Unit 2 Review Lee

Unit 2 Review: Atomic Structure, Nuclear Chemistry, Quantum Theory, Periodic Table

Basic Atomic Structure
1. Complete the following chart.

2. Atomic mass is a decimal. Why?

3. Define Isotope.

4. Positively charged ions are formed as atoms _______________(lose, gain) electrons.
5. Calculate the atomic mass of the following sample of Silicon. 92.21 % 28Si, 4.70% 29Si, and 3.09% 30Si. Answer to 2 decimal places, remember units.

6. When an atom gains two electrons, it becomes an ion with a charge of __________.
Nuclear Chemistry
Complete the following nuclear decay reactions. Type of Decay (α, β, γ)

7. ______________ 99m43Tc  9943Tc + ______
8. ______________ 24795Am  0-1e + _______
9. ______________ 17593Np  42He + _______
10. What is the difference between fission and fusion? Which releases more energy?

11. What is the difference between nuclear reactions and chemical reactions? (hint: which parts of the atom are involved)

The Bohr Model and Quantum Theory
12. The probability region through which an electron may move is a(n) ______________________________.
13. At a p sublevel, there are (how many) ____________ orbitals. At an s sublevel, there are ___________ orbitals. At a d sublevel, there are ____________ orbitals.
14. The maximum number of electrons possible to any p sublevel is ____________.
15. What was Bohr’s major contribution to our understanding of atomic structure? _______________________
16. If an electron has absorbed energy and has shifted to a higher energy level, the electron is said to be in an .
17. When all the electrons in an atom are in the lowest available energy levels, the atom is in the .
18. Spectral lines of elements are caused by (1) electrons turning in their orbitals, (2) electrons jumping to higher energy levels, (3) the vibration of the nucleus, (4) electrons falling to lower energy levels.
19. Write the full electron configurations (not shortcut) for Sulfur (S) and Manganese (Mn). Circle the valence electrons.

20. Write the shortcut electron configuration for Strontium (Sr) and Oxygen (O). Circle the valence electrons.

Organization of the Periodic Table
21. Each horizontal row of the periodic table is called a(n) ____________; each vertical row is called a(n) ___________________.
22. Which element is in group 15 and period 2? _________________________
23. Which elements are halogens? What charge of ions will they make? Why (what is happening)?

24. Which elements are alkaline earth metals? What charge of ions will they make?

25. List at least three elements that are metals. List three characteristics of metals.

26. List at least three elements that are nonmetals. List three characteristics of nonmetals.

27. Which elements are the metalloids? ___________________________________________
28. Describe electronegativity. ___________________________________________________
29. What happens to the atomic radius as you move left to right across one period? Why?

30. Which element has the highest electronegativity on the whole table? ______________________
31. An atom is chemically when all of the orbitals in the outermost energy level are filled.
32. Elements may react to form ions that have electron configurations like those of the ___________.
33. Label the regions of the periodic table with group and period numbers as well as group names. Also label the s, p, d, and f orbital blocks.