The reason this happens is because the slightly positive and slightly negative sides of water interact with the positive and negative ions of sodium and chloride, allowing the sodium and chloride to break up. When hydrogen and oxygen combine into a water molecule, the hydrogenatoms and the oxygen atoms share some of their electrons. But theoxygen atom holds the electrons tighter than the hydrogen atom. Thismakes a water molecule where the oxygen atom has a bit of a negativecharge, and the hydrogen atoms have bits of positive charge.
So thenthe water molecules are attracted to each other, so that the positivecharge on the hydrogen atoms are near the negative charges on theoxygen atoms. In hydrogen gas and oxygen gas, the 2 atoms in a molecule share theelectrons equally, so there aren't different charges on the differentsides of the molecules. The interactions between hydrogen and oxygen on different moleculesare called 'hydrogen bonds.
For example, hydrogen bonds hold the 2 DNA strands together inthe double helix in all our chromosomes. Hydrogen and oxygen are only gasses at the temperature and pressure you're used to dealing with them on - cool them down, and they become liquids, and even freeze and become solids. Heat them up enough and they will become plasmas. The same is true for water, except that at room temperature and sea-level pressure, water can exist as either a liquid or as a gas.
The reason for the much higher boiling and freezing points for water is that the oxygen atoms in water accumulate negative electric charge, while the hydrogen atoms accumulate positive electric charge. Because opposite charges attract, the molecules can orient themselves into chains, fit together like building blocks to become crystals, etc. This means that you really have to heat water up a lot in order to break up the crystal structure that is ice, and heat it up even more to break up the chains that make liquid water.
By contrast, it takes very little heat to break up the poorly held-together crystal structure of oxygen or hydrogen - so much so that there is nowhere on Earth cold enough naturally to have these two substances in liquid, let alone solid, form. Go to Pluto, however, and you might find your oxygen turning to a liquid. If water is made up of hydrogen and oxygen, two gasses, then how is it a liquid? Answer 1: Hydrogen and oxygen are elements. Answer 3: Water isnt just a liquid, but in fact water can exist in three different states: solid, liquid, or gas.
Answer 4: Great question. Answer 5: I like your thoughtful question. When a molecule, like water, has slightly different charges on 2sides, that's called a 'dipole. Image explanation. The image represents the fundamental importance of the element in air and, when bonded to hydrogen, in water.
The greatest commercial use of oxygen gas is in the steel industry. Large quantities are also used in the manufacture of a wide range of chemicals including nitric acid and hydrogen peroxide.
It is also used to make epoxyethane ethylene oxide , used as antifreeze and to make polyester, and chloroethene, the precursor to PVC. Oxygen gas is used for oxy-acetylene welding and cutting of metals. A growing use is in the treatment of sewage and of effluent from industry. Biological role. Photosynthesis uses energy from the sun to split water into oxygen and hydrogen.
The oxygen passes into the atmosphere and the hydrogen joins with carbon dioxide to produce biomass. When living things need energy they take in oxygen for respiration. The oxygen returns to the atmosphere in the form of carbon dioxide.
Oxygen gas is fairly soluble in water, which makes aerobic life in rivers, lakes and oceans possible. Natural abundance. The element and its compounds make up There are two key methods used to obtain oxygen gas. The first is by the distillation of liquid air. The second is to pass clean, dry air through a zeolite that absorbs nitrogen and leaves oxygen. A newer method, which gives oxygen of a higher purity, is to pass air over a partially permeable ceramic membrane.
In the laboratory it can be prepared by the electrolysis of water or by adding a manganese IV oxide catalyst to aqueous hydrogen peroxide. Help text not available for this section currently.
Elements and Periodic Table History. This was oxygen although it was not identified as such. The credit for discovering oxygen is now shared by three chemists: an Englishman, a Swede, and a Frenchman.
Joseph Priestley was the first to publish an account of oxygen, having made it in by focussing sunlight on to mercuric oxide HgO , and collecting the gas which came off. He noted that a candle burned more brightly in it and that it made breathing easier. He had written an account of his discovery but it was not published until Atomic data.
Bond enthalpies. Glossary Common oxidation states The oxidation state of an atom is a measure of the degree of oxidation of an atom. Oxidation states and isotopes. Glossary Data for this section been provided by the British Geological Survey.
Relative supply risk An integrated supply risk index from 1 very low risk to 10 very high risk. Recycling rate The percentage of a commodity which is recycled.
Substitutability The availability of suitable substitutes for a given commodity. Reserve distribution The percentage of the world reserves located in the country with the largest reserves. Political stability of top producer A percentile rank for the political stability of the top producing country, derived from World Bank governance indicators.
Political stability of top reserve holder A percentile rank for the political stability of the country with the largest reserves, derived from World Bank governance indicators. Supply risk. Young's modulus A measure of the stiffness of a substance. Shear modulus A measure of how difficult it is to deform a material. Bulk modulus A measure of how difficult it is to compress a substance. Vapour pressure A measure of the propensity of a substance to evaporate. Pressure and temperature data — advanced.
Listen to Oxygen Podcast Transcript :. You're listening to Chemistry in its element brought to you by Chemistry World , the magazine of the Royal Society of Chemistry.
And welcome to Chemistry in its element, where we take a look at the stories behind the elements that make up the world around us. I'm Chris Smith. This week, we are continuing our tour of the periodic table with a lung full of a gas that we can't do without. It protects us from solar radiation, it keeps us alive and by helping things to burn, it also keeps us warm.
It is of course oxygen. And to tell its story, here's Mark Peplow. Little did those humble cyanobacteria realize what they were doing when two and a half billion years ago, they started to build up their own reserves of energy-rich chemicals, by combining water and carbon dioxide. Powered by sunlight, they spent the next two billion years terraforming our entire planet with the waste products of their photosynthesis, a rather toxic gas called oxygen.
In fact, those industrious bugs are ultimately responsible for the diversity of life, we see around us today. Overall, it's the most abundant element on the earth's surface and the third most abundant in the universe after hydrogen and helium.
Oxygen is also in virtually every molecule in your body including fats, carbohydrates and DNA. In particular, it's the atom that links together the phosphate groups in the energy-carrying molecule ATP.
Oxygen is obviously pretty useful for keeping us going, but is also widely used in industry as an oxidant, where it can give up some of that solar energy captured by plant and those cyanobacteria.
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