DOCSLIB.ORG

Stable Ion Charges Metals Form Cagons. Nonmetals Form Anions

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
Stable Ion Charges Metals Form Cagons. Nonmetals Form Anions 11 (€) ()) (q) (closer distance). luole UOI,IJ Smaller the ions 2. stronger the aEracGon IJ l€rlnaN à uollJaIa u€ sule) ,i aEracGon. Higher the charges of ions 1. stronger the à ic iq turuole eN I€4naN distance Energy charge1 x charge2 H"l Lld .tI fi Described by Coulomb’s law: H • 's1e1s,tl l{ :f'4 '(le1) apuolq) utnlpos;o aldues V (r) View of Solid Ionic Compounds (NaCl) (NaCl) Compounds Ionic Solid of View Strength of Ionic Bonding Bonding Ionic of itStrength 'suol ale suorue s€aJar{^\ 'suor 1e1aur apFoltll ulnlpos pllos ul suol asaql lo spunodwffi Jtuox,[lluenbasuo) Ielauluou H relnl (q) 'uof e pue uol e ,,1 '.torlriodruor'sll uror; (sapcaloru Jo Supslsuor) ruaua6uelly -l) +eN ."-i"t 1ni"rr"e uotleuJol aql ol speal ulolP ll lPJlneu "r" luot s punodruoJ e JaqlaqM llal uago u€f aM lo fit -a1ourro-(suor;o Suqsriuor) e ol ulolp eN lellnau P uloJ, uolpale qtoQsu'e1"oo leql prmodurooe 'punod 'punodurol r1uol [| .".i p"g)"r{r'i1",runs"rr-p,i"r1"iutt"d ue lo rapueJl eql (e) Jailaq mou{ am q)1.{1\t [{ jo aldure*" tn .,'lps a1qe1uotuuroJ se uP lo uotleurol orll g7'7 an617 s --o, ue J "r.ro, punoduroc aql ruroJ o1 raq1a3o1pulq 'apuolqJ runlpos'(tfeN aprrolt{r runrpos asnerag'uor € pue J,,,'itntlin agreqr alrsoddo;o spafqo -IJ h.{ suor -IJ aql *"N e ol ruol€ unrpos IPJlnau il pu€ uol e rpllv\ ry"1 Jtn aM'ruole alrJolqJ IeJlnau it +€N pa/urol1€sr runrpos .ror1r"i" ue 'aurrolqr qlrm PeaJ ol H E ruoJ; sJaJsueJl Ieluaruale 1l' 'Jaqloue ol ruol€ l€J}nau auo ruoq JaJ pluaruala uaqff\ ]€ql s1v\ot{ss27'7an3rd Jaqlou€ ol eJuPls alour JO auo uar{.MruJoJ suol '|\es lsnf am sv charge =0 -suPJl suoJlJala d1r'l'rpe }o Ieap lear8 y charges. -qns auo ruory suoJlJala Jo JeJSu€rlar{+ sa^Io^u I€JnuaqJ h Group 8A (noble gases): covalent compound?) (Why does Nonmetal + Nonmetal • à spunodulo] lluol u Many have variable charge = -1 TransiGons metals: I • Group 7A (halogens): • ,i, charge = group # 'sa1nraldrurs Kim Chem 30A Group 6A: charge = -2 • – + 1l aas Groups 1A,2A,3A: Jalel ari} dueur '+xa+erD ur t • sdnor8 Group 5A: charge = -3 op q)ns ol sallasruar{l pual lou jaqlg ;o • ionic compound) + Anion CaGon ( urro; (suaSopq à y9 dnorS ar{1pu € 'suor -1 E . 'suol 4 Metals form caGons . firm a/v\sv -z;;L;sluaruala Nonmetals form anions aprs raqlo aq+uo 'suol +z urroJ (sqpea { lr{tt ilr;"1a y7 dior8 Jo ionic compound Metal + Nonmetal u "qr "1qnl^".Rà urro; (qelaur aql) auqDII€ arn) sruarual" y7 a"tre ;* p;" 'suol +r w>II€ aprs aql uo 'alqel aql uI ;il;;:I" y1 dnorg aql 'aldurexa rol 'a1qe1aql Jo ual 'suot -L pue +[ qloq su.lo; ua6o'rp'{;1 saS.reqrar4 's1v\ot{svzz'z saleledesosle ,l"rrir,ia ,pqr ol dervr'a1dur1s€ uI alelar suor asaql;o 'suotue uloJl suollel pue aql uo-slua,'ala aql Jo asoql d1e' slelauruou uloll slPleuJsapl^lp leql aull a.rn8rgsv 'alqel fo i"p1t lq8ir UaI transfers electrons to nonmetal. aq1 a1r1da1saql leql aflloN 'suot uourulot "q1 aq1Surraqruarual JoJ dra'r $ aIqE+rrpotrad "' -adsa'suor;o sa8ruqc InJasn e-ot;osa6ruq1 metals combine with nonmetals Metal 77'7en65v à Most commonly, ionic form when compunds • *Memorize the following Common Ion Charges! Stable Ion Charges Charges Ion Stable Ionic Compounds Compounds Ionic 2 2 magnesium bromide MgBr d (IV) oxide lea PbO potassium chloride KCl copper (I) bromide CuBr amples of Binary Ionic Compound Ex s = iodide I = hydride H – – = bromide Br = nitride N – – 3 = chloride Cl = sulfide S – – sleleru uoqrsuEJl 2 = fluoride F = oxide O – – 2 have name of element followed by Monatomic anions ide. – onmetal) N ( Anion 2. = copper (II) Cu 2+ = copper (I) Eg. Cu + : wriGng symbols Probs Ex followed by a Roman numeral in parentheses to indicate charge. name of element bromide ion; O Br sulfide ion oxide ion; S stly transition metals) have (mo cations with variable charges etal Monatomic m b) 2- - 2- atom followed by the suffix -ide: chloride ion; Cl - = calcium ion Ca = sodium ion Eg. Na 2+ + Anions are named by using the root of the parent • suol pu€'sa1nra1o141'sruolv Z UIIICIVHf, 99 name as the element. (mostly main group metals) have same cations with fixed charge Monatomic metal a) etal) (M Cation 1. METAL + NONMETAL A. Binary Ionic Compounds: *{fl after the name of cation. *!-r{!..+ specify charge in (Roman numerals) f cation can have variable charges, remember to I * Name the cation first, anion second. : General Rule Ionic Compounds . I form anions (negaGve ions) . Cl + e Cl à – – Naming Compounds elements tend to Nonmetal electrons and gain • caGons form (posiGve ions). Chemical Nomenclature electrons to form negaGve ions called . anions Metal elements tend to electrons and lose • Anions : Atoms can gain one or more • Ions Ions Ions Ions 8/27/16 B. Polyatomic Ionic Compounds: Contain polyatomic ion as the cation, anion, or both. *Memorize the following names and charges of polyatomic ions! 1. Polyatomic cations: Names end in -ium. + + NH4 = ammonium H3O = hydronium 2. Polyatomic anions: Many contain oxygen. – 2– OH = hydroxide CO3 = carbonate – 3– NO3 = nitrate PO4 = phosphate 2– – SO4 = sulfate CN = cyanide Examples of Polyatomic Ionic Compounds NH4Cl ammonium chloride Na2CO3 sodium carbonate Mn(OH)2 manganese (II) hydroxide (NH4)2SO4 ammonium sulfate ----------------------------------------------------------------- A List of Some Polyatomic Ions Cations + Ammonium = NH4 2+ Mercury(I) = Hg2 Anions - - 2- Acetate = C2H3O2 or CH3COO Thiosulfate = S2O3 Cyanide = CN- 3- Hydroxide = OH- Phosphate = PO4 2- - Carbonate = CO3 Perchlorate = ClO4 - - Hydrogen Carbonate (bicarbonate) = HCO3 Chlorate = ClO3 Hypochlorite = ClO- - Nitrate = NO3 - 2- Nitrite = NO2 Chromate = CrO4 2- Dichromate = Cr2O7 2- Sulfate = SO4 2- - Sulfite = SO3 Permanganate = MnO4 - Hydrogen Sulfate (bisulfate) = HSO4 II. Molecular Compounds (Binary): NONMETAL + NONMETAL General Rules: Name first element first, second element second. 1. First element: Greek prefix + parent element (Exception: Don’t use “mono-”). 2. Second element: Greek prefix + parent element + “-ide” (as if it were an anion). Greek Prefixes Examples of Binary Molecular Compounds mono one N2O5 dinitrogen pentoxide di two P4O6 tetraphosphorus hexoxide tri three BF3 boron trifluoride tetra four NO nitrogen monoxide penta five CO carbon monoxide hexa six hepta seven Chem 30A Kim octa eight III. Acids 1. Binary acids: “hydro” + parent element + “ic acid” HCl hydrochloric acid HBr hydrobromic acid 2. Oxoacids: Names are derived from oxoanions. If oxoanion name ends with –ate, then acid name ends with –ic acid. – eg. NO3 is nitirite à HNO3 is nitric acid If oxoanion name ends with –ite, then acid name ends with –ous acid. – eg. NO2 is nitrite à HNO2 is nitrous acid. *Memorize the following common acids! Strong Acids Weak Acids HCl hydrochloric acid HC2H3O2 or CH3COOH acetic acid HBr hydrobromic acid H2CO3 carbonic acid HI hydroiodic acid HNO3 nitric acid H2SO4 sulfuric acid HClO4 perchloric acid Writing Formulas I. Ionic Compounds Balance charges, since compounds must be neutral! (Principle of Electrical Neutrality) Positive Charge + Negative Charge = 0 eg., magnesium bromide = MgBr2 iron(II) sulfide = FeS II. Molecular Compounds (Binary) Greek prefixes indicate number of atoms. eg., dinitrogen pentoxide = N2O5 boron trifluoride = BF3 Chem 30A Kim .
Load more

Recommended publications
  • 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
    [Show full text]
  • 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.
    [Show full text]
  • 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.
    [Show full text]
  • 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.
    [Show full text]