Unit 2: Atomic Structure Review Packet
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1 Name: Unit 2: Atomic Structure Review Packet Dalton s Model: 1. I can describe John Dalton s contribution to our Thomson s Experiment: 2. I can describe JJ Thomson s contribution to our Thomson s Model: Rutherford s Experiment: 3. I can describe Ernest Rutherford s contribution to our Rutherford s Model: Bohr s Model: 4. I can describe Niels Bohr s contribution to our understanding of the atom. What does the modern model of the atom look like? 5. I can describe our Where, in an atom, are electrons likely to be found according to the modern model?
2 From oldest to newest, list the models that we have used to describe an atom. 6. I can state the chronological order of atomic models. Particle #1 Particle #2 Particle #3 7. I can state the three subatomic particles, their location in an atom, their charges, and their masses (in amu). Name Charge Mass Location in Atom 8. I can explain why atoms are electrically neutral.. I can define mass number and atomic number. Atoms are electrically neutral because the number of is equal to the number of. Definitions: mass number atomic number 10. Given the mass number, I can determine the number of protons, neutron, and electrons in an atom. 11. I can use the Periodic Table to determine the atomic number of an element. 12. I can define isotope. In an atom of 212 Po, how many protons are present? In an atom of 212 Po, how many electrons are present? In an atom of 212 Po, how many neutrons are present? How many protons are in an atom of selenium? How many protons are in an atom of silicon? isotope
3 13. I can represent an atom in any of the four methods of isotopic notation. Write the four different methods of isotopic notation for an atom of bromine that has 45 neutrons. Method 1 Method 2 Method 3 Method I can calculate average atomic mass given the masses of the naturally occurring isotopes and the percent abundances. Element Q has two isotopes. If 77% of the element has an isotopic mass of 83.7 amu and 23% of the element has an isotopic mass of 8.3 amu, what is the average atomic mass of the element? Definitions: ion 15. I can define ion, cation, and anion. cation anion How many protons are in 1 F 1-? 16. Given the mass number and the charge, I can determine the number of protons, neutrons, and electrons in an ion. How many neutrons are in 1 F 1-? How many electrons are in 1 F 1-?
4 Definitions: principal energy level orbital 17. I can define principal energy level, orbital, ground state, excited state, electron configuration, and bright line spectrum. ground state excited state electron configuration bright line spectrum 18. I can state the relationship between distance from the nucleus and energy of an electron. 1. I can explain, in terms of subatomic particles and energy states, how a bright line spectrum is created. As the distance between the nucleus and the electron increases, the energy of the electron. A brightline spectrum is created when 20. I can identify the elements shown in a bright line spectrum. Which element(s) is/are present in the mixture?
5 21. I can define valence electrons. valence electron 22. I can locate and interpret an element s electron configuration on the Periodic Table. How many valence electrons does an atom of rubidium have in the ground state? How many principal energy levels contain electrons in an atom of iodine in the ground state? Which electron configuration represents an atom of potassium in the excited state? 23. I can identify an electron configuration that shows an atom in the excited state. 24. I can draw Lewis electron dot diagrams for a given element. A) B) C) D) Draw the Lewis electron dot diagram for the following atoms: Li Be B C N O F Ne octet of valence electrons 25. I can define and state the importance of octet of valence electrons. The importance of having a complete octet of valence electrons is
Unit 2: Atomic Structure Practice Packet
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