Student Name: ________________________
Student Number: ________________________
Materials needed for this exam include a scientific calculator and a periodic table. If you don’t have a scientific calculator, you can use the calculator available at desmos.com (https://www.desmos.com/scientific). A periodic table from your course is included below for you to use. You can also reference an interactive version (https://www.rsc.org/periodic-table) from the Royal Society of Chemistry website. Please be sure to write in your own words and to show all the steps to solve equations.
1. Define physical and chemical properties, provide three examples of each, discuss their reversibility, and explain the fundamental differences between them.
2. Density is a physical property of a molecule that’s measured as mass per unit volume. Given that density is usually expressed in the units of g/cm3, calculate the density of a cube of plastic that has a mass of 2.331 g and an edge length of 1.500 cm (volume of a cube is V = l3). Be sure to show all steps in the process and include units throughout the problem.
3. Two liquids are in a graduated cylinder – Liquid A has a density of 1.004 g/cm3 and Liquid B has a density of 0.6223 g/cm3. Assuming that they do NOT mix, which liquid is on top and which liquid is on bottom? Where would you expect to find the plastic cube from Question #2 if it is dropped into the graduated cylinder with these two liquids?
4. Three quantum numbers are derived from Schrodinger’s equation that describe the probability of finding an electron around a nucleus: the principal quantum number, the angular momentum quantum number, and the magnetic quantum number. Explain each quantum number, including associated shapes, numbers, letters, and values in your own words.
5. Write the full electron configuration for phosphorus, atomic symbol P
6. Identify if phosphorous is paramagnetic or diamagnetic and explain why.
7. Compare and contrast the alkali metals and the alkaline earth metals by filling in the table below. Discuss 3 physical and 3 chemical properties of both groups, their magnetic properties, and their electron configurations.
Physical Properties (include at least 3)Chemical Properties (include at least 3)Magnetic PropertiesElectron ConfigurationsAlkali MetalsAlkaline Earth Metals
8. Identify what kind of bonding takes place between sodium and chlorine? Explain this bonding. What is the name of the resulting compound? Explain what happens to the compound in water and why it acts this way?
9. Is the bonding in carbon tetrachloride, CCl4 covalent or ionic? Explain how you know.
10. Explain what each of the following represent on the periodic table?
- Rows
- Columns
- Trends
- SPDF Blocks
- Families
For chemical drawings, you can use the Chemical Equation editor in the submission box for the assignment. You can also download a program called Marvin Sketch (https://chemaxon.com/products/marvin).
11. Draw the Lewis structure for sulfur tetrafluoride, SF4
12. Draw the electron pair geometry for sulfur tetrafluoride, SF4. What’s the name of the molecular shape of sulfur tetrafluoride? Note: You can draw this on paper, take a picture, and paste the picture in your document.
13. Draw the structure of water. Is water considered polar or nonpolar? Explain why? Note: You can draw this on paper, take a picture, and paste the picture in your document.
14. When someone is injured, responding medical personnel may use either hot packs or cold packs to treat the injuries. These are examples of miniature chemical reactions. Using hot packs and cold packs as an example, explain the terms endothermic reactionand exothermic reaction.
15. Combustion reactions take place between a fuel and oxygen and produce carbon dioxide and water. Balance the following combustion reaction.
16. Aqueous lead (II) nitrate, Pb(NO3)2 undergoes a double displacement reaction with aqueous sodium chloride, NaCl, in which a precipitate forms. If the precipitate contains lead, write the balanced chemical equation for this reaction. Be sure to include the states of each of the reactants and products.
17. Explain the four basic types of chemical reactions. Be sure to include a sample equation for each type.
18. Describe how rate relationships and activation energy are important in chemical reactions.
19. Write the equilibrium expression for the following reaction.
20. Using the equilibrium expression from Question #19 and based upon the value of K, would you expect there to be more or less product in the equilibrium mixture? Explain why.
