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- Water molecules are polar and hydrogen bonds form between them
- Hydrogen bonds and bipolarity explain the cohesive, adhesive, thermal and solvent properties of water
- Substances can be hydrophilic or hydrophobic
Hydrogen bonds are relatively stronger than other polar associations due to the high electronegativity of O
Hydrogen bonds are relatively stronger than other polar associations due to the high electronegativity of O
Water is described as being polar because it has a slight charge difference across the different poles of the molecule
- The oxygen atom is slightly negative (δ–) while the hydrogen atoms are slightly positive (δ+)
This charge difference across the molecule (dipole) allows water to form weak associations with other polar molecules
- The slightly negative poles (δ–) will attract the slightly positive poles (δ+) of other molecules, and vice versa
The dipolarity of a water molecule enables it to form polar associations with other charged molecules (polar or ionic)
Water can form hydrogen bonds with other water molecules (between a δ+ hydrogen and a δ– oxygen of two molecules)
This intermolecular bonding between water molecules gives water distinct properties not seen in other substances:
- Thermal properties – Water can absorb much heat before changing state (requires breaking of hydrogen bonds)
- Cohesive / adhesive properties – Water will ‘stick’ to other water molecules (cohesion) and charged substances (adhesion)
- Solvent properties – Water dissolves polar and ionic substances (forms competing polar associations to draw materials apart)
Properties of Water that are Biologically Significant
Properties of Water that are Biologically Significant
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