Chemistry 110 Lecture Exam 2 Materials

Transcription

1 Chamras Chemistry 110 Lecture Exam 2 Materials A Brief Detour on the Development of the Periodic Table of Elements In Ancient Chinese Philosophy: In Greek Philosophy: Dmitri Mendeleev s Original Periodic Table: (Based on Average Atomic Mass) Chemical Nomenclature 1

2 A brief review on the Periodic Table: The Periodic Table: Lists all the elements that are so far known to us. Most of the elements are naturally occurring but some are human-made. Metals and non-metals are separated by the zigzag line starting at B(boron), and ending At(astatine). With the exception of aluminum (Al), all the elements touching the metal-non-metal separation line are called metalloids or semi-metals. Metals lose electrons (become cations) and non-metals gain electrons (become anions) when ionized. Metals of Groups 1, 2, and 13 assume charges of +1, +2, and +3 respectively, when ionized. Non-metals of groups 15, 16, and 17, assume charges of 3, 2, and 1 respectively, when ionized. When formulating an ionic compound, the Principle of Neutrality applies. Compound: Definition: Chemical Bonding: Ionic Bonding: Covalent Bonding: Types of Compounds: Ionic Compounds: Molecular Compounds: 2

3 Review Exercise: Determine the formulas for ionic compounds made with the following ions: a) Al 3+ and O 2 : b) Ca 2+ and P 3 : c) Li + and Cl : d) Fe 2+ and N 3 : Charges of Ions: H Li Be Simple Cations with Fixed Charges Na Mg Al K Ca Zn Rb Sr Ag Cd Cs Ba Fr Ra Simple Cations with Variable Charges Cr Mn Fe Co Ni Cu As Sn Au Hg Pb Sb Bi 3

4 H Simple Anions N O F P S Cl Br I Chemical Nomenclature: IUPAC: Types of Naming: a) Ionic Compounds b) Binary Molecular Compounds c) Acids d) Bases How to tell these types apart by just looking at the formula? Formula Indicator Example Ionic à Molecular------à Acid à Base à 4

5 Naming Ions: 1. Cations with fixed charge: {Name of Neutral Element + ion } 2. Cations with variable charge: Two methods: a) {Name of Neutral Element + Charge + ion } b) {Latin Rootname of Neutral Element + ous for lower charge, and ic for higher charge + ion } Simple Anions: {Rootname of element + ide } Naming Ionic Compounds: Element Name Lower Name Higher Name Charge Ion Charge Ion Cr chromium Cr 2+ chromous Cr 3+ chromic Mn manganese Mn 2+ manganous Mn 3+ manganic Fe ferrum Fe 2+ ferrous Fe 3+ ferric Co cobalt Co 2+ cobaltous Co 3+ cobaltic Ni nickel Ni 2+ nickelous Ni 3+ nickelic Cu cuprum Cu + cuprous Cu 2+ cupric Au aurum Au + aurous Au 3+ auric Hg mercury Hg 2+ 2 [Hg + ] mercurous Hg 2+ mercuric (hydrargyrum) Sn Stannum Sn 2+ stannous Sn 4+ stannic Pb Plumbum Pb 2+ plumbous Pb 4+ plumbic As arsenicum As 3+ arsenous As 5+ arsenic Sb antimonium Sb 3+ antimonious Sb 5+ antimonic (stibium) Bi bisemutum Bi 3+ bisemutous Bi 5+ bisemutic 5

6 1. Naming ionic compounds made of simple (monatomic) cations and anions: { Remember: Formula for ionic compoundsà cation-anion sequence} The name follows the same sequence as the formula does: a) If the cation is fixed-charge: {Name of the cation + Name of the anion} b) If the cation is a variable-charge, there are two methods: 1) { Name of element + (Charge of cation indicated in Roman numeral form) + Name of the anion} 2) { Latin name of cation + ous or ic + Name of the anion} 6

7 Practice problems for writing names and formulas: Complete the following Table: Chemical Formula IUPAC Name Chem. Formula IUPAC Name Na 3 P potassium chloride CaO FeN (two ways) aurous nitride barium fluoride manganic oxide Fe 3 N 2 (two ways) HgCl 2 Al 2 S 3 MgBr 2 SnO 2 chromium (III) phosphide iron(ii) iodide cuprous nitride silver oxide aluminum bromide copper(i) phosphide 2. Naming ionic compounds made of simple cations and polyatomic anions: Polyatomic Ions: Ions made of more than one atom. 7

8 List of Polyatomic Ions The Only Polyatomic Cation: + 2+ NH 4 ammonium ion Hg 2 mercury(i) or mercurous ion Polyatomic anions: Charge 1 Charge 2 Charge 3 H 2 PO 4 dihydrogen phosphate HPO 4 2 monohydrogen phosphate PO 4 3 phosphate H 2 PO 3 dihydrogen phosphite HPO3 2 monohydrogen phosphite PO 3 3 phosphite HCO 3 HSO 4 HSO 3 NO 3 2 bicarbonate CO 3 (hydrogen carbonate) 2 bisulfate SO 4 (hydrogen sulfate) 2 bisulfite SO 3 (hydrogen sulfite) 2 nitrate O 2 carbonate sulfate sulfite peroxide NO 2 nitrite CrO 4 2 chromate C 2 H 3 O 2 acetate Cr 2 O 7 2 BrO 4 perbromate C 2 O 4 2 dichromate oxalate BrO 3 BrO 2 BrO CN OCN SCN MnO 4 OH bromate bromite hypobromite cyanide cyanate thiocyanate permanganate hydroxide 8

9 Practice problems for writing names and formulas: Complete the following table: Chemical Formula IUPAC Name Chem. Formula IUPAC Name Na 3 PO 4 potassium chlorate CaO 2 Fe(NO 2 ) 2 (two ways) aurous nitrite barium perbromate manganic peroxide Fe(NO 3 ) 3 (two ways) mercury (I) phosphite iron(ii) hypoiodite Hg 2 Cl 2 Al 2 (SO 4 ) 3 Mg(BrO 2 ) 2 Sn(CO 3 ) 2 cuprous sulfate silver oxalate aluminum acetate copper(ii) permanganate Naming Binary Molecular Compounds: Remember: Molecular compounds are made of non-metals. Rules: 1. Naming takes the form: {(# prefix + name of the first element) + (# prefix + name of the second ion)} 9

10 2. The number of each type of element must be specified using Latin prefixes (see table below). 3. The only exception is the first element. If there is only one of the first written element in the formula, then the number should not be specified. Latin Number Prefixes: Prefix Meaning Prefix Meaning mono- one hexa- six di- two hepta- seven tri- three octa- eight tetra- four nona- nine penta- five deca- ten Practice problems for naming binary molecular compounds: Complete the following table: IUPAC Name dichloro pentaphosphide dinitrogen monoxide CO 2 N 2 O 4 NO Chemical Formula Naming Acids: Definition of Acids: 10

11 There are two methods of naming the acids: a) Binary Acids: { hydro + rootname of the second element + ic acid } HBr(aq) à b) Oxy-Acids: { rootname of the non-oxygen, non-hydrogen element + ic acid (with higher # of oxygens OR ous acid with lower # of oxygens} Examples: HBrO 3 (aq) à HBrO 2 (aq) à ***If the formula of the acid is displayed without the (aq) solution indicator, then name it as an ionic compound (name the hydrogen as a cation) uniformly, regardless of the type being binary or oxy-acid. Examples: HBr à HBrO 3 à HBrO 2 à Practice problems for naming acids: Complete the following table: IUPAC Name hydrobromic acid hydrogen nitrite hypoiodous acid hydrogen sulfide HClO 4 (aq) HClO 3 HNO 2 (aq) H 3 PO 4 Chemical Formula 11

12 Naming Bases: Definition for bases: Bases should be named as ionic compounds. Examples: NaOH KOH LiOH Ca(OH) 2 Ba(OH) 2 NH 4 OH Nomenclature Exercise: Complete the following naming tables: Name Formula Name Formula barium nitrate H 2 SO 4 (aq) dichloro pentoxide AlI 3 mercurous peroxide Hg 3 (PO 4 ) 2 bromic acid AuOH ammonium sulfite Ag 2 O 2 hydrogen perchlorate HBrO 2 sulfur trioxide Mn(NO 2 ) 3 ferric bicarbonate K 2 O hydroiodic acid NO periodic acid HCl Naming Hydrates: Hydrate (Definition): Naming: 12

13 Nomenclature Chart: 13