Ionic bonding intermolecular forces

There are five types of interactions within and between molecules. Intramolecular interactions include covalent and ionic bonds. Intermolecular interactions include van der Waals s forces, dipole-dipole, and hydrogen bonds. Table 1 lists the typical energies for these interactions. 

Bonding in Solids Atoms, molecules, or ions are held in a solid by (hflerent types of bonding. Electrostatic forces are responsible for ionic solids, intermolecular forces are responsible for molecular solids, covalent bonds are responsible for covalent solids, and a special type of interaction, which involves electrons being delocalized over the entire crystal, accounts for the existence of metals. 

What Do We Need to Know Already This chapter assumes that we are familiar with the concept of energy (Section A), stoichiometry (Sections L and M), and the ideal gas law (Chapter 4). Some of the explanations refer to intermolecular forces (Sections 4.12 and 5.1-5.5). Ionic bonding (Sections 2.3-2.4) and bond strengths (Sections 2.14-2.15) are developed further in this chapter. 

The effect of molecular interactions on the distribution coefficient of a solute has already been mentioned in Chapter 1. Molecular interactions are the direct effect of intermolecular forces between the solute and solvent molecules and the nature of these molecular forces will now be discussed in some detail. There are basically four types of molecular forces that can control the distribution coefficient of a solute between two phases. They are chemical forces, ionic forces, polar forces and dispersive forces. Hydrogen bonding is another type of molecular force that has been proposed, but for simplicity in this discussion, hydrogen bonding will be considered as the result of very strong polar forces. These four types of molecular forces that can occur between the solute and the two phases are those that the analyst must modify by choice of the phase system to achieve the necessary separation. Consequently, each type of molecular force enjoins some discussion. 

Covalent, metallic, and ionic bonds are very strong interactions. Some people consider these to be intermolecular forces. The following are weaker intermolecular forces. They appear in approximate order of decreasing strength. Even though weaker than bonds, they are nonetheless important. 

We can begin with any of the intermolecular forces other than London forces. It is usually easiest to begin with the normal bonds (covalent, ionic, and metallic). Bonds only occur in specific circumstances. For example, metallic bonds only occur in metals or metal alloys. The only metal or alloy in the seven substance fist is iron. For this reason, the strongest intermolecular force in iron is metallic bonding. 

Note Examples of intermolecular forces include covalent, ionic, van der Waals, and hydrogen bonds. 

You also learned about intermolecular forces in Organic 1. Intermolecular forces (forces between chemical species) are extremely important in explaining the interaction between molecules. Intermolecular forces that you saw in Organic 1 and see again in Organic II include dipole-dipole interactions, London, hydrogen bonding, and sometimes ionic interactions. 

Given the following intermolecular forces— hydrogen bonds, London dispersion forces, ionic interactions and dipole-dipole interactions—if arranged in order from the strongest to the weakest the order would be... 

Intermolecular forces are responsible for the condensed states of matter. The particles making up solids and liquids are held together by intermolecular forces, and these forces affect a number of the physical properties of matter in these two states. Intermolecular forces are quite a bit weaker than the covalent and ionic bonds discussed in Chapter 7. The latter requires several hundred to several thousand kilojoules per mole to break. The strength of intermolecular forces are a few to tens of kilojoules per... 

Because intermolecular forces are relatively weak, breaking them doesn t take that much energy. Unlike solids containing ionic bonds, covalently bonded solids tend to have low melting points. 

The dyeing procedure for paper can be described basically by two processes the penetration of the dye molecule into the capillary spaces of the cellulose and then its adsorption on the surface of the fiber. The bonding forces are due to the effects charge (ionic bonds), precipitation, and intermolecular forces. 

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