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Bonding and structure: Chapter 3 Part 3 - Coggle Diagram
Bonding and structure
:
Chapter 3
Part 3
Cont. Other covalent compounds:
Carbon dioxide (CO2):
Stable electronic configurations are achieved by
forming 2 double covalent bonds
in which two pairs of electrons are shared in each case, as shown in the figure.
It forms a
linear molecule
(atoms lie in a straight line)- This is because the
bonding pairs repel.
Ethene (C2H4): Each carbon gets 4 paired electrons.
Methanol (CH3OH):
Pointers about Covalent Compounds:
Ionic bonds are stronger than covalent bonds.
Ionic bonds are formed between ions, whereas
covalent bonds are formed between atoms.
Intramolecular bonds are bonds between the atoms of a molecule.
Intermolecular bonds are bonds between the molecules.
Intramolecular bonds are stronger than intermolecular bonds.
Covalent compounds have
lower melting and boiling points
than ionic compounds since their
intermolecular bonds are weak.
Giant covalent compounds
have very big covalent structures. Thus bonds are stronger and they have
high melting and boiling points.
Properties of covalent compounds:
Covalent compounds are
usually gases
.
Giant covalent compounds have high melting and boiling point.
Covalent compounds, even when molten or dissolved in water, do not conduct electricity
since they are in their atomic form. One exception is Hydrogen chloride.
Covalent compounds
cannot be dissolved in water
.
Melting and boiling point is low
because of the weak intermolecular forces of attraction.