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Interações de Van der Waals
As interações de Van der Waal são atrações inespecíficas criadas quando um átomo se aproxima o suficiente de outro para perturbar os seus eletrões—ind…
Van der Waals interactions are weak intermolecular forces that arise from electrostatic interactions between atoms and molecules that are electrically neutral overall.
These interactions are broadly classified into three types: London dispersion forces, dipole–dipole forces, and dipole-induced dipole forces.
All molecules, even nonpolar ones, have temporary partial charges.
Due to the varying distribution of electrons, a higher electron density in one region of the electron cloud results in an instantaneous dipole or a temporary dipole.
This then causes another instantaneous dipole in the neighboring molecule. The domino effect of dipoles gives rise to weak intermolecular attractive forces, which exist between all molecules, whether polar or nonpolar.
These interactions between temporary dipoles are called London dispersion forces.
Dipoles in polar molecules like water electrostatically interact through dipole-dipole forces.
Dipole-induced dipole forces happen when a polar molecule, like water, disturbs the electronic arrangement of a non-polar molecule, like diatomic oxygen, and causes a dipole.
All these interactions are attractive when the atoms are close enough for their electron clouds to just contact. If the atoms get any closer, these forces become repulsive.
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Q1: What are the three main types of van der Waals interactions?
Van der Waals interactions are classified into London dispersion forces, dipole-dipole forces, and dipole-induced dipole forces. London dispersion forces occur between temporary dipoles in all molecules. Dipole-dipole forces involve electrostatic interactions between polar molecules like water. Dipole-induced dipole forces happen when a polar molecule disturbs the electron arrangement of a nonpolar molecule, creating an induced dipole.
Q2: How do London dispersion forces form between nonpolar molecules?
London dispersion forces arise from temporary, instantaneous dipoles created by uneven electron distribution. When electrons concentrate in one region of a molecule's electron cloud, they create a temporary dipole. This dipole induces a similar temporary dipole in neighboring molecules, producing weak attractive forces. These fluctuating dipoles exist between all molecules, whether polar or nonpolar.
Q3: Why are dipole-dipole forces stronger in polar molecules like water?
Polar molecules have permanent partial charges: a partial positive charge on one end and a partial negative charge on the other. In water, the electronegative oxygen atom bears the partial negative charge while hydrogen carries the partial positive charge. These permanent dipoles electrostatically attract each other, creating stronger intermolecular forces than temporary dipoles alone.
Q4: What happens to van der Waals forces when atoms get very close together?
Van der Waals interactions are attractive when atoms are close enough for their electron clouds to just contact. However, if atoms approach even closer, these forces become repulsive. This transition occurs because electron cloud overlap creates electrostatic repulsion that overcomes the attractive forces between the nuclei and electrons.
Q5: How do ion-dipole forces help dissolve ionic compounds in water?
Ion-dipole forces are electrostatic attractions between ions and polar molecules. When an ionic compound like KCl dissolves in water, ion-dipole forces attract the positive ends of water molecules to negative chloride ions and negative ends to positive potassium ions. These forces reduce the strong interionic bonds holding the solid together, allowing individual ions to disperse uniformly in solution.
Q6: Why do larger molecules exhibit stronger dispersion forces than smaller ones?
Larger and heavier atoms and molecules have more electrons distributed across greater electron clouds, creating more pronounced temporary dipoles. These larger temporary dipoles induce stronger dipoles in neighboring molecules, resulting in stronger electrostatic attractions. The increased electron mobility in larger molecules also allows for more frequent and intense fluctuating dipole interactions.
Q7: What factors determine the strength of ion-dipole interactions?
The strength of ion-dipole interactions is directly proportional to two factors: the charge magnitude on the ion and the magnitude of the dipole in the polar molecule. Ions with higher charges create stronger electrostatic fields that attract polar molecules more intensely. Similarly, polar molecules with larger dipole moments experience stronger attractions to ions.