Chemical Bonding

Chapter 8

8.1 Types of Bonds

Ionic and Covalent Bonds

• Chemical Bonds are the force that holds atoms together in a compound or molecule

• Ionic Bonds are bonds between ions held together by electrostatic force.

• Covalent Bonds are where electrons are shared between atoms.

PROBLEM

Identify which type of Chemical Bond is most likely in the following.• NaF• ClO2

• FeSO4

• H2O

• NaNO3

Polar and Nonpolar Covalent Bonds

• Rarely are covalent bonds a completely equal sharing.

• Polarity is the degree of transfer from one member of a covalent bond to the other.

• Nonpolar Covalent Bonds have little to no polarity and share the electrons equally.

• Polar Covalent Bonds have detectable polarity and have an uneven sharing of electrons.

Polarity Continuum

Electronegativity

• Electronegativity – The ability for an atom to bonding electrons.

• Varies in a periodic fashion• The greater the difference in

electronegativity the greater the polarity of the bond.

Electronegativity

8.2 Ionic Bonds

Lewis Symbols

• Lewis Symbols – A shorthand to show the valence electrons of an atom.

• Examples

PROBLEM

Draw the Lewis Structures of the following.

• NaF

• CaCl2

• Be3N2

Structure of Ionic Crystals

• An ionic crystal is an arrangement of ions that maximize attraction and minimize repulsion of ions.

• The crystals structure makes ionic solids very hard, brittle and poor conductors.

• Crystal structure also accounts for high melting and boiling temperatures.

8.3 Covalent Bonds

The Octet Rule

• In the Main Group elements, stability is reached by becoming isoelectronic with the noble gases.

• This completes the Valance Shell for the principal energy level

• Since the s and p orbitals take eight electrons, this is called the octet rule.

Octet Examples

Na Ca S Cl

Lewis Formulas for Diatomics

Valence Electrons

PROBLEM

• Give Possible Identities for each X.

X X XCl

Cl Cl Cl Cl Cl ClCl

Structures of Covalent Molecules

• Write the Skeleton Equation• Sum the Valance Electrons and

determine the total• Place two electrons for each single bond• If you have remaining valance

electrons, add them as unshared pairs to satisfy unfilled octets

• Use double and triple bonds to satisfy octets on the central atoms

EXAMPLE

• Carbon Dioxide

PROBLEM

• H3CCN

• NH2OH

Resonance

PROBLEM

• Nitric Oxide, N2O, NNO arrangement.

Exceptions to the Octet Rule

• Odd Number of Electrons (NO)

• Unfilled Octet (BH3)

• More than eight electrons around the central atom.

Bonding in Carbon Compounds

• Carbon’s versatility comes from its four valance electrons.

• Carbon can readily bond with itself at “normal” temperatures

8.4 Shape of Molecules

The VSEPR Theory

• Valence Shell Electron Pair Repulsion Theory says that pairs of electrons will try to get as far away from each other as possible.

• You use the Lewis structure to determine a general structure then fine tune the model.

Predicting the Shape of Molecules

• Draw the Lewis formula• Count the number of bonds and

unshared pairs on the central atom• The sum gives you the parent

formula (Linear, Trigonal Planar, Tetrahedral)

• Consider on the bonded atoms to determine the sub-shape (AX2, AX3, AX4)

EXAMPLE

• CH4

• NH3

• H20

PROBLEM

• Determine the shape.• CO3

2-

• SCl2

Polarity of Molecules

• If the bonds are polar and the molecular shape is not symmetrical the molecule is polar.

• If the bonds are not polar or the molecule is symmetrical the molecule is nonpolar.