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CHEMICAL BONDING III

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CHEMICAL BONDING III

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Chemical bonding and interactions between atoms can be classified into a number of different types.

Chemical bonds

1. Covalent bonding

2. Ionic bonding

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Multiple covalent bonds

In some cases, more than one pair of valence electrons can be shared between atoms. This kind of bonding is called multiple covalent bond.

For example, in order to form oxygen gas, two atoms share a double bond resulting in the structure O=O.

In nitrogen gas, a triple bond is formed between two

nitrogen atoms, N≡N.

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Electronegativity

Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons.

The relative electronegativities of the two atoms in a bond

will determine whether a covalent bond is polar or

nonpolar. Whenever one element is significantly more

electronegative than the other, the bond between them

will be polar, meaning that one end of it will have a slight

positive charge and the other a slight negative charge.

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Bond Polarity

Bond polarity is determined by the difference in

electronegativity and is defined as the relative ability of an atom to attract electrons when present in a

compound.

• Polar Covalent Bonds

• Nonpolar Covalent Bonds

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Polar Covalent Bonds

Whenever one element is significantly more electronegative than the other, the bond between them will be polar, meaning that one end of it will have a slight positive charge and the other a slight negative charge.

Nonpolar Covalent Bonds

A bond in which the electronegativity difference is less than 1.7 is considered to be mostly covalent in

character.

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Dipol Moment

When atoms in a molecule share electrons

unequally, they create what is called a dipole

moment.

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μ=Qr

where Q is measured in coulombs (C) and r in meters.

The unit for dipole moments is the debye (D):

1D=3.3356×10

−30

cm

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