Periodic PuzzAe W P U D 1A 1. 8A 18 He 2A 2 B 3A 13 4A 5A 6A 7A Class ÿ Date K T A R O S F B L Y. ILr

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2 Name Class ÿ Date Periodic PuzzAe You have been given a list of code letters and clues that correspond to the representative elements in the first four periods of the periodic table. Place each code letter in its proper space in the table. The chemical spmbolfot' each elemen is incittded i/t fhe box. [lint: Do these code letters first: U, A, R, O9 F, L) V, G) Nÿ M IMPORTANT: The code letters fall into these groups on the periodic table: JKQ, WNVG, like, EPFZ, YR, ODS, CXU, THM. CODE LETTER W P U D K T A R O S F L Y CLUE is a noble gas. is the largest atom in its period. has 7 valence electrons in the 2nd energy level. is an element that needs three electrons to become stable. is an atom that forms a 2+ ion. is in the fourth period and forms a 2- ion. has the electron configuration 1s22s22p2. has an atomic number one less than A. has an atomic number one more than A, has 18 more protons in its nucleus than D, has a single electron in the ls-sublevel, has ionization energy less than R but greater than Y. has 8 more protons than A, has atoms that are larger than the atoms of. I C CLUE has its group's smallest ionization energy. has atoms that are larger than those of U, but smaller than those of X. V has one more proton in its nucleus than U, H has the largest first ionization energy in its -- group. G N J has two protons in each atom, has a valence electron configuration of 3s23p6, has valence electrons in the second energy level. M has electron configuration of 3S2 3p4, Q E Z has an atomic mass greater than that of J and less than that of K. has an atomic number less than that of Z but greater than that of P. is the largest atom in its group, X has one less proton in nucleus than W, H 1A 1 8A 18 He Li e 2A 2 3A 13 C 4A 5A 6A 7A N O F Ne Na Mg A! Si P C1 Ar K Ca Ga Ge As Se r ILr Adapled fi'om ChemMatters magazine, Dale Wolf gram, 2

3 Name: Atomic Structure Crossword Puzzle Period: Note: Some clues must be answered with numbers (#) instead of words. Across: Down: 1, the positive particle in the nucleus of an atom, 1, charge on the proton 8, number of electrons in an atom of manganese-55 2, the neutral particle in an atom t0, very reactive metals ("group ÿ") 3, # of electrons in each energy level of sodium (# _# #_) 11, # of electrons in each energy level of potassium (# _# # #_) 4, # of electrons in each energy level of argon (# # #) 12, number of neutrons in an isotope of mass number 9 and atomic 5, mass number of an isotope with 8 electrons and 7 neutrons number 5 6, # of the group containing the 20tÿ element 13, elements with electron configurations ending in "d1'' ("group?") 7, number of valence electrons in the element of atomic 14, atoms with the same number of protons but different numbers number 13 of neutrons 8. number of neutrons in an isotope with mass number4o 17, Rutherford discovered this and atomic number maximum # electrons in 2nd energy level 9, # of valence electrons in the unreactive noble gases 22, charge on the electron 11, # of electrons in each energy level of aluminum (#_ # #) 23, group # containing the 4ÿ element 12, the 7ÿ element has this many valence electrons 25, number of valence electrons in phosphorus 15. reactive metal in period 3 with one valence electron 26, atomic number of fluorine!6, an alkali metal combines with a halogen to make this tasty 28. dlatomic element with seven valence electrons, used in your seasoning for your food pool 18, the smallest subatomic particle 29, element with the electron configuration ts2 2s2 2p8 20. this element has 7 valence electrons and is sometimes 30, number of energy levels in a sodium atom used in a disinfecting solution 21, number of "p" electrons in a helium atom 24, group number of the alkali metals 27, word used to describe the number of neutrons in the hydrogen isotope with mass number 1 3

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5 P RRO#IC TAL WO KSH [T Name 1, Where are the most active metals located? 2, Where are the most active nonmetals located? 3. As you go from left to fight across a period, the atomic size ( decreases / Increases ), Why? 4. As you travel down a group, the atomic size ( decreases / Increases ), Why? 5ÿ 6. 7, 1 9ÿ 10, 11, 12, 1,3, A negattve Ion Is ( larger / smaller ) than Its parent atom. A positive ion Is ( larger / smaller ) than Its parent atom. As you go from left to fight across a period, the first Ionization energy generally ( decreases / increases ), Why? As you go down a group, the first ionization energy generally ( decreases / Increases ), Why? Where Is the highest electronegatlvity found? Where Is the lowest electronegatlvlty found? Elements of Group 1 are called Elements of Group 2 are called Elements of Group 3-12 are called , 16, 17, 18, 19, 20, 21, 22, 23, 24, 25] As you go from left to right across the periodic table, the elements go from ( metals / nonmetals ) to ( metals / nonmetals ),' Group 17 elements are called The most active element In Group 17 Is Group 18 elements are called What sublevels are filling across the Transition Elements? Elements within a group have a similar number of Elements across a series have the same number of A colored ion generally Indicates a_ As you go down a group, the elements generally become ( more / less ) metallic, The majority of elements in the periodic table are (metals / nonmetals ), Elements In the periodic table are arranged according to their An element with both metallic and nonmetallic properties Is called a,. Chemlshy IF8766 Fair, Inc, 5

6 . Reviewsheet: Periodic Table and Periodic Trends Why did Mendeleev's periodic table have blank spaces on it? 2. What contribution did Moseley make to our modern periodic table? 3. State the periodic law. 4. Vertical columns on the periodic table are called are called and horizontal rows 5. Elements with similar chemical properties are placed in the same 6. Complete the table below. Electron Conflg. [Xe]6sÿ4f145d106 ÿ6 [Ar]4sl3ds [He]2sÿ lock Period Group/Type Element 6 1 / Alkali Metal 5 11 / Trans. Metal Fluorine 7. Determine whether the following statements are describing alkali metals (A), alkaline earth metals (AE), transition metals (TM), halogens (H), noble gases (NG): a) most reactive nonometals b) sÿp6 valence configuration c) second most reactive metals d) s1 valence configuration e) exceptions found to e- configurations 0 soft metals g) d orbitals being filled 8. State the group and periodic trends for atomic radius, and ÿ both trends. 9. Compare the atomic radii of the fluorine atom and the iodine atom. 10. Compare the atomic radii of the aluminum atom and the sulfur atom. 6

7 11, Circle the one with the larger radius: Na+ or K+ Na+ or AI3+ F - or CI - F -or N3 12. Circle the one with the smaller radius: Na or Na+ F or F- 13. State the group and periodic trends for ionization energy and exexplain both trends. 14. State the group and periodic trends for electronegativity and ÿ both trends. 15. Compare the ionization energy of sodium to that of potassium. 16. Compare the ionization energy of sodium to that of chlorine. 17, Will the electronegativity of barium be larger or smaller than that of strontium? 18. Arrange oxygen, fluorine, and sulfur in order of increasing electronegativity. 19. For Gro_ÿ, list the element symbol for a) largest atomic radius b) smallest atomic radius c) largest ionic radius d) largest ionization energy e) largest electronegativity 20. For Period 3, list the element symbol for a) largest atomic radius b) smallest atomic radius c) largest ionic radius d) largest ionic radius e) largest electronegatmty 7