Chemistry First nine weeks review Show all work or receive no credit
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1 Chemistry First nine weeks review Show all work or receive no credit Define the following terms chemical change density extensive property intensive property physical change isotope average atomic mass molar mass Conversion factor Mixture Compound Solution alloy 1. Explain how you can tell that a chemical change has occurred. 2. List 3 changes that are physical changes
2 3. Answer the following with the correct number of sig figs a x 4.59 b x / 1.9 x c How many sig figs do each of the following numbers have? a b c d e f If you have a sample of an unknown substance what types of experiments could you conduct to see if it is a pure substance? 6. Give 3 examples of a. Homogenous mixtures b. Heterogenous mixtures c. Compounds d. elements 7. If you have a mole of Carbon, what does that mean to you? 8. Compare a mole of nitrogen to a mole of Calcium. What is different and what is the same?
3 9. Explain how to calculate average atomic mass. Isotope Mass Number (grams) Percent Abundance (%) A B C What is the average atomic mass of the element above? 11. An element has 4 stable isotopes. What is the average atomic mass and which element is this? Mass % Abundance % % % 208? 12. List 3 conversion factors that you have used outside of school 13. What are the molar masses of the following a. Ca b. N c. PbNO3 d. Al(NO3) e. If you had 4.67 grams of aluminum nitrate (listed in part d above), how many moles would that be? How many atoms?
4 14. Explain how the kinetic molecular theory describes the motion of solids, liquids, and gases. 15. Are all particles moving all the time or do some atoms stay still? 16. Do all atoms of the same element have the same mass? Explain. Midterm Practice Questions Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The average atomic mass of an element is the average of the atomic masses of its a. naturally occurring isotopes. c. radioactive isotopes. b. two most abundant isotopes. d. artificial isotopes. 2. A prospector finds g of pure gold (atomic mass amu). She has a atoms of Au. c atoms of Au. b atoms of Au. d atoms of Au. 3. A sample of tin (atomic mass amu) contains atoms. The mass of the sample is a g. c g. b g. d. 11 g. 4. Which of the following is an extensive property of matter? a. melting point c. volume b. boiling point d. Density
5 5. Which of the following is an intensive property of matter? a. amount of energy c. volume b. density d. mass 6. The relationship between the mass m of a material, its volume V, and its density D is a. D = mv. c. D = m/v. b. D = V/m. d. D = m + v g is equivalent to a. 250 kg. c mg. b. 250 mg. d kg. 8. The number of significant figures in the measurement 2010 cm is a. 1. c. 3. b. 2. d Which of the following lists atomic orbitals in the correct order they are filled according to the Aufbau principle? a. 1s 2s 2p 3s 4s 3p 3d 4p 5s b. 1s 2s 2p 3s 3p 4s 3d 4p 5s c. 1s 2s 2p 3s 3p 4s 4p 3d 4d d. 1s 2s 2p 3s 3p 3d 4s 4p 5s 10. The element with electron configuration 1s 2 2s 2 2p 6 3s 2 3p 2 is a. Mg (Z = 12). c. S (Z = 16). b. C (Z = 6). d. Si (Z = 14). 11. The electron notation for aluminum (atomic number 13) is a. 1s 2 2s 2 2p 3 3s 2 3p 3 3d 1. b. 1s 2 2s 2 2p 6 3s 2 2d 1. c. 1s 2 2s 2 2p 6 3s 2 3p 1. d. 1s 2 2s 2 2p 9. Chemistry Nine weeks Review Part 2 Define the following Terms Nuclear reaction
6 Alpha particle Beta particle 1. Explain alpha decay and give 1 example of a nuclear equation that shows alpha decay. 2. Compare and contrast fission and fusion. Where do these reactions occur? We use fission for power but not fusion, even though fusion produces more power. Why don t we use fusion? 3. Describe the differences in charge and mass between alpha, beta, and gamma radiation. 4. Draw a picture of an alpha and a beta particle moving between 2 electrodes. One electrode is positively charged and the other is negatively charged. 5. What was discovered in the cathode ray tube experiment? How were they discovered? Who discovered them? 6. Which of Dalton s postulates disagrees with modern atomic theory? 7. What were the conclusions that resulted from Rutherford s gold foil experiment? 8. Draw and label a picture of the Bohr model.
7 9. Write an electron configuration that is wrong and explain why it s wrong and which rule it violates. 10. What is the energy of a wave with a frequency of 3.45 x Hz? 11. Do all light waves move at the same speed? Explain. 12. If a wave has a wavelength of 5.67 x m what is the frequency? 13. What is the Energy of a 3.45 x 10-8 km wave? 14. How did Mendeleev arrange his periodic table? 15. How is our periodic table different today from Mendeleev s. 16. Name 2 elements from the following groups a. Halogens b. Metalloids c. Alkali metals d. Alkaline earth metals e. Noble gases f. Transition metals g. Lanthanides
8 h. Actinides i. Non metals Midterm Review Part 2 1. Balance the following equation: a. c. b. d. 2. Which of the following processes always decreases the number of protons by an even number? a. fusion c. alpha decay b. beta decay d. fission 3. Alpha particles are a. electrons. c. electromagnetic waves. b. helium nuclei. d. neutrons. 4. Beta particles are a. electrons. c. electromagnetic waves. b. helium nuclei. d. neutrons. 5. Which of the following is the symbol for an alpha particle? a. c. b. d. 6. Which of the following is the nuclear symbol for a beta particle? a. c. b. d.
9 7. A sample of tin (atomic mass amu) contains atoms. The mass of the sample is a g. c g. b g. d. 11 g. 8. How many molecules are there in 5.0 g of methyl alcohol, CH3OH? a c b d Which of the following lists atomic orbitals in the correct order they are filled according to the Aufbau principle? a. 1s 2s 2p 3s 4s 3p 3d 4p 5s b. 1s 2s 2p 3s 3p 4s 3d 4p 5s c. 1s 2s 2p 3s 3p 4s 4p 3d 4d d. 1s 2s 2p 3s 3p 3d 4s 4p 5s 10. The element with electron configuration 1s 2 2s 2 2p 6 3s 2 3p 2 is a. Mg (Z = 12). c. S (Z = 16). b. C (Z = 6). d. Si (Z = 14). 11. The electron notation for aluminum (atomic number 13) is a. 1s 2 2s 2 2p 3 3s 2 3p 3 3d 1. b. 1s 2 2s 2 2p 6 3s 2 2d 1. c. 1s 2 2s 2 2p 6 3s 2 3p 1. d. 1s 2 2s 2 2p 9.
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