Determine which molecule in each pair has the stronger intermolecular forces. Explain why. The main reason that NH3 has [ Select ] intermolecular forces than CH4 is that NH3 [ Select ] . The main reason that NO2 has [ Select ] intermolecular forces than CO2 is that NO2 [ Select ] . The main reason that CS2 has [ Select ] intermolecular forces than CO2 is that CS2 [ Select ] .

As for NH3 and CH4, the former is a polar molecule and possess a dipole. Hence, in addition to dispersion forces, dipole-dipole interaction as well as hydrogen bonding creates a stronger intermolecular interaction than in nonpolar CH4 where only dispersion forces are in operation.

Between NO2 and CO2, the former possesses a dipole moment while the later does not. As a result of that, dipole interaction are in operation in NO2 while only dispersion forces are n operation in CO2.

Between CO2 and CS2, the both molecules are nonpolar but CS2 has a greater molecular mass than CO2. Recall that the greater the molecular mass of a substance the greater its magnitude of intermolecular forces.

CintiaSalazar CintiaSalazar · Answer 2 · 2025-04-11T11:03:31-04:00

Taking into account the intermolecular forces, you get that:

The main reason that NH₃ has weaker intermolecular forces than CH₄ is that NH₃, being nonpolar, possesses London Dispersion Forces, while CH₄ possesses the Hydrogen Bonding forces.
The main reason that NO₂ has the same intermolecular forces than CO₂ is that in NO₂ and CO₂ there are London forces because they are nonpolar molecules.
The main reason that CS₂ has the same intermolecular forces than CO₂ is that CS₂ in CS₂ and CO₂ there are London forces because they are nonpolar molecules.

Intermolecular forces or bonds are those interactions that hold molecules together. These are electrostatic forces.

Van der Waals forces are weak attractions that hold electrically neutral molecules together. At some point these molecules present an induced dipole, that is, the molecule acquires a partially positive and a partially negative charge momentarily, causing them to attract each other. They are Van de Waals forces: Dipole - Dipole Forces, London Forces, Ion - Dipole Forces.

London Dispersion Forces: occurs between nonpolar molecules due to the movement of electrons. At some point there are more electrons to one side, which, being close to another atom or molecule, the electrons of the second are repelled, originating two instantaneous dipoles, which originate an attractive force. In summary, this type of force occurs because when two molecules approach, a distortion of the electronic clouds of both is originated, generating in them, transient induced dipoles, due to the movement of the electrons, thus allowing them to interact with each other. They are very weak forces.
Ion-ion forces: It is the attraction between two ions of different charges: cations (positively charged ion) and anions (negatively charged ion). That is, it occurs between different charged molecules that will tend to form an electrostatic bond between the ends of opposite charges due to the attraction between them.
Ion-dipole forces: these are forces of attraction between an ion (an atom that has lost or gained an electron, so it has a charge) and a polar molecule. A molecule is a dipole when there is an asymmetric distribution of electrons because the molecule is made up of atoms of different electronegativity. The ion then binds to the part of the molecule that has its opposite charge: the positive end of the polar molecule is oriented towards the anion (negatively charged ion) and the negative end of the polar molecule is oriented towards the cation ( positively charged ion).
Dipole-dipole forces: dipole-dipole forces are forces of attraction between polar molecules. These molecules attract when the positive end of one of them is close to the negative of the other.
Hydrogen bonds: they are a type of dipole-dipole force. In this interaction, a molecule that presents hydrogen interacts with another that presents an atom with high electronegativity, such as oxygen, fluorine or nitrogen (O, F, N). In this way, between the hydrogen, which has a low electronegativity and the electronegative atom, an interaction is established, due to their opposite charges.

The relative order of magnitude of the intermolecular forces is:

Ion-ion forces> Ion-dipole forces> Hydrogen bonds> Dipole-dipole forces> London Dispersion Forces

Taking into account all the above, it can be said that:

The main reason that NH₃ has weaker intermolecular forces than CH₄ is that NH₃, being nonpolar, possesses London Dispersion Forces, while CH₄ possesses the Hydrogen Bonding forces.
The main reason that NO₂ has the same intermolecular forces than CO₂ is that in NO₂ and CO₂ there are London forces because they are nonpolar molecules.
The main reason that CS₂ has the same intermolecular forces than CO₂ is that CS₂ in CS₂ and CO₂ there are London forces because they are nonpolar molecules.

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