The video tutorial explores the intermolecular forces present in hydrogen cyanide (HCN). It begins by confirming that HCN is not an ionic compound and lacks ions. The tutorial then examines the polarity of HCN using its Lewis structure, highlighting the linear arrangement and electronegativity differences that make it polar. The video identifies the presence of dipole-dipole and London dispersion forces in HCN, noting the absence of hydrogen bonding due to the hydrogen atom being bonded to carbon. The tutorial concludes with a summary of the intermolecular forces in HCN.

What type of compound is HCN?

• Covalent

• Amphoteric

• Ionic

• Metallic

What is the shape of the HCN molecule?

• Bent

• Trigonal planar

• Linear

• Tetrahedral

Which atom in HCN has a partial negative charge due to electronegativity?

• Oxygen

• Nitrogen

• Carbon

• Hydrogen

Why doesn't HCN exhibit hydrogen bonding?

• Hydrogen is bonded to fluorine

• Hydrogen is bonded to nitrogen

• Hydrogen is bonded to oxygen

• Hydrogen is bonded to carbon

What type of intermolecular force is primarily present in HCN?

• Hydrogen bonding

• Ionic bonding

• Dipole-dipole forces

• Metallic bonding

Which of the following forces is also present in HCN besides dipole-dipole forces?

• Covalent bonding

• London dispersion forces

• Hydrogen bonding

• Ionic forces

What is the significance of the dipole in HCN?

• It is weaker than London dispersion forces

• It is the primary force between molecules

• It results in hydrogen bonding

• It causes the molecule to be non-polar

Which element in HCN is responsible for its polarity?

• Oxygen

• Nitrogen

• Carbon

• Hydrogen

What is the role of London dispersion forces in HCN?

• They are weaker than dipole-dipole forces

• They are absent in HCN

• They cause hydrogen bonding

• They are the strongest force

What is the overall conclusion about the intermolecular forces in HCN?

• Only ionic forces are present

• Both dipole-dipole and London dispersion forces are present

• Only metallic bonding is present

• Only hydrogen bonding is present