PPT-Metallic Bonding Strong forces of attraction are responsible for the high melting point

CA Standards Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds Metallic Bonding The chemical bonding that results from the attraction between metal . Metallic Bonding. Warm Up. What force holds two ions together in an ionic bond?. Agenda. (Covalent bonds). Metallic Bonds. Visual Analogies. Learning Target. Part 3. I can describe what creates an attraction between two atoms in an covalent . IB Topics 4 & 14. Text:. Ch 8 (all except sections 4,5 & 8). Ch 9.1 & 9.5. Ch 10.1-10.7. My Name is Bond. Chemical Bond. PART 5: Giant Covalent Structures, Metallic Bonding & Physical Properties. What . exactly is a bond? Depends…Ionic or Covalent. ? Polar?. NON-POLAR COVALENT=> equal . sharing. . of electron . pair. 0 < ∆EN < 0.4. POLAR COVALENT= unequal . sharing . CA Standards. Students know . the atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular forces are too weak to hold the atoms or molecules in a solid form.. Metals. Look at the Periodic Table…. 75% of elements are metals!. Metals. They can vary a lot…. General Properties of Metals. Dense. Malleable. Ductile. Good conductors of heat and electricity. Shiny Lustre. Strong forces of attraction are responsible for the high melting point of most metals.. CA Standards. Students know . atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds. . IB Topics 4 & 14. Text:. Ch 8 (all except sections 4,5 & 8). Ch 9.1 & 9.5. Ch 10.1-10.7. My Name is Bond. Chemical Bond. PART 5: Giant Covalent Structures, Metallic Bonding & Physical Properties. Describe the difference between the structures of diamond and graphite.. Explain the different properties of these versions of carbon.. Graphite. Diamond. Learning questions. What general properties do metals have?. 4.4.1: Describe the metallic bond as the electrostatic attraction between a lattice of positive ions and delocalized ions. . 4.4.2. : Explain the electrical conductivity and malleability of metals. . Text:. Ch 8 (all except sections 4,5 & 8). Ch 9.1 & 9.5. Ch 10.1-10.7. My Name is Bond. Chemical Bond. PART 4: . Intermolecular Forces. Intermolecular Forces. Dipole-Dipole . Hydrogen Bonding . the forces between (among) individual particles (atoms, ions, molecules); they are weak relative to . intramolecular. forces (i.e. covalent and ionic bonds within a compound). Intermolecular forces are increasingly significant in this order:. Day . 6. – Venn Diagram, . haber. Process. Metallic . Bonding, Properties of Substances reading, . Warm up. ON PAGE 23. What do ionic and covalent bonding have in common? What is different?. Time: . Metallic Bond – the force that holds metal atoms together. Metals do not form covalent bonds with one another because they do not have enough electrons in their outer shells to form stable octets.. Diamond. Covalent bonding. Usually gases or liquids. Covalent bonds in the molecule are strong but forces between molecules (intermolecular) are weak. Low melting and boiling points.. Due. to having w.