Metallic bonding

    Cards (61)

    • What is the main structure of metals?
      Metals consist of a giant structure
    • What happens to the electrons in the outer shell of metal atoms?
      They are delocalized and free to move
    • What holds the atoms together in metallic bonding?
      Electrostatic attraction between ions and electrons
    • How strong is metallic bonding?
      Metallic bonding is very strong
    • What types of compounds are held together by metallic bonding?
      Metallic alloys and compounds
    • What do delocalized electrons in metallic bonds produce?
      All the properties of metals
    • Why do metallic compounds have high melting and boiling points?
      Strong electrostatic forces require lots of energy
    • What state are most metallic compounds at room temperature?
      Generally solid
    • Why are metals generally not soluble in water?
      Due to their strong metallic bonding
    • Why are metals denser than non-metals?
      Metal ions are packed closely together
    • What property allows metals to be hammered into sheets?
      Malleability due to sliding layers of atoms
    • How do delocalized electrons contribute to conductivity?
      They carry electrical current and thermal energy
    • What basic physical properties do all metals share?
      Similar basic physical properties due to metallic bonding
    • Why don't non-metals exhibit the same properties as metals?
      Non-metals lack metallic bonding
    • What types of structures do non-metals form?
      A variety of different structures
    • What are common characteristics of non-metals?
      Dull, brittle, low boiling points
    • How do non-metals generally behave in terms of electrical conductivity?
      They do not generally conduct electricity
    • How do metals and non-metals differ in chemical properties?
      Non-metals gain electrons, metals lose electrons
    • Where are non-metals typically found on the periodic table?
      Top and right-hand side
    • Where are metals typically found on the periodic table?
      Bottom and left-hand side
    • What is the typical state of non-metals at room temperature?
      They are not generally solids
    • What is the significance of the outer shell of electrons in metals?
      They are generally under half-filled
    • What is the significance of the outer shell of electrons in non-metals?
      They are generally over half-filled
    • What is a humorous reference made about a metal on the bus?
      A metal was the conductor
    • What is the metallic element mentioned in the study material?
      Copper
    • What is the term for the positive ions in metallic bonding?
      Metal ions
    • What is the role of delocalized electrons in metallic bonding?
      They create a 'sea of electrons'
    • What is the effect of strong electrostatic forces in metals?
      They require lots of energy to break
    • What happens to the layers of atoms in a pure metal?
      They can slide over each other
    • What is the significance of the term 'delocalized' in metallic bonding?
      Electrons are free to move around
    • How does the structure of metals contribute to their properties?
      Regular structure allows for conductivity and malleability
    • What is the relationship between metallic bonding and the properties of metals?
      Metallic bonding explains their physical properties
    • What is the role of energy in breaking metallic bonds?
      High energy is needed to break them
    • How do the properties of metals differ from those of non-metals?
      Metals are conductive, non-metals are not
    • What is the significance of the periodic table's layout for metals and non-metals?
      It shows their different locations and properties
    • How does the arrangement of electrons affect the properties of metals?
      Delocalized electrons enhance conductivity and malleability
    • What is the impact of metallic bonding on the physical state of metals?
      It generally keeps them solid at room temperature
    • How do the properties of metals relate to their applications?
      Properties like conductivity make them useful
    • What is the significance of the term 'malleable' in relation to metals?
      It means they can be shaped easily
    • How does the presence of delocalized electrons affect the thermal properties of metals?
      They allow metals to conduct heat effectively