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Bonding
A Chemical Bond• The forces that hold groups of atoms
together and make them function as a unit• Bonding involves only the valence electrons
• There are 2 types of bonds:– Ionic: Transfer of electrons from a metal and to
a nonmetal
– Covalent: Sharing of electrons between 2 nonmetals
– Note: When 2 metals bond an alloy is formed
Ionic Bonding
• Chemical bonding that results from the electrical attraction between cations and anions is called ionic bonding.
• Cations give up electrons to anions.
• Ionic compounds form between metallic ions and non-metallic ions.
Covalent Bonds
• A covalent bond results from the sharing of electrons between two atoms.
• The most familiar examples of covalent bonding are seen in the interactions of nonmetallic elements with one another. (CO2, NO)
• Diatomic molecules are held together by covalent bonding (N2, O2, F2 Cl2, Br2, I2, As2, H2).
• Electrons are transferred or shared to give each atom a noble gas configuration (stable octet)– This is known as the octet rule
Octet Rule
• Noble gases have a very stable structure and are somewhat unreactive.
• According to the octet rule, atoms bond in order to achieve an electron configuration that is the same as the electron configuration of a noble gas.
• As an example, Chlorine will gain an electron to have 18, which is how many the atom Argon has. These two atoms are said to be isoelectronic with each other.
Lewis Diagrams
• Valence electrons involved in bonding can be represented by Lewis dot diagrams
• A chemical symbol represents the nucleus and the core electrons (not involved in bonding).
• Dots around the symbol represent valence electrons.
Drawing Lewis Diagrams1. Write the element symbol.
2. Draw dots, one for each valence electron
3. Dots should be spread over 4 sides• It does not matter what side the dots are
placed, but do not start to pair dots until there is one on each side
Cl
• Lewis diagrams for the first 20 elements
Representing Ionic CompoundsLewis Diagrams
• Formation of sodium chloride:
Na · + ® [Na]+ [ ]Cl · ·
· ·
·· ··Cl
· ·
· · ···
Bohr Diagram
Lewis Diagram
It takes two Na to satisfy one sulfur.
Lewis Structures for Ionic Compounds
Ba•
• O•••
•••
••O••
••
••Ba
2+ 2-
Mg•
•
Cl•••
••
••Cl•••
••••
••Cl••
••
••Mg
2+ -2
Ba and O
Mg and Cl
BaO
MgCl2
Covalent Bonding
• Formation of hydrogen chloride:
H · + Cl · ·
· ·
··· ® Cl
· ·
· ·
·· ··H ® H - Cl
· ·
· ·
··
Covalent bond, shared electrons
Lone pairs, valence electrons not involved in covalent bond
Structural Formula: H-Cl (lone pairs are not drawn)
Lewis Structures
H · · H+
® Cl Cl ·· ·· · ·
· ·
· ·
· ·
··
H2or H H
Cl2 Cl · ·
· · ···Cl
· ·
· ·
·· · +
or Cl Cl ·· ··
· ·
· · · ·
· ·
® H H
Structural Formula: Cl-Cl
Multiple Bonds
• Atoms sometimes need to share more than a pair of electrons.
• If an atom is sharing two pairs of electrons, this is a double covalent bond.
• If an atom is sharing three pairs of electrons, this is a triple bond.
Double and Triple Bonds
• Atoms can share 4 electrons to form a double bond or 6 electrons to form a triple bond.
• The number of shared electron pairs (covalent bonds) that an atom can form is thebonding capacity.
O2:
N2:
=O O · ·
· · · ·
· ·
·· ··N N
Multiple Covalent Bonds
N••
••
•N N
•
••
•
•
••
•N••
••
•
N N•
•• ••
•N N •
•
••
Multiple Covalent Bonds
C••
••
O••
• •
• •O••
• •
• •CO O
•
••
•••
••
••
••
•CO O ••
•••
••
••
••CO O
••
••
••
••