PERIODIC TABLE REVIEW
     PERIODIC TABLE REVIEW
        Location of Metals and Nonmetals on the 
          Location of Metals and Nonmetals on the 
         periodic table:
          periodic table:
           Metals are to the left of the “staircase”
            Metals are to the left of the “staircase”
           Nonmetals are to the right of the “staircase”
            Nonmetals are to the right of the “staircase”
           For bonding, the 7 metalloids will treated as 
            For bonding, the 7 metalloids will treated as 
            metals
            metals
           All though hydrogen is to the left of the 
            All though hydrogen is to the left of the 
            “staircase”, it is not, nor has it ever been a 
            “staircase”, it is not, nor has it ever been a 
            metal.  IT IS A NONMETAL!
            metal.  IT IS A NONMETAL!
                                    
                                    
     ATOMS AND IONS REVIEW
     ATOMS AND IONS REVIEW
         Atoms are neutral
           Atoms are neutral
             They have the same number of protons and electrons
               They have the same number of protons and electrons
                 Number of positives = number of negatives
                  Number of positives = number of negatives
             Example:  Na 11 protons, 11 electrons  11 – 11 = 0
                                                        
               Example:  Na     11 protons, 11 electrons     11 – 11 = 0
         Ions have a charge
           Ions have a charge
             They have a different number of protons and electrons
               They have a different number of protons and electrons
                            +1
                             +1
               Example:  Na 11 protons, 10 electrons 11 – 10 = +1
                                                         
               Example:  Na      11 protons, 10 electrons    11 – 10 = +1
             If an atom GAINS an electron  becomes negatively 
                                              
               If an atom GAINS an electron      becomes negatively 
               charged  ANION
                        
               charged     ANION
             If an atom LOSES an electron  becomes positively 
                                               
               If an atom LOSES an electron       becomes positively 
               charged  CATION
                        
               charged     CATION
                                           
                                           
     TYPES OF BONDS
     TYPES OF BONDS
        Bonding occurs because every element is either 
          Bonding occurs because every element is either 
          trying to get to 0 electrons in the valence or 8 
          trying to get to 0 electrons in the valence or 8 
          electrons in the valence (zero and 8 are both 
          electrons in the valence (zero and 8 are both 
          stable)
          stable)
            Valence is the outer electron shell—place where 
             Valence is the outer electron shell—place where 
             bonding occurs
             bonding occurs
        Ionic – Bonding between a metal and a 
          Ionic – Bonding between a metal and a 
          nonmetal
          nonmetal
        Metallic – Bonding between two metals
          Metallic – Bonding between two metals
        Covalent – Bonding between two nonmetals
          Covalent – Bonding between two nonmetals
                                      
                                      
    IONIC BONDING
    IONIC BONDING
        Very stable and strong
         Very stable and strong
        Strongest possible bond
         Strongest possible bond
        Requires a large amount of energy to break an 
         Requires a large amount of energy to break an 
         ionic bond
         ionic bond
        Forms compounds known as “ionic 
         Forms compounds known as “ionic 
         compounds”
         compounds”
        All ionic compounds will dissolve in water and 
         All ionic compounds will dissolve in water and 
         carry a current (electrolyte)
         carry a current (electrolyte)
        Generally have high melting and boiling points
         Generally have high melting and boiling points
        Compounds are generally hard and brittle
         Compounds are generally hard and brittle
                                    
                                    
    IONIC BONDING
    IONIC BONDING
        Draw the dot diagram for Na AND Cl
         Draw the dot diagram for Na AND Cl
       Na has 1 valence electron, wants to give that 1 
       Na has 1 valence electron, wants to give that 1 
         away and get to zero and be stable
         away and get to zero and be stable
       Cl has 7 valence electrons, wants to get 1 
       Cl has 7 valence electrons, wants to get 1 
         electron so it can get to eight and be stable
         electron so it can get to eight and be stable
       Na give an electron to Cl and Cl takes that 
       Na give an electron to Cl and Cl takes that 
                                   
          electron from Na         
         electron from Na