chem exam review
SCH 4U1 FINAL EXAM REVIEW
ATOMIC STRUCTURE AND MOLECULAR ARCHITECTURE
1. Describe the wave mechanical model of the atom.
2. Write the ground state electron configuration for Br.
3. Explain why the first ionization energy for Ne is significantly greater than Na.
4. Distinguish between ionization energy and electronegativity.
5. How does VSEPR Theory account for the fact that the bond angle in H2O is less than NH3?
6. Which of the following molecules are polar? Include diagrams detailing their molecular shape (according to VSEPR), bond angles and molecular dipole (if present).
CO2 BCl3 NF3 AsH3 CCl4 CH2Cl2 N2 H2S
7. Distinguish between intermolecular and intramolecular forces.
8. What is a dipole-dipole force?
9. What are hydrogen bonds?
10. a) Why is the melting and boiling point of H2O significantly higher than H2S? b) Predict and explain the relative melting and boiling points of HF, HCl, HBr and HI.
11. What are London or dispersion forces? How are they affected by molecular size?
12. Which is expected to have the higher boiling point, C8H18 or C22H46? Explain.
13. What type of solid contains particles held together primarily by van der Waals or intermolecular forces?
14. Metals can be rolled into sheets and stamped into various forms. Explain.
15. Ionic solids are hard, with very high melting points, but are very brittle. Explain.
16. Diamond and graphite are allotropes of carbon, composed of carbon atoms covalently bonded in a giant network solid. However, there are distinct differences in their properties. Diamond is extremely hard and brittle. Graphite is soft and slippery, often used as a lubricant. Graphite is also able to conduct electricity, whereas diamond cannot. Both, however, have extremely high melting and boiling points. Explain.
ORGANIC CHEMISTRY
1. Draw structural diagrams of the following:
a) 4-methyl-2-heptene b)
ATOMIC STRUCTURE AND MOLECULAR ARCHITECTURE
1. Describe the wave mechanical model of the atom.
2. Write the ground state electron configuration for Br.
3. Explain why the first ionization energy for Ne is significantly greater than Na.
4. Distinguish between ionization energy and electronegativity.
5. How does VSEPR Theory account for the fact that the bond angle in H2O is less than NH3?
6. Which of the following molecules are polar? Include diagrams detailing their molecular shape (according to VSEPR), bond angles and molecular dipole (if present).
CO2 BCl3 NF3 AsH3 CCl4 CH2Cl2 N2 H2S
7. Distinguish between intermolecular and intramolecular forces.
8. What is a dipole-dipole force?
9. What are hydrogen bonds?
10. a) Why is the melting and boiling point of H2O significantly higher than H2S? b) Predict and explain the relative melting and boiling points of HF, HCl, HBr and HI.
11. What are London or dispersion forces? How are they affected by molecular size?
12. Which is expected to have the higher boiling point, C8H18 or C22H46? Explain.
13. What type of solid contains particles held together primarily by van der Waals or intermolecular forces?
14. Metals can be rolled into sheets and stamped into various forms. Explain.
15. Ionic solids are hard, with very high melting points, but are very brittle. Explain.
16. Diamond and graphite are allotropes of carbon, composed of carbon atoms covalently bonded in a giant network solid. However, there are distinct differences in their properties. Diamond is extremely hard and brittle. Graphite is soft and slippery, often used as a lubricant. Graphite is also able to conduct electricity, whereas diamond cannot. Both, however, have extremely high melting and boiling points. Explain.
ORGANIC CHEMISTRY
1. Draw structural diagrams of the following:
a) 4-methyl-2-heptene b)