Name _________________________ Date _______________ Chemistry 1-2 _____Hour Unit 2 Review Vocabulary: Chapter 3 law of conservation of mass law of definite proportions law of multiple proportions Dalton’s atomic theory atom atomic number isotope mass number hyphen notation nuclear symbol unified atomic mass unit average atomic mass Chapter 5 periodic law periodic table period group alkali metals alkaline earth metals transition metals metalloids nonmetals halogens noble gases lanthanides actinides Chapter 3 1. Describe the law of conservation of mass, law of definite proportions, and law of multiple proportions. 2. What were the five parts of Dalton’s atomic theory? Which parts were proven to be incorrect and why? 3. Describe the contribution to the development of the model of the atom by the following scientists. Democritus John Dalton J. J. Thomson Ernest Rutherford 4. Describe a given isotope in terms of the number of protons, electrons, and neutrons, using the hyphen notation, or using the nuclear symbol. 5. Compare how isotopes contribute to the average atomic mass of an element when given the atomic masses of the naturally occurring isotopes and their percent natural abundance. 6. Describe the contribution to the development of the periodic table of elements by the following scientists. Dmitri Mendeleev Henry Moseley 7. Identify key properties of the chemical families of the periodic table. Use these properties to place an element in the correct family. alkali metals metalloids Noble gases alkaline earth metals non-metals lanthanides transition metals halogens actinides Name _________________________ Date _______________ Unit 2 Review Chemistry 1-2 _____Hour Name _________________________ Date _______________ Chemistry 1-2 _____Hour Unit 2 Review 8. Complete the table below: Hyphen Notation Nuclear Symbol Number of Protons Number of Electrons Number of Neutrons sodium-23 64 29Cu silver-108 20 20 26 30 9. Answer the questions regarding the average atomic mass of each of element using the table below. Isotope Atomic Mass (u) Percent Natural Abundance (%) Potassium-39 38.964 93.258 Potassium-40 39.964 0.012 Potassium-41 40.962 6.730 Iron-54 53.940 5.845 Iron-56 55.935 91.754 Average Atomic Mass (u) 39.098 55.845 Iron-57 56.935 2.119 Iron-58 57.933 0.282 a. Which isotope of potassium contributes most to the average atomic mass of potassium? How do you know? b. Which isotope of potassium contributes least to the average atomic mass of potassium? How do you know? c. Which isotope of iron contributes most to the average atomic mass of iron? How do you know? d. Which isotope of iron contributes least to the average atomic mass of iron? How do you know?
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