What is the strongest intermolecular force that occurs between carbon dioxide molecules?
A. London dispersion forces
B. Hydrogen bond
C. Covalent bond
D. Dipole-induced dipole attractions
I think the answer is D but I am not sure
I tend to believe A is the answer. CO2 has no dipole moment.
It is A!
The correct answer is A. London dispersion forces.
Carbon dioxide (CO2) molecules are nonpolar, meaning the distribution of charge in the molecule is even. Therefore, there are no permanent dipoles or hydrogen bonds present. Instead, carbon dioxide molecules experience London dispersion forces, which are temporary fluctuations in electron distribution that create temporary dipoles. These temporary dipoles induce other temporary dipoles in neighboring molecules, resulting in weak attractions between the molecules. Therefore, the strongest intermolecular force between carbon dioxide molecules is the London dispersion force.
To determine the strongest intermolecular force that occurs between carbon dioxide (CO2) molecules, let's analyze the options provided:
A. London dispersion forces: These forces occur due to temporary fluctuations in electron distribution, resulting in instantaneously induced dipoles. While present in all molecules to some extent, CO2 being a nonpolar molecule does not have a permanent dipole moment and thus does not experience significant London dispersion forces.
B. Hydrogen bond: Hydrogen bonding occurs when a hydrogen atom is directly bonded to highly electronegative elements like oxygen, nitrogen, or fluorine. Since CO2 does not have any hydrogen atoms bonded to these electronegative elements, hydrogen bonding is not present between CO2 molecules.
C. Covalent bond: Covalent bonds occur within molecules, not between molecules. Since we are considering the intermolecular forces between CO2 molecules, the covalent bond is not relevant in this context.
D. Dipole-induced dipole attractions: CO2 is a linear molecule with two oxygen atoms bonded to a carbon atom. The molecule is nonpolar due to its symmetry, resulting in no net dipole. However, CO2 can induce temporary dipoles in neighboring molecules through electron redistribution. These dipole-induced dipole attractions, also known as London dispersion forces, are the primary intermolecular forces acting between CO2 molecules.
Therefore, the correct answer is A. London dispersion forces.