Unit 1: Analyzing Data 1. Measure the following using the appropriate number of significant digits. Name Hour Date. b. o C
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1 Name Hour Date Chemistry Semester 1 Review!!! If you have completed ALL of the review on the assigned days you are allowed to use a cheat sheet that is created on the back of the periodic table found on the last page of this review. Unit 1: Analyzing Data 1. Measure the following using the appropriate number of significant digits a. cm b. o C Measurement in cm for metric ruler on the left. Measurement in ml of graduate cylinder. Measurement in ⁰C. Measurement in ml of graduate cylinder. Measurement in inches. ⁰C Page 1 of 15
2 Draw a cube. Indicate the length of one side in centimeters (cm)? What is the volume of this cube represented by symbols? What is the volume of this cube? What volume (in ml) of water could this box hold if it was filled with water? What is the volume of this cube? What volume (in ml) of water could this box hold if it was filled with water? What is the volume of this cube? What volume (in ml) of water could this box hold if it was filled with water? 2. Does the objects below have the same mass or volume? Explain your answer. In your explanation make sure to include how mass and volume differ. 3. A. Explain the law of conservation of mass. B. Provide an example for the labs that we did to support your explanation. C. Sulfur and Iron are mixed together and heated until they form a compound. Using the picture below determine the mass of the product that was formed. g Page 2 of 15
3 4. What is density? Describe how substances with different densities behave using the pictures below. Use the graph below the answer the following 3 questions. 5. What does the slope of the graph mean? Ma ss (g) Substance A Calculate the slope for substance A. Substance B 6. Which object has a larger density? How do you know? 7. The density of water is 1g/cm 3. Draw the line for water on the graph above. 8. What is the mass of the ethyl alcohol that exactly fills a ml container? The density of ethyl alcohol is g/ml. 9. Calculate the density of sulfuric acid if 35.4 ml of the acid weighs g. 10. A rectangular block of copper metal weighs 1896 g. The dimensions of the block are 8.4 cm by 5.5 cm by 4.6 cm. From this data, what is the density of copper? 11. The diagram below depicts there different gases. Rank the gasses from lowest to highest density. Explain your ranking. Page 3 of 15
4 Unit 2: Gases 12. As the volume of a gas decreases, the pressure (increases/decreases). Particle diagram: Sketch a graph to illustrate this relationship 13. As the temperature of a gas increases, the volume (increases/decreases). Particle diagram: Sketch a graph to illustrate this relationship. 14. As the temperature of a gas decreases, the pressure (increases/decreases). Particle diagram: Sketch a graph to illustrate this relationship. 15. What is the conversion from Celsius to Kelvin: 16. A gas in a 2.0 L container has a pressure of 4.0 atm. When injected into a 1.5 L container, what is the pressure? Initial Final Change Effect P T V n 17. A gas in a closed container is pressurized from 7.00 atm to 10.0 atm. If the original temperature is 10.0⁰C, what is the final temperature of the gas? Initial Final Change Effect P T V n Page 4 of 15
5 18. If 5.0 L of CO2 is heated from K to 150 K, what is the new volume? Initial Final Change Effect P T V n 19. What would be the new volume if 150 cm 3 of gas at 25 C and 0.92 atm pressure were changed to standard conditions of temperature (0 C ) and pressure (1 atm)? Initial Final Change Effect P T V n Unit 3: Energy and States of matter 20. Ice cream is left out and melts. 21. In the previous problem did the system gain or lose energy? Explain your answer. 22. When water is boiling what are in the bubbles? Useful Constants 1 calorie =4.18 joules 1000 joules = I kilojoule 1000 calories = 1 kilocalorie = 1 nutritional calorie 23. A candy bar contains 250 nutritional calories determine how many calories it contains. 24. To boil water it requires 351 kilojoules of energy determine how many calories are required. Page 5 of 15
6 25. How many joules of energy would be required to change the temperature of g of water from 25 o C to 75 o C? 26. Exactly 850 J will raise the temperature of 30.0g of a metal from 25.0⁰C to 60.0⁰C. What is the specific heat capacity of the metal? g of ice at 0.0 C sits on the counter and begins to melt to liquid water. How much energy must be absorbed by the ice if it all melted? 28. While sweating water vapor evaporates from your body, absorbing 125,000 J of energy. (assume no temperature change). What mass of water evaporates? 29. On the graph below label the following items for each region. a. Label the state(s) of matter and describe what is happening during each region. b. Identify how the energy is being stored (Eth or Eph). A B C c. Draw a particle diagram for each region in the boxes below. 29. A 25.0 g sample of water at 20.0⁰C changes to steam at 140⁰C. a. Draw the heating curve for this sample. b. Calculate the total amount of energy this process requires. Page 6 of 15
7 Unit 4: Describing Substances 30. Give an example of a mixture that could be separated using the apparatus shown to the right. 31. Explain how the apparatus below works to separate solutions? 32. Classify the following as Chemical or Physical changes. Verbal Description of Change C or P? a. Melting Iron b. Burning paper c. Metal rusting d. Aluminum foil is cut into smaller pieces. e. Sand is mixed with pebbles and water. 33. Describe and draw a particle drawing of the different categories of matter. ELEMENT: COMPOUND: MIXTURE: 34. Explain how a mixture is different from a compound. Provide an example of each. 35. Consider the four containers below a. Which of these are mixtures? pure substances? b. Which contain only compounds? only elements Page 7 of 15
8 Unit 5: Atomic Structure and Electrons in the Atom 36. Determine whether the statements describe Protons (p + ), Electrons (e - ), Neutrons (n 0 ), or Nucleus (N). There may be more than one answer. Smallest mass Found in the nucleus Positively charged Negatively charged 37. Fill in the chart below Neutral Most dense part of the atom Mass of 1 amu Identifying characteristic of an atom Sc Isotopic Symbol Atomic # Mass # # of protons # of Neutrons # of Electrons What is an isotope? 39. What is the average atomic mass, in amu, for element X? Isotope Mass of the Isotope Percent Abundance X % Identify the element X % Is the average atomic mass from the periodic table closer to or ? EXPLAIN why. 40. Pictured below is the mass spectrogram of a transition metal. a. Based on the experimentally obtained values of mass numbers and percent abundance, calculate the average atomic mass of the element. Show your work below. b. Which isotope is the most abundant? c. Which isotope will deviate the most from the straight line? Page 8 of 15
9 41. Sketch the visible light spectrum below. Include the energy trend. Energy Describe this diagram and indicate which color of visible light has the highest energy? Describe this diagram and indicate which color of visible light has the lowest energy? What energy drop is required to produce a red photon of light? Discuss energy levels. What energy drop is required to produce a violet photon of light? Discuss energy levels. What color of visible light has the lowest energy? What color of visible light has the highest energy? 42. Explain the following rules for electron configuration. a. Aufbau Principle: Page 9 of 15
10 b. Hund s Rule: c. Pauli Exclusion Principle: 43. Rank the following orbitals from lowest to highest energy. 4s, 2p, 3s, 3d, 4p 44. Please study the water flooding buildings analogy below. What sublevel fills after the 3s? The 3s sublevel contains what two elements. What sublevel fills after the 3p? What sublevel fills after the 4s? The 4s sublevel contains what two elements. What sublevel fills after the 5s? This is not shown on the diagram. 45. Write electron configurations and orbital diagrams for the following elements: Be Ni 46. Write the noble gas configuration for the following elements: a. P b. Br Page 10 of 15
11 47. Write the electron configuration for the following elements: a. Kr b. F Unit 6: Periodic Table 48. List common properties of metals and nonmetals. Metals Nonmetals 49. Explain the characteristic that determines the chemical properties of an element. Which characteristic is the most important to determining the chemical properties? 50. Label and the following: alkali metals, alkaline earth metals, halogens, noble gases metals, nonmetals, metalloids # of valence electrons for groups 1-8A s, p, d, and f blocks 51. Identify the trends in atomic size on the periodic table and why each trend exists. Label them on the periodic table above. Page 11 of 15
12 Period Trend: Group Trend: 52. Describe the ionization energy of an atom. 53. Explain why the ionization energy would increase based on the number of protons in the nucleus. The diagram for sodium (Na). The diagram for magnesium (Mg). Write the number of protons in the blank above. Write the electron configuration below. Label the core electrons and valence electrons on the diagram above. Write the number of protons in the blank above. Write the electron configuration below. Label the core electrons and valence electrons on the diagram above. Discuss the force of attraction between the protons in the nucleus and valence (outer electrons). Discuss the force of attraction between the protons in the nucleus and valence (outer electrons). Page 12 of 15
13 54. Identify the trends in ionization energy on the periodic table and why each trend exists. Label them on the periodic table above. Period Trend: Group Trend: 55. Order the following from smallest to largest ionization energy: Ar, He, Rn, Xe 56. Order the following from smallest to largest atomic radius: Ca, Sc, Fe, Br Page 13 of 15
14 57. Explain why the following elements would decrease as you move from left to right on the periodic table. The diagram for sulfur (S). The diagram for chlorine (Cl). Write the number of protons in the blank above. Write the electron configuration below. Write the number of protons in the blank above. Write the electron configuration below. Label the core electrons and valence electrons on the diagram above. Label the core electrons and valence electrons on the diagram above. Discuss the force of attraction between the protons in the nucleus and valence (outer electrons). Discuss the force of attraction between the protons in the nucleus and valence (outer electrons). 58. Draw the electron (Lewis) dot structure for the following elements. a. Sulfur b. Neon 59. What do the dots represent in the above drawing? Page 14 of 15
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Name Hour Date. B. Provide an example for the labs that we did to support your explanation.
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