Questions: Which of the following substances would not exhibit any hydrogen bonding interactions in a pure substance? A H2O B HF C N(CH3)3 D CH3CH2OH E CH3NH2

Which of the following substances would not exhibit any hydrogen bonding interactions in a pure substance?

A H2O

B HF

C N(CH3)3

D CH3CH2OH

E CH3NH2

Transcript text: Which of the following substances would not exhibit any hydrogen bonding interactions in a pure substance? A $\mathrm{H}_{2} \mathrm{O}$ B HF C $\mathrm{N}\left(\mathrm{CH}_{3}\right)_{3}$ D $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}$ E $\mathrm{CH}_{3} \mathrm{NH}_{2}$

Solution

Solution Steps

Step 1: Identify the Electronegative Atoms

Hydrogen bonding typically occurs when hydrogen is bonded to highly electronegative atoms (N, O, F).

Step 2: Check for Hydrogen Atoms

Ensure that there are hydrogen atoms bonded to the identified electronegative atoms.

Step 3: Assess the Molecular Structure

Evaluate the molecular structure to determine if hydrogen bonding is feasible either within its own molecule (intramolecular) or with other molecules of the same kind (intermolecular).

Step 4: Consider the State of Matter

Substances capable of hydrogen bonding are more likely to be liquids or solids at room temperature due to increased intermolecular forces.

Step 5: Eliminate Compounds with Non-polar Bonds Only

Compounds consisting solely of non-polar bonds (e.g., CH4, CH3CH3) are unlikely to exhibit hydrogen bonding.

Step 6: Apply Knowledge of Common Hydrogen Bonding Substances

Use knowledge of well-known hydrogen bonding substances (e.g., H2O, NH3, HF) as a guide.