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Classifying Chemical Equations DO NOW: Balance the following Chemical Reactions: N 2 + H 2 NH 3 K + Cl 2 KCl CH 4 + O 2 CO 2 + H 2 O Al + O 2 Al 2 O 3
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Classifying Chemical Equations SWK: the types of chemical reactions include synthesis, decomposition, single replacement, and double replacement. SWBAT: identify types of chemical reactions. HW: In the Pearson Chemistry textbook, Types of Chemical Reactions, 356- 372 then complete # 21- 24, on page 367 and #29 on 373.
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Classifying Chemical Equations Most of the reactions that you will encounter will be of four general types. I) Combination (synthesis) A + B AB e.g. 2 Na + Cl 2 2 NaCl
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II)Decomposition AB A + B e.g. 2 H 2 O 2H 2 + O 2
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III) Single replacement A + BX AX + B e.g. Mg + CuSO 4 MgSO 4 + Cu
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IV)Double Replacement AX + BY AY + BX e.g. CaCO 3 + 2HCl CaCl 2 + H 2 CO 3
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Note: Combustion Reaction X + O 2 CO 2 + H 2 Ox = hydrocarbon e.g. CH 4 + 2O 2 CO 2 + 2H 2 O
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Complete, identify, and balance the following equations. H 2 + ? 2 H 2 O Na + Cl 2 ? N 2 + ? NO 2 NH 3 + ? NH 4 Cl CO ? + O 2 ? Al + 3Cl 2 CCl 4 C + ? NH 4 OH NH 3 + ?
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Classifying with 3D Models video Let’s Predict the product of these reactions then see then happen… Classifying Chemical Equations
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CLASSWORK:In the Prentice Hall workbook, complete pages 115-118, Sections 11.2 & 11.3 HW: In the Pearson Chemistry textbook, Types of Chemical Reactions, 356- 372 then complete # 21- 24, on page 367 and #29 on 373.
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Nuclear Reaction Take a look at the following reaction. At first glance, you might mistake this for a chemical equation. The format of this equation is similar to that of a chemical equation.
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Nuclear Reaction However, there is an important difference between this equation and chemical equations. DO YOU SEE WHAT IT IS? Notice that we have different elements on either side of the equation! This is evidence that we are looking at a nuclear equation, not a chemical equation.
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Nuclear Reaction The equation shows an atom of potassium (K), transforming into an atom of calcium (Ca). This nuclear equation also contains a particle (e), that we have not learned yet. Remember that with chemical equation you had to have the same number of atoms of each element on either side of the yield sign, or you violate the Law of Conservation of Matter. This nuclear equation DOES violate the Law of Conservation of Matter!
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Nuclear Reaction HOW CAN WE RESOLVE THE VIOLATION OF THIS LAW? Albert Einstein combined the laws of conservation of matter and energy into one law, called the “Law of Conservation of Mass-Energy.” This law states that, in nuclear reactions, a small amount of mass is converted into energy.
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Nuclear Reaction Probably the most interesting thing about nuclear reactions is that elements are being transformed into other elements. (K) ---> (Ca) Also notice that both the mass number ---------> and the nuclear charge -------> are conserved. This will be the key to balancing this type of equation.
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Nuclear Reaction Radioactivity - the spontaneous emission of radiation by unstable atomic nuclei Nuclear reaction – the proton number changes therefore the element changes Radioactive decay – the release of radiation by radioactive isotopes
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Nuclear Reaction Alpha Particle- this particle is identical to the nucleus of a helium atom (2 protons, 2 neutrons). This particle is positively charged, relatively large and doesn’t penetrate deeply into matter Neutron- These particles are sometimes absorbed or released as elements transform into other elements. Sometimes protons will turn into neutrons and vice versa in same reaction.
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Nuclear Reaction Beta Particles- this particle is identical in composition to an electron (no mass and a charge of zero). Can penetrate more substances than alpha particle and is blocked only by heavy material (heavy clothes, metal, wood, etc) Positron- This particle has the same mass as an electron, but has a positive charge. This particle is sometimes called a “beta plus particle”.
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Proton- The proton is identical in composition to the nucleus of a hydrogen atom (mass of 1 and a charge of +1). γ Gamma Ray- high energy form of electromagnetic radiation, without mass or charge. Extremely dangerous to living cells (blocked only by thick concrete or lead) Nuclear Reaction
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Nuclear processes are often categorized as a) natural radioactivity or b) artificial radioactivity Natural radioactivity is applied to nuclear processes that occur in nature, while artificial radioactivity is observed when scientists take stable nuclei and try to combine them in various ways to produce stable isotopes of “new” or previously undiscovered elements.
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Nuclear Reaction If you studied the concept of carbon dating in biology, then you know that carbon-14 is an example of an unstable isotope, which naturally decays into nitrogen-14 according to the following nuclear equation: This is an example of beta decay, because the parent nucleus decays into the daughter nucleus, as it releases a beta particle.
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Nuclear Reaction Concerning artificial radioactivity, all the elements on the Periodic Table with atomic numbers of 93 or greater were produced with the aid of instruments called particle accelerators, which are used to fuse nuclei of known elements together in order to produce still heavier nuclei. For example: Curium-244 is bombarded with carbon-12 to form a new element nobelium-254.
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Nuclear Reaction Nuclear Fission and Nuclear Fusion Nuclear Fission is the process by which a relatively massive nucleus is divided into smaller nuclei and one or more neutrons. The neutron on the left side of the equation can be thought of as the projectile that causes the larger atom of uranium to “split”. The three neutrons that are released on the right side of the equation, can they go on to “split” more atoms of uranium, and release more neutrons. This process is called a chain reaction.
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Nuclear Reaction Nuclear Fusion is the process of less massive nuclei combining into more massive ones. Nuclear fusion is the process that powers the stars, including our sun, with hydrogen nuclei combine to produce helium nuclei. The reactions here show how this occurs.
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