Ionic bonding: Li + O 1e - [ O ] 2– [Li] 2 + 6e - 2e - 8n 0 8p + 1e - 3p + 4n 0 2e - 1e - 3p + 4n 0 2e - 1e - 8e - 2e - 8n 0 8p + 3p + 4n 0 2e - 3p + 4n.

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Presentation transcript:

Ionic bonding: Li + O 1e - [ O ] 2– [Li] 2 + 6e - 2e - 8n 0 8p + 1e - 3p + 4n 0 2e - 1e - 3p + 4n 0 2e - 1e - 8e - 2e - 8n 0 8p + 3p + 4n 0 2e - 3p + 4n 0 2e - 2Li + O [Li] 2 + [O] 2– or 4Li + O 2 2[Li] 2 + [ O] 2– O Li

1e - 17p + 18n 0 7e - 8e - 2e - 13p + 14n 0 2e - 8e - 3e - 17p + 18n 0 7e - 8e - 2e - 17p + 18n 0 7e - 8e - 2e - Ionic bonding: Al + Cl 1e - 17p + 18n 0 8e - 8e - 2e - 17p + 18n 0 8e - 8e - 2e - 17p + 18n 0 8e - 8e - 2e - 13p + 14n 0 2e - 8e -

Ionic bonding: Al + Cl [ Cl ] 3 – [Al] 3+ Al + 3Cl [Al] 3+ [Cl] 3 – ClAlCl

Covalent bonding Thus far we have looked at when atoms bond due to the transfer of electrons An ionic bond forms when an atom has a greater attraction for e – s than a second atom However, if two atoms have approximately the same pull on electrons, they share the electrons (forming a covalent bond) Read Covalent bonding and Covalent bonding continued. Do Q7.

Covalent bonding Q7 CCl 4 - Covalent C Cl HCl - Covalent H Cl MgF 2 - Ionic [ F ] 2 – [Mg] 2+ H 2 O - Covalent H O H NH 3 - Covalent H N H H NaCl - Ionic [ Cl ] – [Na] + OH – - Covalent O H H 2 - Covalent HH For more lessons, visit

Multiple bonds Do Q. 8. Build models of molecules, O 3 as challenge (cant build it or ionic) HCl - Covalent H Cl H CO 2 - Covalent COO Na 2 O - Ionic [ O ] 2– [Na] 2 + H N H H H N H H OO OO O 2 - Covalent OO C II II I 2 - Covalent [ O ] 3 2– [Al] 2 3+ Al 2 O 3 - Ionic NH 3 - Covalent OO O OOO O 3 - Covalent H C H H H H C H H H