Lewis diagrams represent the valence electrons of atoms and are used to show covalent bonding between atoms. Covalent bonds form through the sharing of valence electrons. The octet rule states that atoms want eight electrons in their outer shell and will share electrons to reach eight, except for hydrogen which is stable with two. Lewis structures show the outer shell electrons that participate in bond formation.
Lewis diagrams, also called electron-dot diagrams.pdf
1. Lewis diagrams, also called electron-dot diagrams, are used to represent paired and
unpaired valence (outer shell) electrons in an atom The Lewis structure is used to represent the
covalent bonding of a molecule or ion. Covalent bonds are a type of chemical bonding formed by
the sharing of electrons in the valence shells of the atoms. Covalent bonds are stronger than the
electrostatic interactions of ionic bonds, but keep in mind that we are not considering ionic
compounds as we go through this chapter. Most bonding is not purely covalent, but is polar
covalent (unequal sharing) based on electronegativity differences. The atoms in a Lewis
structure tend to share electrons so that each atom has eight electrons (the octet rule). The octet
rule states that an atom in a molecule will be stable when there are eight electrons in its outer
shell (with the exception of hydrogen, in which the outer shell is satisfied with two electrons).
Lewis structures display the electrons of the outer shells because these are the ones that
participate in making chemical bonds.
Solution
Lewis diagrams, also called electron-dot diagrams, are used to represent paired and
unpaired valence (outer shell) electrons in an atom The Lewis structure is used to represent the
covalent bonding of a molecule or ion. Covalent bonds are a type of chemical bonding formed by
the sharing of electrons in the valence shells of the atoms. Covalent bonds are stronger than the
electrostatic interactions of ionic bonds, but keep in mind that we are not considering ionic
compounds as we go through this chapter. Most bonding is not purely covalent, but is polar
covalent (unequal sharing) based on electronegativity differences. The atoms in a Lewis
structure tend to share electrons so that each atom has eight electrons (the octet rule). The octet
rule states that an atom in a molecule will be stable when there are eight electrons in its outer
shell (with the exception of hydrogen, in which the outer shell is satisfied with two electrons).
Lewis structures display the electrons of the outer shells because these are the ones that
participate in making chemical bonds.
