Goes into detail about different types of bonding - ionic, covalent, co-ordinate and metallic bonding. The physical and chemical properties of these different types of bonding are described. The different types of intermolecular forces are also described in detail. These notes are a summary of the...
Metals have one, two, or three electrons in their outer main level, so the easiest
way for them to attain the electron structure of a noble gas is to lose their outer
electrons.
Non-metals have spaces in their outer main levels, so that the easiest way for
them to attain the electron structure of a noble gas is to gain electrons.
Atoms make bonds between each other by using their outer electrons → to gain
a more stable electron configuration - gaining a full outer shell of electrons
Occurs between metals and non-metals; electrons are transferred from the
outer-shell of the metal to the outer shell of the non-metal.
The metal forms a positive ion (cation), and the non-metal for a negative ion
(anion).
The ions stick together due to an electrostatic attraction between the positive
and negative charges.
Eg: Sodium Chloride
Sodium, Na, has 11 electrons (and 11 protons). The electron arrangement
is 1s2 2s2 2p6 3s1.
Chlorine, Cl, has 17 electrons (and 17 protons). The electron arrangement
is 1s2 2s2 2p6 3s2 3p5.
An electron is transferred. The single outer electron of the sodium atom
moves into the outer main level of the chlorine atom.
Each outer main level is full now.
BONDING 1
, Both sodium and chlorine now have a noble gas electron arrangement.
Sodium has the neon noble gas arrangement whereas chlorine has the
argon noble gas arrangement.
The sodium ion is positively charged because it has lost a negative
electron.
The chloride ion is negatively charged because it has gained a negative
electron.
The two ions are attracted to each other and to other oppositely charged
ions in the sodium chloride compound by electrostatic forces.
Ionic bonding is the result of electrostatic attraction between oppositely charges
ions, extending through the compound so that every negatively charged ion
attracts every positively charges ion and visa versa.
Ionic compounds always exist in a structure called lattice.
Properties of ionically bonded compounds
Ionic compounds are always solids at room temperatures.
They have giant structures and therefore high melting points because in
order to melt an ionic compound, energy must be supplied to break up the
lattice of ions.
Ionic compounds conduct electricity when molten or dissolved in water
(aqueous) but not when solid because the ions that carry the current are
free to move in the liquid state but are not free in the solid state.
Ionic compounds are brittle shatter easily when given a sharp blow because
they form a lattice of alternating positive and negative ions. A blow in the
direction shown may move the ions and produce contact between ions with
like charges.
NATURE OF COVALENT AND DATIVE COVALENT BONDS
Non-metals atoms need to receive electrons to fill the spaces in their outer shells.
A covalent bond forms between a pair of non-metal atoms.
BONDING 2
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