Which type of intermolecular force is

Cl2
MgF2
NH3
Are they dipole-dipole, dispersion,hydrogen bonding and/or ionic?

ionic

MgF2 is ionic

To determine the types of intermolecular forces present in each compound, we need to analyze their molecular structures and properties. Here's how you can identify the intermolecular forces for each compound:

1. Cl2 (Chlorine gas):
Chlorine gas consists of chlorine molecules (Cl2), where two chlorine atoms are covalently bonded to each other. Since chlorine is a nonpolar molecule, the only intermolecular force present in Cl2 is dispersion or London dispersion forces. These forces occur due to temporary fluctuations in the electron distribution, creating temporary dipoles that induce other temporary dipoles.

2. MgF2 (Magnesium fluoride):
MgF2 is an ionic compound composed of magnesium cations (Mg2+) and fluoride anions (F-). Ionic compounds involve the transfer of electrons between atoms, resulting in the formation of positively and negatively charged ions. Due to the strong electrostatic attraction between the positive and negative charges, there are ionic interactions between Mg2+ and F-. Therefore, the dominant intermolecular force in MgF2 is ionic bonding.

3. NH3 (Ammonia):
In ammonia (NH3), there is a polar covalent bond between the nitrogen (N) atom and the three hydrogen (H) atoms. Additionally, as a result of the lone pair of electrons on the nitrogen atom, ammonia molecules can interact through dipole-dipole forces. These dipole-dipole forces occur between the positively charged hydrogen atoms of one molecule and the negatively charged nitrogen atoms of adjacent molecules.

So, to summarize:
- Cl2 exhibits dispersion forces.
- MgF2 exhibits ionic bonding.
- NH3 exhibits dipole-dipole forces.

Remember that hydrogen bonding is a special type of dipole-dipole force that specifically occurs when hydrogen is bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine). In this case, NH3 does not exhibit hydrogen bonding as it does not contain hydrogen bonded to a highly electronegative atom.

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