DOCSLIB.ORG

Chapter 5: Molecules and Compounds

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
Chapter 5: Molecules and Compounds Chemistry 12 Ch 5: Molecules and Compounds P a g e | 1 Chapter 5: Molecules and Compounds Read Chapter 5 Check for MasteringChemistry due dates. Pure Substances and Mixtures: Pure substances have one invariable composition (elements and compounds) Mixtures have a variable composition. Homogeneous mixtures (solutions) mix uniformly throughout the mixture (coffee, salt water, air) while Heterogeneous mixtures are not uniform, they vary in texture and have regions of different composition (soil, pencil). Law of Constant Composition: Joseph Proust (1754-1826) All samples of a pure compound have the same proportions of their elements. Chemistry 12 Ch 5: Molecules and Compounds P a g e | 2 Chemicals: The properties of chemicals (pure substances) vary widely and greatly depend on how they are organized. Table salt is sodium chloride, but its properties are very different than elemental sodium or elemental chloride. We have learned about elements such as where to find metals or nonmetals on the periodic table, their symbols and names, as well as compounds which have a fixed ratio of two or more different elements. Now we will study a how to write out chemical formulas and name them (nomenclature). Chemical Formula: Chemicals are represented by element symbols and subscripts following those elements, indicating the number of atoms. By convention, a subscript of 1 is omitted. Parentheses are used when grouping more than one of the same polyatomic ions together. Example 1: How many atoms of each and atoms total are in the following chemicals? a) H2O b) NH4Cl c) Al2(SO4)3 d) C4H10S e) Cholesterol, C27H45OH Generally, the cation or more metallic element comes first followed by the anion or more nonmetallic elements. When dealing with organic formulas the order is usually, CxHyothers as listed in the table below. The anion hydroxide is one exception to this general order: OH-1 Example 2: Write the formulas when the following atoms make a compound. Remember to write the more metallic element first, except for organic compounds write CxHyothers. a) 4 chlorine and 1 carbon b) 3 oxygen, 2 iron (rust) c) 1 cobalt, 3 bromine d) 8 carbon, 18 hydrogen (octane) e) 2 oxygen, 4 hydrogen, 2 carbon Chemistry 12 Ch 5: Molecules and Compounds P a g e | 3 Chemical Bonds: Compounds and elements may have covalent bonds (molecules) Covalent bonds share electrons and are found in molecules made up when two or more nonmetals combine. Examples: elemental oxygen, O2; compound sucrose table sugar, C12H22O11 Compounds may have ionic bonds (formula units) Ionic bonds transfer electrons and are found in compounds made up from combining cations (metals, positively charged) with anions (nonmetals, negatively charged). Examples: table salt, sodium chloride, NaCl; rust, iron(III) oxide, Fe2O3 Chemical Formulas: Structural Formula will show the specific connections between atoms within a molecule and gives more information than a chemical formula alone. Example: formula = C2H6O, condensed structural formula = CH3CH2OH or structural formula = Empirical Formula gives the relative number of atoms of each element in a compound. Molecular Formula gives the actual number of atoms of each element in a molecule of the compound. Molecular N2O4 Empirical NO2 Comparison microscopic views for methane, CH4: Note: the empirical and molecular formulas of CH4 are the same. Chemistry 12 Ch 5: Molecules and Compounds P a g e | 4 Acids and Bases (Arrhenius’ Definition): 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. Nomenclature: Elements: Elements may be atomic or molecular. (Know your elements by name and symbol) Most elements are written in an atomic form and given the element name: Cu-copper, 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 elements are polyatomic: P4 is phosphorus, sulfur can be S, S2, or S8 (most common pure form) Some elements form more than one molecule/structure (allotropes) O2 is oxygen, O3 is ozone; C(graphite), C(diamond), C60 (buckminsterfullerene) 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 (Made up from nonmetallic elements) 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 (carbon based) Alkanes (CnH2n+2) Methane CH4, ethane C2H6, propane C3H8, butane C4H10, pentane C5H12, hexane C6H14, heptane C7H16, octane C8H18, nonane C9H22, decane C10H22 Organic molecules have functional groups that help identify properties. Combinations of carbon based organic molecules are enormous. Chemistry 12 Ch 5: Molecules and Compounds P a g e | 5 Ionic compounds (write cation name then anion name) In the chemical formula, the sum of positive charges must equal the sum of negative charges. If possible, reduce the subscripts to the smallest whole number ratios. Cations with known oxidation state of metal (Type I) 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 (Type II) 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 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. Be able to evaluate ion names, formulas, and charges following some basic rules. Chemistry 12 Ch 5: Molecules and Compounds P a g e | 6 Hydrates Ionic compounds can be chemically attached to a small number of water . molecules in a solid form. CuSO4 5H2O, copper (II) sulfate pentahydrate Acids + Binary acids-H cation and an anion that ends with ide. Hydro root of element ic acid. H2S, hydrosulfuric acid +1 Ternary oxyacids-H 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 Chemistry 12 Ch 5: Molecules and Compounds P a g e | 7 Formula Mass: Formula mass is the sum of the weighted average atomic masses of all the atoms in the chemical formula. Other names that apply include… molar mass, formula weight, atomic mass/weight, molecular mass, molecular weight. This is the mass in grams for one mole (6.022 x 1023particles). Nomenclature Practice: Fill in the table with formulas and names of the ionic compounds. * -2 -3 -1 Cl CO3 PO4 OH Na+1 Zn* Sn+4 +1 NH4 Al* H+1 *predict the known oxidation number Chemistry 12 Ch 5: Molecules and Compounds P a g e | 8 Nomenclature Practice: Names Formulas Chlorine Aluminum sulfide Sodium carbonate Carbon dioxide Nickel (II) chloride methane Ammonium phosphate Hydrosulfuric acid Sulfuric acid Sulfurous acid Cobalt (II) chloride hexahydrate Nomenclature Practice: H3PO4 H2SO4 (aq) H2O HBr (g) HBr (aq) MgSO4·7H2O CCl4 KMnO4 CuSO4 Al(HCO3)3 Formula Mass practice: solve for the formula masses for the species above. .
Load more

Recommended publications
  • Carbon Dioxide - Made by FILTERSORB SP3
    Technical Article MAR 2015 Chemistry of drinking water Carbon dioxide - made by FILTERSORB SP3 Carbon dioxide is a molecule with the chemical formula CO2. The linear molecule consists of a Carbon atom O C O that is doubly bonded with two Oxygen atoms. CO2 exists in water in the form of dissolved temporary hardness Ca(HCO3)2. Carbon dioxide is only water soluble when pressure is maintained. As the pressure drops CO2 will escape to air as gas. This event is characterized by the CO2 bubbles forming in /L ] Normal Seawater water. Human use carbon dioxide in many meq different ways. The most familiar example is Coca-Cola, Soft Drinks and Beer to make them fizzy. Carbon dioxide has a specific solubility in [ Alkalinity water as CO2 + H2O ⇌ H2CO3. At any given pH there is an exact mathematical relationship between H2CO3 and both bicarbonate (HCO3) and Carbonate (CO3). For example at a pH of about 9.3 in Drinking pH water the carbonate concentration is 100 The theoretical relationship between times that of carbonic acid (H2CO3). At carbonate alkalinity and pH for seawater higher pH this multiplier rises and (green and freshwater (blue) equilibrated consequently there are more HCO and 3 with the atmosphere (350 ppm carbon CO present 3 dioxide) www.watchwater.de Water ® Technology FILTERSORB SP3 WATCH WATER & Chemicals Making the healthiest water How SP3 Water functions in human body ? Answer: Carbon dioxide is a waste product of the around these hollow spaces will spasm and respiratory system, and of several other constrict. chemical reactions in the body such as the Transportation of oxygen to the tissues: Oxygen creation of ATP.
    [Show full text]
  • A Complete Guide to Benzene
    A Complete Guide to Benzene Benzene is an important organic chemical compound with the chemical formula C6H6. The benzene molecule is composed of six carbon atoms joined in a ring with one hydrogen atom attached to each. As it contains only carbon and hydrogen atoms, benzene is classed as a hydrocarbon. Benzene is a natural constituent of crude oil and is one of the elementary petrochemicals. Due to the cyclic continuous pi bond between the carbon atoms, benzene is classed as an aromatic hydrocarbon, the second [n]- annulene ([6]-annulene). It is sometimes abbreviated Ph–H. Benzene is a colourless and highly flammable liquid with a sweet smell. Source: Wikipedia Protecting people and the environment Protecting both people and the environment whilst meeting the operational needs of your business is very important and, if you have operations in the UK you will be well aware of the requirements of the CoSHH Regulations1 and likewise the Code of Federal Regulations (CFR) in the US2. Similar legislation exists worldwide, the common theme being an onus on hazard identification, risk assessment and the provision of appropriate control measures (bearing in mind the hierarchy of controls) as well as health surveillance in most cases. And whilst toxic gasses such as hydrogen sulphide and carbon monoxide are a major concern because they pose an immediate (acute) danger to life, long term exposure to relatively low level concentrations of other gasses or vapours such as volatile organic compounds (VOC) are of equal importance because of the chronic illnesses that can result from that ongoing exposure. Benzene, a common VOC Organic means the chemistry of carbon based compounds, which are substances that results from a combination of two or more different chemical elements.
    [Show full text]
  • Chemical Formula
    Chemical Formula Jean Brainard, Ph.D. Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) AUTHOR Jean Brainard, Ph.D. To access a customizable version of this book, as well as other interactive content, visit www.ck12.org CK-12 Foundation is a non-profit organization with a mission to reduce the cost of textbook materials for the K-12 market both in the U.S. and worldwide. Using an open-content, web-based collaborative model termed the FlexBook®, CK-12 intends to pioneer the generation and distribution of high-quality educational content that will serve both as core text as well as provide an adaptive environment for learning, powered through the FlexBook Platform®. Copyright © 2013 CK-12 Foundation, www.ck12.org The names “CK-12” and “CK12” and associated logos and the terms “FlexBook®” and “FlexBook Platform®” (collectively “CK-12 Marks”) are trademarks and service marks of CK-12 Foundation and are protected by federal, state, and international laws. Any form of reproduction of this book in any format or medium, in whole or in sections must include the referral attribution link http://www.ck12.org/saythanks (placed in a visible location) in addition to the following terms. Except as otherwise noted, all CK-12 Content (including CK-12 Curriculum Material) is made available to Users in accordance with the Creative Commons Attribution-Non-Commercial 3.0 Unported (CC BY-NC 3.0) License (http://creativecommons.org/ licenses/by-nc/3.0/), as amended and updated by Creative Com- mons from time to time (the “CC License”), which is incorporated herein by this reference.
    [Show full text]
  • Introduction, Formulas and Spectroscopy Overview Problem 1
    Chapter 1 – Introduction, Formulas and Spectroscopy Overview Problem 1 (p 12) - Helpful equations: c = ()() and = (1 / ) so c = () / ( ) c = 3.00 x 108 m/sec = 3.00 x 1010 cm/sec a. Which photon of electromagnetic radiation below would have the longer wavelength? Convert both values to meters. -1 = 3500 cm = 4 x 1014 Hz = (1/) = (c / ) = (1/ ) = (3.0 x 108 m/s) / (4 x 1014 s-1) = (1/ cm-1)(1 m/100 cm) = 2.9 x 10-6 m = 7.5 x 10-7 m = longer wavelength = lower energy b. Which photon of electromagnetic radiation below would have the higher frequency? Convert both values to Hz. = 400 cm-1 = 300 nm = (1/ ) = 1/ [(400 cm-1)(100 cm / 1 m)] = (c/) 8 -5 9 = 2.5 x 10-5 m = (3.0 x 10 m/s) / (2.5 x 10 nm)(1m / 10 nm) v = (3.0 x 108 m/s) / (300 nm)(1m / 109 nm) = (c/) v = 1.0 x x 1015 s-1 = (3.0 x 108 m/s) / (2.5 x 10-5 m) v = 1.2 x 1013 s-1 higher frequency c. Which photon of electromagnetic radiation below would have the smaller wavenumber? Convert both values to cm-1. = 1 m = 6 x 1010 Hz = (1 / ) -1 = ( / c) = (1 / 1m) = 1 m-1 100 cm = 100 cm-1 100 cm-1 -1 = (6 x 1010 s-1 / 3.0 x 108 m/s) = 200 m-1 -1 1 m -1 = 20,000 cm smaller wavenumber 1 m Problem 2 (p 14) - Order the following photons from lowest to highest energy (first convert each value to kjoules/mole).
    [Show full text]
  • Third-Generation Synchrotron X-Ray Diffraction of 6- M Crystal of Raite, Na
    Proc. Natl. Acad. Sci. USA Vol. 94, pp. 12263–12267, November 1997 Geology Third-generation synchrotron x-ray diffraction of 6-mm crystal of raite, 'Na3Mn3Ti0.25Si8O20(OH)2z10H2O, opens up new chemistry and physics of low-temperature minerals (crystal structureymicrocrystalyphyllosilicate) JOSEPH J. PLUTH*, JOSEPH V. SMITH*†,DMITRY Y. PUSHCHAROVSKY‡,EUGENII I. SEMENOV§,ANDREAS BRAM¶, CHRISTIAN RIEKEL¶,HANS-PETER WEBER¶, AND ROBERT W. BROACHi *Department of Geophysical Sciences, Center for Advanced Radiation Sources, GeologicalySoilyEnvironmental, and Materials Research Science and Engineering Center, 5734 South Ellis Avenue, University of Chicago, Chicago, IL 60637; ‡Department of Geology, Moscow State University, Moscow, 119899, Russia; §Fersman Mineralogical Museum, Russian Academy of Sciences, Moscow, 117071, Russia; ¶European Synchrotron Radiation Facility, BP 220, 38043, Grenoble, France; and UOP Research Center, Des Plaines, IL 60017 Contributed by Joseph V. Smith, September 3, 1997 ABSTRACT The crystal structure of raite was solved and the energy and metal industries, hydrology, and geobiology. refined from data collected at Beamline Insertion Device 13 at Raite lies in the chemical cooling sequence of exotic hyperal- the European Synchrotron Radiation Facility, using a 3 3 3 3 kaline rocks of the Kola Peninsula, Russia, and the 65 mm single crystal. The refined lattice constants of the Monteregian Hills, Canada (2). This hydrated sodium- monoclinic unit cell are a 5 15.1(1) Å; b 5 17.6(1) Å; c 5 manganese silicate extends the already wide range of manga- 5.290(4) Å; b 5 100.5(2)°; space group C2ym. The structure, nese crystal chemistry (3), which includes various complex including all reflections, refined to a final R 5 0.07.
    [Show full text]
  • 11.2 Alkanes
    11.2 Alkanes A large number of carbon compounds are possible because the covalent bond between carbon atoms, such as those in hexane, C6H14, are very strong. Learning Goal Write the IUPAC names and draw the condensed structural formulas and skeletal formulas for alkanes and cycloalkanes. Chemistry: An Introduction to General, Organic, and Biological Chemistry, Twelfth Edition © 2015 Pearson Education, Inc. Naming Alkanes Alkanes • are hydrocarbons that contain only C—C and C—H bonds • are formed by a continuous chain of carbon atoms • are named using the IUPAC (International Union of Pure and Applied Chemistry) system • have names that end in ane • use Greek prefixes to name carbon chains with five or more carbon atoms Chemistry: An Introduction to General, Organic, and Biological Chemistry, Twelfth Edition © 2015 Pearson Education, Inc. IUPAC Naming of First Ten Alkanes Chemistry: An Introduction to General, Organic, and Biological Chemistry, Twelfth Edition © 2015 Pearson Education, Inc. 1 Condensed Structural Formulas In a condensed structural formula, • each carbon atom and its attached hydrogen atoms are written as a group • a subscript indicates the number of hydrogen atoms bonded to each carbon atom The condensed structural formula of butane has four carbon atoms. CH3—CH2—CH2—CH3 butane Core Chemistry Skill Naming and Drawing Alkanes Chemistry: An Introduction to General, Organic, and Biological Chemistry, Twelfth Edition © 2015 Pearson Education, Inc. Condensed Structural Formulas Alkanes are written with structural formulas that are • expanded to show each bond • condensed to show each carbon atom and its attached hydrogen atoms Expanded Condensed Expanded Condensed Chemistry: An Introduction to General, Organic, and Biological Chemistry, Twelfth Edition © 2015 Pearson Education, Inc.
    [Show full text]
  • H2CS) and Its Thiohydroxycarbene Isomer (HCSH
    A chemical dynamics study on the gas phase formation of thioformaldehyde (H2CS) and its thiohydroxycarbene isomer (HCSH) Srinivas Doddipatlaa, Chao Hea, Ralf I. Kaisera,1, Yuheng Luoa, Rui Suna,1, Galiya R. Galimovab, Alexander M. Mebelb,1, and Tom J. Millarc,1 aDepartment of Chemistry, University of Hawai’iatManoa, Honolulu, HI 96822; bDepartment of Chemistry and Biochemistry, Florida International University, Miami, FL 33199; and cSchool of Mathematics and Physics, Queen’s University Belfast, Belfast BT7 1NN, Northern Ireland, United Kingdom Edited by Stephen J. Benkovic, The Pennsylvania State University, University Park, PA, and approved August 4, 2020 (received for review March 13, 2020) Complex organosulfur molecules are ubiquitous in interstellar molecular sulfur dioxide (SO2) (21) and sulfur (S8) (22). The second phase clouds, but their fundamental formation mechanisms have remained commences with the formation of the central protostars. Tempera- largely elusive. These processes are of critical importance in initiating a tures increase up to 300 K, and sublimation of the (sulfur-bearing) series of elementary chemical reactions, leading eventually to organo- molecules from the grains takes over (20). The subsequent gas-phase sulfur molecules—among them potential precursors to iron-sulfide chemistry exploits complex reaction networks of ion–molecule and grains and to astrobiologically important molecules, such as the amino neutral–neutral reactions (17) with models postulating that the very acid cysteine. Here, we reveal through laboratory experiments, first sulfur–carbon bonds are formed via reactions involving methyl electronic-structure theory, quasi-classical trajectory studies, and astro- radicals (CH3)andcarbene(CH2) with atomic sulfur (S) leading to chemical modeling that the organosulfur chemistry can be initiated in carbonyl monosulfide and thioformaldehyde, respectively (18).
    [Show full text]
  • Ambient Water Quality Criteria for Polycyclic Aromatic Hydrocarbons (Pahs)
    Ambient Water Quality Criteria For Polycyclic Aromatic Hydrocarbons (PAHs) Ministry of Environment, Lands and Parks Province of British Columbia N. K. Nagpal, Ph.D. Water Quality Branch Water Management Division February, 1993 ACKNOWLEDGEMENTS The author is indebted to the following individual and agencies for providing valuable comments during the preparation of this document. Dr. Ray Copes BC. Ministry of Health, Victoria, BC. Dr. G. R. Fox Environmental Protection Div., BC. MOELP, Victoria, BC. Mr. L. W. Pommen Water Quality Branch, BC. MOELP, Victoria, BC. Mr. R. J. Rocchini Water Quality Branch, BC. MOELP, Victoria, BC. Ms. Sherry Smith Eco-Health Branch, Conservation and Protection, Environment Canada, Hull, Quebec Mr. Scott Teed Eco-Health Branch, Conservation and Protection, Environment Canada, Hull, Quebec Ms. Bev Raymond Integrated Programs Branch, Inland Waters, Environment Canada, North Vancouver, BC. 1.0 INTRODUCTION Polycyclic aromatic hydrocarbons (PAHs) are organic compounds which are non- essential for the growth of plants, animals or humans; yet, they are ubiquitous in the environment. When present in sufficient quantity in the environment, certain PAHs are toxic and carcinogenic to plants, animals and humans. This document discusses the characteristics of PAHs and their effects on various water uses, which include drinking Ministry of Environment Water Protection and Sustainability Branch Mailing Address: Telephone: 250 387-9481 Environmental Sustainability PO Box 9362 Facsimile: 250 356-1202 and Strategic Policy Division Stn Prov Govt Website: www.gov.bc.ca/water Victoria BC V8W 9M2 water, aquatic life, wildlife, livestock watering, irrigation, recreation and aesthetics, and industrial water supplies. A significant portion of this document discusses the effects of PAHs upon aquatic life, due to its sensitivity to PAHs.
    [Show full text]
  • Carbohydrates: Occurrence, Structures and Chemistry
    Carbohydrates: Occurrence, Structures and Chemistry FRIEDER W. LICHTENTHALER, Clemens-Schopf-Institut€ fur€ Organische Chemie und Biochemie, Technische Universit€at Darmstadt, Darmstadt, Germany 1. Introduction..................... 1 6.3. Isomerization .................. 17 2. Monosaccharides ................. 2 6.4. Decomposition ................. 18 2.1. Structure and Configuration ...... 2 7. Reactions at the Carbonyl Group . 18 2.2. Ring Forms of Sugars: Cyclic 7.1. Glycosides .................... 18 Hemiacetals ................... 3 7.2. Thioacetals and Thioglycosides .... 19 2.3. Conformation of Pyranoses and 7.3. Glycosylamines, Hydrazones, and Furanoses..................... 4 Osazones ..................... 19 2.4. Structural Variations of 7.4. Chain Extension................ 20 Monosaccharides ............... 6 7.5. Chain Degradation. ........... 21 3. Oligosaccharides ................. 7 7.6. Reductions to Alditols ........... 21 3.1. Common Disaccharides .......... 7 7.7. Oxidation .................... 23 3.2. Cyclodextrins .................. 10 8. Reactions at the Hydroxyl Groups. 23 4. Polysaccharides ................. 11 8.1. Ethers ....................... 23 5. Nomenclature .................. 15 8.2. Esters of Inorganic Acids......... 24 6. General Reactions . ............ 16 8.3. Esters of Organic Acids .......... 25 6.1. Hydrolysis .................... 16 8.4. Acylated Glycosyl Halides ........ 25 6.2. Dehydration ................... 16 8.5. Acetals ....................... 26 1. Introduction replacement of one or more hydroxyl group (s) by a hydrogen atom, an amino group, a thiol Terrestrial biomass constitutes a multifaceted group, or similar heteroatomic groups. A simi- conglomeration of low and high molecular mass larly broad meaning applies to the word ‘sugar’, products, exemplified by sugars, hydroxy and which is often used as a synonym for amino acids, lipids, and biopolymers such as ‘monosaccharide’, but may also be applied to cellulose, hemicelluloses, chitin, starch, lignin simple compounds containing more than one and proteins.
    [Show full text]
  • Material Safety Data Sheet
    MATERIAL SAFETY DATA SHEET InfosafeNo.: ACOFS Issue Date: March 2001 Issued by: Medical Developments International Limited Revision No.: 4 Revision Date: Nov 2011 Product Name: METHOXYFLURANEINHALATIONANALGESIC (Classified as hazardous according to criteria of NOHSC) COMPANY DETAILS Company Name Medical Developments International Pty. Ltd. (ABN 14 106 340 667) Address 7/56 Smith Road, Springvale, Victoria, Australia, 3171 Tel +61 (3) 9547 1888 Fax +61 (3) 9547 0262 IDENTIFICATION Product Code ME-MEOTH, ME-7590-45, ME-MS245, ME-MS246, ME-MS260 Product Name METHOXYFLURANE INHALATION ANALGESIC Proper Shipping None Allocated Name 2,2-dichloro-1 , 1 -difluoroethyl methyl ether UN Number None Allocated DG Class None Allocated Packing Group None Allocated Hazchem Code None Allocated Poisons Schedule S4 Product Use Inhalant analgesic for pre-hospital pain relief and short surgical procedures. PENTHROX INHALER Methoxyflurane must only be administered using the Penthrox Inhaler, a polyethylene tube incorporating a polypropylene wick. Do not exceed recommended dose.. The Penthrox Inhaler is a single-patient use device. After use, replace in the carton and seal in a clean, dry, vapour-tight impervious container (polyethylene bag or jar) for disposal. The container should be clear so that the carton labeling is clearly visible. PHYSICAL DATA Appearance Clear colourless liquid with a fruity odour. Melting Point -35°C Boiling Point 104.6°C Vapour Pressure 2.66 kPa @ 17.7°C Specific Gravity 1.426 @ 25°C Flash Point 62.8°C (as tested using Closed Cup method) Flamm. Limit LEL 7% Flamm. Limit UEL Not available Solubility in Water <1 mg/L @ 19°C OTHER PROPERTIES Volatile Component 100% Evaporation Rate <1 (Ether = 1) Vapour Density >1 pH Value Not applicable Solubility in Organic Soluble in acetone, alcohol, chloroform, ether, oils and rubber.
    [Show full text]
  • The Life and Times of Carbon, Student Workbook
    ELL Chemistry Assignment # 2 Name: __________________________________ Period: Teacher:_____________________ Collecting Carbon Lesson 1 | page 1 of 4 Where Can We Find Carbon? Carbon compounds are take up carbon dioxide from three-fourths of the dry weight everywhere around us. They the air, and use photosynthesis of plants is carbohydrates. In are in our foods, plastics, soils, to turn carbon dioxide into other words, when you look at in water, in the air, and in our carbohydrates. Carbohydrates plant matter (the stem, leaves, bodies. Carbon compounds can are carbon compounds that roots, and grains) you are come in three physical forms: store energy in the forms we call looking largely at carbohydrates. gas, liquid, and solid. Plants “starches” and “sugars.” About Animals (including humans) get their carbohydrates by eating plants, but they do not store much of what they consume. In fact, less than 1% of the body weight of animals is made up of carbohydrates. The main forms of carbon are: nonliving (abiotic) in rocks, soils, and sediments, and in water, such as bicarbonate, carbonate; living (biotic), such as plant and animal matter and dead organic matter; and carbon-based gases, such as carbon dioxide (CO2), methane (CH4), and carbon monoxide (CO). Chemists use a special system to describe compounds. They use a chemical formula of symbols that indicate the elements that make up chemical compounds. A chemical formula is also called a “molecular formula.” The chemical formula of carbon dioxide is CO2 indicating one carbon atom bonded to two oxygen atoms. The symbol for carbon is C; for hydrogen is H; for oxygen is O; for silica is Si.
    [Show full text]
  • Chemical Formulas the Elements
    Chemical Formulas A chemical formula gives the numbers and types of atoms that are found in a substance. When the substance is a discrete molecule, then the chemical formula is also its molecular formula. Fe (iron) is a chemical formula Fe2O3 is a molecular formula The Elements The chemical formulas of most of the elements are simply their elemental symbol: Na (sodium) Fe (iron) He (helium) U (uranium) These chemical formulas are said to be monatomic—only an atom in chemical formula 1 The Elements There are seven elements that occur naturally as diatomic molecules—molecules that contain two atoms: H2 (hydrogen) N2 (nitrogen) O2 (oxygen) F2 (fluorine) Cl2 (chlorine) Br2 (bromine) I2 (iodine) The last four elements in this list are in the same family of the Periodic Table Binary Compounds A binary compound is one composed of only two different types of atoms. Rules for binary compound formulas 1. Element to left in Periodic Table comes first except for hydrogen: KCl PCl3 Al2S3 Fe3O4 2 Binary Compounds 2. Hydrogen comes last unless other element is from group 16 or 17: LiH, NH3, B2H4, CH4 3. If both elements are from the same group, the lower element comes first: SiC, BrF3 Other Compounds For compounds with three or more elements that are not ionic, if it contains carbon, this comes first followed by hydrogen. Other elements are then listed in alphabetical order: C2H6O C4H9BrO CH3Cl C8H10N4O2 3 Other Compounds However, the preceding rule is often ignored when writing organic formulas (molecules containing carbon, hydrogen, and maybe other elements) in order to give a better idea of how the atoms are connected: C2H6O is the molecular formula for ethanol, but nobody ever writes it this way—instead the formula is written C2H5OH to indicate one H atom is connected to the O atom.
    [Show full text]