SOL Review Sheet

SOL Review Sheet

1. Express the following numbers in correct scientific notation:
2. 8 700 000
3. 0.00 000 628
4. How many significant figures are in each of the following numbers:
5. 1837
6. 6005
7. 302400
8. 300.0
9. 0.0040
10. Add or subtract and state the answer with the correct number of sig figs:
11. 85.26 cm + 4.6 cm
12. 1.07 cm + 0.607 cm
13. 186.4 cm – 57.83 cm
14. Multiply or divide and state the answer with the correct number of sig figs:
15. (5.5cm)(4.22cm)
16. (2.6kg)/(9.42cm)
17. ((8.95)(9.162))/((4.25)(6.3))
18. Describe the difference between accuracy and precision.

1. Name the 8 prefixes and their conversion value.

1. What did these scientists discover/determine?
2. Dalton
3. Rutherford
4. Thompson
5. Goldstein
6. Chadwick
7. Mendeleev
8. Mosely
9. Democritus
10. Heisenberg
11. Bohr
12. Charles
13. Boyle
14. Lussac
15. Avagdro
16. The three isotopes of nitrogen are N-14, N-15, and N-16. The relative abundances of these isotopes are 95%, 3%, and 2% respectively. What is the average atomic mass of nitrogen?

1. What family, periods, or section represents the following:
2. Alkali metals
3. Alkaline earth metals
4. Transition metals
5. s block
6. p block
7. d block
8. f block
9. Halogens
10. Noble gases
11. Metals
12. Nonmetals
13. Name the following:
14. KOH
15. H2SO4
16. PCl3
17. Ba3N2
18. CuCl2
19. What are key rules in naming compounds?

1. Define and describe trend according the periodic table the following words:
2. Electronegitivity

1. Ionization energy

1. Atomic size

1. What is the electron configuration and the orbital diagram for the following: ( what rules apply?)
2. Calcium

1. Silicon

1. Oxygen

1. Copper

1. Barium

1. What are the 5 molecular shapes, draw each shape, describe when molecules form each shape, and provide an example of each.

1. What is the difference between an ionic compound and a covalent compound? Provide an example.

1. Compare polar and nonpolar covalent compounds? How is polarity determined?

1. What are the empirical formula and the molecular formula?

1. A compound is composed of 85.6% of carbon and 14.36% of hydrogen. The compound has a formula mass of 42.08 grams. What is the molecular formula?

1. What are the 5 major types of reactions? Give an example of each type.

1. What is a precipitate? How is one formed in a reaction?

1. What conversions come from the mole road map:

1. 2H2S (g) + 3O2(g)  2H2O (g) + 2SO2(g) If 3.50 g of H2S are used in this double replacement reaction, what will be the theoretical yield of oxygen in grams?

1. 2H2 (g) + O2(g)  2H2O(g) How many molecules of oxygen are required to produce 3.1 liters of water at STP?

1. A sample of nitrogen occupies 10.0liters at 25°C and 98.7kPa. What should the volume at 20°C and 102.7 kPa?

1. If the pressure exerted on a confined gas is doubled, the volume of the gas will-

1. Explain direct proportional and indirect (inversely) proportional.

1. Industrial deep sea divers must breathe a mixture of helium and oxygen to prevent a disorienting condition known as nitrogen narcosis. If a diver’s tank is filled with a helium-oxygen mixture to a pressure of 170 atmospheres and the partial pressure of helium is 110 atmospheres, the partial pressure of oxygen is-

1. What is the kinetic molecular theory?

1. Water can be made to boil above the normal boiling point of 100°C by-

1. Draw the phasediagram of water and label and define the triple point, solid phase, liquid phase, gas phase, sublimation process, vaporization process, condensation process, melting process, and solidification process.

1. Compare and Contrast endothermic and exothermic. What are key words that describe each? Provide examples.

1. Compare and Contrast endothermic and exothermic reactions. Include the placement of energy in the reaction.

1. Solid magnesium has a specific heat of 1.01 J/g°C. How much heat is given by a 20.0 gram sample of magnesium when it cools form 70°C to 50°C? Is it endothermic or exothermic?

1. If the heat of fusion is 32.2 kJ/mol, the amount of heat energy required to melt 5.67 grams of FeO is?

1. Calculate the amount of heat produced when 34.8 g of methane, CH4, burns in excess of oxygen, according to the following equation: CH4(g) + 2O2(g)  CO2(g) + 2H2O (l) + 890.2kJ Is it endothermic or exothermic?

1. How many milliliters of 2.00M H2SO4 are needed to provide 0.250 mole of H2SO4?

1. A solution contains 225g of glucose, C6H12O6, dissolved in enough water to make 0.825L of solution. What is the molarity of the solution?

1. How many grams of sodium chloride are required to prepare 500.0mL of a 0.100 M solution?

1. What is the final concentration if 50mL of 2.00M solution is diluted to 500mL?

1. Describe the words concentrated and dilute.

1. What is the difference between solution, suspension, and a colloid?

1. What are the three factors that affect solubility?

1. What is the collision theory?

1. What are the four factors that affect reaction rate? Explain.

1. Draw a endothermic and a exothermic reaction pathway diagram include activation energy, activated complex, products, and reactants. Draw in one or both what a catalyst would do to the reaction.

1. What is entropy? Provide examples.

1. What is Free Energy?

1. What is an acid and what is a base?

1. What is the pH scale?

1. What is the pH of a solution that has a hydrogen concentration of 1 x 10-5?

1. What is the hydrogen concentration if the pH is 8.00?

1. What are pH indicators? Provide some example of pH indicators.

1. The purpose of a titration is-

1. The formula used in a titration is-