Dipoles / dipole molecules

The following image has been seen before:

Molecules can contain one or more polar bonds, and they can yes or no be a dipole.
That depends on the symmetry of the molecules (look at the examples)

Examples:
CS2 (ΔE = ±0) CO2 (ΔE = ±1.0) H2O (ΔE = ±1.3)
Covalent bond Covalent bond Covalent bond
Non polar molecules Non polar molecules Polar molecules
there is no dipole there is no dipole Dipole
There are no δ+ and δ- There are δ+ and δ-; they overlap
the centre points
of each other		 The central points of δ+ and δ- do not
overlap each other
(remain at a distance)
S=C=S
O = C = O
δ-   δ+   δ-
δ+       δ+
H      H
\     /
  O
  δ-


molecules of CCl4 and CH2Cl2

In general, polar substances will attract each other, and dissolve in polar solvents (e.g. sugar in water).
The same way we can say that non polar substances do also attract each other and dissolve in each other (like fat in oil).
Polar and non polar substances do not mix.
More about this in module 5.

A water molecule has no linear, but a triangle structure. The three atoms have not a position in one line. This little difference has an enormous impact in our world. Imagine that the water molecule would be linear. How about the consequences for our world?
Suppose a watermolecule would be linear: the two H atoms and the O atom all on one line. Than this symmetrical molecule as a whole would not be polar, would not be a dipole.
The attraction between the water molecules would be less than between the triangle molecules.
With much less attraction, these watermolecules (very small and light) would be no longer a liquid, but a gas, just like carbondioxyde.
conclusion: there would not be any see, river, rain, no life at all.