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 or 3 CF4(g) C has 4 valence electrons F has 7 valence electrons F │ F – C --- F F Carbon has 0 lone pairs Carbon has 4 bonding electrons Tetra hedral F C Fluorine is more electronegative Dipoles cancel Non polar 4 OCl2(g) O has 6 valence e- Cl has 7 valence e- Cl – O │ Cl Oxygen has 2 lone pairs Oxygen has 2 bonding electrons Angular, bent, O Cl Oxygen is slightly more electronegative than chlorine Unbalanced dipole Polar 5 C2F2(g) C has 4 valence e- F has 7 valence e- F – C Ξ C – F Carbon has 0 lone pairs Carbon has 4 bonding e-, but they all go in one direction Linear F C Fluorine is more electronegative Dipoles cancel Non polar 6 HOF(l) H has 1 valence e- O has 6 valence e F has 7 valence e- H – O │ F Oxygen has 2 lone pairs Oxygen has 2 bonding electrons Angular, Bent, O H Oxygen is more electronegative O F Fluorine is more electronegative 7 NHF2(g) N has 5 valence e H has 1 valence e- F has 7 valence e- F – N – H │ F Nitrogen has one lone pair Nitrogen has 3 bonding e- Pyramidal N F Fluorine is more electronegative N H Nitrogen is more electronegative polar
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
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 13 N2H3F(g) N – 5 valence e- H – 1 valence e- F – 7 valence e- H –N – N F │ H H N has 1 lone pair N has 3 bonding e- Pyramidal and pyramidal N H Nitrogen is more electronegative N N no dipole N F Fluorine is more electronegative polar 14 C2H5OH(l) C – 4 valence e- O – 6 valence e- H – 1 valence e- H H │ │ H -- C – C – O │ H H H C has 0 lone pairs O has 2 lone pairs C – 4 bonding e- O – 2 bonding e- Tetrahedral Tetrahedral Angular or bent or C O Oxygen is more electronegative O H Oxygen is more electronegative H C C is more electronegative polar 15 NH4+ (aq) N – 5 valence e- H – 1 valence e- H+ │ H – N--- H H N has 1 lone pair N – 3 bonding e One coordinate covalent bond with the H+ Tetrahedral N H Nitrogen is more electronegative So polar that it forms an ion 16 CO32-(aq) C has 4 valence e- O has 6 valence e- O- has 7 valence e O- - C = O │ O- C – 0 lone pairs O – 2 lone pairs O- has 2 lone pairs C – 4 bonding e- O – 2 bonding e- O- has 1 bonding e- Trigonal pyramidal C O O is more electronegative C O- O- is more electronegative So polar that it forms an ion