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And we all know that the boiling point of water is 100°C. So despite its small molecular weight, water has an incredibly big boiling point. This is because water requires more energy to break its hydrogen bonds before it can then begin to boil.
- Structure of Water
Water is a simple molecule consisting of one oxygen atom...
- Structure of Water
Water is a simple molecule consisting of one oxygen atom bonded to two different hydrogen atoms. Because of the higher electronegativity of the oxygen atom, the bonds are polar covalent ( polar bonds ).
Two hydrogen atoms form a bond with a single atom of oxygen. Appearance: Water is colorless, odorless and tasteless liquid in its natural state. Boiling Point: As we know, water has a boiling point of 100 C. But this relatively high boiling point of water defies the trend in the periodic table.
The water molecule, visualized three different ways: ball-and-stick model, space-filling model, and structural formula with partial charges. The bent shape of the water molecule is critical because the polar O-H bonds do not cancel one another and the molecule as a whole is polar.
As a general rule "like dissolves like" so polar molecules are soluble in polar solvents (such as water) and vice-versa. For Higher Chemistry, revise the ways that elements are held together and...
In water, each hydrogen nucleus is bound to the central oxygen atom by a pair of electrons that are shared between them; chemists call this shared electron pair a covalent chemical bond. In H 2 O, only two of the six outer-shell electrons of oxygen are used for this purpose, leaving four electrons which are organized into two non-bonding pairs.
Water has unusually high melting and boiling points (0°C and 100°C, respectively) for such a small molecule. The boiling points for similar-sized molecules, such as methane (BP = −162°C) and ammonia (BP = −33°C), are more than 100° lower.
