1 / 50

CHEMISTRY 161 Chapter 3

CHEMISTRY 161 Chapter 3. 1. Structure of an Atom. subatomic particles. electrons (‘cloud’). neutrons (nucleus). protons (nucleus). m(n) / m(e) ≈ 2000. m(n) > m(p). 2. Atomic & Mass Number. mass number (number of protons plus neutrons). atomic number (number of protons)

ebony
Télécharger la présentation

CHEMISTRY 161 Chapter 3

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. CHEMISTRY 161 Chapter 3

  2. 1. Structure of an Atom subatomic particles electrons (‘cloud’) neutrons (nucleus) protons (nucleus) m(n) / m(e) ≈ 2000 m(n) > m(p)

  3. 2. Atomic & Mass Number mass number (number of protons plus neutrons) atomic number (number of protons) (number of electrons)

  4. Compounds & Chemical Reactions • Compounds • 2. The Chemical Formula • 3. The Chemical Equation • 4. The Name of Chemicals

  5. 1. Compounds molecular compounds ionic compounds EXPI

  6. Molecular Compounds 1. consist of electrically neutral particles called molecules 2. each molecule consists of atoms 3. atoms are connected via electrons 4. connections are called bonds (‘springs’) EXPII

  7. Molecular Compounds Group Period IVA VA VIA VIIA Noble Gas 2 CH4 NH3 H2O HF Ne 3 SiH4 PH3 H2S HCl Ar 4 GeH4 AsH3 H2Se HBr Kr 5 SbH3 H2Te HI Xe lots of molecules contain hydrogen EXPIII

  8. Jupiter H2, He CH4 PH3 EXPIV

  9. Saturn H2O (s) H2, He CH4 NH3/PH3

  10. Ionic Compounds I 1. consist of charged particles 2. charged particles are called ions 3. ions are formed by electron transfers from atoms atom (neutral) take electron(s) (oxidation) add electron(s) (reduction) cation(Na+) (positive charge) (metal) anion(Cl-) (negative charge) (non-metal)

  11. Ionic Compounds II 4. ionic compounds are held together by electrostatic forces non-metal metal NaCl MgO EXPV

  12. Compounds & Chemical Reactions 1. Compounds 2. The Chemical Formula 3. The Chemical Equation 4. The Name of Chemicals

  13. 2. The Chemical Formula collection of chemical symbols used to describe the composition of elementsand compounds NaCl H2O Fe2O3 CaSO4  2 H2O

  14. 2. The Chemical Formula collection of chemical symbols used to describe the composition of elements and compounds EXPVI

  15. F2 EXPVII

  16. O2

  17. S8

  18. N2

  19. P4

  20. H2

  21. Compounds & Chemical Reactions 1. Compounds 2. The Chemical Formula 3. The Chemical Equation 4. The Name of Chemicals

  22. 3. The Chemical Equation chemical equation describes what happens in a chemical reaction chemical reaction is combination of elements and/or compounds  2 H2 + O2 H2O 2 balancing & mass conservation

  23. 3. The Chemical Equation 2 H2 + O2 2 H2O s = solid l = liquid g = gas aq = aqueous solution 2 H2(g) + O2 (g)  2 H2O (l)

  24. Examples • phosphor with oxygen 2. sulfur with oxygen 3. methane with oxygen

  25. Compounds & Chemical Reactions 1. Compounds 2. The Chemical Formula 3. The Chemical Equation 4. The Name of Chemicals

  26. Organic Compounds compounds containing mostly hydrogen and carbon minor amount other elements (N, O, S, P…) hydrocarbons H C alkanes CnH2n+2

  27. Organic Compounds? CO2 C4H10 H2CO CO H2O C4H10 combustion EXPVIII

  28. Titan – Saturn’s Largest Moon

  29. Cassini-Huygens Mission

  30. Cassini-Huygens Mission

  31. Inorganic Compounds binary compounds compounds consisting of ONLY TWO different elements NaCl CO2 CaSO4 naming compounds nomenclature nomen (Latin) = name

  32. Metal (Main Group) + Non-Metal part one (metal) part two English name of element stem + ide NaCl MgO BeS symbol stem first element second element O ox- oxygen oxide S sulf- sulfur sulfide N nitr- nitrogen nitride P phosph- phosphorus phosphide F fluor- fluorine fluoride Cl chlor- chlorine chloride Br brom- bromine bromide I iod- iodine iodide

  33. Nomenclature Inorganic Compounds main group metal element + stem + ide ionic compounds (metal + non-metal)

  34. Nomenclature Inorganic Compounds main group metal element + stem + ide ionic compounds (metal + non-metal) molecular compounds prefix + stem + ide prefix + element +

  35. Molecular Compounds PF3 PF5 CO CO2 HCl N2O5 NO NO2 Greek Prefixes mono- = 1 (often omitted) hexa- = 6 di- = 2 hepta- = 7 tri- = 3 octa- = 8 tetra- = 4 nona- = 9 penta- = 5 deca- = 10

  36. Nomenclature Inorganic Compounds main group metal element + stem + ide ionic compounds (metal + non-metal) trans. group metal oxstate + element + stem + ide FeO Fe2O3 molecular compounds stem + ide prefix + element + prefix +

  37. ionic compounds cations & anions compounds must be electrically neutral Mn+ Em- nonmetals metals transition metals charge state of ions

  38. -/+ 2/4 -/+ 3/5 -2 -1 0 +1 +2 +3 CaCl2 K2S main group metals – always start with cation

  39. oxidation states NiCl2 CuO CuCl Mn2O3 B2O3 transition metals – always start with anions

  40. molecular compounds ionic compounds polyatomic ionic compounds ammonium chloride sodium dichromate magnesium carbonate rubidium sulfate calcium phosphate

  41. Nomenclature Inorganic Compounds main group metal element + stem + ide ionic compounds (metal + non-metal) trans. group metal oxstate + element + stem + ide molecular compounds stem + ide prefix + element + prefix +

  42. Mass Percentage Composition P4O10 = X 100 % = X 100 %

  43. Example A sample was analyzed and contains 0.1417 g of nitrogen and 0.4045 g of oxygen. Calculate the percentage composition. = X 100 % 1. mass of whole sample 2. percentages of elements

  44. MOLECULAR FORMULA H2O EMPIRICAL FORMULA H2O2 HO H2O H2O P2O5 P4O10 P2*2O2*5

  45. Example A sample contains 0.522 g of nitrogen and 1.490 g of oxygen. Calculate its empirical formula. N2O5

  46. COMBUSTION CxHy CO2 H2O EXPIX

  47. COMBUSTION C3H8 + O2 + H2O CO2 0.013068 g How many grams of oxygen are consumed? • balance equation • convert to moles

  48. The combustion of a 5.217 g sample of a compound of C, H, and O gave 7.406 g CO2and 4.512 g of H2O. Calculate the empirical formula of the compound. How many grams of Al2O3 are produced when 41.5 g Al react? 2Al(s) + Fe2O3(s) Al2O3(s) + 2 Fe(s)

  49. Compounds & Chemical Reactions • Compounds • 2. The Chemical Formula • 3. The Chemical Equation • 4. The Name of Chemicals

  50. Nomenclature Inorganic Compounds main group metal element + stem + ide ionic compounds (metal + non-metal) trans. group metal oxstate + element + stem + ide molecular compounds stem + ide prefix + element + prefix +

More Related