Ionic and Covalent Bonding
Ionic bonding: The ____________ of electrons resulting in a bond.
Covalent bonding: The ____________ of electrons resulting in a bond.
Polar covalent bonds: The ____________________ of electrons resulting in a bond.
Electronegativity: A measure of an atom’s ability to _________ electrons in a chemical bond.
Periodic Trends
Across the P.T.
EN increases. As the atom decreases in size the nucleus attracts a bonding pair of
electrons more strongly because they are closer to the nucleus.
Down the P.T.
EN decreases. In larger atoms there is an increase distance from the nucleus to
any bonding electrons. Therefore the nucleus does not have a very strong
attraction to them.
Electronegativity Differences
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It is possible to determine bond type using electronegativity differences.
For example:EN for K is 0.8 and the EN for F is 4.0. The EN is 3.2, therefore this is an ionic bond.
Ionic bond: The EN is greater than 1.7
Covalent bond: The EN is 0.0
Polar covalent bonds: The EN is less than 1.7 and greater than 0.
Octet Rule: Atoms bond in order to achieve an electron configuration that is the same as that of a noble
gas.
Eg. The forming of LiBr is a result of two ions Li1+ and Br1-.
Li1+ has the same structure as He.
Br1- has the same structure as Kr.
Isoelectronic: Two atoms or ions having the same electron configuration.
Ex. The calcium ion (Ca2+) and sulphide ion (S2-) have the same electron configuration as
Argon.