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1.1 Atoms And Bonding
- 5. 1.1 Atoms and Bonding
- 13. Ionic Bonding sodium atom (Na) sodium ion (Na + ) 11 protons (+) 10 electrons (-) one (+) charge 11p 12n 11p 12n + electron given up
- 14. Ionic Bonding 17p 18n 17p 18n electron accepted 17 protons (+) 18 electrons (-) one (-) charge chlorine atom (Cl) chlorine ion (Cl - ) -
- 15. Ionic Bonding 11p 12n 17p 18n Na Cl +
- 16. Ionic Bonding sodium chloride (NaCl) 11p 12n + 17p 18n -
- 18. Covalent Bonding Cl + Cl 17p 18n 17p 18n
- 19. Covalent Bonding Cl-Cl chlorine gas (Cl 2 ) 17p 18n 17p 18n
- 23. Electronegativity larger eletronegativity - smaller electronegativity = difference in electronegativity
- 24. Electronegativity Examples: O 2 -> oxygen has an EN of 3.44 3.44 - 3.44 = 0 ∆ EN = 0, therefore each atom in an oxygen molecule has an equal attraction for the bonding pair of electrons. This is a covalent bond.
- 25. Electronegativity Examples: HCl -> H has an EN of 2.20, Cl has an EN of 3.16 3.16 - 2.20 = 0.96 ∆ EN = 0.96, therefore chlorine has a slightly great pull on the bonding pair of electrons. This is a polar covalent bond.
- 26. Electronegativity Examples: NaCl -> Na has an EN of 0.93, Cl has an EN of 3.16 3.16 - 0.93 = 2.23 ∆ EN = 2.23, therefore chlorine has a substantially greater pull on the bonding pair of electrons. This is an ionic bond.
- 30. Hydrogen Bonding hydrogen bonding in water