Section 2.5 Atomic Bonding

Transcription

1 Section 2.5 Atomic Bonding Metallic bond, Covalent bond, Ionic bond, van der Waals bond are the different types of bonds. Van der Waals interactions: London forces, Debye interaction, Keesom interaction Glass temperature is a temperature above which many polymers and inorganic glasses no longer behave as brittle materials Ductility refers to the ability of materials to be stretched or bent without breaking Intermetallic compound is a compound such as Al 3 V formed by two or more metallic atoms 23

2 Figure 2.9 The metallic bond forms when atoms give up their valence electrons, which then form an electron sea. The positively charged atom cores are bonded by mutual attraction to the negatively charged electrons 24

3 When voltage is applied to a metal, the electrons in the electron sea can easily move and carry a current 25

4 Figure 2.10 Covalent bonding requires that electrons be shared between atoms in such a way that each atom has its outer sp orbital filled. In silicon, with a valence of four, four covalent bonds must be formed 26

5 Figure 2.10 Covalent bonds are directional. In silicon, a tetrahedral structure is formed, with angles of required between each covalent bond 27

6 Example 2.3 How Do Oxygen and Silicon Atoms Join to Form Silica? Assuming that silica (SiO 2 ) has 100% covalent bonding, describe how oxygen and silicon atoms in silica (SiO 2 ) are joined. SOLUTION Silicon has a valence of four and shares electrons with four oxygen atoms, thus giving a total of eight electrons for each silicon atom. However, oxygen has a valence of six and shares electrons with two silicon atoms, giving oxygen a total of eight electrons. Figure 2-11 illustrates one of the possible structures.similar to silicon (Si), a tetrahedral structure also is produced. We will discuss later in this chapter how to account for the ionic and covalent nature of bonding in silica. 28

7 Figure 2.11 The tetrahedral structure of silica (Si0 2 ), which contains covalent bonds between silicon and oxygen atoms (for Example 2-6) 29

8 Figure 2.12 An ionic bond is created between two unlike atoms with different electronegativities. When sodium donates its valence electron to chlorine, each becomes an ion; attraction occurs, and the ionic bond is formed 30

9 When voltage is applied to an ionic material, entire ions must move to cause a current to flow. Ion movement is slow and the electrical conductivity is poor 31

10 Figure 2.13 Illustration of London forces, a type of a van der Waals force, between atoms 32

11 2003 Brooks/Cole Publishing / Thomson Learning Figure 2.14 The Keesom interactions are formed as a result of polarization of molecules or groups of atoms. In water, electrons in the oxygen tend to concentrate away from the hydrogen. The resulting charge difference permits the molecule to be weakly bonded to other water molecules 33

12 Figure 2.15 (a) In polyvinyl chloride (PVC), the chlorine atoms attached to the polymer chain have a negative charge and the hydrogen atoms are positively charged. The chains are weakly bonded by van der Waals bonds. This additional bonding makes PVC stiffer, (b) When a force is applied to the polymer, the van der Waals bonds are broken and the chains slide past one another 2003 Brooks/Cole Publishing / Thomson Learning 34

13 Section 2.6 Binding Energy and Interatomic Spacing Interatomic spacing is the equilibrium spacing between the centers of two atoms. Binding energy is the energy required to separate two atoms from their equilibrium spacing to an infinite distance apart. Modulus of elasticity is the slope of the stress-strain curve in the elastic region (E). Yield strength is the level of stress above which a material begins to show permanent deformation. Coefficient of thermal expansion (CTE) is the amount by which a material changes its dimensions when the temperature changes. 35

14 Figure 2.16 Atoms or ions are separated by an equilibrium spacing that corresponds to the minimum inter-atomic energy for a pair of atoms or ions (or when zero force is acting to repel or attract the atoms or ions) 2003 Brooks/Cole Publishing / Thomson Learning 36

15 Table 2.2 Binding energies for the four bonding mechanisms 37

16 Figure 2.17 The force-distance curve for two materials, showing the relationship between atomic bonding and the modulus of elasticity, a steep dflda slope gives a high modulus 38

17 2003 Brooks/Cole Publishing / Thomson Learning Figure 2.25 The inter-atomic energy (IAE)-separation curve for two atoms. Materials that display a steep curve with a deep trough have low linear coefficients of thermal expansion 39