Metallic Bonding

    Cards (48)

    • What is the main difference between alloys and pure metals?
      Alloys contain two or more elements
    • What type of bonding occurs between metal atoms?
      Metallic bonding
    • What type of bonding occurs between metals and non-metals?
      Ionic bonding
    • What type of bonding occurs between non-metals?
      Covalent bonding
    • What do metal atoms do with their outer shell electrons in metallic bonding?
      They give up and share them
    • What are the electrons called that are free to move about in metallic bonding?
      Delocalized electrons
    • Why do metal atoms become positive ions in metallic bonding?
      They lose negative electrons
    • What type of attraction holds the structure together in metallic bonding?
      Electrostatic attraction
    • What are the melting and boiling points of most metallic structures?
      High
    • Which particles are attracted to each other in metallic bonding?
      Positive ions and negative electrons
    • Why are metals good conductors of electricity and heat?
      Delocalized electrons carry energy
    • Why are pure metals able to be bent or hammered easily?
      Layers can slide over one another
    • What is the name for the property that metals can be hammered into shapes?
      Malleable
    • What is the effect of adding different sized atoms to a metal structure to make an alloy?
      Disrupts the regular structure
    • Why are alloys harder than pure metals?
      Layers can no longer slide easily
    • What are the main elements in steel?
      Iron and carbon
    • Besides iron and carbon, what other elements can be found in steel?
      Chromium, manganese, or vanadium
    • In what applications are alloys like steel used due to their strength?
      Cars and planes
    • How do alloys differ from pure metals in terms of their structure and properties?
      • Structure: Alloys have a disrupted, irregular structure due to different sized atoms.
      • Hardness: Alloys are harder than pure metals.
      • Sliding Layers: Layers in alloys cannot slide over one another as easily as in pure metals.
    • What topic will be covered regarding the periodic table in this two-part video?
      Periodicity, bonding, and structure
    • What three types of structures will be looked at?
      Giant metallic, giant covalent, simple molecular
    • What properties have previously been covered regarding periodicity?
      Electron configuration, atomic radius, ionization energy
    • What trend is observed in the periodic table regarding metals and non-metals?
      Metals on the left, non-metals on the right
    • What are metalloids also called?
      Semi-metals
    • What characteristic defines metalloids?
      They have properties of both metals and non-metals
    • What elements are being focused on from Period 2?
      Lithium and beryllium
    • How many protons does a lithium atom have?
      Three
    • How many electrons are in lithium's outer shell?
      One
    • What happens to the outer shell electrons in metals?
      They are delocalized
    • What term describes the sharing of electrons in metals?
      Delocalization
    • What charge do lithium atoms have after donating their outer electron?
      One positive
    • What are positively charged metal ions called?
      Cations
    • What type of attraction occurs between delocalized electrons and positive cations?
      Electrostatic attraction
    • What is the electrostatic attraction in metals called?
      Metallic bonding
    • What is the overall structure of a metal referred to as?
      Giant metallic lattice
    • What are the two key features of a giant metallic lattice?
      • Cations are fixed in place and cannot move.
      • Delocalized electrons are free to move.
    • What property of metals does the movement of delocalized electrons explain?
      Good conductors of electricity
    • In what states do metals conduct electricity?
      Solid or liquid
    • What pole are delocalized electrons attracted towards?
      Positive pole
    • What role do delocalized electrons play in electrical conductivity?
      Mobile charge carriers