2. Bonding

Electronegativity — Quiz

Test your understanding of electronegativity with 5 practice questions.

Practice Questions

Question 1

Using Pauling’s empirical formula for percent ionic character $\%IC = \bigl(1-\exp[-0.25(\Delta EN)^2]\bigr)\times100\%$, calculate the approximate ionic character of the H–Cl bond given EN(H)=2.20 and EN(Cl)=3.16.

Question 2

Calculate the bond dipole moment $\mu$ (in Debye) for HCl given partial charge $\delta=0.20\,e$ and bond length $d=1.27\,\mathrm{\AA}$. Use $e=1.602\times10^{-19}\,\mathrm C$ and $1\,\mathrm D=3.336\times10^{-30}\,\mathrm{C\cdot m}$.

Question 3

Why does carbon dioxide ($\mathrm{CO_2}$) exhibit no net dipole moment despite having polar C–O bonds?

Question 4

Between acetone ($\mathrm{(CH_3)_2CO}$) and acetyl chloride ($\mathrm{CH_3COCl}$), which has a more polar carbonyl group and is thus more susceptible to nucleophilic attack?

Question 5

Given the bonds C–H, C–Br, C–Cl, and C–F with EN(H)=2.20, EN(Br)=2.96, EN(Cl)=3.16, and EN(F)=3.98, arrange them in order of decreasing bond polarity.