Metallic bond properties - PowerPoint PPT Presentation
Metallic Bond
Metallic Bond. IB. Formation of metallic bond. the metal atoms "lose" one or more of their outer electrons These electrons become delocalized, and free to move throughout the entire metal. These negative delocalized electrons hold the metal cations together strongly.
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Metallic Bonding
Metallic Bonding. Metallic Bonds. The bonding in metals is explained by the electron sea model , which proposes that the atoms in a metallic solid contribute their valence electrons to form a “sea” of electrons that surrounds metallic cations. . Metallic Bonds.
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Metallic bond properties High melting and boiling points
Metallic bond properties High melting and boiling points To cause metals to melt, enough energy has to be added to overpower the sea of electrons which holds the island of cations together and allow them to move. Malleable and ductile
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Metallic Bonding
Metallic Bonding. Metal Ions and Electrons. Metals lose their valence electrons and become cations “Loose” valence electrons form a “sea of electrons” Loose electrons are “free to move”. Metals and Electrons. Metal bonds. Metallic Bond Properties. Strength Malleability Ductility
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Metallic Bond
Metallic Bond. IB. The Periodic Table of Elements. Periodic Table. Formation of metallic bond. the metal atoms "lose" one or more of their outer electrons These electrons become delocalized, and free to move throughout the entire metal.
METALLIC BOND
METALLIC BOND. Metals tend to have high melting points and boiling points suggesting strong bonds between the atoms. Even a metal like sodium (melting point 97.8°C) melts at a considerably higher temperature than the element (neon) which precedes it in the Periodic Table. METALLIC BOND.
Metallic Bond
Metallic Bond. IB. Formation of metallic bond. the metal atoms "lose" one or more of their outer electrons These electrons become delocalized, and free to move throughout the entire metal. These negative delocalized electrons hold the metal cations together strongly.
Metallic Bond
Metallic Bond. Chapter 15. Metallic Bonds. Holds metals together by sharing the electrons (sea of electrons) VERY STRONG. Metallic Bonds. How atoms are held together in the solid. Metals hold onto their valence electrons very weakly.
The Metallic bond
The Metallic bond. Cu 1+ Cu 1+ Cu 1+ Cu 1+. Cu • Cu • Cu • Cu •. Cu • Cu • Cu • Cu •. Cu 1+ Cu 1+ Cu 1+ Cu 1+. Cu • Cu • Cu • Cu •. Cu 1+ Cu 1+ Cu 1+ Cu 1+. The Metallic bond.
Metallic bond properties High melting and boiling points
Metallic bond properties High melting and boiling points To cause metals to melt, enough energy has to be added to overpower the sea of electrons which holds the island of cations together and allow them to move. Malleable and ductile
Bond Properties
Bond Properties. What is the effect of bonding and structure on molecular properties ?. Buckyball in HIV-protease. Double bond. Single bond. Triple bond. Bond Order # of bonds between a pair of atoms. Acrylonitrile. Bond Order.
Metallic Bonds and Bond Energy
Metallic Bonds and Bond Energy. Metallic Bond. Bond that exists between metal atoms Alloy – two or more different metal atoms bonded together. Electron Sea Model. Metal atoms give up valence electrons and form + ions The released electrons move freely around the + metal ions.
Metallic Bonds and Properties
Metallic Bonds and Properties. Metallic Bonds. is a chemical bond resulting from the attraction between positive ions and surrounding mobile e-. Metallic bonds- electrons are free to move throughout the material. Metals. Hybridization -The Blending of Orbitals.