Chapter 7 over view notes 

Valence electrons- electrons in the highest occupied energy level if an element’s atom S and P orbitals 1s 3p- Up to eight valence electrons

 Dot structure- represents valence electrons as a dot

Octet rule- completely filled valence electrons Noble gasses have filled valence electrons and are stable metals lose electrons Cations

• Metals lose electrons

  • Cations
  • + charge (groups 1-3)
  • Add ion

• Non-metals gain electrons

  • Anionions- when an atoms gains electrons  
  • - charge 
  • Add ied

• Opposite charges attract cations and anions create a net charge of zero  

  • Cross over the charges 
  • Mg2+ N3-
  • Mg3N2
  • Check that the total charge equals zero

• 3 properties of ionic compounds 

  • Crystalline solid at room temperature
  • High melting point
  • Conduct electric current in the liquid state 
  • Free to move/ have a moving charge
  • Properties unique to metals
  • valence electrons of an atom in a pure metal can me modeled as a sea of electrons
    • Sea of electrons- when the valence electrons are mobile and can drift freely and part of the metal to another
    • present the valence electrons of a pure metal. They can freely move through metal. Metallic bonds draw positively charged ions to their free floating electrons. 
    • When metals have pressure the metal cations easily slide past one another
  • Alloys- have some properties that are better 
  • Bronze 
    • Copper is most abundant being 88% of bronze 
    • Tin is 12%
    • Harder and more fusible than copper 

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