Inorganic Chemistry Assignment

Inorganic Chemistry Assignment Words: 3524

The Inorganic Chemistry of Carbon Inorganic Carbon For more than 200 years, chemists have divided compounds into two categories. Those that were isolated from plants or animals were called organic, while those extracted from ores and minerals were inorganic. Organic chemistry is often defined as the chemistry of carbon. But this definition would include calcium carbonate (Cacao) and graphite, which more closely resemble inorganic compounds. We will therefore define organic chemistry as the study of compounds, such as formic acid (WHICH), methane (CHI), and vitamin C (CHICHI), that contain both carbon and hydrogen.

The chemistry of carbon is dominated by three factors. 1 . Carbon forms unusually strong C-C single bonds, C=C double bonds, and carbon- carbon triple bonds. 2. The electronegative of carbon (EN = 2. 55) is too small to allow carbon to form CA- ions with most metals and too large for carbon to form CA+ ions when it reacts with nonmetals. Carbon therefore forms covalent bonds with many other elements. 3. Carbon forms strong double and triple bonds with a number of other nonmetals, including N, O, P, and S. Elemental Forms of Carbon: Graphite, Diamond, Coke, and Carbon Black Carbon occurs as a variety of allotrope.

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There are two crystalline forms diamond and graphite a number of amorphous (neocolonialist) forms, such as charcoal, coke, and carbon black. References to the characteristic hardness of diamond (from the Greek Adams, “invincible”) date back at least 2600 years. It was not until 1797, however, that Smithson Tenant was able to show that diamonds consist solely of carbon. The properties of diamond are remarkable. It is among the least volatile substances known (PM = 35500C, BP = 48270C), it is also the hardest substance known, and it expands less on heating than any other material.

The properties of diamond are a logical consequence of its structure. Carbon, with four valence electrons, forms covalent bonds to four neighboring carbon atoms arranged toward the corners of a tetrahedron, as shown in the figure below. Each of these SSP-hybridism atoms is then bound to four other carbon atoms, which form bonds to four other carbon atoms, and so on. As a result, a perfect diamond can be thought of as a single giant molecule. The strength of the individual C-C bonds and their arrangement in space give rise to the unusual properties of diamond.

In some ways, the properties of graphite are like those of diamond. Both compounds boil at 48270C, for example. But graphite is also very different from diamond. Diamond (3. 514 g/cam) is much denser than graphite (2. 26 g/cam). Whereas diamond is the hardest substance known, graphite is one of the softest. Diamond is an excellent insulator, with little or no tendency to carry an electric current. Graphite is such a good conductor of electricity that graphite electrodes are used in electrical cells. The physical properties of graphite can be understood from the structure of the solid shown in the figure below.

Graphite consists to extended planes to SSP-inebriated carbon atoms in which each arbor is tightly bound to three other carbon atoms. (The strong bonds between carbon atoms within each plane explain the exceptionally high melting point and boiling point of graphite. ) The distance between these planes of atoms, however, is very much larger than the distance between the atoms within the planes. Because the bonds between planes are weak, it is easy to deform the solid by allowing one plane of atoms to move relative to another.

As a result, graphite is soft enough to be used in pencils and as a lubricant in motor oil. “Lead” pencils do not, incidentally, contain lead. This is fortunate because many people chew pencils and lead compounds are toxic. ) Lead pencils contain graphite, or “black lead” as it was once known, which is mixed with clay (20% to by weight) and then baked to form a ceramic rod. Increasing the percentage of clay makes the pencil harder, so that less graphite is deposited on the paper. The characteristic properties of graphite and diamond might lead you to expect that diamond would be more stable than graphite.

This is not what is observed experimentally. The standard enthalpy of formation of diamond (Hoff = 2. 425 k/mol) is slightly larger than the enthalpy of formation of rapier, which is the most stable form of carbon at ICC and 1 ATM pressure. At very high temperatures and pressures, diamond becomes more stable than graphite. In 1955 General Electric developed a process to make industrial-grade diamonds by treating graphite with a metal catalyst at temperatures of 2000 to 3000 K and pressures above 125,000 ATM. Roughly 40% of industrial-quality diamonds are now synthetic.

Although gem-quality diamonds can be synthesized, the costs involved are prohibitive. Both diamond and graphite occur as regularly packed crystals. Other forms of carbon roundhouses they lack a regular structure. Charcoal, carbon black, and coke are all amorphous forms of carbon. Charcoal results from heating wood in the absence of oxygen. To make carbon black, natural gas or other carbon compounds are burned in a limited amount of air to give a thick, black smoke that contains extremely small particles of carbon, which can be collected when the gas is cooled and passed through an electrostatic precipitated.

Coke is a more regularly structured material, closer in structure to graphite than either charcoal or carbon black, which is made from coal. Carbides: Covalent, Ionic, and Interstitial Although carbon is essentially inert at room temperature, it reacts with less electronegative negative elements at high temperatures to form compounds known as carbides. When carbon reacts with an element of similar size and electronegative, a covalent carbide is produced. Silicon carbide, for example, is made by treating silicon dioxide from quartz with an excess of carbon in an electric furnace at 2300 K.

Isis(S) SIC(S) 2 CO(g) Covalent carbides have properties similar to those of diamond. Both Sic and diamond are inert to chemical reactions, except at very high temperatures; both have ere high melting points; and boot are among the hardest substances known. Is was first synthesized by Edward Achaeans in 1891. Shortly thereafter, Achaeans founded the Corundum Company to market this material. Then, as now, materials in this class are most commonly used as abrasives. Compounds that contain carbon and one of the more active metals are called ionic carbides.

Cacao(s) ca(s) CO(g) It is useful to think about these compounds as if they contained negatively charged carbon ions: [Ca+][CA-] or [AAA+]4[CA-]3. This model is useful because it explains why these carbides burst into flame when added to water. The ionic carbides that formally contain the CA- ion react with water to form methane, which is ignited by the heat given off in this reaction. CA- CHI 4 OH- The ionic carbides that formally contain the CA- ion react with water to form acetylene, which is ignited by the heat of reaction.

CA- 2 H2O CASH At one time, miners’ lamps were fueled by the combustion of acetylene prepared from the reaction of calcium carbide with water. Interstitial carbides, such as tungsten carbide (WAC), form when carbon combines with a metal that has an intermediate electronegative and a relatively large atomic radius. In these compounds, the carbon atoms pack in the holes (interstices) between planes of metal atoms. The interstitial carbides, which include Tic, Cry, and MOCK retain the properties of metals. They act as alloys, rather than as either salts or covalent compounds.

The Oxides of Carbon Although the different forms of carbon are essentially inert at room temperature, they combine with oxygen at high temperatures to produce a mixture of carbon monoxide and carbon dioxide. 2 C(s) 02(g) HO = -1 10. 52 k,t-mol CO CA(g) HO = -393. 51 k/mol CA CO can also be obtained when red-hot carbon is treated with steam. C(s) H2O(g) H2O(g) Because this mixture of gases is formed by the reaction of charcoal or coke with water it is often referred to as water gas. It is also known as town gas because it was once made by towns and cities for use as a fuel.

Water gas, or town gas, was a common fuel for both home and industrial use before natural gas became readily available. The H2O burns to form water, and the CO is oxidized to CA. Eventually, as our supply of natural gas is depleted, it will become economical to replace natural gas with other fuels, such as water gas, that can be produced from our abundant supply of coal. CO and CA are both colorless gases. CO boils at -191. ICC, and CA sublimes at -78. ICC. Although CO has no odor or taste, CA has a faint, pungent odor and a distinctly acidic taste.

Both are dangerous substances but at very different levels of exposure. Air contaminated with as little as 0. 002 grams of CO per liter can be fatal because CO binds tightly to the hemoglobin and mycologist that carry oxygen through the blood. CA is not lethal until the concentration in the air approaches 15%. At that point, it has replaced so much oxygen that a person who attempts to breathe this atmosphere suffocates. The danger of CA poisoning is magnified by the fact that CA is roughly 1. 5 times more dense than the air in our atmosphere. Thus, CA can accumulate at the bottom of tanks or wells.

CA In the Atmosphere CA influences the temperature of the atmosphere through the greenhouse effect, which works as follows. CA absorbs some of the lower energy, longer wavelength infrared radiation from the sun that would otherwise be reflected back from the surface of the planet. Thus, CA in the atmosphere traps heat. Although there are other factors at work, it is worth noting that Venus, whose atmosphere contains a read deal of CA, has a surface temperature of roughly ICC, whereas Mars, with little or no atmosphere, has a surface temperature of -ICC.

There are many sources to CA in the atmosphere. Over geologic time scales, the largest source NAS been volcanoes. Within the last century, the combustion of petroleum, coal, and natural gas has made a significant contribution to atmospheric levels of CA (see figure below). Between 1958 and 1978, the average level of CA in the atmosphere increased by 6%, from 315. 8 to 334. 6 pump. At one time, the amount of CA released to the atmosphere was not a matter for once because natural processes that removed CA from the atmosphere could compensate for the CA that entered the atmosphere.

The vast majority of the CA liberated by volcanic action, for example, was captured by calcium oxide or magnesium oxide to form calcium carbonate or magnesium carbonate. Cacao(s) cacao(s) MGM(S) Magic(S) Cacao is found as limestone or marble, or mixed with Magic as dolomite. The amount of CA in deposits of carbonate minerals is at least several thousand times larger than the amount in the atmosphere. CA also dissolves, to some extent, in water. H2O CA(aqua) It then reacts with water to form carbonic acid, WHICH. H2O(l) WHICH(aqua) As a result of these reactions, the sea contains about 60 times more CA than the atmosphere.

Can the sea absorb more CA from the atmosphere, or is it near its level of saturation? Is the rate at which the sea absorbs CA greater than the rate at which we are adding it to the atmosphere? The observed increase in the concentration of CA in recent years suggests pessimistic answers to these two questions. A gradual warming of the earth’s atmosphere could result from continued increases in CA levels, Witt adverse detects on the climate and therefore the agriculture to at least the northern hemisphere. The Chemistry of Carbonates: CHIC- and HACK- Egg shells are almost pure calcium carbonate.

Cacao can also be found in the shells of many marine organisms and in both limestone and marble. The fact that none of these substances dissolve in water suggests that Cacao is normally insoluble in water. Calcium carbonate will dissolve in water saturated with CA, however, because carbonated water (or carbonic acid) reacts with calcium carbonate to form calcium bicarbonate, which is soluble in water. Cacao(s) ca+(aqua) 2 HACK-(aqua) When water rich in carbon dioxide flows through limestone formations, part of the mention dissolves.

If the CA escapes from this water, or if some of the water evaporates, solid Cacao is redeposit. When this happens as water runs across the roof of a cavern, stalactites, which hang from the roof of the cave, are formed. If the water drops before the carbonate repatriates,stalagmites, which grow from the floor of the cave, are formed. The chemistry of carbon dioxide dissolved in water is the basis of the soft drink industry. The first artificially carbonated beverages were introduced in Europe at the end of the nineteenth century.

Carbonated soft drinks today consist of carbonated water, a sweetening agent (such as sugar, saccharin, or aspartame), an acid to impart a sour or tart taste, flavoring agents, coloring agents, and preservatives. As much as 3. 5 liters of gaseous CA dissolve in a liter of soft drink. The Contributes the characteristic bite associated with carbonated beverages. Carbonate chemistry plays an important role in other parts of the food industry as well. Baking soda, or bicarbonate of soda, is sodium bicarbonate, Enhance, a weak base, which is added to recipes to neutralize the acidity of other ingredients.

Baking powder is a mixture of baking soda and a weak acid, such as tartaric acid or calcium hydrogen phosphate (Capped). When mixed with water, the acid reacts with the HACK- ion to form CA gas, which causes the dough or batter to nose. HACK-(aqua) Before commercial baking powders were available, cooks obtained the same effect by mixing roughly a teaspoon of baking soda with a cup of sour milk or buttermilk. The acids that give sour milk and buttermilk their characteristic taste also react with the bicarbonate ion to give CA.

Fullness In 1985 Richard Smaller and co-workers at Rice University made a uniquely stable Oromo of carbon by vaporizing graphite with a laser. The apparatus in which this experiment was performed was designed to create small molecules that were clusters of atoms. In this cluster generator, a pulse of helium gas was swept over the surface of the graphite as it was excited with the laser. The mixture of helium and carbon atoms that vaporized from the graphite surface cooled as the gas expanded, and molecules with the formula CA were formed that have a structure that has the symmetry of a soccer-ball.

Because this structure resembles the geodesic dome invented by R. Businessmen Fuller, CA was named buckminsterfullerene, or “Buckley” for short. Although it was formally a new form of pure carbon, CA seemed to be nothing more than a laboratory curiosity until 1990, when Wolfgang Scratchier and Sanitations Osteoporosis, at the Max Planck Institute in Heidelberg, reported that this material could be made by heating a graphite rod in an atmosphere of helium until the graphite evaporated.

Once it was known that CA could be synthesized in large quantities, researchers looked for, and found it, in such common sources as the flame of a soot candle. It has even been found in the lack soot that collects on the glass screen in front of a fireplace. Some of the excitement chemists experienced when CA was synthesized can be understood by contrasting this form of pure carbon with diamond and graphite. CA is unique because it exists as distinct molecules, not extended arrays of atoms.

Equally important, CA can be obtained as a pure substance, whereas the surfaces of diamond and graphite are inevitably contaminated by hydrogen atoms that bind to the carbon atoms on the surface. CA is now known to be a member of a family of compounds known as the fullness. Other compounds in this family include CA, CA, CA, CA, and CA. CA may be the most important of the fullness because it is the most perfectly symmetric molecule possible, spinning in the solid at a rate of more than 100 million times per second.

Because of their symmetry, CA molecules pack as regularly as Ping-Pong balls. The resulting solid has unusual properties. Initially, it is as soft as graphite, but when compressed by 30%, it becomes harder than diamond. When this pressure is released, the solid springs back to its original volume. CA therefore has the remarkable property that it bounces back when shot at a metal surface at high speeds. CA also has the remarkable ability to form compounds in which it is an insulator, a conductor, a semiconductor, or a superconductor. By itself, CA is a semiconductor.

When mixed with Just enough potassium to give a compound with the empirical formula KICKS, it conducts electricity like a metal. When excess potassium is added, this solid becomes an insulator. When KICKS is cooled to 18 K, the result is a superconductor. The potential of fulfiller chemistry for both practical materials and laboratory curiosities is large enough to explain why this molecule can be described as “exorcism” it exudes charm. Organic Chemistry Carbon is an especially noteworthy element in living systems. The chemistry to carbon, organic chemistry, is a complete study unto itself.

We will touch on several highlights that will be useful in succeeding sections. The Uniqueness of Carbon The carbon atom has four valence (outermost) electrons. Because of this unique configuration, it is easier for the carbon atom to share its four electrons with another atom or atoms than to lose or gain four electrons. Because each carbon is identical, they all have four valence electrons, so they can easily bond with other carbon atoms to form long chains or rings. In fact, a carbon atom can bond with another carbon atom two or three times to make double and triple covalent bonds between two carbon atoms.

Long chains of carbon atoms with double and triple bonds are quite common in biology. Carbon’s tendency toward covalent bonding with itself generates three unique characteristics that create a vast array of compounds, including those necessary to construct and support life: The single bond that connects carbon atoms to carbon atoms is quite strong, so the subsequent long chains and ring structures are not fragile. The carbon-carbon covalent bonding pattern satisfies the Octet rule, asking carbon compounds unwilling to react.

Because carbon has four valence electrons and needs eight to satisfy the Octet rule, it can bond with up to four additional atoms, creating countless compound possibilities. Functional Groups In the simplest terms, the reactive part of any compound is called the functional group. Normally a functional group is a collection of atoms that operates as one reactive unit and is also the part of the molecule involved in a chemical reaction. Whereas carbon-to-carbon bonds are nonrestrictive, the instability of the functional groups drives chemical reactions that involve stable carbon-based compounds.

For simplicity and reference, three functional groups are presented: Amine is identified by a central nitrogen atom that has three bonds, usually to hydrogen atoms. Amine groups form the basis for amino acids, which when bonded together form proteins. A Carboxylic group (COHO) is attached to the long carbon chains that form fatty acid molecules, which are a type of lipid lipids. Hydroxyl groups (OH) are very reactive. They are a component of alcohols, such as ethanol, the alcoholic component of adult beverages. The oxygen-hydrogen association is unique to this functional group and easily identifies it as an alcohol.

Dehydration Synthesis and Polymer Formation Bonnet A hydration reaction is the reverse of a dehydration reaction in that water serves as a reactant to split apart large poly-molecules. Polymers are small molecules that can be bonded together to create larger molecules. Complex carbohydrates are made from small simple sugars Joined together, and giant protein molecules are simply a series of smaller amino acid molecules bonded together. The prefix poly identifies this type of molecular addition. For instance, polysaccharides are large carbohydrates composed of multiple saccharine (sugar) units.

The chemical reaction that powers polymer formation is known by several names, including dehydration synthesis and condensation reaction. Regardless of the name, the molecules are Joined by bonding sites created when a positively charged hydrogen ion (H+) is lost from one molecule and a negatively charged hydroxide (OH-) ion is lost from a neighboring molecule. The H+ and OH- combine to form water. So a dehydration synthesis Joins two smaller units Togo The there Witt the loss to one water molecule. Chemistry Of Carbon Submitted By: Cycad O. Embank Submitted to: Janis, Jeanine Rose B.

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