Properties and Bonds of NF3

The video tutorial explores the intermolecular forces in nitrogen trifluoride (NF3). It begins by confirming the absence of ions due to the covalent bonds between nitrogen and fluorine. The video then examines the polarity of NF3, highlighting the significant electronegativity difference and the molecular geometry that results in a polar molecule. Finally, it identifies the intermolecular forces present in NF3, which include dipole-dipole interactions and London dispersion forces.

What type of bonds are present in NF3?

• Ionic bonds

• Hydrogen bonds

• Covalent bonds

• Metallic bonds

Why are there no ions present in NF3?

• Because it is a polar molecule

• Because it contains hydrogen atoms

• Because it is composed of non-metals forming covalent bonds

• Because it is a metallic compound

Why is NF3 considered a polar molecule?

• Because of the difference in electronegativity between nitrogen and fluorine

• Because it contains hydrogen atoms

• Due to the presence of ions

• Because it has a symmetrical shape

What is the electronegativity of fluorine in NF3?

• 4.04

• 2.98

• 3.04

• 3.98

What is the molecular geometry of NF3?

• Linear

• Trigonal planar

• Tetrahedral

• Trigonal pyramidal

What role does the lone pair on nitrogen play in NF3's geometry?

• It has no effect on the molecular shape

• It causes the molecule to be non-polar

• It makes the molecule linear

• It pushes the fluorine atoms down, creating a trigonal pyramidal shape

Does NF3 exhibit hydrogen bonding?

• Yes, because it is a polar molecule

• No, because it lacks hydrogen atoms

• No, because it is non-polar

• Yes, because it contains hydrogen atoms

Which intermolecular forces are present in NF3?

• Only hydrogen bonds

• Only London dispersion forces

• Dipole-dipole and London dispersion forces

• Only dipole-dipole forces

What is the significance of London dispersion forces in NF3?

• They cause the molecule to be non-polar

• They are present alongside dipole-dipole forces

• They are stronger than dipole-dipole forces

• They are the only forces present