Resonance in Action: Bond Length, Acidity & More!

The video tutorial explores the impact of resonance on chemical properties such as bond length, dipole moment, acidic strength, and basic strength. It highlights how resonance shortens the carbon-chlorine bond in vinyl chloride, leading to a specific dipole moment. The tutorial also compares the acidic strength of phenol and cyclohexanone, attributing phenol's higher acidity to resonance stabilization. Additionally, it contrasts the basicity of aniline and ammonia, explaining that resonance decreases aniline's basicity.

Why is the carbon-chlorine bond length in vinyl chloride shorter than in ethyl chloride?

• Due to the absence of resonance

• Due to the presence of a triple bond

• Because chlorine is a smaller atom

• Because of resonance giving it a double bond character

What causes the dipole moment in vinyl chloride?

• The presence of a single bond

• The presence of a triple bond

• The lone electron pair on chlorine in conjugation with the π bond

• The absence of a dipolar structure

Why is phenol more acidic than cyclohexanol?

• Due to the presence of a triple bond in phenol

• Because of resonance stabilization in phenoxide ion

• Because phenol has a higher molecular weight

• Due to the absence of resonance in phenol

What effect does resonance have on the basicity of aniline compared to ammonia?

• Resonance makes aniline a stronger base than ammonia

• Resonance has no effect on aniline's basicity

• Resonance decreases the basicity of aniline

• Resonance increases the basicity of aniline

Which of the following statements is true about ammonia's basicity?

• Ammonia is less basic due to resonance

• Ammonia is less basic because it has a double bond

• Ammonia is more basic because it lacks resonance

• Ammonia is more basic due to a triple bond