Chemistry Chapter on Atomic Structure and Oxygen
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Questions and Answers

What defines an unstable atom?

  • An atom with a stable nucleus and no excess energy
  • An atom that is chemically inert and does not emit radiation
  • An atom with a balanced number of protons and neutrons
  • An atom with an unstable nucleus characterized by excess energy (correct)

    • What is the penetrating power of alpha particles?

  • Infinite, can travel through any material
  • High, able to penetrate 10 cm in water
  • Moderate, capable of penetrating up to 1 inch of aluminum
  • Very low, can be stopped by a sheet of paper (correct)

    • Which statement about beta particle emissions is true?

  • They decrease the mass number without changing the atomic number
  • They do not affect the atomic number or mass number
  • They increase the mass number and decrease the atomic number
  • They do not alter the mass number but change the atomic number (correct)

    • What happens during the emission of a negatron?

    <p>A neutron is transformed into a proton with beta radiation emission</p> Signup and view all the answers

    What is the mass of a beta particle?

    <p>Equal to that of an electron</p> Signup and view all the answers

    What is the form in which polonium occurs as a result of decay?

    <p>Radioisotopes</p> Signup and view all the answers

    Which of the following best describes oxygen?

    <p>Non-metallic element</p> Signup and view all the answers

    Which of the following statements is true regarding the electronegativity of oxygen?

    <p>It is the second most electronegative element.</p> Signup and view all the answers

    What condition describes an inadequate oxygen tension in the air?

    <p>Anoxic</p> Signup and view all the answers

    What is one use of oxygen gas in medical treatment?

    <p>Treatment of hypoxia</p> Signup and view all the answers

    Which of the following best describes a method for administering oxygen gas?

    <p>Tubes, masks, tents</p> Signup and view all the answers

    Which of the following sources is NOT associated with sulfur?

    <p>O2 – Oxygen gas</p> Signup and view all the answers

    What is the atomic number of iron?

    <p>26</p> Signup and view all the answers

    Which of the following sources is NOT a source of iron?

    <p>Copper Sulfate</p> Signup and view all the answers

    What color is associated with ferrous compounds?

    <p>Green</p> Signup and view all the answers

    Which vitamin enhances the absorption of iron?

    <p>Vitamin C</p> Signup and view all the answers

    What is the common oxidation state of iron in its most stable forms?

    <p>Iron(II) and Iron(III)</p> Signup and view all the answers

    Which compound is known as Green Vitriol?

    <p>Ferrous Sulfate</p> Signup and view all the answers

    What is a potential adverse effect of taking Ferrous Sulfate?

    <p>Black stool</p> Signup and view all the answers

    What is the antidote for iron toxicity?

    <p>Deferoxamine</p> Signup and view all the answers

    Which triad does iron belong to?

    <p>1st Triad</p> Signup and view all the answers

    In which form of iron is it characterized as a lustrous metallic with a grayish tinge?

    <p>Elemental iron</p> Signup and view all the answers

    What is the physical state of chlorine at room temperature?

    <p>Greenish yellow gas</p> Signup and view all the answers

    Which of the following is NOT a compound of chlorine mentioned in the content?

    <p>HCl</p> Signup and view all the answers

    What test differentiates fluorine from chlorine, bromine, and iodine?

    <p>Etching test</p> Signup and view all the answers

    Which compound is used as a refrigerant and propellant?

    <p>Dichlorofluoromethane</p> Signup and view all the answers

    What is a common treatment for bromism?

    <p>Sodium chloride or Ammonium chloride</p> Signup and view all the answers

    Which statement about bromine is true?

    <p>It has a high electron affinity.</p> Signup and view all the answers

    What type of precipitate is formed when AgNO3 is used to test for chlorine?

    <p>White precipitate soluble in NH3</p> Signup and view all the answers

    Fluorine is primarily used in which of the following applications?

    <p>Dental products</p> Signup and view all the answers

    What chemical property makes chlorine essential for maintaining osmotic pressure?

    <p>It is the most predominant anion.</p> Signup and view all the answers

    What is Ferrous Gluconate known for?

    <p>Less gastric irritation</p> Signup and view all the answers

    What is the common name for Cobaltous Chloride?

    <p>Lover’s Ink</p> Signup and view all the answers

    What is the typical oxidation state of nickel?

    <p>+2</p> Signup and view all the answers

    What compound is known for its astringent and styptic properties?

    <p>Ferric Chloride</p> Signup and view all the answers

    What color does Dimethylglyoxime produce when testing for nickel?

    <p>Green</p> Signup and view all the answers

    Which iron compound is associated with titration?

    <p>Ferrous Ammonium Sulfate</p> Signup and view all the answers

    Which iron-containing compound is known as Prussian Blue?

    <p>Ferric Ferrocyanide</p> Signup and view all the answers

    What is a known deficiency associated with cobalt?

    <p>Megaloblastic Anemia</p> Signup and view all the answers

    What is Ferrous Carbonate commonly known as?

    <p>Chalybeate pills</p> Signup and view all the answers

    Which nickel compound is used as a parasiticide?

    <p>Ni+ Sulfate</p> Signup and view all the answers

    Study Notes

    Group VA - The Nitrogen Family

    • Elements: Nitrogen (N), Phosphorus (P), Arsenic (As), Antimony (Sb), Bismuth (Bi)

    Chemical Properties

    • Outer electron configuration: s2p3
    • Sharing of 3 or 5 outer electrons → 3+ & 5+ oxidation states
    • Also exhibit a -3 oxidation state (except Bismuth - Bi)
    • Bismuth does not readily accept electrons
    • Compounds of Sb, As, P, and N can accept three electrons to pair up electrons in outer p orbitals forming antimonides, arsenides, phosphides, and nitrides
    • Compounds are covalent

    Hydrides

    • M + H2 → Hydrides
    • Examples:
      • Ammonia (NH3)
      • Phosphine (PH3)
      • Arsine (AsH3)
      • Stibine (SbH3)
      • Bismuthine (BiH3)
    • All except ammonia (NH3) are highly flammable and poisonous.

    Nitrogen Cycle

    • Microbes "fix" nitrogen in nodules on the roots of pulse crops.

    Nitrogen Fixation

    • Used to making ammonia

    Nitrogen Gas

    • Used as a container
    • Used as a coolant

    Liquid Nitrogen

    • Used as a refrigerant
    • Used in cryogenics

    Other Information

    • N2O ("Laughing Gas")

      • General anesthetic (inhalational)
      • Not used alone – causes diffusion hypoxia
      • Blue cylinder

    • N2O3

      • Gas (brown color or pale blue liquid)

    • NO2

      • Brown gas

    • Phosphorus (P)

      • Normally a white waxy solid
      • Colorless and translucent
      • Stored under water
      • "St. Elmo's Fire"
      • Light carrier (match)
      • Apatite:
        • White/Yellow – Poisonous
        • Red – Non-poisonous
        • Use in preparation of matches

    • Allotropic Modification of Phosphorus: -White Phosphorus: P4 tetrahedron -Scarlet Phosphorus: made by heating PBr3 (phosphorus tribromide) with Hg at 240°C -Violet Phosphorus: heating P with a small quantity of Na at 200°C -Metallic or Black Phosphorus: heating P with Pb at 530°C

    • Arsenic (As) -Toxic, protoplasmic poison -Lewisite metal -Anti-syphilis discovered by Paul Erlich -Component of Salvarsan, Arsphenamine, Compound 606 -Antileukemia -Preparation of various insecticides -Sources: Arsenopyrite (FeAsS), Cu Aceto Arsenate, "Paris Green", K Arsenite, Fowler's Solution, Donovan's solution, AsI3 (HgI2) -Gutzeit Test: presence of arsenic in a light brown spot is a result in a filter paper moistened with silver nitrate solution -Symptoms of Arsenic poisoning: - Melanosis, Bowens disease, facial oedema, Hyperpigmentation, skin cancer, Dimness of vision, Tremor, Anorexia, Nausea, Vomiting, Diarrhoea, Weight loss, Perforation of nasal septum, Chronic laryngitis, Bronchitis

      • Antidote: BAL

    • Antimony (Sb) -Sources: Senarmontite (Sb2O3), Valentinite (Sb2O3), Cervantite (Sb2O4), Antimony Glance (Stibnite, Sb2S) -Pharmaceutical use: expectorant, emetic, anthelmintic -Antimony Potassium Tartrate ("Tartar Emetic") - Component of Brown mixture - Emetic, Expectorant, Treatment of Schistosomiasis -Babbit Metal: - Alloy of Antimony (80% Tin and 20% Antimony)

    • Bismuth (Bi) -Sources: Bismuthite (Bi2S3), Tetradymite (Bi2Te3), Bismite (Bi2O3) -Pharmaceutical use: - "Beautiful meadow" - Use in silvering of mirrors -Astringent, antiseptic, internal protective

      • Adverse effects:
        • Blue black lining of gums
        • Black stools
      • antidote: BAL -Bismuth Subcarbonate: Antacid, antiseptic, astringent; 60 grams render alimentary canal opaque to x-ray
      • Bismuth Subgallate: Active ingredient in Devrom®, an over-the-counter FDA-approved medicine -Bismuth Subnitrate ("White Bismuth"): used in the treatment of ulcer and inflammation of the GIT; Incompatible with tragacanth -Milk of Bismuth ("Bismuth Cream"): Bi(OH)3 + Bismuth Subcarbonate, for H. pylori; internal protective for gastric ulcer

    • Identification and Tests of Group VA elements:*

    • NH4+ -Nessler's reagent (alkaline K2HgI4): orange ppt of HgO.HgNH2I (iodide of Millon's base) -Heated with strong alkali: evolution of NH3 detected by its characteristic odor and change red litmus paper to blue

    • CN- -AgNO3: white ppt of AgCN (silver cyanide); insoluble in HNO3 -Hg2(NO3)2: black ppt of metallic Hg

    • Sb3+ -H2S: orange ppt of Sb2S3 soluble in Na2S -Al metal: black ppt of metallic Sb insoluble in NaOBr reagent

    • Bi3+ -H2S: brownish black ppt of Bi2S3 insoluble in Na2S reagent -Na2SnO2: black ppt of metallic Bi

    • SO32- -dil. H2SO4: evolves SO2 [odor of burnt sulfur]

    • SO42- -dil. H2SO4: NR; BaCl2: white ppt of BaSO4, which is insoluble in all acids

    • S2O32- -dil. H2SO4: evolves SO2 [odor of burnt sulfur]; KMnO4 or I2 solution: the solutions are decolorized

    • Cr3+ -NaOH: grayish green ppt of Cr(OH)3 which will dissolve in excess of the alkali to form a green solution, NaCrO2. -When an oxidizing agent like Na2O2 is added, it turns yellow due to Na2CrO4

    • CrO42- -BaCl2: yellow ppt of BaCrO4 -AgNO3: brownish red ppt of Ag2CrO4 -H2O2 and ether → blue ethereal layer due to perchromic acid (Perchromic Acid Test or Vanishing Blue Test)

    Group VB - The Vanadium Subgroup

    • Elements: Vanadium (V), Niobium (Nb), Tantalum (Ta)
    • Oxidation states: 2+ through 5+
    • Lower valence states tend to be unstable (except in the elements with the highest atomic number)
    • Acidity of oxides, basicity of hydroxides generally decrease with increasing atomic number (for V)
    • Compounds in lower oxidation states are colorful
    • Inert to chemical action in finely divided form (V, Nb, Ta)
    • Tantalum (Ta) -Unaffected by bloody fluids -Use in sheet form for surgical repair of bones, nerves, tissues -Corrosion resistant -Source: Tantalite
    • Vanadium (V)
      • Hard, silvery-grey, ductile and malleable transition metal -Source: Carnotite, Patronite, Vanadinite
    • Niobium (Nb) -Soft, grey, ductile transition metal -Often found in pyrochlore mineral (main commercial source) and columbite

    Group VI - The Chalcogens

    • Elements: Oxygen (O), Sulfur (S), Selenium (Se), Tellurium (Te), Polonium (Po)
    • Properties: Primarily non-metals, but some are metalloids; most are highly electronegative, exist primarily in their diatomic form (O2 etc.), tend to form compounds of the form M2X (where M is metal and X is a chalcogen)

    Other Information

    • Oxygen (O) -Properties: -Most abundant element in the Earth's crust. -Common element known to ancients as brimstone or burning stone. -Found on Earth as a free element/in combined form (metal sulfides/sulfates). -“Dephlogisticated Air” and “Empyreal Air”. -Most abundant element. -Nonmetallic element -2nd most electronegative element -Responsible for oxidative changes in paints, fats, fixed oils. -Green cylinder. -Allotropes: Ozone (O3), Oxygen (O2), Nascent Oxygen ([O]) -Oxygen Requirements: -Anoxic – inadequate O2 tension in air -Anemic – decrease hemoglobin -Histotoxic – tissue or cell oxidation -Stagnant – blood circulation is retarded -Uses: Treatment of hypoxia

    • Sulfur (S) -Properties: - Known to ancients as brimstone/burning stone -Common element on Earth’s crust—found free or in combined form (sulfides & sulfates). -Sources: FeS2 – Iron Pyrite, PbS – Galena, HgS – Cinnabar, ZnS – Zinc blend, CaSO4 • 2H2O – Gypsum, BaSO4 - Heavy spar -Allotropes: Rhombic, Monoclinic, Mobile, Viscous, Plastic/Amorphous, Sulfur Vapor -Different Forms: Precipitated sulfur, sublimed sulfur -Uses: Preparation of scabicidal and keratolytic ointments and lotions, stimulant cathartic, stimulant in alopecia, fumigate (SO2), Depilatory (sulfides), Keratolytic (SrS), Antiseborrheic (CdS) -Sulfuric acid ("Oil of Vitriol") -Sulfonating agent -Dehydrating agent -Sodium Thiosulfate: use in photography, treatment for ringworm, antidote for cyanide and iodine poisoning

    • Hydrogen Sulfide -"Aitch-tu-es-gas" -Reducing agent, precipitating agent of metal ions -Rotten egg odor

    • Sulfur Ointments
      -Precipitated sulfur -Liquid petrolatum -White ointment -Scabicide -Parasiticide

    • Selenium (Se) -"Moon" -Trace element -Antioxidant -Synergistic with vitamin E -Toxic when taken internally -Use in the manufacture of photocopying machines -Catalyst in nitrogen determination -Selenium Sulfide: Active constituent of Selsun Blue; Anti-seborrheic

    • Polonium (Po)

      • Radioactive isotope from the decay of actinide elements -Identification Tests: -h2S: salmon or flesh colored ppt of MnS -NaBiO3: purple solution of HMno4 (permanganic acid)

    Group VII-A - The Halogens

    • Elements: Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At)

    Other Information

    • Halogens: -Most active family of nonmetals -Exist as diatomic molecules

      • Never free in nature -Oxidation property decreases with increasing atomic number

    • Fluorine (F) -Physical state: Pale yellow gas -Chemical properties: Most electronegative element, strongest oxidizing agent, reacts violently with nonmetals -Natural Sources: Fluorospar (CaF2), Fluoroapatite (3Ca3(PO4)2Ca(CIF)), Cryolite (Na3AlF6) -Poisoning: Fluorosis (mottled enamel and abnormal bone growth) -Identification tests: Etching test (H2SO4); AgNO3: no ppt -Compounds and uses: -NaF - 2% in 4 application -SnF2- 8% freshly preparation -Dichlorofluoromethane (Freon): refrigerant & propellant

    • Chlorine (Cl) -Physical state: greenish-yellow gas -Chemical properties: Predominantly an anion, does not readily react with carbon -AKA Dephlogisticated muriatic acid -Found in large quantities as sodium chloride (NaCl) in seawater/land deposits -Identification tests: Various tests listed above -Uses: H₂O Disinfictant, various compounds

    • Bromine (Br) -Physical state: reddish brown fuming liquid -Chemical properties: toxicity—Bromism (skin eruption, psychosis, weakness), Treatment – NaCl or NH4Cl -Identification tests: AgNO3: yellow ppt of AgBr insoluble in HNO3; KMnO4, H2SO4, chloroform: orange to brown layer due to the liberation of Br2 -Compounds and uses: Koppeschaar's solution - 0.1N Bromine solutionn; Sedative; used in iodometry

    • Iodine (I) -Physical state: grayish black solid, violet-colored vapor -Chemical properties: Combines directly many elements; reacts with most metals and some nonmetals to form iodides -Identification tests: AgNO3: yellow ppt of AgI insoluble in HNO3; KMnO4, H2SO4, chloroform: violet layer due to the liberation of I2. -Uses: Expectorant, antiseptic, antimicrobial -lodine Preparations: -Strong iodine solution/ Lugol's solution -Saturated solution of potassium iodide (KISS)

    • Astatine (At) -Least electronegative element -Only synthetic halogen -Only radioactive halogen -Only metallic halogen

    Group VII-B - The Manganese Subgroup

    • Elements: Manganese (Mn), Technetium (Tc), Rhenium (Re)

    Other Information

    • Manganese (Mn) -Only metal of pharmaceutical importance in this group -Occurs mostly as oxide (MnO2) -Difficult to prepare in pure state -Used in alloy steels -Physical state: Hard, silvery-grey metal that resembles iron -Chemical Properties: exhibit oxidation states of 2+ to 7+ -2+ Compounds are good reducing agents -MnO4- (permanganate) is a good oxidizing agent -Salts: Hausmannite (complex oxide containing di- and tri-valent manganese); Braunite (silicate mineral containing di- and tri-valent manganese) -Identification tests: H2S: salmon or flesh colored ppt of MnS; NaBiO3: purple solution of HMnO4 (permanganic acid)
      -Compounds and use: -Manganese Sulfide: Trace element; cofactor in CHON synthesis for riboflavin; phosphorylation; fatty acid and cholesterol synthesis; Similar to parkinsonism -KMnO4: Mineral chameleon; oxidizing agent; volumetric soln in permanganometry

    • Technetium (Tc) -1st element produced artificially

      • Used in preparation of radiopharmaceuticals -Diagnostic agent

    • Rhenium (Re) -Extremely rare -Knowledge of its properties is available

    Group VIII-A - The Noble Gases

    • Elements: Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn)

    Other Information

    • Characteristics: -Colorless, odorless, tasteless, nonflammable gases -Traditionally labeled "group 0" because they are believed not to bond with other atoms. -Uses: -Neon: Advertising purposes; 2nd lightest noble gas; bright reddish orange light -Argon: Most abundant inert gas; present in air, natural gas, occluded minerals, dissolved in oceans and fresh waters; substitutes nitrogen; inert atmosphere for pharmaceuticals -Krypton and Xenon: Used in flash lamps and arc lamps -Radon: Inert gas given off by radium salts as decomposition product; It is itself radioactive

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