii) Using the concept of bond polarity and molecular geometry, determine whether $$H_2S$$ and $$CH_4$$ are polar or non-polar molecules overall. (Approximate electronegativity values: H = 2.20, C = 2.55, S = 2.58)