consider the following compound: h2s indicate which of the van der waals forces of attraction exist between…
consider the following compound: h2s indicate which of the van der waals forces of attraction exist between molecules of this substance. give complete reasoning for your answer, including shape, electronegativity difference, the types of bonds present and polarity
Answer
Explanation:
Step1: Determine molecular shape
The central sulfur atom in $H_2S$ has 2 bonding pairs and 2 lone - pairs. Using VSEPR theory, its shape is bent.
Step2: Calculate electronegativity difference
The electronegativity of $H$ is 2.2 and of $S$ is 2.58. The electronegativity difference $\Delta\chi=2.58 - 2.2=0.38$. Since $0<\Delta\chi<1.7$, the $H - S$ bonds are polar covalent.
Step3: Analyze polarity
Due to the bent shape and polar $H - S$ bonds, the $H_2S$ molecule is polar.
Step4: Identify Van der Waals forces
Polar molecules exhibit dipole - dipole forces. Also, all molecules have London dispersion forces. So, $H_2S$ has both London dispersion forces and dipole - dipole forces.
Answer:
London dispersion forces and dipole - dipole forces exist between $H_2S$ molecules.