Robert Pickett Wildlife Photography

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  • Paper Chromatography of Ink. Chromatography is an analytical process, which separates a compound into its constituent chemicals. Chromatography paper is dipped vertically in a solvent with the ink painted on it. Capillary action draws the solvent up through the paper and dissolves the ink. As the solvent travels up the paper it takes the various chemicals in the ink with it, separating them into a series of colored bands.
    38357RKP.jpg
  • Paper Chromatography of Ink. Chromatography is an analytical process, which separates a compound into its constituent chemicals. Chromatography paper is dipped vertically in a solvent with the ink painted on it. Capillary action draws the solvent up through the paper and dissolves the ink. As the solvent travels up the paper it takes the various chemicals in the ink with it, separating them into a series of colored bands.
    38359RKP.jpg
  • Paper Chromatography of Ink. Chromatography is an analytical process, which separates a compound into its constituent chemicals. Chromatography paper is dipped vertically in a solvent with the ink painted on it. Capillary action draws the solvent up through the paper and dissolves the ink. As the solvent travels up the paper it takes the various chemicals in the ink with it, separating them into a series of colored bands.
    38358RKP.jpg
  • Paper Chromatography of Ink. Chromatography is an analytical process, which separates a compound into its constituent chemicals. Chromatography paper is dipped vertically in a solvent with the ink painted on it. Capillary action draws the solvent up through the paper and dissolves the ink. As the solvent travels up the paper it takes the various chemicals in the ink with it, separating them into a series of colored bands.
    38356RKP.jpg
  • Lab Technician & Laboratory fume cupboard. The fume cupboard is a ventilation system used in science laboratories where hazardous chemicals are handled, especially those that produce hazardous fumes. The chemicals are handled behind a glass screen that can be raised and lowered. Extraction fans remove fumes through the pipes at top.
    38248RKP.jpg
  • Lab Technician & Laboratory fume cupboard. The fume cupboard is a ventilation system used in science laboratories where hazardous chemicals are handled, especially those that produce hazardous fumes. The chemicals are handled behind a glass screen that can be raised and lowered. Extraction fans remove fumes through the pipes at top.
    38247RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38382RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38377RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38386RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38385RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38383RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38384RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38381RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38380RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38387RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38379RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38378RKP.jpg
  • Eye Wash Area in Laboratory, showing signs and how to use flexible water tap
    38246RKP.jpg
  • Eye Wash Area in Laboratory, showing signs and how to use flexible water tap
    38245RKP.jpg
  • Saponification is an exothermic (gives off heat) chemical reaction that occurs when fats or oils (fatty acids) come into contact with lye (a base.) Saponification literally means turning into soap
    38390RKP.jpg
  • Saponification is an exothermic (gives off heat) chemical reaction that occurs when fats or oils (fatty acids) come into contact with lye (a base.) Saponification literally means turning into soap
    38392RKP.jpg
  • Saponification is an exothermic (gives off heat) chemical reaction that occurs when fats or oils (fatty acids) come into contact with lye (a base.) Saponification literally means turning into soap
    38393RKP.jpg
  • Saponification is an exothermic (gives off heat) chemical reaction that occurs when fats or oils (fatty acids) come into contact with lye (a base.) Saponification literally means turning into soap
    38391RKP.jpg
  • glass jars with chemicals inside, against black background - Sodium Chloride, Copper Sulphate, Litium Carbonate, Nickle Sulphate & Potassium Iodine
    38273RKP.jpg
  • Gas jars filled with chlorine (Cl2, left) and oxygen (O2, right) gases. These gaseous chemical elements are made up of diatomic molecules. Chlorine has a faint green colour, and is a toxic gas. It is used in the chlorination of water as a disinfectant. Oxygen is a reactive gas that is essential to life. It fuels reactions like the rapid combustion seen in fires, and also the slower reaction of respiration, the use of oxygen to fuel body metabolism. Oxygen makes up a fifth of the atmosphere by volume. Chlorine is obtained from seawater where it is present in salt (sodium chloride).
    38394RKP.jpg
  • Lithium burning in the flame of a bunsen burner producing a pink/red flame. The colour of the flame is caused by electrons that have been excited to a higher energy state. When they relax they emit energy in the form of a characteristic wavelength of light. The colour of the flame is different for different elements and can be used to identify unknown substances.
    38269RKP.jpg
  • Room freshener spray. This is an aerosol mist of liquid particles, seen in the air against black background. The freshener is in liquid form in the spray can, and the spray mechanism disperses it in the form of fine liquid droplets.  Model Release
    38681RKP.jpg
  • Magnesium metal reacts with oxygen to form magnesium oxide.
    38296RKP.jpg
  • Magnesium metal reacts with oxygen to form magnesium oxide.
    38297RKP.jpg
  • Lithium burning in the flame of a bunsen burner producing a pink/red flame. The colour of the flame is caused by electrons that have been excited to a higher energy state. When they relax they emit energy in the form of a characteristic wavelength of light. The colour of the flame is different for different elements and can be used to identify unknown substances.
    38268RKP.jpg
  • Hydrated Copper Sulphate in left hand tube (blue) and un-hydrated copper sulphate in right hand tube (white) Adding water to de-hydrated copper sulphate. Water being added to a test tube containing de-hydrated (anhydrous) copper (II) sulphate (CuSO4, white). The copper (II) sulphate forms hydration bonds with the water in an exothermic (heat-producing) reaction, resulting in hydrated copper (II) sulphate (blue).
    38368RKP.jpg
  • pH measurement. Electrometrical measurement of the pH of water. The pH of a solution is a measure of the amount of free hydrogen ions present. This indicates acidity and alkalinity. The more free ions present, the more acidic the solution is said to be. pH is measured on an inverse scale: the smaller the number, the more acidic the solution. Here, the pH meter is showing 5.48, indicating weakly acidic water. The scale runs from 0-14, with pure (distilled and deionised) water considered neutral at pH 7. There are several reasons why water may deviate from pH 7, including the presence of dissolved salts and gases.
    38325RKP.jpg
  • Bromine gas diffusion. Bromine vapour (orange) filling the lower of two gas jar before the seal between them is removed to demonstrate gas diffusion. Because gas molecules can move independently of each other and do so randomly, a gas spreads out from its source in a process called diffusion. The diffusion rate depends mainly on the temperature and the medium through which the diffusion takes place. In this case, the medium is air. The gas colour allows the diffusion to be observed. Sequence 1 of 4
    38292RKP.jpg
  • Magnesium burns in chlorine
    38283RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38411RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38409RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38408RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38407RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38405RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38404RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38401RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38402RKP.jpg
  • Parafin oil being poured into a beaker as a demonstration of its viscosity. Viscosity is the internal resistance of a fluid to the flow of that fluid.
    38398RKP.jpg
  • Parafin oil being poured into a beaker as a demonstration of its viscosity. Viscosity is the internal resistance of a fluid to the flow of that fluid.
    38397RKP.jpg
  • Parafin oil being poured into a beaker as a demonstration of its viscosity. Viscosity is the internal resistance of a fluid to the flow of that fluid.
    38395RKP.jpg
  • Hydrated Copper Sulphate in left hand tube (blue) and un-hydrated copper sulphate in right hand tube (white) Adding water to de-hydrated copper sulphate. Water being added to a test tube containing de-hydrated (anhydrous) copper (II) sulphate (CuSO4, white). The copper (II) sulphate forms hydration bonds with the water in an exothermic (heat-producing) reaction, resulting in hydrated copper (II) sulphate (blue).
    38366RKP.jpg
  • Hydrated Copper Sulphate in left hand tube (blue) and un-hydrated copper sulphate in right hand tube (white) Adding water to de-hydrated copper sulphate. Water being added to a test tube containing de-hydrated (anhydrous) copper (II) sulphate (CuSO4, white). The copper (II) sulphate forms hydration bonds with the water in an exothermic (heat-producing) reaction, resulting in hydrated copper (II) sulphate (blue).
    38365RKP.jpg
  • Hydrated Copper Sulphate in left hand tube (blue) and un-hydrated copper sulphate in right hand tube (white) Adding water to de-hydrated copper sulphate. Water being added to a test tube containing de-hydrated (anhydrous) copper (II) sulphate (CuSO4, white). The copper (II) sulphate forms hydration bonds with the water in an exothermic (heat-producing) reaction, resulting in hydrated copper (II) sulphate (blue).
    38364RKP.jpg
  • Lead iodide precipitate (yellow), the product of a reaction between lead nitrate and potassium iodide (both colourless liquids, right). The precipitate forms because it is insoluble in water. Potassium iodide is commonly used to test for lead.
    38361RKP.jpg
  • Lead iodide precipitate (yellow), the product of a reaction between lead nitrate and potassium iodide (both colourless liquids, right). The precipitate forms because it is insoluble in water. Potassium iodide is commonly used to test for lead.
    38360RKP.jpg
  • Fat test. Test tube containing a fatty emulsion (suspension of one liquid in another) floating on top of water. This test is used to identify fats in food. A sample of a food stuff is mixed with bromine and added to water. If the emulsion floats on top of the water, fat is present.
    38355RKP.jpg
  • An assortment of laboratory glassware consisting of Glass beakers and Erlenmeyer flask or conical flasks
    38347RKP.jpg
  • pH measurement. Electrometrical measurement of the pH of water. The pH of a solution is a measure of the amount of free hydrogen ions present. This indicates acidity and alkalinity. The more free ions present, the more acidic the solution is said to be. pH is measured on an inverse scale: the smaller the number, the more acidic the solution. Here, the pH meter is showing 5.48, indicating weakly acidic water. The scale runs from 0-14, with pure (distilled and deionised) water considered neutral at pH 7. There are several reasons why water may deviate from pH 7, including the presence of dissolved salts and gases.
    38324RKP.jpg
  • Bunsen Burner beneath Tripod with Gauze and tongs at side.  Laboratory tripod stand. This stand is used in conjunction with gauze and a Bunsen burner when heating objects in a laboratory. The heat-resistant mat protects the bench from the heat of the Bunsen burner. The gauze provides support for what is being heated, and also helps to spread the heat evenly.
    38321RKP.jpg
  • Reading a burette. A burette is a vertical, cylindrical piece of laboratory glassware, with a volumetric graduation marked along its full length. A precision tap, or stopcock, on the bottom allows highly accurate control over the release of liquid contained within the burette. Burettes are used to dispense known amounts of a liquid in experiments where precise measurements are necessary, such as a titration experiment.
    38319RKP.jpg
  • Reading a burette. A burette is a vertical, cylindrical piece of laboratory glassware, with a volumetric graduation marked along its full length. A precision tap, or stopcock, on the bottom allows highly accurate control over the release of liquid contained within the burette. Burettes are used to dispense known amounts of a liquid in experiments where precise measurements are necessary, such as a titration experiment.
    38318RKP.jpg
  • Lab Technician adding Potassium to water to see reaction -  Potassium reacting with water. Potassium (K) is a highly reactive metallic element. On contact with water it undergoes an exothermic (heat-producing) reaction to form potassium hydroxide (KOH) and hydrogen gas (H2). The purple flame is produced as the high temperature causes the hydrogen gas to ignite. The purple colour is produced by small amounts of vaporised potassium in the flame.
    38311RKP.jpg
  • Lab Technician adding Potassium to water to see reaction -  Potassium reacting with water. Potassium (K) is a highly reactive metallic element. On contact with water it undergoes an exothermic (heat-producing) reaction to form potassium hydroxide (KOH) and hydrogen gas (H2). The purple flame is produced as the high temperature causes the hydrogen gas to ignite. The purple colour is produced by small amounts of vaporised potassium in the flame.
    38310RKP.jpg
  • Lab Technician universal indicator to water after previously adding Sodium. Water turns colour and is then checked against chart for reference.
    38307RKP.jpg
  • Lab Technician adding Potassium to water to see reaction -  Potassium reacting with water. Potassium (K) is a highly reactive metallic element. On contact with water it undergoes an exothermic (heat-producing) reaction to form potassium hydroxide (KOH) and hydrogen gas (H2). The purple flame is produced as the high temperature causes the hydrogen gas to ignite. The purple colour is produced by small amounts of vaporised potassium in the flame.
    38309RKP.jpg
  • Lab Technician universal indicator to water after previously adding Sodium. Water turns colour and is then checked against chart for reference.
    38308RKP.jpg
  • Experiement - Lab Technician dropping Lithiumin into water, showing reaction  Lithium (Li) is a highly reactive metallic element. It is light enough to float on water, with which it reacts violently to produce hydrogen (H2) gas and lithium hydroxide (LiOH). Bubbles of H2 can be seen around the piece of metal
    38302RKP.jpg
  • Experiement - Lab Technician dropping Universal Indicator into water with Lithiumin previously added.  Water Turns blue and is compated to chart for reference.  Lithium (Li) is a highly reactive metallic element. It is light enough to float on water, with which it reacts violently to produce hydrogen (H2) gas and lithium hydroxide (LiOH). Bubbles of H2 can be seen around the piece of metal
    38303RKP.jpg
  • Experiement - Lab Technician dropping Lithiumin into water, showing reaction  Lithium (Li) is a highly reactive metallic element. It is light enough to float on water, with which it reacts violently to produce hydrogen (H2) gas and lithium hydroxide (LiOH). Bubbles of H2 can be seen around the piece of metal
    38301RKP.jpg
  • Experiement items for testing elements in water, Lithium, Sodium & Potassium, with Universal Indicator and colour chart, plus safety goggles and safety screen around bowl of water
    38299RKP.jpg
  • Experiement - Lab Technician dropping Lithiumin into water, showing reaction  Lithium (Li) is a highly reactive metallic element. It is light enough to float on water, with which it reacts violently to produce hydrogen (H2) gas and lithium hydroxide (LiOH). Bubbles of H2 can be seen around the piece of metal
    38300RKP.jpg
  • Bromine gas diffusion. Bromine vapour (orange) filling the lower of two gas jar before the seal between them is removed to demonstrate gas diffusion. Because gas molecules can move independently of each other and do so randomly, a gas spreads out from its source in a process called diffusion. The diffusion rate depends mainly on the temperature and the medium through which the diffusion takes place. In this case, the medium is air. The gas colour allows the diffusion to be observed. Sequence 4 of 4
    38295RKP.jpg
  • Bromine gas diffusion. Bromine vapour (orange) filling the lower of two gas jar before the seal between them is removed to demonstrate gas diffusion. Because gas molecules can move independently of each other and do so randomly, a gas spreads out from its source in a process called diffusion. The diffusion rate depends mainly on the temperature and the medium through which the diffusion takes place. In this case, the medium is air. The gas colour allows the diffusion to be observed. Sequence 3 of 4
    38294RKP.jpg
  • Sodium reacting with chlorine to form sodium chloride (NaCl, common salt). A burning piece of the alkali metal sodium (Na) has a gas jar containing the halogen gas chlorine (Cl2) placed over it.  The reaction is violent and exothermic (heat-releasing).
    38291RKP.jpg
  • Sodium reacting with chlorine to form sodium chloride (NaCl, common salt). A burning piece of the alkali metal sodium (Na) has a gas jar containing the halogen gas chlorine (Cl2) placed over it.  The reaction is violent and exothermic (heat-releasing).
    38290RKP.jpg
  • Sodium reacting with chlorine to form sodium chloride (NaCl, common salt). A burning piece of the alkali metal sodium (Na) has a gas jar containing the halogen gas chlorine (Cl2) placed over it.  The reaction is violent and exothermic (heat-releasing).
    38288RKP.jpg
  • Sodium reacting with chlorine to form sodium chloride (NaCl, common salt). A burning piece of the alkali metal sodium (Na) has a gas jar containing the halogen gas chlorine (Cl2) placed over it.  The reaction is violent and exothermic (heat-releasing).
    38286RKP.jpg
  • Sodium reacting with chlorine to form sodium chloride (NaCl, common salt). A burning piece of the alkali metal sodium (Na) has a gas jar containing the halogen gas chlorine (Cl2) placed over it.  The reaction is violent and exothermic (heat-releasing).
    38287RKP.jpg
  • Flame test. Potassium burning in the flame of a bunsen burner producing a lilac flame. The colour of the flame is caused by electrons that have been excited to a higher energy state. When they relax they emit energy in the form of a characteristic wavelength of light. The colour of the flame is different for different elements and can be used to identify unknown substances.
    38270RKP.jpg
  • Flame test for copper. A compound containing the element copper (symbol Cu) produces a characteristic blue-green flame when heated in a bunsen burner. This colour is produced when copper electrons give off extra energy as a specific type of radiation (in this case it is visible light but it can be radio waves or gamma rays). This distinct energy release is known as an emission spectrum. Each element has its own emission spectrum, which allows it to be identified in different materials.
    38267RKP.jpg
  • Flame test. Barium burning in the flame of a bunsen burner producing a green flame. The colour of the flame is caused by electrons that have been excited to a higher energy state. When they relax they emit energy in the form of a characteristic wavelength of light. The colour of the flame is different for different elements and can be used to identify unknown substances.
    38265RKP.jpg
  • Experiment showing stages of Magnesium strip burning in flame
    38256RKP.jpg
  • Experiment showing stages of Magnesium strip burning in flame
    38255RKP.jpg
  • Experiment showing stages of Magnesium strip burning in flame
    38254RKP.jpg
  • Experiment showing stages of Magnesium strip burning in flame
    38253RKP.jpg
  • Showing set up for burning magnesium in bunsen burner flame
    38251RKP.jpg
  • Lemon Battery - Copper (orange) and zinc (silver) electrodes have been inserted into a lemon and connected to wires to produce electricity. The voltmeter (top) is showing the voltage generated.
    38243RKP.jpg
  • Lemon Battery - Copper (orange) and zinc (silver) electrodes have been inserted into a lemon and connected to wires to produce electricity. The voltmeter (top) is showing the voltage generated.
    38242RKP.jpg
  • Lemon Battery - Copper (orange) and zinc (silver) electrodes have been inserted into a lemon and connected to wires to produce electricity. The voltmeter (top) is showing the voltage generated.
    38241RKP.jpg
  • Room freshener spray. This is an aerosol mist of liquid particles, seen in the air against black background. The freshener is in liquid form in the spray can, and the spray mechanism disperses it in the form of fine liquid droplets.  Model Release
    38680RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38410RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38406RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38403RKP.jpg
  • Parafin oil being poured into a beaker as a demonstration of its viscosity. Viscosity is the internal resistance of a fluid to the flow of that fluid.
    38396RKP.jpg
  • Hydrated Copper Sulphate in left hand tube (blue) and un-hydrated copper sulphate in right hand tube (white) Adding water to de-hydrated copper sulphate. Water being added to a test tube containing de-hydrated (anhydrous) copper (II) sulphate (CuSO4, white). The copper (II) sulphate forms hydration bonds with the water in an exothermic (heat-producing) reaction, resulting in hydrated copper (II) sulphate (blue).
    38367RKP.jpg
  • Hydrated Copper Sulphate in left hand tube (blue) and un-hydrated copper sulphate in right hand tube (white) - showing difference
    38363RKP.jpg
  • Lead iodide precipitate (yellow), the product of a reaction between lead nitrate and potassium iodide (both colourless liquids, right). The precipitate forms because it is insoluble in water. Potassium iodide is commonly used to test for lead.
    38362RKP.jpg
  • Fat test. Test tube containing a fatty emulsion (suspension of one liquid in another) floating on top of water. This test is used to identify fats in food. A sample of a food stuff is mixed with bromine and added to water. If the emulsion floats on top of the water, fat is present.
    38354RKP.jpg
  • pH measurement. Electrometrical measurement of the pH of water. The pH of a solution is a measure of the amount of free hydrogen ions present. This indicates acidity and alkalinity. The more free ions present, the more acidic the solution is said to be. pH is measured on an inverse scale: the smaller the number, the more acidic the solution. Here, the pH meter is showing 5.48, indicating weakly acidic water. The scale runs from 0-14, with pure (distilled and deionised) water considered neutral at pH 7. There are several reasons why water may deviate from pH 7, including the presence of dissolved salts and gases.
    38323RKP.jpg
  • Lab Technician adding universal indicator to water after Potassium previously added to see reaction.  Water turns colour and chart is used as reference -  Potassium reacting with water. Potassium (K) is a highly reactive metallic element. On contact with water it undergoes an exothermic (heat-producing) reaction to form potassium hydroxide (KOH) and hydrogen gas (H2).
    38312RKP.jpg
  • Experiement - Lab Technician dropping Universal Indicator into water with Lithiumin previously added.  Water Turns blue and is compated to chart for reference.  Lithium (Li) is a highly reactive metallic element. It is light enough to float on water, with which it reacts violently to produce hydrogen (H2) gas and lithium hydroxide (LiOH). Bubbles of H2 can be seen around the piece of metal
    38304RKP.jpg
  • Bromine gas diffusion. Bromine vapour (orange) filling the lower of two gas jar before the seal between them is removed to demonstrate gas diffusion. Because gas molecules can move independently of each other and do so randomly, a gas spreads out from its source in a process called diffusion. The diffusion rate depends mainly on the temperature and the medium through which the diffusion takes place. In this case, the medium is air. The gas colour allows the diffusion to be observed. Sequence 2 of 4
    38293RKP.jpg
  • Sodium reacting with chlorine to form sodium chloride (NaCl, common salt). A burning piece of the alkali metal sodium (Na) has a gas jar containing the halogen gas chlorine (Cl2) placed over it.  The reaction is violent and exothermic (heat-releasing).
    38289RKP.jpg
  • Sodium reacting with chlorine to form sodium chloride (NaCl, common salt). A burning piece of the alkali metal sodium (Na) has a gas jar containing the halogen gas chlorine (Cl2) placed over it.  The reaction is violent and exothermic (heat-releasing).
    38285RKP.jpg
  • Magnesium burns in chlorine
    38284RKP.jpg
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