Chemical Structure Of Hydrogen Bonds

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Introduction Water ( ) has a simple molecular structure. It is composed of one oxygen atom and two hydrogen atoms. The water properties are, adhesive forces, cohesive forces, it is a universal solvent, also has a boiling point of 100°C and has a freezing point of 0°C. Adhesive forces are the attractive forces between unlike molecules. Dipole – dipole is a common type of adhesive force. Dipole – dipole forces account for water being attracted to most substances. Dipole – dipole forces are attractions and repulsion between polar moles. These are forces that attract partial positive and negative charge. Dipole – dipole interactions and dipole – ionic interactions accounts for solubility of substances in water. A special type of dipole – dipole interaction is hydrogen bonds. Cohesive forces are intermolecular forces such has those from hydrogen bonding which cause a tendency in liquids to resist separation. Cohesive forces exist between molecules of the same substance. Hydrogen bonds occur when hydrogen is bonded with either a nitrogen, oxygen or fluorine. So in water hydrogen is bonds with oxygen. Hydrogen bonds accounts for water molecules being attracted to each other. Water molecules consist of two hydrogen atoms bonded to an oxygen atom, and its overall structure is bent, form a V shape. This is because the oxygen atom, in addition to forming bonds with the hydrogen atoms, also carries two pairs of unshared electrons. Due to this hydrogen bonds water has a high melting
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