2. Periodic Table 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 Atomic Theory Atomic Structure Periodic Trends Electron Configuration

3. This is where electrons are found in an atom. A. In fixed energy levels B. In the nucleus C. In a probable location in the electron cloud D. In an exact location in the electron cloud ?1 $100

4. This was J.J. Thompson’s contribution to atomic structure. A. He discovered the proton B. He discovered the neutron C. He discovered the electron D. He was the first to propose the idea of the atom ?1 $200

5. This conclusion made by Dalton was later proven to be wrong. A. Atoms of the same element are identical B. Atoms are indivisible, solid particles C. Elements can physically mix to form mixtures D. Elements can chemically combine to form compounds ?1 $300

6. This is not a conclusion that Ernest Rutherford made after performing the gold foil experiment. A. The nucleus has a positive charge B. The nucleus is dense C. The nucleus contains protons, neutrons, and electrons D. The atom is mainly empty space ?1 $400

7. This is what Rutherford’s work demonstrates. A. Science is an ongoing endeavor that changes B. Scientific theory is the law C. When experimental data is not consistent with the hypothesis, a scientist creatively relates the two D. It is often difficult for one scientist to reproduce another’s results E. Describe the overall structure of the atom, included but not limited to the following: electrons, protons, nucleus. A1 $500

8. ?2 $100 This is an element/ion that has 7 protons, 5 neutrons, and 10 electrons. A.N 3+ B.N 3- C.N D.Ne

9. This is the mass number of an element with 27 protons, 25 electrons, and 27 neutrons. A. 2 B. 52 C. 54 D. 79 ?2 $200

10. ?2 $300 Be 2+ has this number of electrons.

11. Two isotopes of arsenic have different numbers of this subatomic particle. A. protons B. neutrons C. electrons D. mass number ?2 $400

12. ?2 $500 Element X has two isotopes. If 72% of the element has an isotopic mass of 84 atomic mass units, and 28% of the element has an isotopic mass of 87 atomic mass units. This is the average atomic mass of element X. A. 84 amu B. 84.8 amu C. 85.5 amu D. 87 amu

13. This is the atomic number of the most electronegative element. (Options 1-10) ?3 $100

14. This is the order obtained when placing the elements C, N, Si in order from smallest to largest atomic radius. A. C, N, Si B. N, C, Si C. Si, C, N D. Si, N, C E. C, Si, N F. N, Si, C ?3 $200

15. ?3 $300 This is the reason why ionization energy decreases down a group. A. Shielding

16. This property explains why lithium is most likely of the period 2 elements to give up an electron. A. Atomic Radius B. Density C. Electronegativity D. Ionization energy ?3 $400

17. ?3 $500 This is how metals are different from nonmetals in terms of ionization energies and electronegativies. A. Metals have lower IE and lower electroneg. B. Metals have higher IE and lower electroneg. C. Metals have higher IE and higher electroneg. D. Metals have lower IE and higher electroneg.

18. Elements in group 6A have electron configurations ending in this notation. A. p 2 B. p 3 C. p 4 D. p 5 E. p 6 ?4 $100

19. This is the electron configuration of bromine. A. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 B. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 5 C. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 D. 1s 2 2s 2 2p 4 3s 2 3p 6 3d 8 4s 2 4p 6 ?4 $200

20. For the electron configuration 5s 2, this is what the 5, the s, and the 2 represent. A. principle energy level/period, shape, # e - in sublevel B. principle energy level/group, shape, # e - in sublevel C. principle energy level/period, shape, # e - in element D. principle energy level/group, shape, # e - in element ?4 $300

21. This is the number of unpaired electrons Oxygen has. ?4 $400

22. This electron configuration is a violation of this rule. A. Aufbau’s Principle B. Hund’s Rule C. Pauli’s Exclusion Principle ?4 $500

23. The periodic law is applicable when elements are arranged by this. A. Increasing atomic mass B. Increasing mass number C. Increasing atomic number D. Decreasing atomic mass ?5 $100

24. These elements are generally non- reactive. A. Alkali metals B. Alkaline earth metals C. Transition metals D. Inner transition metals E. Metalloids F. Halogens G. Noble gases ?5 $200

25. This is not a property of a metal at room temperature. A. Conducts electricity B. Lustrous C. Malleable D. Gas ?5 $300

26. Halogens have this number of valence electrons. ?5 $400

27. The element in period 2 that has the largest atomic radius is a member of this family of elements. A. Alkali metals B. Alkaline earth metals C. Transition metals D. Inner transition metals E. Metalloids F. Halogens G. Noble gases ?5 $500