Stable Ion Charges Metals Form Cagons. Nonmetals Form Anions
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Properties of Acids
Properties of Acids Solutions of acids have a sour taste Don’t taste them in the lab !!! 1 They change the colors of many indicators Acids turn blue litmus to red Acids turn bromothymol blue from blue to yellow They react with metals to generate hydrogen gas, H2 1 Metal Activity Series More active Li, K, Ca, Na, Mg, Al, Mn, Zn, Fe, Co, Ni, Pb, H, Cu, Hg, Ag, Pt, Au Less active Active enough to displace Cannot displace hydrogen from an acid hydrogen from an acid 2 Properties of Acids They react with metal oxides forming the salt of the metal and water CaO + 2HCl → CaCl2 + H2O They react with metal hydroxides forming the salt of the metal and water Ca(OH)2 + 2HCl → CaCl2 + 2H2O 3 Oxides Compounds of oxygen and another element There are two ways to name oxides Based on the oxidation number of the element Li2O – lithium oxide BaO – barium oxide FeO – iron(II) oxide Fe2O3 – iron(III) oxide Based on the number of atoms of each element Li2O – dilithium oxide BaO – barium oxide FeO – iron oxide Fe2O3 – diiron trioxide 4 Example 1 Name the following compounds: BeO, Al2O3, Cu2O, OsO4, Cr2O3, CrO3 5 Example 2 Write formulas for the following compounds: Potassium oxide Boron oxide Diindium trioxide Cobalt(II) oxide Dinitrogen pentoxide Rhenium(VI) oxide Xenon tetroxide Carbon monoxide Carbon dioxide Manganese(VII) oxide 6 Example 3 Write total and net ionic equations for the reaction between cobalt (III) oxide and diluted hydroiodic acid 7 Example 4 Write total and net ionic equations for the reaction between dialuminum -
United States Patent (19) 11 3,970,745 Takeuchi (45) July 20, 1976
United States Patent (19) 11 3,970,745 Takeuchi (45) July 20, 1976 (54) METHOD FOR PRODUCING HYDROGEN son, vol. 3, 1949 Ed., p. 535, Reinhold Pub. Corp., FROM WATER New York. 75) Inventor: Norio Takeuchi, Isehara, Japan P. Pascal's “Nouveau Traite' de Chimie Minerale', Tome 8, 1963, pp. 54, 55; Masson et Cie., Paris, 73 Assignee: Director-General of the Agency of France. Industrial Science and Technology, J. W. Mellor's "A Comp. Treatise on Inorg. and Theo. Tokyo, Japan Chem.", vol. 7, Longmans, Green & Co., N. Y. 22 Filed: Mar. 24, 1975 Primary Examiner-Edward Stern (21 Appl. No.: 561,161 Attorney, Agent, or Firm-William J. Daniel 30 Foreign Application Priority Data 57 ABSTRACT May 9, 1974 Japan................................ 49-51.538 A method for producing hydrogen from water in May 17, 1974 Japan................................ 49-54504 which hydrogen is produced by reducing water using metallic germanium and the by-product, germanium 52 U.S. Cl................................... 423/657; 423193; monoxide, is reduced with a reducing agent to metal 423/532; 423/539; 423/655; 4231592 lic germanium which is recycled and reused. In this 51) Int. C.’.................so e s so C01B 1/07; COB 1102; case, it is necessary to regulate the oxidation of metal CO1G 7700 lic germanium so as to stop at the germanium monox (58) Field of Search............. 423/657, 539, 532, 93, ide stage since the reduction of germanium dioxide to 423/592 metallic germanium is difficult. Therefore, water 56) References Cited vapor is advantageously reduced by using not less than 1 mole of metallic germanium to 1 mole of water OTHER PUBLICATIONS vapor or it is indirectly reduced with an intermediate "Comp. -
Types of Chemical Reactions
Types of Chemical Reactions Synthesis (combination) reactions – two or more substances combine to form a single substance. A + B = AB Group A metals combine with nonmetals to form ionic compounds. (To get the correct formula you must know the charges of the cations and anions that the metal and nonmetal form). 2K(s) + Cl2(g) 2KCl(s) When two nonmetals react in a synthesis reaction, there is more than one possible product. – you must be given the product name S(s) + O2(g) SO2(g) or 2S(s) + 3O2 2SO3(g) When a transition metal and a nonmetal react in a synthesis reaction, there may be more than one possible product because the transition metal could form more than one cation. – you must be given at least the charge on the cation. Fe(s) + S(s) FeS(s) Iron (II) sulfide 2Fe(s) + 3S(s) Fe2S3 Iron (III) sulfide. Nonmetal oxides (nonmetal with oxygen) react with water to produce an acid (H+ compound). SO2(g) + H2O(l) H2SO3(aq) sulfurous acid Metallic oxides (metal with oxygen) react with water to give a base (OH- compounds). Use ionic charges to write formula of product. CaO(s) + H2O(l) Ca(OH)2(aq) A metal oxide and nonmetal oxide combine to form a salt. CO2(g) + Na2O(cr) Na2CO3(s) Decomposition Reactions – a single compound is broken down into two or more products and usually require energy (heat, light or electricity) to take place. AB A + B When a binary (2 elements only) compound breaks down, the products will be those 2 elements. -
Ap Chemistry Summer Work Naming & Writing the Formulas of Chemical Compounds
Summer Work: Naming & Writing Formulas AP Chemistry AP CHEMISTRY SUMMER WORK NAMING & WRITING THE FORMULAS OF CHEMICAL COMPOUNDS Summer Work: Naming & Writing Formulas AP Chemistry Naming Simple Compounds Molecule or molecular compound is an assembly of two or more non-metal atoms tightly bonded together. A diatomic molecule is a molecule made from two atoms of the same element. The following seven elements form diatomic molecules in their natural state: H2, N2, O2, F2, Cl2, Br2, I2 An allotrope is one of two or more distinct forms of an element, such as: graphite and diamond (for carbon) and dioxygen (O2 - usually referred to simply as oxygen) and ozone (O3). Molecular compounds (also known as covalent compounds) are composed of nonmetal elements that bond together into larger particles using covalent bonds (bonds created by the sharing of their valence electrons. Molecular formulas show the exact number of atoms of each element in the molecule. Empirical formulas are the simplest whole-number ratio of the atoms in a molecular compound or an ionic compound... Ionic compounds are composed of ions and usually contain both metals and non-metals. The ions in an ionic compound form when the metal atoms give one or more electrons to the nonmetal atoms. Consequently, the metal ion is positively charged (called an cation) and the nonmetal ions are negatively charged (called the anions). Ionic compounds must be electrically neutral, so the sum of the charges of the anions and cations must equal zero. Because the formulas of ionic compounds must be empirical formulas, make sure the subscripts are reduced to their simplest ratio.