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Ebook Chemistry (10th edition): Part 2

(BQ) Part 2 book "Chemistry" has contents: Intermolecular forces and liquids and solids, physical properties of solutions, chemical kinetics, chemical equilibrium, acids and bases, acid base equilibria and solubility equilibria, chemistry in the atmosphere,. and other contents. | Intermolecular Forces and Liquids and Solids Under atmospheric conditions, solid carbon dioxide (dry ice) does not melt; it only sublimes. The models show a unit cell of carbon dioxide (face-centered cubic cell) and gaseous carbon dioxide molecules. Chapter Outline A Look Ahead Types of Crystals Next, we examine the different types of intermolecular forces between molecules and between ions and molecules. We also study a special type of intermolecular interaction called hydrogen bonding that involves hydrogen and electronegative elements nitrogen, oxygen, and fluorine. (11.2) • We see that two important properties of liquids—surface tension and viscosity— can be understood in terms of intermolecular forces. (11.3) • We then move on to the world of solids and learn about the nature of crystals and ways of packing spheres to form different unit cells. (11.4) • We see that the best way to determine the dimensions of a crystal structure is by X-ray diffraction, which is based on the scattering of X rays by the atoms or molecules in a crystal. (11.5) • The major types of crystals are ionic, covalent, molecular, and metallic. Intermolecular forces help us understand their structure and physical properties such as density, melting point, and electrical conductivity. (11.6) We learn that solids can also exist in the amorphous form, which lacks orderly three-dimensional arrangement. A well-known example of an amorphous solid is glass. (11.7) We next study phase changes, or transitions among gas, liquids, and solids. We see that the dynamic equilibrium between liquid and vapor gives rise to equilibrium vapor pressure. The energy required for vaporization depends on the strength of intermolecular forces. We also learn that every substance has a critical temperature above which its vapor form cannot be liquefied. We then examine liquid-solid and solid-vapor transitions. (11.8) The various types of phase transitions are summarized in a phase diagram, which helps .