Chemical properties of water

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1. Hydrogen Bonds: Water is a polar molecule that tends to be slightly positive on the hydrogen side and slight negative on the oxygen side.  The electrostatic bond between the positive hydrogen side of this molecule and other megative ions or polar molecules is called a hydrogen bond. Molecules and ions with which water forms hydrogen bonds (such as sodium chloride) are hydrophylic. On the other hand, Ions and molecules that do not form hydrogen bonds with water are hydrophobic.
2. Liquidity at Room Temperature: At room temperature, most compounds with low molecular weights take gaseous form. With water, however, hydrogen bonding helps to keep it a liquid at room temperature. Kept relatively close together, the moluecules at room temperature are unable to dissipate sufficiently to form a gas. Temperatures of 212°F (or 100°C) are required to break the hydrogen bonds and convert liquid water into water vapor.
3. Chemical Reactions: When ionic compounds such as sodium chloride are added to water, hydrogen bonding will tend to pull those ionic compounds apart. This makes water a natural solvent. Once ionic compounds dissolve, their anions and cations circulate through the water allowing further reactions to occur. Thus, water also sponsors and facilitates chemical reactions.
4. Stable Temperatures: Water takes more heat to raise its temperature than other common compounds, since much of that heat is required to first break the hydrogen bonds. Water also retains heat, so its temperature falls slowly. This means that larger systems of water (such as the ocean or a body) tend to maintain more or less constant temperatures, which in turn helps the earth (and us) to maintain relatively constant temperatures.
5. Freezing Point :At 32°F (or 0°C) and below, water molecules form hydrogen bonds in a chrystalline lattice structure. This bonding spaces the molecules a bit farther apart than usual, causing water to expand when it freezes. This results in ice being less dense than liquid water, which is why ice floats.

Chemical formula H 2OMolar mass18.01528(33) g/molAppearanceWhite solid or almost colorless, transparent, with a slight hint of blue, crystalline solid or liquid[2]OdorNoneDensityLiquid:[3] 0.9998396 g/mL at 0 °C 0.9970474 g/mL at 25 °C 0.961893 g/mL at 95 °C Solid:[citation needed] 0.917 g/ml ≈ 57.2 lb/ft3Melting point0.00 °C (32.00 °F; 273.15 K) [a]Boiling point99.98 °C (211.96 °F; 373.13 K) [4][a]SolubilityPoorly soluble inhaloalkanes,aliphatic andaromatichydrocarbons,ethers.[5] Improved solubility incarboxylates,alcohols, ketones,amines. Miscible with methanol, propanol,isopropanol, glycerol,1,4-dioxane,tetrahydrofuran,acetaldehyde,dimethylformamide,dimethoxyethane,dimethyl sulfoxide.Vapor pressure3.1690 kilopascals or 0.031276 atm[6]Acidity (pKa)13.995[7][b]Basicity (pKb)13.995Thermal conductivity0.6065 W/m·K[9] Refractive indexD) 1.3330 (20°C)[10]