Metallic Bonding Flashcards
How strong is the attraction between a metal’s valence electron and it’s nucleus?
they are weakly attracted
How would you describe a metallic bond?
Positive ions/cations floating in a sea of electrons
What is a sea of electrons
the electrons are free to move throughout the solid
What do metals form?
Giant metallic lattices
What are the metallic lattices made of?
positive metals ions surrounded by a sea of delocalized electrons. the metal ions are attracted to the negative electrons
What are delocalized electrons?
electrons that are not associated with any single atom
What are some of the properties of metals?
Shiny,lustrous
Conductive
Able to bend/malleable
Ductile
High MP and BP
Why are metals conductive?
The movement of the cations and the electrons also let the electrical currents move through them as well
Why is the melting point and boiling point for metals high?
the moving electrons makes it harder for the bonds to break, which requires more energy/heat to break it
Why are metals ductile?
Since there are no direct bonds, the metals can slide over each other
Why are metals malleable?
the aren’t brittle like ionic crystalline solids because of the sea of electrons. When they are bend, the cations and anions move so they are still bonded together. Unlike in ionic crystalline solids, when they are bent, the similar charges line up and repel each other causing the breakage
What are alloys?
mixture of 2 or more elements, 1 of which is at least a metal
How to make alloys?
Melting a mixture of ingredients, then cooling
Ionic properties
hard, brittle, conductive when melted or dissolved, crystalline solids, high MP
Covalent properties
poor conductors, low Mp, soft
