1. What is the difference between intermolecular forces and intramolecular bonds? Variations in the Boiling Point of Noble Gases
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1 NAME: DATE: Chemical Bonding Forces Assignment 1. What is the difference between intermolecular forces and intramolecular bonds? 2. Use your data booklet to fill in the following chart Variations in the of Noble Gases Element Number of ( o C) (K) He 2 Ne Ar Xe Rn (the number of electrons = the number of protons in an atom) Type of intermolecular force(s) 3. Graph the Number of vs the in K.
2 4. What trend is shown by the graph above? 5. Complete the following table. Variations in the of Halogens Element Number of F 2 18 Cl 2 Br 2 I 2 ( o C) (K) Type(s) of intermolecular forces present 6. Does the trend continue? 7. How does the number of electrons affect the boiling point? 8. Why are the boiling points of Ar (-186 o C) and F 2 (-188 o C) similar? 9. Complete the following table. Elements and Electronegativity Electronegativity Difference H - H H - Cl 0 Type of Bond non polar covalent moderately polar covalent Forces present London Dispersion (LD) London Dispersion (LD) Dipole (DP) Li - I H - F Ionic Very polar covalent Ionic (I) London Dispersion (LD) Dipole (DP) Hydrogen Bonding (HB) Na - Br Cl - F H - O H
3 10. The boiling points for C 6 H 5 F is 85 o C, C 6 H 5 Cl is 132 o C, C 6 H 5 I is 188 o C Circle the boiling point of C 6 H 5 Br ( 78 o C, 110 o C, 156 o C, 205 o C, 298 o C) 11. Explain the difference in boiling points between (-152 o C) and HBr (-67 o C) by HBr 12. Explain the difference in boiling points between Cl 2 (-35 o C) and C 2 H 5 Cl (13 o C) by Cl 2 C 2 H 5 Cl 13. Explain the difference in boiling points between BrF (-20 o C) and C 3 H 8 (-45 o C) by BrF C 3 H Explain the difference in boiling points between CH 3 F (-78 o C) and CH 3 OH (65 o C) by CH 3 F CH 3 OH
4 15. Explain the difference in boiling points between BrCl (5 o C) and C 2 H 5 Br (65 o C) by Compound # of electrons Difference in electronegativity Br Cl BrCl Forces C 2 H 5 Br C - Br O 16. Dimethyl ether ( CH 3 CH 3 ) has a boiling point of 24.9 o C and ethanol has a boiling point of 78 o C complete the chart and writing a sentence explaining the chart CH 3 -O-CH 3 C 2 H 5 OH 17. Which substance would be more polar CH 3 I or CH 3 F? 18. Which substance would probably have a higher boiling point? Why? 19. Complete the following table Number of Forces Rank (lowest to highest) NaCl Na C 3 H 8 C 2 H 5 OH SiO 2 C 2 H 3 Cl
5 20. Complete the following table Substance Number Boiling Type(s) of forces Polar or of Point NonPolar ( o L.D. D.P. H.B. I M N.C. C) eg. He 2 non -269 Ne Al 2 O SiO Cu H 2 Se -20 H 2 S -52 H 2 O 100 SO 2-10 CH C (diamond) 4826 C 2 H 5 F -38 C 2 H 5 Cl 13 C 2 H 5 Br 38 C 2 H 5 I 72 C 2 H 5 OH 78 KBr 1435 Al Ba(OH) CH 3 OH 65 SiC 4827 C 3 H 5 (OH) 3 glycerol 290 Explain why H 2 Se and H 2 S follow the trend of the more electrons the higher the boiling point for Group 16 but H 2 O does not. Substance #2 21. Complete the following table. Force(s) # of electrons Substance #2 Force(s) # of electrons Substance with Higher (a) HCl(g) I 2 (b) CH 3 F (c) H 2 O CH 3 OH H 2 S (d) SiO 2 SO 2 (e) Fe (f) CH 3 OH CuO (g) NH 3 CH 4 (h) HCl(g) (i) SiC NaCl Cu
6 22. Complete the table by filling in the appropriate bond type. (London Dispersion, Dipole-Dipole, Hydrogen Bonding, Ionic, Metallic, Network Covalent) Bond Type Characteristics of Some General Properties Examples Formulation by covalent bonds of an atom by adjacent atoms within a 3-D lattice of atoms. Very hard, very high melting point, insoluble in most ordinary solvents, non conductors of electricity. C (s) SiO 2(s) SiC (s) of an ion by it s surrounding ions of opposite charge within an ionic crystal lattice of free valence electrons by metallic cations High melting and boiling points: dissolve in polar liquids to form conducting solutions; electrical conductors in liquid phase. Lustrous, malleable, good electrical conductors, wide range of melting points. NaCl (s) CuSO 4(s) Al (s) Fe (s) Hg (l) of electrons of one molecule by their own nucleus and by the nuclei of adjacent molecules. of a hydrogen ion (proton) by the electron pairs of adjacent N, O or F atoms of a molecular dipole by the surrounding molecular dipoles Relatively low melting solids, gases or liquids because of relatively weak intermolecular forces Relatively high melting solids gases or liquids because of relatively strong intermolecular attraction A weak intermolecular force which exists in addition to London Dispersion forces in polar molecules. Low melting solids, liquids and gases. H 2(g) CO 2(g) H 2 O (l) NH 3(g) CH 3 COOH (l) H 2 S 23. Complete the table by filling in the appropriate bond type. (London Dispersion, Dipole-Dipole, Hydrogen Bonding, Ionic, Metallic, Network Covalent)
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