2. *Electronegativity: the tendency of an atom to
attract electrons
*The higher the electronegativity, the stronger
the atoms attraction for electrons
*The values range from 0.6-4.8
*Atoms will gain, lose or share electrons when
they bond depending on the relative
electronegativity's of the atoms participating in
the bond.
*Metals have low electronegativity's
*Non metals have high electronegativity's
*Electronegativity
3. *Ionic Bonding
*Ionic bonds form between metals and
nonmetals and result in the formation of ions
*Ions are atoms that have gained or lost
electrons and are therefore charged
*Nonmetals have higher electronegativity’s so
they will take electrons from metals
5. *Covalent Bonds
*Covalent bonds form between nonmetals
*Nonmetals all have relatively high
electronegativity’s so they share electrons
*Electrons being shared are represented by a
straight line
6.
7. *Covalent Bonds
*Covalent bonds are either nonpolar or polar
depending on the electronegativity’s of the
nonmetals and their 3-D arrangement in space
*Nonpolar covalent bonds form when electrons
are equally shared
*Polar covalent bonds form when electrons are
not equally shared
*Polar covalent bonds contain atoms (or ends of
a molecule) with partial charges
9. *Hydrogen Bonds
*A hydrogen bond is a slight attraction of a
hydrogen on one molecule to a nitrogen or
oxygen on another molecule.
*Hydrogen bonds occur between polar molecules
since they have partial charges
*Hydrogen bonds are represented with dashed
lines
10. *All of the dashed lines below are hydrogen bonds
*The solid lines are covalent bonds.
*Are these covalent bonds polar or nonpolar? How do
you know?
11. *The bonds have to be polar since hydrogen
bonds are being formed.
*Oxygen atoms and nitrogen atoms will always
have a partial negative charge in a hydrogen
bond.
*Hydrogen atoms will always have a partial
positive charge in a hydrogen bond.
