1. Structure of Solids Chapter 7

11. Metallic Bonding In a metal, the outer electrons are shared among all the atoms in the solid. Each atom gives up its outer electrons and becomes slightly positively charged. The negatively charged electrons hold the metal atoms together. Since the electrons are free to move, they lead to good thermal and electrical conductivity. The phrase used is: “a lattice of positive ions in a sea of negative electrons”

16. elements non-metals molecular structure metallic structure atoms positive ions in small numbers of atoms in large numbers of atoms have do not conduct electricity form are joined together by covalent bonds ionic structure giant covalent structure have diamond, silicon dioxide, graphite have H 2 , C l 2 , I 2 , H 2 O, CO 2 , CH 4 conduct electricity metals are joined together by metallic bonds in large numbers of atoms Na, Cu, Fe, A l , Mg consist of consist of negative ions form NaC l , MgC l 2 , MgO have loss of electrons gain of electrons ionic bonds in large numbers of ions are joined together by consist of contains