BOHR DIAGRAMS FOR ATOMS
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1 1 SCIENCE 1206 UNIT 2 CHEMISTRY November 2012 January 2013 NAMING COMPOUNDS AND WRITING CHEMICAL FORMULAS NAME: OUTLINE BOHR DIAGRAMS FOR ATOMS TYPES OF CHEMICAL BONDS IUPAC MOLECULAR COMPOUNDS TYPES 1. SIMPLE COVALENT 2. COMMON NAME IONIC COMPOUNDS SIMPLE IONIC MULTIVALENT POLYATOMIC/COMPLEX HYDRATED IONIC ACIDS BOHR DIAGRAMS FOR ATOMS AKA: and are found in the nucleus. are found in energy levels o 1 st level o 2 nd level o 3 rd level atomic # = = # of n o = eg. Sodium (Na) o atomic # = o mass # = o # of p + = o # of e - = o # of n o =
2 2 VALENCE LEVEL Electrons in this level are called To become more stable, atoms electrons such that their valence level has the maximum number of electrons. (ie. they have the electron structure of the nearest inert noble gas.) Example: Draw a Bohr diagram for a Li atom: Example: Draw a Bohr diagram for a Ne atom: Example: Draw a Bohr diagram for a S atom: Which Bohr diagram above is drawn incorrectly?
3 3 TYPES OF CHEMICAL BONDS A CHEMICAL BOND is a. 2 TYPES of Chemical bonds o o COVALENT BOND IONIC BOND A COVALENT BOND. AKA: Occurs between. Solutions of covalently bonded substances are. An IONIC BOND is. Usually between. Solutions of ionic bonded substances are. consist of atoms or ions of two or more elements bonded together. ELECTROLYTES A solution that. General Examples: Specific Examples: NON-ELECTROLYTES A solution that. General Examples: Specific Examples:
4 4 IUPAC A global organization that. One job of the IUPAC is to give compounds. MOLECULAR ELEMENTS There are 7 elements that are, in their natural state. Other molecular elements: Memory tool: MOLECULAR COMPOUNDS Composed of. 2 TYPES: o o BINARY MOLECULAR COMPOUNDS AKA:. Composed of two types of elements (binary) Binary Molecular Compounds use IUPAC prefixes to indicate the number of each atom present:
5 5 Writing the Name from the Molecular Formula RULES: examples o N2O4 o P2O5 o CCl4 o SO3 Writing the Molecular Formula from the Name RULES: examples carbon monoxide triphosphorus pentabromide sulfur hexafluoride dicarbon tetrasulfide
6 6 TRIVIAL NAME Molecular Compounds AKA:. There are SOME molecular compounds that go by their COMMON NAMES, and we must memorize these names. Formula Trivial / Common Name O 3 H 2 O H 2 O 2 NH 3 CH 4 CH 3 OH C 2 H 5 OH C 6 H 12 O 6 C 12 H 22 O 11 HOMEWORK ALERT!!! Complete TABLES A, B, C and D in your booklet for HOMEWORK. Refer to the following notes for help: Table A o Writing the Formula from the Name Table B o Writing the Name from the Formula Table C & D o Everything! o Watch out for those common name molecular compounds!!!
7 7 TABLE A. Writing the Formula from the Name Molecular Compounds Name Formula Name Formula 1. chlorine monoxide 11. sulfur dioxide 2. oxygen difluoride 12. carbon tetrafluoride 3. boron phosphide 13. disulfur dichloride 4. dinitrogen monoxide 14. triarsenic dibromide 5. nitrogen trifluoride 15. silicon tetrachloride 6. sulfur tetrachloride 16. xenon hexafluoride 7. xenon trioxide 17. krypton difluoride 8. carbon dioxide 18. dichlorine monoxide 9. diphosphorus pentoxide 19. selenium dioxide 10. phosphorus trichloride 20. dinitrogen pentasulfide B. Writing the Name from the Formula Molecular Compounds Formula Name Formula Name 21. As 4 O P 2 O BrO S 2 Cl PH ICl N 2 O SO NI P 4 S SF SiF N 2 O OF PCl Cl 2 O 29. CO 39. SiO PBr N 2 S 5
8 8 C. Write the formulas for the following compounds in the space provided. 41. carbon dioxide 51. nitrogen monoxide 42. silicon dioxide 52. tetraphosphorus decoxide 43. water 53. silicon monocarbide 44. carbon disulfide 54. methanol 45. ammonia 55. diphosphorus pentabromide 46. carbon tetrachloride 56. arsenic tribromide 47. methane 57. carbon monoxide 48. ozone 58. sulfur dioxide 49. fluorine 59. neon 50. diphosphorus trioxide 60. dinitrogentetroxide D. Write the names for the following compounds, in the space provided. 61. CBr N 2 O 62. I C 2 H 5 OH 63. PF O N 2 O Ar 65. CO 75. P NH ClO H 2 O SiCl SCl BH SO C 2 S P 4 O OF 2
9 9 IONS Atoms other than the are, and need to to become more stable. Sharing electrons results in a. If they, atoms become and form with other atoms. WHAT IS AN ION? Ions are that have lost or gained electrons to achieve the valence configurations of a noble gas. OCTET RULE o. o NOTE: TWO TYPES OF IONS: 1. CATIONS o ions that form when an atom loses electrons. o A cation has more than and therefore has a net charge. o form cations. o MEMORY TOOL: o EXAMPLE: lithium ion 2. ANIONS: o ions that are formed when an atom electrons. o It has more than and therefore has a net charge. o form anions. o NOTE: Change the ending of the name of anions to. o MEMORY TOOL: o EXAMPLE: fluoride ion
10 10 HOMEWORK!!! Complete TABLE E in your booklet for homework! Do a few examples in class so that when you go home, you know what you are doing!!! TABLE E - SIMPLE ION FORMATION An ION forms when an atom gains or loses one or more valence electrons. Ions have a FILLED VALENCE LEVEL resulting in the SAME # OF ELECTRONS AS THE NEAREST NOBLE GAS. Positive ions (CATIONS) form when atoms lose electrons. Negative ions (ANIONS) form when atoms gain electrons. Complete the following table. Remember that the name for an ANION or nonmetallic ion ends in - ide while the full element name is used for CATIONS (metallic ions). Ion Name Ion Symbol Number of p + Number of e - Number of e - lost or gained Same electrons as which noble gas e.g. fluoride F Gained one Ne Gained two 3. potassium Lost one 4. Ca Sr H + (none) 8. 8 Gained two Lost two 10. aluminum H lithium Lost one 14. Rb
11 11 IONIC COMPOUNDS Composed of a and an. Metals form cations when they electrons. Nonmetals form anions by electrons. An ionic bond is the between these oppositely charged ions. Ions stay together in. Example: NaCl (Draw on your sheet) Example: NaCl
12 12 Ex. How does sodium fluoride form? 3 TYPES: 1. Binary Ionic Compounds SIMPLE MULTIVALENT 2. Polyatomic Ionic Compounds 3. Hydrated Ionic Compounds BINARY IONIC COMPOUNDS Binary means only 2 types of ions involved. Simple Ionic Compounds Simple ionic compounds are composed of. Given formula, write name o Rules: EXAMPLES: MgBr2 KCl Na2S Mg3P2 Ba3N2
13 13 EXAMPLES: WHAT S WRONG WITH THE FOLLOWING NAMES FOR BaS? barium sulfur Barium Sulfide barium sulfuride HOMEWORK! Do TABLE F and G in the booklet for homework. Follow rules for: o GIVEN FORMULA, WRITE NAME for Ionic Compounds. TABLE F. Writing the Name from the Formula Simple Ionic Formula Name Formula Name 1. MgS 11. K 2 S 2. KBr 12. LiBr 3. Ba 3 N Sr 3 P 2 4. Al 2 O BaCl 2 5. NaI 15. NaBr 6. SrF MgF 2 7. Li 2 S 17. Na 2 O 8. RaCl SrS 9. CaO 19. BN 10. AlP 20. AlN
14 14 TABLE G Give the correct chemical formula and name for the compounds possible between the following ions. Ion / Cl - N 3- O 2- S 2- P 3- name Na + Mg 2+ Al 3+ Ca 2+ K + Zn 2+ Li + Ba 2+ Ga 3+
15 15 Simple Ionic Compounds GIVEN NAME, WRITE FORMULA o RULES: EXAMPLES: sodium bromide barium iodide magnesium oxide aluminum oxide HOMEWORK!!! Complete TABLES H and I for homework! TABLE H: o Given NAME, Write FORMULA TABLE I: o TOP HALF Molecular Compound Naming o BOTTOM HALF Ionic Compound Naming
16 16 TABLE H. Writing the Formula from the Name Simple Ionic Name Formula Name Formula 1. magnesium oxide 11. cesium sulfide 2. lithium bromide 12. potassium chloride 3. calcium nitride 13. strontium phosphide 4. aluminum sulfide 14. barium iodide 5. potassium iodide 15. sodium fluoride 6. strontium chloride 16. calcium bromide 7. sodium sulfide 17. beryllium oxide 8. radium bromide 18. strontium sulfide 9. magnesium sulfide 19. barium fluoride 10. aluminum nitride 20. aluminum phosphide
17 Binary Ionic Compounds Simple Ions Molecular Compounds 17 TABLE I. Writing the Formula from the Name Molecular & Simple Ionic Name Formula Name Formula 1. P 4O iodine trifluoride 2. S 2F chlorine dioxide 3. N 2O methane 4. ICl boron trifluoride 5. SF 6 15 diboron hexahydride 6. CH 3OH 16. phosphorous trihydride 7. S 4N ethanol 8. H 2O carbon disulfide 9. N 2O sulfur trioxide 10. NH diarsenic trioxide 21. CaCl potassium iodide 22. MgO 32. aluminum chloride 23. NaBr 33. lithium nitride 24. Al 2O barium chloride 25. CaO 35. magnesium hydride 26. ZnO 36. magnesium chloride 27. Ag 2S 37. sodium sulfide 28. CaF zinc sulfide 29. CaH potassium chloride 30. K 2S 40. silver bromide
18 18 MULTIVALENT IONIC COMPOUNDS Ions of some transition elements can have more than one possible charge. Such elements are called. For example, what are the 2 possible charges for copper Cu? o o We use to indicate the type of charge on these multivalent ions. 1+ I 2+ II 3+ III 4+ I V 5+ V 6+ VI NOTE: GIVEN NAME, WRITE FORMULA RULES EXAMPLES: copper (II) oxide lead (IV) sulfide tin sulfide HOMEWORK!!! Do Tables J and K on the following pages! Remember to ONLY use the ROMAN NUMERAL with the MULTIVALENT IONS!!!
19 19 TABLE J. Writing the Formula from the Name Multivalent Ionic Name Formula Name Formula 1. iron(ii) chloride 11. iron(iii) chloride 2. copper(i) sulfide 12. copper(ii) sulfide 3. lead(iv) iodide 13. lead(ii) bromide 4. tin(ii) fluoride 14. tin(iv) iodide 5. mercury(i) bromide 15. mercury(ii) fluoride 6. nickel(ii) oxide 16. nickel(iv) oxide 7. chromium(iii) oxide 17. manganese(iii) chloride 8. gold(i) iodide 18. chromium(ii) nitride 9. manganese(ii) nitride 19. gold(iii) oxide 10. cobalt(iii) phosphide 20. cobalt(ii) phosphide TABLE K Give the correct chemical formula and name for the compounds possible between the following ions. Sn 2+ Cl - N 3- O 2- S 2- B r- Sn 4+ Ni 2+ Ni 3+ Au 1+ Au 3+ Cu 2+ Cu 1+
20 20 GIVEN FORMULA, WRITE NAME RULES There are 2 METHODS: a. METHOD 1 Charges must add up to zero. b. METHOD 2 Charge of Anion X Subscript of Anion Subscript of Cation Examples: PbI 2 Fe 2 O 3 CuCl MnO 2 HOMEWORK!!! Do Tables L & M for homework! Remember, doing some workings can help prevent any mistakes!!!
21 21 TABLE L. Writing the Name from the Formula Multivalent Ionic Formula Name Formula Name 1. NiS 11. CuI 2 2. VBr CuBr 3. Mn 3 N PbSe 4. Fe 2 O Fe 2 Se 3 5. FeI NiCl 2 6. Mn 3 P MnO 2 7. Cu 2 S 17. Cu 2 Se 8. CuCl TiO 2 9. NiO 19. NiSe CrF CrO TABLE M. Fill in the proper name or formula of the multivalent ionic compounds below. Formula Name Formula Name eg. CuS copper (I) sulfide 1. uranium (IV) oxide 11. lead (IV) oxide 2. lead (IV) sulfide 12. HgO 3. SnO V 2O 5 4. manganese (IV) oxide 14. tin (II) fluoride 5. Sb 2 S chromium (III) oxide 6. iron (III) oxide 16. TiO 2 7. HgS 17. AuF 3 8. PdS uranium (VI) bromide 9. copper (II) sulfide 19. NiBr FeS 20. cobalt chloride
22 22 POLYATOMIC IONIC COMPOUNDS DEFINITION:. On the back of your periodic table, there is a POLYATOMIC ION TABLE. Endings of polyatomic ions are easily recognizable as they are often or, which provides a good clue. EXAMPLES: nitrate nitrite cyanide hydroxide bicarbonate chlorate carbonate sulfate phosphate ammonium acetate GIVEN NAME, WRITE FORMULA lithium sulfate ammonium carbonate hydrogen dichromate sodium acetate GIVEN FORMULA, WRITE NAME HNO 3 NaOH KMnO 4 Cu 2 SO 4 SOME OTHER NAMES...
23 23 HOMEWORK!!! Do Tables N & O for homework!!! Remember to use the crossover method for charges. You may find it helpful to use BRACKETS around ALL polyatomic ions when writing the formulae. TABLE N. Place the symbol for each ion in the space provided, then write the correct chemical formula for the ionic compound. Be sure to balance the charges. Remember complex ions end in -ite, and -ate, except for hydroxide and ammonium. Ex : potassium K + sulfate SO4 2- K 2 SO 4 1. aluminum chloride 2. calcium sulfite 3. sodium phosphate 4. copper(ii) nitrate 5. chromium(ii) nitride 6. silver chromate 7. nickel(iii) iodide 8. barium nitride 9. sodium carbonate 10. zinc acetate 11. magnesium hydroxide 12. iron(iii) nitrite 13. mercury(i) oxide 14. copper(ii) chlorate 15. potassium tetraborate 16. aluminum bicarbonate 17. lead(ii) bisulfate 18. beryllium iodide 19. mercury(ii) nitride 20. ammonium oxide 21. iron(ii) bromide 22. strontium sulfite 23. nickel(ii) hydroxide 24. copper(ii) hydrogen sulfate 25. mercury(i) chlorate 26. aluminum carbonate 27. potassium nitrate 28. calcium phosphate
24 24 TABLE O. Provide the name of the compound or chemical formula. Chemical Formula Compound Name Chemical Formula Compound Name 1. Li2CO3 15. KH2PO4 2. K2SO4 16. potassium hydroxide 3. Al(OH)3 17. lithium phosphate 4. Fe(ClO)3 18. iron (III) hydroxide 5. H2SO4 19. sodium bicarbonate 6. Ca(HCO3)2 20. calcium chlorate 7. Pb3(PO4)2 21. hydrogen borate 8. Zn(CH3COO)2 22. ammonium nitrate 9. Cu(NO3)2 23. sodium hypochlorite 10. Cu(NO2)2 24. potassium nitrate 11. K2S2O3 12. CaCO3 25. calcium cyanide 26. chromium (III) nitrite 13. Na2Cr2O7 27. iron (II) chlorite 14. NaCN
25 25 HYDRATED IONIC COMPOUNDS Hydrated ionic compounds have attached to their crystal lattice structure. Solutions become hydrated when they are crystallized from a water solution. They are often recognizable by eye because they are often and. Examples: BLUESTONE CuSO 4 5H 2 O o. o. We indicate the presence of water with the word and we indicate the number of water molecules with our GREEK PREFIXES: o ANHYDROUS: GIVEN NAME, WRITE FORMULA barium chloride dehydrate potassium hydroxide hexahydrate sodium carbonate octahydrate cobalt (II) chloride decahydrate GIVEN FORMULA, WRITE NAME CaSO 4 2H 2 O Na 3 PO 4 4H 2 O HCN 3H 2 O HOMEWORK: COMPLETE TABLE P ON THE NEXT PAGE OF YOUR HANDOUT.
26 26 TABLE P. Provide the name or formula for each of the following. Compound Name Formula 1. copper (II) sulfate pentahydrate MgSO 4 7 H 2 O 3. potassium carbonate octahydrate MgCl 2 6 H 2 O 5. barium chloride dehydrate Cd(NO 3 ) 2 4 H 2 O 7. lithium bromide trihydrate Na 2 S 2 O 3 5 H 2 O 9. cobalt (II) chloride hexahydrate AlCl 3 6 H 2 O 11.zinc sulfate nonahydrate CaCl 2 2 H 2 O 13.barium hydroxide monohydrate Na 2 SO 4 10 H 2 O 15.magnesium silicate pentahydrate
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