Atomic Bonding

Atomic Bonding

1. Each kind of atomic relationship requires a different type of energy, but they all do best when they settle into the lowest stress situation possible.

   • The nature of bond between atoms is related to the distance between them and how positive or negative they are
     • Types of Chemical Bonds
       • Atoms do whatever they can to reduce their overall energy. They reach their largest energy by achieving a balance between attractive and repulsive forces.
         • Electrostatic Force: when 2 atoms approach each other, the electrons of each are attracted to the protons of the other (like charges repel, opposites attract)
           • Bond Length: distance between two nuclei at the point of minimum energy (where the attractive and repulsive forces cancel out)
       • Covalent Bond
         • Electrons are attracted to both nuclei in the molecule. They spend most of their time in the space between them. A bond found by atoms sharing electrons.
           • Electronegativity: the ability of an atom to attract shared electrons
             • If two atoms in a bond have very different electronegativities, the electrons are more attracted to the atom with the higher electronegativity.
         • nonmetals, metalloids
         • Covalent Compounds tend to be softer solids, liquids, or gases like Cl2 and are often not soluble in water
       • Ionic Bonds
         • A bond formed by the transfer of electrons from one atom to another (formed by the transfer of electrons from one atom to another)
           • Charles-Augustin De Coulomb
             • E=(2.31x10^-19 Jnm) (Q1xQ2/r^2)
               • Ionic Bonds are extremely polar because they consist of a positive ion and a negative ion
                 • Ionic compounds are often crystalized in their solid form, generally soluble in water because the two ions interact separately with the positively and negatively charged areas in a water molecule, and once they are separated or dissolved the ions allow the solution to conduct electricity

2. Polarity

   • When the electrons hangout closer to one side of the bond, it creates a slight negative charge in that area and a slight positive charge around the other atom.
     • Separation of Charges
   • Polar Covalent Bond
     • Electrons are attracted to one atom more than the other
       • a covalent bond in which the two atoms have different electronegativities, causing separation of charges
   • Nonpolar Covalent Bond
     • A covalent bond in which the two atoms have identical or very similar electronegativites, so that the charges are distributed evenly