COVALENT COMPOUNDS Unit 2 COVALENT BOND

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COVALENT COMPOUNDS Unit 2 COVALENT BOND Forms between two non-metals! Electrons are shared! Co= share Valent = electrons Since electrons are shared, no need to balance charges Covalent bonds form molecules. Molecule - group of neutral atoms held together with a covalent bond Diatomic molecules – molecule consisting of 2 atoms MOLECULES H2O2Br2F2I2N2Cl2 Compound composed of molecules is a molecular compound. MOLECULAR COMPOUNDS Molecular Compounds Properties Gases or liquids Low melting/boiling points Usually made from 2 nonmetals bonded covalently Do not conduct electricity (solid or dissolved) Molecular chemical formula shows how many atoms of each element a molecule contains. H2O – Molecular formula of water 2 Hydrogen atoms, 1 Oxygen atom CO2 – Molecular formula for Carbon Dioxide MOLECULAR 1 Carbon atom, 2 Oxygen atoms FORMULAS H:H - Lewis Dot H-H – Structural Formula H2 – Molecular chemical formula LEWIS STRUCTURES COVALENT BONDING To draw a Lewis Structure, one must know the types of atoms in the molecule, the number of atoms in the molecule and the number of valence electrons for each atom in the molecule. DOUBLE & TRIPLE COVALENT BONDS Sharing a pair of electrons creates a single covalent bond Sharing more than one pair of electrons creates double and triple covalent bonds. 2 shared pairs – Double covalent bond 3 shared pairs – Triple covalent bond Carbon, Nitrogen, Oxygen 1. First element is named first, using the full name of the element 2. The second element is named by dropping ending and adding RULES FOR “–ide” NAMING 3. Prefixes are used to denote # COVALENT of each atom present COMPOUNDS 4. Prefix mono- is never used on the first element 5. Do not reduce the subscripts PREFIXES EXAMPLE BF3 boron trifluoride N2O3 dinitrogen trioxide CO2 carbon dioxide CO Carbon monoxide NO H O NAMING 2 PRACTICE N2O5 PROBLEMS CO CCl3 Nitrogen monoxide Dihydrogen monoxide ANSWERS Dinitrogen pentoxide Carbon monoxide Carbon trichloride WRITING PRACTICE PROBLEMS Carbon Nonafluoride Diphosphorous monoxide Tetraoxygen tetrasulfide.

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AP Chemistry Free Response
AP Chemistry Exam Reactions: Questions and Answers With the new format of the exam in 2007 and the availability of both questions and answers on the web at AP Central (http://apcentral.collegeboard.com:80/apc/public/courses/4606.html), I have determined not to update this page any longer. Please create an account as a teacher at AP Central and navigate to the full exams and scoring rubrics which are available back to 2003 Beginning in 2007, question 4 is no longer 5 out of 8 responses but rather three required responses. Also, in addition to writing the reactants and products, the equation must be balanced and there is a question about the chemical reaction. 2007 (a) A solution of sodium hydroxide is added to a solution of lead(II) nitrate. If 1.0 L volumes of 1.0 M solutions of sodium hydroxide and lead(II) nitrate are mixed together, now many moles of product(s) will be produced? Assume the reaction goes to completion. (b) Excess nitric acid is added to solid calcium carbonate. Briefly explain why statues made of marble (calcium carbonate) displayed outdoors in urban areas are deteriorating. (c) A solution containing silver(I) ion (an oxidixing agent) is mixed with a; solution containing iron(II) ion (a reducing agent). If the contents of the reaction mixture described above are filtered, what substance(s), if any, would remain on the filter paper? - 2+ → (a) (i) Balanced equation: 2OH + Pb Pb(OH)2 (s) (ii) The moles of each reactant are obtained by multiplying the volume times the molarity.
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Nitrogen Oxide - Wikipedia, the Free Encyclopedia Page 1 of 3
Nitrogen oxide - Wikipedia, the free encyclopedia Page 1 of 3 Nitrogen oxide From Wikipedia, the free encyclopedia Nitrogen oxide can refer to a binary compound of oxygen and nitrogen, or a mixture of such compounds: Contents ■ Nitric oxide (NO), nitrogen(II) oxide ■ Nitrogen dioxide (NO2), nitrogen(IV) oxide ■ 1 NOx ■ Nitrous oxide (N2O), nitrogen(I) oxide ■ 2 Derivatives ■ Nitrate radical (NO3), nitrogen(VI) oxide ■ 3 See also ■ Dinitrogen trioxide (N2O3), nitrogen(II,IV) oxide ■ 4 References ■ Dinitrogen tetroxide (N2O4), nitrogen(IV) oxide ■ Dinitrogen pentoxide (N2O5), nitrogen(V) oxide In atmospheric chemistry and air pollution and related fields, nitrogen oxides refers specifically to NOx [1][2] (NO and NO2). Only the first three of these compounds can be isolated at room temperature. N2O3, N2O4, and N2O5 all decompose rapidly at room temperature. Nitrate radical is very reactive. N2O is stable and rather unreactive at room temperature, while NO and NO2 are quite reactive but nevertheless quite stable when isolated. Dinitrogen trioxide, Nitric oxide, NO Nitrogen dioxide, NO2 Nitrous oxide, N2O N2O3 Dinitrogen tetroxide, Dinitrogen pentoxide, N2O4 N2O5 http://en.wikipedia.org/wiki/Nitrogen_oxide 11/2/2010 Nitrogen oxide - Wikipedia, the free encyclopedia Page 2 of 3 NOx Main article: NOx NOx (often written NOx) refers to NO and NO2. They are produced during combustion, especially at high temperature. These two chemicals are important trace species in Earth's atmosphere. In the troposphere, during daylight, NO reacts with partly oxidized organic species (or the peroxy radical) to form NO2, which is then photolyzed by sunlight to reform NO: NO + CH3O2 → NO2 + CH3O NO2 + sunlight → NO + O The oxygen atom formed in the second reaction then goes on to form ozone; this series of reactions is the main source of tropospheric ozone.
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Binary Covalent Common Names
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Nitrate Formation from Heterogeneous Uptake of Dinitrogen Pentoxide During a Severe Winter Haze in Southern China” by Hui Yun Et Al
Atmos. Chem. Phys. Discuss., https://doi.org/10.5194/acp-2018-698-RC1, 2018 © Author(s) 2018. This work is distributed under the Creative Commons Attribution 4.0 License. Interactive comment on “Nitrate formation from heterogeneous uptake of dinitrogen pentoxide during a severe winter haze in southern China” by Hui Yun et al. Anonymous Referee #1 Received and published: 23 September 2018 The manuscript of Yun et al., reported half month measurement of N2O5, ClNO2 and other relative parameters during heavy haze episodes in Pearl River Delta (PRD) of southern China. The N2O5 uptake coefficient and ClNO2 yield were determined from the observations. The study showed the observation evidence of the enhancement of particulate nitrate in the first several hours can be fully explained by the N2O5 het- erogeneous hydrolysis and even comparable with the nitric acid formed by OH+NO2 during daytime. Overall, the paper contributes to the knowledge of N2O5 heteroge- neous chemistry and highlight the heterogeneous reactions in the formation of partic- ulate nitrate in southern China. The following comments should be addressed before publishing on ACP. C1 Major comments: The steady state assumption to derive the N2O5 uptake coefficient needs to be verified by model simulations under the observed conditions (with input from NO, NO2, O3, VOCs). It is useful to try other method (e.g. Brown et al., 2006) to derive N2O5 uptake coefficient. Brown, S. S., Ryerson, T. B., Wollny, A. G., Brock, C. A., Peltier, R., Sullivan, A. P., Weber, R. J., Dube, W. P., Trainer, M., Meagher, J. F., Fehsenfeld, F. C., and Ravishankara, A.
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Chemical Names and CAS Numbers Final
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The Multiphase Chemical Kinetics of Dinitrogen Pentoxide with Aerosol Particles
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Nitrogen Oxides (Nox), Why and How They Are Controlled
United States Office of Air Quality EPA 456/F-99-006R Environmental Protection Planning and Standards November 1999 Agency Research Triangle Park, NC 27711 Air EPA-456/F-99-006R November 1999 Nitrogen Oxides (NOx), Why and How They Are Controlled Prepared by Clean Air Technology Center (MD-12) Information Transfer and Program Integration Division Office of Air Quality Planning and Standards U.S. Environmental Protection Agency Research Triangle Park, North Carolina 27711 DISCLAIMER This report has been reviewed by the Information Transfer and Program Integration Division of the Office of Air Quality Planning and Standards, U.S. Environmental Protection Agency and approved for publication. Approval does not signify that the contents of this report reflect the views and policies of the U.S. Environmental Protection Agency. Mention of trade names or commercial products is not intended to constitute endorsement or recommendation for use. Copies of this report are available form the National Technical Information Service, U.S. Department of Commerce, 5285 Port Royal Road, Springfield, Virginia 22161, telephone number (800) 553-6847. CORRECTION NOTICE This document, EPA-456/F-99-006a, corrects errors found in the original document, EPA-456/F-99-006. These corrections are: Page 8, fourth paragraph: “Destruction or Recovery Efficiency” has been changed to “Destruction or Removal Efficiency;” Page 10, Method 2. Reducing Residence Time: This section has been rewritten to correct for an ambiguity in the original text. Page 20, Table 4. Added Selective Non-Catalytic Reduction (SNCR) to the table and added acronyms for other technologies. Page 29, last paragraph: This paragraph has been rewritten to correct an error in stating the configuration of a typical cogeneration facility.
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Toxicological Profile for Nitrate and Nitrite
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The Chemistry of Solvated Nitric Oxide
The Chemistry of Solvated Nitric Oxide: As the Free Radical and as Super-saturated Dinitrogen Trioxide Solutions By Kristopher A. Rosadiuk March, 2015 A thesis submitted to McGill University in partial fulfillment of the requirements in the degree of: DOCTORATE OF PHILOSOPHY Department of Chemistry, Faculty of Science McGill University Montreal, Quebec, Canada © Kristopher Rosadiuk, 2015. Abstract The unusual behaviour of the mid-oxidation state nitrogen oxides, nitric oxide (NO) and dinitrogen trioxide (N2O3), are explored in solution. Nitric oxide is shown to catalyze the cis-trans isomerizations of diazo species in aqueous and organic solutions, and a model is presented by which this proceeds by spin catalysis, making use of the unpaired electron of NO to permit access to triplet patways. Five diazo compounds are tested and compared to stilbene, which is not found to isomerize under these conditions. Dinitrogen trioxide is found to form easily in organic solvents, which stabilize the molecule even above room temperature. Solutions can be formed at chemically useful concentrations and levels of purity, and this result is compared with the sparse literature concerning this phenomenon. The chemistry of these solutions at 0˚C is surveyed extensively, with 23 distinct organic reactions and 15 inorganic reactions being described. The first reported room temperature adduct of dinitrogen trioxide is presented, as well as novel syntheses for nitrosyl chloride and nitrosylsulfuric acid. X-ray structures are also given for a previously reported benzoquinone-phenol adduct, as well as a new mixed valent-mercury nitride salt of the form Hg4N4O9. Résumé Le comportement inhabituel des oxydes d'azote aux états d’oxydations moyens, comme l’oxyde nitrique (NO) et le trioxyde dinitrique (N2O3), est exploré en solution.
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Chemical Bonding
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100 Most Important Chemical Compounds
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The Thermodynamic Properties of Nitrogen Tetroxide
NBS REFERENCE PUBLICATIONS NBSIR 86-3054 THE THERMODYNAMIC PROPERTIES OF NITROGEN TETROXIDE A111D2 Sb4bbD NAri INST OF STANDARDS & TECH R.I.C. All 102564660 D/The thermodynamic prop OCIOO U56 N0.86-3054 1906 VI 9 C.1 NBS-P Hooert u. McCarty Hans-Ulrich Steurer C.M. Daily National Bureau of Standards U.S. Department of Commerce Boulder, Colorado 80303 July 1986 -QC 100 . U56 86-3054 1986 NBS RESEARCH INFORMATION CENTER NBSIR 86-3054 THE THERMODYNAMIC PROPERTIES OF NITROGEN TETROXIDE Robert D. McCarty Hans-Ulrich Steurer C.M. Daily Thermophysics Division Center for Chemical Engineering National Engineering Laboratory National Bureau of Standards Boulder, Colorado 80303 July 1986 Sponsored by NASA John F. Kennedy Space Center, Florida 32899 (Final Report on NASA Contract CC-26848B) U.S. DEPARTMENT OF COMMERCE, Malcolm Baldrige, Secretary NATIONAL BUREAU OF STANDARDS, Ernest Ambler, Director Contents Page 1 . Introduction 1 2. Literature Search 1 3. N 2OH Dissociation 1 i). Vapor Pressure 2 5. Saturation Densities 2 6 . Conversion of P-p-T Data 3 7 . Equation of State for the Pure Components 7 8 . Mathematical Model of the Equation of State 9 9. Derived Thermodynamic Properties 11 10. Discussion 11 1 1 . Conclusions 11 12. Acknowledgments 11 13 . References 12 Appendix A 18 Appendix B 31 Appendix C 78 List of Tables Table 1. Coefficients for eq (3) 2 Table 2. Coefficients for eq ( 6 ) 3 Table 3. Coefficients for eq (Ml) 10 Table 4. Critical Point Constraints 10 Table A1 . Comparison of Experimental and Calculated Densities Used in Fitting eq (41 ) 19 Table A2.
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