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Chemistry 1A: Chapter 3 Part A Page |1 Chapter 3: Molecules, Compounds and Chemical Equations: Nomenclature, sections 3.1-3.6, 3.11 Homework: Read Chapter 3: Work out sample/practice exercises. Memorize the polyatomic ions, diatomic elements, prefixes for binary molecules, the first ten alkanes, and the Nomenclature rules of naming. Bonus Chapter 3 Problems: 23, 29, 33, 39, 41, 43, 45, 49, 51, 55 Check for the MasteringChemistry.com assignment and complete before due date Pure Substances and Mixtures: Pure substances have one invariable composition (elements and compounds) Mixtures have a variable composition. Homogeneous mixtures (solutions) are those in which the mixing is uniform throughout the mixture (coffee, salt water, air) while Heterogeneous mixtures are those in which the mixture is not uniform, they vary in texture and have regions of different composition (soil, pencil). This section will give the rules on how to name simple pure substances. Chemistry 1A: Chapter 3 Part A Page |2 Chemical Bonds: Covalent bonds share electrons and are found in molecules made up when two or more nonmetals combine. Ionic bonds transfer electrons and are found in compounds made up from combining cations (metals, positively charged) with anions (nonmetals, negatively charged). The cation is always before the anion in the formula. The net charge of the compound is zero. Propane, C3H8 Sodium Chloride, NaCl Acids and Bases: Acids are substances that increase H+1 ions in water. The cation is H+1. Bases are substances that increase OH-1 ions in water. The anion is often OH-1. Structural Formula will show the specific connections between atoms within a molecule and gives more information than a chemical formula alone. Chemistry 1A: Chapter 3 Part A Page |3 Empirical Formula is the simplest whole number ratio between atoms. Nomenclature: Elements Most elements are written in an atomic form and given the element name: Cucopper, He-Helium, Zn-zinc Seven elements are diatomic and are called by their element name: H2-hydrogen, N2, O2, F2, Cl2, Br2, I2 A couple are polyatomic: P4 is phosphorus, S8 is sulfur Some elements form more than one molecule/structure (allotropes) O2 is oxygen, O3 is ozone; C(graphite), C(diamond), C60 Chemistry 1A: Chapter 3 Part A Page |4 Common names Some molecules have been around so long they go by a common name: H2O-water, NH3-ammonia, CH4-methane, SiH4-silane Binary molecules CO2, P2O4, CCl4 Mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca Prefix (not mono) element name prefix root of element plus ide Carbon dioxide Drop the a before an o, pentoxide, not pentaoxide. Organic molecules Alkanes (CnH2n+2) Methane CH4, ethane C2H6, propane C3H8, butane C4H10, pentane C5H12, hexane C6H14, heptane C7H16, octane C8H18, nonane C9H20, decane C10H22 Functionalized hydrocarbons: alcohol, ether, aldehyde, ketone, carboxylic acid, ester amine to name a few. Alcohols (replace one H in alkane with an OH) Methanol, CH3OH; propanol, C3H7OH Carboxylic acids ( X–COOH, where the C is both double bonded to one O and single bonded to an OH). These compounds generally use their common name HCOOH; formic acid and also known as methanoic acid CH3COOH or HC2H3O2; acetic acid, also known as ethanoic acid Ionic compounds (write cation name then anion name) Cations with known oxidation state of metal Group 1A (+1), 2A (+2) , Al and Ga (+3), Zn and Cd (+2), Ag (+1) Name of ion is identical to the name of the atom for cations Variable oxidation state of metal Transition metals and metals below the nonmetal on the right have a variable oxidation state that must be indicated by Roman Numerals in parenthesis (this method is what I expect you to learn. Fe+3, iron (III); Fe+2, iron (II); Cu+1, copper (I); Sn+4, tin (IV) An alternative method differentiates from the higher oxidation number and lower oxidation number using the old form of the name and ic or Chemistry 1A: Chapter 3 Part A Page |5 ous as an ending respectively. (you should be aware of this method, but it will not be on a test) Fe+3, ferric Fe+2, ferrous; Cu+2, cupric; Cu+1, cuprous; Sn+4, stannic; Sn+2, stannous. Elemental Anions Group VA (-3); VIA (-2), VIIA (-1) Name of the element root followed by ide. N-3, nitride; S-2, sulfide, Br-1, bromide Polyatomic cations and anions Memorize the polyatomic ions and be able to evaluate ion names, formulas, and charges following some basic rules. Acids Binary acids-H+ cation and an anion that ends with ide. Hydro root of element ic acid. H2S, hydrosulfuric acid Ternary oxyacids-H+1 cation with and anion ending in ate or ite ate changes to ic acid, do not use hydro H2SO4 becomes sulfuric acid ite changes to ous acid, do not use hydro H2SO3 becomes sulfurous acid Hydrates Ionic compounds can be chemically attached to a small number of water molecules in a solid form. CuSO4.5H2O, copper (II) sulfate pentahydrate Chemistry 1A: Chapter 3 Part A Page |6 Nomenclature Practice: Fill in the table with formulas and names of the ionic compounds. Cl* CO3-2 AsO4-3 H+1 Zn* Fe+3 Sn+4 NH4+1 Al* *predict the known oxidation number OH-1 Chemistry 1A: Chapter 3 Part A Page |7 Nomenclature Practice: Names Formulas Aluminum sulfide Sodium carbonate Tetraphosphorus decoxide Nickel (II) chloride Butane Ammonium phosphate Ethanol Hydrosulfuric acid Sulfuric acid Sulfurous acid Cobalt (II) chloride hexahydrate H3PO4 H2C2O4 (aq) H2O2 HBr (g) HBr (aq) CCl4 C8H18 VClO3 CuCr2O7 (NH4)2HPO4 KMnO4