...This element will only be found naturally in combination with other elements like carbon and oxygen. Magnesium is very flammable and can be mixed with other metals that need to be light and sturdy. Magnesium burns at relatively low temperatures. The melting point of Magnesium is 1,202 degrees Fahrenheit or 650 degrees Celsius. (Facts about Magnesium) When Magnesium is being burnt, it gives off a bright white light. When the Magnesium is done burning it will not give off a bright white light. This tells us when the combustion is complete. (It’s...
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...five major types. These are: (1) synthesis, (2) decomposition, (3) single replacement, (4) double replacement, and (5) combustion. Most reactions can be put into one of these categories. In a synthesis reaction, two or more substances (elements or compounds) combine to form a more complex substance. A decomposition reaction is exactly the opposite of a synthesis reaction. In a decomposition reaction, a compound breaks down into two or more simpler substances (elements or simpler compounds.) In a single replacement reaction, one element in a compound is replaced by a more active element. In a double replacement reaction, the positive ions of two different ionic compounds can be thought of as “replacing each other.” Most replacement reactions (both single and double) take place in aqueous solutions containing free ions. In a double replacement reaction, one of the products must be removed from the solution as a precipitate, water, or an insoluble gas. A precipitate is a solid that is produced as a result of a chemical reaction in solution. As the precipitate separates from the solution, the solution appears cloudy. In a combustion reaction a substance combines with oxygen, releasing a large amount of energy in the form of light and heat. If an organic compound (one that contains carbon) is a reactant, then the products of the combustion reaction are always carbon dioxide gas and water vapor. Form a Hypothesis If a chemical reaction has occurred, then __________________________________________ ...
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...good example of a chemical reaction that releases chemical energy. Batteries and explosives are other examples of objects that contain stored chemical energy. There are six basic types of chemical reactions: combustion, synthesis, single displacement, decomposition, double displacement, and acid-base. During combustion, chemical energy in the form of heat is released when oxygen combines with other substances to form water and carbon dioxide. Example: Magnesium and oxygen react to produce heat and light energy. The potential energy stored in chemical bonds holding the object together. Chemical energy is released due to chemical reaction. It is a type of potential energy. Chemical energy is stored within the bonds of the atoms and molecules that make up a substance. Once chemical energy is released from a substance, the substance is transformed into a new substance. Chemical energy is stored inside a substance or object until it is involved in a chemical reaction. Our bodies use chemical energy to perform daily functions. Cooking is a good example of a chemical reaction that releases chemical energy. Batteries and explosives are other examples of objects that contain stored chemical energy. There are six basic types of chemical reactions: combustion, synthesis, single displacement, decomposition, double...
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...Chemistry behind Fireworks Did you know that when you see a commercial fireworks display you are looking at chemistry in action. You may have asked yourself “I wonder what is going on to make all those pretty colors and patterns” It is controlled chaos!! I tell you. Let us break this down to the basic we will start with a typical shell. Starting at the bottom we have a lifting charge which contains good ole black powder. The lifting charge gets the party started by creating an explosion after it is ingnited by the fuse. An explosion occurs which produces hot rapidly expanding gases . This is an example of the “Law of Volumes” which is an experimental gas law which describes how gases tend to expand when heated. Since all the kenetic energy is contained in a tube the shell has no place to go but up. This is Newton’s third law in action which states (in laymans terms) “for every action there is an opposite and equal reaction”. The next two stages in the process happen almost simultaniously the bursting charge, explodes out ward dispersing the pellets or stars which give us our colors and patterns. This happens when the ariel shell is at the apex of its climb via a time delay fuse. Chemical Agents Oxidizer, what is an oxidizer? The word "burning" describes the oxidation of a fuel in air. A campfire, for instance, uses oxygen from the air to turn wood (cellulose) into steam (H2O) and carbon dioxide (CO2), among other things. So why do fireworks need an oxidizer...
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...reactants (starting products) are different from the products. Chemical reactions involve the breaking of old bonds and the formation of new bonds. They can result in the formation of precipitates, changes in color, production or absorption of heat, or formation of gas bubbles. Chemical reactions can be placed in the following five categories: (i) synthesis (ii) decomposition (iii) single-replacement (iv) double-replacement and (v) combustion. 1. Synthesis (also known as combination) is the simplest of the five types of reactions. In synthesis reactions, two or more elements or compounds bond to form one product. For example, magnesium and oxygen combine to from magnesium oxide. 2Mg(s) + O2 (g) → 2MgO(s) In this synthesis reaction, Mg has lost electrons and O has gained electrons resulting in an ionic bond. Synthesis reactions can also happen between a pair of compounds to form a new compound. Here is an example of a synthesis reaction: MgO(s) + H2(s) → Mg(OH)(aq). Magnesium Oxide and hydrogens combine to create magnesium hydroxide. Also, notice that the two solid compounds have turned into an aqueous solution, a change which is a key characteristic of a chemical reaction. 2. Decomposition is basically the opposite of synthesis. In decomposition reactions, a compound is broken down into two or more simpler substances. Decomposition can occur when certain compounds are heated or and electric current is passed through it (Chemistry, An Experimental...
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...Fire Fire is the rapid oxidation of a material in the exothermic chemical process of combustion, releasing heat, light, and various reaction products. Fire in its most common form can result in conflagration, which has the potential to cause physical damage through burning. Fire is an important process that affects ecological systems across the globe. The positive effects of fire include stimulating growth and maintaining various ecological systems. Fire has been used by humans for cooking, generating heat, signaling, and propulsion purposes. The negative effects of fire include water contamination, soil erosion, atmospheric pollution and hazard to human and animal life. PHASES OF A FIRE First Phase – Incipient Oxygen content 20% - 21% with ceiling temperatures of approximately 37˚ C°. At this stage the produces of combustion are water vapour, carbon dioxide and sulphur dioxiode, and hot gases rising. Smoldering fires my last for a few seconds to several hours before breaking into flames. A large volume of smoke will be present until flaming starts and then progress is rapid. Second Phase – free burning, flame producing or steady state At this stage the oxygen content is 15% - 19% and the ceiling temperatures are above 537°C and the products of combustion are water vapour, carbon dixiode, carbon monoxide and sulphur dioxide. There large quantities of dark grey smoke and rapid destruction of combustible materials. It is at this point that flash over occurs. Flash...
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...Mia Katola Chemistry Mr. C By Mia Katola Chemistry Mr. C By Air and water Air and water questions Are Core and Extended. Contents Page Questionnumber | Core: | Page Number | 1 | Describe chemical tests for water using cobalt (2) chloride and copper (2) sulfate | Describe methods of rust prevention, specially paint and other coatings to exclude oxygen | | 2 | Describe, in outline the treatment of the water supply in terms of filtration and chlorination. | Describe the need for nitrogen, phosphorus and potassium containing fertilizers | | 3 | Name some of the uses of water in the home | Describe the displacement of ammonia from its salts | | 4 | Describe the composition of clean water as being approximately 79% nitrogen, 20% oxygen and the remainder as being a mixture of noble gasses, water vapor and carbon dioxide. | State that carbon dioxide and methane are greenhouse gases and may contribute to climate change | | 5 | Name the common pollutants in the air as being carbon monoxide, sulfur dioxide, oxides of nitrogen and lead compounds | Describe the formation of carbon dioxide | | 6 | State the source of each of these pollutanatsCarbon monoxideSulfer dioxideOxides of nitrogen from car exhausts | State the sources of methane, including decomposition of vegetation and waste gases from digestion in animals | | 7 | State the adverse effect of common pollutanats on buildings and on health | Describe sacrificial protection in terms of the reactive...
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...(CO2) on the Earth’s environment by converting CO2 into materials with a broad range of commercial applications. The first example of ERC are 19th century, when there is reduction of carbon dioxide to formic acid using a zinc cathode. [2] The rate of formation of CO2 and the rate of reduction of CO2 in the atmosphere are not proportional. The conversion of CO2into more useful organic fuels (like methanol) using energy that is not produced from fossil fuels is believed to be one such alternative method. The various souses of CO2 emmisionin 2015 is shown in fig. Fig -1: Sources of carbon dioxide emissions in 2015. 2. Effects of carbon dioxide- 2 carbon dioxide is waste byproduct emitted by coal-fired power station or in general by any combustion of fossil fuels it is major contributor to climate change as well as environmental and ocean acidification. 2.1 Effects of carbon dioxide On Human -1 The health of individuals near carbon transport and appropriation sites must be considered in site risk account. The toxic effects of high CO2 concentrations are well known, but the literature also discloses cause for concern for both the survivors of high-level CO2 exposure and individuals who experience continued low-level exposure [3]. As human populations continue to increase, simultaneous increases in energy and food will be required The effects of CO2 in an exact individual depend on the concentration and period of exposure as well as distinct factors, such as age, health, physiologic...
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...electrons. Simple molecular covalent compounds: Low Melting and Boling points. Strong in atoms. Weak in electrons. Easy to break apart. Cannot conduct electricity. Giant Molecular Covalent Compounds; Diamond-Very Hard. Very high melting and boiling points. Cannot Conduct Electricity. Graphite-Soft. High Melting and Boiling Points. Conducts Electricity. Metallic Bonding: A ladus of ions in a sea of electrons. Properties of Metals: Conduct Electricity-Usually Dense-Malleable, ductile-High Melting and Boiling Points. Diatomic Molecules-These consist of two atoms the same, covalently bonded. CHEMICAL REACTIONS Mixture-2 or more elements not combined by a chemical reaction. Compound-2 or more elements chemically combined. Combustion of fuels= Fuel + Oxygen -----> Water + Carbon Dioxide...
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...1. Why did magnesium react with zinc nitrate and why can’t lead react with zinc nitrate? The reason why magnesium reacted with zinc nitrate is because magnesium is two elements higher than zinc on the activity series. When a metal is higher than another on the series, it means it is capable of replacing whichever metal is beneath it in a single displacement reaction. The distance between the two metals has a correlation with the slow execution of the reaction as the closer the elements are on the series the slower the reaction takes place. Since zinc is the metal in the compound zinc nitrate, it being two elements below magnesium insures that a reaction will occur at a slower pace. For this same reason lead cannot react with zinc nitrate because zinc is above it in the activity series. 2. What kinds of indication did sodium iodide have with silver nitrate to confirm that this is a double displacement reaction?...
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...Alkali metals Cations occur in wide variety of important chemicals The metals are all very reactive when pure – strongly reducing Their cations (with the exception of lithium) have low charge densities – often leads to good solubility and an ability to stabilize anions that can not be formed along with any other cation Alkali metal physical properties Element Li Na K Rb Cs Density (gcm-3) 0.53 0.97 0.86 1.53 1.87 Melting point (oC) 180 98 64 39 29 ∆Hatm (kJmol-1) 162 108 90 82 78 1 Reactivity towards Bronsted acids The alkali metals react even with weak Bronsted acids such as water – The rate of reaction depends upon the acidity of the medium 2Na + 2H2O 2Na + 2EtOH 2Na + 2NH3 2NaOH + H2 2NaOEt + H2 2NaNH2 + H2 – very slow reaction in absence of catalyst Alkali metals and liquid NH3 Alkali metals react very slowly with liquid ammonia – however, they typically dissolve rapidly in ammonia to form highly colored solutions Na(s) --(ammonia)--> Na(am) + e-(am) – fast 2e-(am) + 2NH3 2NH2- + H2 – slow in absence of catalyst 2 Sodide anions and electrides 2Na(s) + C12H24O6 [Na(C12H24O6)]+Na– complexing or chelating agent is used to stabilize the cation » Na- is the sodide anion. It is the most stable alkalide ion Other complexing agents have been used to form solid salts where e- is the anion – electrides Lithium Lithium is the most reducing of all the alkali metals – but not the most reactive Unlike the other alkali metals it reacts with nitrogen to form a nitride Used...
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...This is a lab in which we will be using combustion to make magnesium and turn into a fine powder. We will first put the crucible on a mesh above bunser burner to heat it up to get out any moisture. We will then record the weight and weigh the magnesium in the crucible. Then we will put the crucible over a flame with the magnesium inside until it turns into the powder. There are many changes in the world. These changes are like changes in chemistry because some you don’t see and there is some you do see. The changes that you can see in chemistry are called physical changes. A physical change is when it does not change the substances chemical identity, although in a chemical change it does change its chemical identity. The actual atoms still remain they are just rearranged into new ways that make them into the substance that they need to be. Even though a substance changes it still keeps the same mass because of the law of conservation of mass. The law of conservation of mass states that mass can’t be created or destroyed. There are three (technically 4) states of matter. The states of matter are solids, liquids, and gases (plasma). These states can transform into one another but not lose their mass do the law of conservation of mass in a closed...
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...I Intro In this lab we are going to observe chemical reactions. A chemical reaction is the rearrangement of stuff into new stuff. When a chemical reaction occurs there is color change, temperature change, energy change, gas release, odor, and precipitation. There are 5 different types of chemical reactions: synthesis, decomposition, single displacement, double displacement, and combustion. A chemical reaction has to be balanced because of the law of conservation of mass. Conservation of mass is mass neither created nor destroyed. The product has to be the same amount of substances as the reactants. II Purpose The purpose of this lab is to observe different typed of chemical reactions. III Data / Observations Reaction #1: 2Mg + O2 2MgO Synthesis * Burning magnesium metal turns it into an ultraviolet light while on fire. Product is a white powder. Reaction #2: Mg + HCl MgCl2 + H2 Single displacement * When magnesium was added to HCl, it started to bubble and the test tube became hot. When a flame lit on a wooden splint was added it made a loud pop sound. Reaction #3: (NH4)2 + CO3 (NH4)2 + CO3 Decomposition * Ammonium carbonate was added into a test tube and heated up it up with fire. After adding a piece of litmus paper a strong odor was released. The litmus paper turned from a color pink to a color of blue. Reaction #4: CaCo3 + 2HCl CaCl2 + H2CO3 Double displacement * When HCl was added to calcium carbonate it began...
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...between elements, mixtures and compounds and give examples of each; (c) Recall that some metals are reactive and others are not; (d) Demonstrate an understanding of the reactivity series; (e) Arrange metals in order of reactivity (Sodium, Calcium, Magnesium, Zinc, Iron, Copper, Silver and Gold); (f) Recall what are acids and bases; (g) State the importance of acids and bases; (h) Recall the colours of indicators (methyl orange, phenolphthalein, litmus) in acids and alkalis 2. THE LANGUAGE OF CHEMISTRY Students should be able to: (a) Describe physical changes giving examples; (b) Describe chemical changes giving examples; (c) Give the symbols and valencies of elements; (d) Work out the formulae of compounds; (e) Define the term radical and give the names and valencies of the following radicals: hydroxide, carbonate, sulfate, ammonium and nitrate; (f) Demonstrate an understanding of chemical reactions, reactants and products; (g) Represent chemical reactions by word equations; (h) Convert word equations to balanced chemical equations; (i) Write and balance chemical equations 3. CHEMICAL REACTIONS IN GENERAL Students should be able to: (a) Describe the reaction of selected metals (sodium, magnesium, iron and copper)with oxygen; (b) Describe the reaction of selected metals with water and/or steam; (c) Describe the reaction of metals with dilute acids; (d) Describe displacement reactions; (e) Predict the reaction of a particular metal using...
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...During the experiment we encountered various problems. While weighing the magnesium, some of the strips fell and other strips fell off, therefore we had to weigh it again. When we did the first reaction, the final temperature of the reaction rose to only about 65C due to the fan and air conditioning in the area that we were working in. We consulted with the instructor, and he told us that the final temperature had to be at least 70C. We moved to another area where the fan was not blowing directly at us, and we did the first reaction again, finally obtaining the desired temperature. The next problems we encountered were in the calculations of the enthalpy for the reaction: Mg(s) + 1/2O2(g) MgO(s) At first, we forgot to change the enthalpies from the reactions that we produced to kilo Joules. Then, we consulted the instructor with our final answer, he said that we had to divide the enthalpies we found from the reactions that we produced by .05 mol, in order to calculate it with the other enthalpies, because the unit for enthalpy is kJ/mol. Theoretical Value: Mg(s) + 1/2O2(g) MgO(s) H = -601.8 kJ Experimental Value: Mg(s) + 1/2O2(g) MgO(s) H = -578.4 kJ Our experimental value is -23.4 kJ more than the theoretical value. Compared to the theoretical value, our percent error is: Percent Error: 578.4 kJ - 601.8 kJ x 100 % 601.8 kJ ...
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