<p> GHS Spring Chemistry Final Review 2014 (Use the STAAR Chemistry Reference Materials) Atomic Structure Problems</p><p>1. If the wavelength of a certain light is 6.5X10-7m what is the frequency?</p><p>2. The frequency of a wave is found to be 9.0X1014Hz. What is the wavelength?</p><p>3. The frequency of a wave is 4.0X1014Hz. Calculate the energy.</p><p>4. Electrons travel as waves within the atom. Calculate the wavelength of a wave if the energy is 6.9X10 -19J.</p><p>5. What happens to the wavelength and energy of the photons of light when the frequency becomes lower?</p><p>Behavior of Gases</p><p>6. Four gases are placed into the same container. Each gas has a partial pressure of 1.0atm what is the total pressure of the gases within the container?</p><p>7. A gas with an initial pressure of 3060 mm Hg and an initial volume of 0.520 L expands to a volume of 2.03 L. What is the final pressure of the gas after the expansion?</p><p>8. What is the volume of 2.00 moles of chlorine gas (Cl2) at STP, to the nearest tenth of a liter?</p><p>9. Explain why doubling the temperature of a gas in a closed vessel doubles the pressure.</p><p>10. Describe the kinetic molecular theory. How does it affect the structure of different states of matter?</p><p>Solutions 11. What volume of 1.0 M sodium phosphate must be used to produce 4.0L of 0.80 M sodium phosphate?</p><p>12. To prepare a dilute solution a student used 500.mL of a 12.0M HCl solution. The final volume of the dilute solution was 1750.mL. Calculate the molarity of the dilute solution.</p><p>13. Find the volume of a solution if 5.00 moles of solute are present and the molarity is 2.25M.</p><p>14. What is the pH of a substance that has a hydrogen ion concentration [H+] of 1.2 x 10-2? 15. Calculate the [OH-] in a 0.004M HCl solution.</p><p>16. Calculate the [H+] in a 0.09M NaOH solution.</p><p>Other Formulas 17. A 10.0mL sample of water has a mass of 10.0g. Calculate the density of water. </p><p>18. The density of aluminum is 2.70g/cm3. Calculate the volume of a 25.0g sample of aluminum.</p><p>19. An electronic balance used to mass a 10.0g weight reported the mass to be 20.0g. Determine percent error.</p><p>20. During a reaction 15.0g of magnesium reacted with excess oxygen. After the reaction students collected 20.2g of magnesium oxide powder. Determine the percent yield for this reaction.</p><p>2Mg(s) + O2(g) → 2MgO(s) </p><p>21. During a reaction 30.0L of nitrogen gas reacted with excess oxygen. If 59.0L of NO2 were collected what is the percent yield for this reaction?</p><p>N2(g) + 2O2(g) → 2NO2(g) </p><p>Constants and Conversions 22. How many particles are in 5.0 moles of any substance?</p><p>23. How many particles are in 10.0 moles of CaCO3? </p><p>24. How many atoms are in 10.0 moles of CaCO3? 25. How many oxygen atoms are in 10.0 moles of CaCO3? </p><p>24 26. How many moles of particles are in 3.01X10 CaCO3 particles?</p><p>24 27. How many moles of atoms are in 3.01X10 CaCO3 particles?</p><p>Conversions and Significant Figures</p><p>28. Convert 500.mL of water into L.</p><p>29. Determine the number of significant figures in each of the following quantities:</p><p> a. 100.0mL</p><p> b. 450mL</p><p> c. 8.00X10-19J</p><p> d. 0.000540kg</p><p>30. Write the formulas for the following compounds:</p><p> a. Sodium sulfate</p><p> b. Sodium sulfite</p><p> c. Disulfur decafluoride</p><p>31. Write the name of the compound for the following names</p><p> a. H3PO4</p><p> b. CO2</p><p> c. FeCl3 Periodic Table</p><p>32. Identify and label the groups and periods on the above periodic table.</p><p>33. Label the following groups: alkali metals, alkaline earth metals, halogens, transition metals, and noble gases. List a few properties of each.</p><p>34. Label the charges of the elements in following groups: 1, 2, (skip transition metals) 13, 14, 15, 16, 17</p><p>35. On the periodic table show the order electrons fill energy levels starting at 1s and ending at 7s.</p><p>36. Use the periodic table to identify and explain periodic trends, including atomic and ionic radii, electronegativity, and ionization energy.</p><p> a. Which has the larger atomic radii? Mg or Cl</p><p> b. Which has the greater electronegativity? P or O</p><p> c. Which has the lower ionization energy? K or Br</p><p>37. Write the electron configuration for the following atoms:</p><p> a. Bromine</p><p> b. Germanium</p><p> c. Strontium</p><p>38. Draw the Lewis valence electron dot structures for the following atoms and compounds:</p><p> a. Bromine (Br2)</p><p> b. Nitrogen (N) c. MgCl2 (IONIC!!!!!!!!)</p><p>39. Draw and identify the molecular geometric shape for the following atoms and compounds:</p><p> a. Water (H2O)</p><p> b. Carbon Dioxide (CO2)</p><p> c. Methane (CH4)</p><p>40. Which of the following are physical changes and which are chemical changes:</p><p> a. Salt dissolving in water</p><p> b. Magnesium reacting with hydrochloric acid</p><p> c. Milk turning sour</p><p> d. Dry ice changing to a gas</p><p>41. Classify the following as either pure substances or mixtures. Define each term.</p><p> a. Element</p><p> b. Compound</p><p> c. Heterogeneous Mixture</p><p> c.i. Colloid</p><p> c.ii. Suspension</p><p> d. Homogenous Mixture d.i. Solution 42. Balance the following chemical equations: a. ___C3H8 + ___O2 → ___H2O + ___CO2</p><p> b. ___LiOH → ___Li2O + ___H2O</p><p> c. ___Mg + ___Al2(CO3)2 → ___Al + ___MgCO3</p><p>43. Define the following terms: a. Intensive Property</p><p> b. Extensive Property</p>