√ Definition of Van Der Waals Force and its Types (Full Discussion)
Understanding the Van Der Waals Force and its Types (Full Discussion) - This time aroundknowledge.co.id will discuss about what is the law or Van Der Waals Force. Before discussing in more detail and specifically about this van der Waals force, we already know that there are many the types of chemical bonds that can affect the chemical and physical properties of a material that contains a substance chemistry. One of them that will be discussed is the Van Der Waals Force. Then what is the meaning of the van der Waals force?
Understanding the Van Der Waals Force and its Types (Full Discussion)
Let's discuss van der Waals forces carefully here.
Definition of Van Der Waals Force
There is also a definition of van der Waals force is the amount of force that attracts or repels between molecules or between the inside the same molecule other than those caused by covalent bonds or ion electrostatic interactions with molecules that are neutral or have payload. There are several terms commonly used in van der Waals forces, namely:
- The force between two permanent dipole.
- The force between a permanent dipole and an induced dipole.
- The force between two temporary induced dipole.
The van der Waals force was first developed by scientists from the Netherlands namely, Johannes Diderik Van der Waals. These van der Waals forces are classified as attractive and repulsive forces between atoms, molecules and surfaces as well as between other molecules. The existence of this van der Waals force occurs between the same or different particles. This force also occurs due to the polarity of the particles. The smaller the polarity, the smaller the van der Waals force. The polarity of the particles is either permanent or not permanent. Particle copolarity can be permanent or non-permanent. Permanent polarity occurs due to the polarity of the bonds in the molecule. Meanwhile, the non-permanent polarity is caused by being induced by charged particles, so that the molecule is spontaneously polar for a moment.
Types of Van Der Waals Forces
In essence, van der Waals forces are the weakest intermolecular forces and consist of dipole-dipole forces and dispersion forces. The following describes the two styles.
1. Dipole-dipole force
Dipole-dipole forces are the attractive forces that occur between polar molecules. A hydrogen chloride molecule has partially positive hydrogen atoms and partially negative chlorine atoms. In a collection of many hydrogen chloride molecules, they will align themselves so that the oppositely charged regions of the neighboring molecules are close to one another. Dipole-dipole forces in nature are similar in shape to, but much weaker than, ionic bonds.
2. London Dispersion Force
Dispersion forces are also considered to be of the van der Waals type and are the weakest of all intermolecular forces. They are often referred to as London style after Fritz London (1900-1954), first proposed their existence in the 1930s. London dispersion forces are intermolecular forces that occur between atoms and between nonpolar molecules due to the motion of electrons. Then an electron cloud is formed. The electron cloud of a helium atom contains two electrons, which are normally expected to be spatially distributed around the nucleus. However, at certain times the distribution of electrons may be uneven, resulting in a momentary dipole. This weak and temporary dipole can then affect neighboring helium atoms through electrostatic attraction and repulsion. This will induce a dipole of the nearest helium atom. The dipole moments will then be weakly induced, then attracted to each other. The dispersion forces increase as the number of electrons in a nonpolar atom or molecule increases. The halogen group itself consists of four elements which all take the form of nonpolar diatomic molecules.
The dispersion forces are strong enough for the iodine molecule to have a large number of electrons. These forces are relatively strong and result in the high melting and boiling points of the halogen groups. The force is strong enough to hold the iodine molecules close together in the solid state at room temperature. The dispersion forces are progressively weaker for bromine, chlorine, and fluorine and this is illustrated in their lower melting and boiling points.
Thus, it can be concluded that this van der Waals force is a weak interaction between molecules involving dipole. Then polar molecules have permanent dipole-dipole interactions. And then non-polar molecules can interact by means of london dispersion forces.
Thus our discussion of Understanding the Van Der Waals Force and its Types (Full Discussion), I hope this article is useful for all of us. Thank You.
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