What type of representative particle is sulfur

In a multi-step problem, be sure that the units check. Work the practice problems at the link below. Focus on conversions between volume and moles, but try some of the others:. Why does carbon dioxide sink in air? When we run a reaction to produce a gas, we expect it to rise into the air. Many students have done experiments where gases such as hydrogen are formed.

The gas can be trapped in a test tube held upside-down over the reaction. Carbon dioxide, on the other hand, sinks when it is released.

Carbon dioxide has a density greater that air, so it will not rise like these other gases would. As you know, density is defined as the mass per unit volume of a substance. Since gases all occupy the same volume on a per mole basis, the density of a particular gas is dependent on its molar mass. A gas with a small molar mass will have a lower density than a gas with a large molar mass. Gas density can be calculated from molar mass and molar volume.

Balloons filled with helium gas float in air because the density of helium is less than the density of air. What is the density of nitrogen gas at STP? Molar mass divided by molar volume yields the gas density at STP. Alternatively, the molar mass of a gas can be determined if the density of the gas at STP is known. What is the molar mass of a gas whose density is 0. Molar mass is equal to density multiplied by molar volume.

How do I get from here to there? If I want to visit the town of Manteo, North Carolina, out on the coast, I will need a map of how to get there. I may have a printed map or I may download directions from the internet, but I need something to get me going in the right direction. Chemistry road maps serve the same purpose.

How do I handle a certain type of calculation? There is a process and a set of directions to help. Previously, we saw how the conversions between mass and number of particles required two steps, with moles as the intermediate. This concept can now be extended to also include gas volume at STP. The resulting diagram is referred to as a mole road map see Figure below. The mole road map shows the conversion factors needed to interconvert between mass, number of particles, and volume of a gas.

The mole is at the center of any calculation involving amount of a substance. The sample problem below is one of many different problems that can be solved using the mole road map.

What is the volume of The given mass of neon is equal to about 4 moles, resulting in a volume that is about 4 times larger than molar volume.

Use the link below to carry out some practice calculations. Do problems 1, 2, and 5 you can try the others if you are feeling especially brave :. Is there anything healthy in this jar? Packaged foods that you eat typically have nutritional information provided on the label. The label on a jar of peanut butter shown above reveals that one serving size is considered to be 32 g.

The label also gives the masses of various types of compounds that are present in each serving. One serving contains 7 g of protein, 15 g of fat, and 3 g of sugar. By calculating the fraction of protein, fat, or sugar in one serving of size of peanut butter and converting to percent values, we can determine the composition of the peanut butter on a percent by mass basis.

Chemists often need to know what elements are present in a compound and in what percentage. The percent composition is the percent by mass of each element in a compound. It is calculated in a similar way that we just indicated for the peanut butter. The sample problem below shows the calculation of the percent composition of a compound based on mass data.

A certain newly synthesized compound is known to contain the elements zinc and oxygen. When a Determine the percent composition of the compound. Subtract to find the mass of oxygen in the compound. By mass, the compound is mostly zinc. The percent composition of a compound can also be determined from the formula of the compound.

The subscripts in the formula are first used to calculate the mass of each element in one mole of the compound. The percent composition of a given compound is always the same as long as the compound is pure. Dichlorineheptoxide Cl 2 O 7 is a highly reactive compound used in some organic synthesis reactions. Calculate the percent composition of dichlorineheptoxide.

Percent composition can also be used to determine the mass of a certain element that is contained in any mass of a compound. In the previous sample problem, it was found that the percent composition of dichlorineheptoxide is Suppose that you needed to know the masses of chlorine and oxygen present in a You can set up a conversion factor based on the percent by mass of each element. The sum of the two masses is Use the link below to review material and do calculations.

Read both parts of the lesson and do as many calculations as you have time for. Why does the color change? If you look at a typical bottle of copper sulfate, it will be a bluish-green. You are both right; it just depends on the copper sulfate.

Why the difference? The water molecules interact with some of the d electrons in the copper ion and produce the color. When the water is removed, the electron configuration changes and the color disappears. Many ionic compounds naturally contain water as part of the crystal lattice structure.

A hydrate is a compound that has one or more water molecules bound to each formula unit. Ionic compounds that contain a transition metal are often highly colored. Interestingly, it is common for the hydrated form of a compound to be of a different color than the anhydrous form, which has no water in its structure.

A hydrate can usually be converted to the anhydrous compound by heating. For example, the anhydrous compound cobalt II chloride is blue, while the hydrate is a distinctive magenta color. On the left is anhydrous cobalt II chloride, CoCl 2. The hydrated form of cobalt II chloride contains six water molecules in each formula unit. The formula for water is set apart at the end of the formula with a dot, followed by a coefficient that represents the number of water molecules per formula unit.

It is useful to know the percent of water contained within a hydrate. The sample problem below demonstrates the procedure. The mass of water in the hydrate is the coefficient 6 multiplied by the molar mass of H 2 O.

The molar mass of the hydrate is the molar mass of the CoCl 2 plus the mass of water. Nearly half of the mass of the hydrate is composed of water molecules within the crystal. Use the following link to practice calculating percent water in a hydrate:.

What is occuring in this picture? In the early days of chemistry, there were few tools for the detailed study of compounds. Much of the information regarding the composition of compounds came from the elemental analysis of inorganic materials.

The relative amounts of elements could be determined, but so many of these materials had carbon, hydrogen, oxygen, and possibly nitrogen in simple ratios.

We did not know exactly how many of these atoms were actually in a specific molecule. An empirical formula is one that shows the lowest whole-number ratio of the elements in a compound. Because the structure of ionic compounds is an extended three-dimensional network of positive and negative ions, all formulas of ionic compounds are empirical. However, we can also consider the empirical formula of a molecular compound.

Ethene is a small hydrocarbon compound with the formula C 2 H 4 see Figure below. While C 2 H 4 is its molecular formula and represents its true molecular structure, it has an empirical formula of CH 2.

The simplest ratio of carbon to hydrogen in ethene is There are two ways to view that ratio. Considering one molecule of ethene, the ratio is 1 carbon atom for every 2 atoms of hydrogen. Considering one mole of ethene, the ratio is 1 mole of carbon for every 2 moles of hydrogen. So the subscripts in a formula represent the mole ratio of the elements in that formula.

Ball-and-stick model of ethene, C 2 H 4. In a procedure called elemental analysis , an unknown compound can be analyzed in the laboratory in order to determine the percentages of each element contained within it.

These percentages can be transformed into the mole ratio of the elements, which leads to the empirical formula. The steps to be taken are outlined below. A compound of iron and oxygen is analyzed and found to contain Find the empirical formula of the compound. Steps to follow are outlined in the text. Divide both moles by the smallest of the results.

Since the moles of O, is still not a whole number, both moles can be multiplied by 2, while rounding to a whole number. The empirical formula of the compound is Fe 2 O 3. The subscripts are whole numbers and represent the mole ratio of the elements in the compound.

The compound is the ionic compound iron III oxide. Use the link below to read about calculating empirical formulas and practice working some problems:. How can you determine the differences between these two molecules? Above we see two carbohydrates: glucose and sucrose.

Sucrose is almost exactly twice the size of glucose, although their empirical formulas are very similar. The best way is to determine the molecular weights — this approach allows you to easily tell which compound is which. Molecular formulas give the kind and number of atoms of each element present in a molecular compound. The subatomic particles in an atom determine the properties of the atom. Some atoms exist naturally as neutral, or uncharged, atoms.

An uncharged atom is electrically neutral because electrons and protons have opposite charges of equal sizes. When the number of protons and electrons in an atom are same, the charges cancel out, or counteract each other. Every atom of a particular element has the same number of protons. The atomic number is equal to the number of protons in an element. On the periodic table, the atomic number is usually given as the whole number above the symbol for the element see Fig.

For example, hydrogen H has an atomic number of one 1. This means a hydrogen atom has one proton. If a hydrogen atom is neutral, it must also have one electron. An oxygen atom O has an atomic number of eight 8. This means a neutral oxygen atom has eight protons and eight electrons. The element Actium Ac has an atomic number of 89, so it has 89 protons and 89 electrons in a neutral atom. Table 2. Neutrons affect the mass of an atom and play a role in the stability of atoms.

Unlike protons, the numbers of neutrons in elements varies. For example, most hydrogen atoms have no neutrons, but a few have one neutron, and some rare hydrogen atoms have two neutrons. Most helium atoms have two neutrons, but some have three neutrons. The periodic table Fig. In Fig. In Figure 2. The periodic table has three prominent features.

First, the periodic table is arranged in horizontal rows, which are called periods. There are seven periods.

In Period 1 there are two elements, hydrogen H and helium He. The second and third periods both contain eight elements, the fourth and fifth periods contain 18 elements, and the sixth and seventh periods contain 32 elements.

Second, all of the elements are listed sequentially according to their atomic numbers. For example, in Figure 2. Third, the periodic table is arranged in columns of elements that react similarly. These columns are called groups. The group number is found at the top of the column. Groups 1—12 contain only metals, Groups 13—16 contain both metals and nonmetals, and Groups 17 and 18 contain only nonmetals.

One exception is hydrogen. Although technically a nonmetal, hydrogen has properties of both metals and nonmetals and is often placed in Group 1. The two long rows that are at the bottom of the periodic table are exceptions.

The elements in each of these rows behave similarly, so are considered groups. These two groups are arranged in rows rather than columns. Metals are elements that conduct heat and electricity. Metals are usually malleable , they can be bent or molded without breaking, and lustrous , or shiny. Most metals are silvery in color Fig. Most metals are solid at room temperature. One exception is mercury Hg , which is a liquid at room temperature Fig.

The elements in Group 1, including lithium Li , sodium Na, Fig. These metallic Group 1 elements have similar reactive properties. 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. And that new element was Argon nicknamed the lazy element because originally scientists thought that it wouldn't react with anything.

Now we know that's not true and John Emsley will be here to unlock Argon secrets on next week's Chemistry in its Element, I hope you can join us. I'm Chris Smith, thank you for listening and goodbye. Chemistry in its element is brought to you by the Royal Society of Chemistry and produced by thenakedscientists.

There's more information and other episodes of Chemistry in its element on our website at chemistryworld. Click here to view videos about Sulfur. View videos about. Help Text. Learn Chemistry : Your single route to hundreds of free-to-access chemistry teaching resources. We hope that you enjoy your visit to this Site.

We welcome your feedback. Data W. Haynes, ed. Version 1. Coursey, D. Schwab, J. Tsai, and R. Dragoset, Atomic Weights and Isotopic Compositions version 4. Periodic Table of Videos , accessed December Podcasts Produced by The Naked Scientists. Download our free Periodic Table app for mobile phones and tablets.

Explore all elements. D Dysprosium Dubnium Darmstadtium. E Europium Erbium Einsteinium. F Fluorine Francium Fermium Flerovium. G Gallium Germanium Gadolinium Gold. I Iron Indium Iodine Iridium. K Krypton. O Oxygen Osmium Oganesson. U Uranium. V Vanadium. X Xenon. Y Yttrium Ytterbium. Z Zinc Zirconium. Membership Become a member Connect with others Supporting individuals Supporting organisations Manage my membership.

Facebook Twitter LinkedIn Youtube. Discovery date. Discovered by. Origin of the name. The name is derived either from the Sanskrit 'sulvere', or the Latin 'sulfurium'. Melting point. Boiling point. Atomic number.

Relative atomic mass. Key isotopes.