Questions: What kind of intermolecular forces act between a carbon tetrachloride molecule and a chlorine (Cl2) molecule? Note: If there is more than one type of intermolecular force that acts, be sure to list them all, with a comma between the name of each force.

What kind of intermolecular forces act between a carbon tetrachloride molecule and a chlorine (Cl2) molecule?

Note: If there is more than one type of intermolecular force that acts, be sure to list them all, with a comma between the name of each force.

Transcript text: What kind of intermolecular forces act between a carbon tetrachloride molecule and a chlorine (Cl_2) molecule? Note: If there is more than one type of intermolecular force that acts, be sure to list them all, with a comma between the name of each force.

Solution

Solution Steps

Step 1: Identify the Molecules Involved

We need to identify the types of molecules involved in the interaction. Here, we have a carbon tetrachloride (CCl\(_4\)) molecule and a chlorine (Cl\(_2\)) molecule.

Step 2: Determine the Nature of Each Molecule

Carbon tetrachloride (CCl\(_4\)) is a nonpolar molecule because it has a symmetrical tetrahedral shape, which causes the dipole moments to cancel out. Chlorine (Cl\(_2\)) is also a nonpolar molecule because it consists of two identical atoms sharing electrons equally.

Step 3: Identify Possible Intermolecular Forces

Since both CCl\(_4\) and Cl\(_2\) are nonpolar molecules, the primary intermolecular force acting between them will be London dispersion forces (also known as van der Waals forces). These forces arise due to temporary dipoles that occur when electron clouds fluctuate.

Final Answer

\(\boxed{\text{London dispersion forces}}\)

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