Instructions: 1. Read through the compounds and the types of intermolecular forces present in each. 2. Research the molecular structures of each of the compounds. 1. CO₂ (Carbon Dioxide) 2. NH3 (Ammonia) 3. C6H12O6 (Glucose) 4. N₂ (Nitrogen) 5. KBr (Potassium Bromide) 6. HBr (Hydrogen bromide) 3. Explain in your own words why each compound experiences the intermolecular forces listed.

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Introduction to Intermolecular forces

Intermolecular forces refer to the forces between molecules that are strong enough to influence the physical properties of a substance. These forces are electrostatic in nature and can be either attractive or repulsive. The most common types of intermolecular forces are hydrogen bonding, London Dispersion Forces, and dipole-dipole interactions.
Hydrogen bonding occurs when a hydrogen atom, which is covalently bound to a more electronegative atom such as oxygen or nitrogen, forms an electrostatic interaction with another electronegative atom. London dispersion forces are the weakest intermolecular forces and are caused by instantaneous dipoles that are formed when electrons are unevenly distributed in molecules. Dipole-dipole interactions occur between two molecules that have permanent dipoles.