The intermolecular forces, such as hydrogen bonds or van der Waals attractions, which draw one molecule to its neighbors, govern a substance's physical properties. Due to the relatively weak intermolecular forces of attraction, molecular substances typically take the form of gases, liquids, or low melting point solids.
<h3>How do the intermolecular forces affect physical properties?</h3>
The forces that bind two molecules together are known as intermolecular forces. Intermolecular forces have an impact on physical properties. Strong and weak forces both exist; the stronger the force, the more energy is needed to separate the molecules from one another. As intermolecular forces increase melting, boiling, and freezing points rise.
The following intermolecular forces are listed in order of strength:
- Van der Waals dispersion forces
- Van der Waals dipole-dipole interactions
- Hydrogen bonding
- Ionic bonds
It would take very little energy to separate two molecules if they are connected by van der Waals dispersion forces. On the other hand, it requires a lot more energy to separate two molecules that are joined together by ionic bonds.
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Answer:
2 LiOH + CO2 = Li2CO3 + H2O
Explanation:
Answer:
The answer is "Each student will get a glass of water and drop the bead into it but the beads float 0.6 g / cm3 and slip down to 1.2 g / cm3
".
Explanation:
One's masses would've been dissimilar, even though their width and concentrations were also equal. Whenever the type-A mass is m, then the type-B mass is 2 m. One should measure then, therefore.
Water has a 1g / cm^3 density. Although Type A is higher than air, Type B is much more compact. it means will float if they place it in water type-A where type-B sinks.
