Question e03c2. Question d. Question Question 79c1f. Question 79c Every solid, liquid, gas, and plasma is composed of neutral or ionized atoms.
The chemical properties of the atom are determined by the number of protons, in fact, by number and arrangement of electrons. It is the Pauli exclusion principle that requires the electrons in an atom to occupy different energy levels instead of them all condensing in the ground state.
This fact has key implications for the building up of the periodic table of elements. The first two columns on the left side of the periodic table are where the s subshells are being occupied. Because of this, the first two rows of the periodic table are labeled the s block. Similarly, the p block are the right-most six columns of the periodic table, the d block is the middle 10 columns of the periodic table, while the f block is the column section that is normally depicted as detached from the main body of the periodic table.
It could be part of the main body, but then the periodic table would be rather long and cumbersome. For atoms with many electrons, this notation can become lengthy and so an abbreviated notation is used. The electron configuration can be visualized as the core electrons, equivalent to the noble gas of the preceding period, and the valence electrons e. Oxidation states are typically represented by integers which may be positive, zero, or negative.
Most elements have more than one possible oxidation state. An element that is not combined with any other different elements has an oxidation state of 0.
Oxidation state 0 occurs for all elements — it is simply the element in its elemental form. An atom of an element in a compound will have a positive oxidation state if it has had electrons removed. Similarly, adding electrons results in a negative oxidation state. We have also distinguish between the possible and common oxidation states of every element. Main Menu. 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. Relative supply risk 3. 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 Sulfur Podcast Transcript :.
You're listening to Chemistry in its element brought to you by Chemistry World , the magazine of the Royal Society of Chemistry. Hello, this week stinky sediments, skunks and the smell of hell.
Well they all begin with the letter S, and so does this week's element. Here's Steve Mylon. The smell of the sediment tells a great deal about the underlying chemistry. Thick black anoxic sediments can be accompanied by a putrid smell which is unique to reduced sulfur. Maybe this is why sulfur has such a bad reputation. My son wouldn't eat eggs for 6 months when he got a smell of his first rotten one. In the bible it seems that whenever something bad happens or is about to happen burning sulfur is in the picture:.
And in Revelation we read that the sinners will find their place in a fiery lake of burning sulfur. The odd thing is that in both cases we shouldn't expect anything smelly to be produced.
When sulfur burns in air, it generally forms sulfur dioxide or sulfur trioxide, the latter of which lacks any smell [amended from the podcast audio file, which states that sulfur dioxide does not smell].
These compounds can further oxidize and rain out as sulfuric or sulfurous acid. This is the mechanism for acid rain which has reeked havoc on the forests of the northeastern United States as sulfur rich coals are burned to generate electricity in midwestern states and carried east by prevailing winds where sulfuric acid is rained out causing all sorts of ecological problems.
Additionally, the combination of burning coal and fog creates smog in many industrial cities causing respiratory problems among the locals. Here too, sulfur dioxide and sulfuric acid are implicated as the culprits. But again, there is no smell associated with this form of sulfur. But reduce sulfur by giving it a couple of electrons, and its smell is unmistakable. The requirement of sulfur reduction to sulfide has clearly been lost in translation.
Hell that smells like hydrogen sulfide or any number of organic-sulfur compound will not be a nice place at all. The organic sulfide compounds known as thiols or mercaptans smell so bad, that they are commonly added to odorless natural gas in very small quantities in order to serve as a 'smell alarm' should there be leak in a natural gas line. Skunks take advantage of the foul smell of butyl seleno-mercaptan as a means of defending themselves against their enemies.
And for me, personally, the worst chemistry of all occurs when reduced sulfur imparts a bad skunky taste in bottles of wine or beer. So, where does the "smell of hell" come from in anoxic sediments.
Interestingly, some bacteria have evolved to make use of oxidized sulfur , sulfate, as an electron acceptor during respiration. In a similar manner to the way humans reduce elemental oxygen to water, these bacteria reduce sulfate to hydrogen sulfide- They clearly don't mind the smell. Smell is not the only interesting chemistry that accompanies reduced sulfur.
The deep black associated with anoxic sediments results from the low solubility of most metal sulfides. Sulfate reduction to sulfide generally accompanies the precipitation of pyrite iron sulfide , cinnabar mercury sulfide , galena lead sulfide and many more minerals. These metal sulfides have become an important industrial source for many of these important metals.
Industry is one place you are almost certain to find sulfur or more importantly sulfuric acid which is used in processes ranging from fertilizer production to oil refining. In fact sulfuric acid ranks as the most highly produced chemical in the industrialized world.
Imagine that, the element with such a hellish reputation has become one of the most important. And some even suggest that sulfur could save the planet. The biogenic compound dimethylsulfide DMS is produced from the cleavage of dimethylsufonoprioponate, an osmotic regulatory compound produced by plankton in the ocean. DMS is oxidized to SO2 and finally to sulfuric acid particles which can act as cloud condensation nuclei forming clouds which have a net cooling effect to the planet.
Imagine warmer temperatures followed by greater biological activity resulting in more DMS to the atmosphere. The resulting cloud formation might work to cool a warming planet. It's almost like the plankton are opening an umbrella made up-in part- of sulfur. From a symbol of damnation to savior Steve Mylon sniffing out the stinky story of Sulfur. Thankfully next week's element is a lot less odiforous.
The story of its discovery started when Rayleigh found that the nitrogen extracted from the air had a higher density than that made by decomposing ammonia. The difference was small but real. Ramsay wrote to Rayleigh suggesting that he should look for a heavier gas in the nitrogen got from air, while Rayleigh should look for a lighter gas in that from ammonia. Ramsay removed all the nitrogen from his sample by repeatedly passing it over heated magnesium.
He was left with one percent which would not react and found it was denser than nitrogen. Its atomic spectrum showed new red and green lines, confirming it a new element. When we write the configuration we'll put all 16 electrons in orbitals around the nucleus of the Sulfur atom. In writing the electron configuration for Sulfur the first two electrons will go in the 1s orbital.
Since 1s can only hold two electrons the next 2 electrons for sulfur go in the 2s orbital.
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