Anomalous properties, water, properties of water, polar molecule, particles
Water may seem like a very simple molecule, but in fact it has many anomalies. These make it hard to predict the properties of water. This essay will explain just a few of its unusual properties.
[...] This is why ice is able to float on water. References; Structure of a water molecule- www.ausetute.com.au/shapemol.html Polar molecules- www.biology-online.org/dictionary/polar_molecule Anomalous properties of water- www.hcli.com/anomalous-and-unique- properties-of-water/ Polarity and structure of molecules- OCR AS Chemistry (Heinemann) repel each other as well as the lone pairs of electrons, and as lone pair- lone pair repulsion is greater than lone pair-bonding pair or bonding pair- bonding pair repulsion, the lone pairs push the bonding pairs of electrons close together. This results in the molecule having a bent tetrahedral shape lone pairs slight negative charge around the oxygen atom. [...]
[...] These make it hard to predict the properties of water. This essay will explain just a few of its unusual properties. Water, H2O, is composed of 3 atoms which are covalently bonded- 2 atoms of hydrogen and 1 atom of oxygen. The central atom is oxygen, which has 6 electrons in its outer shell, otherwise known as valence electrons of these electrons are used to form bonding pairs with hydrogen, forming 2 covalent bonds (as one pair is used from the hydrogen) lone pairs of electrons are formed as 4 of oxygen's valence electrons are not used for bonding. [...]
[...] Most molecules only have to overcome the weakly attractive van der Waals' forces before melting/boiling can occur. However, the hydrogen bonds present in water are an additional force that must be overcome before melting/boiling can occur. In almost all other materials, the solid is denser than the liquid, with the particles in solids being packed tightly together. Water is the exception to this rule, as ice is less dense than water. This is because of hydrogen bonds holding the water molecules apart in an open lattice structure. [...]
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