Metallic Bonding PDF

Science & Health GRADE 9  WORK PLAN Attendance/Update Science Routines Review (Ionic and Covalent Bonding) Discussion (Metallic Bonding) Wrap up/ Agreement/Reminders  Chemical Bonding Metallic Crystals  Metallic Bonding Pure metals are crystalline solids, but...

Science & Health GRADE 9  WORK PLAN Attendance/Update Science Routines Review (Ionic and Covalent Bonding) Discussion (Metallic Bonding) Wrap up/ Agreement/Reminders  Chemical Bonding Metallic Crystals  Metallic Bonding Pure metals are crystalline solids, but unlike ionic compounds, every point in the crystal lattice is occupied by an identical atom. https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/section/8.10/primary/lesson/metallic-bonding-chem Metallic Bonding The electrons in the outer energy levels of a metal are mobile and capable of drifting from one metal atom to another. Metal is viewed as an array of positive ions surrounded by a sea of mobile valence electrons called delocalized electrons. https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/section/8.10/primary/lesson/metallic-bonding-chem  Metallic Bonding A metallic bond is the attraction of the stationary metal cations to the surrounding mobile electrons. https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/section/8.10/primary/lesson/metallic-bonding-chem Metallic Bonding Metallic Bonding In a metal, the stationary metal cations are surrounded by a sea of mobile valence electrons that are not associated with any one cation. https://www.youtube.com/watch?time_continue=3&v=eVv3TpaQ2-A&feature=emb_logo Properties of Metals Metals conduct electricity and heat very well because of their free-flowing electrons. As electrons enter one end of a piece of metal, an equal number of electrons flow outward from the other end. https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/section/8.10/primary/lesson/metallic-bonding-chem Properties of Metals The American Platinum Eagle is the official platinum bullion coin of the United States and was first minted in 1997. The luster of a metal is due to its metallic bonds. When light is shone on to the surface of a metal, its electrons absorb small amounts of energy and become excited into one of its many empty orbitals. The electrons immediately fall back down to lower energy levels and emit light. This process is responsible for the high luster of metals. https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/section/8.10/primary/lesson/metallic-bonding-chem Properties of Metals When a force is applied to a metal, the free-flowing electrons can slip in between the stationary cations and prevent them from coming in contact. Imagine ball bearings that have been coated with oil sliding past one another. https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/section/8.10/primary/lesson/metallic-bonding-chem Properties of Metals As a result, metals are very malleable and ductile. They can be hammered into shapes, rolled into thin sheets, or pulled into thin wires. https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/section/8.10/primary/lesson/metallic-bonding-chem Metallic Bonding The metallic bond is responsible for the properties of metals. Metals conduct electricity and heat well. Metals are ductile and malleable. Metals have luster.