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chlorine dioxide carbon monoxide dinitrogen pentaoxide phosphorus pentachloride

chlorine dioxide carbon monoxide dinitrogen pentaoxide phosphorus pentachloride silicon monocarbide sulfur hexafluoride disulfur dichloride silicon tetrachloride silicon dioxide chlorine trifluoride tetraphosphorus decaoxide sulfur dioxide dioxygen difluoride nitrogen trichloride

riordan-nyhan
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chlorine dioxide carbon monoxide dinitrogen pentaoxide phosphorus pentachloride

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  1. chlorine dioxide carbon monoxide dinitrogen pentaoxide phosphorus pentachloride silicon monocarbide sulfur hexafluoride disulfur dichloride silicon tetrachloride silicon dioxide chlorine trifluoride tetraphosphorus decaoxide sulfur dioxide dioxygen difluoride nitrogen trichloride diboron trioxide diarsenic trisulfide

  2. chlorine monoxide oxygen difluoride beryllium oxide carbon tetrachloride phosphorus triiodide potassium permanganate zinc oxide trisilicon tetranitride nitrogen dioxide phosphorus pentabromide nitrogen dinitrogen monoxide tin(IV) cyanide dichlorine monoxide nitrogen trifluoride dichlorine octaoxide sulfur trioxide

  3. TODAY: read page 37 and pages 164-167 Diatomic molecules Lewis Dot Diagrams for Molecules HW: Worksheet – Lewis Structure exercises Retest: Monday Feb. 4 Quiz: Thursday or Fri Feb. 7 or 8

  4. ELECTRONEGATIVITYAND POLARITY • electronegativity = ability of an atom to attract electrons in a covalent bond • most electroneg. element = flourine • least electroneg. element = francium • Unequal sharing of electrons will produce a polar bond.

  5. ELECTRONEGATIVITYAND POLARITY • F–F • H–F • H2O • NH3

  6. MOLECULAR FORMULA • diatomic molecules: molecules with 2 atoms of the same element • there are 7 – know them! N2 O2 H2 Cl2 I2 F2 Br2 or Br2 I2 N2 Cl2 H2 O2 F2

  7. LEWIS DOT DIAGRAMS(ELECTRON DOT DIAGRAMS) • show the valence electrons as dots • inner electrons and atomic nuclei are represented by the symbol

  8. LEWIS DOT DIAGRAMS(ELECTRON DOT DIAGRAMS) • group 1A: 1 valence e- • group 2A: 2 valence e-, etc.

  9. LEWIS DOT DIAGRAMS(ELECTRON DOT DIAGRAMS) • diatomic molecules

  10. LEWIS STRUCTURES: STEPS 1. Count valence electrons and bonds using periodic table and octet rule – make a chart to get valence and shared electrons 2. Choose an arrangement of atoms (carbon in center, hydrogen or halogens on outside)

  11. LEWIS STRUCTURES: STEPS 3. Put in calculated number of bonds; single bonds first, then multiple bonds if necessary. 4. Where necessary to complete octets, put in non-bonding electrons in pairs.

  12. LEWIS STRUCTURES: STEPS 5. Check work by counting electrons in Lewis structure and comparing calculated number of valence electrons.

  13. lO H–C–H LEWIS STRUCTURES CH2O VS C 4 4 H 1 1 H 1 1 O 62 12 8 / 2 = 4 bonds

  14. H–N–H H LEWIS STRUCTURES NH3 VS N 5 3 H 1 1 H 1 1 H 11 8 6 / 2 = 3 bonds

  15. 2- LEWIS STRUCTURES SO32–VS S 6 2 O 6 2 O 6 2 O 62 24 8 +2-2 26 6 / 2 = 3 bonds O–S–O O

  16. POLYATOMIC IONS FROM NOW ON: know NO CO SO PO ions (–ates and –ites) know NH4+ know –ides: cyanide, hydroxide know chlorine containing ions

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