1. BASED ON LEWIS DOT STRUCTURES 4 TYPES OF BONDING  IONIC BONDING  COVALENT BONDING  HYDROGEN BONDING  METALLIC BONDING

2.  H Electrons in the outer shell He 1 2 Li Be B C N O F Ne 1 2 3 4 5 6 7 8

3. All Noble gases have filled outer shells. All Noble gases are HAPPY and stable.  Helium has 2e- in outer shell therefore already Happy.  Other Noble gases have 8 e-’s which fill their outer shells ( Octet )  Filled outer shells prevents the Noble gases from reacting with other elements.  All other atoms try to get outer shells like the Noble Gases have.

4.  A filled outer shell is called an OCTET and is the HEAVEN condition for ions or atoms  All other atoms try to reach the HAPPY condition by doing 1 of 3 options

5.  Ionic Bonding  Gain an e- : H + 1e-  H (H -1 ) (2e- in outer shell)  Lose an e- : H  H + + 1e- (H +1 ) (Zero e-’s in outer shell)  Covalent Bonding  Share e-’s : (2e- in both outer shells)

6.  One atom loses an e- and becomes positive(+)  One atom gains an e- and becomes negative(-)  Opposite charged particles attract, bond & neutralize.  Usually a weak bond which can be broken by water.  Free ions in water allow for flow of e-’s (electricity).  Usually form crystal lattice.

7.  Alkalies can ONLY LOSE 1e- to become: Li  Li + + 1e-  If it gains or shares 1e- it would then have 1 or more e-‘s in a shell that wants 8e-‘s. This would not be stable.  This is true for the rest of the Alkali Metals.

8.  The Alkaline Earth elements are most likely to lose 2e’s to reach a filled outer shell.  Mg  Mg +2 + 2e-  They all become a +2 ion.  Be +2, Mg +2, Ca +2 and so on.  Gaining or sharing will not reach OCTET.

9.  The Boron Family are most likely to lose 3e’s to reach a filled outer shell. B  B +3 + 3e-  Therefore they prefer to be a +3 ion.  B +3, Al +3, Ga +3 and so on.  Gaining or sharing will not reach OCTET

10.  Covalent bonding is sharing of 2 e-’s between 2 nuclei  No CHARGES are involved  Based on the Lewis Dot Structure outer shell  Strongest bonds  Shared e-’s add toward the OCTET completion  Electron pair is not always shared equally leading to a POLAR BOND & Molecule

11.  The Carbon Family can lose the outer 4e - ‘s to become C +4 ions falling to a previously filled outer shell 2 e - ’s. C  C +4 + 4e - ’s  The Carbon Family can gain 4e - ‘s to become C -4 and fill the outer shell with 8e - s(OCTET). C + 4e -  C -4  They can share their outer 4e - ‘s with other atoms wanting to share( COVALENT BONDING) and reach OCTET in the shape of a TETRAHEDRON.

12.  The Nitrogen Family can gain 3e - ’ s to become N -3 ions. N 2 + 6e -  2N -3  The Nitrogen Family can share 3e - ‘s to reach the OCTET.   Two e - ’s are found between N and each H.  Diatomic Nitrogen requires a triple bond sharing 6 e - ’s.

13.  The Oxygen Family can gain 2e - ‘s to become O -2 ions. O 2 + 4e -  2O -2  The Oxygen Family can share 2e - ‘s to reach the Octet. 4e - shared is a Double bond.

14.  The Halogens could gain 1e - to become a negative ion.  F 2 + 2e -  2 F -1  The other possibility is to share 1 non-paired electron with another atom.  H + F  

15.  Oxygen attracts e-’s more than Hydrogen.  When H and O are bonded, the electrons are closer to the Oxygen than the Hydrogen.  This causes a partial + near Hydrogen and a partial – near the Oxygen.  This is a polar attraction between water molecule.  This polarity causes molecules to attract each other requiring more energy to pull molecules apart.  These attractions cause a higher Melting & Boiling Points for chemicals that have polarity & Hydrogen.

17.  Orderly arrangement of molecules caused by Hydrogen bonding in the solid state of water causes solid to expand and float which is unique.

18.  Most solid metals arrange themselves so that 1 atom constantly contacts 12 +other atoms.  The e-’s become very free in this tight packing and can flow as a river of e-’s down the line.  This is the definition of electricity : the flow of loosely held e-’s through a metal.  High melting temperatures are usually noted.

19.  Ionic Bonding  Roman Numeral  Non-Ionic Bonding

20.  Always between a Metal and a Non-metal  Name the as found on the periodic table  Change the name of the non-metal to –ide ending  For the formula, use the charges from the Common Ion Chart or Periodic Table families to determine needed subscripts. The + and – ion charges MUST to cancel to “ZERO”.  Ba +2 + 2Cl - add up to zero then charges disappear  BaCl 2 is called Barium Chloride using subscripts

21.  Na +1 + Cl -1  NaCl (1:1)  Ba +2 + 2NO 3 -1  Ba(NO 3 ) 2 (1:2)  Al +3 + 3I -1  AlI 3 (1:3)  2 Al +3 + 3CO 3 -2  Al 2 (CO 3 ) 3 (2:3)

22.  Some metals can have 2 or more common ions  Fe +2, Fe +3, Cu +1, Cu +2, Pb +2, Pb +4  You must indicate which ion is being used by placing a Roman Numeral behind the symbol  Elements that must use Roman Numerals are: Fe, Cu, Pb, Ni, Co, Hg, Cr, Sn

23.  Fe +2 = Fe II Fe +3 = Fe III  Fe +2 + 2OH -1  Fe(OH) 2 Iron II Hydroxide   Fe +3 + 3OH -1  Fe(OH) 3 Iron III Hydroxide

24.  Only used if both elements are Non-metals  Use prefixes to declare number of atoms used  Mono = 1(used only for second element)  Di = 2, Tri = 3, Tetra = 4, Penta = 5, Hexa = 6, Septa = 7, Octa = 8, Nona = 9, Deca = 10  The “a” is sometimes dropped  CO = Carbon Monoxide, CO 2 = Carbon Dioxide  N 2 O 4 = DiNitrogen TetrOxide  P2O5 = DiPhosphorus PentOxide