Molecules and Compounds Compounds Display Constant Composition

1. Molecules and CompoundsCompounds Display Constant Composition • Elements combine in fixed Proportions • Law of Constant Composition • H2O • CO2

2. Molecules and CompoundsCompounds Display Constant Composition If we decompose water, we find 16.0 grams of oxygen to every 2.00 grams of hydrogen. This produces an Oxygen to Hydrogen mass ratio of 8.0. Mass ratio = 16.0 grams = 8.0 2.00 grams Water has a constant Mass Ratio of Oxygen to Hydrogen of 8.0.

3. Molecules and CompoundsChemical Formulas: How to Represent Compounds • Chemical Formula • Elements present • Relative numbers • Subscripts • Part of the definition • Changing subscript changes compound • Metals – Left-hand side of Periodic Table • Listed first • Nonmetals – Right-hand side of the Periodic Table • Those to the left- • More Metal-like • Listed first

4. Significance of Chemical Formulas • A chemical formula indicates the relative number of atoms of each kind in a chemical compound. • For a molecular compound, the chemical formula reveals the number of atoms of each element contained in a single molecule of the compound. • example: octane —C8H18

5. Molecules and CompoundsWriting Chemical Formulas • Compound containing 2 aluminum atoms to every 3 oxygen atoms • Al2O3 • Compound containing 3 oxygen atoms to every 1 sulfur atom • SO3

6. Molecules and CompoundsChemical Formulas: How to Represent Compounds • Water – H2O • Hydrogen and oxygen atoms • 2:1 ratio • Symbol and subscript • Dihydrogen monoxide

7. Chemical Formulas and CompoundsChemical Formulas: How to Represent Compounds • Carbon dioxide – CO2 • Carbon and oxygen atoms • 1:2 ratio • Symbol and subscript • Carbon dioxide • Two nonmetals • Left-most listed first • One carbon – not mono

8. The chemical formula for an ionic compound represents one formula unit—the simplest ratio of the compound’s positive ions (cations) and its negative ions (anions). • example: aluminum sulfate — Al2(SO4)3 • Parentheses surround the polyatomic ion SO42- to identify it as a unit. The subscript 3 refers to the unit.

9. Molecules and CompoundsWriting Chemical FormulasPolyatomic Ions • Contain several identical groupings of atoms • Polyatomic Ions • Parenthesis • Mg(NO3)2 • Magnesium nitrate

10. Molecules and CompoundsWriting Chemical FormulasPolyatomic Ions • Mg(NO3)2 • 1 Mg • 2 N • 6 O

11. Molecules and CompoundsMolecular View of Elements and Compounds • Atomic Elements • Single atoms • Most Elements • Molecular Elements • Diatomic atoms • Two atoms bonded together • H2,N2, O2, F2, Cl2, Br2, I2 • Molecular Compounds • Two or more Nonmetals • Ionic Compounds • Metal and nonmetal

12. Molecules and CompoundsMolecular View of Elements and Compounds

13. Molecules and CompoundsWriting Formulas for Ionic Compounds • Charge Neutral • Most elements form only one type of ion • Predictable charge • Sodium chloride • Na  +1 • Cl  –1 • NaCl • Magnesium chloride • Mg  +2 • Cl  –1 • MgCl2

14. Common Monatomic Ions(pg.221 in your textbook)

15. Common Monatomic Ions…

16. Molecules and CompoundsWriting Formulas for Ionic Compounds • Write the symbol for the metal and its charge • Write the symbol for the nonmetal and its charge • Charge (without sign) becomes subscript for other ion • Reduce subscripts to smallest whole number ratio • Check that the sum of the charges of the cation cancels the sum of the anions

17. Molecules and CompoundsWriting Formulas for Ionic Compounds Ionic compound between aluminum and oxygen Al3+ O2– Al2O3 2 (+3) = +6 3 (–2) = –6

18. Molecules and CompoundsWriting Formulas for Ionic Compounds Ionic compound between magnesium and oxygen Mg2+ O2– MgO 1 (+2) = +2 1 (–2) = –2 Smallest whole number ratio is 1:1

19. Molecules and Compounds Naming Ionic Compounds • Metal and Nonmetal • Two Types • Type I • Metal has constant predictable charge • Inferred from group number in Periodic Table • Type II • Charge NOT always the same • Transition Metals

20. Molecules and Compounds Naming Ionic CompoundsType I Binary Ionic Compounds • Binary compounds • Two different kinds of elements • Cation + anion with IDE • Metal • Predictable constant charge • Name of metal • Nonmetal • Name of nonmetal • Ending  IDE

21. Molecules and Compounds Naming Ionic CompoundsType I Binary Ionic Compounds • Binary compounds • Two different kinds of elements • Cation + anion with IDE • Metal • Predictable constant charge • Name of metal • Nonmetal • Name of nonmetal • Ending  IDE

22. Molecules and Compounds Naming Ionic CompoundsType I Binary Ionic Compounds • MgF2 • Metal  Magnesium • Nonmetal  Fluoride • Magnesium fluoride • KBr • Metal  Potassium • Nonmetal  Bromine • Potassium bromide

23. Molecules and Compounds Naming Ionic CompoundsType I Binary Ionic Compounds • CaCl2 • Metal  Calcium • Nonmetal  Chlorine • Calcium chloride • Na2O • Metal  Sodium • Nonmetal  Oxygen • Sodium oxide

24. Molecules and Compounds Naming Ionic CompoundsType II Binary Ionic Compounds • Binary compounds • Two different kinds of elements • Cation + anion with IDE • Metal • Charge NOT always the same • Transition metals and roman numeral for charge • Name of metal • Nonmetal • Name of nonmetal • Ending  IDE

25. Molecules and Compounds Naming Ionic CompoundsType II Binary Ionic Compounds • FeCl3 • Metal  Iron • Nonmetal  Chlorine • Charge on Iron must be +3 • Iron(III) chloride • CrO • Metal  Chromium • Nonmetal  Oxygen • Charge on Chromium must be +2 • Chromium(II) oxide

26. Molecules and Compounds Naming Ionic CompoundsType II Binary Ionic Compounds • PbCl4 • Metal  Lead • Nonmetal  Chlorine • Charge on Lead must be +4 • Lead(IV) chloride • Must determine charge of Cation from the Formula

27. Molecules and Compounds Naming Ionic CompoundsPolyatomic Ions • Group of atoms with an overall charge • Common Polyatomic Ions on pg. 226 in textbook. MEMORIZE (flashcards?)

30. Molecules and Compounds Naming Ionic CompoundsPolyatomic Ions • KNO3 • Metal  Potassium • Nonmetal  Nitrate • Potassium nitrate • FeSO4 • Metal  Iron • Nonmetal  Sulfate • Iron(II) sulfate

31. Ionic Compounds Containing Polyatomic Ions…. • Write the formula for tin(IV) sulfate • Sn(SO4)2

32. Molecules and Compounds Naming Molecular Compounds • Prefixes Mono – 1 Di – 2 Tri – 3 Tetra – 4 Penta – 5 Hexa – 6 Hepta – 7 Octa – 8 Nona – 9 Deca - 10 • Molecular Compounds • Two or more nonmetals • Right of the Periodic Table • Binary Molecular Compounds • Two elements • Most “metal-like” first • Prefix [Element 1] Prefix [Element 2] • Do not begin with “mono” and if prefix is two syllables (& element starts with vowel) then drop the ending vowel of prefix.

33. Molecules and CompoundsNomenclature: Naming Compounds • Systematic ways to name compounds • Common names • Water • H2O • Common name  Water • Systematic name  Dihydrogen monoxide

34. Molecules and Compounds Naming Molecular Compounds • CO2 • Most “metal-like” – Carbon • Nonmetal – Oxygen • Carbon dioxide • N2O • Most “metal-like” – Nitrogen • Nonmetal – Oxygen • Dinitrogen monoxide

35. Give name for As2O5: • Write formula for oxygen difluoride:

36. Molecules and Compounds Naming Acids • Acids • Molecular Compounds • Form H+ • Sour Taste • Binary Acids- acids that consist of two elements (usually hydrogen and a halogen) • Oxyacids – acids that contain hydrogen, oxygen and a third element (usually a nonmetal)

37. Binary Acids… If anion ends in “ide” then acid name is “hydro—ic” • HCl hydrochloric acid • HBrhydrobromic acid • HI hydroiodic acid

38. Naming Oxyacids • No “hydro” in name • If anion ends in “ate” then acid name is “—ic” • If anion ends in “ite” then acid name is “—ous”

39. Oxyacids Anion Acid _____ sulfate SO42- sulfuric acid H2SO4 sulfite SO32- sufurous acid H2SO3 nitrate NO3- nitric acid HNO3 phosphate PO43- phosphoric acid H3PO4

40. Salts • An ionic compound composed of a cation and the anion from an acid is often referred to as a salt. • examples: • Table salt, NaCl, contains the anion from hydrochloric acid, HCl. • Calcium sulfate, CaSO4, is a salt containing the anion from sulfuric acid, H2SO4.

41. Molecules and Compounds Nomenclature Summary

42. Oxidation Numbers • The charges on the ions in an ionic compound reflect the electron distribution of the compound. • In order to indicate the general distribution of electrons among the bonded atoms in a molecular compound or a polyatomic ion, oxidation numbers are assigned to the atoms composing the compound or ion. • Unlike ionic charges, oxidation numbers do not have an exact physical meaning: rather, they serve as useful “bookkeeping” devices to help keep track of electrons.

43. Assigning Oxidation Numbers In general when assigning oxidation numbers, shared electrons are assumed to “belong” to the more electronegative atom in each bond. More-specific rules are provided by the following guidelines. • The atoms in a pure element have an oxidation number of zero. examples: all atoms in sodium, Na, oxygen, O2, phosphorus, P4, and sulfur, S8, have oxidation numbers of zero.

44. Assigning Oxidation Numbers, continued.. • The more-electronegative element in a binary compound is assigned a negative number equal to the charge it would have as an anion. Likewise for the less-electronegative element. • Fluorine has an oxidation number of –1 in all of its compounds because it is the most electronegative element.

45. Assigning Oxidation Numbers, continued.. 4. Oxygen usually has an oxidation number of –2. • Exceptions: • In peroxides, such as H2O2, oxygen’s oxidation number is –1. • In compounds with fluorine, such as OF2, oxygen’s oxidation number is +2. 5. Hydrogen has an oxidation number of +1 in all compounds containing elements that are more electronegative than it; it has an oxidation number of –1 with metals.

46. Assigning Oxidation Numbers, continued.. • The algebraic sum of the oxidation numbers of all atoms in an neutral compound is equal to zero. • The algebraic sum of the oxidation numbers of all atoms in a polyatomic ion is equal to the charge of the ion. • Although rules 1 through 7 apply to covalently bonded atoms, oxidation numbers can also be applied to atoms in ionic compounds similarly.

47. Assigning Oxidation Numbers, continued.. Assign oxidation numbers to each atom in the following compounds or ions: a. UF6 b. H2SO4 c. ClO3-

48. Molecules and Compounds Formula Mass & Molar Mass • Formula Mass - Average mass of the Molecules that compose a compound (in a.m.u.’s) • Molar Mass – Average mass of the molecules that compose a mole (6.02x1023) of the compound (in grams/mole) Same values different units!

49. Molar Mass Calculation What is the molar mass of barium nitrate, Ba(NO3)2? • 261.35 g/mol What is the mass in grams of 2.50 molof oxygen gas (O2)? • 80.0g

50. Molar Mass as a Conversion Factor… Ibuprofen, C13H18O2, is the active ingredient in many nonprescription pain relievers. Its molar mass is 206.31 g/mol. • If the tablets in a bottle contain a total of 33 g of ibuprofen, how many moles of ibuprofen are in the bottle? • How many molecules of ibuprofen are in the bottle? • What is the total mass in grams of carbon in 33 g of ibuprofen?