– Empirical Lewis Diagram Central Atom(s) Central shape(s) Bond dipoles Polar or – formula / Show valence e- lone pairs Atoms(s) around each Non-polar Molecular only formula bonding e- central formula atom – Ξ – 8 C2IBr(l) C has 4 valence e Br C C I Both C atoms Both C atoms Linear C Br polar – I and Br both have have 0 lone pairs have 4 Br is more 7 valence e bonding electronegative electrons – C I but only 2 I is slightly more directions electronegative 9 CHClBr2(l) C- 4 valence e- Br C has 0 lone pairs C has 4 tetrahedral C Br polar H – 1 valence d │ bonding e- Br is more – – Cl and Br 7 H C--- Br electronegative valence e- C Cl Cl Chlorine is more electronegative C H C is more electronegative 10 C – 4 valence e- F – C = C – F C has 0 lone pairs C has 4 Trigonal C H polar – │ │ H 1 valence e- bonding e-, planar C is more – F 7 valence e- H F but 3 electronegative directions C F Fluorine is more electronegative 11 H2O2(l) H – 1 valence e- H – O O has 2 lone pairs O has 2 Angular, O H polar O – 6 valence e- │ bonding e- bent, Oxygen is more O – H electronegative Can also be a ‘boat shape’ 12 CO2(g) C – 4 valence e- O = C = O C has 0 lone pairs C has 4 Linear C O Non polar – O 6 valence e- bonding e- Oxygen is more electronegative Dipole cancel
Empirical formula / Molecular formula Lewis Diagram Show valence e- only formula Central Atom(s) – lone pairs Central Atoms(s) – bonding e- shape(s) around each central atom Bond dipoles Polar or Non-polar 8 C2IBr(l) C has 4 valence e I and Br both have 7 valence e Br – C Ξ C – I Both C atoms have 0 lone pairs Both C atoms have – 4 bonding electrons – but only 2 directions Linear C Br Br is more electronegative C I I is slightly more electronegative polar 9 CHClBr2(l) C- 4 valence e- H – 1 valence d Cl and Br – 7 valence e- Br │ H – C--- Br Cl C has 0 lone pairs C has 4 bonding e- tetrahedral C Br Br is more electronegative C Cl Chlorine is more electronegative C H C is more electronegative polar 10 C – 4 valence e- H – 1 valence e- F – 7 valence e- F – C = C – F │ │ H F C has 0 lone pairs C has 4 bonding e-, but 3 directions Trigonal planar C H C is more electronegative C F Fluorine is more electronegative polar 11 H2O2(l) H – 1 valence e- O – 6 valence e- H – O │ O – H Can also be a ‘boat shape’ O has 2 lone pairs O has 2 bonding e- Angular, bent, O H Oxygen is more electronegative polar 12 CO2(g) C – 4 valence e- O – 6 valence e- O = C = O C has 0 lone pairs C has 4 bonding e- Linear C O Oxygen is more electronegative Dipole cancel Non polar
Teacher_notes_Stereochemistry_Lab.docx