Chemistry: What's Hot Now: Lightning Photograph

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Lightning Photograph Aug 25th 2011, 10:02 Lightning Photograph Charles Allison, Oklahoma Lightning This image was obtained from a NOAA website, but I recommend contacting the owner, Charles Allison, Oklahoma Lightning, before using this photo, particularly for commercial purposes. 13 of 162 Gallery Index: Science Pictures More Science Image Galleries Chemical StructuresElement PhotographsLab Safety Signs See More About: lightning electricity science pictures lightning photos static electricity Anne Marie Helmenstine, Ph.D. Chemistry Guide Sign up for My Newsletter

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Chemistry: This Day in Science History - August 25 - Herschell, Big Telescopes and Moon Creatures

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This Day in Science History - August 25 - Herschell, Big Telescopes and Moon Creatures Aug 24th 2011, 22:05 August 25th marks the passing of the English astronomer, Frederick William Herschel. He was one of the foremost English astronomers of the time. He constructed nearly 400 different telescopes, including the "Great Forty-Foot" reflecting telescope. It was the largest telescope in the world for 50 years. It had a 40 foot focal length and used a 48 inch mirror. Another August 25th event involved his son, John William Herschel. Beginning on August 25, 1835, six articles were published by the New York Sun newspaper describing John Herschel's observation of Moon creatures such as unicorns, bipedal beavers and bat-winged humanoids. The Great Moon Hoax was written by Richard A. Locke to increase circulation for the New York Sun. It wasn't exposed as a hoax for two weeks and no retraction was ever made. Herschel was initially amused by the stories, but grew tired of trying to explain to people he had nothing to do with it or denying the observations to people who believed the hoax. Find out what else occurred on this day in science history. Follow Chemistry on Facebook or Twitter.

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Chemistry: How to Use the Periodic Table

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How to Use the Periodic Table Aug 24th 2011, 09:52 The periodic table of the elements can be incredibly useful for chemistry, especially if you know what information is available and how to use it. The table isn't just for looking up element symbols and atomic weights. You can use it to predict the properties and reactions of the elements, too. How to Use the Periodic Table | Online Periodic Table

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Chemistry: How Blueprints Work

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How Blueprints Work Aug 24th 2011, 08:06 A blueprint is a paper-based reproduction of a drawing, usually a technical drawing, such as an architect or engineer would use. Blueprints use the cyanotype process that was invented by the astronomer John Herschel in 1842. The paper (or vellum or plastic) is coated with a solution of two soluble iron(III) salts - potassium hexacyanoferrate(III) (potassium ferricyanide) and iron(III) ammonium citrate. The two iron salts do not react with each other in the dark, but when they are exposed to ultraviolet light the iron(III) ammonium citrate becomes an iron(II) salt. The iron(II) ion reacts with the potassium ferricyanide to form an insoluble blue compound, KFeFe(CN)6·H2O. This compound is blue ferric ferrocyanide, also known as Prussian blue. How Blueprints Are Made A blueprint starts out as a black ink sketch on clear plastic or translucent tracing paper. The ink sketch is laid on top of a sheet of blueprint paper and exposed to ultraviolet light (e.g., placed in sunlight). Where the light strikes the paper, it turns blue. The black ink prevents the area under the drawing from turning blue. After exposure to UV light, the water-soluble chemicals are washed off the blueprint, leaving a white (or whatever color the paper is) drawing on a blue background. The resulting print is light-stable and as permanent as the substrate upon which it is printed. Make Blueprint Paper

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Chemistry: What's Hot Now: Periodic Table of Element Photos - Photos of the Elements - Periodic Table of the Elements

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Periodic Table of Element Photos - Photos of the Elements - Periodic Table of the Elements Aug 24th 2011, 10:02 Click on an element symbol in the periodic table to see a photograph of the element. Unless otherwise noted, these element photos are public domain images that you may save and use. Photos are unavailable for many of the extremely rare man-made radioactive elements. Be sure to visit the standard Periodic Table of the Elements if you need detailed element facts. 1 H 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na 12 Mg 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba * 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra ** 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 Ds 111 Rg 112 Cp 113 Uut 114 Uuq 115 Uup 116 Uuh 117 Uus 118 Uuo 57 La 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu 89 Ac 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96 Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr Alkali Metal Alkaline Earth Basic Metal Halogen Noble Gas Non Metal Rare Earth Semi-Metal Transition Metal

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Chemistry: What's Hot Now: Element Groups

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Element Groups Aug 24th 2011, 10:02 These are the element groups found in the periodic table of the elements. There are links to lists of elements within each group. 1. Metals Ben Mills Most elements are metals. In fact, so many elements are metals there are different groups of metals, such as alkali metals, alkaline earths, and transition metals. Most metals are shiny solids, with high melting points and densities. Many of the properties of metals, including large atomic radius, low ionization energy, and low electronegativity, are due to the fact that the electrons in the valence shell of a metal atoms can be removed easily. One characteristic of metals is their ability to be deformed without breaking. Malleability is the ability of a metal to be hammered into shapes. Ductility is the ability of a metal to be drawn into wire. Metals are good heat conductors and electrical conductors. 2. Nonmetals U.S. Geological Survey The nonmetals are located on the upper right side of the periodic table. Nonmetals are separated from metals by a line that cuts diagonally through the region of the periodic table. Nonmetals have high ionization energies and electronegativities. They are generally poor conductors of heat and electricity. Solid nonmetals are generally brittle, with little or no metallic luster. Most nonmetals have the ability to gain electrons easily. Nonmetals display a wide range of chemical properties and reactivities. 3. Noble Gases or Inert Gases pslawinski, wikipedia.org The noble gases, also known as the inert gases, are located in Group VIII of the periodic table. The noble gases are relatively nonreactive. This is because they have a complete valence shell. They have little tendency to gain or lose electrons. The noble gases have high ionization energies and negligible electronegativities. The noble gases have low boiling points and are all gases at room temperature. 4. Halogens Greenhorn1, public domain The halogens are located in Group VIIA of the periodic table. Sometimes the halogens are considered to be a particular set of nonmetals. These reactive elements have seven valence electrons. As a group, halogens exhibit highly variable physical properties. Halogens range from solid to liquid to gaseous at room temperature. The chemical properties are more uniform. The halogens have very high electronegativities. Fluorine has the highest electronegativity of all elements. The halogens are particularly reactive with the alkali metals and alkaline earths, forming stable ionic crystals. 5. Semimetals or Metalloids Dschwen, wikipedia.org The metalloids or semimetals are located along the line between the metals and nonmetals in the periodic table. The electronegativities and ionization energies of the metalloids are between those of the metals and nonmetals, so the metalloids exhibit characteristics of both classes. The reactivity of the metalloids depends on the element with which they are reacting. For example, boron acts as a nonmetal when reacting with sodium yet as a metal when reacting with fluorine. The boiling points, melting points, and densities of the metalloids vary widely. The intermediate conductivity of metalloids means they tend to make good semiconductors. 6. Alkali Metals Justin Urgitis, wikipedia.org The alkali metals are the elements located in Group IA of the periodic table. The alkali metals exhibit many of the physical properties common to metals, although their densities are lower than those of other metals. Alkali metals have one electron in their outer shell, which is loosely bound. This gives them the largest atomic radii of the elements in their respective periods. Their low ionization energies result in their metallic properties and high reactivities. An alkali metal can easily lose its valence electron to form the univalent cation. Alkali metals have low electronegativities. They react readily with nonmetals, particularly halogens. 7. Alkaline Earths Warut Roonguthai The alkaline earths are the elements located in Group IIA of the periodic table. The alkaline earths possess many of the characteristic properties of metals. Alkaline earths have low electron affinities and low electronegativities. As with the alkali metals, the properties depend on the ease with which electrons are lost. The alkaline earths have two electrons in the outer shell. They have smaller atomic radii than the alkali metals. The two valence electrons are not tightly bound to the nucleus, so the alkaline earths readily lose the electrons to form divalent cations. 8. Basic Metals Foobar, wikipedia.org Metals are excellent electric and thermal conductors, exhibit high luster and density, and are malleable and ductile. 9. Transition Metals Tomihahndorf, wikipedia.org The transition metals are located in groups IB to VIIIB of the periodic table. These elements are very hard, with high melting points and boiling points. The transition metals have high electrical conductivity and malleability and low ionization energies. They exhibit a wide range of oxidation states or positively charged forms. The positive oxidation states allow transition elements to form many different ionic and partially ionic compounds. The complexes form characteristic colored solutions and compounds. Complexation reactions sometimes enhance the relatively low solubility of some compounds. 10. Rare Earths Deglr6328, wikipedia.org The rare earths are metals found in the two rows of elements located below the main body of the periodic table. There are two blocks of rare earths, the lanthanide series and the actinide series. In a way, the rare earths are special transition metals, possessing many of the properties of these elements. 11. Lanthanides JKleo, wikipedia.org The lanthanides are metals that are located in block 5d of the periodic table. The first 5d transition element is either lanthanum or lutetium, depending on how you interpret the periodic trends of the elements. Sometimes only the lanthanides, and not the actinides, are classified as rare earths. Several of the lanthanides form during the fission of uranium and plutonium. 12. Actinides U.S. Department of Energy The electronic configurations of the actinides utilize the f sublevel. Depending on your interpretation of the periodicity of the elements, the series begins with actinium, thorium, or even lawrencium. All of the actinides are dense radioactive metals that are highly electropositive. They tarnish readily in air and combine with most nonmetals.

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Chemistry: What's Hot Now: How to Calculate Molarity

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How to Calculate Molarity Aug 24th 2011, 10:02 Molarity is a unit of concentration measuring the number of moles of a solute per liter of solution. The strategy to solving molarity problems is fairly simple. This outlines a straightforward method to calculate molarity of a solution. The key to calculating molarity is to remember the units of molarity: moles per liter. Find the number of moles of the solute dissolved in liters of solution. Take the following example: Calculate the molarity of a solution prepared by dissolving 23.7 grams of KMnO4 into enough water to make 750 mL of solution. This example has neither moles or liters needed to find molarity. Find the number of moles of the solute first. To convert grams to moles, the molar mass of the solute is needed. From the periodic table: Molar mass of K = 39.1 g Molar mass of Mn = 54.9 g Molar mass of O = 16.0 g Molar mass of KMnO4 = 39.1 g + 54.9 g + (16.0 g x 4) Molar mass of KMnO4 = 158.0 g Use this number to convert grams to moles. moles of KMnO4 = 23.7 g KMnO4 x (1 mol KMnO4/158 grams KMnO4) moles of KMnO4 = 0.15 moles KMnO4 Now the liters of solution is needed. Keep in mind, this is the total volume of the solution, not the volume of solvent used to dissolve the solute. This example is prepared with 'enough water' to make 750 mL of solution. Convert 750 mL to liters. Liters of solution = mL of solution x (1 L/1000 mL) Liters of solution = 750 mL x (1 L/1000 mL) Liters of solution = 0.75 L This is enough to calculate the molarity. Molarity = moles solute/Liter solution Molarity = 0.15 moles of KMnO4/0.75 L of solution Molarity = 0.20 M The molarity of this solution is 0.20 M. Review: To calculate molarity Find the number of moles of solute dissolved in solution. Find the volume of solution in liters. Divide moles solute by liters solution. More Molarity Example Problems Molarity Worked Example Molarity and Concentration Example Problem

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